CHM 103 Skills Check

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Which of these unit conversions would allow you to convert the cost of steak ($6.99/pound) into dollar per gram? Given English-metric unit relationships: 1 kg = 2.20 lb, 1 lb = 454 grams

($6.99/ 1 lb)(2.20 lb/ 1000 g)

Which unit relationship below is not correct for this balanced chemical equation, which describes the reaction of zinc metal with hydrochloric acid (aqueous HCl)? Zn + 2HCl --> H2 + ZnCl2 2 moles of hydrochloric acid is equivalent to 1 mole of Zn 1 mole of hydrogen gas is equivalent to 1 mole of Zn 1 mole of hydrogen gas is equivalent to 2 moles of hydrochloric acid 1 mole of Zn is equivalent to 1 mole of zinc (II) chloride 1 mole of Zn is equivalent to 2 moles of hydrogen gas

1 mole of Zn is equivalent to 2 moles of hydrogen gas

What is the oxidation number of Sn in tin (IV) sulfide? +1 +4 +2 -2 -4

Consider the reaction of nitrogen and hydrogen to make ammonia. What is the oxidation number of nitrogen in the ammonia molecule? N2 + 3H2 --> 2NH3 +3 0 -3 +1 -1

-3

In working Gas Law calculations, we use the Kelvin temperature scale, rather than Celsius. But since most temperatures are measured in Celsius, it's essential to be able to convert between the two scales. Convert a temperature of 210 K into a Celsius temperature. 242 oC 63.0 oC -63.0 oC 483 oC

-63.0 oC

Work this calculation, and express the result with the appropriate number of significant figures. (3.4 × 10^2) (9.81 × 10^3)/(−7.02) (6.2309 × 10^−4 ) = 7.6 x 10^8 -7.6 -7.6 x 10^8 3.0 x 10^2 -3.0 x 10^2

-7.6 x 10^8

Calculate the new temperature in °C when 6.00 L of helium gas at 20.0 °C is compressed to 4.00 L. 30.0 °C -77.9 °C 13.3 °C 166.4 °C

-77.9 °C

Consider the reaction below for the fermentation of glucose, C6H12O6. What volume of a 1.50 molar glucose solution should be used in order to produce 3.00 moles of ethanol, C2H5OH? C6H12O6 (aq) → 2 C2H5OH (aq) + 2 CO2 (g) 1 liter glucose 2.25 liters glucose 4.00 liters glucose 3.00 liters glucose 1.00 x 10^3 mL glucose

1.00 x 10^3 mL glucose

Consider the reaction below for the fermentation of glucose, C6H12O6. What volume of a 1.50 molar glucose solution should be used in order to produce 3.00 moles of ethanol, C2H5OH? C6H12O6 (aq) → 2 C2H5OH (aq) + 2 CO2 (g) 2.25 liters glucose 1 liter glucose 4.00 liters glucose 3.00 liters glucose 1.00 x 10^3 mL glucose

1.00 x 10^3 mL glucose

What volume of a 0.125 M H2SO4 solution would contain 12.5 grams of solute? 1.02 mL 100 mL 3.81 mL 1.02 x 10^3 mL 1.00 x 10^2 mL

1.02 x 10^3 mL

What volume of a 0.125 M H2SO4 solution would contain 12.5 grams of solute? 100 mL 1.02 x 10^3 mL 1.00 x 10^2 mL 1.02 mL 3.81 mL

1.02 x 10^3 mL

Which Density probably represents a Liquid? 21.5 g/ml 2.70/ g/ml 1.032 g/ml 0.00143 g/ml

1.032 g/ml

A sample of blood has a density of 1.05 g/mL. Which is the correct mass of 1.000 liter of the blood? Set up and solve the unit conversion. 1.05 x 10^-3 grams 1.050 x 10^3 grams 105 grams 1.05 kilograms more than one of these is correct

1.05 kilograms

When the measurement 105.00 grams is written in scientific notation, it becomes: 1.0500 x 10^-2 grams 1.0500 x 10^2 grams 1.05 x 10^-2 grams 1.0500 x 10^4 grams 1.05 x 10^2 grams

1.0500 x 10^2 grams

Which measurement below has the fewest significant figures? 4700. m 1.20 x 10^4 g 1.060 x 10^-2 g 410.0 g 7.200 x 10^5 g

1.20 x 10^4 g

Consider the balanced chemical equation below for the reaction of zinc metal with hydrochloric acid (aqueous HCl). How many moles of zinc (II) chloride would be produced from the reaction of 2.50 moles of hydrochloric acid? Zn + 2HCl --> H2 + ZNCl2 1.25 moles zinc (II) chloride 2.00 moles zinc (II) chloride 1.75 moles zinc (II) chloride 1.50 moles zinc (II) chloride 2.25 moles zinc (II) chloride

1.25 moles zinc (II) chloride

Which unit conversion would allow you to convert 1.3 yards to centimeters? Given English-metric unit relationships: 1.094 yard = 1 meter, 1 inch = 2.54 cm

1.3 yards (1 m/1.094 yd)(10^2 cm/1 m)

What is the molarity of a solution that contains 0.325 moles of NaOH in 2.50 x 102 mL? 1.30 x 103 M NaOH 1.30 M NaOH 1.30 x 10-3 M NaOH 0.769 M NaOH 1.3 M NaOH

1.30 M NaOH

Work this calculation, and express the result with the correct number of significant figures/decimal places. (1.21 x 10^-3 + 0.0013) x (6.453 x 10^2) = 2 1.61 1.619 1.62 1.6

1.6

Which unit conversion would allow you to convert 1.75 grams of silver atoms into moles? 107.9 grams of silver (1 mole of silver/1.75 grams) = 1.75 grams of silver (1 mole of silver/32.06 grams) = 1.75 grams of silver (1 mole of silver/6.02 × 10^23 grams) = 1.75 grams of silver (1 mole of silver/107.9 grams) = 1.75 grams of silver (1 mole of silver/87.62 grams) =] 1.75 grams of silver (1 mole of silver/28.09 grams) =

1.75 grams of silver (1 mole of silver/107.9 grams) =

Consider the balanced chemical equation below for the reaction of zinc metal with hydrochloric acid (aqueous HCl). How many moles of zinc metal would be needed to react with 3.50 moles of hydrochloric acid? Zn + 2HCL --> H2 + ZnCl2 1.25 moles of Zn 1.50 moles of Zn 1.75 moles of Zn 2.00 moles of Zn 1.00 mole of Zn

1.75 moles of Zn

Consider the balanced chemical equation below for the reaction of zinc metal with hydrochloric acid (aqueous HCl). How many moles of zinc metal would be needed to react with 3.50 moles of hydrochloric acid? Zn + 2HCl --> H2 + ZnCl2 2.00 moles of Zn 1.00 mole of Zn 1.75 moles of Zn 1.25 moles of Zn 1.50 moles of Zn

1.75 moles of Zn

Which unit conversion would allow you to convert 1.78 deciliters into cubic centimeters? 1.78 dL (10 dL/1 L)(100 cm^2/ 1 L) = 1.78 dL (0.1 L1 dL)(10^3 cm^3/ 1 L) = 1.78 dL (1 dL/10^−1 L)(1 L/1000 cm^2) = 1.78 dL (1 L/10 dL)(100 cm^3/1 L) =

1.78 dL (0.1 L1 dL)(10^3 cm^3/ 1 L) =

Work this calculation, and express the answer with the appropriate number of significant figures. (6.09 x 10^-7) x (2.97 x 10^2) = 2.05 x 10^5 1.8 x 10^-4 1.81 x 10^-4 2.05 x 10^-9 1.80 x 10^-4

1.81 x 10^-4

Which is the correct unit relationship between deciliters and liters?(You should not need to consult a table. Your goal is to be fluent in the metric units.) 10^-1 dL = 1 L 1/10 dL = 1 L 10 dL = 1 L 10 L = 1 dL 0.1 dL = 1 L

10 dL = 1 L

How many 100 mg capsules of penicillin could be made from 1 kilogram of penicillin? Set up and solve the unit conversion. 100,000 capsules 1000 capsules 10 capsules 100 capsules 10,000 capsules

10,000 capsules

The density of a irregularly-shaped sample of metal is calculated after making mass and volume measurements: (21.5 g − 10.5 g)/(34.50 mL − 33.40 mL) = The final result should be reported as: 10 g/mL 10.0 g/mL 10.00 g/mL 1.00 g/mL 10. g/mL

10.0 g/mL

Consider the balanced chemical equation below, which describes the combustion of ethane, C2H6. If 5.00 moles of ethane was burned, how many moles of carbon dioxide would be produced? 2C2H6 + 7O2 --> 4Co2 + 6H2O 4.00 moles CO2 8.00 moles CO2 2.50 moles CO2 10.0 moles CO2 20.0 moles CO2

10.0 moles CO2

Consider the balanced chemical equation below, which describes the combustion of ethane, C2H6. If 3.00 moles of ethane is burned, how many moles of oxygen gas are needed to participate in the reaction? 2C2H6 + 7O2 --> 4CO2 + 6H20 21.0 moles of oxygen gas 12.0 moles of oxygen gas 8.00 moles of oxygen gas 10.5 moles of oxygen gas 7.00 moles of oxygen gas

10.5 moles of oxygen gas

If acid rain causes pond water to change from pH 6 to pH 4, the hydronium ion concentration becomes 100 times higher 2 times higher 20 times higher 100 times lower 20 times lower 2 times lower

100 times higher

If acid rain causes pond water to change from pH 6 to pH 4, the hydronium ion concentration becomes 100 times lower 20 times lower 2 times lower 20 times higher 100 times higher 2 times higher

100 times lower

If consuming antacids and proton pump inhibitors causes stomach pH to increase from pH 2 to pH 4, the hydronium ion concentration becomes 100 times lower 20 times lower 2 times higher 20 times higher 2 times lower 100 times higher

100 times lower

Chloroacetic acid (Ka = 1.4 x 10^-3) is a stronger acid than acetic acid (Ka = 1.8 x 10^-5). Approximately how much stronger is it? 1000 times stronger 100 times stronger 2 times stronger 20 times stronger

100 times stronger

Chloroacetic acid (Ka = 1.4 x 10^-3) is a stronger acid than acetic acid (Ka = 1.8 x 10^-5). Approximately how much stronger is it? 1000 times stronger 2 times stronger 20 times stronger 100 times stronger

100 times stronger

Assuming that the volumes are additive, what volume of water must be added to 35.0 mL of 12.0 M HCl to make a solution which is 3.00 M? 1.40 x 10^2 mL 87.5 mL 70.0 mL 105 mL

105 mL

Assuming that the volumes are additive, what volume of water must be added to 35.0 mL of 12.0 M HCl to make a solution which is 3.00 M? 105 mL 1.40 x 102 mL 87.5 mL 70.0 mL

105 mL

Which is the correct unit relationship between cubic centimeters and liters?(You should not need to consult a table. Your goal is to be fluent in the metric units.) 100 cm^3 = 1 liter 10^3 cm^3 = 1 liter 10^-2 cm^3 = 1 liter 1 cm^3 = 10^-2 liter These units aren't related!cm^3 is length, and liters is volume

10^3 cm^3 = 1 liter

The mass of an Avogadro's number of octane molecules (C8H18) is: 114 grams 6.02 x 10^23 atomic mass units 114.22 grams 6.02 x 10^23 grams 114.22 atomic mass units 13.02 grams

114.22 grams

Complete this Avogadro's Statement for the element Tin by supplying the missing mass:1 mole of Tin = 6.02 x 10^23 atoms = ____ 204.4 grams 118.7 grams 47.88 grams 207.2 grams 127.6 grams

118.7 grams

Which is the correct translation of the concentration unit 12 molar HCl? 12 moles HCl/100 liters solution 12 moles HCl/1 liter solvent 12 molecules HCl/1 mL solution 12 moles HCl/1 liter solution 12 grams HCl/100 mL solvent

12 moles HCl/1 liter solution

How much heat, in kilocalories, is need to raise the temperature of a 500.0 g of steam from 110 °C to 160 °C? 68.9 kcal 0.0196 kcal 12.8 kcal 28.2 kcal

12.8 kcal

Consider the reaction shown below. What volume of a 2.00 M H2SO4 solution would be needed to react with 0.250 moles of CaCO3? CaCO3 (s) + H2SO4 (aq) → H2CO3 (aq) + CaSO4 (aq) 0.250 L H2SO4 1.25 L H2SO4 125 mL H2SO4 0.0125 liters H2SO4 5.00 x 10^2 mL H2SO4

125 mL H2SO4

The formula weight of CuSO4 is ____ amu. 111.61 112 160. 159.61

159.61

An atom with 74 protons, 109 neutrons, and 74 electrons would have an atomic mass (and a mass number) of: 148 183 257 109 74

183

An atom with 74 protons, 109 neutrons, and 74 electrons would have an atomic mass (and a mass number) of: 148 257 183 74 109

183

Ethane, C2H6, burns to produce carbon dioxide and water by the chemical reaction shown below. C2H6 + O2 --> CO2 + H2O What coefficient should be placed in front of the ethane when this equation is properly balanced with the lowest set of whole numbers? 4 5 3 7 6 2

The maximum number of electrons that can occupy a f orbital is: 6 2 5 14 3 7

When the chemical equation below is properly balanced, what coefficient should be placed in front of the product, ammonia? N2 +H2 --> NH3 5 4 1 2 3

When this chemical equation is properly balanced, what coefficient should be placed in front of the potassium chloride? KCIO3 --> KCI + O2 2 5 1 4 3

Arrange the following items by relative entropy, from lowest entropy (1) to highest entropy (4). 50 g of melted butter in a warm sauce pan. 50 g of bubbling hot butter in a hot sauce pan. 50 g of butter all evaporated from a very hot sauce pan. 50 g of solid butter at refrigerator temperature.

2 3 4 1

Which unit conversion would allow you to convert 0.500 grams of oxygen gas into moles? 0.500 grams of oxygen (32.00 grams O2/1 mole of O2) = 32.00 grams of oxygen (1 mole of O2/0.500 grams O2) 0.500 grams of oxygen (1 mole of O2/32.00 grams O2) 0.500 grams of oxygen (1 mole of O/16.0 grams O) = 0.500 grams of oxygen (1 mole of O/26.02 × 1023 grams O2) = 6.02 × 1023 grams of oxygen (1 mole of O2/0.500 grams O2) =

0.500 grams of oxygen (1 mole of O2/32.00 grams O2)

3.00 liters of solution contain 1.75 moles of copper (II) oxide. Express the concentration of the CuO solution in molarity units. 0.583 M CuO 5.83 x 10^-4 M CuO 1.71 M CuO 1.71 x 10^4 M CuO 5.83 x 10^4 M CuO

0.583 M CuO

Consider the reaction shown below. How many moles of HCl would be needed to react with the Al(OH)3 contained in 1.00 liter of a 0.200 M Al(OH)3 solution? Al(OH)3 (aq) + 3 HCl (aq) → 3 H2O (l) + AlCl3 (aq) 0.600 moles HCl 0.200 moles HCl 0.6 moles HCl 0.0667 moles HCl 3.00 moles HCl

0.600 moles HCl

Consider the reaction shown below. How many moles of HCl would be needed to react with the Al(OH)3 contained in 1.00 liter of a 0.200 M Al(OH)3 solution? Al(OH)3 (aq) + 3 HCl (aq) → 3 H2O (l) + AlCl3 (aq) 0.0667 moles HCl 0.200 moles HCl 0.6 moles HCl 0.600 moles HCl 3.00 moles HCl

0.600 moles HCl

Consider the reaction shown below. How many moles of Cl2 gas would be needed to react with 6.00 liters of a 0.250 M NaClO2 solution? 2 NaClO2 (aq) + Cl2 (g) → 2 ClO2 (g) + 2 NaCl (aq) 0.300 moles Cl2 1.50 moles Cl2 1.50 moles Cl2 0.750 moles Cl2 0.75 moles Cl2

0.750 moles Cl2

Which unit relationship below is not correct for this balanced chemical equation, which describes the reaction of zinc metal with hydrochloric acid (aqueous HCl)? Zn + 2HCl --> H2 + ZnCl2 1 mole of hydrogen gas is equivalent to 1 mole of Zn 1 mole of Zn is equivalent to 2 moles of hydrogen gas 1 mole of Zn is equivalent to 1 mole of zinc (II) chloride 2 moles of hydrochloric acid is equivalent to 1 mole of Zn 1 mole of hydrogen gas is equivalent to 2 moles of hydrochloric acid

1 mole of Zn is equivalent to 2 moles of hydrogen gas

Which unit relationship below is not correct for this balanced chemical equation (which describes the combustion of ethane, C2H6)? 2C2H6 + 7O2 --> 4CO2 + 6H2O 7 moles of O2 is equivalent to 4 moles of CO2 2 moles of C2H6 is equivalent to 2 moles of CO2 2 moles of C2H6 is equivalent to 7 moles of O2 6 moles of H2O is equivalent to 2 moles of C2H6 7 moles of O2 is equivalent to 6 moles of H2O

2 moles of C2H6 is equivalent to 2 moles of CO2

Which of these samples of matter would have the largest mass in grams? 5 moles of hydrogen gas, H2 2 moles of carbon dioxide, CO2 4 moles of water, H2O 3 moles of carbon monoxide, CO

2 moles of carbon dioxide, CO2

Which unit relationship below is not correct for this balanced chemical equation (which describes the decomposition of potassium chlorate)? 2 KClO3 --> 2 KCl + 3O2 2 moles of potassium chlorate is equivalent to 2 moles of oxygen gas 3 moles of oxygen gas is equivalent to 2 moles of potassium chlorate 2 moles of potassium chloride is equivalent to 2 moles of potassium chlorate 2 moles of potassium chloride is equivalent to 3 moles of oxygen gas

2 moles of potassium chlorate is equivalent to 2 moles of oxygen gas

Which unit relationship below is not correct for this balanced chemical equation (which describes the decomposition of potassium chlorate)? 2KClO3 --> 2KCl + 3O2 2 moles of potassium chloride is equivalent to 2 moles of potassium chlorate 2 moles of potassium chloride is equivalent to 3 moles of oxygen gas 3 moles of oxygen gas is equivalent to 2 moles of potassium chlorate 2 moles of potassium chlorate is equivalent to 2 moles of oxygen gas

2 moles of potassium chlorate is equivalent to 2 moles of oxygen gas

The result of an addition calculation is 1999.69 grams. But the 'worst' number in the addition had its uncertainty in the 'hundreds' place, three places in front of the decimal point!Which value should be reported as the final result? 1.9 x 10^3 grams 19 grams 20. grams 2.0 x 10^3 grams 2.0 x 10^-3 grams

2.0 x 10^3 grams

Consider the reaction below for the fermentation of glucose, C6H12O6. How many moles of carbon dioxide are produced when the glucose in 500.0 mL of a 2.00 M glucose solution decomposes? C6H12O6 (aq) → 2 C2H5OH (aq) + 2 CO2 (g) 4.00 moles CO2 1.00 moles CO2 2 moles CO2 0.500 moles CO2 2.00 moles CO2

2.00 moles CO2

How many moles of ClO2 gas would be produced from the reaction of 4.00 liters of a 0.500 M NaClO2 solution? 2 NaClO2 (aq) + Cl2 (g) → 2 ClO2 (g) + 2 NaCl (aq) 2 moles ClO2 2.00 moles ClO2 4.00 moles ClO2 0.500 moles ClO2 1.00 moles ClO2

2.00 moles ClO2

The mass value 1999.69 grams, correctly rounded to three significant figures, should be written as: 2.00 x 10^2 grams 2.00 x 10^3 grams 199 grams 200 grams 1.99 x 10^3 grams

2.00 x 10^3 grams

Complete this Avogadro's Statement for the element hydrogen by supplying the missing mass: 1 mole of hydrogen gas = 6.02 x 10^23 H2 molecules = ____ 2.016 amu 1.204 x 10^24 grams 1.008 grams 2.016 grams 1.008 amu

2.016 grams

Complete this Avogadro's Statement for the element hydrogen:1 mole of Hydrogen gas = 6.02 x 10^23 H2 molecules = ____ (number) ____ (unit) 2.016 grams 1.204 x 10^24 grams 1.008 amu 1.008 grams 2.016 amu

2.016 grams

In an experiment to find the density of a sample of metal, mass and volume measurements are made, and the calculation below is performed. (57.675 g- 3.047 g)/(25.65 mL -0.15 mL) = 2.1422745098 g/mL Express this result with the appropriate number of decimal places/significant figures. 2.1422 g/mL 2.142 g/mL 2.14 g/mL 2.1423 g/mL 2.1 g/mL

2.142 g/mL

Consider the balanced chemical equation below for the decomposition of potassium chlorate, KClO3. How many moles of oxygen gas would be produced from the decomposition of 1.50 moles of KClO3? 2KClO3 --> 2KCl + 3O2 2.25 moles of oxygen gas 2.75 moles of oxygen gas 2.50 moles of oxygen gas 3.00 moles of oxygen gas 3.50 moles of oxygen gas

2.25 moles of oxygen gas

Which is the correct measurement of the length of this paper clip? 2.70 cm 2.7 cm 2.07 cm 2.75 cm

2.7 cm

The density of a block of wood is calculated after measuring its length, width, and height, and then its mass: 23.423 grams /(2.15 cm × 1.1 cm × 3.73 cm) The final result should be reported as: 45 g/cm^3 2.66 g/cm^3 2.6552 g/cm^3 2.7 g/cm^3 3.0 g/cm^3

2.7 g/cm^3

The density of a block of wood is calculated after measuring its length, width, and height, and then its mass: 23.423 grams/(2.15 cm × 1.1 cm × 3.73 cm) The final result should be reported as: 2.6552 g/cm^3 45 g/cm^3 2.66 g/cm^3 3.0 g/cm^3 2.7 g/cm^3

2.7 g/cm^3

Which is the correct measurement of the length of this paper clip? 2.07 cm 2.75 cm 2.7 cm 2.70 cm 2.700 cm

2.70 cm

Ringer's Solution, used in the treatment of burns and other wounds, is prepared by dissolving 0.330 grams of CaCl2, 8.60 grams of NaCl, and 0.300 grams of KCl in enough water to bring the total volume to 1.00 x 10^3 mL. Determine the molarity of the CaCl2 in the Ringer's Solution. 0.330 moles CaCl2/liter 2.97 x 10^-3 moles CaCl2/liter 3.66 x 10^-2 moles CaCl2/liter 4.37 x 10^-3 moles CaCl2/liter 2.49 x 10^-2 moles CaCl2/liter

2.97 x 10^-3 moles CaCl2/liter

Ringer's Solution, used in the treatment of burns and other wounds, is prepared by dissolving 0.330 grams of CaCl2, 8.60 grams of NaCl, and 0.300 grams of KCl in enough water to bring the total volume to 1.00 x 10^3 mL. Determine the molarity of the CaCl2 in the Ringer's Solution. 4.37 x 10^-3 moles CaCl2/liter 3.66 x 10^-2 moles CaCl2/liter 0.330 moles CaCl2/liter 2.97 x 10^-3 moles CaCl2/liter 2.49 x 10^-2 moles CaCl2/liter

2.97 x 10^-3 moles CaCl2/liter

If consuming antacids and proton pump inhibitors causes stomach pH to increase from pH 2 to pH 4, the hydronium ion concentration becomes 20 times lower 100 times lower 20 times higher 2 times higher 100 times higher 2 times lower

20 times higher

Which unit conversion would allow you to convert 21.0 gallons into milliliters? Given English and English-metric unit relationships: 1 liter = 1.057 quarts, 1 gallon = 4 quarts

21.0 gal (4 qt/1 gal)(1 L/1.057 qt)(10^3 mL/1 L)

Consider the balanced chemical equation below, which describes the combustion of ethane, C2H6. If 7.00 moles of ethane was burned, how many moles of water would be produced? 2 C2H6 + 7O2 --> 4CO2 + 6H2O 18.0 moles of water 21.0 moles of water 14.0 moles of water 6.00 moles of water 12.0 moles of water

21.0 moles of water

Consider the balanced chemical equation below, which describes the combustion of ethane, C2H6. If 7.00 moles of ethane was burned, how many moles of water would be produced? 2C2H6 + 7O2 --> 4CO2 + 6H2O 18.0 moles of water 12.0 moles of water 14.0 moles of water 21.0 moles of water 6.00 moles of water

21.0 moles of water

Express this measurement in standard notation: 2.35 x 10^4 grams. Be sure to consider the significant figures in this measurement, and the decimal place that contains the uncertainty. 0.000235 grams 23,500 grams 23,500. grams 235 grams 23,500.0 grams

23,500 grams

If 22.5 L of nitrogen gas is stored at 748 mm Hg, what will be the new volume is the pressure is reduced to 725 mm Hg at constant temperature? 19.l L 23.2 L 21.8 L 28.5 L

23.2 L

Which is the correct measurement of the length of this paper clip? 20.75 cm 27 cm 20.7 cm 27.5 cm 27.0 cm

27 cm

Which is the correct measurement of the length of this paper clip? 27.0 cm 20.7 cm 27 cm 20.75 cm 27.5 cm

27 cm

An Avogadro's number of elemental nitrogen (N2 molecules) would have a mass of: 6.02 x 10^23 grams 14.01 amu 28.02 grams 28.02 amu 14.01 grams

28.02 grams

Write a balanced chemical equation for the neutralization reaction of phosphoric acid with magnesium hydroxide. H3PO4 + 2Mg(OH)2 → Mg3(PO4)2 + 3H2O 2H3PO4 + 3Mg(OH)2 → Mg2(PO4)3 + 6H2O H3PO4 + 3Mg(OH)2 → Mg3(PO4)2 + 3H2O 2H3PO4 + 3Mg(OH)2 → Mg3(PO4)2 + 6H2O

2H3PO4 + 3Mg(OH)2 → Mg3(PO4)2 + 6H2O

Consider the balanced chemical equation below for the decomposition of potassium chlorate, KClO3. How many moles of potassium chloride would be produced from the decomposition of 3.00 moles of KClO3? 2KClO3 --> 2 KCL + 3O2 1.00 mole of potassium chloride 5.00 moles of potassium chloride 4.00 moles of potassium chloride 2.00 moles of potassium chloride 3.00 moles of potassium chloride

3.00 moles of potassium chloride

Determine the number of moles of zinc chloride in 1.00 x 10^2 mL of a 0.300 M ZnCl2 solution. 30.0 moles ZnCl2 3.00 moles ZnCl2 3.00 x 10^-2 moles ZnCl2 0.300 moles ZnCl2 0.030 moles ZnCl2

3.00 x 10^-2 moles ZnCl2

Determine the number of moles of zinc chloride in 1.00 x 10^2 mL of a 0.300 M ZnCl2 solution. 30.0 moles ZnCl2 0.030 moles ZnCl2 3.00 x 10^-2 moles ZnCl2 0.300 moles ZnCl2 3.00 moles ZnCl2

3.00 x 10^-2 moles ZnCl2

A gas balloon has a volume of 100.0 L at 25.0 °C and 1 atm pressure. It is tied to a cinder block and dropped into the Bay. It comes to rest on the bottom where the temperature is 12.0 °C. The volume of the balloon is now 31 liters. What is the water pressure in atms? 6.72 atm 0.296 atm 3.37 atm 3.09 atm

3.09 atm

What mass of ammonia is needed to prepare 7.50 x 10^2 mL of a 0.250 M NH3 solution? 3.19 grams NH3 9.08 x 10^-2 grams NH3 31.9 grams NH3 9.08 grams NH3 4.26 grams NH3

3.19 grams NH3

What mass of ammonia is needed to prepare 7.50 x 10^2 mL of a 0.250 M NH3 solution? 31.9 grams NH3 4.26 grams NH3 3.19 grams NH3 9.08 grams NH3 9.08 x 10^-2 grams NH3

3.19 grams NH3

Consider the balanced chemical equation below, which describes the combustion of ethane, C2H6. How many moles of ethane would need to be burned to produce 7.50 moles of carbon dioxide? 2C2H6 + 7O2 --> 4CO2 + 6H2O 3.75 moles of ethane 2.50 moles of ethane 3.50 moles of ethane 5.50 moles of ethane 15.0 moles of ethane

3.75 moles of ethane

A gas tank holds 2785 L of propane at 830.0 mm Hg. What is the volume of the propane at standard pressure? 3042 L 1492 L 2550 L 5592 L

3042 L

In working Gas Law calculations, we use the Kelvin temperature scale, rather than Celsius. But since most temperatures are measured in Celsius, it's essential to be able to convert between the two scales. Convert a temperature of 45 oC into a Kelvin temperature. 318 K -228 K -45 K 228 K

318 K

An Avogadro's number of oxygen molecules (O2) would have a mass of: 16.00 amu 32.00 amu 16.00 grams 32.00 grams 6.02 x 10^23 grams

32.00 grams

An Avogadro's number of oxygen molecules (O2) would have a mass of: 16.00 amu 32.00 grams 16.00 grams 32.00 amu 6.02 x 10^23 grams

32.00 grams

An atom with 15 protons, 15 electrons, and 17 neutrons will have the isotopic symbol: 45Ge 47Zn 32P 32Cl 47P

32P

The measured value 0.00720 grams, correctly expressed in scientific notation, would be: 7.20 x 10^2 grams 7.2 x 10^3 grams 7.20 x 10^-2 grams 7.2 x 10^-3 grams 7.20 x 10^-3 grams

7.20 x 10^-3 grams

What pressure is required to compress 196 liters of air at 1.00 atmosphere into a gas cylinder whose volume is 26.0 liters at constant temperature? 7.54 atm 0.133 atm 8.67 atm 5.39 atm

7.54 atm

How many ml of 0.125 M NaOH would be needed to titrate 20.00 ml of 0.150 M H3PO4? 48 mL of NaOH 40 mL of NaOH 72 mL of NaOH 64 mL of NaOH

72 mL of NaOH

The mass of one mole of calcium hydroxide, Ca(OH)2, is 73.09 grams 74.10 grams 57.09 grams 58.10 grams

74.10 grams

Which unit conversion would allow you to convert 75.0 grams of hydrogen gas, H2, into moles? 75.0 grams H2 (1.008 grams H2/1 mole H2) = 75.0 grams H2 (1 mole H2/1.008 grams H2) = 75.0 grams H2 (2.016 grams H2/1 mole H2) = 75.0 grams H2 (1 mole H2/2.016 grams H2) =

75.0 grams H2 (1 mole H2/2.016 grams H2) =

Which unit conversion would allow you to convert 75.0 grams of hydrogen gas, H2, into moles? 75.0 grams H2 (1.008 grams H2/1 mole H2) = 75.0 grams H2 (2.016 grams H2/1 mole H2) = 75.0 grams H2 (1 mole H2/1.008 grams H2) = 75.0 grams H2 (1 mole H2/2.016 grams H2) =

75.0 grams H2 (1 mole H2/2.016 grams H2) =

Suppose the speedometer in your car reads 55.0 mph. What is your speed in km/hour? Set up and solve the unit conversion. Given English-metric unit relationship: 1 km = 0.621 mile 0.0291 km/hour 0.0113 km/hour 34.1 km/hour 88.6 km/hour

88.6 km/hour

A crime investigation team finds that an entry wound is 0.36 inch in diameter. Which of the following guns was likely to have been used in the shooting? Set up and solve the unit conversion. Given English-metric unit relationship: 1 inch = 2.54 cm 9 mm Beretta 200 mm Howitzer 12 mm Uzi 0.5 cm pellet gun

9 mm Beretta

A gas balloon has a volume of 106.0 liters when the temperature is 45.0 °C and the pressure is 740.0 mm of mercury. What will the balloon's volume at 20.0 °C and 780 .0 mm of mercury pressure? 44.7 L 103.0 L 92.7 L 109.1 L

92.7 L

Ethanol (ethyl alcohol) has a density of 0.789 g/mL at 25°C. If 75.5 g of alcohol is needed for a reaction, what volume in milliliters should be used? Set up and solve the unit conversion. 0.0105 mL 59.6 mL 95.7 mL 78.9 mL

95.7 mL

Work this calculation:107.2 g + 0.0234 g - 7.365 g = ? The result should be reported as: 99.9 g 99.8584 g 99.86 g 99.858 g 100.0 g

99.9 g

A person can not walk though a brick wall because... A brick wall is a collection of liquid particles which have very strong adhesive forces holding it together. A brick wall is a collection of gas particles which have very weak adhesive forces holding it together. A brick wall is a collection of solid particles which have very strong adhesive forces holding it together. A brick wall is a collection of solid particles which have very weak adhesive forces holding it together.

A brick wall is a collection of solid particles which have very strong adhesive forces holding it together.

What is a colligative property? A colligative property is a solution property that depends only on the concentration of solute particles. A colligative property is a solution property that depends only on the basic nature of the solute particles . A colligative property is a solution property that depends only on the acidic nature of the solute particles. A colligative property is a solution property that depends only on the ionic nature of the solute particles.

A colligative property is a solution property that depends only on the concentration of solute particles.

What is a micelle? A micelle is an aggregate (or supramolecular assembly) of surfactant molecules dispersed in a liquid colloid. A micelle is an aggregate (or supramolecular assembly) of surfactant molecules dispersed in a liquid solution. A micelle is a single surfactant molecule dispersed in a liquid colloid. A micelle is a single surfactant molecules dispersed in a liquid solution.

A micelle is an aggregate (or supramolecular assembly) of surfactant molecules dispersed in a liquid colloid.

What is an Arrhenius acid? An Arrhenius acid is a compound that ionizes in water to produce hydronium ions. An Arrhenius acid is a compound that absorbs hydronium ions in water. An Arrhenius acid is a compound that dissolves in water. An Arrhenius acid is a compound that ionizes in water to produce hydroxide ions.

An Arrhenius acid is a compound that ionizes in water to produce hydronium ions.

What is true of an acidic solution? An acidic solution contains more hydroxide ions than hydronium ions. An acidic solution contains the same number of hydronium ions as hydroxide ions. An acidic solution contains more OH- ions than H3O+ ions. An acidic solution contains more hydronium ions than hydroxide ions.

An acidic solution contains more hydronium ions than hydroxide ions.

What is true of an alkaline solution? An alkaline solution has more hydroxide ions than hydronium ions. An alkaline solution has the same number of hydroxide ions as hydrondium ions. An alkaline solution contains more H3O+ ions than OH- ions. An alkaline solution has more hydrondium ions than hydroxide ions.

An alkaline solution has more hydroxide ions than hydronium ions.

One of the key skills in Chapter 4 is classifying compounds as either ionic (electrons transferred) or molecular (electrons shared), based on the combination of elements in the compound's chemical formula. Now that you're learning about electronegativity (the electron-pulling power of elements), you can further classify the molecular compounds as having either polar or nonpolar covalent bonds. Which compound below has polar covalent bonds? CoF3 PbF2 CH2F2 MgF2 SnF2

CH2F2

In which of these carbon compounds is the carbon atom in its most reduced form (lowest oxidation state)? HCOOH CH3OH CH4 CH2O CO2

CH4

In which of these carbon compounds is the carbon atom in its most oxidized form (highest oxidation state)? CH4 CO2 CH3OH CH2O HCOOH

CO2

In which of these carbon compounds is the carbon atom in its most oxidized form (highest oxidation state)? CO2 CH4 HCOOH CH3OH CH2O

CO2

Which of these molecular compounds has a Lewis structure that contains four lone pairs of electrons? CH4O CO2 H2O CH3Cl N2H4

CO2

Which of these molecular compounds has a Lewis structure that contains four lone pairs of electrons? CO2 N2H4 CH3Cl H2O CH4O

CO2

Classify both condensation and boiling. Condensation and boiling are both exothermic. Condensation and boiling are both endothermic. Condensation is endothermic and boiling is exothermic. Condensation is exothermic and boiling is endothermic

Condensation is exothermic and boiling is endothermic

Consider the ionic compound that forms when calcium metal chemically combines with the non-metal phosphorus. What is the chemical formula for that ionic compound? (What is the fixed proportion in which these ions combine?) Ca2P3 CaP3 CaP Ca3P2 Ca2P

Ca3P2

When 1 mole of Ca(OH)2 chemically reacts with 1 mole of H2SO4, what salt is formed? Ca2SO4 is the salt formed. Ca(OH)2 is the salt formed CaOH is the salt formed. CaSO4 is the salt formed.

CaSO4 is the salt formed.

When 1 mole of Ca(OH)2 chemically reacts with 1 mole of H2SO4, what salt is formed? CaOH is the salt formed. Ca2SO4 is the salt formed. Ca(OH)2 is the salt formed CaSO4 is the salt formed.

CaSO4 is the salt formed.

What is true about fog? Fog is a true solution where air is the solute and water droplets are the solvent. Fog is a colloidal suspension where air is are the dispersed phase and water droplets are the dispersing medium. Fog is a true solution where water droplets are the solute and air is the solvent. Fog is a colloidal suspension where water droplets are the dispersed phase and air is the dispersing medium.

Fog is a colloidal suspension where water droplets are the dispersed phase and air is the dispersing medium.

Which state of matter has very weak internal cohesive forces, is very compressible and can not keep its own volume or its own shape. Solid Liquid Gas Gel

Gas

Consider the balanced chemical equation below for the reaction of zinc metal with hydrochloric acid (aqueous HCl). Which element is being reduced? Zn + 2HCL --> H2 + ZNCl2 Zn of the zinc metal Cl in HCl H in HCl

H in HCl

Acids and bases are defined as substances that donate or accept: OH- H2O H+ H3O+

H+

Which of these covalent bonds would be considered nonpolar? H-F H-N H-C H-O

H-C

Which of these covalent bonds would be the most polar (have the strongest partial charges on the atoms)? H-F H-C H-N H-O

H-F

Acids and bases are defined as substances that donate or accept: H2O H+ OH- H3O+

H3O+

Which of these is the correct formula and charge for the hydronium ion? H2O+ OH- OH+ H3O- H3O+

H3O+

Which of these is the correct formula and charge for the hydronium ion? OH+ OH- H3O- H3O+ H2O+

H3O+

Which of these is the correct formula and charge for the hydroxide ion? H3O- H3O+ H2O+ OH- OH+

H3O+

Which is phosphoric acid HNO3 HBr H2SO4 H3PO4

H3PO4

Which of these molecular compounds would have a Lewis structure that contains a total of 10 valence electrons? H2O NH3 CO2 CH3Cl HCN

HCN

Which of these molecular compounds would have a Lewis structure that contains a total of 10 valence electrons? NH3 CO2 H2O CH3Cl HCN

HCN

Write a balanced chemical equation for the neutralization reaction of hydrochloric acid with sodium hydroxide. HCl + NaOH → NaCl + H2O 2HCl + NaOH → NaCl + 2H2O HCl + 2NaOH →2NaCl + H2O 2HCl + 2NaOH → 2NaCl + 2H2O

HCl + NaOH → NaCl + H2O

Which one of these compounds is an acid? NaCl is an acid. NaOH is an acid HCl is an acid. NH3 is an acid.

HCl is an acid.

Which is hydrofluoric acid HCl HF HOCl HBr

Chemical equations can be balanced by changing the numerical subscripts in the chemical formulas of the reactant and product compounds. True False

False

Cyclohexane (C6H12) would be a good solvent for ionic compounds. True False

False

If the temperature of a sample of gas is increased, either the pressure or the volume or both must decrease. True False

False

In the kinetic molecular theory, the mobility of particles is a direct function of their temperature, and absolute zero corresponds to the temperature at which particle motion will cease. This temperature value is 0 oC. True False

False

Metal atoms tend to lose protons when they react with nonmetal atoms to form an ionic compound. True False

False

Nonmetal atoms tend to gain protons when they react with metal atoms to form an ionic compound. True False

False

Some chemical reactions involve only an atom being oxidized, with no reduction reaction taking place. True False

False

The advantage of using Celsius temperatures to work gas law problems is that the Celsius scale has no negative temperature values. True False

False

The components within a compound can be separated on the basis of differences in their physical properties (e.g., freezing point, boiling point, solubility). True False

False

The covalent bonds within a polar molecule are usually broken when the substance dissolves in water. True False

False

The covalent bonds within the molecules are broken when a molecular compound like water boils and undergoes the phase change from liquid to gas. True False

False

The geometry of the central atom in a Lewis structure is determined by its bonds to other atoms. Lone pairs of electrons don't play a significant role in determining the spatial arrangement of the atoms bonded to the central atom in a molecule. True False

False

The molarity concentration unit is defined as moles of solute per liter of solvent. True False

False

The molecular compounds HCl and HBr are capable of hydrogen bonding with one another. True False

False

The weak acid lactic acid has an acid dissociation constant value Ka = 1.8 x 10^-4. A 0.10 M solution of lactic acid should have a pH value = -log(1.8 x 10^-4) = 3.85. True False

False

To convert 125 micrograms to grams, You would multiply 125 micrograms by the conversion factor: (106 μg/1 g) True False

False

To convert 678 centimeters to meters, you would multiply 678 cm by the conversion factor: (1 m/10^-2 cm) True False

False

When one nonmetal atom shares electrons (forms a covalent bond) with another, the driving force is always to achieve the stability of an octet of electrons: the s2p6 electron configuration of every noble gas. True False

False

When used in the unit relationship 1 dozen eggs = 12 eggs, the number 12 has two significant figures. True False

False

Which of these is the correct symbol for the element iron? Fe In Ir Rn I

When 1 mole of Fe(OH)3 chemically reacts with 1 mole of H3PO4, what salt is formed? Fe(OH)3 is the salt formed. H3PO4 is the salt formed. Fe3(PO4)2 is the salt formed. FePO4 is the salt formed.

FePO4 is the salt formed.

Write a balanced chemical equation for the neutralization reaction of nitric acid with potassium hydroxide. HNO3 + KOH → 2KNO3 + H2O HNO3 + 2KOH → KNO3 + H2O HNO3 + KOH → KNO3 + 2H2O HNO3 + KOH → KNO3 + H2O

HNO3 + KOH → KNO3 + H2O

If you can spill it into a puddle, it is most likely... In a solid state In a gaseous state. In a liquid state. Unable to tell.

In a liquid state.

If you can smell it in the air, it is most likely .. In the Liquid state In the solid state In the gaseous state Unable to tell.

In the gaseous state

If you can pick it up with chop sticks, it is most likely... In the gaseous state In the liquid state In the solid state Un able to tell.

In the solid state

Refer to the energy level diagram below. Which letter corresponds to the change in enthalpy (ΔH) for the forward reaction? N L P M K O

Refer to the energy level diagram below. Which letter corresponds to the change in enthalpy (ΔH) for the forward reaction? P N M O K L

Which state of matter has strong internal cohesive forces, is not very compressible and has its own volume but can not keep its own shape. Solid Gas Liquid Dark matter

Liquid

Which two states of matter DO NOT have a definite shape? Liquids and solids do not have definite shape. Solids and gases do not have definite shape. Liquids and gases do not have definite shape. Only gases do not have definite shape.

Liquids and gases do not have definite shape.

The video lesson showed Lewis Structures for two elements that exist as diatomic molecules: hydrogen (H2) and fluorine (F2). Which diatomic molecule below would have to contain a triple bond in order for each atom to achieve its octet? N2 Cl2 O2 Br2

Which is ammonia. NH3 KOH H3PO4 NaOH

NH3

When 1 mole of NH4OH chemically reacts with 1 mole of HC2H3O2, what salt is formed? NH4OH is the salt, HC2H3O2, is the salt. NH4C2H3O2, is the salt. NH4(C2H3O2)2, is the salt.

NH4C2H3O2, is the salt.

The video lesson showed Lewis Structures for two elements that exist as diatomic molecules: hydrogen (H2) and fluorine (F2). Which diatomic molecule below would have to contain a double bond in order for each atom to achieve its octet? Cl2 N2 O2 Br2

The video lesson showed Lewis Structures for two elements that exist as diatomic molecules: hydrogen (H2) and fluorine (F2). Which diatomic molecule below would have to contain a double bond in order for each atom to achieve its octet? N2 Cl2 O2 Br2

If you tried to use a can a spray paint in sub-zero weather, what would you expect to happen... Paint spray is vigorous because the sub-zero temperature has increased the pressure inside the paint can. Paint spray is vigorous because the sub-zero temperature has decreased the pressure inside the paint can. Paint spray is very weak because the sub-zero temperature has decreased the pressure inside the paint can. Paint spray is very weak because the sub-zero temperature has increased the pressure inside the paint can.

Paint spray is very weak because the sub-zero temperature has decreased the pressure inside the paint can.

In which form is sulfur most highly oxidized (in the highest oxidation state)? PbS2 H2S S Na2S SO2

SO2

What is true about sea water? Sea water is a true solution where NaCl is the solvent and water is the major solute. Sea water is a true solution where water is the solvent and NaCl is the major solute. Sea water is a colloidal suspension where NaCl is the dispersing medium and water is the major dispersed phase. Sea water is a colloidal suspension where water is the dispersing medium and NaCl is the major dispersed phase.

Sea water is a true solution where water is the solvent and NaCl is the major solute.

In which compound does the metal have the highest oxidation number? Na2O CuO SnO2 Al2O3 Fe2O3

SnO2

Under what conditions is a chemical process always spontaneous. System is exergonic and the entropy is decreasing. System is exergonic and the entropy is increasing. System is endergonic and the entropy is decreasing. System is endergonic and the entropy is increasing.

System is exergonic and the entropy is increasing.

Under what conditions is a chemical process always spontaneous. System is exergonic and the entropy is increasing. System is endergonic and the entropy is increasing. System is endergonic and the entropy is decreasing. System is exergonic and the entropy is decreasing.

System is exergonic and the entropy is increasing.

Which element has the distinguishing electron 5p4? Cr Te Mo Pm Po

Which element has the distinguishing electron 5p4? Po Mo Pm Cr Te

According to the Bronsted-Lowry theory, what is the Bronsted-Lowry base in the following equation, HNO2 + H2O <==> H3O+ + NO2- The Bronsted-Lowry base is HNO2 The Bronsted-Lowry base is H2O The Bronsted-Lowry base is H3O+ The Bronsted-Lowry base is NO2-

The Bronsted-Lowry base is H2O

According to the Bronsted-Lowry theory, what is the Bronsted-Lowry base in the following equation, NH3 + H2O <==> OH- + NH4+ The Bronsted-Lowry base is H2O The Bronsted-Lowry base is OH- The Bronsted-Lowry base is NH3 The Bronsted-Lowry base is NH4+

The Bronsted-Lowry base is NH3

Which is NOT part of the Kinetic Molecular theory? The motion of atomic particles increases as the surrounding temperature increases. At the same temperature, smaller particles move more quickly that larger particles. The motion of atomic particles decreases as the surrounding temperature increases Pressure of a gas is a measure of the number of hits the gas molecules have on its container.

The motion of atomic particles decreases as the surrounding temperature increases

When a Solid becomes a Liquid this is called.... This is an Endothermic process called Melting. This is an Endothermic process called Evaporation. This is an Exothermic process called Condensation. This is an Exothermic process called Freezing.

This is an Endothermic process called Melting.

When a Solid becomes a Gas, this is called... This is an Exothermic process called Depositon. This is an Exothermic process called Evaporation. This is an Endothermic process called Sublimation. This is an Endothermic process called Fusion.

This is an Endothermic process called Sublimation.

When a Liquid becomes a Gas, this is called ... This is an Exothermic process called Crystallization. This is an Exothermic process called Deposition. This is an Endothermic process called Vaporization. This is an Endothermic process called Liquefaction.

This is an Endothermic process called Vaporization.

When a Gas becomes a Liquid, this is called... This is an Endothermic process called Liquefaction. This is an Exothermic process called Evaporation. This is an Exothermic process called Condensation. This is an Endothermic process called Vaporization.

This is an Exothermic process called Condensation.

When a Gas becomes a Solid, this is called... This is an Exothermic process called Deposition. This is an Endothermic process called Vaporization. This is an Exothermic process called Condensation. This is an Endothermic process called Sublimation.

This is an Exothermic process called Deposition.

When a Liquid becomes a Solid, this is called... This is an Exothermic process called Freezing. This is an Endothermic process called Evaporation. This is an Exothermic process called Liquefaction. This is an Endothermic process called Fusion.

This is an Exothermic process called Freezing.

What is the Tyndall effect? The Tyndall effect is the linear passage of light through a colloidal suspension. The Tyndall effect is the linear passage of light as it pass through a liquid solution. The Tyndall effect is the scatter of light as it pass through a colloidal suspension. The Tyndall effect is the scatter of light as it pass through a liquid solution.

The Tyndall effect is the scatter of light as it pass through a colloidal suspension.

Not all ionic compounds are soluble in water. NaCl is highly soluble in water but AgCl is insoluble even in hot water. Why do you think this is so? The attractive ionic forces in the AgCl lattice are weaker that the attractive forces of the energetic hot water molecules to the Ag and Cl ions. The attractive ionic forces in the AgCl lattice are weaker that the repulsive forces of the energetic hot water molecules to the Ag and Cl ions. The attractive ionic force in the AgCl lattice are stronger that the attractive forces of the energetic hot water molecules to the Ag and Cl ions. The attractive ionic forces in the AgCl lattice are stronger that the repulsive forces of the energetic hot water molecules to the Ag and Cl ions.

The attractive ionic force in the AgCl lattice are stronger that the attractive forces of the energetic hot water molecules to the Ag and Cl ions.

How are the boiling point and the freezing point affected by the addition of a dissolved solute? The boiling point is elevated and the freezing point is depressed. The boiling point is depressed and the freezing point is depressed. The boiling point is depressed and the freezing point is elevated. The boiling point is elevated and the freezing point is elevated.

The boiling point is elevated and the freezing point is depressed.

According to the Bronsted-Lowry theory, what is the conjugate acid in the following equation, NH3 + H2O <==> OH- + NH4+ The conjugate acid is OH- The conjugate acid is H2O The conjugate acid is NH3 The conjugate acid is NH4+

The conjugate acid is NH4+

According to the Bronsted-Lowry theory, what is the conjugate base in the following equation, NH3 + H2O <==> OH- + NH4+ The conjugate base is NH3 The conjugate base is H2O The conjugate base is OH- The conjugate base is NH4+

The conjugate base is OH-

What is the dispersed phase. The dispersed phase is the name for the substance present in a colloidal dispersion in amounts less than the major component called the dispersing medium. The dispersed phase of a colloidal dispersion is analogous to the solute of a solution. The dispersed phase is the name for the substance present in greatest amount in a colloidal dispersion. The dispersed phase of a colloidal dispersion is analogous to the solvent of a solution. The dispersed phase is the name for the substance present in a colloidal dispersion in greatest amount. The dispersed phase of a colloidal dispersion is analogous to the solute of a solution. The dispersed phase is the name for the substance present in a colloidal dispersion in amounts less than the major component called the dispersing medium. The dispersed phase of a colloidal dispersion is analogous to the solvent of a solution.

The dispersed phase is the name for the substance present in a colloidal dispersion in amounts less than the major component called the dispersing medium. The dispersed phase of a colloidal dispersion is analogous to the solute of a solution.

What is the dispersing medium? The dispersing medium is the name for the substance in a colloidal dispersion in the lesser amount, which is analogous to the solvent in a true solution. The dispersing medium is the name for the substance in a colloidal dispersion in the largest amount, which is analogous to the solvent in a true solution. The dispersing medium is the name for the substance in a colloidal dispersion in the largest amount, which is analogous to the solute in a true solution. The dispersing medium is the name for the substance in a colloidal dispersion in the smaller amount, which is analogous to the solute in a true solution.

The dispersing medium is the name for the substance in a colloidal dispersion in the largest amount, which is analogous to the solvent in a true solution.

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: the equilibrium mixture is transferred to a container with a much greater volume. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would increasing the volume of the equilibrium mixture affect the concentration of Cl2 gas? decrease increase can't be determined no change

decrease

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: the reaction system is heated by placing the reaction container in an hot water bath. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would increasing the temperature affect the concentration of HCl? decrease increase can't be determined no change

decrease

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: the reaction system is heated by placing the reaction container in an hot water bath. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would increasing the temperature affect the concentration of HCl? no change increase can't be determined decrease

decrease

In the TedEd video lesson on increasing reaction kinetics, narrowing the hallways is analogous to: decreasing the volume of the reaction system adding more reactant particles to the volume of the reaction system increasing the reactant surface area increasing the temperature of the reaction system adding a catalyst to the reaction system

decreasing the volume of the reaction system

In a chemical equation, when the physical state of a substance is indicated as (aq), it means that the substance is a liquid acquired in a laboratory dissolved in water an Aquarius

dissolved in water

Atoms and ions are considered isoelectronic if they have the same: number of neutrons electron configuration number of protons number of outermost electrons

electron configuration

Two ions would be isoelectronic if they have the same: electron configuration number of neutrons number of valence electrons number of protons

electron configuration

Two ions would be isoelectronic if they have the same: electron configuration number of protons number of neutrons number of valence electrons

electron configuration

If energy is gained during a chemical reaction, then the reaction is said to be... endergonic exergonic exothermic isogonic

endergonic

If energy is gained during a chemical reaction, then the reaction is said to be... exergonic endergonic exothermic isogonic

endergonic

Which correctly describes the reverse reaction in this energy level diagram? endothermic, and ΔH is positive exothermic, and ΔH is negative endothermic, and ΔH is negative exothermic, and ΔH is positive

endothermic, and ΔH is positive

Which correctly describes the reverse reaction in this energy level diagram? exothermic, and ΔH is negative endothermic, and ΔH is positive exothermic, and ΔH is positive endothermic, and ΔH is negative

endothermic, and ΔH is positive

If energy is lost during a chemical reaction, then the reaction is said to be... endothermic endergonic exergonic isogonic

exergonic

Which correctly describes the forward reaction in this energy level diagram? endothermic, and ΔH is negative exothermic, and ΔH is positive endothermic, and ΔH is positive exothermic, and ΔH is negative

exothermic, and ΔH is negative

Which of these is not a physical property? boiling point solubility flammability density

flammability

Which of these is not a physical property? flammability density solubility boiling point

flammability

In which of the pairs below are both of the properties chemical properties? attracted to magnet; conducts electricity boils at 161 degrees C; flammable flammable; produces a gas when treated with bleach density of 0.78 g/mL; freezes at 25 degrees C decomposes when heated; dissolves in water

flammable; produces a gas when treated with bleach

In which of the pairs below are both of the properties chemical properties? density of 0.78 g/mL; freezes at 25o] degrees C flammable; produces a gas when treated with bleach attracted to magnet; conducts electricity boils at 161 degrees C; flammable decomposes when heated; dissolves in water

flammable; produces a gas when treated with bleach

In which of the pairs below are both of the properties chemical properties? flammable; produces a gas when treated with bleach density of 0.78 g/mL; freezes at 25 degrees C boils at 161 degrees C; flammable decomposes when heated; dissolves in water attracted to magnet; conducts electricity

flammable; produces a gas when treated with bleach

Which element has the smallest atomic radius (meaning smallest electron cloud)? fluorine cesium lithium iodine

fluorine

Which element has the smallest atomic radius (meaning smallest electron cloud)? iodine lithium fluorine cesium

fluorine

A 0.0010 M solution of the strong base NaOH would have a pH = 11. True False

True

A CHM 105 lab experiment requires the use of a 6.00 M HCl solution. The Beaupre stockroom has only 12.0 M HCl. Doubling the volume of a sample of 12.0 M HCl with water will produce a 6.00 M HCl solution. True False

True

A neutral aqueous solution has the same hydronium ion concentration as a sample of pure water. True False

True

A reaction is non-spontaneous if the energy change is energonic. True False

True

A spontaneous reaction can occur slowly. True False

True

All of the transition elements are metals. True False

True

Atoms of nonmetal elements are reduced when they react with metal elements to form ionic compounds. True False

True

For the Representative Elements (also known as the Main Group Elements), the Group Number is equal to the number of valence electrons. True False

True

If the formula weight of the compound CaCl2 is 110.98 amu, then the mass of one mole of CaCl2 is 110.98 grams. True False

True

The components of a solution can be separated on the basis of differences in their physical properties (e.g., freezing point, boiling point, solubility). True False

True

The intermolecular attractive forces between solute and solvent particles are an important consideration in predicting the solubility of a given solute in a particular solvent. True False

True

The ionic bonds in a salt crystal are broken when an ionic compound (like NaCl) dissolves in water. True False

True

To convert 175 inches into feet, you would multiply 175 inches by the conversion factor: (1 ft/ 12 in) True False

True

What is the effect on vapor pressure by dissolving a salt in water. Vapor pressure increases. Vapor pressure stays the same. Vapor pressure decreases.

Vapor pressure decreases.

What is the effect on vapor pressure of adding heat to a liquid? Vapor pressure goes down. Vapor pressure goes up. Vapor pressure stays the same.

Vapor pressure goes up.

A person can swim in water because... Water is a solid and the particles have only a weak adhesion to each other. Water is a gas and the particles have only a strong adhesion to each other. Water is a liquid and the particles have only a weak adhesion to each other. Water is a liquid and the particles have only a strong adhesion to each other.

Water is a liquid and the particles have only a weak adhesion to each other.

Apply the Classification System of Matter to sodium chloride, commonly known as table salt. Sodium chloride is best classified as: a compound an element a homogeneous mixture a heterogenous mixture

a compound

Apply the Classification System of Matter to sodium chloride, commonly known as table salt. Sodium chloride is best classified as: a homogeneous mixture an element a heterogenous mixture a compound

a compound

Apply the Classification System of Matter to sodium chloride, commonly known as table salt. Sodium chloride is best classified as: an element a compound a homogeneous mixture a heterogenous mixture

a compound

Tropicana Pure Premium Lots-of-Pulp Orange Juice is labeled "100% Pure." This orange juice would be classified as: a compound a heterogeneous mixture a solution an element a pure substance

a heterogeneous mixture

Tropicana Pure Premium Lots-of-Pulp Orange Juice is labeled "100% Pure." This orange juice would be classified as: a pure substance an element a heterogeneous mixture a compound a solution

a heterogeneous mixture

Tropicana Pure Premium Lots-of-Pulp Orange Juice is labeled "100% Pure." This orange juice would be classified as: a solution an element a heterogeneous mixture a pure substance a compound

a heterogeneous mixture

A higher pH value corresponds to a higher hydroxide ion concentration a higher hydronium ion concentration a lower hydroxide ion concentration a more acidic solution

a higher hydronium ion concentration

A lower pH value corresponds to a more basic solution a higher hydronium ion concentration a higher hydroxide ion concentration a lower hydronium ion concentration

a lower hydronium ion concentration

Names and Ka values for four weak acids are listed below. The Acid Dissociation equilibrium constant (Ka) describes the extent to which the acid dissociates in water: HA (aq) + H2O (l) ⇔ H3O+ (aq) + A- (aq) If a 0.10 M solution is made of each acid, which solution would have the highest concentration of hydronium ions? acetic acid (CH3COOH), Ka = 1.8 x 10^-5 hypochlorous acid (HOCl), Ka = 2.9 x 10^-8 hydrofluoric acid (HF), Ka = 6.6 x 10^-4 carbonic acid (H2CO3), Ka = 4.3 x 10^-7

acetic acid (CH3COOH), Ka = 1.8 x 10^-5

In the TedEd video lesson on increasing reaction kinetics, using a Matchmaker to facilitate students finding dance partners is analogous to: increasing the temperature of the reaction system adding a catalyst to the reaction system increasing the reactant surface area adding more reactant particles to the volume of the reaction system decreasing the volume of the reaction system

adding a catalyst to the reaction system

In the TedEd video lesson on increasing reaction kinetics, increasing the number of students is analogous to: decreasing the volume of the reaction system increasing the reactant surface area increasing the temperature of the reaction system adding a catalyst to the reaction system adding more reactant particles to the volume of the reaction system

adding more reactant particles to the volume of the reaction system

Which of these molecules would not be able to participate in hydrogen bonds with water molecules? CH3CH2CH2-O-CH3 CH3-CH2-CH2-NH-CH3 CH3CH2CH2-NH2 all of these can participate in hydrogen bonds with water

all of these can participate in hydrogen bonds with water

Which of these statements applies to s subshells? they contain a single s orbital they can hold a total of two electrons they have a spherical shape they are found in all of the energy levels (shells) of the atom all of these statements apply to s subshells

all of these statements apply to s subshells

What is the molecular geometry of the nitrogen atom labeled #2? linear trigonal bipyramidal tetrahedral trigonal pyramid bent trigonal planar octahedral

bent

What is the molecular geometry of the oxygen atom labeled #1? octahedral bent tetrahedral trigonal pyramid trigonal bipyramidal linear trigonal planar

bent

Which of these molecular hydrocarbon compounds has the largest molar mass? ethane, C2H6 propane, C3H8 methane, CH4 butane, C4H10 all have same molar mass, since atomic weight of carbon = 12.01, and atomic weight of hydrogen = 1.008

butane, C4H10

Which of these metals would not have a Roman numeral as part of its name in an ionic compound? calcium chromium copper manganese cobalt

calcium

Which of these metals would not have a Roman numeral as part of its name in an ionic compound? manganese copper chromium calcium cobalt

calcium

Which element would you predict to have the largest atomic radius (meaning largest electron cloud)? lithium cesium fluorine iodine

cesium

Two different molecules are isomers if they have the same chemical formula number of protons number of neutrons electron configuration number of valence electrons

chemical formula

Which two pieces of information are needed to determine the molar mass of a compound? Avogadro's number, atomic weights from Periodic Table chemical formula of the compound, atomic numbers from Periodic Table chemical formula of the compound, atomic weights from Periodic Table Avogadro's number, atomic numbers from Periodic Table chemical formula of the compound, Avogadro's number

chemical formula of the compound, atomic weights from Periodic Table

Which two pieces of information are needed to determine the molar mass of a compound? chemical formula of the compound, atomic numbers from Periodic Table chemical formula of the compound, Avogadro's number Avogadro's number, atomic weights from Periodic Table chemical formula of the compound, atomic weights from Periodic Table

chemical formula of the compound, atomic weights from Periodic Table

Which statement best explains why chlorine atoms have a smaller atomic radius than sodium atoms? chlorine has a higher effective nuclear charge, which pulls the shells closer chlorine has a higher atomic weight than sodium sodium is a metal; chlorine is a nonmetal Cl atoms have a larger radius than Na atoms, because Cl atoms have more electrons chlorine is to the right of sodium on the Periodic Table

chlorine has a higher effective nuclear charge, which pulls the shells closer

Which statement best explains why chlorine atoms have a smaller atomic radius than sodium atoms? chlorine has a higher effective nuclear charge, which pulls the shells closer chlorine is to the right of sodium on the Periodic Table Cl atoms have a larger radius than Na atoms, because Cl atoms have more electrons sodium is a metal; chlorine is a nonmetal chlorine has a higher atomic weight than sodium

chlorine has a higher effective nuclear charge, which pulls the shells closer

Which of these correctly describes the combination of elements in a compound? can be separated by a physical change combined in fixed proportion combined in variable proportion physical combination of two or more elements

combined in fixed proportion

Which of these correctly describes the combination of elements in a compound? can be separated by a physical change combined in fixed proportion physical combination of two or more elements combined in variable proportion

combined in fixed proportion

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: Cl2 gas is removed from the reaction container. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would removing Cl2 from the reaction container affect the concentration of HCl gas? no change increase decrease can't be determined

decrease

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: Cl2 gas is removed from the reaction container. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would removing Cl2 from the reaction container affect the concentration of HCl gas? no change increase can't be determined decrease

decrease

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: heat is removed by placing the reaction vessel in an ice bath. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would decreasing the temperature affect the concentration of HI? can't be determined no change increase decrease

decrease

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: more HCl gas is added to the reaction container. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would adding HCl to the reaction container affect the amount of I2 solid in the reaction mixture? increase decrease can't be determined no change

decrease

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: the external pressure is increased, so that the volume of the container decreases. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would increasing the volume of the equilibrium mixture affect the concentration of HCl gas? increase no change decrease can't be determined

increase

In the TedEd video lesson on increasing reaction kinetics, preventing students from traveling in packs is analogous to: decreasing the volume of the reaction system adding more reactant particles to the volume of the reaction system increasing the temperature of the reaction system increasing the reactant surface area adding a catalyst to the reaction system

increasing the reactant surface area

In the TedEd video lesson on increasing reaction kinetics, preventing students from traveling in packs is analogous to: increasing the reactant surface area adding a catalyst to the reaction system increasing the temperature of the reaction system adding more reactant particles to the volume of the reaction system decreasing the volume of the reaction system

increasing the reactant surface area

In the TedEd video lesson on increasing reaction kinetics, shortening the passing periods is analogous to: adding more reactant particles to the volume of the reaction system decreasing the volume of the reaction system increasing the temperature of the reaction system increasing the reactant surface area adding a catalyst to the reaction system

increasing the temperature of the reaction system

Which compound has a larger n-value? ionic MgO sucrose a non-electrolyte ionic NaCl ionic CaCl2

ionic CaCl2

If the electronegativity difference between two different elements is 2.3, which type of bond is likely to form when atoms of those elements chemically combine to form a compound? no way to tell nonpolar covalent bond ionic bond polar covalent bond

ionic bond

In comparing the relative strengths of the 'inter-particle' attractive forces available to ionic and molecular compounds, the strongest type (which results in solids with high melting points) is the: ionic bond dipole-dipole interaction (dipolar force) instantaneous dipole-dipole interaction (dispersion force) hydrogen bond

ionic bond

Which trio of elements below consists of transition elements? lithium, sodium, potassium magnesium, calcium, strontium neon, argon, krypton iron, cobalt, nickel silicon, germanium, arsenic

iron, cobalt, nickel

Consider a gas sample contained in a balloon. What happens to the density of the gas sample as the balloon is heated at constant pressure? it increases it could increase or decrease, depending on how much the gas is heated it decreases it remains the same

it decreases

Which statement is true for a neutral aqueous solution? it has a hydronium ion concentration of 1 x 10-7 M all of these are true for a neutral aqueous solution it has a pH = 7 it has a hydroxide ion concentration of 1 x 10-7 M it has hydroxide and hydronium in equal concentrations

it has a pH = 7

Compound X is insoluble in water, but quite soluble in the hydrocarbon solvent hexane (CH3CH2CH2CH2CH2CH3). What can you conclude about the nature of Compound X? it is an electrolyte it is nonpolar it is ionic it is electronegative it is polar

it is nonpolar

Which statement about the nucleus of the atom is correct? it contains only neutrons it is positively-charged it contains only protons it accounts for the positive charge and most of the volume of the atom. it contains protons and electrons

it is positively-charged

Which statement is correct regarding Avogadro's number? it has the value 6.02 x 10^-23 it is the mass in grams of one mole of any element or compound it is the number of molecules in one mole of any molecular substance it is the mass in atomic mass units (amu) of one mole of any substance

it is the number of molecules in one mole of any molecular substance

Iodine crystals are only slightly soluble in water, but extremely soluble in hexane (C6H14), a hydrocarbon solvent.What conclusion can you make about iodine? it's nonpolar it's ionic it's polar no conclusion

it's nonpolar

Iodine crystals are only slightly soluble in water, but extremely soluble in hexane (C6H14), a hydrocarbon solvent.What conclusion can you make about iodine? no conclusion it's nonpolar it's ionic it's polar

it's nonpolar

Which element is in the fourth period and Group VIIIA (commonly called Group 8)? cobalt krypton iron potassium nickel

krypton

Consider making this change to a balloon filled with one mole of helium: The balloon floats to a high altitude, where the external pressure is lower. Assume the temperature and the number of moles of helium inside the balloon remain constant. Does the volume of the balloon become larger, or smaller, or does it remain the same? remains the same larger smaller can't be determined

larger

Consider making this change to a balloon filled with one mole of helium: The balloon floats to a high altitude, where the external pressure is lower. Assume the temperature and the number of moles of helium inside the balloon remain constant. Does the volume of the balloon become larger, or smaller, or does it remain the same? smaller larger remains the same can't be determined

larger

Consider making this change to a balloon filled with one mole of helium: Two moles of helium are added to the balloon. Assume the temperature and pressure remain constant. Does the volume of the balloon become larger, or smaller, or does it remain the same? can't be determined smaller remains the same larger

larger

Consider making this change to a balloon filled with one mole of helium: Two moles of helium are added to the balloon. Assume the temperature and pressure remain constant. Does the volume of the balloon become larger, or smaller, or does it remain the same? smaller remains the same can't be determined larger

larger

You should think of an element's electronegativity value as a measure of its electron-pulling power: the ability of that atom to attract electrons toward itself. Every element on the Periodic Table has an electronegativity value; these were originally assigned by Dr. Linus Pauling (the two-time Nobel laureate). Electronegativity values for the most common Representative Elements are given in Table 4.4 of your Seager textbook (Skills Book page 114). Which element on has the greatest electronegativity (the most electron-pulling power)? iodine hydrogen lithium fluorine cesium

fluorine

Which set of elements are in the group known as the halogens? copper, silver, gold, platinum helium, neon, argon, krypton beryllium, magnesium, calcium, strontium fluorine, chlorine, bromine, iodine lithium, sodium, potassium, rubidium

fluorine, chlorine, bromine, iodine

How would a halogen achieve the stability of a noble gas electron configuration when reacting with a nonmetal atom to form a covalent (molecular) compound? form one bond, three lone pairs form two bonds, two lone pairs gain one electron form three bonds, one lone pair lose one electron

form one bond, three lone pairs

How would nitrogen achieve an octet when reacting with a nonmetal atom to form a covalent (molecular) compound? form one bond, three lone pairs lose three electrons form three bonds, one lone pair gain three electrons

form three bonds, one lone pair

How would nitrogen achieve an octet when reacting with a nonmetal atom to form a covalent (molecular) compound? gain three electrons form one bond, three lone pairs lose three electrons form three bonds, one lone pair

form three bonds, one lone pair

How would phosphorus achieve an octet when reacting with a nonmetal atom to form a covalent (molecular) compound? form three bonds, one lone pair gain three electrons lose three electrons form one bond, three lone pairs

form three bonds, one lone pair

How would sulfur achieve an octet when reacting with a nonmetal atom to form a covalent (molecular) compound? form three bonds, one lone pair form two bonds, two lone pairs gain two electrons lose two electrons form one bond, three lone pairs

form two bonds, two lone pairs

Work this calculation: 6.02 + 5.119 + 0.04218 = ? How many significant figures are in the final result? five seven three four six

four

Which correctly indicates the number of groups of electrons and the electron group geometry of the carbon atom labeled #5? two groups, linear two groups, trigonal planar four groups, tetrahedral three groups, trigonal planar four groups, trigonal planar two groups, tetrahedral three groups, linear three groups, tetrahedral four groups, linear

four groups, tetrahedral

Which correctly indicates the number of groups of electrons and the electron group geometry of the carbon atom labeled #5? two groups, tetrahedral four groups, trigonal planar three groups, tetrahedral four groups, linear two groups, linear two groups, trigonal planar three groups, linear four groups, tetrahedral three groups, trigonal planar

four groups, tetrahedral

Which correctly indicates the number of groups of electrons and the electron group geometry of the nitrogen atom labeled #3? two groups, tetrahedral four groups, tetrahedral two groups, trigonal planar three groups, linear three groups, tetrahedral two groups, linear four groups, linear four groups, trigonal planar three groups, trigonal planar

four groups, tetrahedral

Which correctly indicates the number of groups of electrons and the electron group geometry of the nitrogen atom labeled #3? two groups, tetrahedral three groups, trigonal planar four groups, tetrahedral three groups, linear three groups, tetrahedral two groups, linear two groups, trigonal planar four groups, linear four groups, trigonal planar

four groups, tetrahedral

Which correctly indicates the number of groups of electrons and the electron group geometry of the oxygen atom labeled #1? two groups, linear four groups, trigonal planar three groups, tetrahedral four groups, tetrahedral four groups, linear two groups, trigonal planar three groups, trigonal planar three groups, linear two groups, tetrahedral

four groups, tetrahedral

Which correctly indicates the number of groups of electrons and the electron group geometry of the oxygen atom labeled #1? two groups, trigonal planar three groups, tetrahedral two groups, linear two groups, tetrahedral four groups, trigonal planar four groups, linear three groups, trigonal planar three groups, linear four groups, tetrahedral

four groups, tetrahedral

In which of the pairs below are both of the properties physical properties? conducts electricity; flammable freezes at 10 degrees C; conducts electricity density of 0.78 g/mL; produces a gas when treated with acid decomposes at 75 degrees C; attracted to magnetic field

freezes at 10 degrees C; conducts electricity

In which of the pairs below are both of the properties physical properties? decomposes at 75 degrees C; attracted to magnetic field conducts electricity; flammable freezes at 10 degrees C; conducts electricity density of 0.78 g/mL; produces a gas when treated with acid

freezes at 10 degrees C; conducts electricity

How would a halogen achieve the stability of a noble gas electron configuration when reacting with a metal atom to form an ionic compound? form three bonds, one lone pair form one bond, three lone pairs lose one electron gain one electron

gain one electron

How would a halogen achieve the stability of a noble gas electron configuration when reacting with a metal atom to form an ionic compound? form three bonds, one lone pair gain one electron lose one electron form one bond, three lone pairs

gain one electron

A ___ is a physical combination of pure substances, has variable composition, and multiple phases. solution compound liquid homogeneous mixture heterogeneous mixture

heterogeneous mixture

Names and Ka values for four weak acids are listed below. The Acid Dissociation equilibrium constant (Ka) describes the extent to which the acid dissociates in water: HA (aq) + H2O (l) ⇔ H3O+ (aq) + A- (aq) If a 0.10 M solution is made of each acid, which solution would have the lowest pH? hypochlorous acid (HOCl), Ka = 2.9 x 10^-8 hydrofluoric acid (HF), Ka = 6.6 x 10^-4 acetic acid (CH3COOH), Ka = 1.8 x 10^-5 carbonic acid (H2CO3), Ka = 4.3 x 10^-7

hydrofluoric acid (HF), Ka = 6.6 x 10^-4

Consider the four types of substances described in both the Content lesson and your Skills Book: covalent network solids metallic solids ionic compounds molecular solids Of the inter-particle forces for these substances which are listed below, which is the weakest? covalent bonds metallic bonds hydrogen bonds ionic bonds

hydrogen bonds

Consider the four types of substances described in both the Content lesson and your Skills Book: covalent network solids metallic solids ionic compounds molecular solids Of the inter-particle forces for these substances which are listed below, which is the weakest? metallic bonds hydrogen bonds ionic bonds covalent bonds

hydrogen bonds

Consider the three types of attractive forces that molecular substances use to adhere to one another. Which of these attractive forces is the strongest? instantaneous dipole-dipole interactions (dispersion forces) all three types are of similar strength dipole-dipole interactions (dipolar forces) hydrogen bonds

hydrogen bonds

Two balloons with equal volumes contain different gases (X and Y) at the same temperature and pressure. The mass of gas X is 0.48 grams, and the mass of gas Y is only 0.34 grams. If gas X is ozone (chemical formula = O3), which of these is most likely to be gas Y? carbon dioxide, CO2 oxygen, O2 hydrogen sulfide, H2S sulfur dioxide, SO2 can't be determined

hydrogen sulfide, H2S

Two balloons with equal volumes contain different gases (X and Y) at the same temperature and pressure. The mass of gas X is 0.48 grams, and the mass of gas Y is only 0.34 grams. If gas X is ozone (chemical formula = O3), which of these is most likely to be gas Y? sulfur dioxide, SO2 hydrogen sulfide, H2S carbon dioxide, CO2 oxygen, O2 can't be determined

hydrogen sulfide, H2S

Names and Ka values for four weak acids are listed below. The Acid Dissociation equilibrium constant (Ka) describes the extent to which the acid dissociates in water: HA (aq) + H2O (l) ⇔ H3O+ (aq) + A- (aq) If a 0.10 M solution is made of each acid, which solution would have the highest concentration of un-dissociated acid molecules? carbonic acid (H2CO3), Ka = 4.3 x 10^-7 hypochlorous acid (HOCl), Ka = 2.9 x 10^-8 hydrofluoric acid (HF), Ka = 6.6 x 10^-4 acetic acid (CH3COOH), Ka = 1.8 x 10^-5

hypochlorous acid (HOCl), Ka = 2.9 x 10^-8

Names and Ka values for four weak acids are listed below. The Acid Dissociation equilibrium constant (Ka) describes the extent to which the acid dissociates in water: HA (aq) + H2O (l) ⇔ H3O+ (aq) + A- (aq) If a 0.10 M solution is made of each acid, which solution would have the highest concentration of un-dissociated acid molecules? hydrofluoric acid (HF), Ka = 6.6 x 10^-4 hypochlorous acid (HOCl), Ka = 2.9 x 10^-8 acetic acid (CH3COOH), Ka = 1.8 x 10^-5 carbonic acid (H2CO3), Ka = 4.3 x 10^-7

hypochlorous acid (HOCl), Ka = 2.9 x 10^-8

Names and Ka values for four weak acids are listed below. The Acid Dissociation equilibrium constant (Ka) describes the extent to which the acid dissociates in water: HA (aq) + H2O (l) ⇔ H3O+ (aq) + A- (aq) If a 0.10 M solution is made of each acid, which solution would have the highest pH? carbonic acid (H2CO3), Ka = 4.3 x 10^-7 hydrofluoric acid (HF), Ka = 6.6 x 10^-4 acetic acid (CH3COOH), Ka = 1.8 x 10^-5 hypochlorous acid (HOCl), Ka = 2.9 x 10^-8

hypochlorous acid (HOCl), Ka = 2.9 x 10^-8

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the transition metals. As you move your cursor across that region, look at which block these elements are in. (Also look at the electron configurations shown at the top right of the table.) The distinguishing electron for a transition metal is in a d orbital in an s orbital in an f orbital in a p orbital

in a d orbital

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the transition metals. As you move your cursor across that region, look at which block these elements are in. (Also look at the electron configurations shown at the top right of the table.) The distinguishing electron for a transition metal is in an s orbital in a d orbital in a p orbital in an f orbital

in a d orbital

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the halogens. As you move your cursor down that group, look at which block the element is in. (Also look at the electron configurations shown at the top right of the table.) The distinguishing electron for a halogen is: in an f orbital in a p orbital in an s orbital in a d orbital

in a p orbital

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the noble gases. As you move your cursor down that group, look at which block these elements are in. (Also look at electron configuration shown at the top right of the table.) The distinguishing electron for a noble gas is: in an f orbital in a d orbital in an s orbital

in a p orbital

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the inner transition metals (sometimes called the lanthanoids and actinoids). As you move your cursor across that region, look at which block these elements are in. (Also look at the electron configurations shown at the top right of the table.) The distinguishing electron for an inner transition metal is in a d orbital in a p orbital in an f orbital in an s orbital

in an f orbital

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the inner transition metals (sometimes called the lanthanoids and actinoids).As you move your cursor across that region, look at which block these elements are in. (Also look at the electron configurations shown at the top right of the table.) The distinguishing electron for an inner transition metal is in an s orbital in a p orbital in an f orbital in a d orbital

in an f orbital

The distinguishing electron for a Representative Element is located in a d or f orbital in an s orbital in a p orbital in an s or p orbital in an f orbital in a d orbital

in an s or p orbital

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the alkali metals. As you move your cursor down that group, look at which block these elements are in. (Also look at electron configuration shown at the top right of the table.) The distinguishing electron for an alkali metal is: in a p orbital in an s orbital in a d orbital in an f orbital

in an s orbital

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the alkali metals. As you move your cursor down that group, look at which block these elements are in. (Also look at electron configuration shown at the top right of the table.) The distinguishing electron for an alkali metal is: in an f orbital in a p orbital in an s orbital in a d orbital

in an s orbital

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the alkaline earth metals. As you move your cursor down that group, look at which block these elements are in. (Also look at electron configuration shown at the top right of the table.) The distinguishing electron for an alkaline earth metal is: in a d orbital in an s orbital in an f orbital in a p orbital

in an s orbital

In the Dynamic Periodic Table of the Elements, with the Orbitals tab selected, mouse-over the alkaline earth metals. As you move your cursor down that group, look at which block these elements are in. (Also look at electron configuration shown at the top right of the table.) The distinguishing electron for an alkaline earth metal is: in an f orbital in a p orbital in a d orbital in an s orbital

in an s orbital

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: HI gas is removed from the reaction container. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would removing HI from the reaction container affect the concentration of Cl2 gas? can't be determined no change decrease increase

increase

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: more HCl gas is added to the reaction container. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would adding HCl to the reaction container affect the concentration of HI gas? decrease can't be determined no change increase

increase

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: more HCl gas is added to the reaction container. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would adding HCl to the reaction container affect the concentration of HI gas? increase can't be determined no change decrease

increase

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to shift the equilibrium: the external pressure is increased, so that the volume of the container decreases. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would increasing the volume of the equilibrium mixture affect the concentration of HCl gas? can't be determined no change decrease increase

increase

A non-spontaneous reaction occurs in a given set of conditions. These are: with continual intervention with some intervention at the beginning with some intervention at the end. with no intervention.

with continual intervention

A spontaneous reaction occurs in a given set of conditions. These are: with continual intervention with some intervention at the beginning with no intervention. with some intervention at the end.

with some intervention at the beginning

A spontaneous reaction occurs in a given set of conditions. These are: with continual intervention with some intervention at the beginning with some intervention at the end. with no intervention.

with some intervention at the beginning

Which of these best describes a proton? located in distinct shells surrounding nucleus; has negative charge and negligible mass located in nucleus at center of atom; has positive charge and negligible mass located in distinct shells surrounding nucleus; has positive charge and negligible mass located in nucleus at center of atom; has positive charge and significant mass located in nucleus at center of atom; is electrically neutral; has significant mass

located in nucleus at center of atom; has positive charge and significant mass

Which of these best describes a proton? located in nucleus at center of atom; has positive charge and negligible mass located in distinct shells surrounding nucleus; has positive charge and negligible mass located in nucleus at center of atom; is electrically neutral; has significant mass located in distinct shells surrounding nucleus; has negative charge and negligible mass located in nucleus at center of atom; has positive charge and significant mass

located in nucleus at center of atom; has positive charge and significant mass

Which of these best describes a neutron? located in nucleus at center of atom; is electrically neutral; has significant mass located in distinct shells surrounding nucleus; is electrically neutral and has negligible mass located in nucleus at center of atom; is electrically neutral and has negligible mass located in nucleus at center of atom; has positive charge and significant mass located in distinct shells surrounding nucleus; has negative charge and negligible mass

located in nucleus at center of atom; is electrically neutral; has significant mass

How would an alkaline earth metal achieve the stability of a noble gas electron configuration when reacting with a non-metal element to form an ionic compound? gain one electron gain two electrons lose two electrons share two electrons lose one electron

lose two electrons

How would an alkaline earth metal achieve the stability of a noble gas electron configuration when reacting with a non-metal element to form an ionic compound? lose one electron share two electrons gain two electrons lose two electrons gain one electron

lose two electrons

Which property is characteristic of the nonmetal elements? may be solid, liquid or gas at room temperature are malleable and ductile have a luster can conduct heat and electricity

may be solid, liquid or gas at room temperature

Which pair of compounds is most likely to be completely miscible with one another? The term miscible means soluble in all proportions: no matter how much solute is added to the solvent, a homogeneous mixture (a solution) will result. sodium chloride (NaCl) and water hexane (C6H12) and water methanol (CH3OH) and water table sugar (sucrose, C12H22O11) and water

methanol (CH3OH) and water

Which pair of compounds is most likely to be completely miscible with one another? The term miscible means soluble in all proportions: no matter how much solute is added to the solvent, a homogeneous mixture (a solution) will result. table sugar (sucrose, C12H22O11) and water sodium chloride (NaCl) and water hexane (C6H12) and water methanol (CH3OH) and water

methanol (CH3OH) and water

Which of these elements is a noble gas? neon hydrogen platinum nitrogen oxygen

neon

HCl and I2 are placed in a reaction vessel. The endothermic forward reaction begins, and after a period of time, the system reaches equilibrium. 2 HCl (g) + I2 (s) ⇔ 2 HI (g) + Cl2 (g) A change is made to the system: a catalyst is added to the reaction mixture. Use LeChatelier's Principle to predict the shift in the equilibrium. Specifically: how would adding a catalyst to the reaction container affect the concentration of HI gas? decrease increase no change can't be determined

no change

If the electronegativity difference between two different elements is 0.3, which type of bond is likely to form when atoms of those elements chemically combine to form a compound? ionic bond no way to tell polar covalent bond nonpolar covalent bond

nonpolar covalent bond

Which combination of substances is most likely to form a heterogeneous mixture? ethanol and water sugar and water oil and table salt table salt and water

oil and table salt

Which combination of substances is most likely to form a heterogeneous mixture? oil and table salt table salt and water sugar and water ethanol and water

oil and table salt

What is the new pH of a 100 ml aliquot of 0.5 M HCl diluted to 500 ml? pH = 0.1 pH = 1.0 pH = 0.50 pH = -0.50

pH = 1.0

What is the new pH of a 100 ml aliquot of 0.5 M HNO3 diluted to 500 ml? pH = 0.5 pH = -0.1 pH = 0.1 pH = 1.0

pH = 1.0

What is the new pH of a 100 ml aliquot of 0.5 M HNO3 diluted to 500 ml? pH = 0.5 pH = -0.1 pH = 1.0 pH = 0.1

pH = 1.0

What is the new pH of a 25 ml aliquot of 0.4 M HCl diluted to 400 ml? pH = 0.5 pH = 1.6 pH = 4.5 pH = -1.0

pH = 1.6

What is the new pH of a 25 ml aliquot of 0.4 M HCl diluted to 400 ml? pH = 4.5 pH = 0.5 pH = -1.0 pH = 1.6

pH = 1.6

What is the new pH of a 25 ml aliquot of 0.4 M HNO3 diluted to 400 ml? pH = 1.5 pH = -1.0 pH = 1.6 pH = 1

pH = 1.6

What is the new pH of a 25 ml aliquot of 0.4 M HNO3 diluted to 400 ml? pH = 1.6 pH = 1 pH = -1.0 pH = 1.5

pH = 1.6

A aqueous solution is found to have a hydronium ion concentration [H3O+] = 1 x10^-10 M. The pH is a way to express the hydronium ion concentration [H3O+] (or hydrogen ion concentration [H+]) of an aqueous solution: pH = - log [H+] = - log [H3O+] Determine the pH of the solution with the hydronium ion concentration above, and indicate whether this solution is acidic, basic, or neutral. pH = 4, basic pH = 10, basic pH = 10, acidic pH = 4, acidic pH = -10, acidic pH = -10, basic

pH = 10, basic

A aqueous solution is found to have a hydroxide ion concentration [OH-] = 1 x10^-10 M. Determine the pH of the solution with the hydroxide ion concentration above, and indicate whether this solution is acidic, basic, or neutral. pH = 4, acidic pH = 10, acidic pH = 10, basic pH = -10, acidic pH = -10, basic pH = 4, basic

pH = 10, basic

Which solution is most basic? pH = 12 pOH = 4 [H3O+] = 1 x 10^-13 M [OH-] = 1 x 10^-3 M

pH = 12

What is the new pH of a 25 ml aliquot of 0.4 M KOH diluted to 400 ml? pH = 1.6 pH = 7.6 pH = 11 pH = 12.4

pH = 12.4

What is the new pH of a 25 ml aliquot of 0.4 M NaOH diluted to 400 ml? pH = 4.6 pH = 11.0 pH = 12.4 pH = 6.4

pH = 12.4

What is the new pH of a 100 ml aliquot of 0.5 M KOH diluted to 500 ml? pH = 13 pH = 6.4 pH = 1.0 pH = 11

pH = 13

Calculate the pH of a buffer solution that contains [H3PO4] = 0.10 M and [NaH2PO4] = 0.40 M? Use pKa =2.12 pH = 2.72 pH = 2.12 pH = 6.07 pH = 4.92

pH = 2.72

A strong acid is one that dissociates 100% into ions, so that the hydronium ion concentration is equal to the molarity of the acid.This means that a 0.0010 M solution of the strong acid HCl would have a: pH = 11 can't be determined pH = 1 pH = 2 pH = 3

pH = 3

A aqueous solution is found to have a hydronium ion concentration [H3O+] = 1 x10^-10 M. The pH is a way to express the hydronium ion concentration [H3O+] (or hydrogen ion concentration [H+]) of an aqueous solution: pH = - log [H+] = - log [H3O+] Determine the pH of the solution with the hydronium ion concentration above, and indicate whether this solution is acidic, basic, or neutral. pH = 10, acidic pH = 4, acidic pH = 10, basic pH = -10, acidic pH = 4, basic pH = -10, basic

pH = 4, acidic

A aqueous solution is found to have a hydroxide ion concentration [OH-] = 1 x10-10 M. Determine the pH of the solution with the hydroxide ion concentration above, and indicate whether this solution is acidic, basic, or neutral. pH = -10, acidic pH = 10, basic pH = 4, acidic pH = 4, basic pH = -10, basic pH = 10, acidic

pH = 4, acidic

Calculate the pH of a buffer solution that contains [CH3COOH] = 0.40 M and [NaCH3COO] = 0.60 M? Use pKa 4.74 pH = 2.72 pH = 6.07 pH = 4.92 pH = 4.74

pH = 4.92

A aqueous solution is found to have a hydronium ion concentration [H3O+] = 1 x10^-6 M. The pH is a way to express the hydronium ion concentration [H3O+] (or hydrogen ion concentration [H+]) of an aqueous solution: pH = - log [H+] = - log [H3O+] Determine the pH of the solution with the hydronium ion concentration above, and indicate whether this solution is acidic, basic, or neutral. pH = 8, acidic pH = 8, basic pH = -6, basic pH = -6, acidic pH = 6, acidic pH = 6, basic

pH = 6, acidic

A aqueous solution is found to have a hydronium ion concentration [H3O+] = 1 x10^-6 M. The pH is a way to express the hydronium ion concentration [H3O+] (or hydrogen ion concentration [H+]) of an aqueous solution: pH = - log [H+] = - log [H3O+] Determine the pH of the solution with the hydronium ion concentration above, and indicate whether this solution is acidic, basic, or neutral. pH = 8, basic pH = 6, acidic pH = -6, basic pH = 6, basic pH = 8, acidic pH = -6, acidic

pH = 6, acidic

A aqueous solution is found to have a hydroxide ion concentration [OH-] = 1 x10^-6 M. Determine the pH of the solution with the hydroxide ion concentration above, and indicate whether this solution is acidic, basic, or neutral. pH = 8, basic pH = 6, basic pH = 6, acidic pH = -6, basic pH = -6, acidic pH = 8, acidic

pH = 6, acidic

Calculate the pH of a buffer solution that contains [H3BO3] = 0.40 M and [NaH2BO3] = 0.20 M? Use pKa = 9.14 pH = 8.84 pH = 6.37 pH = 4.92 pH = 2.72

pH = 8.84

What is the new pH of a 100 ml aliquot of 0.5 M NaOH diluted to 500 ml? pH = -1 pH = 1 pH = 11 pH =13

pH =13

Which combination of compounds is most likely to form a heterogeneous mixture? iron (III) chloride and water ammonia (NH3) and water pentane (CH3CH2CH2CH2CH3) and water 1-pentanol (HO-CH2CH2CH2CH2CH3) and water carbon dioxide and water

pentane (CH3CH2CH2CH2CH3) and water

The atom with atomic number = 15 and mass number = 31 is sulfur, and its nucleus contains 16 protons and 15 neutrons gallium, and its nucleus contains 31 protons and 15 neutrons phosphorus, and its nucleus contains 31 neutrons and 15 protons phosphorus, and its nucleus contains 16 neutrons and 15 protons sulfur, and its nucleus contains 15 protons and 16 neutrons

phosphorus, and its nucleus contains 16 neutrons and 15 protons

Which of these best describes the combination of compounds in a solution? fixed proportion multiple phases chemical combination physical combination

physical combination

Which of these best describes the combination of compounds in a solution? fixed proportion multiple phases physical combination chemical combination

physical combination

Which of these correctly describes the combination of compounds in a homogeneous mixture? fixed proportion chemical combination physical combination multiple phases

physical combination

Which of these correctly describes the combination of compounds in a homogeneous mixture? fixed proportion physical combination multiple phases chemical combination

physical combination

Which of these correctly describes the combination of compounds in a homogeneous mixture? physical combination chemical combination multiple phases fixed proportion

physical combination

If the electronegativity difference between two different elements is 1.4, which type of bond is likely to form when atoms of those elements chemically combine to form a compound? ionic bond polar covalent bond nonpolar covalent bond no way to tell

polar covalent bond

Which of these elements is an alkali metal? chlorine potassium calcium phosphorus aluminum

potassium

Which pair of elements would have the greatest difference in electronegativity? hydrogen and phosphorus sulfur and bromine copper and nickel potassium and chlorine

potassium and chlorine

Which of these metal-nonmetal pairs become isoelectronic with the same noble gas when they react with one another to form an ionic compound? calcium, oxygen lithium, fluorine magnesium, sulfur potassium, chlorine sodium, chlorine

potassium, chlorine

Which of the following pairs is about equal in mass? proton and neutron proton and electron nucleus and surrounding shells neutron and electron

proton and neutron

Which statement is correct for pure water? if truly pure, water contains only H2O molecules, and no ions pure water contains no hydronium ions pure water contains no hydroxide ions pure water contains hydronium and hydroxide ions in equal concentrations

pure water contains hydronium and hydroxide ions in equal concentrations

Consider making this change to a balloon filled with one mole of helium: The Kelvin temperature doubles, and one-half of the helium is released from the balloon. Assume the pressure remains constant. Does the volume of the balloon become larger, or smaller, or does it remain the same? can't be determined larger remains the same smaller

remains the same

Consider making this change to a balloon filled with one mole of helium: The Kelvin temperature doubles, and one-half of the helium is released from the balloon. Assume the pressure remains constant. Does the volume of the balloon become larger, or smaller, or does it remain the same? remains the same larger can't be determined smaller

remains the same

What subshells are in the third energy level (third shell) of an atom? s, p, d and f s and p only s only s, p, and d only

s, p, and d only

The calculator answer obtained by adding the measurements 8.1, 2.19 and 3.123 is 13.413. This result... should be rounded to two significant figures is correct as written should be rounded to 13.4 should be expressed in scientific notation should be rounded to 13.41

should be rounded to 13.4

Consider making this change to a balloon filled with one mole of helium: The balloon is placed in a hyperbaric chamber, where the air pressure is two times greater than normal atmospheric pressure. Assume the temperature and the number of moles of helium inside the balloon remain constant. Does the volume of the balloon become larger, or smaller, or does it remain the same? larger smaller remains the same can't be determined

smaller

Consider making this change to a balloon filled with one mole of helium: The balloon is placed in a hyperbaric chamber, where the air pressure is two times greater than normal atmospheric pressure. Assume the temperature and the number of moles of helium inside the balloon remain constant. Does the volume of the balloon become larger, or smaller, or does it remain the same? smaller remains the same can't be determined larger

smaller

Consider making this change to a balloon filled with one mole of helium: The balloon is placed into a sub-zero freezer. (Assume the external pressure and the number of moles of helium inside the balloon remain constant.) Does the volume of the balloon become larger, or smaller, or does it remain the same? smaller remains the same larger can't be determined

smaller

An atom has 11 protons and 12 neutrons. This is an atom of the element: hydrogen boron oxygen vanadium magnesium sodium

sodium

Which statement best describes the ionic compound sodium chloride? sodium chloride consists of a pair of Na+ and Cl- ions; these NaCl ion pairs then pack closely together to form a solid sodium chloride consists of an array of Na and Cl atoms packed closely together in a fixed one-to-one proportion sodium chloride molecules contain one Na and one Cl atom, sharing electrons; these NaCl molecules pack closely together to form a solid sodium chloride consists of an array of Na+ and Cl- ions packed closely together in a fixed one-to-one proportion

sodium chloride consists of an array of Na+ and Cl- ions packed closely together in a fixed one-to-one proportion

Everyone's favorite ionic compound is sodium chloride, NaCl. When we name the ionic compound formed from a metal cation and a non-metal anion, first we say the name of the metal element (e.g., sodium), then we say the name of the anion as nonmetalide (e.g., chloride). Which of these would be the correct name for the ionic compound formed from sodium and the nonmetal nitrogen? sodium nitric sodium nitrite sodium nitrate sodium nitride sodium nitrous

sodium nitride

A ___ is a physical combination of pure substances, has variable composition, and has a single phase. solution compound liquid element heterogeneous mixture

solution

A ___ is a physical combination of pure substances, has variable composition, and has a single phase. solution liquid compound heterogeneous mixture element

solution

Which statement(s) correctly describe the subatomic particles? 1. value of charge: e- < n < p+ 2. mass: e- = p+ < n 3. location in atom: e- outside nucleus; p+ and n inside nucleus statements 2 and 3 only statements 1 and 3 only statements 1, 2 and 3 statement 3 only statement 2 only

statements 1 and 3 only

An atom has 38 protons and 47 neutrons. This is an atom of the element: selenium sulfur strontium silver tin

strontium

An atom has 38 protons and 47 neutrons. This is an atom of the element: tin sulfur silver selenium strontium

strontium

In which element does the distinguishing electron occupy an s orbital? selenium scandium strontium silicon silver

strontium

In which element does the distinguishing electron occupy an s orbital? silicon silver selenium scandium strontium

strontium

A length is measured as 2.70 x 10^3 meters. This value has its uncertainty in which decimal place? ones place hundredths place hundreds place tens place tenths place

tens place

A length is measured as 2.70 x 10^3 meters. This value has its uncertainty in which decimal place? tens place ones place hundreds place hundredths place tenths place

tens place

What is the molecular geometry of the carbon atom labeled #5? tetrahedral trigonal pyramid trigonal planar linear bent trigonal bipyramidal octahedral

tetrahedral

What is the molecular geometry of the carbon atom labeled #5? trigonal pyramid octahedral linear bent trigonal bipyramidal trigonal planar tetrahedral

tetrahedral

The term 'strong acid' refers to: the ability for the acid molecule to dissociate 100% in water the ability for the acid molecule to dissolve 100% in water the low pH of the solution the high concentration of the acid molecules in solution

the ability for the acid molecule to dissociate 100% in water

The classification of acetic acid (CH3COOH) as a 'weak acid' refers to: the low concentration of acetic acid in aqueous solution the acetic acid molecule's limited ability to dissolve in water the slightly acidic pH of acetic acid solutions the acetic acid molecule's limited ability to ionize in water

the acetic acid molecule's limited ability to ionize in water

The classification of acetic acid (CH3COOH) as a 'weak acid' refers to: the low concentration of acetic acid in aqueous solution the slightly acidic pH of acetic acid solutions the acetic acid molecule's limited ability to dissolve in water the acetic acid molecule's limited ability to ionize in water

the acetic acid molecule's limited ability to ionize in water

The classification of ammonia (NH3) as a 'weak base' refers to: the ammonia molecule's limited ability to dissolve in water the ammonia molecule's limited ability to ionize in water the low concentration of ammonia in aqueous solution the slightly basic pH of aqueous ammonia solutions

the ammonia molecule's limited ability to ionize in water

The classification of ammonia (NH3) as a 'weak base' refers to: the ammonia molecule's limited ability to ionize in water the ammonia molecule's limited ability to dissolve in water the slightly basic pH of aqueous ammonia solutions the low concentration of ammonia in aqueous solution

the ammonia molecule's limited ability to ionize in water

Two balloons have equal volumes at the same temperature and pressure. Each balloon contains a different gas: one is filled with hydrogen, the other with nitrogen. Which of these statements about the gases in the balloons is false? the number of gas molecules is the same in both balloons the average speed of the molecules is the same in both balloons can't be determined the number of moles of gas is the same in both balloons

the average speed of the molecules is the same in both balloons

Two balloons have equal volumes at the same temperature and pressure. Each balloon contains a different gas: one is filled with hydrogen, the other with nitrogen. Which of these statements about the gases in the balloons is false? the number of moles of gas is the same in both balloons the average speed of the molecules is the same in both balloons can't be determined the number of gas molecules is the same in both balloons

the average speed of the molecules is the same in both balloons

Which statement is not correct for a reaction system that has reached equilibrium? the reaction system has reached steady state the rates of the forward and reverse reactions are equal the concentrations of the reactants and products are no longer changing the forward and reverse reactions have stopped

the forward and reverse reactions have stopped

What do the elements in a Group on the periodic table have in common? the number of protons the number of electrons the number of neutrons possession of electrons within the same energy level (shell) the number and arrangement of electrons in the outermost energy level (shell)

the number and arrangement of electrons in the outermost energy level (shell)

What do the elements in a Group on the periodic table have in common? the number of protons the number of neutrons the number and arrangement of electrons in the outermost energy level (shell) possession of electrons within the same energy level (shell) the number of electrons

the number and arrangement of electrons in the outermost energy level (shell)

Which statement below is correct for this chemical equation for the combustion of methane, CH4? 2Ch4 +3O2 --> 2CO2 + 4H2O the products are methane and oxygen gas the reactants are carbon dioxide and water the reactants are methane and oxygen gas the chemical equation is properly balanced

the reactants are methane and oxygen gas

An aqueous solution of sodium chloride can conduct electricity because: sodium atoms lose electrons, and chlorine atoms gain electrons sodium is a metal, and metals conduct electricity the solution contains free sodium and chloride ions chlorine atoms have a relatively high electronegativity

the solution contains free sodium and chloride ions

An aqueous solution of sodium chloride can conduct electricity because: sodium is a metal, and metals conduct electricity sodium atoms lose electrons, and chlorine atoms gain electrons the solution contains free sodium and chloride ions chlorine atoms have a relatively high electronegativity

the solution contains free sodium and chloride ions

According to the Law of Conservation of Matter, which of these will never occur as a result of a chemical reaction? a new chemical substance is formed the total mass of the reaction mixture is reduced atoms rearrange and form new combinations electrons are transferred from one atom to another

the total mass of the reaction mixture is reduced

According to the Law of Conservation of Matter, which of these will never occur as a result of a chemical reaction? the total mass of the reaction mixture is reduced electrons are transferred from one atom to another atoms rearrange and form new combinations a new chemical substance is formed

the total mass of the reaction mixture is reduced

Which statement correctly describes the shells surrounding the nucleus of the atom? they account for the positive charge and most of the mass of the atom they contain only protons they account for the negative charge and most of the mass of the atom they contain electrons and neutrons they account for the negative charge and most of the volume of the atom

they account for the negative charge and most of the volume of the atom

Which statement is true about the various isotopes of a particular element? they always have a different number of neutrons than protons they always have the same atomic mass they always have the same number of neutrons they always have the name number of protons

they always have the name number of protons

Which of these statements is not correct for the various isotopes of a particular element? for neutral atoms, they have equal numbers of electrons and protons they always have the same atomic number they always have the same number of protons they always have the same mass number

they always have the same mass number

Which of these statements is not correct for the various isotopes of a particular element? they always have the same mass number for neutral atoms, they have equal numbers of electrons and protons they always have the same number of protons they always have the same atomic number

they always have the same mass number

Which of these statements applies to d subshells? their orbitals have a dumbbell shape they can hold a total of ten electrons they contain three d orbitals they are found in all of the energy levels (shells) of the atom all of these apply to d subshells

they can hold a total of ten electrons

Which of these statements applies to p subshells? they contain a set of three p orbitals their orbitals have a cloverleaf shape they can hold a total of 10 electrons they are found in all of the energy levels (shells) of the atom all of these apply to p subshells

they contain a set of three p orbitals

What does the symbol 2H indicate about this atom of Hydrogen? this H atom has a mass of 2 amu this H atom has two protons this H atom has two isotopes this H atom has a mass of 2 grams this H atom has two neutrons

this H atom has a mass of 2 amu

What does the symbol 2H indicate about this atom of Hydrogen? this H atom has two protons this H atom has two neutrons this H atom has two isotopes this H atom has a mass of 2 grams this H atom has a mass of 2 amu

this H atom has a mass of 2 amu

A volume is measured as 3.1 x 10-2 liters. This value has its uncertainty in which decimal place? thousands place tenths place hundredths place tens place thousandths place

thousandths place

A volume is measured as 3.1 x 10^-2 liters. This value has its uncertainty in which decimal place? tens place thousandths place tenths place thousands place hundredths place

thousandths place

Complete this subtraction: 1123.123 - 0.000012 - 1100.1 = ? How many significant figures should be in the final result? five two three four one

three

How many significant figures are appropriate when recording the measurement of a length between 9 and 10 centimeters when the smallest increment on the measuring device (a centimeter ruler) is 0.1 cm? one two three four can't be determined

three

Which correctly indicates the number of groups of electrons and the electron group geometry of the carbon atom labeled #2? three groups, linear three groups, tetrahedral two groups, tetrahedral three groups, trigonal planar four groups, tetrahedral two groups, trigonal planar four groups, trigonal planar two groups, linear four groups, linear

three groups, trigonal planar

Which correctly indicates the number of groups of electrons and the electron group geometry of the carbon atom labeled #2? three groups, trigonal planar four groups, trigonal planar two groups, tetrahedral two groups, trigonal planar four groups, tetrahedral two groups, linear three groups, tetrahedral four groups, linear three groups, linear

three groups, trigonal planar

Which correctly indicates the number of groups of electrons and the electron group geometry of the carbon atom labeled #4? four groups, trigonal planar two groups, tetrahedral three groups, linear two groups, trigonal planar two groups, linear four groups, linear three groups, trigonal planar four groups, tetrahedral three groups, tetrahedral

three groups, trigonal planar

Which correctly indicates the number of groups of electrons and the electron group geometry of the nitrogen atom labeled #2? three groups, linear two groups, linear three groups, trigonal planar four groups, linear four groups, tetrahedral two groups, trigonal planar three groups, tetrahedral four groups, trigonal planar two groups, tetrahedral

three groups, trigonal planar

Which correctly indicates the number of groups of electrons and the electron group geometry of the nitrogen atom labeled #2? two groups, linear two groups, trigonal planar three groups, trigonal planar four groups, trigonal planar three groups, linear four groups, linear two groups, tetrahedral three groups, tetrahedral four groups, tetrahedral

three groups, trigonal planar

How are atoms of 238U different from those of 235U? no difference, since both are uranium three more protons three more neutrons three more electrons

three more neutrons

In which element does the distinguishing electron occupy a p orbital? cesium plutonium strontium tin titanium

tin

Which is NOT a meaning of reduction? to lose electrons to lose bonds to oxygen to gain bonds to hydrogen to gain electrons

to lose electrons

What is the molecular geometry of the carbon atom labeled #2? tetrahedral octahedral trigonal pyramid linear bent trigonal planar trigonal bipyramidal

trigonal planar

What is the molecular geometry of the carbon atom labeled #4? trigonal bipyramidal trigonal pyramid tetrahedral octahedral linear trigonal planar bent

trigonal planar

What is the molecular geometry of the nitrogen atom labeled #3? tetrahedral bent trigonal planar trigonal bipyramidal octahedral trigonal pyramid linear

trigonal pyramid

A reaction is spontaneous if the change in entropy is positive. True False

true

A reaction is spontaneous if the energy change is exergonic. True False

true

Atoms of metal elements are oxidized when they react with nonmetal elements to form ionic compounds. True False

true

The maximum number of electrons that can occupy a p orbital is: eight two fourteen ten three six

two

Which correctly indicates the number of groups of electrons and the electron group geometry of the carbon atom labeled #5? four groups, tetrahedral two groups, trigonal planar three groups, tetrahedral two groups, tetrahedral three groups, trigonal planar four groups, trigonal planar four groups, linear two groups, linear three groups, linear

two groups, linear

Which of these best describes an ionic bond? two molecules with partial charges are attracted to one another two nonmetal atoms with very similar electronegativities share electrons two nonmetal atoms with very different electronegativities share electrons two ions with opposite charges attract one another

two ions with opposite charges attract one another

Which of these best describes a hydrogen bond? two molecules with partial charges are attracted to one another two non-metals with different electronegativities share electrons two non-metals with similar electronegativities share electrons two ions with opposite charges are attracted to one another

two molecules with partial charges are attracted to one another

Which of these best describes a polar covalent bond? two ions with opposite charges attract one another a metal atom and a nonmetal atom exchange electrons two nonmetal atoms with very similar electronegativities share electrons two nonmetal atoms with very different electronegativities share electrons

two nonmetal atoms with very different electronegativities share electrons

Which of these best describes a nonpolar covalent bond? a metal atom and a nonmetal atom exchange electrons two nonmetal atoms with very different electronegativities share electrons two nonmetal atoms with very similar electronegativities share electrons two ions with opposite charges attract one another

two nonmetal atoms with very similar electronegativities share electrons

Which of these best describes an electron? located in nucleus at center of atom; has positive charge and substantial mass located in nucleus at center of atom; is electrically neutral and has significant mass located in distinct shells surrounding nucleus; has negative charge and significant mass located in distinct shells surrounding nucleus; has negative charge and negligible mass located in nucleus at center of atom; has negative charge and negligible mass

located in distinct shells surrounding nucleus; has negative charge and negligible mass

Which statement explains why ionic compounds, such as sodium chloride (NaCl), tend to dissolve in water? both water molecules and sodium chloride molecules are polar water molecules have partial charges; sodium and chloride ions have full ionic charges both water and sodium chloride are highly electronegative, and like dissolves like in the sodium chloride molecule, the sodium is partial positive and the chloride is partial negative

water molecules have partial charges; sodium and chloride ions have full ionic charges

A non-spontaneous reaction occurs in a given set of conditions. These are: with continual intervention with no intervention. with some intervention at the end. with some intervention at the beginning

with continual intervention

Which Density probably represents a Gas? 11.3 g/ml 0.675 g/ml 0.00196 g/ml 0.440 g/ml

0.00196 g/ml

A solution is made by dissolving 5.84 grams of NaCl in distilled water to give a final volume of 1.00 liter. What is the molarity of this solution? 0.0250 M NaCl 0.400 M NaCl 5.84 M NaCl 0.100 M NaCl 1.00 M NaCl

0.100 M NaCl

Which measurement below has the most significant figures? 500.5 g 2.001 g 1.661 x 10^-24 kg 0.11000 kg 2.998 x 10^8 m/sec

0.11000 kg

Which is the correct translation of the concentration unit 0.125 M NH3? 0.125 grams NH3/100 mL solution 0.125 moles NH3/100 mL solution 0.125 moles NH3/100 L solution 0.125 moles NH3/1 L solution 0.125 molecules NH3/1 mL solution

0.125 moles NH3/1 L solution

Which is the correct translation of the concentration unit 0.125 M NH3? 0.125 molecules NH3/1 mL solution 0.125 grams NH3/100 mL solution 0.125 moles NH3/1 L solution 0.125 moles NH3/100 mL solution 0.125 moles NH3/100 L solution

0.125 moles NH3/1 L solution

Ringer's Solution, used in the treatment of burns and other wounds, is prepared by dissolving 0.330 grams of CaCl2, 8.60 grams of NaCl, and 0.300 grams of KCl in enough water to bring the total volume to 1.00 x 10^3 mL. Determine the molarity of the NaCl in the Ringer's Solution. 0.147 moles NaCl/liter 1.47 x 10^-4 moles NaCl/liter 0.503 moles NaCl/liter 8.60 moles NaCl/liter 6.80 moles NaCl/liter

0.147 moles NaCl/liter

How many moles of neon gas would be required to fill 2.5 L of hollow glass tubing to a pressure of 1.5 atm at 25 °C? 0.15 moles Ne 0.013 moles of Ne 1.5 1.8 moles of Ne

0.15 moles Ne

How many moles of NaOH would be needed to neutralize 500 mL of 0.300 M HNO3? 0.250 moles 0.150 moles 0.480 moles 0.100 moles

0.150 moles

A solution is prepared by adding 25.0 mL of a 1.30 M AlCl3 solution to a flask, then adding enough water to give a final volume of 200.0 mL. What is the concentration of the diluted 1.30 M AlCl3 solution? 0.260 M AlCl3 1.24 M AlCl3 6.50 M AlCl3 0.163 M AlCl3

0.163 M AlCl3

A solution is prepared by adding 25.0 mL of a 1.30 M AlCl3 solution to a flask, then adding enough water to give a final volume of 200.0 mL. What is the concentration of the diluted 1.30 M AlCl3 solution? 6.50 M AlCl3 1.24 M AlCl3 0.163 M AlCl3 0.260 M AlCl3

0.163 M AlCl3

How many moles of NaOH would be needed to neutralize 750 mL of 0.500 M HClO4? 0.150 moles 0.480 moles 0.375 moles 0.100 moles

0.375 moles

How many moles of NaOH would be needed to neutralize 800 mL of 0.600 M CH3COOH? 0.250 moles 0.480 moles 0.375 moles 0.100 moles

0.480 moles

Which unit conversion would allow you to convert 0.500 grams of oxygen gas into moles? 32.00 grams of oxygen (1 mole of O2/0.500 grams) = 6.02 x 1023 grams of oxygen (1 mole of O2/0.500 grams)= 0.500 grams of oxygen (32.00 grams/1 mole of O2) = 0.500 grams of oxygen (1 mole of O/16.00 grams) = 0.500 grams of oxygen (1 mole of O2/6.02 x 1023 grams) = 0.500 grams of oxygen (1 mole O2/32.00 grams O2) =

0.500 grams of oxygen (1 mole O2/32.00 grams O2) =

When the chemical equation below is properly balanced, what coefficient should be placed in front of the diatomic oxygen gas product? KCIO3 --> KCI + O2 4 1 5 2 3

When this chemical equation is properly balanced, what coefficient should be placed in front of the carbon monoxide? CO + O2 ---> CO2 5 1 2 3 4

When this chemical equation is properly balanced, what coefficient should be placed in front of the diatomic hydrogen? N2 + h2 --> NH3 1 2 5 4 3

Arrange the following items by relative entropy, from lowest entropy (1) to highest entropy (4). 50 coins arranged in loose piles by denominations: penny, nickel, dime, quarter. Bag of 50 loose coins. 50 coins arranged in one vertical column by size and date. 50 coins arrange in vertical stacks by denominations: penny, nickel, dime, quarter.

3 4 1 2

Arrange the following items by relative entropy, from lowest entropy (1) to highest entropy (4). 50 leaves at the base of the tree._ 50 leaves scattered all over the yard by the wind. 50 leaves still on a tree._ 25 leaves still on a trees and 25 leaves at the base of the tree.

3 4 1 2

Consider the balanced chemical equation below, which described the combustion of propane gas, C3H8. Which unit relationship below is not correct for this chemical reaction? C3H8 + 5O2 --> 3CO2 + 4H2O 3 moles of carbon dioxide is equivalent to 10 moles of oxygen gas 1 mole of propane is equivalent to 3 moles of carbon dioxide 4 moles of water is equivalent to 1 mole of propane 3 moles of carbon dioxide is equivalent to 4 moles of water 1 mole of propane is equivalent to 5 moles of oxygen gas

3 moles of carbon dioxide is equivalent to 10 moles of oxygen gas

Consider the balanced chemical equation below, which described the combustion of propane gas, C3H8. Which unit relationship below is not correct for this chemical reaction? C3H8+ 5O2 --> 3CO2 + 4H20 1 mole of propane is equivalent to 5 moles of oxygen gas 4 moles of water is equivalent to 1 mole of propane 1 mole of propane is equivalent to 3 moles of carbon dioxide 3 moles of carbon dioxide is equivalent to 10 moles of oxygen gas 3 moles of carbon dioxide is equivalent to 4 moles of water

3 moles of carbon dioxide is equivalent to 10 moles of oxygen gas

While you can reliably predict the charges for ions formed from the representative (main group) elements, it's more challenging to predict the charges of the ions of transition metals or post-transition metals. Since they can't achieve the stability of a noble gas electron configuration (octet of s2p6), they settle for the semi-stability of filled or half-filled s or d subshells. When you're given the chemical formula for an ionic compound formed from a transition metal with a non-metal, you can deduce the charge on the transition metal cation, since you know the charge on the nonmetal anion. Here's the chemical formula for an ionic compound that forms when the post-transition metal lead reacts with the nonmetal oxygen: Fe2S3. What's the charge on the iron ion? 2- 3+ 2+ 1+ 3-

Consider the balanced chemical equation below for the decomposition of potassium chlorate, KClO3. How many moles of potassium chloride would be produced from the decomposition of 3.00 moles of KClO3? 2 KClO3 --> 2KCl + 3O2 2.00 moles of potassium chloride 1.00 mole of potassium chloride 3.00 moles of potassium chloride 5.00 moles of potassium chloride 4.00 moles of potassium chloride

3.00 moles of potassium chloride

How many protons, neutrons, and electrons are present in an atom of bromine described by the isotopic symbol 81Br? 35 p+, 46 n, 35 e- 35 p+, 81 n, 35 e- 46 p+, 81 n, 81 e- 81 p+, 35 n, 81 e- 35 p+, 46 n, 81 e-

35 p+, 46 n, 35 e-

How many protons, neutrons, and electrons are present in an atom of bromine described by the isotopic symbol 81Br? 46 p+, 81 n, 81 e- 81 p+, 35 n, 81 e- 35 p+, 46 n, 81 e- 35 p+, 81 n, 35 e- 35 p+, 46 n, 35 e-

35 p+, 46 n, 35 e-

One mole of potassium atoms would have a mass of: 30.97 grams 39.10 grams 209 amu 209 grams 30.97 amu 39.10 amu

39.10 grams

Propane, C3H8, burns to produce carbon dioxide and water by the chemical reaction shown below. C3H8 + O2 --> CO2 + H2O What coefficient should be placed in front of the water when this equation is properly balanced with the lowest set of whole numbers? 2 3 4 1 5

While you can reliably predict the charges for ions formed from the representative (main group) elements, it's more challenging to predict the charges of the ions of transition metals or post-transition metals. Since they can't achieve the stability of a noble gas electron configuration (octet of s2p6), they settle for the semi-stability of filled or half-filled s or d subshells. When you're given the chemical formula for an ionic compound formed from a transition metal with a non-metal, you can deduce the charge on the transition metal cation, since you know the charge on the nonmetal anion. Here's the chemical formula for an ionic compound that forms when the post-transition metal lead reacts with the nonmetal oxygen: PbO2. What's the charge on the lead ion? 1- 4+ 1+ 2+ 4-

An Avogadro's number of helium atoms would have a mass of 4.003 g 4.003 amu 2 grams 6.02 x 10^23 grams 2 amu

4.003 g

Ringer's Solution, used in the treatment of burns and other wounds, is prepared by dissolving 0.330 grams of CaCl2, 8.60 grams of NaCl, and 0.300 grams of KCl in enough water to bring the total volume to 1.00 x 10^3 mL. Determine the molarity of the KCl in the Ringer's Solution. 0.300 moles KCl/liter 2.24 x 10-2 moles KCl/liter 3.00 x 10-4 moles KCl/liter 4.02 x 10-3 moles KCl/liter 4.02 moles KCl/liter

4.02 x 10-3 moles KCl/liter

Ringer's Solution, used in the treatment of burns and other wounds, is prepared by dissolving 0.330 grams of CaCl2, 8.60 grams of NaCl, and 0.300 grams of KCl in enough water to bring the total volume to 1.00 x 10^3 mL. Determine the molarity of the KCl in the Ringer's Solution. 4.02 x 10^-3 moles KCl/liter 0.300 moles KCl/liter 4.02 moles KCl/liter 3.00 x 10^-4 moles KCl/liter 2.24 x 10^-2 moles KCl/liter

4.02 x 10^-3 moles KCl/liter

Work this calculation, and express the answer with the appropriate number of significant figures. 0.012 x 342 ÷ 100.0 = 0.0041 0.0410 4.1 x 10^-3 4.1 x 10^-2 0.04104

4.1 x 10^-2

Work this calculation, and express the answer with the appropriate number of significant figures. 0.012 x 342 ÷ 100.0 = 0.0410 0.04104 4.1 x 10^-2 4.1 x 10^-3 0.0041

4.1 x 10^-2

Consider the balanced chemical equation below, which described the combustion of propane gas, C3H8. How many moles of carbon dioxide would be produced from the reaction of 7.00 moles of oxygen gas with excess propane? C3H8 + 5O2 --> 3Co2 +4H2O 5.00 moles of carbon dioxide 4.00 moles of carbon dioxide 4.20 moles of carbon dioxide 4.80 moles of carbon dioxide 4.60 moles of carbon dioxide

4.20 moles of carbon dioxide

What mass of solid potassium chloride is needed to prepare 2.50 x 10^2 mL of a 0.235 M KCl solution? 15.6 grams KCl 4.38 grams KCl 9.32 grams KCl 31.3 grams KCl 3.43 grams KCl

4.38 grams KCl

How many ml of 0.125 M NaOH would be needed to titrate 20.00 ml of 0.250 M HBr? 40 ml of NaOH 32 mL NaOH 72 ml NaOH 64 mL of NaOH

40 ml of NaOH

Which value below has the most significant figures? 2.998 x 10^8 meters/second 6.022 x 10^23 atoms/mole 21.09 grams/cm3 40.078 amu 92.42% natural abundance

40.078 amu

Which value below has the most significant figures? 40.078 amu 21.09 grams/cm3 2.998 x 10^8 meters/second 6.022 x 10^23 atoms/mole 92.42% natural abundance

40.078 amu

A volume of 5.00 L of oxygen gas is collected in a super tough balloon at 100 K and then heated until is expands to 20.0 L. What must be the new temperature of the oxygen gas. 1032 K 400 K 62.5 1 K

400 K

How many ml of 0.125 M NaOH would be needed to titrate 20.00 ml of 0.300 M CH3COOH? 32 mL of NaOH 72 ml of NaOH 48 mL of NaOH 40 mL of NaOH

48 mL of NaOH

Consider the reaction shown below. What volume of 4.00 M NaOH would be needed to react with 10.0 moles of chlorine gas? 2 NaOH (aq) + Cl2 (g) → NaCl (aq) + NaClO (aq) + H2O (l) 5.00 x 10^2 mL NaOH 2.00 liters NaOH 5 liters NaOH 4.00 liters NaOH 5.00 liters NaOH

5.00 liters NaOH

Consider the balanced chemical equation below for the reaction of zinc metal with hydrochloric acid (aqueous HCl). How many moles of aqueous HCl would be needed to make 2.50 moles of zinc (II) chloride? Zn + 2HCl --> H2 + ZnCl2 2.50 mole of HCl 5 moles of HCl 1.25 moles of HCl 5.00 moles of HCl 1 mole of HCl

5.00 moles of HCl

Consider the balanced chemical equation below for the reaction of zinc metal with hydrochloric acid (aqueous HCl). How many moles of aqueous HCl would be needed to make 2.50 moles of zinc (II) chloride? Zn + 2HCl --> H2 + ZnCl2 1.25 moles of HCl 5.00 moles of HCl 1 mole of HCl 5 moles of HCl 2.50 mole of HCl

5.00 moles of HCl

What volume of a 0.150 M CuSO4 solution would contain 7.50 x 10^-2 moles of solute? 5.00 L 2.00 x 10^3 mL 500 mL 5.00 x 10^2 mL 2.0 L

5.00 x 10^2 mL

What volume of a 0.150 M CuSO4 solution would contain 7.50 x 10^-2 moles of solute? 500 mL 5.00 x 10^2 mL 5.00 L 2.0 L 2.00 x 10^3 mL

5.00 x 10^2 mL

Consider the reaction shown below. What volume of 6.00 M HCl would be needed to react with 1.00 mole of Al(OH)3? Al(OH)3 (g) + 3 HCl (aq) → 3 H2O (l) + AlCl3 (aq) 0.5 liters HCl 887 mL HCl 234 mL HCl 5.00 x 10^2 mL HCl 5.00 liters HCl

5.00 x 10^2 mL HCl

Which unit conversion would allow you to convert 5.76 kilograms to milligrams?

5.76 kg (10^3 g/1 Kg)(1 mg/10^-3 g)

What volume of 6.00 M HCl should be diluted to prepare 1.50 x 10^3 mL of 0.200 M HCl? 1.80 x 10^4 mL HCl 125 mL HCl 50.0 mL HCl 2.00 x 10^-3 mL HCl

50.0 mL HCl

What volume of 6.00 M HCl should be diluted to prepare 1.50 x 10^3 mL of 0.200 M HCl? 50.0 mL HCl 1.80 x 10^4 mL HCl 2.00 x 10^-3 mL HCl 125 mL HCl

50.0 mL HCl

75.0 mol of hydrogen gas is confined to a volume of 260. L in an exterior storage take. In the Winter the temperature on the tank reaches -20 °C. What is the pressure? 975 atm 59.9 atm 6.00 atm -0.474 atm

6.00 atm

Complete this Avogadro's Statement for the element oxygen: 1 mole of oxygen gas contains ____ O2 molecules and has a mass of ____ grams. 1.204 x 10^24; 32.00 6.02 x 10^23; 32.00 6.02 x 10^23; 16.00 1.204 x 10^24; 16.00

6.02 x 10^23; 32.00

Consider the reaction shown below. What mass of CaSO4 would be produced if 1.00 liters of a 0.500 M H2SO4 solution reacts with excess CaCO3? CaCO3 (s) + H2SO4 (aq) → H2CO3 (aq) + CaSO4 (aq) 68.1 grams CaSO4 44 .1 grams CaSO4 68 grams CaSO4 136 grams CaSO4 50.0 grams CaSO4

68.1 grams CaSO4

Ethane, C2H6, burns to produce carbon dioxide and water by the chemical reaction shown below. C2H6 + O2 --> CO2 + H2O What coefficient should be placed in front of the diatomic oxygen gas when this equation is properly balanced with the lowest set of whole numbers? 3 5 4 7 6 2 8

The number of f orbitals in an f subshell is 3 1 2 7 14 5

Consider the reaction shown below. What mass of chlorine gas would be needed to react with 2.00 liters of a 0.100 M NaOH solution? 2 NaOH (aq) + Cl2 (g) → NaCl (aq) + NaClO (aq) + H2O (l) 7.09 grams Cl2 3.55 grams Cl2 14.2 grams Cl2 35.5 grams Cl2 70.9 grams Cl2

7.09 grams Cl2

Consider the reaction shown below. What mass of chlorine gas would be needed to react with 2.00 liters of a 0.100 M NaOH solution? 2 NaOH (aq) + Cl2 (g) → NaCl (aq) + NaClO (aq) + H2O (l) 70.9 grams Cl2 35.5 grams Cl2 14.2 grams Cl2 7.09 grams Cl2 3.55 grams Cl2

7.09 grams Cl2

75.0 mol of hydrogen gas is confined to a volume of 260. L in an exterior storage take. In the Summer the temperature on the tank reaches 30 °C. What is the pressure? 650 atm 71.8 atn 7.18 atm 0.023 atm

7.18 atm

What is a nonelectrolyte? A nonelectolyte is a solute which will dissolve in a solution but does not dissociate into ions and can conduct electricity. A nonelectolyte is a solute which will dissolve in a solution and does dissociate into ions and can conduct electricity. A nonelectolyte is a solute which will dissolve in a solution but does dissociate into ions and can not conduct electricity. A nonelectolyte is a solute which will dissolve in a solution but does not dissociate into ions and can not conduct electricity.

A nonelectolyte is a solute which will dissolve in a solution but does not dissociate into ions and can not conduct electricity.

What is the difference between a solute and a solvent in a solution? A solute is the major component in a solution and the solvent is the minor component. A solvent is the minor component in a solution. A solvent is the major component in a solution and the solute is the minor component. A solute is the major component in a solution.

A solvent is the major component in a solution and the solute is the minor component.

What is an electrolyte? A type of solute that when dissolved in a solution do not dissociate into ions but still can conduct electricity. A type of solute that when dissolved in a solution do not dissociate into ions which can not conduct electricity. A type of solute that when dissolved in a solution will dissociate into ions which conduct electricity. A type of solute that when dissolved in a solution dissociates into ions but the solution does not conduct electricity.

A type of solute that when dissolved in a solution will dissociate into ions which conduct electricity.

How are the freezing point and the vapor pressure affected by the addition of a dissolved solute? Adding a solute will elevate the freezing point of the solution and lower the vapor pressure compared to the solvent alone. Adding a solute will depress the freezing point of the solution and raise the vapor pressure compared to the solvent alone. Adding a solute will elevate the freezing point of the solution and raise the solution vapor pressure compared to the solvent alone. Adding a solute will depress the freezing point of the solution and lower the vapor pressure compared to the solvent alone.

Adding a solute will depress the freezing point of the solution and lower the vapor pressure compared to the solvent alone.

How are the boiling point and the vapor pressure affected by the addition of a dissolved solute? Adding a solute will depress the boiling point of the solution and raise the vapor pressure compared to the solvent alone. Adding a solute will elevate the boiling point of the solution and elevate the vapor pressure compared to the solvent alone. Adding a solute will depress the boiling point of the solution and lower the vapor pressure compared to the solvent alone. Adding a solute will elevate the boiling point of the solution and lower the vapor pressure compared to the solvent alone.

Adding a solute will elevate the boiling point of the solution and lower the vapor pressure compared to the solvent alone.

Which of these is the correct symbol for the element silver? Sr Sn Ag S Si

A person can walk though air because,,,, Air is a collection of liquids and the particles have little or no adhesion to each other. Air is a collection of solids and the particles have little or no adhesion to each other. Air is a collection of gases and the particles have little or no adhesion to each other. Air is a collection of gases and the particles have a great deal of adhesion to each other.

Air is a collection of gases and the particles have little or no adhesion to each other.

Consider the ionic compound that forms when aluminum metal chemically combines with the non-metal bromine. What is the chemical formula for that ionic compound? (What is the fixed proportion in which these ions combine?) Al3Br2 Al2Br3 AlBr3 Al3Br AlBr

AlBr3

When 1 mole of Al(OH)3 chemically reacts with 1 mole of H3PO4, what salt is formed? Al3PO4 is the salt formed. Al(OH)3 is the salt formed. AlPO4 is the salt formed. H3PO4 is the salt formed.

AlPO4 is the salt formed.

Classify both alcohol evaporating and iron melting in a furnace Alcohol evaporating and iron melting in a furnace are both exothermic. Alcohol evaporating is exothermic and iron melting in a furnace is endothermic. Alcohol evaporating is endothermic and iron melting in a furnace is exothermic. Alcohol evaporating and iron melting in a furnace are both endothermic.

Alcohol evaporating and iron melting in a furnace are both endothermic.

Classify both alcohol evaporating and water freezing. Alcohol evaporating is exothermic and water freezing is endothermic. Alcohol evaporating and water freezing are both endothermic. Alcohol evaporating and water freezing are both exothermic. Alcohol evaporating is endothermic and water freezing is exothermic.

Alcohol evaporating is endothermic and water freezing is exothermic.

In which of these carbon compounds is the carbon atom in its most reduced form (lowest oxidation state)? CO2 CH3OH HCOOH CH2O CH4

CH4

Lowering the temperature of a NaCl solution promotes crystal formation because. As the solution temperature goes down, the molecular motion of the water increases, which allows the attractive ionic force of the Na+ and Cl- ions begin to dominate bringing ions together to form the NaCl crystal lattice. As the solution temperature goes down, the molecular motion of the water increases, which allows the repulsive ionic force of the Na+ and Cl- ions begin to dominate pushing ions apart to form the NaCl crystal lattice. As the solution temperature goes down the molecular motion of the water decreases, which allows the attractive ionic force of the Na+ and Cl- ions begin to dominate bringing ions together to form the NaCl crystal lattice. As the solution temperature goes down the molecular motion of the water decreases, which allows the repulsive ionic force of the Na+ and Cl- ions begin to dominate pushing ions apart to form the NaCl crystal lattice.

As the solution temperature goes down the molecular motion of the water decreases, which allows the attractive ionic force of the Na+ and Cl- ions begin to dominate bringing ions together to form the NaCl crystal lattice.

Consider the combustion of ethane gas to form carbon dioxide and water. Which element is being oxidized in this reaction? 2C2H6 + 7O2 --> 4CO2 + 6H2O H in C2H6 C in C2H6 O in O2

C in C2H6

Examine the structures of the molecules below. These are condensed structures, with the hydrogen atoms grouped together with a subscript. You'll need to expand them out, either on paper or in your head, so you're aware of every atom, every covalent bond, and every lone pair of electrons. For each molecule: determine the type(s) of attractive forces the molecule could use to interact with others of its own kind. consider the relative strengths of those attractive forces consider the molecule's mass and surface area Which of these compounds would you predict to have the highest boiling point?Put another way: which compound would require the most heat to overcome the attractive forces between the molecules? CH3-CH2-CH2-CH2-CH2-CH2-CH2-CH2-OH CH3-CH2-CH2-CH2-CH2-CH2-OH CH3-CH2-CH2-CH2-OH CH3-CH2-OH

CH3-CH2-CH2-CH2-CH2-CH2-CH2-CH2-OH

Examine the structures of the molecules below. Which of these would you predict to have the lowest water solubility? CH3-CH2-CH2-O-CH3 CH3-CH2-CH2-CH2-OH CH3-CH2-CH2-CH3

CH3-CH2-CH2-CH3

Examine the structures of the molecules below. These are condensed structures, with the hydrogen atoms grouped together with a subscript. You'll need to expand them out, either on paper or in your head, so you're aware of every atom, every covalent bond, and every lone pair of electrons. For each molecule: determine the type(s) of attractive forces the molecule could use to interact with others of its own kind. consider the relative strengths of those attractive forces consider the molecule's mass and surface area Which of these compounds would you predict to have the lowest boiling point?Put another way: which compound would require the smallest amount heat to overcome the attractive forces between the molecules? CH3-CH2-CH2-CH3 CH3-CH2-CH2-CH2-OH CH3-CH2-CH2-O-CH3

CH3-CH2-CH2-CH3

Examine the structures of the molecules below. These are condensed structures, with the hydrogen atoms grouped together with a subscript. You'll need to expand them out, either on paper or in your head, so you're aware of every atom, every covalent bond, and every lone pair of electrons. For each molecule: determine the type(s) of attractive forces the molecule could use to interact with others of its own kind. consider the relative strengths of those attractive forces consider the molecule's mass and surface area Which of these compounds would you predict to have the lowest boiling point?Put another way: which compound would require the smallest amount heat to overcome the attractive forces between the molecules? CH3-CH2-CH2-O-CH3 CH3-CH2-CH2-CH3 CH3-CH2-CH2-CH2-OH

CH3-CH2-CH2-CH3

Examine the structures of the molecules below. Which of these would you predict to have the highest water solubility? CH3-CH2-CH2-CH2-CH2-CH2-CH2-CH2-OH CH3-CH2-CH2-CH2-CH2-CH2-OH all can hydrogen bond with water, so they would be equally water soluble. CH3-CH2-CH2-CH2-OH CH3-CH2-OH

CH3-CH2-OH

Which sketch correctly shows the hydrogen bonding between molecules of methylamine, CH3NH2?

CH3-N(above H)-H-----N (above H, below CH3)-H

Which sketch correctly shows hydrogen bonding between molecules of methanol, CH3OH?

CH3-O(H below)---H-O (Below CH3)

Which of these molecular compounds has a Lewis structure that contains three lone pairs of electrons? CH3Br H2S N2H4 CH4O CO2

CH3Br

Which of these molecular compounds would have a Lewis structure that contains a total of 14 valence electrons? HCN CO2 H2O CH3Cl NH3

CH3Cl

Which of these molecular compounds would have a Lewis structure that contains a total of 14 valence electrons? H2O CH3Cl HCN NH3 CO2

CH3Cl

Examine the structures of the molecules below. These are condensed structures, with the hydrogen atoms grouped together with a subscript. You'll need to expand them out, either on paper or in your head, so you're aware of every atom, every covalent bond, and every lone pair of electrons. For each molecule: determine the type(s) of attractive forces the molecule could use to interact with others of its own kind. consider the relative strengths of those attractive forces consider the molecule's mass and surface area (including the relative sizes of the electron clouds) Which correctly lists the molecules in order of increasing boiling point (from lowest boiling point to highest boiling point)? CH3I < CH3Br < CH3Cl CH3Cl < CH3I < CH3Br CH3I < CH3Cl < CH3Br CH3Cl < CH3Br < CH3I CH3Br < CH3Cl < CH3I CH3Br < CH3I < CH3Cl

CH3Cl < CH3Br < CH3I

Examine the structures of the molecules below. These are condensed structures, with the hydrogen atoms grouped together with a subscript. You'll need to expand them out, either on paper or in your head, so you're aware of every atom, every covalent bond, and every lone pair of electrons. For each molecule: determine the type(s) of attractive forces the molecule could use to interact with others of its own kind. consider the relative strengths of those attractive forces consider the molecule's mass and surface area (including the relative sizes of the electron clouds) Which correctly lists the molecules in order of increasing boiling point (from lowest boiling point to highest boiling point)? CH3Cl < CH3Br < CH3I CH3I < CH3Br < CH3Cl CH3Br < CH3Cl < CH3I CH3I < CH3Cl < CH3Br CH3Br < CH3I < CH3Cl CH3Cl < CH3I < CH3Br

CH3Cl < CH3Br < CH3I

Identify the key type of 'inter-particle' attractive force that each compound below is capable of using to interact with others of its own kind. Then answer this question: Which correctly lists the three compounds in order of increasing strength of 'inter-particle' attractive force (from weakest to strongest)? CH3OH < CH3Cl < NaCl CH3Cl < NaCl < CH3OH NaCl < CH3OH < CH3Cl CH3OH < NaCl < CH3Cl CH3Cl < CH3OH < NaCl NaCl < CH3Cl < CH3OH

CH3Cl < CH3OH < NaCl

Identify the key type of 'inter-particle' attractive force that each compound below is capable of using to interact with others of its own kind. Then answer this question: Which correctly lists the three compounds in order of increasing strength of 'inter-particle' attractive force (from weakest to strongest)? NaCl < CH3OH < CH3Cl NaCl < CH3Cl < CH3OH CH3Cl < NaCl < CH3OH CH3Cl < CH3OH < NaCl CH3OH < CH3Cl < NaCl CH3OH < NaCl < CH3Cl

CH3Cl < CH3OH < NaCl

Boiling is the temperature at which the vapor pressure of the liquid exceeds the atmospheric pressure. Campers in the Rocky Mountains notice that their food takes longer to cook. Why do you think that is so. Cooking depends on how much heat the food absorbs. At high altitude there is less air pressure, so water boils at a higher temperature, which produces less heat in the water so it takes longer for the food to absorb the necessary heat. Cooking depends on how much heat the food absorbs. At high altitude there is less air pressure, so water boils at a higher temperature, which produces more heat in the water so it takes longer for the food to absorb the necessary heat. Cooking depends on how much heat the food absorbs. At high altitude there is less air pressure, so water boils at a lower temperature, which produces less heat in the water so it takes longer for the food to absorb the necessary heat. Cooking depends on how much heat the food absorbs. At high altitude there is less air pressure, so water boils at a lower temperature, which produces more heat in the water so it takes longer for the food to absorb the necessary heat.

Cooking depends on how much heat the food absorbs. At high altitude there is less air pressure, so water boils at a lower temperature, which produces less heat in the water so it takes longer for the food to absorb the necessary heat.

Boiling is the temperature at which the vapor pressure of the liquid exceeds the atmospheric pressure. Campers in Dead Valley, which is below sea level notice that their food takes cooks faster than at home. Why do you think that is so. Cooking depends on how much heat the food absorbs. At low altitude there is more air pressure, so water boils at a lower temperature, which produces more heat in the water so it takes less time for the food to absorb the necessary heat. Cooking depends on how much heat the food absorbs. At low altitude there is more air pressure, so water boils at a higher temperature, which produces less heat in the water so it takes less time for the food to absorb the necessary heat. Cooking depends on how much heat the food absorbs. At low altitude there is more air pressure, so water boils at a higher temperature, which produces more heat in the water so it takes less time for the food to absorb the necessary heat. Cooking depends on how much heat the food absorbs. At low altitude there is more air pressure, so water boils at a lower temperature, which produces less heat in the water so it takes less time for the food to absorb the necessary heat.

Cooking depends on how much heat the food absorbs. At low altitude there is more air pressure, so water boils at a higher temperature, which produces more heat in the water so it takes less time for the food to absorb the necessary heat.

Which of these is the correct symbol for the element copper? Co Cu Cr Kr C

Which polar covalent bond below is correctly labeled to indicate the partial positive and partial negative charges on the participating atoms? Nδ+ − Hδ− Fδ+ − Oδ− Clδ+ − Cδ− Cδ+ − Oδ−

Cδ+ − Oδ−

Put into a car on a cold winter's day, one would expect a balloon to... Increase in size because the decrease in temperature causes less motion in the gas in the balloon which makes the balloon expand. Decrease in size because the decrease in temperature causes more motion in the gas in the balloon which makes the balloon contract. Decrease in size because the decrease in temperature causes less motion in the gas in the balloon which makes the balloon contract. Increase in size because the decrease in temperature causes more motion in the gas in the balloon which makes the balloon expand.

Decrease in size because the decrease in temperature causes less motion in the gas in the balloon which makes the balloon contract.

Classify both deposition and condensation. Deposition and condensation are both exothermic. Deposition and condensation are both endothermic. Deposition is endothermic and condensation is exothermic. Deposition is exothermic and condensation is endothermic.

Deposition and condensation are both exothermic.

What is true about dialysis. Dialysis is the movement of water molecules and small solutes through a semi-permeable membrane from a region of low concentration to a region of high concentration. Dialysis is the movement of water molecules and small solutes through a semi-permeable membrane from a region of high concentration to a region of low concentration. Dialysis is the movement of water molecules and small solutes through a non-permeable membrane from a region of high concentration to a region of low concentration. Dialysis is the movement of water molecules but not small solutes through a semi-permeable membrane from a region of high concentration to a region of low concentration.

Dialysis is the movement of water molecules and small solutes through a semi-permeable membrane from a region of high concentration to a region of low concentration.

What is true about a colloidal dispersion? Dispersed phase in a colloidal dispersion will not settle out over time; there is a light scattering Tyndall effect because the particles are large and the colloid is a heterogenous mixture. Dispersed phase in a colloidal dispersion will not settle out over time; there is no light scattering Tyndall effect because the particles are large and the colloid is a homogenous mixture. Dispersed phase in a colloidal dispersion will settle out over time; there is a light scattering Tyndall effect because the particles are large and the colloid is a homogenous mixture. Dispersed phase in a colloidal dispersion will not settle out over time; there is a light scattering Tyndall effect because the particles are large and the colloid is a homogenous mixture.

Dispersed phase in a colloidal dispersion will not settle out over time; there is a light scattering Tyndall effect because the particles are large and the colloid is a homogenous mixture.

A 0.010 M solution of the strong acid HCl would have a pH = 1. True False

False

A drug is to be administered in liquid form, as part of a heterogeneous mixture. Since heterogeneous mixtures are consistent throughout, this medication would not need to be shaken prior to measuring out the appropriate dose. True False

False

A non-spontaneous reaction usually occur quickly by itself. True False

False

A reaction is non-spontaneous if the change in entropy is positive. True False

False

All numbers will have some uncertainty associated with them. True False

False

Heating a solution will increase the solubility of NaCl because.. Heating a solution increases molecular motion, which tends to make NaCl ions come apart less easily and also causes more water molecules to contact NaCl ions with more force, esulting in pulling more NaCl ions into solution. Heating a solution increases molecular motion, which tends to make NaCl ions come apart more easily and also causes more water molecules to contact NaCl ions with less force, esulting in pulling more NaCl ions into solution. Heating a solution increases molecular motion, which tends to make NaCl ions come apart more easily and also causes more water molecules to contact NaCl ions with more force, esulting in pulling more NaCl ions into solution. Heating a solution decreases molecular motion, which tends to make NaCl ions come apart less easily and also causes more water molecules to contact NaCl ions with more force, esulting in pulling more NaCl ions into solution. Heating a solution decreases molecular motion, which tends to make NaCl ions come apart more easily and also causes more water molecules to contact NaCl ions with more force, esulting in pulling more NaCl ions into solution. Heating a solution decreases molecular motion, which tends to make NaCl ions come apart more easily and also causes more water molecules to contact NaCl ions with less force, esulting in pulling more NaCl ions into solution.

Heating a solution increases molecular motion, which tends to make NaCl ions come apart more easily and also causes more water molecules to contact NaCl ions with more force, esulting in pulling more NaCl ions into solution.

How does heating a liquid facilitate more evaporation. Heating the liquid increases the molecular motion in the liquid molecules which decreases the number of molecules that have sufficient energy to break the cohesive forces of the liquid and go into the vapor phase. Heating the liquid decreases the molecular motion in the liquid molecules which increases the number of molecules that have sufficient energy to break the cohesive forces of the liquid and go into the vapor phase. Heating the liquid increases the molecular motion in the liquid molecules which increases the number of molecules that have sufficient energy to break the cohesive forces of the liquid and go into the vapor phase. Heating the liquid decreases the molecular motion in the liquid molecules which decrease the number of molecules that have sufficient energy to break the cohesive forces of the liquid and go into the vapor phase.

Heating the liquid increases the molecular motion in the liquid molecules which increases the number of molecules that have sufficient energy to break the cohesive forces of the liquid and go into the vapor phase.

Coconut oil is a solid at room temperature, but it will melt to a clear oil at body temperature. How does this happen.. Heating the solid increases the molecular motion of the coconut oil molecules which forms more internal cohesive forces in the solid to allow the molecules to relax into a fluid liquid state. Heating the solid decreases the molecular motion of the coconut oil molecules which overcomes enough of the internal cohesive forces in the solid to allow the molecules to relax into a fluid liquid state. Heating the solid increases the molecular motion of the coconut oil molecules which overcomes enough of the internal cohesive forces in the solid to allow the molecules to relax into a fluid liquid state. Heating the solid decreases the molecular motion of the coconut oil molecules which forms more internal cohesive forces in the solid to allow the molecules to relax into a fluid liquid state.

Heating the solid increases the molecular motion of the coconut oil molecules which overcomes enough of the internal cohesive forces in the solid to allow the molecules to relax into a fluid liquid state.

The solvent hexane (C6H14) is a liquid at room temperature as is the solvent heptane (C7H16). How is the vapor pressure different in this two solvents? Heptane is a larger molecule and has a lower vapor pressure. Hexane is a smaller molecule and has a higher vapor pressure. Hexane is a smaller molecule and has a lower vapor pressure. Heptane is a smaller molecule and has a higher vapor pressure.

Hexane is a smaller molecule and has a higher vapor pressure.

Consider the reaction of hydrogen gas with oxygen gas to make water. Which statement is correct for this reaction? Both hydrogen and oxygen are being reduced in this reaction. Hydrogen is being reduced; oxygen is being oxidized. Hydrogen is being oxidized; oxygen is being reduced. Both hydrogen and oxygen are being oxidized in this reaction.

Hydrogen is being oxidized; oxygen is being reduced.

An acid is a compound that dissociates in water to produce ______ions, which are ________ Hydroxide ions, which are anions. Hydroxide ions, which are cations. Hydronium ions, which are anions. Hydronium ions, which are cations.

Hydronium ions, which are cations.

Put into a car on a hot summer's day, one would expect a balloon to... Decrease in size because the increase in temperature causes more motion in the gas in the balloon which makes the balloon contract. Increase in size because the increase in temperature causes less motion in the gas in the balloon which makes the balloon expand. Increase in size because the increase in temperature causes more motion in the gas in the balloon which makes the balloon expand. Decrease in size because the increase in temperature causes less motion in the gas in the balloon which makes the balloon contract.

Increase in size because the increase in temperature causes more motion in the gas in the balloon which makes the balloon expand.

Suppose you have two large beakers each containing 1 liter of water at room temperature. Now pretend that you add the 1 drop of ink A to the first beaker and 1 drop of ink B to the second beaker. Now if ink A is twice a large a molecule as ink B, which ink will disperse fulling first, A or B? Ink B, is the smaller molecule, so it should disperse SLOWLY because it is EASIER for the random motion of the water molecules to push it around. Ink B, is the smaller molecule, so it should disperse SLOWLY because it is HARDER for the random motion of the water molecules to push it around. Ink B, is the smaller molecule, so it should disperse QUICKLY because it is EASIER for the random motion of the water molecules to push it around. Ink B, is the smaller molecule, so it should disperse QUICKLY because it is HARDER for the random motion of the water molecules to push it around.

Ink B, is the smaller molecule, so it should disperse QUICKLY because it is EASIER for the random motion of the water molecules to push it around.

Refer to the energy level diagram below. Which letter corresponds to the average energy of the reactant molecules? O L K M N P

Which of these is the correct symbol for the element potassium? P Pm Po Pt K

Which equilibrium constant value below indicates a reaction that goes essentially 100% to completion? K = 1.0 x 10^-14 K = 1.0 x 10^1 K = 1.0 x 10^14 K = 1.0 x 10^0

K = 1.0 x 10^14

Equilibrium constants were measured for a series of reaction of the general type: AB + CD ⇔ AD + BC. These equilibrium constant values are shown below. In which reaction is the concentration of products the largest at equilibrium? K = 1 K = 9.7 x 10^-8 K = 125 K = 0.0875 K = 3.5 x 10^8

K = 3.5 x 10^8

Equilibrium constants were measured for a series of reaction of the general type: AB + CD ⇔ AD + BC. These equilibrium constant values are shown below. In which reaction is the concentration of products the smallest at equilibrium? K = 0.0875 K = 1 K = 3.5 x 10^8 K = 125 K = 9.7 x 10^-8

K = 9.7 x 10^-8

Equilibrium constants were measured for a series of reaction of the general type: AB + CD ⇔ AD + BC. These equilibrium constant values are shown below. In which reaction is the concentration of products the smallest at equilibrium? K = 1 K = 9.7 x 10^-8 K = 125 K = 0.0875 K = 3.5 x 10^8

K = 9.7 x 10^-8

Which is the correct Equilibrium Constant expression for this reaction?N2 (g) + 3 F2 (g) ⇔ 2 NF3 (g) K =[N2] [F2]3/[NF3]2 K = [NF3]/[N2][F2] K = [NF3]2/[N2][F2]3 K = [N2][F2]/[NF3]

K = [NF3]2/[N2][F2]3

In which compound does the metal have the lowest oxidation number? MgO SnS CoCl3 K2O PbS2

K2O

In which compound does the metal have the lowest oxidation number? PbS2 SnS K2O CoCl3 MgO

K2O

Refer to the energy level diagram below. Which letter corresponds to the energy of the transition state (activated complex)? N P O K M L

Refer to the energy level diagram below. Which letter(s) indicate values that would be changed by the addition of a catalyst to the reaction system? K K, L, and P L M, N, and O O M N P

M, N, and O

Which letter(s) indicate values that would be changed by the addition of a catalyst to the reaction system? O M, N, and O L K M P N K, L, and P

M, N, and O

Classify both melting and evaporation. Melting and evaporation are both exothermic. Melting is endothermic and evaporation is exothermic. Melting is exothermic and evaporation is endothermic. Melting and evaporation are both endothermic.

Melting and evaporation are both endothermic.

Consider the ionic compound that forms when manganese ions (with a +4 charge) combine with sulfide ions. What is the chemical formula for that ionic compound? (What is the fixed proportion in which these ions combine?) Mn4S2 Mn2S4 MnS2 MnS Mn4S

MnS2

Refer to the energy level diagram below. Which letter corresponds to the Activation Energy (Ea) for the forward reaction? M L K O P N

Refer to the energy level diagram below. Which letter corresponds to the Activation Energy (Ea) for the forward reaction? O L M P N K

When 1 mole of NaOH chemically reacts with 1 mole of HCl, what salt is formed? NaCl is the salt formed. NaOH is the salt formed. HCL is the salt formed. Water is the salt formed.

NaCl is the salt formed.

Which is sodium hydroxide HNO3 NaOH H3PO4 H2SO4

NaOH

Which one of these compounds is an Arrhenius base? NH3 is an Arrhenius base. HCl is an Arrhenius base. NaCl is an Arrhenius base. NaOH is an Arrhenius base.

NaOH is an Arrhenius base.

Which state of matter has weak internal cohesive forces, is very compressible and can keep its own volume and shape. Gas Liquid None of them Solid

None of them

Which polar covalent bond below is correctly labeled to indicate the partial positive and partial negative charges on the participating atoms? Cδ− − Oδ+ Nδ− − Hδ+ Fδ+ − Pδ− Oδ+ − Hδ−

Nδ− − Hδ+

Refer to the energy level diagram below. Which letter corresponds to the Activation Energy (Ea) for the reverse reaction? K L P N O M

Refer to the energy level diagram below. Which letter corresponds to the Activation Energy (Ea) for the reverse reaction? P O K N M L

Consider the reaction below for the decomposition of potassium chlorate. Which element is being oxidized? 2 KClO3 --> 2 KCl + 3O2 O in KClO3 Cl in KClO3 K in KClO3

O in KClO3

Consider the reaction below for the decomposition of potassium chlorate. Which element is being oxidized? 2 KClO3 --> 2KCl + 3O2 O in KClO3 Cl in KClO3 K in KClO3

O in KClO3

If you have two bottles of the same perfume, but one is cold and the other is warm, which do you think will be easier to smell. One should smell the COLDER perfume first because its molecules have more molecular motion and should diffuse in the air more QUICKLY. One should smell the COLDER perfume first because its molecules have more molecular motion and should diffuse in the air more SLOWLY. One should smell the WARMER perfume first because its molecules have more molecular motion and should diffuse in the are more QUICKLY. One should smell the WARMER perfume first because its molecules have more molecular motion and should diffuse in the are more SLOWLY.

One should smell the WARMER perfume first because its molecules have more molecular motion and should diffuse in the are more QUICKLY.

What is osmosis. Osmosis is like Dialysis in that the movement of water molecules and small solutes through a semi-permeable membrane from a region of high concentration to a region of low concentration. Osmosis is the movement of water molecules but not small solutes through a semi-permeable membrane from a region of high solute concentration to a region of low solute concentration. Osmosis is the movement of water molecules and small solutes through a semi-permeable membrane from a region of low solute concentration to a region of high solute concentration. Osmosis is the movement of water molecules but not small solutes through a semi-permeable membrane from a region of low solute concentration to a region of high solute concentration.

Osmosis is the movement of water molecules but not small solutes through a semi-permeable membrane from a region of low solute concentration to a region of high solute concentration.

Refer to the energy level diagram below. Which letter corresponds to the average energy of the product molecules? L P K O N M

Refer to the energy level diagram below. Which letter corresponds to the average energy of the product molecules? M O K N L P

PF3

Identify the key type of 'inter-particle' attractive force that each compound below is capable of using to interact with others of its own kind. Then answer this question: Which correctly lists the three compounds in order of increasing strength of 'inter-particle' attractive force (from weakest to strongest)? PF3 < H2O < KCl H2O < PF3 < KCl H2O < KCl < PF3 KCl < PF3 < H2O KCl < H2O < PF3 PF3 < KCl < H2O

PF3 < H2O < KCl

Identify the key type of 'inter-particle' attractive force that each compound below is capable of using to interact with others of its own kind. Then answer this question: Which correctly lists the three compounds in order of increasing strength of 'inter-particle' attractive force (from weakest to strongest)? PF3 < H2O < KCl H2O < KCl < PF3 KCl < PF3 < H2O KCl < H2O < PF3 H2O < PF3 < KCl PF3 < KCl < H2O

PF3 < H2O < KCl

If you tried to use a can a spray paint that sat out in the summer sunshine, what would you expect to happen.. Paint spray is very weak because the high summer temperature has decreased the pressure inside the paint can. Paint spray is very weak because the high summer temperature has increased the pressure inside the paint can. Paint spray is vigorous because the high summer temperature has increased the pressure inside the paint can. Paint spray is vigorous because the high summer temperature has decreased the pressure inside the paint can.

Paint spray is vigorous because the high summer temperature has increased the pressure inside the paint can.

In which state of matter are the Particles usually very close together? Particles in a Gas phase are usually very close together. Particles in a Liquid phase are usually very close together. Particles in a Solid phase are usually very close together. Particles in a Plasma phase are usually very close together.

Particles in a Solid phase are usually very close together.

Which of these pairs of elements is most likely to form an ionic bond? K and He N and I Pb and F H and Br

Pb and F

Which of these pairs of elements is most likely to form an ionic bond? Pb and F K and He N and I H and Br

Pb and F

The solvent pentane (C5H12) is a liquid at room temperature as is the solvent heptane (C7H16). How is the vapor pressure different in this two solvents? Pentane is a smaller molecule and has a lower vapor pressure. Heptane is a larger molecule and has a lower vapor pressure. Heptane is a smaller molecule and has a higher vapor pressure. Pentane is a smaller molecule and has a higher vapor pressure.

Pentane is a smaller molecule and has a higher vapor pressure.

The solvent pentane (C5H12) is a liquid at room temperature as is the solvent hexane (C6H14). How is the vapor pressure different in this two solvents? Pentane is a smaller molecule and has a higher vapor pressure. Pentane is a smaller molecule and has a lower vapor pressure. Hexane is a smaller molecule and has a higher vapor pressure. Hexane is a larger molecule and has a lower vapor pressure.

Pentane is a smaller molecule and has a higher vapor pressure.

What is the proper order of increasing solute particles sizes... Pure solvent, colloid, solution and suspension. Pure solvent, solution, colloid and suspension. Pure solvent, solution, suspension and colloid. Solution, pure solvent, colloid and suspension.

Pure solvent, solution, colloid and suspension.

Which of these pairs of elements is most likely to form a covalent bond? S and I Ba and Br Sn and I Ne and H

S and I

How do soaps clean? Soap cleans because it contains large molecules which form micelles that trap water on the interior but attract oil and grease on the exterior to form a colloidal dispersion. Soap cleans because it contains large molecules which form micelles that trap oil and grease on the interior but attract water molecules on the exterior to form a colloidal dispersion. Soap cleans because it contains large molecules which form micelles that trap ionic compounds on the interior but attract water molecules on the exterior to form a colloidal dispersion. Soap cleans because it contains large molecules which bind to oil and grease on a one to one basis.

Soap cleans because it contains large molecules which form micelles that trap oil and grease on the interior but attract water molecules on the exterior to form a colloidal dispersion.

Which State of matter has the least spacing between particles. Liquid Gas Solid Plasma

Solid

Which state of matter has strong internal cohesive forces, is not very compressible and can keep its own volume and shape. Gas Liquid Solid Electricity

Solid

Which two states have a fixed volume? Solids and Gases both have a fixed volume. Gases and Liquids both have a fixed volume. Solids and Liquids both have a fixed volume. Gases and Plasma both have a fixed volume.

Solids and Liquids both have a fixed volume.

Which two states of matter normally have a small thermal expansion? Only Solids normally have a small thermal expansion. Gases and Liquids normally have a small thermal expansion. Solids and Liquids normally have a small thermal expansion. Solids and Gases normally have a small thermal expansion.

Solids and Liquids normally have a small thermal expansion.

Which two states of matter have small compressibility? Solids and Liquids usually have small compressibility. Only Solids have small compressibility. Gases and Liquids usually have small compressibility. Solids and Gases usually have small compressibility.

Solids and Liquids usually have small compressibility.

What is true about a solution? Solutes in a true solution will settle out over time: there is no light scattering Tyndall effect and the solution is a homogenous mixture. Solutes in a true solution will not settle out over time: there is no light scattering Tyndall effect and the solution is a homogenous mixture. Solutions in a true solution will settle out over time: there is no light scattering Tyndall effect and the solution is a heterogeneous mixture. Solutes in a true solution will not settle out over time: there is a light scattering Tyndall effect and the solution is a homogenous mixture.

Solutes in a true solution will not settle out over time: there is no light scattering Tyndall effect and the solution is a homogenous mixture.

A homogeneous mixture is also known as a ... Solution Solute Suspension Solvent

Solution

What would be the pH of a solution if 0.0015 moles of KOH was mixed with 0.0010 moles of HNO3? Solution pH = 10.7 Solution pH = 2.8 Solution pH = 11.2 Solution pH = 3.0

Solution pH = 10.7

What would be the pH of a solution if 0.0015 moles of KOH was mixed with 0.0010 moles of HNO3? Solution pH = 2.8 Solution pH = 10.7 Solution pH = 3.0 Solution pH = 11.2

Solution pH = 10.7

What would be the pH of a solution if 0.0010 moles of KOH was mixed with 0.0015 moles of HNO3? Solution pH = 3.0 Solution pH = 11.0 Solution pH = 3.3 Solution pH = 2.8

Solution pH = 3.3

What would be the pH of a solution if 0.0010 moles of KOH was mixed with 0.0010 moles of HNO3? Solution pH = 0 Solution pH = 3.0. Solution pH = 11.0 Solution pH = 7.0

Solution pH = 7.0

What would be the pH of a solution if 0.0010 moles of KOH was mixed with 0.0010 moles of HNO3? Solution pH = 3.0. Solution pH = 0 Solution pH = 7.0 Solution pH = 11.0

Solution pH = 7.0

Which element has the distinguishing electron 5s2? Pb Ba Pa Sn Sr

Which element has the distinguishing electron 5s2? Sn Pa Pb Ba Sr

Pretend you have Beaker A with 1 liter of hot water in it and Beaker B with 1 liter of ice-cold water in it. Then you put 1 drop of red food coloring in both beakers. Into which beaker will the red dye diffuse first. The red food coloring should diffuse more quickly in Beaker B because the cold water molecules are moving around more RAPIDLY which will push the dye around more EASILY. The red food coloring should diffuse more quickly in Beaker B because the cold water molecules are moving around more RAPIDLY which will push the dye around more SLOWLY. The red food coloring should diffuse more quickly in Beaker A because the hot water molecules are moving around more RAPIDLY which will push the dye around more EASILY. The red food coloring should diffuse more quickly in Beaker A because the hot water molecules are moving around more RAPIDLY which will push the dye around more SLOWLY.

The red food coloring should diffuse more quickly in Beaker A because the hot water molecules are moving around more RAPIDLY which will push the dye around more EASILY.

Water is an unusual material because... The gas phase of water is more dense than the liquid phase. The solid phase of water is less dense than the gas phase. The solid phase of water is less dense than the liquid phase. The solid phase of water is more dense than the liquid phase.

The solid phase of water is less dense than the liquid phase.

In order for a solid to form from a liquid what has to happen? The temperature must be low enough so that the self-adhesive forces are less than that the dispersive forces due to thermal agitation. The temperature must be high enough so that the self-adhesive forces are greater than the dispersive forces due to thermal agitation. The temperature must be low enough so that the self-adhesive forces are greater than the dispersive forces due to thermal agitation. The temperature must be high enough so that the self-adhesive forces are less than the dispersive forces due to thermal agitation.

The temperature must be low enough so that the self-adhesive forces are greater than the dispersive forces due to thermal agitation.

When 1 mole of Mg(OH)2 chemically reacts with 1 mole of H2S, what salt is formed? Yes, MgS is the salt magnesium sulfide formed when the cation of the base combines with the anion of the acid. MgS2 is the salt formed H2S is the salt formed. Mg(OH)2 is the salt formed.

Yes, MgS is the salt magnesium sulfide formed when the cation of the base combines with the anion of the acid.

If you open two bottles of perfume which will you smell first. Perfume A which contains small aromatic molecules or Perfume B which contain larger aromatic molecules. You will smell perfume B first because the motion of the air molecules will move the SMALLER aromatic molecules more easily. You will smell perfume B first because the motion of the air molecules will move the LARGER aromatic molecules more easily. You will smell perfume A first because the motion of the air molecules will move the SMALLER aromatic molecules more easily. You will smell perfume A first because the motion of the air molecules will move the LARGER aromatic molecules more easily.

You will smell perfume A first because the motion of the air molecules will move the SMALLER aromatic molecules more easily.

Two pure substances, X and Y, chemically react with one another to form a new pure substance: Z. Observing this chemical reaction, we could conclude that: X and Y are both elements. Z is an element. X and Y are both compounds. Z is a compound. X and Y may or may not be elements. X, Y, and Z are compounds.

Z is a compound. X and Y may or may not be elements.

Which of the following reactions is correctly balanced?

Zn + 2 HC; --> H2 + ZnCl2

Consider the balanced chemical equation below for the reaction of zinc metal with hydrochloric acid (aqueous HCl). Which element is being oxidized? Zn + 2HCL --> H2 + ZNCl2 H in HCl Cl in HCl Zn of the zinc metal

Zn of the zinc metal

Which element has the distinguishing electron 4d2? Ti Zr Sr Ca Sn

Which solution is most basic? [H3O+] = 1 x 10^-13 M pOH = 4 [OH-] = 1 x 10^-3 M pH = 12

[H3O+] = 1 x 10^-13 M

Which solution is most acidic? [H3O+] = 1 x 10^-3 M pOH = 12 pH = 4 [OH-] = 1 x 10^-13 M

[H3O+] = 1 x 10^-3 M

Which is the correct shorthand electron configuration for the Iodine atom? Note that a shorthand electron configuration uses the symbol for the previous noble gas in brackets to indicate the electron configuration of that noble gas, thus emphasizing the outermost electrons. [Kr] 3s2 3d10 3p5 [Kr] 5s2 5d10 5p5 [Kr] 5s2 4d10 5p5 [Kr] 4s2 4d10 4p5 [Cd] 5p5

[Kr] 5s2 4d10 5p5

Which solution is most acidic? pH = 4 pOH = 12 [H3O+] = 1 x 10^-3 M [OH-] = 1 x 10^-13 M

[OH-] = 1 x 10^-13 M

Imagine that separate bottles of hydrogen sulfide gas (H2S, rotten egg smell), nitrous oxide (N2O, laughing gas) and helium are opened at the same time at the front of the lecture hall. From your seat in the back row, you consider the relative speeds of the different gas molecules at room temperature. Which will happen first? you'll inhale the hydrogen sulfide and feel nauseated can't be determined you'll inhale the nitrous oxide and start giggling all will happen at the same time (you'll giggle like Donald Duck, while feeling nauseous) you'll inhale the helium and your voice will sound like Donald Duck

you'll inhale the helium and your voice will sound like Donald Duck

Imagine that separate bottles of hydrogen sulfide gas (H2S, rotten egg smell), nitrous oxide (N2O, laughing gas) and helium are opened at the same time at the front of the lecture hall. From your seat in the back row, you consider the relative speeds of the different gas molecules at room temperature. Which will happen first? you'll inhale the nitrous oxide and start giggling you'll inhale the hydrogen sulfide and feel nauseated you'll inhale the helium and your voice will sound like Donald Duck all will happen at the same time (you'll giggle like Donald Duck, while feeling nauseous) can't be determined

you'll inhale the helium and your voice will sound like Donald Duck

Examine the structures of the molecules below. These are condensed structures, with the hydrogen atoms grouped together with a subscript. You'll need to expand them out, either on paper or in your head, so you're aware of every atom, every covalent bond, and every lone pair of electrons. For each molecule: determine the type(s) of attractive forces the molecule could use to interact with others of its own kind. consider the relative strengths of those attractive forces consider the molecule's mass and surface area Which of these compounds would you predict to have the highest boiling point?Put another way: which compound would require the most heat to overcome the attractive forces between the molecules? CH3-CH2-CH2-O-CH3 CH3-CH2-CH2-CH2-OH CH3-CH2-CH2-C(above O)-OH CH3-CH2-CH2-CH3

CH3-CH2-CH2-C(above O)-OH

Examine the structures of the molecules below. These are condensed structures, with the hydrogen atoms grouped together with a subscript. You'll need to expand them out, either on paper or in your head, so you're aware of every atom, every covalent bond, and every lone pair of electrons. For each molecule: determine the type(s) of attractive forces the molecule could use to interact with others of its own kind. consider the relative strengths of those attractive forces consider the molecule's mass and surface area Which of these compounds would you predict to have the highest boiling point?Put another way: which compound would require the most heat to overcome the attractive forces between the molecules? CH3-CH2-CH2-O-CH3 CH3-CH2-CH2-CH3 CH3-CH2-CH2-CH2-OH CH3-Ch2-Ch2-C^O-OH

CH3-Ch2-Ch2-C^O-OH

Which orbital diagram violates the Pauli Exclusion Principle for pairing the electrons within the same orbital (i.e., the electron must have opposite spin)? ↑↑1s ↑↑2s ↑ 2p↑ 2p↑ 2p ↑↓1s ↑↓2s ↑ 2p↑ 2p↑ 2p ↑↓1s ↑↓2s ↑↓2p↑ 2p 2p

↑↑1s ↑↑2s ↑ 2p↑ 2p↑ 2p

Which orbital diagram violates Hund's Rule for filling orbitals within the same subshell (i.e., electrons prefer to occupy empty orbitals, rather than pairing up)? ↑↓1s ↑↓2s ↑↓2p↑ 2p 2p ↑↓1s ↑↓2s ↑ 2p↑ 2p↑ 2p ↑↑1s ↑↑2s ↑ 2p ↑ 2p ↑ 2p

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