Chemistry Final Exam

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temperature of absolute zero measured in C

-273 C

In the following unbalanced reaction, what is the total decrease in oxidation number for the reduced element? HNO3 + HBr --> NO + Br2 + H2O

-3

In the following unbalanced reaction, what is the total decrease in oxidation number for the reduced element? HNO3 + HI --> NO + I2+ H2O

-3

What is the change in oxidation number of chromium when Na2Cr2O7 becomes CrI3?

-3

What is the change in the oxidation number of chromium when K2Cr2O7 becomes CrCl3?

-3

What is the freezing point of a solution of 0.5 mol of LiBr in 500 mL of water? (Kf= 1.86 C/m)

-3.72 C

C3H5OH

...

How many valence electrons are transferred from the nitrogen atom to potassium in the formation of the compound potassium nitride?

0

The oxidation number of bromine in bromine gas...

0

calcium dihydrogen phosphate

Ca(H2PO4)2

calcium hydroxide

Ca(OH)2

What are quanta of light called?

photons

What is the sum of the oxidation numbers in calcium carbonate?

0

What is the sum of the oxidation numbers in lithium carbonate?

0

The temperature at which the motion of particles theoretically ceases

0 K

molecular compounds

composed of two or more nonmetallic elements

What is the number of moles of solute in a 0.3 molal solution containing 0.10 kg of solvent?

0.3 moles

What is the density of an object having a mass of 8.0 g and a volume of 25 cm^3?

0.32 g

composed of two or more substances chemically combined in a fixed proposition

compound

if 1 mL of 6M HCl is added to 499 mL of water to give exactly a 500 mL solution, what is the molarity of the dilute solution?

0.01M

If 2.0 mL of 6.0M HCl is used to make a 500 mL aqueous solution, what is the molarity of the dilute solution?

0.024M

A 500-g sample of Al2(SO4)3 is reacted with 450 g of Ca(OH)2. A total of 596 g of CaSO4 is produced. (i) What is the limiting reagent in this reaction? (ii) How many moles of excess reagent are unreacted? Al2(SO4)3 + 3Ca(OH)2 --> 2Al(OH)3 + 3CaSO4

(i) Al2(SO4)3 (ii) 1.69 moles

In the following unbalanced reaction, what is the total increase in oxidation number for the oxidized element? H2O + Cl2 + SO2 --> HCl + H2SO4

+2

The oxidation number of magnesium in magnesium chloride is...

+2

What is the oxidation number of magnesium in magnesium iodide?

+2

What is the total increase in oxidation number for the atom that is oxidized in the following balanced redox equation? Cr2O7^-2 + 8H+ + 3SO3^-2 --> 2Cr^+3 + 3SO4^-2 + 4H2O

+2

What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?

10M

How many moles of N2 are in a flask with a volume of 250 mL at a pressure of 300.0 kPa and a temperature of 300 K?

0.03 moles

charge of the strontium ion

+2

charge on the cation CuSO4

+2

What is the change in oxidation number of aluminum in the reaction of aluminum with oxygen gas to make aluminum oxide?

+3

ionic charge on zirconium ion in the ionic compound ZrO2?

+4

What is the change in oxidation number of manganese when MnO2 becomes Mn2O3?

-1

What is the sum of the oxidation numbers in the chlorate ion?

-1

charge of a chloride ion

-1

charge on the polyatomic ions nitrite and chlorite

-1

What is the temperature of 128 K expressed in degrees Celsius?

-145 C

what is the freezing point of a solution that has 5 moles of NaI in 1250 g of water? (Kf= 1.86 C/m)

-15 C

A 55 g piece of copper wire is heated, and the temperature of the wire changes from 19 C to 86 C. The amount of heat absorbed is 343 cal. What is the specific heat of copper?

0.093 cal/g x C

What is the concentration of undissociated acid if the hydrogen-ion concentration is 0.001 M and the acid dissociation constant is 0.0000001?

0.1 M

A gas occupies a volume of 140 mL at 35 C and 97 kPa. What is the volume of the gas at STP?

0.12 L

It takes 770 joules of energy to raise the temperature of 50 g of mercury by 110 C. What is the specific heat of mercury?

0.14 J/g X C

calculate the number of moles of Al2O3 that are produced when 0.60 mol of Fe is produced in the following reaction. 2Al + 3FeO --> 3Fe + Al2O3

0.20 mol

What is the number of moles of solute in 650 mL of a 0.4M solution?

0.26 moles

What is the mole faction of ethanol in a solution of 3 moles of ethanol and 5 moles of water?

0.375

When 45 g of an alloy, at 25 C, are dropped into 100 g of water, the alloy absorbs 956 J of heat. If the final temperature of the alloy is 37 C, what is its specific heat?

0.423

If the solubility of a gas in water is 4.0 g/L when the pressure of the gas above the water is 3.0 atm, what is the pressure of the gas above the water when the solubility of the gas is 1.0 g/L?

0.75 atm

how many liters of a 0.3M solution are needed to give 2.7 moles of solute?

0.9 L

How many iron (II) ions combine with oxygen to form iron (II) oxide?

1

How many pi bonds are formed when sp2 hybridization occurs in the ethene, C2H4?

1

how many half-filled orbitals are in a bromine atom?

1

how many valence electrons are in rubidium?

1

If the [H+] in a solution is 1 x 10^-1 mol/L, what is the [OH-]?

1 x 10^-13

Calculate the hydrogen ion concentration [H+] for an aqueous solution in which [OH-] is 1 x 10^-11 mol/L. Is this solution acidic, basic, or neutral?

1 x 10^-3 M; acidic

If the pH is 9, what is the concentration of hydroxide ion?

1 x 10^-5 M

What is the ion-product constant for water?

1.0 x 10^-14

What is the measurement 1042 L rounded off to two significant digits?

1.0 x 10^3

What is the frequency of ultraviolet light with wavelength 2.94 x 10^-8 m? (c=3.00 x 10^8)

1.02 x 10^16 s^-1

What is the frequency of a radar photon with energy 6.80 x 10^-25 J? (h=6.63 x 10^-34)

1.03 x 10^9 Hz

What is the molality of a solution containing 15 g of solute in 0.5 kg of solvent? (molar mass of solute= 24 g)

1.25m

the diameter of a carbon atom 0.000000000154 m. What is this number expressed in scientific notion?

1.54 x 10^-10 m

What is the molality of a solution containing 5 moles of solute in 3.2 kg of solvent?

1.56m

The volume of a gas is 250 mL at 340.0 kPa pressure. What will the volume be when the pressure is reduced to 50.0 kPa, assuming the temperature remains constant?

1.7 L

The molality of a solution containing 8.1 moles of solute in 4847 g of solvent is...

1.7m

What is the hydrogen-ion concentration if the pH is 3.7?

1.99 x 10^-4 M

If [OH-]= 1 x 10^-4 M, what is the pH of the solution?

10

How many liters of hydrogen gas are needed to react with CS2 to produce 2.50 L of CH4 at stp? 4H2 + CS2 --> CH4 + 2H2S

10.0 L

boiling point of water

100

What is the boiling point of a solution of 0.1 mole of glucose in 200 mL of water? (Kb= 0.512 C/m)

100.26 C

What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (Kb= 0.512 C/m)

101.4 C

What is the bond angle in a water molecule?

105

What is the pressure exerted by 32 g of O2 in a 22 L container at 30 C?

114.45 kPa

How much heat is required to raise the temperature of 5.5 x 10^2 g of aluminum by 10 C? (specific heat= 0.21)

1155 cal

Express the sum of 7.68 m and 5.0 m using the correct number of significant digits

12.7 m

bond angles in ethene, C2H4, are... (90, 109.5, 120, 180)

120

A rigid container of O2 has a pressure of 340 kPa at a temperature of 713 K. What is the pressure at 273 K?

130.18 kPa

Express the sum of 1111 km and 222 km using the correct number of significant digits

1333 km

how many grams of CO are needed to react with an excess of Fe2O3 to produce 209.7 g Fe? Fe2O3 + 3CO --> 3CO2 + 2Fe

157.75 g

What is the mass number for an oxygen atom that has 10 neutrons in its nucleus?

18

Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 19.0 is 55% abundant; the isotope with a mass number of 21 is 45% abundant. What is the average atomic mass for element Z?

19.9 amu

how many electrons are in the highest occupied energy level of copper?

1e-

give the electron configuration for a neutral atom of beryllium

1s2 2s2

give the electron configuration for a neutral atom of chlorine

1s2, 2s2, 2p6, 3s2, 3p5

Electron configuration of the calcium ion

1s2, 2s2, 2p6, 3s2, 3p6

electron configuration of the gallium ion

1s2, 2s2, 2p6, 3s2, 3p6, 3d10

What is the electron configuration of potassium?

1s2, 2s2, 2p6, 3s2, 3p6, 4s1

write the electron configuration for chromium

1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d5

give the electron configuration for a neutral atom of selenium

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p4

Determine the subscript for ammonium in the chemical formula for ammonium dichromate

2

How many electrons are shared in a single covalent bond?

2

How many electrons does barium have to give up to achieve a noble-gas electron configuration?

2

How many energy sublevels are in the second principal energy level?

2

How many unpaired electrons are in a sulfur atom?

2

What is the pH of a solution with a concentration of 0.01 M hydrochloric acid?

2

What will the coefficient of HNO3 be when the following equation is compltely balanced using the smallest whole-number coefficients? HNO3 + MnCl2 + HCl --> NO + MnCl4 + H2O

2

how many nonbonding pairs of electrons are in a water molecule?

2

how many phases are present in a colloid?

2

If the volume of solute is 6 mL and the volume of solution is 300 mL, what is the solute's percent by volume?

2& v/v

What is the pH when the hydrogen ion concentration is 7.0 x 10^-3M?

2.15

What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute= 26 g)

2.2M

The specific heat of silver is 0.24. How many joules of energy are needed to warm 4.37 g of silver from 25 C to 27.5 C?

2.62 J

Convert 6 feet to mm

203.3898 mm

the density of osmium, which is the densest metal, is 22.57 g/cm^3. What is the mass of a block of osmium that measures 1.00 cm x 4.00 cm x 2.50 cm?

226 grams

A mixture of gases at a total pressure of 95 kPa contains N2, CO2, and O2. The partial pressure of the CO2 is 24 kPa and the partial pressure of the N2 is 48 kPa. What is the partial pressure of the O2?

23 kPa

Balance: Ag2(NO3)2 + CuCl2 -->

2AgNO3 + CuCl2 --> 2AgCl + Cu(NO3)2

Balance C2H6 + O2 -->

2C2H6 + 7O2 --> 4CO2 + 6H2O

Balance: C2H6 + O2-->

2C2H6 + 7O2 --> 4CO2 + 6H2O

Balance: propanol is combusted

2C3H7OH + 9O2 --> 6CO2 + 8H2O

Balance: C4H10 + O2 -->

2C4H10 + 13O2 --> 10H2O + 8CO2

Balance: pentanol is combusted

2C5H11OH + 15O2 --> 10CO2 + 12H2O

Balance: hydrochloric acid is added to limestone

2HCl + CaCO3 --> CaCl2 + H2O + CO2

Balance: potassium is added to water

2K + 2H2O --> 2KOH + H2

Balance: Li + H2O-->

2Li + 2H2O --> 2LiOH + H2

Balance: lithium is placed in water

2Li + 2H2O --> 2LiOH + H2

Balance: magnessium is combusted

2Mg + O2 --> 2MgO

Balance Na + H2O -->

2Na + 2H2O --> 2NaOH + H2

Balance: solid sodium is placed in sulfuric acid

2Na + H2SO4 --> Na2SO4 + H2

how many electrons are in the highest occupied energy level of a neutral strontium atom?

2e-

From which orbital in a lithium atom is an electron transferred to form Li+ ?

2s

How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?

3

How many unshared pairs of electrons are in a molecule of hydrogen iodide?

3

how many electrons does a gallium atom give up when it becomes an ion?

3

how many electrons does a nitrogen atom need to gain in order to attain a noble-gas electron configuration?

3

in how many physical states does water exist

3

in the measurement of 0.503 L, which digit is the estimated digit?

3

The gaseous product of a reaction is collected in a 25 L container at 27 C. The pressure in the container is 300 kPa and the gas has a mass of 96 g. HOw many moles of the gas are in the container?

3.01 moles

A 0.500M solution of a weak acid, HX, is only partially ionized. The [H+] was found to be 4.02 x 10^-3. Find the dissociation constant for this acid

3.21 x 10^-5

A gas storage tank has a volume of 3.5 x 10^5 m^3 when the temperature is 27 C and the pressure is 101 kPa. What is the new volume of the tank if the temperature drops to -10 C and the pressure drops to 95 kPa?

3.26 x 10^8

What is the acid dissociation constant of a weak acid if a concentration of 0.3M gives a hydrogen-ion concentration of 0.001 M

3.34 x 10^-6

when a mixture of sulfur and metallic silver is heated, silver sulfide is produced. What mass of silver sulfide is produced from a mixture of 3.0 g Ag and 3.0 g S8? 16Ag + S8 --> 6Ag2S

3.45 g

What is the product of the number 1000 and the measurement 0.00357 m expressed in the correct number of significant layers?

3.57 m

what is the molarity of a solution containing 9 moles of solute in 2500 mL of solution?

3.6M

If the solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the solubility of a gas when the pressure is 202 kPa?

3.75 g/L

How many kilocalories of heat are required to raise the temperature of 225 g of aluminum from 20 C to 100 C? (specific heat= 0.21)

3.8 kcal

A 10-g mass of krypton occupies 15.0 L at a pressure of 210 kPa. Find the volume of the krypton when the pressure is increased to 790 kPa.

3.99 L

if 5.0 g of H2 are reacted with excess CO, how many grams of CH3OH are produced, based on a yield of 86%? CO + 2H2 --> CH3OH

34.12 g

What mass of sucrose, C12H22O11, is needed to make 500 mL of a 0.200M solution?

34.2 g

A balloon filled with helium has a volume of 30.0 L at a pressure of 100 kPa and a temperature of 15.0 C. What will the volume of the balloon be if the temperature is increased to 80 C and the pressure remains constant?

36.77 L

boiling point of water in K

373 K

What is the pressure of 0.520 atm equal to in mm of Hg?

395.2 mm Hg

What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?

3M

Balance the following reaction that occurs in an acidic solution using the redox method. S + NO3- --> SO2 + NO

3S + 4NO3- + 4H+ --> 3SO2 + 4NO + 2H2O

If the hydroxide ion concentration is 10^-10 M, what is the pH of the solution?

4

What coefficient of H+ balances the atoms in the following half-reaction?

4

What coefficient of H+ balances the atoms in the following half-reaction? H+ + MnO2 --> Mn^+2 + H2O

4

What is the total number of covalent bonds normally associated with a single carbon atom in a compound?

4

how many electrons are shared in a double covalent bond?

4

how many valence electrons are in a silicon atom?

4

At what temperature does liquid water have its maximum density?

4 C

How many protons are present in an atom of Be-9?

4 protons

What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL?

4.34 mL

A gas has a pressure of 710 kPa at 227 C. What will its pressure be at 27 C, if the volume does not change?

426 kPa

What is the percentage of water in the hydrate CoCl2 • 6H2O?

45.42%

Calculate the energy required to produce 7 mol Cl2O7 on the basis of the following balanced equation. 2Cl2 + 7O2 + 130 kcal --> 2Cl2O7

455 kcal

what electron configuration of the 4f energy sublevel is most stable

4f14

What is the maximum number of d orbitals in a principal energy level?

5

how many valence electrons are in an atom of phosphorus?

5

If the percent by volume is 2% and the volume of solution is 250 mL, what is the volume of solute in solution?

5 mL

express 0.05 grams in kilograms

5 x 10^-5 kg

the expression of 5008 km in scientific notation is...

5.008 x 10^3 km

what is the sum of 2.7 g and 2.47 g expressed in the correct number of significant digits?

5.2 g

How many mL of a 2.0M NaBr solution are needed to make 200 mL of 0.5M NaBr?

50 mL

how many electrons are there in the highest occupied energy level of atoms in Group 5A elements?

5e-

Which orbital is filled when iodine gains an electron to become a negative ion?

5p

express 0.06 liters in cubic meters

6 x 10^-5 m^3

solid sodium reacts violently with water, producing heat, hydrogen gas, and sodium hydroxide. How many molecules of hydrogen gas are formed when 48.7 g of sodium are added to water? 2Na + 2H2O --> 2NaOH + H2

6.38 x 10^23 molecules

how many grams of liquid water are produced when 60 grams of ice melt

60 grams

how many joules are in 148 calories? (1 cal= 4.18 J)

619 J

when glucose is consumed, it reacts with oxygen in the body to produce carbon dioxide, water, and energy. How many grams of carbon dioxide would be produced if 45 g of C6H12O6 completely reacted with oxygen?

66 g

How many liters of O2 are needed to react completely with 45.0 L of H2S at STP? 2H2S + 3O2 --> 2SO2 + 2H2O

67.5 L

What is the volume of an object with a density of 7.73 g/cm^3 and a mass of 5.40 x 10^2 g?

69.9 cm^3

How many valence electrons does an iodine atom have?

7

If the hydrogen ion concentration is 10^-7 M, what is the pH of the solution?

7

Which of the following measurements is expressed to 3 significant figures? (0.007, 7077, 7.30 x 10^-7, 0.070)

7.30 x 10^-7

What mass of Na2SO4 is needed to make 2.5 L of 2.0M solution?

710 g

How many water molecules are in 39 formula units of calcium chloride dihydrate (CaCl2 • 2H2O)?

78

how many electrons are in the highest occupied energy level of a neutral chlorine atom?

7e-

What is the approximate frequency of a photon having an energy 5 x 10^-24 J? (h= 6.6 x 10^-34 J•s)

8 x 10^9 Hz

What is the result of multiplying 2.5 x 10^10 by 3.5 x 10^-7?

8.75 x 10^3

How many grams of copper sulfate pentahydrate (CuSO4 • 5H2O) would you heat to produce 29.8 g of water?

82.62 g

What is the sum of 6.210 L and 3 L expressed in the correct number of significant digits?

9 L

Aluminum Oxide

Al2O3

Aluminum is a group 3A metal. Which ion does Al typically form?

Al^+3

the first step in balancing a redox reaction by the oxidation number change method

Assign oxidation numbers

Which was originally a tenet of Dalton's atomic theory, but had to be revised about a century ago?

Atoms are tiny indivisible particles

Dalton's atomic theory included which idea? (all atoms of all elements are the same size, atoms of different elements always combine in one-to-one ratios, atoms of the same element are always identical, individual atoms can be seen with a microscope)

Atoms of the same element are always identical

barium chlorate

Ba(ClO3)2

for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure

Boyle's law

chaotic movement of colloidal particles

Brownian motion

ethene

C2H4

ethanol

C2H5OH

Balance: C2H5OH + O2-->

C2H5OH + 3O2 --> 2CO2 + 3H2O

Balance: Ethanol is combusted

C2H5OH + 3O2 --> 2CO2 + 3H2O

butanoic acid

C3H7COOH

Propanol

C3H7OH

propanol

C3H7OH

Balance: C3H8 + O2 -->

C3H8 + 5O2 --> 3CO2 + 4H2O

Balance: C3H8 + O2-->

C3H8 + 5O2 --> 3CO2 + 4H2O

butane

C4H10

Butanol

C4H9OH

Balance: butanol is combusted in oxygen

C4H9OH + 6O2 --> 4CO2 + 5H2O

pentane

C5H12

Balance: pentane is combusted in oxygen

C5H12 + 8O2 --> 5CO2 + 6H2O

cyclohexane

C6H12

Which of the following substances is NOT an electrolyte? (KCl, CCl4, LiCl, Na2SO4)

CCl4

Predict which one of the following compounds would be insoluble in water. (NaCl, HCl, CF4, CuSO4)

CF4

Which of the following substances dissolves most readily in gasoline? (CH4, HCl, NH3, NaBr)

CH4

Which of these would you expect to be soluble in the non polar solvent carbon disulfide, CS2?

CI4

Which of the following substances is less soluble in hot water than in cold water? (CO2, NaCl, NaNO3, KBr)

CO2

Balance: calcium hydroxide reacts with hydrochloric acid

Ca(OH)2 + 2HCl --> CaCl2 + 2H2O

the non-SI scale for temperature

Celsius temperature scale

the volume of a fixed mass of gas is directly proportional to its Kelvin temperature, if the pressure is kept constant

Charle's Law

Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37. The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant?

Cl-35

CuCl2

Copper (II) Chloride

copper (II) bicarbonate

Cu(HCO3)2

At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases

Dalton's Law

this man lived from 460 BC-370 BC and was among the first to suggest the idea of atoms

Democritus

Use Graham's law to calculate how much faster flourine gas, F2, will effuse than chlorine gas, Cl2, will. The molar mass of F2= 38; the molar mass of Cl2= 70.9

F2 effuses 1.366 faster

chemical symbol for iron

Fe

iron (III) oxide

Fe2O3

Iron (III) Chloride

FeCl3

Iron (II) Oxide

FeO

the pressure of a gas is directly proportional to its Kelvin temperature if the volume is kept constant

Gay-Lussac's law

The rate at which a gas will effuse is inversely proportional to the square root of the gas's molar mass

Graham's Law

Which of the following covalent bonds is the most polar? (H-F, H-C, H-H, H-N)

H-F

what is the limiting reagent when 150.0 g of nitrogen react with 32.1 g of hydrogen? N2 + 3H2 --> 2NH3

H2

Which of the following represents a compound (H, H-3, H2O, O-16)?

H2O

What are the acids in the following equilibrium reaction? CN- + H2O -->HCN + OH-

H2O and HCN

Sulfurous acid

H2SO3

sulfurous acid

H2SO3

Balance: H2SO4 + NaOH -->

H2SO4 + 2NaOH --> 2H2O + Na2SO4

Balance: H2SO4 + NaOH-->

H2SO4 + 2NaOH --> 2H2O + Na2SO4

Balance: sulfuric acid reacts with sodium hydroxide

H2SO4 + 2NaOH --> 2H2O + Na2SO4

phosphoric acid

H3PO4

Which of the following shows both the correct formula and correct name of an acid? (HClO2 chloric acid, HNO2 hydronitrous acid, H3PO4 phosphoric acid, HI iodic acid)

H3PO4 phosphoric acid

hydrochloric acid

HCl

Balance: chloric acid reacts with sodium hydroxide

HClO3 + NaOH --> H2O + NaClO3

hypoiodous acid

HIO

iodic acid

HIO3

nitric acid

HNO3

states the impossibility of knowing both velocity and position of a moving particle at the same time

Heisenberg uncertainty principle

at a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid

Henry's law

states that if you add two or more thermochemical equations to give a final equation, you can also add the heats of reaction to give the final heat of reaction

Hess's law of heat summation

FeCl2

Iron (II) Chloride

FeO

Iron (II) oxide

If oxygen is removed from a sample of air as iron rusts, what happens to the total pressure of the air?

It decreases

What happens to the temperature of a liquid as it evaporates?

It decreases

What is the formula of the ion formed when potassium achieves noble-gas electron configuration?

K+

potassium sulfite

K2SO3

Which temperature scale is directly proportional to average kinetic energy?

Kelvin

the SI scale for temperature

Kelvin temperature scale

Of the elements Pt, V, Li, and Kr, which is a nonmetal?

Kr

can accept an electron pair

Lewis acid

Lithium nitrate

LiNO3

MgCl2

Magnesium chloride

Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?

Mendeleev

Balance: Mg + H2SO4

Mg + H2SO4 --> MgSO4 + H2

Magnessium sulfate

MgSO4

Who conducted experiments to determine the quantity of charge carried by an electron?

Millikan

Identify the atom that increases in oxidation number in the following redox reaction: 2MnO2 + 2K2CO3 + O2 --> 2KMnO4 + 2CO2

Mn

Which of the following compounds contains the Mn+3 ion? (MnS, MnBr2, Mn2O3, MnO)

Mn2O3

what is the oxidizing agent in the following reaction: I- + MnO4- --> I2 + MnO2

MnO4-

Which of the following substances dissolves most readily in water? (BaSO4, CaCO3, NH3, CH4)

NH3

What is the reducing agent in the following reaction: 2Na + S --> Na2S

Na

Balance: sodium carbonate reacts with magnessium chloride

Na2CO3 + MgCl2 --> 2NaCl + MgCO3

sodium sulfate

Na2SO4

Balance: sodium sulfate reacts with strontium chloride

Na2SO4 + SrCl2 --> 2NaCl +SrSO4

What is the formula unit of sodium nitride?

Na3N

sodium bicarbonate

NaHCO3

sodium hydroxide

NaOH

Which of the following compounds contains the lead(II) ion? (PbO, PbCl4, Pb2O, Pb2S)

PbO

Which of these elements does not exist as a diatomic molecule? (Ne, F, H, I)

Ne

Which of the following elements has the smallest ionic radius? (Li, K, O, S)

O

melting point of water

O degrees Celsius

Oxygen gas

O2

Which of the following diatomic molecules is joined by a double covalent bond? (O2, Cl2, N2, He2)

O2

Phosphorous diflouride

PF2

each orbital has at most two electrons

Pauli exclusion principle

Lead (II) Nitrate

Pb(NO3)2

Balance Pb(NO3)2 + KCl -->

Pb(NO3)2 + 2KCl --> PbCl2 + 2KNO3

write the formula for the compound rubidium phosphide

Rb3P

The oxidation number of sulfur in each of the following is +6 EXCEPT for... (SO3, Na2SO4, SO4^-2, S2O4^-2)

S2O4^-2

In which of the following compounds is the octet expanded to include 12 electrons? (H2S, PCl3, PCl5, SF6)

SF6

Sulfur hexaflouride

SF6

Which of the following represents a molecular compound? (ZnO, Xe, SO2, BeF2)

SO2

What is the formula of the ion formed when tin achieves a stable electron configuration?

Sn^+4

Which of the following is true about subatomic particles? (electrons are negatively charged and are the heaviest subatomic particle, protons are positively charged and the lightest subatomic particle, neutrons have no charge and are the lightest subatomic particle, the mass of a neutron nearly equals the mass of a proton)

The mass of a neutron nearly equals the mass of a proton

Which of the following is correct concerning subatomic particles? (electron was discovered by Goldstein in 1886, neutron was discovered by Chadwick in 1932, proton was discovered by Thomson in 1880, cathode rays were found to be made of protons)

The neutron was discovered by Chadwick in 1932

If 4 moles of gas are added to a container that already holds 1 mole of gas, how will the pressure change inside the container?

The pressure will be 5 times higher

phenomenon observed when beam of light passes through a colloid

Tyndall effect

Zinc metal

Zn

An ionic bond is a bond between what?

a cation and an anion

each period in the periodic table corresponds to...

a principal energy level

All of the following are physical properties of matter EXCEPT... (mass, color, melting point, ability to rust)

ability to rust

the lowest point on the Kelvin scale

absolute zero

When an electron moves from a lower to a higher energy level, the electron ____________

absorbs a quantum of energy

Lewis acid is a substance that...

accepts a pair of electrons

closeness to true value

accuracy

the closeness of a measurement to its true value is a measure of its what?

accuracy

ratio of the concentration of the dissociated to the undissociated form

acid dissociation constant

the amount of product formed when a reaction is carried out in the laboratory

actual yield

If the hydrogen ion concentration of a solution is 10^-10 M, is the solution acidic, alkaline, or neutral?

alkaline

Which of the following are considered physical properties of a substance... (color and odor, melting and boiling points, malleability and hardness, all of the above)

all of the above

Which of the following statements is part of the kinetic theory? (the particles of a gas move independently of each other, the particles in a gas move rapidly, the particles in a gas are relatively far apart, all of the above)

all of the above

what type of ions have names ending -ide?

anions

homogeneous mixture of water and dissolved substances

aqueous solution

the pressure resulting from the collision of atoms and molecules with objects

atmospheric pressure

the smallest particle of an element that retains the properties of that element

atom

frequencies of light emitted by an element

atomic emission spectrum

region of high probability of finding an electron

atomic orbital

one-half the distance between the nuclei of two atoms when the atoms are joined

atomic radius

tendency of electrons to enter orbitals of lowest energy first

aufbau principle

a device used to measure atmospheric pressure

barometer

What is the best description for a solution with a hydroxide ion concentration of 1 x 10^-4 M?

basic

shape of NO2

bent

shape of O3

bent

shape of a water molecule

bent

sulfur hexaflouride is an example of a... (monoatomic ion, polyatomic ion, binary compound, polyatomic compound)

binary compound

a colligative property related to a decrease in the vapor pressure of a solution

boiling point elevation

In the following unbalanced reaction, which atom is oxidized? HNO3 + HBr --> NO + Br2 + H2O

bromine

mixture in which particle size averages between 1 nm and 1000 nm

colloid

Ca(OH)2

calcium hydroxide

CaO

calcium oxide

device used to measure the heat absorbed or released during a chemical or physical process

calorimeter

CO

carbon monoxide

Which of the following compounds is a nonelectrolyte? (sodium bromide, magnesium sulfate, copper chloride, carbon tetrachloride)

carbon tetrachloride

type of ion formed by Group 2A elements

cation

element with lowest electronegativity value

cesium

process in which substances are changed into different substances

chemical reaction

in the reaction of calcium with chlorine, which atom is the oxidizing agent?

chlorine

ClO2

chlorine dioxide

the next to the last step in balancing a redox reaction by the oxidation number change method

choose coefficients to make the change in oxidation number equal to 0

CoCl2

cobalt (II) chloride

measure of the amount of solute dissolved in a specified quantity of solvent

concentration

An ideal gas CANNOT be... (condensed, cooled, heated, compressed)

condensed

a covalent bond in which the shared electron pair comes from only one of the atoms

coordinate covalent bond

the number of ions of opposite charge surrounding each ion in a crystal

coordination number

a repetition of properties occurs when elements are arranged in order of increasing atomic number

periodic law

Which of the following does NOT involve a physical change? (mixing, melting, grinding, decomposing)

decomposing

As the density of a substance increases, then the volume of a mass....

decreases

N2O

dinitrogen monoxide

N2O5

dinitrogen pentaoxide

N2O4

dinitrogen tetraoxide

What type of acid is sulfuric acid ? (monoprotic, diprotic, triprotic, none of the above)

diprotic

acid with two ionizable protons

diprotic acid

colloidal particles spread throughout a suspension

dispersed phase

a process in which a liquid is boiled to produce a vapor that is condensed again into a liquid

distillation

separating a solid from a liquid by evaporating the liquid

distillation

a covalent bond in which two pairs of electrons are shared

double covalent bond

What is the shape of the 3p atomic orbital?

dumbbell

MnO4-

permanganate

compound that will conduct current in the liquid state or in the aqueous solution

electrolyte

a negatively charged subatomic particle

electron

arrangement of electrons around atomic nucleus

electron configuration

a depiction of valence electrons around the symbol of an electron

electron dot structure

ability of an atom to attract electrons when the atom is in a compound

electronegativity

Which of the following are free to drift in metals (protons, electrons, neutrons, cations)?

electrons

subatomic particles that are transferred to form positive and negative ions

electrons

What causes the shielding effect to remain constant across a period? (electrons are added to the same principal energy level, electrons are added to different principal energy levels, the charge on the nucleus is constant, the atomic radius increases)

electrons are added to the same principle energy level

substance that cannot be changed into simpler substances by chemical means

element

colloid of a liquid in a liquid

emulsion

in the Bohr model of the atom, the electron in an orbit has a fixed what?

energy

The principal quantum number indicates what property of an electron?

energy level

another name for the acid dissociation constant

equilibrium constant

C2H6

ethane

which of the following is a physical change... (corrosion, explosion, evaporation, rotting of food)

evaporation

the reactant that is not completely used up in a reaction

excess reagent

a colligative property related to the fact that ice will form at higher temperatures in the Great Lakes than in the ocean

freezing point depression

number of wave cycles passing a point per unit of time

frequency

Which of the following electromagnetic waves have the highest frequencies? (ultraviolet light waves, x-rays, microwaves, gamma rays)

gamma rays

what state of matter is a vapor

gas

what state of matter takes both the shape and volume of its container?

gas

What expression is generally used for solubility?

grams of solute per 100 grams of solvent

lowest energy level

ground state

vertical column in the periodic table

group

Elements that are characterized by the filling of p orbitals are classified as...

groups 3A-8A

part of a sample having uniform composition and properties

phase

reaction showing either the reduction or the oxidation reaction

half-reaction

an anion of chlorine or other halogen

halide ion

Which of the following is NOT an example of matter? (air, heat, smoke, water vapor)

heat

heat content of a system at constant pressure

heat capacity

the change in enthalpy that accompanies the formation of a compound from its elements

heat of formation

the energy required to melt a solid at its melting point

heat of fusion

the enthalpy change for a chemical reaction exactly as it is written

heat of reaction

the enthalpy change caused by dissolving a substance

heat of solution

not uniform in composition

heterogeneous mixture

which of the following cannot be considered a single phase? (pure solid, pure liquid, homogeneous mixture, heterogeneous mixture)

heterogeneous mixture

describes mixture with a uniform composition

homogeneous

HBr

hydrobromic acid

HCl

hydrochloric acid

in the reaction of hydrogen with iodine, which atom is oxidized?

hydrogen

a type of bond that is very important in determining the properties of water and of important biological molecules such as proteins and DNA

hydrogen bond

What causes water's low vapor pressure?

hydrogen bonding

What is responsible for the high thermal energy required to melt ice?

hydrogen bonding

bonds between adjacent water molecules

hydrogen bonds

primarily responsible for holding water molecules together in the liquid state

hydrogen bonds

When dissolved in water, acids produce... (negative ions, polyatomic ions, hydrogen ions, oxide ions)

hydrogen ions

H2O2

hydrogen peroxide

Bronsted-Lowry acid

hydrogen-ion donor

HI

hydroiodic acid

a crystal that absorbs water vapor from the air

hygroscopic

why is ice less dense than water?

ice has a molecular structure that is an open framework held together by hydrogen bonds

PV=nRT

ideal gas law

describes liquids that are insoluble in one another

immiscible

how is the modern periodic table arranged?

increasing atomic number

What is the key difference between a liquid and a gas?

intermolecular attractions

HIO3

iodic acid

Which of the following elements has the ability to undergo sublimation? (Oxygen, carbon, sodium, iodine)

iodine

the force of attraction binding oppositely charged ions together

ionic bond

Which of the following are weak electrolytes in water? (ionic compounds that partially dissassociate in water, ionic compounds that are soluble, polar compounds that ionize, nonpolar compounds that do not ionize)

ionic compounds that partially dissociate in water

Which of the following decreases with increasing atomic number in Group 2A? (shielding effect, ionic size, ionization energy, number of electrons)

ionization energy

energy required to remove an electron from an atom

ionization energy

When the vapor pressure of a liquid is equal to the atmospheric pressure, what happens to the liquid?

it begins to boil

How does the energy of an electron change when the electron moves closer to the nucleus?

it decreases

How does the surface tension of water compare with the surface tension of most other liquids?

it is higher

During a phase change, what happens to the temperature of a substance?

it remains constant

When an iron is ground into powder, what happens to its mass?

it stays the same

How does atomic radius change from top to bottom in a group in the periodic table?

it tends to increase

SI unit of energy

joule

the energy an object has due to its motion

kinetic energy

all matter consists of tiny particles that are in constant motion

kinetic theory

N2O

laughing gas

the reactant that determines the amount of product that can be formed in a reaction

limiting reagent

What element in the second period has the largest atomic radius?

lithium

Li2O

lithium oxide

Mg(OH)2

magnesium hydroxide

Which hydroxide compound yields the lowest concentration of hydroxide ions in aqueous solution? (sodium hydroxide, potassium hydroxide, calcium hydroxide, magnesium hydroxide)

magnesium hydroxide

the next to the last step in balancing a redox reaction by the half reaction method

make the electron changes equal

MnO2

manganese (IV) oxide

An example of an extensive property of matter is... (temperature, pressure, mass, hardness)

mass

amount of matter an object contains

mass

the heat capacity of an object depends on its...

mass

the quantity of matter an object contains

mass

this is conserved in every ordinary chemical reaction

mass

type of element that is a good conductor of heat and electric current

metal

the attraction of valence electrons for metal ions

metallic bond

What is the metric system prefix for the quantity 0.000001?

micro-

a physical blend of two or more components

mixture

number of moles of solute dissolved in 1 kg of solvent

molality

The amount of heat needed to melt one mole of a solid at a constant temperature

molar heat of fusion

number of moles of solute dissolved in 1 L of solution

molarity

ratio of moles of solute in solution to total number of moles of both solvent and solute

mole faction

Which type of solid has the highest melting point?

network solid

a subatomic particle with no charge

neutron

What is the correct name for the N^-3 ion?

nitride ion

HNO2

nitrous acid

the central part of an atom, containing protons and neutrons

nucleus

this quantity can always be used in the same way as moles when interpreting balanced chemical equations

number of molecules

What does NOT change when a solution is diluted by the addition of solvent? (volume of solvent, mass of solvent, number of moles of solute, molarity of solution)

number of moles of solute

What do colligative properties depend upon?

number of solute particles in a solution

Isotopes of the same element have different...

numbers of neutrons

atoms react so as to acquire the stable electron structure of a noble gas

octet rule

How many hydrogen bonds can be formed between one hydrogen atom in a water molecule and oxygen atoms of surrounding water molecules?

one

How is an emulsifying agent characterized?

one polar end and one nonpolar end

under what conditions can potassium bromide conduct electricity?

only when melted or dissolved in water

the letter "p" in the symbol 4p3 indicates what?

orbital shape

Cu--> Cu^+2 + 2e-... wat type of reaction is this?

oxidation

integer related to the number of electrons under an atom's control

oxidation number

substance that accepts electrons (agent)

oxidizing agent

Which atom in a water molecule has the greatest electronegativity?

oxygen atom

negative logarithm of the hydrogen ion concentration

pH

If the hydroxide-ion concentration is 1 x 10^-12 M, what is the pH of the solution?

pH=2

SI unit of pressure

pascal

the ratio of the actual yield to the theoretical yield

percent yield

HClO4

perchloric acid

horizontal row in the periodic table

period

a covalent bond between two atoms of significantly different electronegativities

polar bond

The Ka of carbonic acid is 4.3 x 10^-7. H2CO3 --> H+ + HCO3-... this means that H2CO3 is...

poor hydrogen-ion donor

What is the charge of a cation?

positive

Which of the following elements has the smallest first ionization energy? (sodium, calcium, potassium, magnesium)

potassium

Which of the following compounds is a strong electrolyte? (ammonia, acetic acid, sugar, potassium sulfate)

potassium sulfate

narrowness of range of measurements

precision

a substance formed in a chemical reaction

product

C3H8

propane

C3H7OH

propanol

a positively charged subatomic particle

proton

particles that are found in the nucleus of an atom

protons and neutrons

energy needed to move an electron from one energy level to another

quantum

starting substance in a chemical reaction

reactant

substance that donates electrons (agent)

reducing agent

A compound held together by ionic bonds is called....

salt

When an acid reacts with a base, what compounds are formed?

salt and water

solution containing maximum amount of solute

saturated solution

known or estimated in a measurement

significant figure

a covalent bond in which only one pair of electrons is shared

single covalent bond

Which element increases its oxidation number in the following reaction? 2Na + 2H2O --> 2NaOH + H2

sodium

NaHCO3

sodium bicarbonate

Which of the following substances is the most soluble in water? (sodium chloride, methane, bromine, carbon)

sodium chloride

Which of the following compounds is an electrolyte? (rubbing alcohol, sugar, carbon tetrachloride, sodium hydroxide)

sodium hydroxide

Na2O

sodium oxide

Na2SO4

sodium sulfate

which state of matter is characterized by having a definite shape and definite volume?

solid

Which of the following occurs as temperature increases? (solubility decreases, solubility increases, solubility remains the same, molarity doubles)

solubility increases

dissolved particle

solute

solute ions or molecules are surrounded by solvent molecules

solvation

dissolving medium

solvent

What occurs in salvation?

solvent molecules surround solute ions

the ∆Hsoln is... (always negative, always positive, sometimes both, always 0)

sometimes positive, sometimes negative

quantity of heat required to change the temperature of 1 g of a substance by 1 C

specific heat

discrete bundle of electromagnetic energy

spectrum

shape of XeF4

square planar

law of conservation of mass

states that the mass of the reactants is equal to the mass of the products

average kinetic energy of water molecules is greatest in... (steam at 100 C, liquid water at 90 C, liquid water at 373 K, ice at O C)

steam at 100 C

a depiction of the arrangement of atoms in molecules and polyatomic ions

structural formula

What is an acid according to Arrhenius?

substance that ionizes to yield protons in aqueous solution

Which of the following is NOT a common hydrate? (epsom salt, borax, sugar, alum)

sugar

Which of the following mixtures is NOT a colloid? (fog, milk, paint, sugar water)

sugar water

Which of the following is NOT a cation? (Iron iii ion, sulfate, Ca+2, mercurous ion)

sulfate

SO2

sulfur dioxide

H2SO4

sulfuric acid

H2SO3

sulfurous acid

how can you calculate the change in enthalpy

sum of products minus sum of reactants

If a chrystal added to an aqueous solution causes many particles to come out of the solution, the original solution was...

supersaturated

solution containing more solute than can theoretically dissolve at a given temperature

supersaturated solution

inward force tending to minimize surface area of a liquid

surface tension

interferes with hydrogen bonding between water molecules

surfactant

mixture in which particle size averages greater than 1000 nm in diameter

suspension

shape of the methane molecule

tetrahedral

What is the basis of a metallic bond?

the attraction of metal ions to mobile electrons

What does the symbol ∆H stand for?

the heat of reaction for a chemical reaction

Which is a typical characteristic of an ionic compound? (electron pairs are shared among atoms, the ionic compound has a low solubility in water, the ionic compound is described as a molecule, the ionic compound has a high melting point)

the ionic compound has a high melting point

What does the number 84 in the name krypton-84 represent?

the mass number

If the volume of a container of gas is reduced, what will happen to the pressure inside the container?

the pressure will increase

What happens to the solubility of a gas, in a liquid, if the partial pressure of the gas above the liquid decreases?

the solubility decreases

For group 2A metals, which electron is the most difficult to remove?

the third

If a liter of water is heated from 20 C to 50 C, what happens to its volume?

the volume increases

the maximum amount of product that could be formed from given amounts of reactants

theoretical yield

Which of the following is NOT a characteristic of most ionic compounds? (they are solids, they have low melting points, when melted they conduct an electric current, they are composed of metallic and nonmetallic elements)

they have low melting points

What characteristic of metals make them good electrical conductors?

they have mobile valence electrons

how many significant figures are in the measurement 40,500 mg?

three

Sn3(PO4)2

tin (II) phosphate

Why do atoms share electrons in covalent bonds?

to attain a noble-gas electron configuration

type of element characterized by the presence of electrons in the d orbital

transition metal

an electron in the highest occupied energy level of an atom

valence electron

What is the name given to the electrons in the highest occupied energy level of an atom?

valence electrons

gaseous state of substance that is a liquid or solid at room temperature

vapor

a measure of the force exerted by a gas above a liquid

vapor pressure

According to the Heisenberg uncertainty principle, if the position of a moving particle is known, what other quantity CANNOT be known?

velocity

this is conserved only in reactions where the temperature is constant and the number of moles of gaseous reactants is the same as that of gaseous products

volume

Which of the following substances has the highest specific heat? (steel, water, alcohol, chloroform)

water

another term for the water of hydration

water of crystallization

Which of the following is an example of a phase? (pressure, water vapor, temperature, triple point)

water vapor

distance between wave crests

wavelength

compound that ionizes incompletely in aqueous solution

weak electrolyte

the force of gravity on an object

weight

the first step in balancing a redox reaciton by the half-reaction method

write the equation showing ions seperately

Use the information below to calculate the enthalpy change for the following reaction. 2NO2 --> N2O4; N2 + 2O2-->2NO2 (∆H=67.7 kJ); N2 + 2O2--> N2O4 (∆H= 9.7 kJ)

∆H= -58


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