Chemistry 1151- Final Exam Study Guide

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Naturally occurring carbon consists of three isotopes: 12 C, 13 C, and 14 C. State the number of protons, neutrons, and electrons in each of the three isotopes.

12C6 6p, 6n, 6e 13C6 6p, 7n, 6e 14C6 6p, 8n, 6e

How many moles of iron are present in 3.15 × 1024 atoms of iron? A) 5.23 moles B) 1.90 moles C) 292 moles D) 0.523 moles E) 1.90 × 1048 moles

Hydrogen bonds are a major factor in the structure of A) DNA. B) hydrogen chloride. C) dry ice. D) air. E) table salt.

Identify the Brønsted-Lowry acids in the following reaction. H2O + CO32- → HCO3- + OH A) H2O/HCO3- B) CO32-/HCO3- C) OH-/HCO3- D) CO32-/OHE) H2CO3/H2O

Identify the noble gas in the following list. A) helium B) nitrogen C) oxygen D) gold E) chlorine

Give the names of the elements with the following symbols: A. P B. Al C. Mn D. H E. K

A. P-Phosphorus B. Al-Aluminum C. Mn-Manganese D. H-Hydrogen E. K-Potassium

Double and triple bonds form because A) the atoms involved have high electronegativities. B) single covalent bonds do not give all of the atoms in the molecule eight valence electrons. C) one of the atoms in the molecule has more than eight valence electrons. D) the ions involved have charges larger than one. E) there is at least one hydrogen atom involved in the bond.

A homogeneous mixture that does not settle out upon standing is A) an element. B) a colloid. C) a suspension. D) homogeneous. E) hydrated.

A liquid has a volume of 34.6 mL and a mass of 46.0 g. What is the density of the liquid? A) 1.00 g/mL B) 1.33 g/mL C) 0.752 g/mL D) 1330 g/mL E) 0.663 g/mL

A reaction that releases energy as it occurs is classified as a(n) A) endothermic reaction. B) exothermic reaction. C) oxidation-reduction reaction. D) catalyzed reaction. E) decomposition reaction.

A slice of pizza contains 29 g of carbohydrate, 13 g of protein and an unknown amount of fat. If the pizza contains 280 kcal, how many grams of fat are present? Report the answer to 2 significant figures. A) 10. g B) 12 g C) 25 g D) 55 g E) 250 g

A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution, H2O is the A) solute. B) solvent. C) solution. D) solid. E) ionic compound.

A solution which has [ H3O+] = 6.7 × 10-8 M is A) acidic. B) basic. C) neutral.

A solution which has [OH-] = 4.6 × 10-6 M is A) acidic. B) basic. C) neutral.

A solution with a pH of 4 is A) extremely acidic. B) moderately acidic. C) neutral. D) slightly basic. E) extremely basic.

According to Henry's law, the solubility of a gas in a liquid A) decreases as the gas pressure above the liquid increases. B) increases as the gas pressure above the liquid increases. C) remains the same as the temperature increases. D) depends on the liquid polarity. E) depends on the liquid density.

According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as A) a base. B) an acid. C) a source of hydroxide ions. D) a source of H- ions. E) a proton acceptor.

According to the Atomic Theory, A) all atoms are different. B) atoms are neither created nor destroyed during a chemical reaction. C) atoms of the same element combine to form compounds. D) all matter is made up of tiny particles called electrons. E) a compound can contain different numbers of atoms as long as it has the same kinds of atoms.

An example of kinetic energy is A) a coiled spring. B) running water. C) a tree. D) natural gas. E) chemical energy.

Calculate the molar mass of magnesium chloride, MgCl2 . A) 24.3 g B) 95.2 g C) 125.9 g D) 59.8 g E) 70.0 g

Choose the best electron-dot structure for CH2Cl2

Coins in a piggy bank is a(n) A) compound. B) heterogeneous mixture. C) element. D) homogeneous mixture. E) None of the above.

Consider an isotope of sodium with a mass number of 25. The number of neutrons in this isotope of sodium is A) 11. B) 14. C) 16. D) 25. E) 32.

Diamond has a density of 3.52 g/mL. What is the volume in cubic centimeters of a diamond with a mass of 15.1 g? A) 4.3 cm3 B) 4.29 cm3 C) 0.233 cm3 D) 53 cm3 E) 53.2 cm3

What is the metric relationship between grams and micrograms? A) 1 g = 100 μg B) 1 g = 1 000 000 μg C) 1 g = 0.000 001 μg D) 1 g = 1000 μg E) 1 g = 0.001 μg

What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL? A) 0.267 M B) 0.150 M C) 0.200 M D) 6.67 M E) 0.100 M

What is the pH of a solution with [ H3O+] = 3.0 × 10-3 M? A) 3.0 × 10-3 B) 2.52 C) 3.0 D) -2.52 E) 9.0

What type of reaction is: CH4 + 2O2 → CO2 + 2H2O + 218 kcal? A) an endothermic reaction B) an exothermic reaction C) a single replacement reaction D) a combination reaction E) a decomposition reaction

What volume of a 2.00 M KCl solution is required to prepare 500. mL of a 0.100 M KCl solution? A) 0.0400 mL B) 25.0 mL C) 2.00 mL D) 1.00 × 104 mL E) 5.00 × 102 mL

When 200. mL of water are added to 100. mL of 12% KCl solution the final concentration of KCl is (Assume the volumes add.) A) 12%. B) 4.0%. C) 36%. D) 6.0%. E) 8.0%.

When 3.05 moles of CH4 are mixed with 5.03 moles of O2 the limiting reactant is CH4 + 2O2 → CO2 + 2H2O A) CH4. B) O2. C) CO2. D) H2O.

Which element would have physical and chemical properties similar to chlorine? A) Ar B) Br C) S D) O E) P

Which of the following compounds contains a polar covalent bond? A) NaF B) HCl C) Br2 D) MgO E) O2

Which of the following correctly gives the best coefficients for the reaction below? N2H4+ H2O2 → N2+ H2O A) 1, 1, 1 ,1 B) 1, 2, 1, 4 C) 2, 4, 2, 8 D) 1, 4, 1, 4 E) 2, 4, 2, 4

Which of the following could be a buffer? A) NaF B) HF + NaF C) HF + H2O D) NaF + H2O E) NaCl + HF

Which of the following describes an oxidation reaction? A) loss of electrons or loss of oxygen B) loss of electrons or gain of oxygen C) loss of electrons or gain of hydrogen D) gain of electrons or gain of oxygen E) gain of electrons or loss of H

Which of the following electron configurations is impossible? A) 1s 22s 22p 63s 23p 1 B) 1s 22s 42p 63s 23p 3 C) 1s 22s 22p 63s 23p 5 D) 1s 22s 22p 63s 23p 6 E) 1s 22s 22p 63s 23p 3

Which of the following is a neutralization reaction? A) KCl + NaNO3→ KNO3 + NaCl B) HNO3+ KOH → H2O + KNO3 C) H2O + SO3 → H2SO4 D) 4Na + O2 → 2Na2O E) 2NO2 → 2NO + O2

Which of the following is a physical change? A) baking a cake B) dry ice subliming C) fermenting grapes to produce wine D) digesting a meal E) a tomato ripening

Which of the following is an example of potential energy? A) chewing food B) water stored in a reservoir C) burning wood D) a fan blade turning E) riding an exercise bike

Which of the following is correctly identified? A) NH3, strong acid B) NaOH, strong base C) HCl, weak acid D) H2CO3, strong acid E) Ca(OH)2, weak base

Which of the following is the basic unit of mass in the SI? A) pound B) kilogram C) milligram D) microgram E) gram

How many milliliters of 0.100 M Ba(OH)2 are required to neutralize 20.0 mL of 0.250 M HCl? A) 100. mL B) 50.0 mL C) 25.0 mL D) 0.250 mL E) 0.50 mL

How many significant figures are in the measured number 0.00208 m? A) six B) two C) three D) four E) five

How many valence electrons are in the electron-dot structures for the elements in group 3A(13)? A) 1 B) 2 C) 3 D) 4 E) 6

In a neutralization reaction, how many moles of HClO4 react with 1 mole of Al(OH)3? A) 1 B) 2 C) 3 D) 4 E) 5

In a solution, the solvent A) is a liquid. B) can be a liquid or gas. C) can be a solid, liquid, or gas. D) is never a solid. E) is the substance present in the smallest concentration.

In the following reaction, when the equation is correctly balanced, what is the correct coefficient for H2?Fe(s) + HCl(aq) → FeCl3(aq) + H2(g) A) 1 B) 2 C) 3 D) 4 E) 5

In the reaction of nitrogen gas, N2 , with hydrogen gas, H2 , to form ammonia gas, NH3 , how many moles of hydrogen are needed to react with two moles of nitrogen? A) 2 moles B) 4 moles C) 6 moles D) 8 moles E) 10 moles

What is the coefficient of hydrogen, H2 , when the following equation is balanced? Al + H2SO4 → Al2(SO4)3+ ? H2 A) 1 B) 2 C) 3 D) 4 E) 5

What is the correct answer for the calculation ? A) 0.65645 B) 0.656 C) 0.66 D) 1.52 E) 1.5

What is the formula for aluminum nitrite? A) Al2NO2 B) AlNO3 C) Al(NO2)3 D) Al2(NO3)3 E) Al2(NO2)2

What is the ionic charge of an ion with 13 protons and 10 electrons? A) 1+ B) 2+ C) 3+ D) 2- E) 3-

What is the mass of 53 mL of ethanol, which has a density of 0.79 g/mL? A) 67.1 g B) 41.9 g C) 42 g D) 67 g E) 53 g

What is the molar mass of sodium phosphate, Na3PO4 ? A) 119 g B) 308 g C) 164 g D) 226 g E) 354 g

What is the pH of a solution with [OH-] = 2.0 × 10-10 M? A) 9.70 B) -9.70 C) 4.30 D) -4.30 E) 2.0 × 10-10

What is the symbol of the element in Period 4 and Group 2? A) Be B) Mg C) Ca D) C E) Si

What is the volume of a cube that measures 4.00 cm on each side? A) 16.0 mL B) 64.0 L C) 64.0 mL D) 64.00 mL E) 0.640 L

What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH? A) 0.075 L B) 0.25 L C) 0.75 L D) 0.083 L E) 750 L

What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH? A) 3.0 L B) 0.50 L C) 2.0 L D) 4.5 L E) 0.22 L

When 60.0 g of CH4 reacts with excess O2, the actual yield of CO2 is 112 g. What is the percent yield? CH4 + 2O2 → CO2 + 2H2O A) 53.6 % B) 187 % C) 67.9 % D) 46.4 %

What is the molar mass of sucrose (C12H22O11)? A) 29.0 g B) 50.2 g C) 210 g D) 342 g E) 182 g

What is the molarity of a KOH solution if 25.0 mL neutralizes 35.0 mL of a 0.200 M HCl solution? A) 0.267 M B) 0.143 M C) 0.200 M D) 0.280 M E) 0.100 M

What is the molarity of a solution that contains 3.25 moles of NaNO3 in 250. mL of solution? A) 3.25 M B) 6.50 M C) 0.0130 M D) 13.0 M E) 2.60 M

What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution? A) 0.500 M B) 1.00 M C) 1.50 M D) 2.00 M E) 4.00 M

What is the symbol of the element in Group 4A(14) and Period 2? A) Be B) Mg C) Ca D) C E) Si

When 10.0 g of NH3 reacts, the actual yield of N2 is 8.50 g. What is the percent yield? 4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(l) A) 85.0% B) 51.5% C) 20.6% D) 41.3% E) 8.5%

When 2610 + 11.7 + 0.22 are added, the answer to the correct number of decimal places is A) 2621.92. B) 2621.9. C) 2621. D) 2620. E) 2600.

When 4 moles of aluminum are allowed to react with an excess of chlorine gas, Cl2 , how many moles of aluminum chloride are produced? A) 1 mole B) 2 moles C) 3 moles D) 4 moles E) 5 moles

When KCl dissolves in water A) the Cl- ions are attracted to dissolved K+ ions. B) the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule. C) the K+ ions are attracted to Cl- ions on the KCl crystal. D) the K+ ions are attracted to the partially negative oxygen atoms of the water molecule. E) the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.

When a reaction is at equilibrium, A) all reaction stops. B) no more reactants are converted to products. C) the reaction is no longer reversible. D) the forward and reverse reactions occur at the same rate. E) the products and reactants have the same energy content.

When hyperventilation (rapid breathing) causes a patient to exhale large amounts of CO2, the blood pH rises in a condition called A) metabolic acidosis. B) metabolic alkalosis. C) respiratory acidosis. D) respiratory alkalosis. E) pulmonary distress.

When solutions of KCl and Pb(NO3)2 are mixed, a precipitate forms. Which of the following is the balanced equation for the double replacement reaction that occurs? A) KCl(aq) + Pb(NO3) 2(aq) → KNO3(aq) + PbCl2(s) B) KNO3(aq) + PbCl2(s) → KCl(aq) + Pb(NO3) 2(aq) C) K+(aq) + NO3-(aq) → KNO3(aq) D) 2KCl (aq) + Pb(NO3)2(aq) → 2KNO3(aq) + PbCl2 (s) E) KCl(aq) + Pb(NO3)2(aq) → KNO3(aq) + PbCl(s)

When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is A) dilute. B) polar. C) nonpolar. D) saturated. E) unsaturated.

When you open a bottle of a soft drink and leave it open, the drink eventually goes flat. This happens because the equilibrium between carbonic acid and carbon dioxide shifts to produce A) more carbonic acid. B) more water. C) more oxygen. D) more carbon dioxide. E) more hydrogen ions.

Which of the following elements is a metal? A) nitrogen B) fluorine C) argon D) strontium E) phosphorus

Which of the following elements is a noble gas? A) oxygen B) chlorine C) bromine D) argon E) nitrogen

Which of the following gives the balanced equation for this reaction? K3PO4 + Ca(NO3 )2 → Ca3 (PO4 )2 + KNO3 A) KPO4 + CaNO3 + KNO3 B) K3PO4 + Ca(NO3 )2 → Ca3 (PO4 )2 + 3KNO3 C) 2K3PO4 + Ca(NO3 )2 → Ca3 (PO4 )2 + 6KNO3 D) 2K3PO4 + 3Ca(NO3 )2 → Ca3 (PO4 )2 + 6KNO3 E) K3PO4 + Ca(NO3 )2 → Ca3 (PO4 )2 + KNO3

Which of the following is a characteristic of nonmetals? A) shiny B) malleable C) good conductors of heat D) low melting points E) good conductors of electricity

Which of the following is a chemical change? A) cutting a rope B) bending a steel rod C) making a snowman D) burning sugar E) melting gold

) A red blood cell will undergo crenation in A) water. B) 0.5% NaCl. C) 3% glucose. D) 5% glucose. E) 7% NaCl.

0.50 mole of NaCl is added to 1.0 kg of water. The freezing point of the solution will be ________. A) 0.00 °C B) 0.93 °C C) 1.86 °C D) -0.93 °C E) -1.86 °C

1.25 moles of PbO2 have a mass of A) 191 g. B) 279 g. C) 178 g. D) 239 g. E) 299 g.

2H2O2 → 2H2O + O2 How many moles of oxygen gas can 0.88 mole of hydrogen peroxide (H2O2) produce, if decomposition is complete? A) 0.50 mole B) 0.88 mole C) 1.8 moles D) 2.0 moles E) 0.44 mole

4.00 moles of sodium have a mass of A) 4.60 g. B) 11.0 g. C) 23.0 g. D) 44.0 g. E) 92.0 g.

A 10.0 mL of 0.121 M H2SO4 is neutralized by 17.1 mL of KOH solution. The molarity of the KOH solution is A) 0.207 M. B) 0.4141 M. C) 0.0708 M. D) 0.428 M. E) 0.142 M.

A 2.5 g sample of french fries is placed in a calorimeter with 500.0 g of water at an initial temperature of 21 °C. After combustion of the french fries, the water has a temperature of 48 °C. What is the caloric value (kcal/g) of the french fries? A) 14 kcal/g B) 11 kcal/g C) 0.14 kcal/g D) 4.2 kcal/g E) 5.4 kcal/g

A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all reactants have been converted to products. C) all products have been removed from the reaction mixture. D) the catalyst has been used up. E) the rate of the forward reaction equals the rate of the reverse reaction.

A nugget of gold with a mass of 521 g is added to 50.0 mL of water. The water level rises to a volume of 77.0 mL. What is the density of the gold? A) 10.4 g/mL B) 6.77 g/mL C) 1.00 g/mL D) 0.0518 g/mL E) 19.3 g/mL

A potato contains 20 g of carbohydrate. If carbohydrate has a caloric value of 4 kcal/g, how many kcal are obtained from the carbohydrate in the potato? A) 5 kcal B) 20 kcal C) 40 kcal D) 60 kcal E) 80 kcal

A value of 345 cm is a measure of A) density. B) mass. C) temperature. D) volume. E) distance.

An anion always A) has a positive charge. B) contains a group of two or more atoms with a positive charge. C) contains a metal and a nonmetal. D) forms covalent bonds. E) has a negative charge.

An ionic compound A) has a net positive charge. B) has a net negative charge. C) contains only cations. D) contains only anions. E) has a net charge of zero.

Choose the best electron-dot structure for OCl2

The correct formula for a compound formed from the elements Al and O is A) AlO. B) Al2O. C) Al3O2 . D) AlO3 . E) Al2O3 .

The correct name for the compound N2O3 is A) nitrogen oxide. B) nitrogen trioxide. C) dinitride trioxide. D) dinitrogen oxide. E) dinitrogen trioxide.

The correct name of the compound is NCl3 A) nitrogen chloride. B) trinitrogen chloride. C) nitrogen(III) chloride. D) nickel chloride. E) nitrogen trichloride.

The energy of motion is referred to as A) work. B) freezing. C) specific heat. D) potential energy. E) kinetic energy.

The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is Kc = 2 × 1011. This means that the reaction mixture at equilibrium is likely to consist of A) mostly starting materials. B) an equal mixture of products and reactants. C) twice as much starting material as product. D) twice as much product as starting material. E) mostly products

The number of dots in the electron dot structure of nitrogen is A) one. B) two. C) three. D) four. E) five.

The strongest interactions between atoms of helium He are examples of A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces.

The strongest interactions between molecules of hydrogen ( H2) are A) ionic bonds. B) hydrogen bonds. C) polar covalent. D) dipole-dipole. E) dispersion forces.

The strongest interactions between molecules of iodine I2 are examples of A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces.

Using a kidney machine to remove waste products from the blood is known as ________. A) osmosis B) osmolysis C) autolysis D) hemolysis E) hemodialysis

What element has the electron configuration 1s22s22p63s23p2? A) carbon B) oxygen C) sulfur D) iron E) silicon

What is the [ H3O+] in a solution with [OH-] = 1 × 10-12 M? A) 1 × 10-12 M B) 1 × 102 M C) 1 × 10-7 M D) 1 × 10-8 M E) 1 × 10-2 M

What is the [OH-] in a solution that has a [ H3O+] = 2.0 × 10-4 M? A) 2.0 × 10-10 M B) 5.0 × 10-10 M C) 1.0 × 10-10 M D) 2.0 × 10-4 M E) 5.0 × 10-11 M

What is the correct formula for iron(III) sulfide? A) Fe2S2 B) Fe2S C) FeS D) FeS2 E) Fe2S3

What is the molar mass of Mg3 (PO4 )2 , a substance formerly used in medicine as an antacid? A) 71.3 g B) 118 g C) 150. g D) 214 g E) 263 g

What is the pH of a solution with [ H3O+] = 1 × 10-9 M? A) 1.0 × 10-5 M B) -9.0 C) 5.0 D) -5.0 E) 9.0

What is the symbol for the ion with 19 protons and 18 electrons? A) F+ B) F C) Ar+ D) K- E) K+

What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH? A) 18 mL B) 0.13 mL C) 13 mL D) 120 mL E) 8.0 × 102 mL

What volume of 2.5% (m/v) KOH can be prepared from 125 mL of a 5.0% KOH solution? A) 0.0040 mL B) 63 mL C) 0.10 mL D) 125 mL E) 250 mL

When a piece of magnesium metal is added to hydrochloric acid, what gas is produced? A) oxygen B) chlorine C) nitrogen D) carbon dioxide E) hydrogen

When a solid is converted directly to a gas, the change of state is called A) freezing. B) melting. C) boiling. D) condensation. E) sublimation.

Which of the following elements does NOT exist as a diatomic molecule? A) hydrogen B) nitrogen C) chlorine D) oxygen E) carbon

Which of the following examples illustrates a number that is correctly rounded to three significant figures? A) 4.05438 grams to 4.054 grams B) 0.03954 grams to 0.040 grams C) 103.692 grams to 103.7 grams D) 109,526 grams to 109 500 grams E) 20.0332 grams to 20.0 grams

Which of the following is a property of a solid? A) It takes the shape of the container. B) It fills the volume of the container. C) The particles move at a rapid rate. D) The interactions between its particles are very weak. E) The particles have fixed positions and are very close together.

Which of the following is often used to determine an individual's percentage of body fat? A) temperature B) height C) weight loss D) weight gain E) density

Which of the following is the largest unit? A) millimeter B) micrometer C) meter D) decimeter E) kilometer

Which of the following is the smallest unit? A) gram B) milligram C) kilogram D) decigram E) microgram

Which of the following is the strongest acid? A) H3PO4 B) NH4+ C) NaOH D) H2CO3 E) HCl

Which of the following substances contains a nonpolar covalent bond? A) H2O B) NaCl C) NH3 D) MgF2 E) N2

Which one of the following elements forms two or more ions with different ionic charges? A) K B) F C) Ca D) O E) Fe

he name of Al2(SO4)3 is A) aluminum(III) sulfate. B) dialuminum trisulfate. C) dialuminum sulfate. D) dialuminum trisulfide. E) aluminum sulfate.

List all of the elements that match the description. A.metals in Group 4A (14) Sn, Pb, C, Si, Ge B.nonmetals in Group 5A (15) Bi, N, P, As, Sb C.metalloids in Group 4A (14) C, Si, Ge, Sn, Pb

List all of the elements that match the description. A. metals in Group 4A (14) Sn, Pb B. nonmetals in Group 5A (15) N, P C. metalloids in Group 4A (14) Si, Ge

groups

contain elements with similar properties in vertical columns

Ionization energy decreases down a

group and increases going across a period from left to right

ionic compounds consist of

positive and negative charges held together by the strong electrical attractions between oppositely charged ions

In the periodic table, elements are arranged according to

properties

All atoms of an element have the same number of

protons and the same atomic number

Metalloids are located along the heavy

zigzag line

Ionization energy is the energy required to remove one of the outermost electrons

•As the distance from the nucleus to the valence electrons increases, the ionization energy decreases. •The ionization energy is low for metals and high for the nonmetals.

Write the formula and symbol of an ion with 16 protons and 18 electrons

•The element with 16 protons is sulfur, with the symbol S. •An ion of sulfur with 18 electrons gives sulfur a charge of 2−. •The sulfide ion is S2−

Polyatomic ions

•are a group of covalently bonded atoms with an overall ionic charge. •often consist of a nonmetal such as phosphorus, sulfur, carbon, or nitrogen covalently bonded to oxygen atoms .•usually have a 1−, 2−, or 3− charge. •have a negative charge, except for NH4+, ammonium, which has a positive charge

Isotopes are

•are atoms of the same element. •have different mass numbers. •have the same number of protons but different numbers of neutrons. •can be distinguished by their atomic symbols

Metals, except for hydrogen located on the left of the periodic table, are :

•are shiny and ductile, and conduct heat and electricity. •are solids, except for mercury (Hg), which is a liquid.

In Dalton 's atomic theory , atoms are

•are tiny particles of matter. •of an element are similar to each other and different from those of other elements .•of two or more different elements combine to form compounds. •are rearranged to form new combinations in a chemical reaction. -Atoms are never created or destroyed during a chemical reaction

Ionic compounds

•consist of positive and negative ions. •have attractions called ionic bonds between positively and negatively charged ions. •have high melting points. •are solids at room temperature.

Metalloids located along the heavy zigzag line on the periodic table (except for aluminum and oganesson)

•exhibit properties of metals and nonmetals. •are better conductors than nonmetals but not as good as metals. •are used as semiconductors and insulators, because they can be modified to function as conductors or insulators

Group 2A (2) elements are called

alkaline earth metals

periods

are horizontal rows of elements, counted from top to bottom of the table as Periods 1−7

Group numbers are written where ?

at the top of each vertical column. •Use the letter A for representative elements (Groups 1A-8A). •Use the letter B for transition elements (Groups 3B-12B)

Number of protons =

atomic number

Atomic size •is determined by the atom's

atomic radius,the distance between the nucleus and the outermost electrons. •increases for representative elements from top to bottom of the periodic table. •decreases within a period as a result of increased number of protons in the nucleus

unlike charges

attract one another

What is the formula of carbon tetraiodide? A) CI B) CI4 C) C4I D) CI3 E) C2I4

Nonmetals located on the right side of the periodic table are

-are dull, brittle, and poor conductors but often good insulators. -have low densities and melting points

•Recall that 1cm3 =

1 mL · Therefore, 1000 mL = 1000 cm3 = 1L

The number of particles in 1 mole of hydrogen gas is ________.

6.02 × 1023

What is the correct form of the equilibrium constant for this reaction? 2H2O2 (g) ⇌ 2H2O (g) + O2 (g)

What is a buffer solution?

A system that minimises pH changes when small amounts of an acid or a base are added

) The equation for the formation of ammonia from nitrogen and hydrogen is shown below. What is the form of the equilibrium constant? 3H2(g) + N2(g) ⇌ 2NH3(g)

0.50 mole of KCl is added to 2.0 kg of water. The boiling point of the solution will be ________ the boiling point of pure water. A) higher than B) lower than C) the same as

1.00 pint of milk has a volume of how many milliliters? (2 pints = 1 quart) A) 472 mL B) 530. mL C) 1000 mL D) 1890 mL E) 106 mL

2SO2(g) + O2(g) ⇌ 2SO3(g) For the reaction at equilibrium, if O2 is added, the amount of SO2 present will A) decrease. B) increase. C) stay the same.

3.00 moles of NO2 have a mass of A) 138 g. B) 46.0 g. C) 30.0 g. D) 90.0 g. E) 45.0 g.

A hydrogen bond is A) an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom on another molecule. B) a covalent bond between H and O. C) an ionic bond between H and another atom. D) a bond that is stronger than a covalent bond. E) the polar O-H bond in water.

A patient needs to receive 85 grams of glucose every 12 hours. What volume of a 5.0%(m/v) glucose solution needs to be administered to the patient each 12 hours? A) 1700 mL B) 60 mL C) 6000 mL D) 17 mL E) 204 mL

A polar covalent bond is found in which of these compounds? A) H2O B) F2 C) NaCl D) H2 E) N2

A reaction that can proceed in either the forward or the reverse direction as written is called a ________ reaction. A) reversible B) miniscule C) microscopic D) solid phase E) favored

A red blood cell will undergo hemolysis in A) water. B) 0.9% NaCl. C) 5% glucose. D) 5% NaCl. E) 10% glucose.

A sample of silicon has three naturally occurring isotopes: Si-28 (mass 28.0 amu); Si-29 (mass 29.0 amu) and Si-30 (mass = 30.0 amu). If the average atomic mass of silicon is 28.1 amu, which isotope is the most abundant? A) Si-28 B) Si-29 C) Si-30 D) All isotopes have the same natural abundance.

A serving of fish contains 50.g of protein and 4.0 g of fat. If protein has a caloric value of 4.0 kcal/g and fat has 9.0 kcal/g, how many kcal are in the serving? Report the answer to 2 significant figures. A) 240 kcal B) 54.0 kcal C) 470 kcal D) 220 kcal E) 490 kcal

A solution which has [OH-] = 3.4 × 10-12 M is A) acidic. B) basic. C) neutral..

A solution with the same osmotic pressure as the blood is A) isotonic to the blood. B) hypotonic to the blood. C) hypertonic to the blood. D) nontonic to the blood. E) molar to the blood.

According to the Arrhenius concept, if NaOH were dissolved in water, it would act as A) a base. B) an acid. C) a source of hydronium ions. D) a source of H- ions. E) a proton donor.

An aqueous mixture containing starch (a colloid), NaCl, glucose, and albumin (a colloid) is placed in a dialyzing bag and immersed in distilled water. Which of the following correctly describes the location of the indicated substance after dialysis? A) albumin, inside B) starch outside C) albumin inside and outside D) water inside only E) starch inside and outside

An intravenous replacement solution contains 4.0 mEq/L of Ca2+ ions. How many grams of Ca2+ are in 3.0 L of the solution? A) 0.24 g B) 0.80 g C) 0.40 g D) 240 g E) 4.0 g

Any reaction that absorbs 150 kcal of energy can be classified as A) endothermic. B) exothermic. C) activated. D) reduction. E) oxidation.

Avogadro's number is the number of A) particles in 1 mole of a substance. B) amu in 1 mole of a substance. C) grams in 1 mole of a substance. D) moles in 6.02 × 1023 grams of an element. E) moles in 6.02 × 1023 amu of an element.

Calculate the molar mass of potassium chloride, KCl. A) 74.6 g B) 54.5 g C) 6.74 g D) 67.4 g E) 19.0 g

Carbon monoxide binds to hemoglobin 140 times more strongly than oxygen does. What does this tell you about the equilibrium constants for the two reactions of hemoglobin with carbon monoxide and oxygen? A) The equilibrium constant for the binding of CO is greater. B) The equilibrium constant for the binding of oxygen is greater. C) The concentration of carbon monoxide at equilibrium is twice that of oxygen. D) Oxygen and carbon monoxide have the same formula mass. E) Oxygen and carbon monoxide react with hemoglobin in different fashions.

Consider a neutral atom with 30 protons and 34 neutrons. The atomic number of the element is A) 30. B) 32. C) 34. D) 64. E) 94.

Consider a neutral atom with 30 protons and 34 neutrons. The number of electrons in this atom is A) 30. B) 32. C) 34. D) 64. E) 94.

During the process of diluting a solution to a lower concentration, A) the amount of solute does not change. B) the amount of solvent does not change. C) there is more solute in the concentrated solution. D) the volume of the solution does not change. E) water is removed from the concentrated solution.

For Kw, the product of [ H3O+] and [OH-] is A) 1.0 × 10-14. B) 1.0 × 10-7. C) 1.0 × 10-1. D) 1.0. E) 1.0 × 1014

For the following reaction, the equilibrium constant Kc is 0.60 at a certain temperature. If the concentration of NO(g) and NOBr(g) are both 0.50 M,at equilibrium, what is the concentration of Br2(g)? 2NO(g) + Br2(g) ⇌ 2NOBr(g) A) 1.7 M B) 0.60 M C) 0.36 M D) 2.8 M E) 1.0 M

For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. Bromine can be liquefied easily and removed from the reaction vessel as it is formed. If this is done, how will it affect the equilibrium reaction? 2NOBr(g) ⇌ 2NO(g) + Br2(g) A) More products will be made as Br2 is removed. B) There will be a larger proportion NOBr in the vessel when equilibrium is reached. C) Less NO will be made. D) The pressure in the vessel will increase. E) The equilibrium constant will change.

For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. The reaction is endothermic. What do you expect to happen to the concentration of NO if the temperature is doubled? 2NOBr(g) ⇌ 2NO(g) + Br2(g) A) The concentration of NO will increase. B) The concentration of NO will decrease. C) There will be no change in [NO]. D) A catalyst will be needed to make a change in concentration. E) The change in concentration of [NO] will depend on the size of the vessel.

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane. Which starch solution will decrease in volume as osmosis occurs? A) 4% B) 10% C) Neither exerts osmotic pressure. D) They exert equal osmotic pressures. E) They exert opposite osmotic pressures.

How many calories are required to raise the temperature of a 35.0 g sample of iron from 25 °C to 35 °C? Iron has a specific heat of 0.108 cal/g °C. A) 38 cal B) 1.1 cal C) 3.8 cal D) 93 cal E) 130 cal

How many electrons will lithium gain or lose when it forms an ion? A) lose 1 B) gain 5 C) lose 2 D) lose 3 E) gain 1

How many equivalents are present in 5.0 moles of Al3+? A) 15 Eq B) 1.3 Eq C) 5.0 Eq D) 0.67 Eq E) 3.0 Eq

How many grams of Fe2O3 are there in 0.500 mole of Fe2O3 ? A) 79.9 g B) 35.9 g C) 63.8 g D) 51.9 g E) 160. g

How many grams of NO are required to produce 145 g of N2 in the following reaction? 4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(l) A) 186 g B) 155 g C) 125 g D) 129 g E) 145 g

How many kilograms are in 30.4 lb? A) 13.8 kg B) 14 kg C) 67 kg D) 66.88 kg E) 66.9 kg

How many milliliters of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H3PO4? A) 7.50 mL B) 2.50 mL C) 0.833 mL D) 5.00 mL E) 15.0 mL

If the electronegativity difference between elements X and Y is 2.1, the bond between the elements XY is A) ionic. B) nonpolar ionic. C) nonpolar covalent. D) polar covalent. E) impossible.

In a catalytic converter in an automobile, the reaction of carbon monoxide with oxygen produces A) carbon dioxide. B) carbon and more oxygen. C) water. D) methane. E) nitrogen oxide.

In a catalyzed chemical reaction, one function of a catalyst is to A) increase the number of successful reactant collisions. B) decrease the concentration of reactants. C) change the equilibrium concentrations of the products and reactants. D) increase the energy given off during the reaction. E) increase the temperature at which the reaction is carried out.

In the following gas phase reaction, Kc is much less than 1. At equilibrium, which of the following statements is true? COCl2(g) ⇌ CO(g) + Cl2(g) A) The concentration of reactant is much greater than the concentration of products. B) The concentration of products is much greater than the concentration of reactants. C) The concentrations of products and reactants are approximately equal. D) A catalyst will increase the concentration of products formed. E) At equilibrium, the concentrations of reactants and products are equal.

In the reaction of carbon dioxide with water to give carbonic acid, the only gaseous component is the carbon dioxide. What will happen to the equilibrium concentration of carbonic acid if the pressure of carbon dioxide is increased in the container? A) The concentration of carbonic acid will increase. B) The carbonic acid concentration will decrease. C) The carbonic acid concentration will stay the same. D) There will be twice as much carbonic acid as carbon dioxide. E) There will be more water available for the reaction.

In the reaction of nitrogen and hydrogen to give ammonia, all the reactants and products are A) gases. B) liquids. C) solids. D) boiling. E) frozen.

In this reaction, what is the coefficient for calcium oxide? CaO(s) + CO2(g) → CaCO3(s) A) 1 B) 2 C) 3 D) 4 E) 5

In water, a substance that partially ionizes in solution is called a A) weak electrolyte. B) nonelectrolyte. C) semiconductor. D) nonconductor. E) strong electrolyte.

In which of the following are the pH values arranged from the most acidic to the most basic? A) 1, 3, 6, 8, 11, 14 B) 2, 5, 7, 9, 10, 1.1 C) 14, 10, 7, 4, 3, 1 D) 14, 10, 7, 1, 3, 5 E) 7, 10, 14, 4, 3, 1

Mg3N2 (s) + 6H2O(l) → 3Mg (OH)2 (s) + 2NH3 (g) What is the correct form of the conversion factor needed to convert the number of moles of H2O to the number of moles of NH3 produced?

PCl5 (g) ⇌ PCl3 (g)+ Cl2 (g) For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl5 present will A) decrease. B) increase. C) double. D) stay the same. E) triple.

Predict whether the equilibrium of the following reaction favors reactants or products: NH4+ + H2O ⇌ NH3 + H3O+ A) Reactants are favored. B) Products are favored. C) Neither side is favored.

The Group 8A(18) elements A) are unreactive and are rarely found in combination with other elements. B) are good conductors of electricity. C) melt at high temperatures. D) are liquids at room temperature. E) react vigorously with water.

The VSEPR theory allows us to determine the most favorable A) shape of a molecule. B) charge on an ion. C) color of a compound. D) bond type for a molecule. E) formula for a compound.

The ability of an atom to attract the shared electrons in a covalent bond is its A) electronegativity. B) bonding ability. C) polarity. D) ionic character. E) nonpolarity.

The ammonia molecule ( NH3) is A) a polar molecule with polar bonds. B) a nonpolar molecule with polar bonds. C) a nonpolar molecule with nonpolar bonds. D) a polar molecule with nonpolar bonds. E) a polar molecule with ionic bonds.

The carbon tetrachloride molecule, CCl4 , has the shape of a A) tetrahedron. B) square. C) cube. D) circle. E) sphere.

The correct formula for sulfuric acid is A) H2SO4. B) H2SO3. C) H2SO4-. D) H2SO3-. E) SO42-.

The correct formula for the compound formed from Mg and S is A) MgS. B) MgS2. C) Mg2S. D) Mg2S2 E) Mg2S3

The correct symbol for the isotope of potassium with 22 neutrons is A) 41K19. B) 19K41. C) 37P15. D) 15P37. E) 22K19

The formation of a gas resulting from the escape of high-energy particles from the surface of a liquid is known as A) evaporation. B) deposition. C) boiling. D) melting. E) sublimation.

The metric base unit for length is the A) meter. B) inch. C) millimeter. D) kilometer. E) foot.

The molar mass of C3H8O2 is A) 76.0 g. B) 60.0 g. C) 29.0 g. D) 69.0 g. E) 52.0 g.

The molarity (M) of a solution refers to A) moles of solute/L of solution. B) moles of solute/L of solvent. C) moles of solute/100 mL of solution. D) grams of solute/100 mL of solution. E) grams of solute/L of solution.

The name given to an aqueous solution of HNO3 is A) nitric acid. B) nitrous acid. C) hydrogen nitrate. D) hydronitrogen acid. E) hyponitric acid.

The rate of any chemical reaction can be determined by observing A) the amount of product formed in a unit of time. B) the ratio of product concentration to reactant concentration. C) the percent composition of the final product. D) the theoretical yield of the reaction. E) the number of chemical bonds broken and remade.

The reaction for the decomposition of PCl5 to chlorine and PCl3 is shown below. PCl5(g) ⇌ PCl3(g) + Cl2(g) If the equilibrium concentrations are [PCl5] = 1.0 M, [PCl3] = 0.10 M, [Cl2] = 0.10 M, what is the value of the equilibrium constant? A) 1.0 × 10-2 B) 1.0 × 10-4 C) 10 × 10-2 D) 1.0 × 102 E) 2.0 × 10-2

The reaction of hemoglobin with oxygen can be written as follows. Hb + O2 ⇌ HbO2 If the amount of oxygen available to the blood decreases significantly, what happens to the individual involved? A) Hypoxia results. B) Anemia results. C) Nitrogen narcosis results. D) Oxygen poisoning results. E) Acclimatization results.

The shape of the carbon dioxide (CO2) is A) linear. B) square. C) pyramidal. D) hexagonal. E) bent.

The strongest interactions in the compound sodium fluoride, NaF, are examples of A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces.

The temperature of liquid nitrogen is - 196 °C. What is the corresponding reading on the Kelvin scale? A) 77 K B) -127 K C) -91 K D) 48 K E) 146 K

Valence electrons are electrons located A) in the outermost energy level of an atom. B) in the nucleus of an atom. C) in the innermost energy level of an atom. D) throughout the atom. E) in the first three shells of an atom.

What is oxidized and what is reduced in the following reaction? 2Al(s) + 3Br2 (g) → 2AlBr3 (s) A) Al is oxidized and Br2 is reduced. B) AlBr3 is reduced and Br2 is oxidized. C) Al is reduced and Br2 is oxidized. D) AlBr3 is reduced and Al is oxidized. E) AlBr3 is oxidized and Al is reduced.

What is the [ H3O+] in a solution that has a [OH-] = 5.0 × 10-2 M? A) 2.0 × 10-12 M B) 2.0 × 10-2 M C) 1.0 × 10-14 M D) 2.0 × 10-4 M E) 5.0 × 10-12 M

What is the correct answer for the calculation of a volume (in mL) with measured numbers 28.58/16*8.02? A) 0.22 mL B) 0.223 mL C) 57 mL D) 14 mL E) 14.3 mL

What is the correct form of the equilibrium constant for the reaction of hydrogen and oxygen to form water? The equation is: 2H2(g) + O2(g) ⇌ H2O(g)

What is the correct formula for the oxide ion? A) O2- B) O- D) O2+ E) O3+

What is the density of a substance with a mass of 45.00 g and a volume of 26.4 mL? A) 1.70 g/mL B) 1.7 g/mL C) 0.59 g/mL D) 0.587 g/mL E) 45.0 g/mL

What is the electron configuration for aluminum? A) 1s 22s 22p 63s 23p 1 B) 1s 22s 22p 63s 23p 3 C) 1s 22s 22p 63s 23p 5 D) 1s 22s 22p 63s 23p 6 E) 1s 22s 22p 63s 23p 8

What is the formula of a compound that contains Na+ and PO43- ions? A) Na3PO4 B) NaPO4 C) Na2PO3 D) Na3PO3 E) Na3P

What is the formula of the nitride ion? A) N3- B) NO2- C) NO3 3- D) NO32- E) NO3-

What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution? A) 2.5 M B) 1.0 M C) 5.0 M D) 10. M E) 2.0 M

What is the name of the medical condition of an asthmatic patient with a blood pH of 7.30? A) respiratory acidosis B) respiratory alkalosis C) metabolic acidosis D) metabolic alkalosis E) diabetes mellitus

What is the new mass/volume (m/v)% of a KOH solution that is prepared by diluting 110 mL of a 6% (m/v) KOH solution to 330 mL? A) 2% B) 1% C) 6% D) 12% E) 18%

What is the pH of a solution with [OH-] = 1 × 10-4 M? A) 10.0 B) -10.0 C) 4.0 D) -4.0 E) 1.0 × 10-10

When 85.0 g of CH4 are mixed with 160. g of O2 what is the maximum amount of CO2 that can be produced? CH4 + 2O2 → CO2 + 2H2O A) 2.50 moles B) 5.00 moles C) 5.31 moles D) 7.81 moles

When solutions of NaCl and AgNO3 are mixed, A) a precipitate of AgCl forms. B) a precipitate of NaNO3 forms. C) no precipitate forms. D) precipitate of NaNO3 and AgCl form. E) a precipitate of AgCl2 forms.

Which of the following descriptions of a subatomic particle is correct? A) A proton has a positive charge and a mass of approximately 1 amu. B) An electron has a negative charge and a mass of approximately 1 amu. C) A neutron has no charge and its mass is negligible. D) A proton has a positive charge and a negligible mass. E) A neutron has a positive charge and a mass of approximately 1 amu.

Which of the following elements has the lowest electronegativity? A) Li B) C C) N D) O E) F

Which of the following elements is a nonmetal? A) nitrogen B) sodium C) iron D) silver E) calcium

Which of the following equilibrium constants indicates the reaction that gives the smallest amount of product? A) Kc = 5 × 10-10 B) Kc= 5 × 10-1 C) Kc= 5 × 100 D) Kc= 5 × 101 E) Kc= 5 × 1010

Which of the following is NOT true for the atoms 13N, 14N, and 15N? A) They all have the same mass number. B) They are isotopes. C) They all have the same atomic number. D) They all have 7 protons. E) They all have 7 electrons.

Which of the following is an example of a physical change? A) grinding coffee beans B) baking a cake C) converting water to hydrogen and oxygen D) digesting a cheeseburger E) burning coal

Which of the following is the strongest acid? A) HF (Ka for HF is 7.2 × 10-4) B) HCN (Ka for HCN is 4.9 × 10-10) C) HCNO (Ka for HCNO is 2 × 10-4) D) H3BO3 (Ka for H3BO3 is 5.4 × 10-10)

Which solution has the lowest pH? A) a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate B) a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate C) a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate D) a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate E) All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.

A temperature of 41 °F is the same as A) 5 °C. B) 310 °C. C) -9 °C. D) 16 °C. E) 42 °C.

A) To Find: 41 F -32 divided by 9/5 or 1.8 =5

650. J is the same amount of energy as A) 155 cal. B) 2720 cal. C) 650 cal. D) 1550 cal. E) 2.72 cal.

A) To find: 650 J / 4.184 J= 155 cal

A dose of aspirin of 5.0 mg per kilogram of body weight has been prescribed to reduce the fever of an infant weighing 8.5 pounds. The number of milligrams of aspirin that should be administered is A) 19 mg. B) 53 mg. C) 1.6 mg. D) 5.0 mg. E) 0.59 mg.

A) To find: Convert 8.5 lbs to kg = 3.86 kg Next , 3.86 kg x 5.0 mg = 19.3 mg

How many pounds are in 3.5 kg? A) 7.7 lb B) 1.59 lb C) 0.629 lb D) 1.6 lb E) 7.70 lb

A) To find: 3.5 kg x 2.2 lbs

5.21 cm is the same distance as A) 0.0521 m. B) 52.1 dm. C) 5.21 mm. D) 0.00521 km. E) 5210 m.

A) To find: 5.21 cm / 100 m= 0.0521 m

Grapes are $1.49 per pound. What is the cost of 1.20 kg of grapes? A) $3.93 B) $2.73 C) $1.79 D) $0.81 E) $0.56

A) To find: convert 1.20 kg to lbs , 1.2 x 2.2=2.64 Next multiply 2.64 lbs by $1.49= 3.93

Which of the following subatomic particles fits each of the descriptions below? protons, neutrons, or electrons A. found outside the nucleus B. have a positive charge C.have mass but no charge

A. Electron B. Proton C.Neutron

What is the correct formula for the iron(II) ion? A) Fe+ B) Fe2+ C) Fe3+ D) Fe2- E) Fe3-

Complete each of the following statements with decreasesor increases. A. Going down Group 6A (16), the ionization energy _______. B. Going across Period 3, from left to right, the atomic size _______. C. Going down Group 2A (2), the metallic character _______

A. Going down Group 6A (16), the ionization energy decreases. B. Going across Period 3, from left to right, the atomic size decreases. C. Going down Group 2A (2), the metallic character increases

Write the atomic symbols for atoms with the following subatomic particles: A. 8 protons 8 neutrons 8 electrons B. 17 protons 20 neutrons 17 electrons C. 47 protons 60 neutrons 47 electrons

A. O B.Cl C.Ag

Write the names of the following compounds. A.CaO___________ B.Al2O3___________ C.MgCl2___________

A. The name of CaO is calcium oxide. B. The name of Al2O3 is aluminum oxide. C. The name of MgCl2 is magnesium chloride.

Write the correct chemical symbols for each of the following elements: A. iodine B. iron C. magnesium D. zinc E.nitrogen

A. iodine- I B. iron-Fe C. magnesium-Mg D. zinc-Zn E.nitrogen-N

Write chemical formulas for the following compounds: A. nickel(II) sulfide B. zinc chloride C. iron(III) oxide

A.nickel(II) sulfideNiS B.zinc chlorideZnCl2 C.iron(III) oxideFe2O3

Identify each of the following elements as a metal, a nonmetal, or a metalloid: A.sodium B.chlorine C.silicon D.iron E.carbon

A.sodium -metal B.chlorine-non-metal C.silicon -mellatoid D.iron-metal E.carbon-non metal

What is the element with the abbreviated electron configuration [Kr]5s24d8? A) Ni B) Pd C) Pt D) Kr E) Xe

2Mg + O 2 → 2MgO2 The number of moles of oxygen gas needed to react with 4.0 moles of Mg is A) 1.0 mole. B) 2.0 moles. C) 3.0 moles. D) 4.0 moles. E) 6.0 moles.

3H2(g) + N2(g) ⇌ 2NH3(g) + heat For the reaction at equilibrium, if the temperature is raised, the amount of N2 will A) decrease. B) increase. C) stay the same.

What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution? A) 34 M B) 2.0 M C) 0.50 M D) 0.029 M E) 1.0 M

A calculator answer of 423.6059 must be rounded off to three significant figures. What answer is reported? A) 423 B) 424 C) 420 D) 423.6 E) 423.7

) 2SO2(g) + O2(g) ⇌ 2SO3(g) For the reaction at equilibrium, if O2 is removed, the amount of SO2 present will A) decrease B) increase C) stay the same

) A cheeseburger from a fast food restaurant contains 19 g of fat, 20. g of carbohydrate, and 28 g of protein. How many kcal of energy does the cheeseburger contain? (The accepted caloric values for foods are 4.0 kcal/g for carbohydrate, 9.0 kcal/g for fat, and 4.0 kcal/g for protein.) Report the answer to 2 significant figures. A) 70. kcal B) 360 kcal C) 17 kcal D) 630 kcal E) 280 kcal

1.0 mole of NaCl is added to 1.0 kg of water. The freezing point of the solution will be ________ the freezing point of pure water. A) higher than B) lower than C) the same as

What is the element with the electron configuration 1s22s22p63s23p5? A) Be B) Cl C) F D) S E) Ar

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane. Which of the following occurs in this system? A) Water flows equally in both directions. B) There is a net flow of water from the 4% starch solution into the 10% starch solution. C) There is a net flow of water from the 10% starch solution into the 4% starch solution. D) Water does not cross the membrane at all. E) Starch moves out of the 10% starch solution into the 4% starch solution.

Given the following: X, X, X, and X. Which are isotopes of each other? A) X and X are isotopes of each other; and X and X are isotopes of each other. B) X and X are isotopes of each other. C) X, X, X, and X are isotopes of each other. D) None are isotopes of each other.

How many electrons will chlorine gain or lose when it forms an ion? A) lose 1 B) gain 1 C) lose 7 D) gain 2 E) lose 3

How many equivalents are present in 5.0 g of Al3+? A) 15 Eq B) 0.56 Eq C) 0.19 Eq D) 0.37 Eq E) 3 Eq

How many grams of barium chloride are needed to make 100. grams of barium sulfate? A) 44.9 g B) 89.2 g C) 208.3 g D) 233.3 g E) 46.6 g

How many grams of glucose (C6H12O6 ) are in 3.55 moles of glucose? A) 180. g B) 639 g C) 103 g D) 426 g E) 50.7 g

How many moles of H2O are produced when 1 mole of Mg(OH)2 reacts with 1 mole of H2SO4? A) 1 B) 2 C) 3 D) 4 E) 5

How many moles of barium sulfate are produced from 0.100 mole of barium chloride? A) 0.0100 mole B) 0.100 mole C) 0.200 mole D) 1.00 mole E) 2.00 moles

How many moles of carbon atoms are there in 0.500 mole of C2H6 ? A) 0.500 moles B) 1.00 moles C) 3.00 moles D) 6.02 × 1023 moles E) 4.00 moles

How many moles of magnesium are needed to react with 0.50 mole of O2 ? A) 0.50 mole B) 1.0 moles C) 2.0 moles D) 3.0 moles E) 4.0 moles

How many moles of water, H2O, are present in 75.0 g of H2O? A) 4.41 moles B) 4.16 moles C) 75.0 moles D) 7.50 moles E) 1.35 × 103 moles

If 100. mL of water is added to 25 mL of 5.0 M NaCl, the final concentration is ________. A) 25 M B) 1.0 M C) 5.0 M D) 2.0 M E) 1.3 M

If a condition of hyperventilation occurs, the blood pH of the patient is expected to A) saturate. B) increase. C) decrease. D) stay the same. E) concentrate.

If the reaction shown below is exothermic, the energy level of the reactants is H2 + O2 → 2H2O A) lower than that of the products. B) higher than that of the products. C) the same as that of the products. D) possibly lower, possibly higher than that of the products. E) higher than the activation energy of the reaction.

In a buffer system of HF and its salt, NaF, A) the HF neutralizes added acid. B) the HF neutralizes added base. C) the HF is not necessary. D) the F- neutralizes added H2O. E) the F- neutralizes added base.

In a sulfuric acid solution, where the [ H3O+] is 0.01 M, what is the pH? A) pH = 12.0 B) pH = 2.0 C) pH = 3.0 D) pH = 11.0 E) pH = 5.0

In an atom, the nucleus contains A) an equal number of protons and electrons. B) all the protons and neutrons. C) all the protons and electrons. D) only neutrons. E) only protons.

In an electron-dot structure of an element, the dots are used to represent A) all of the electrons in the atom. B) the valence electrons. C) the electron arrangement. D) only the electrons that will participate in bond formation. E) the electrons that the element will gain when it forms a compound.

In an endothermic reaction A) heat flows out of the system. B) energy is absorbed by the system. C) the temperature of the system increases. D) the products have less energy that the reactants. E) the products have the same energy that the reactants.

In an exothermic reaction, heat can be considered a A) reactant. B) product. C) rate. D) catalyst. E) determinant.

In an oxidation-reduction reaction, the substance oxidized always A) takes on oxygen atoms. B) shows a loss of electrons. C) gives up hydrogen atoms. D) shows a gain of electrons. E) becomes a charged species.

In any balanced chemical equation, the number of each type of atom on both sides of the equation is A) doubled. B) the same. C) decreased by one. D) increased by one. E) dependent on the temperature.

In the following reaction, when the equation is correctly balanced, what is the correct coefficient for aluminum chloride? Al(s) + Cl2(g) → AlCl3(s) A) 1 B) 2 C) 3 D) 4 E) 5 Answer:

In the following reaction, when the equation is correctly balanced, what is the correct coefficient for sodium chloride? Pb(NO3)2(aq) + NaCl(aq) → PbCl2(s) + NaNO3(aq) A) 1 B) 2 C) 3 D) 4 E) 5

In the reaction of nitrogen gas with oxygen gas to produce nitrogen oxide, what is the effect of adding more oxygen gas to the initial reaction mixture? The reaction is shown below. N2(g) + O2(g) ⇌ 2NO(g) A) The equilibrium shifts to produce more N2. B) The equilibrium shifts to produce more NO. C) The equilibrium is not affected. D) Extra catalyst is required to reach equilibrium. E) The temperature of the reaction mixture is raised.

In this reaction, what is the correct coefficient for hydrogen gas? ? H2 + ? O2 → ? H2O A) 1 B) 2 C) 3 D) 4 E) 5

Ionic bonding is expected in which of these compounds? A) Cl2 B) KF C) OF2 D) HF E) H2

Ionization energy is A) the energy an ion acquires from an electron. B) the energy needed to remove the least tightly bound electron. C) highest for metals in Group 1A (1). D) higher for potassium than for lithium. E) None of the above.

What is the conversion factor for the relationship between millimeters and centimeters? A) 1 mm/1 cm B) 10 mm/1 cm C) 1 cm/1 mm D) 100 mm/1 cm E) 10 cm/1 mm

Iron metal reacts with oxygen gas to produce iron(III) oxide. What will be the effect of increasing the pressure of oxygen gas in a closed reaction vessel? A) Less reaction will take place. B) More iron oxide will be produced. C) The reaction mixture will catch fire. D) There is no effect; a catalyst is needed. E) The rate of production of iron oxide will slow down

Oil does not dissolve in water because A) oil is polar. B) oil is nonpolar. C) water is nonpolar. D) water is saturated. E) oil is hydrated.

The O-H bond in water is polar because A) it is an ionic bond. B) oxygen is much more electronegative than hydrogen. C) oxygen occupies more space than hydrogen. D) hydrogen is much more electronegative than oxygen. E) it is a hydrogen bond.

The ________ is the minimum energy needed for a chemical reaction to begin. A) reaction energy B) activation energy C) energy of reactants D) energy of products E) heat of reaction

The atomic size of atoms A) increases going across a period. B) decreases going across a period. C) decreases going down within a group. D) does not change going across a period. E) None of the above.

The bond in Cl2 is a(n) A) ionic bond. B) nonpolar covalent bond. C) metallic bond. D) polar ionic bond. E) no bond.

The carbon tetrachloride molecule, CCl4 , is A) a polar molecule with polar bonds. B) a nonpolar molecule with polar bonds. C) a nonpolar molecule with nonpolar bonds. D) a polar molecule with nonpolar bonds. E) a polar molecule with ionic bonds.

The conjugate base of HClO3 is A) HClO2. B) ClO3-. C) Cl(OH)2. D) ClO3. E) HClO.

The correct answer for the addition of 7.5 g + 2.26 g + 1.311 g + 2 g is A) 13.071 g. B) 13 g. C) 13.0 g. D) 10 g. E) 13.1 g.

The dietary calorie (Cal) is equal to A) 1000 kilocalories. B) 1000 calories. C) 100 calories. D) 10 calories. E) 1 calorie.

The elements sodium, magnesium, and silicon A) are isotopes of each other. B) are in the same period of elements. C) have the same number of neutrons. D) are in the same group. E) have the same mass number.

The formula of copper(I) sulfide is A) CuS. B) Cu2S. C) Cu2(SO4)3 .D) CuSO4. E) CuS2.

The function of a buffer is to A) change color at the end point of a titration. B) maintain the pH of a solution. C) be a strong base. D) maintain a neutral pH. E) act as a strong acid.

The ionization energy of atoms A) decreases going across a period. B) decreases going down within a group. C) increases going down within a group. D) does not change going down within a group. E) None of the above.

The mass number of an atom can be calculated from A) the number of electrons. B) the number of protons plus neutrons. C) the number of protons. D) the number of electrons plus protons. E) the number of neutrons.

The name given to an aqueous solution of HBr is A) hydrogen bromide. B) hydrobromic acid. C) bromic acid. D) bromous acid. E) hypobromous acid.

The name of the Cu+ ion is A) copper(II). B) copper(I). C) cobalt. D) copper. E) cuprum.

The name of the HSO4- ion is A) sulfate. B) hydrogen sulfate. C) sulfite. D) hydrogen sulfite. E) sulfide.

The number of electrons in the outer energy level of a neutral atom of boron (atomic number 5) is A) 2. B) 3. C) 5. D) 8. E) 10.

The process by which a semipermeable membrane allows water molecules, small molecules, and ions to pass through while retaining large particles is called A) osmotic pressure. B) dialysis. C) solvation. D) dilution. E) hydration.

The ratio of the mass of a substance to its volume is its A) specific gravity. B) density. C) buoyancy. D) weight. E) conversion factor.

The specific heat of a substance is the amount of heat needed to A) change 1 g of the substance from the solid to the liquid state. B) raise the temperature of 1 g of the substance by 1 °C. C) change 1 g of the substance from the liquid to the solid state. D) convert 1 g of a liquid to gas. E) convert 1 g of a solid to a gas.

The stronger the acid, the ________ the conjugate base. A) stronger B) weaker

The strongest interactions between molecules of ammonia ( NH3) are A) ionic bonds. B) hydrogen bonds. C) polar covalent. D) dipole-dipole. E) dispersion forces.

The water molecule has a dipole with the negative portion A) localized between the hydrogen atoms. B) pointing toward the oxygen atom. C) localized on one of the hydrogens. D) pointing from the oxygen through the hydrogen atoms. E) surrounding the molecule.

Treatment of carbon monoxide poisoning can be accomplished by the use of pure oxygen for breathing. This is an example of the use of ________ in a clinical setting. A) the ideal gas law B) Le Châtelier's principle C) Henry's law D) conservation of mass E) a precipitation reaction

What elements are in hydroxyapatite, Ca5 (PO4)3OH, a major compound in human bones and teeth? A) carbon, potassium, oxygen, hydrogen B) calcium, phosphorus, oxygen, hydrogen C) carbon, phosphorus, oxygen, helium D) calcium, phosphorus, oxygen, helium E) carbon, potassium, oxygen, helium

What is the abbreviated electron configuration for nickel (atomic number 28)? A) [He]2s 22p 3 B) [Ar]4s 23d 8 C) [Kr]4s 23d 8 D) [Ar]4s 24p 4 E) [Ar]3d 8

What is the classification for this reaction? SO3(g) + H2O (l) → H2SO4(l) A) decomposition B) combination C) replacement D) double replacement E) oxidation reduction

What is the concentration, in m/v percent, of a solution prepared from 50. g NaCl and 2.5 L of water? A) 5.0% B) 2.0% C) 0.020% D) 0.050% E) 20.%

What is the correct form for the equilibrium constant expression for this reaction? H2(g) + F2(g) ⇌ 2HF(g)

Which of the following is the weakest acid? A) HF (Ka for HF is 7.2 × 10-4) B) HCN (Ka for HCN is 4.9 × 10-10) C) HCNO (Ka for HCNO is 2 × 10-4) D) H3BO3 (Ka for H3BO3 is 5.4 × 10-10)

Which one of the following compounds will NOT be soluble in water? A) NaOH B) PbS C) K2SO4 D) LiNO3 E) MgCl2

Which one of the following properties describes a liquid? A) has its own shape B) particles are close together and move randomly C) particles move very rapidly D) fills the entire volume of the container E) There is essentially no interaction between the particles.

Which one of the following substances will float in gasoline, which has a density of 0.66 g/mL? A) table salt (density = 2.16 g/mL) B) balsa wood (density = 0.16 g/mL) C) sugar (density = 1.59 g/mL) D) aluminum (density = 2.70 g/mL) E) mercury (density = 13.6 g/mL)

measurement 0.000 0043 m, expressed correctly using scientific notation, is A) 4.3 × 10-7 m. B) 4.3 × 10-6 m. C) 4.3 × 106 m. D) 0.43 × 10-5 m. E) 4.3 m

If the temperature is - 55 °C, what is the corresponding temperature on the Kelvin scale? A) 225 K B) 218 K C) 55 K D) 273 K E) 328 K

B) -55c+273k

What is the mass of 2.00 L of an intravenous glucose solution with a density of 1.15 g/mL? A) 0.023 kg B) 2.30 kg C) 1.15 kg D) 0.015 kg E) 0.58 kg

B) To find: Conver 2.00L to ml ---> 2.00 x 1000= 2000 ml Next, multiply 1.15 kg by 2000 ml and divide by 1000 ml to get 2.30 kg

If the temperature is 20 °C, what is the corresponding temperature on the Fahrenheit scale? A) -22 °F B) 68 °F C) 43 °F D) 239 °F E) 94 °F

B) To find: 20 C x 5/9 + 32

A driver is traveling at 60 km/h. Is the driver speeding if the speed limit is 45 mph? A) Yes B) No

B) To find: 60 x 0.609 / 1 hr =36.54 mph

What is the coefficient for carbon dioxide in the balanced equation? A) 2 B) 4 C) 5 D) 6 E) 8

) The [ H3O+] of a solution with pH = 5.60 is A) 3 × 10-6 M. B) 2.5 × 10-8 M. C) 2.5 × 10-6 M. D) 4.0 × 10-6 M. E) 4.0 × 10-9 M.

2Mg + O 2 → 2MgO2 ) The number of moles of MgO produced when 0.20 mole of O2 reacts completely is A) 0.10 mole. B) 0.20 mole. C) 0.40 mole. D) 0.60 mole. E) 0.80 mole.

A 25.0 mL sample of H2SO4 requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid? H2SO4 + 2KOH → K2SO4 + 2H2O A) 2.00 M B) 2.50 M C) 0.800 M D) 1.60 M E) 1.25 M

A 50.0 mL urine sample has a mass of 50.7 g. The specific gravity of the urine is A) 1.014 g/mL. B) 0.986 g/L. C) 1.01. D) 0.986. E) 50.7.

A catalyst is A) a reactant in a chemical reaction. B) a product in a chemical reaction. C) a substance that speeds up a reaction without being consumed in the reaction. D) a substance that increases the energy of the products. E) a substance that decreases the energy of the products.

A group of covalently bonded atoms that has an overall electrical charge is called a(n) A) ionic compound. B) anion. C) polyatomic ion. D) cation. E) molecule.

A mixture in which one component settles is called a(n) ________. A) solution B) colloid C) suspension D) electrolyte E) nonelectrolyte

A value of 25 °C is a measurement of A) distance. B) volume. C) temperature. D) mass. E) density.

A(n) ________ is the smallest neutral unit of two or more atoms held together by a covalent bond. A) ionic compound B) nucleus C) molecule D) formula E) unit

Acetic acid can be classified as a(n) ________. A) gas B) solid C) weak electrolyte D) strong electrolyte E) ionic compound

An equivalent is A) the amount of ion that has a 1+ charge. B) the amount of ion that has a 1- charge. C) the amount of ion that carries 1 mole of electrical charge. D) 1 mole of any ion. E) 1 mole of an ionic compound.

An increase in the temperature of a solution usually A) increases the boiling point. B) increases the solubility of a gas in the solution. C) increases the solubility of a solid solute in the solution. D) decreases the solubility of a solid solute in the solution. E) decreases the solubility of a liquid solute in the solution.

Elements in group 2A(2) of the periodic table form ions with a charge of A) 1+. B) 1-. C) 2+. D) 3+. E) 0.

Fe2(SO4)3 is called A) iron sulfate. B) iron(II) sulfate. C) iron(III) sulfate. D) diiron trisulfate. E) iron trisulfate.

Find the mass of AlCl3 that is produced when 10.0 grams of Al2O3 react with 10.0 g of HCl according to the following equation. Al2O3(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2O(aq) A) 16.2 g B) 20.0 g C) 12.2 g D) 10.0 g E) 6.10 g

Find the mass of AlCl3 that is produced when 25.0 grams of Al2O3 react with excess HCl according to the following equation. Al2O3(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2O(l) A) 155 g B) 72.9 g C) 65.4 g D) 32.6 g E) 16.3 g

For the following reaction, the equilibrium concentration of NO2 is 0.38 M and equilibrium concentration of N2O4 is 1.0M. What is the value of the equilibrium constant? 2NO2(g) ⇌ N2O4(g) A) 0.14 B) 2.6 C) 6.9 D) 0.38 E) 1.0

For the reaction: 2H2O(l) + 137 kcal → 2H2 (g) + O2 (g), how many kcal are needed to form 2.00 moles O2 (g)? A) 68.5 kcal B) 137 kcal C) 274 kcal D) 190. kcal E) 548 kcal

Gold in a wedding ring is a(n) A) compound. B) heterogeneous mixture. C) element. D) homogeneous mixture. E) None of the above.

Helium is a(n) A) compound. B) heterogeneous mixture. C) element. D) homogeneous mixture. E) electron.

How many atoms of neon are present in 1.30 moles of neon? A) 3.15 × 1023 atoms B) 4.63 × 1023 atoms C) 7.83 × 1023 atoms D) 6.02 × 1023 atoms E) 7.83 × 1024 atoms

How many calories are required to increase the temperature of 13 g of alcohol from 11 °C to 23 °C? The specific heat of alcohol is 0.588 cal/g °C. A) 83 cal B) 0.63 cal C) 92 cal D) 0.54 cal E) 170 cal

How many grams of PbCl2 are formed when 25.0 mL of 0.654 M KCl react with Pb(NO3)2? 2KCl(aq) + Pb(NO3) 2(aq) → 2KNO3(aq) + PbCl2(s) A) 22.7 g B) 1.64 g C) 2.27 g D) 4.54 g E) 9.08 g

How many grams of barium sulfate can be produced from 20.8 g of barium chloride? A) 1.37 g B) 2.33 g C) 23.3 g D) 137 g E) 233 g

How many grams of glucose are needed to prepare 400. mL of a 2.0%(m/v) glucose solution? A) 800. g B) 0.0050 g C) 8.0 g D) 2.0 g E) 200. g

How many grams of hydrogen are needed to produce 1.80 g of water according to this equation? 2H2 + O2 → 2H2O A) 0.100 g B) 0.180 g C) 0.200 g D) 2.00 g E) 4.00 g

How many kcal are produced when 32.0 g of CH4 react? CH4 + 2O2 → CO2 + 2H2O + 218 kcal A) 218 kcal B) 109 kcal C) 436 kcal D) 6.81 kcal

How many lone pairs of electrons are in the electron-dot structure of H2O? A) 0 B) 1 C) 2 D) 3 E) 4

In the reaction of silver nitrate with sodium chloride, how many grams of silver chloride will be produced from 100. g of silver nitrate when it is mixed with an excess of sodium chloride? The equation for the reaction is below. AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) A) 107.9 g B) 169.9 g C) 84.4 g D) 0.589 g E) 58.9 g

In which of the following are the pH values arranged from the most basic to the most acidic? A) 1, 3, 6, 8, 11, 14 B) 2, 5, 7, 9, 10, 11 C) 14, 10, 7, 4, 3, 1 D) 14, 10, 7, 1, 3, 5 E) 7, 10, 14, 4, 3, 1

In which of the following would the particles move most rapidly? A) ice at -20 °C B) water at 20 °C C) steam at 110 °C D) boiling water E) ice at 0 °C

Of the elements: B, C, F, Li, and Na, the element with the smallest atomic radius is A) B. B) C. C) F. D) Li. E) Na.

Of the elements: B, C, F, Li, and Na. The element with the highest ionization energy is A) B. B) C. C) F. D) Li. E) Na.

Of the elements: B, C, F, Li, and Na. The element with the least metallic character is A) B. B) C. C) F. D) Li. E) Na.

On a hot day, the thermometer read 95 °F. What is the temperature in degrees Celsius? A) 77 °C B) 113 °C C) 35 °C D) 63 °C E) 178 °C

Refrigerating perishable foods affects biochemical reactions by A) increasing concentrations of antioxidants. B) removing bacteria. C) decreasing the rate of reactions affecting spoilage. D) catalyzing the removal of harmful chemicals from the foods. E) improving the appearance of the foods

Semiconductors are located in the periodic table on (or in) the A) left side of the table. B) right side of the table. C) line dividing metals from nonmetals in the table. D) first period of the table. E) last period of the table.

The Ka for hydrofluoric acid is 7.2 × 10-4. This means that HF is A) neutral in water solution. B) able to react with HCl. C) a weak acid. D) a strong acid. E) ionic.

The [OH-] of a solution with pH = 8.34 is A) 5 × 10-9 M. B) 4.6 × 10-9 M. C) 2.2 × 10-9 M. D) 3 × 10-6 M. E) 2.2 × 10-6 M.

The activation energy of a chemical reaction is the energy that A) must be removed from the mixture. B) must be released from the mixture. C) initiates the reaction. D) activates the catalyst. E) is the difference in the energies of the starting materials and products.

The conjugate acid of HSO4- is A) SO42-. B) HSO4. C) H2SO4.. D) H2SO4-. E) HSO3-.

The cubic centimeter (cm3 or cc) has the same volume as a A) cubic inch. B) cubic liter. C) milliliter. D) centimeter. E) cubic decimeter.

The density of a solution is 0.847 g/mL. Its specific gravity is A) 11.8. B) 0.118. C) 0.847. D) 1.18. E) 1.2.

The electron arrangement of any particular atom shows A) the number of isotopes possible. B) a description of the shape of each energy level. C) the number of electrons in each energy level. D) a diagram of an atomic nucleus. E) the maximum number of electrons each energy level can hold.

The energy stored in the chemical bonds of a carbohydrate molecule is A) specific heat. B) kinetic energy. C) potential energy. D) work. E) a calorie.

The formula for a molecule formed from N and Cl would be A) NCl. B) NCl2 C) NCl3 D) N3Cl. E) NCl5

The ion of aluminum is A) Al+. B) Al2+. C) Al3+. D) Al3- E) Al2-

The metric unit for volume is the A) meter. B) quart. C) liter. D) pint. E) centimeter.

The molar mass of calcium hydroxide, Ca(OH)2 , is A) 58.1 g. B) 57.1 g. C) 74.1 g. D) 114.2 g. E) 38.0 g.

The molarity of a solution of 5.0 g of KCl in 100. mL of solution is ________. A) 0.038 M B) 0.067 M C) 0.67 M D) 0.13 M E) 1.3 M

The name given to an aqueous solution of HClO3 is A) chlorous acid. B) hypochlorous acid. C) chloric acid. D) hydrochloric acid. E) hypochloric acid.

The name of Al(OH)3 is A) aluminum trihydroxide. B) monoaluminum trihydroxide. C) aluminum hydroxide. D) aluminum(III) hydroxide. E) aluminum oxygen hydride.

The name of PbO2 is A) lead dioxide. B) lead(II) oxide. C) lead(IV) oxide. D) plumbum oxide. E) lead oxygen.

The number of electron levels in a magnesium atom is A) 1. B) 2. C) 3. D) 4. E) 5.

The number of valence electrons found in an atom of a Group A element is equal to A) its atomic number. B) its mass number. C) its group number. D) eight. E) eight minus the group number.

The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons.

The reaction of carbon with oxygen to produce carbon monoxide is an example of which class of reaction? 2C(s) + O2(g) → 2CO(g) A) single replacement B) double replacement C) combination D) catalytic E) endothermic

The shape of the ammonia molecule ( NH3) is A) linear. B) square. C) pyramidal. D) hexagonal. E) octagonal.

Use the reaction: 2AgNO3(aq) + H2SO4(aq) → Ag2SO4(s) + 2H2O(l). What volume of 0.123 M AgNO3(aq) is needed to form 0.657 g of Ag2SO4(s)? A) 34.2 L B) 17.1 mL C) 34.3 mL D) 10.7 mL E) 53.4 mL

Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute? A) mineral oil, soluble in water B) CaCl2, soluble in hexane C) NaHCO3, soluble in water D) CCl4, soluble in water E) octane, soluble in water

What is the [OH-] in a solution that has a [ H3O+] = 1 × 10-6 M? A) 1 × 10-2 M B) 1 × 10-6 M C) 1 × 10-8 M D) 1 × 10-10 M E) 1 × 10-12 M

Which of the answers for the following conversions contains the correct number of significant figures? A) 2.543 m × = 100.1942 in B) 2 L × = 2.12 qt C) 24.95 min × = 0.4158 hr D) 12.0 ft × × = 370 cm E) 24.0 kg × = 11 lb

Which of the following compounds contains an ionic bond? A) NH3 B) H2O C) CaO D) H2 E) CH4

Which of the following gives the correct numbers of protons, neutrons, and electrons in a neutral atom of 118Sn50? A) 118 protons, 50 neutrons, 118 electrons B) 118 protons, 118 neutrons, 50 electrons C) 50 protons, 68 neutrons, 50 electrons D) 68 protons, 68 neutrons, 50 electrons E) 50 protons, 50 neutrons, 50 electrons

Which of the following is a buffer system? A) NaCl and NaNO3 B) HCl and NaOH C) H2CO3 and KHCO3 D) NaCl and NaOH E) H2O and HCl

Which of the following is a characteristic of the modern periodic table? A) A group is a horizontal row on the periodic table. B) A period is a column on the periodic table. C) The elements in each group have similar chemical properties. D) The B groups contain the representative elements. E) The A groups contain the transition elements.

Which of the following is a measurement of mass in the metric system? A) milliliter B) centimeter C) kilogram D) Celsius E) meter

Which of the following is a measurement of temperature in the metric system? A) oz B) lb C) Celsius D) kilogram E) meter

Which of the following is an oxidation-reduction reaction? A) CaCl2+ Na2SO4 → CaSO4+ 2NaCl B) KOH + HNO3 → H2O + KNO3 C) N2 + O2 → 2NO D) AgNO3+ NaCl → AgCl + NaNO3 E) Al2(SO4)3 + 6KOH → 2Al(OH)3+ 3K2SO4

Which of the following is the correct electron-dot structure for carbon? A) B) C) D) E)

Which of the following is the strongest base? A) H3PO4 B) NH3 C) NaOH D) NaCl E) HCl

Which of the following measured numbers contains the designated CORRECT number of significant figures? A) 0.04300 5 significant figures B) 0.00302 2 significant figures C) 156 000 3 significant figures D) 1.04 2 significant figures E) 3.0650 4 significant figures

Which of the following measurements has three significant figures? A) 0.005 m B) 510 m C) 0.510 m D) 0.051 m E) 5100 m

Which of the following molecules can form hydrogen bonds? A) CH4 B) NaH C) NH3 D) BH3 E) HI

Which of the following setups would convert centimeters to feet? A) B) C) D) E)

Which one of the following compounds contains an ion with a 3+ charge? A) KCl B) Na2O C) FeCl3 D) CuCl E) MgCl2

Which one of the following compounds will NOT be soluble in water? A) LiOH B) K2S C) BaSO4 D) NaNO3 E) MgCl2

Which one of the following compounds will be soluble in water? A) AgBr B) Cu(OH)2 C) NH4Cl D) CaCO3 E) PbS

Which one of the following compounds will be soluble in water? A) AgCl B) Cu(OH)2 C) LiCl D) CaSO4 E) PbCO3

Which one of the following is characteristic of a base? A) produces H3O+ in water B) has a sour taste C) has a slippery, soapy feel D) turns blue litmus red E) is insoluble in water

Which solution has the highest pH? A) a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate B) a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate C) a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate D) a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate E) All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.

A doctor's order is 0.125 g of ampicillin. The liquid suspension on hand contains 250 mg/5.0 mL. How many milliliters of the suspension are required? A) 0.0025 mL B) 3.0 mL C) 2.5 mL D) 6.3 mL E) 0.0063 mL

C) Dosage cal: To find, First, convert 0.125 g to mg--> 0.125 g x 1000= 125 Next, divide 125/250 x 5mL to get 2.5 mL

How many liters of soft drink are there in 5.25 qt? A) 4950 L B) 55.7 L C) 4.95 L D) 5.57 L E) 5.0 L

C) To find: 5.25 qt x 0.946 L= 4.95 L

How many centimeters are there in 57.0 in.? A) 22 cm B) 0.0445 cm C) 145 cm D) 22.4 cm E) 140 cm

C) To find: multiply 57.0 in by 2.54 cm , to get 144.78, round to 2 sig figs, to get 145 cm

Exceptions to these rules are the following:

CN−cyanide OH−hydroxide

Halogens form 4 polyatomic ions with oxygen. Each has a −1 charge

ClO4−perchlorate ClO3−chlorate ClO2−chlorite ClO−hypochlorite

What is the mass number of an atom of potassium that has 20 neutrons? A) 15 B) 19 C) 35 D) 39 E) 59

A Roman numeral equal to the ion charge is placed in parentheses immediately after the metal name

Cu2+copper(II) Pb2+lead(II) Cu+copper(I) Pb4+lead(IV) Fe2+iron(II) Cr2+chromium(II) Fe3+iron(III) Cr3+chromium(III)

What is the molar mass of copper(II) sulfate, CuSO4 ? A) 16.0 g B) 63.6 g C) 111.6 g D) 159.6 g E) 319.2 g

The elements lithium, sodium, and potassium A) are isotopes of each other. B) are in the same period of elements. C) have the same number of neutrons. D) are in the same group. E) have the same mass number.

For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. If the concentration of both products is 0.10 M at equilibrium, what is the concentration of the starting material, NOBr? 2NOBr(g) ⇌ 2NO(g) + Br2(g) A) 5 × 10-4 M B) 2.2 × 10-4 M C) 5 × 10-2 M D) 2.2 × 10-2 M E) 2.2 M

For the reaction: 2H2O(l) + 137 kcal → 2H2 (g) + O2 (g), how many kcal are needed to react 50.0 g H2O(l)? A) 380. kcal B) 137 kcal C) 274 kcal D) 190. kcal E) 760. kcal

(Q) What coefficient is placed in front of O2 to complete the balancing of the following equation? C5H8+ ? O2 → 5CO2 + 4H2O A) 1 B) 3 C) 5 D) 7 E) 9

0.100 mole of lithium has a mass of A) 3.00 g. B) 0.300 g. C) 6.94 g. D) 0.694 g. E) 0.700 g.

25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl solution is A) 0.212 M. B) 0.115 M. C) 0.500 M. D) 0.390 M. E) 0.137 M.

2Mg + O2 → 2MgO How many grams of MgO are produced when 40.0 grams of O2 react completely with Mg? A) 30.4 g B) 50.4 g C) 60.8 g D) 101 g E) 201 g

3.25 kcal is the same amount of energy as A) 3.25 J. B) 0.777 J. C) 777 J. D) 13600 J. E) 13.6 J.

9.31 g is the same mass as A) 931 μg. B) 931 kg. C) 93.1 cg. D) 9310 mg. E) 0.0931 dg.

A 25.0 mL sample of H3PO4 requires 50.0 mL of 1.50 M NaOH for complete neutralization. What is the molarity of the acid? H3PO4 + 3NaOH →Na3PO4 + 3H2O A) 0.333 M B) 3.00 M C) 1.50 M D) 1.00 M E) 0.750 M

A chemical equation is balanced when A) the total number of molecules is the same in reactants and products. B) the total number of ions is the same in reactants and products. C) the sum of the coefficients of the reactants is equal to the sum of the coefficients of the products. D) the number of atoms of each element is the same in reactants and products. E) the charge on each atom is the same in reactants and products.

A conversion factor set up correctly to convert 15 inches to centimeters is A) 100 cm/1 m. B) 1 inch/2.54 cm. C) 1 cm/10 mm. D) 2.54 cm/1 inch. E) 10 cm/1 inch.

A kilocalorie of heat is required to raise the temperature of A) 1 g of water from 14 °C to 15 °C. B) 1 g of water by 10 °C. C) 10 g of water by 10 °C. D) 100 g of water by 10 °C. E) 100 g of water by 100 °C.

A researcher added three samples of sodium chloride solution; the volumes were: 0.351 mL, 0.350 mL and 0.349 mL. The total volume should be reported as A) 1.05 mL. B) 1.0 mL. C) 11 mL. D) 1.050 mL. E) 1.0500 mL.

A sample of chlorine has two naturally occurring isotopes. The isotope Cl-35 (mass 35.0 amu) makes up 75.8% of the sample, and the isotope Cl-37 (mass = 37.0 amu) makes up 24.3% of the sample. What is the average atomic mass for chlorine? A) 36.0 amu B) 35 amu C) 36.6 amu D) 35.5 amu E) 35.521 amu

A solution that has an osmotic pressure less than that of red blood cells is called A) saturated. B) hypertonic. C) isotonic. D) hypotonic. E) unsaturated.

A value of 36 mL is a measure of A) density. B) mass. C) temperature. D) volume. E) distance.

Absolute zero is A) the freezing point of water using the Celsius scale. B) the boiling point of liquid nitrogen. C) the temperature on the Kelvin scale corresponding to 32 °F. D) the coldest temperature possible. E) the freezing point of liquid nitrogen.

According to the Brønsted-Lowry definition, A) an acid is a proton acceptor. B) a base produces H+ ions in aqueous solutions. C) a base is a proton donor. D) a base is a proton acceptor. E) an acid acts as the solvent.

Air is a(n) A) compound. B) heterogeneous mixture. C) element. D) homogeneous mixture. E) None of the above.

Ammonium hydroxide is a weak base because A) it is a dilute solution. B) it is only slightly soluble in water. C) it cannot hold on to its hydroxide ions. D) it dissociates only slightly in water. E) it is completely ionized in aqueous solution.

An acid and base react to form a salt and water in a(n) ________ reaction. A) ionization B) dissociation C) oxidation D) neutralization E) reduction

An equilibrium in which all the components are gases is a ________ equilibrium. A) heterogeneous B) liquid C) catalytic D) homogeneous E) reversible

Consider a neutral atom with 30 protons and 34 neutrons. The mass number for this atom is A) 30. B) 32. C) 34. D) 64. E) 94.

How many calories are required to raise the temperature of a 150. g sample of gold from 25 °C to 175 °C? The specific heat of gold is 0.0308 cal/g °C. A) 4.62 cal B) 116 cal C) 22500 cal D) 693 cal E) 130 cal

How many electrons will aluminum gain or lose when it forms an ion? A) lose 1 B) gain 5 C) lose 2 D) lose 3 E) gain 1

How many equivalents are present in 0.40 moles of SO4 2-? A) 0.10 Eq B) 0.20 Eq C) 0.40 Eq D) 0.80 Eq E) 1.2 Eq

How many grams of CO2 are produced from 125 g of O2 and excess CH4? CH4 + 2O2 → CO2 + 2H2O A) 125 g of CO2 B) 62.5 g of CO2 C) 172 g of CO2 D) 85.9 g of CO2 E) 250. g of CO2

How many grams of H2O are needed to produce 150 g of Mg(OH)2? A) 46 g B) 18 g C) 130 g D) 93 g E) 23 g

How many grams of N2 are produced from 100. g of NH3 in the following reaction? 4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(l) A) 165 g B) 132 g C) 125 g D) 206 g E) 7.35 g

How many grams of water will 100. grams of hydrogen peroxide (H2O2) produce? A) 3600 g B) 360. g C) 5.88 g D) 52.9 g E) 106 g

How many molecules of water, H2O, are present in 75.0 g of H2O? A) 75.0 molecules B) 4.17 molecules C) 7.53 × 1024 molecules D) 2.51 × 1024 molecules E) 5.02 × 1024 molecules

How many moles of CaCl2 are in 250 mL of a 3.0 M of CaCl2 solution? A) 750 moles B) 1.3 moles C) 83 moles D) 0.75 mole E) 3.0 moles

How many moles of K2 SO4 are in 15.0 g of K2 SO4 ? A) 0.172 moles B) 2.61 × 103 moles C) 0.111 moles D) 0.0861 moles E) 0.119 moles

How many valence electrons are in the electron-dot structure of H2O? A) 2 B) 4 C) 6 D) 8 E) 10

Hydrogen sulfide, H2 S, has a shape similar to A) carbon dioxide. B) carbon monoxide. C) hydrogen chloride. D) water. E) carbon tetrachloride.

In a molecule with covalent bonding A) oppositely charged ions are held together by strong electrical attractions. B) atoms of metals form bonds to atoms of nonmetals. C) atoms of different metals form bonds. D) atoms are held together by sharing electrons. E) atoms of noble gases are held together by attractions between oppositely charged ions.

In an oxidation-reduction reaction, the substance reduced always A) takes on oxygen atoms. B) shows a loss of electrons. C) gives up hydrogen atoms. D) shows a gain of electrons. E) becomes a charged species.

In the following gas phase reaction, what is the effect on the direction of the reaction if more SO3 is added to the reaction mixture? 2SO2(g) + O2(g) ⇌ 2SO3(g) A) The equilibrium shifts to produce more products. B) The position of the equilibrium remains unchanged. C) The rate of formation of products is increased. D) The equilibrium shifts to produce more reactants. E) The catalyst for the reaction is used up.

In the process known as osmosis, ________ moves through a semipermeable membrane into an area of ________ concentration. A) solute; lower solute B) solute; higher solute C) solvent; lower solute D) solvent; lower solvent E) solvent; higher solvent

In this reaction, what is the substance oxidized? Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g) A) chlorine B) zinc chloride C) hydrogen D) zinc E) oxygen

Isotopes are atoms of the same element that have A) different atomic numbers. B) the same atomic numbers but different numbers of protons. C) the same atomic numbers but different numbers of electrons. D) the same atomic number but different numbers of neutrons. E) the same atomic mass but different numbers of protons.

Mg3N2 (s) + 6H2O(l) → 3Mg (OH)2 (s) + 2NH3 (g) When 36.0 g of H2O react, how many grams of NH3 are produced? A) 34.0 g B) 10.0 g C) 5.67 g D) 11.3 g E) 102 g

N2(g) + O2(g) ⇌ 2NO(g) For the reaction at equilibrium, if the volume of the container is decreased, the amount of NO present will A) decrease. B) increase. C) double. D) stay the same. E) triple.

NaCl can be classified as a ________. A) gas B) liquid C) weak electrolyte D) strong electrolyte E) nonelectrolyte

One cup of kidney beans contains 15 g of protein, 1.0 g of fat, and 42 g of carbohydrate. How many kilocalories, to two significant figures, does this sample contain? A) 60 kcal B) 88 kcal C) 230 kcal D) 240 kcal E) 520 kcal

One metal that is used as a catalyst in a catalytic converter in an automobile is A) carbon. B) iron. C) copper. D) platinum. E) plutonium

One mole of helium gas has a mass of A) 1.00 g. B) 2.00 g. C) 3.00 g. D) 4.00 g. E) 8.00 g.

One mole of neon atoms has a mass of A) 6.02 × 1023 grams. B) 14.0 g. C) 10.0 g. D) 20.2 g. E) 30.2 g.

One mole of particles of any substance contains how many particles? A) 106 B) 3 × 10-10 C) 3 × 1010 D) 6.02 × 1023 E) 6.02 × 10-23

Significant figures are important because they indicate A) the accuracy of a measurement. B) the number of digits on a calculator. C) the number of measurements. D) the precision of a measurement. E) the accuracy of the conversion factor.

The [ H3O+] of a solution with pH = 2 is A) 10 M. B) -10 M. C) 1 × 102 M. D) 1 × 10-2 M. E) 1 × 10-12 M.

The atomic mass of an element is equal to A) its mass number. B) its atomic number. C) one-twelfth of the mass of a carbon-12 atom. D) a weighted average mass of all of the naturally occurring isotopes of the element. E) the average mass of all of the naturally occurring isotopes of the element.

The compound MgCl2 is named A) magnesium chlorine. B) magnesium dichloride. C) magnesium(II) chloride. D) magnesium chloride. E) dimagnesium chloride.

The element in this list with chemical properties similar to magnesium is A) sodium. B) boron. C) carbon. D) strontium. E) chlorine.

The equilibrium for the reaction for the decomposition of PCl5 to chlorine and PCl3 is 0.042. PCl5(g) ⇌ PCl3(g)+ Cl2(g) If the equilibrium concentrations are [PCl3] = 0.010 M, [Cl2] = 0.10 M, what is the value of [PCl5]? A) 0.010 M B) 0.0020 M C) 0.042 M D) 0.024 M E) 0.0010 M

The following reaction takes place when an electric current is passed through water. It is an example of a ________ reaction. 2H2O → 2H2 + O2 A) combination B) single replacement C) dehydration D) decomposition E) double replacement

The mass percent concentration refers to A) grams of solute in 1 kg of solvent. B) grams of solute in 1 kg of solution. C) grams of solute in 100 g of solvent. D) grams of solute in 100 g of solution. E) grams of solvent in 100 g of solution.

The mass/volume percent concentration refers to A) grams of solute in 1 L of solvent. B) grams of solute in 1 L of solution. C) grams of solute in 100 mL of solvent. D) grams of solute in 100 mL of solution. E) grams of solvent in 100 mL of solution.

The maximum number of electrons that may occupy the third energy level is A) 2. B) 8. C) 10. D) 18. E) 32.

The molar mass of potassium is A) 19 g. B) 31.0 g. C) 6.02 × 1023 grams. D) 39.1 g. E) 15g.

The neutralization reaction between Al(OH)3 and HNO3 produces the salt with the formula A) H2O. B) AlNO3. C) AlH2. D) Al(NO3)3. E) NO3OH.

The normal blood pH is about A) 6.8. B) 7.0. C) 7.2. D) 7.4. E) 7.6.

The number of dots in the electron dot structure of carbon is A) one. B) two. C) three. D) four. E) five.

The number of electrons in an ion with 20 protons and an ionic charge of 2+ is A) 24. B) 22. C) 20. D) 18. E) 16.

The number of neutrons in an atom is equal to A) the atomic number. B) the mass number. C) the mass number + the atomic number. D) the mass number - the atomic number. E) the number of protons.

The number of significant figures in the measurement of 45.030 mm is A) none. B) three. C) four. D) five. E) six.

The octet rule indicates that A) all of the noble gases have eight total electrons. B) all of the shells in an atom hold a maximum of 8 electrons. C) all of the Group A elements have 8 valence electrons. D) atoms lose, gain, or share valence electrons to have 8 valence electrons. E) the noble gases react with other compounds to get 8 valence electrons.

The physical state(s) present when a substance is melting is (are) A) solid. B) liquid. C) gas. D) solid + liquid. E) liquid + gas.

The physiological equilibrium system that keeps the temperature of the body constant is called A) stimulation. B) regulation. C) metabolism. D) homeostasis. E) catalysis.

The reaction of methane with oxygen to produce carbon dioxide and water is an example of which class of reaction? CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) A) single replacement B) double replacement C) combination D) oxidation E) endothermic

The shape of the carbon tetrachloride molecule is A) linear. B) square. C) pyramidal. D) tetrahedral. E) octagonal.

The shape of the water molecule ( H2O) is A) linear. B) tetrahedral. C) pyramidal. D) bent. E) octagonal.

The smallest particle of an element that retains the characteristics of the element is a(n) A) electron. B) neutron. C) proton. D) atom. E) nucleus.

The solubility of KI is 50 g in 100 g of H2O at 20 °C. If 110 grams of KI are added to 200 grams of H2O A) all of the KI will dissolve. B) the solution will freeze. C) the solution will start boiling. D) a saturated solution will form. E) the solution will be unsaturated.

The specific gravity of a solution is 1.18. Its density is A) 11.8 g/mL. B) 0.118 g/mL. C) 0.847 g/mL. D) 1.18 g/mL. E) 1.2 g/mL.

The strongest interactions between molecules of hydrogen chloride are A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces.

The types of compounds that use prefixes in their names are A) ionic compounds. B) ionic compounds involving transition metals. C) polyatomic ions. D) covalent compounds. E) compounds that contain polyatomic ions.

The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 × 10-9. What does this tell you about the concentrations of materials in the equilibrium mixture? A) The concentration of products exceeds the concentration of reactants. B) The concentrations of reactants and products are equal. C) The reactants are solids. D) The concentration of reactants exceeds the concentration of products. E) The products are solids.

To form an ion, a sodium atom A) gains one electron. B) gains two electrons. C) loses seven electrons. D) loses one electron. E) loses two electrons.

What is the answer, with the correct number of decimal places, for this problem? 4.392 g + 102.40 g + 2.51 g = A) 109.302 g B) 109 g C) 109.3 g D) 109.30 g E) 110 g

What is the classification for this unbalanced reaction? Fe + HCl → FeCl3+ H2 A) dehydration B) combination C) decomposition D) single replacement E) double replacement

What is the coefficient for water in the balanced equation? A) 2 B) 4 C) 5 D) 6 E) 8

What is the concentration, in mass percent, of a solution prepared from 50.0 g NaCl and 150.0 g of water? A) 0.250% B) 33.3% C) 40.0% D) 25.0% E) 3.00%

What is the correct electron configuration for the lithium atom? A) 1s 3 B) 2s 1 C) 1s 12s 2 D) 1s 2 2s 1 E) 1s 22s 5

What is the electron configuration for potassium (atomic number 19)? A) 1s 22s 22p 63s 23p 7 B) 1s 22s 22p 6 3s 23p 53d 2 C) 1s 22s 22p 83s 23p 5 D) 1s 22s 22p 63s 23p 64s 1 E) 1s 22s 22p 63s 23p 54s 1

Which of the following is a physical property of both liquids and gases? A) has its own shape B) has a definite volume C) has strong interactions between its particles D) has randomly arranged particles E) has large spaces between molecules

Which of the following is the correctly balanced equation for the complete neutralization of H3PO4 with Ca(OH)2? A) H3PO4 + Ca(OH)2 → CaHPO4 + 2H2O B) 3H3PO4 + Ca(OH)2 → Ca3(PO4)2 + 5H2O C) H3PO4 + Ca(OH)2 → Ca3(PO4)2+ H2O D) 2H3PO4 + 3Ca(OH)2 → Ca3(PO4)2 + 6H2O E) 4H3PO4 + 6Ca(OH)2 → 2Ca3(PO4)2 + 12H2O

Which of the following polyatomic ions has a 3- ionic charge? A) hydroxide B) nitrate C) sulfate D) phosphate E) bicarbonate

Which of the following polyatomic ions has a positive charge? A) hydroxide B) sulfate C) hydrogen carbonate D) ammonium E) nitrate

Which of the following properties is NOT a characteristic of the Group 1A(1) elements (alkali metals)? A) They are shiny. B) They are good conductors of heat. C) They react vigorously with water. D) Most of them are liquids at room temperature. E) They are good conductors of electricity.

Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution? A) In acids, [OH-] is greater than [ H3O+]. B) In bases, [OH-] = [ H3O+]. C) In neutral solutions, [ H3O+] = [ H2O]. D) In bases, [OH-] is greater than [ H3O+]. E) In bases, [OH-] is less than [ H3O+].

Which of the following would NOT be a physical change? A) freezing water to make ice cubes B) tearing a piece of aluminum foil C) boiling water for soup D) burning gasoline in a lawnmower E) melting gold to make jewelry

Which one of the following compounds will be insoluble in water? A) AgNO3 B) CaCl2 C) NH4Cl D) CaCO3 E) Pb(C2H3O2)2

Which solution is isotonic to a red blood cell? A) water B) 0.5% NaCl C) 2% glucose D) 0.9% NaCl E) 10% glucose

) Mercury has a specific gravity of 13.6. How many milliliters of mercury have a mass of 0.35 kg? A) 0.0257 mL B) 0.026 mL C) 25.7 mL D) 26 mL E) 4760 mL

D) To find: 0.35 kg/ 13.6=0.0257 , round to two sig figs to get 26

What is 6.5 m converted to inches? A) 1700 in B) 1651 in C) 39 in D) 260 in E) 255.9 in

D) To find: Convert 6.5 m to cm, 6.5 x 100 cm =650 cm / 2.54 cm =255.9, round to 2 sig figs to get 260

For the following equilibrium reaction, which cause and effect are correctly matched? CO(g) + 2H2(g) ⇌ CH3OH(g) + heat A) add heat, shift right B) add CO, shift left C) remove CH3OH, shift left D) remove heat, no change E) remove H2, shift left

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane. The process that occurs in this system is A) filtration. B) hydration. C) neutralization. D) dialysis. E) osmosis.

Given the following equation, what is the correct form of the conversion factor needed to convert the number of moles of O2 to the number of moles of Fe2O3 produced?

How many electrons will iodine gain or lose when it forms an ion? A) lose 1 B) gain 5 C) lose 2 D) lose 3 E) gain 1

How many grams of hydrogen peroxide (H2O2) are needed to produce 25.0 g of oxygen? A) 106 g B) 26.6 g C) 5.88 g D) 25.0 g E) 53.1 g

How many hydrogen atoms are present in 75.0 g of H2O? A) 75.0 atoms B) 4.17 atoms C) 7.53 × 1024 atoms D) 2.51 × 1024 atoms E) 5.02 × 1024 atoms

How many mL of 0.246 M Pb(NO3)2 are needed to react with 36.0 mL of 0.322 M KCl ? 2KCl(aq) + Pb(NO3) 2(aq) → 2KNO3(aq) + PbCl2(s) A) 36.0 mL B) 18.0 mL C) 72.0 mL D) 47.1 mL E) 23.6 mL

How many milliliters of 0.400 M NaOH are required to completely neutralize 20.0 mL of 0.200 M HCl? A) 50.0 mL B) 40.0 mL C) 0.100 mL D) 20.0 mL E) 10.0 mL

How many milliliters of a 25% (m/v) NaOH solution would contain 75 g of NaOH? A) 25 mL B) 75 mL C) 33 mL D) 19 mL E) 3.0 × 102 mL

How many moles of hydrogen peroxide (H2O2) are needed to produce 5.0 moles of water? A) 1.0 mole B) 2.0 moles C) 4.0 moles D) 5.0 moles E) 8.0 moles

How many valence electrons are in the electron-dot structure of CCl4 ? A) 0 B) 82 C) 6 D) 8 E) 32

How many valence electrons does nitrogen have? A) one B) two C) three D) four E) five

Identify the metalloid in the following list. A) sulfur B) fluorine C) silver D) copper E) germanium

If 2.00 g of Mg reacts completely with 50.0 mL of HCl solution, what is the molarity of the HCl solution? A) 1.65 M B) 80.0 M C) 8.00 M D) 0.823 M E) 3.29 M

In a ________ reaction, two or more elements or compounds form one product. A) decomposition B) single replacement C) dehydration D) double replacement E) combination

In a covalently bonded molecule, the number of electrons that an atom shares with others is usually equal to the number of electrons A) in the atom. B) in its nucleus. C) in all the atoms. D) in its ion. E) needed to give it a stable electron configuration.

In a gas, the distance between the particles is A) very close relative to the size of the molecules. B) close relative to the size of the molecules. C) fixed relative to the size of the molecules. D) small relative to the size of the molecules. E) very large relative to the size of the molecules.

In a neutralization reaction A) two acids react to form water. B) water and a salt react to form an acid and a base. C) an acid and a salt react to form water and a base. D) a base and a salt react to form water and an acid. E) an acid and a base react to form a salt and water.

In any chemical reaction, the rate of the reaction can be increased by A) decreasing the temperature. B) changing the size of the container. C) adding water to the reaction. D) adding product molecules to the reaction mixture. E) increasing the concentrations of the reactants.

In ionic compounds, ________ lose their valence electrons to form positively charged ________. (5,2) A) metals; anions B) nonmetals; cations C) metals; polyatomic ions D) nonmetals; anions E) metals; cations

In the following gas phase reaction, what is the effect of adding more NO2 to the starting reaction mixture? 2NO2(g) ⇌ N2O4(g) A) It would make the reaction more endothermic. B) It would make the reaction more exothermic. C) It would slow the reaction down. D) It would decrease the final quantity of products. E) It would increase the final quantity of products.

In water, a substance that ionizes completely in solution is called a A) weak electrolyte. B) nonelectrolyte. C) semiconductor. D) nonconductor. E) strong electrolyte.

Methanol, CH3OH, can be classified as a ________. A) gas B) solid C) weak electrolyte D) strong electrolyte E) nonelectrolyte

Of the elements: B, C, F, Li, and Na. The element with the most metallic character is A) B. B) C. C) F. D) Li. E) Na

Of the elements: B, C, F, Li, and Na. The element with the smallest ionization energy is A) B. B) C. C) F. D) Li. E) Na.

Of the elements: B, C, F, Li, and Na., the element with the largest atomic radius is A) B. B) C. C) F. D) Li. E) Na.

Pentane (C5H12) reacts with oxygen (O2) to form carbon dioxide (CO2) and water (H2O) according to thefollowing reaction. Answer the question(s) that follow about this reaction. C5H12 + ? O2 → ? CO2+ ? H2O What is the coefficient for oxygen in the balanced equation? A) 2 B) 4 C) 5 D) 6 E) 8

Rubbing alcohol is 70.% isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a 1 pint (473 mL) container? A) 70. mL B) 0.15 mL C) 680 mL D) 470 mL E) 330 mL

The ________ is the energy difference between reactants and products in a chemical reaction. A) transition energy B) activation energy C) product energy D) overall energy E) heat of reaction

The amount of space occupied by a substance is its A) mass. B) density. C) weight. D) length. E) volume.

The atomic number of an atom is equal to the number of A) nuclei. B) neutrons. C) neutrons plus protons. D) electrons plus protons. E) protons.

Elements

Elements •are pure substances from which all other things are built. •cannot be broken down into simpler substances.

Given the elements C, N, and F, A. which is the largest atom? B. which has the highest ionization energy? C. which belongs to Group 5A (15)?

Given the elements C, N, and F, A. which is the largest atom? C B. which has the highest ionization energy? F C. which belongs to Group 5A (15)? N

groups 7A (17)

Halogens

groups 3A through 6A (13-16)

No common names

When a related ion has one less oxygen, its name ends in ite.

SO32−sulfite PO33−phosphite NO2−nitrite

Names of most common polyatomic ions end in ate

SO42−sulfate PO43−phosphate NO3−nitrate

Group 1A elements (1)

alkali metals

An element with metallic character is one that loses valence electrons

easily

An atom is the smallest particle of an

element that retains the characteristics of that element

electrons

have a negative (-) charge

protons

have a positive (+) charge

Neutrons

have no charge

Metallic character

is more prevalent in metals on the left side of the periodic table. •is less for nonmetals on the right side of the periodic table that do not lose electrons easily. •decreases going down a group, as electrons are farther away from the nucleus.

Metals are located to the

left

Number of protons + neutrons =

mass number

Number of neutrons=

mass number - atomic number Note: Mass numbers are given for specific isotopes only

Density

mass/volume

Covalent bonds occur when nonmetal atoms share electrons to attain a

noble gas arrangement

Groups 8A (18)

noble gases

Ionic bonds occur when valence electrons of a metal atom are transferred to the atom of a

nonmetal.

Like charges

repel each other

What type of reaction is the following? Zn + 2HCl → ZnCl2 + H2

single replacement reaction

Nonmetals are located to

the right

solid, liquid, gas

three states of matter

Groups 3B-2B (3-12)

transition metals

Group 7A (17)the halogens, are highly reactive and form compounds with most of the elements. Group 7A includes the following:

•fluorine (F) •chlorine (Cl) •bromine (Br) •iodine (I)

When naming an ionic compound

•the name of the metal is written first and is the same as the name of the element. •the name of the nonmetal is the first syllable of the nonmetal name + ide ending and is written second. •a space is placed between the name of the metal and nonmetal ion.

In a chemical formula

•the symbols and subscripts are written in the lowest whole-number ratio of the atoms or ions. •the sum of ionic charges in the formula equals zero. •the total positive charge = total negative charge

To calculate atomic mass

•use the experimental percent abundance of each isotope of the element. •multiply the percent abundance by the atomic mass of that isotope. •sum the total mass of all isotopes.

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