acs practice questions

CHEM 101 American Chemical Society (ACS) Final Practice Questions CHEM101 2011SP

Yegor Timofeyenko May 2011

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

1. For the following reaction, what is the correct coefficient for the H2?

Fe (s) + HCl (aq) → FeCl3 (aq) + H2 (g)

A) 1 B) 2 C) 3 D) 4 E) 5

1.

Answer: C

2. How many moles of Al are needed to react exactly with 10.00 moles of Fe2O3 according to the

following equation?

Fe2O3 + 2 Al Al2O3 + 2Fe

A) 60.0 moles B) 30.0 moles C) 15.0 moles D) 20.0 moles

2.

Answer: D

3. The state of matter a substance is in is determined by its ________.

A) electrical conductivity B) density

C) solubility D) temperature

3.

Answer: D

4. Consider the following precipitation reaction:

K2S (aq) + Fe(NO3)2 (aq) → FeS (s) + 2KNO3 (aq)

What is the correct net ionic equation for the reaction?

A) Fe2+(aq) + S2-(aq) → FeS(s)

B) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq)

C) K+(aq) + NO3-(aq) → KNO3(s)

D) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s)

E) No reaction occurs.

4.

Answer: A

5. Arrange the following elements in order of increasing atomic radii.

Sr, Rb, Sb, I, In

A) I Sb In Sr Rb B) I Sb In Rb Sr

C) Rb Sr In Sb I D) In Sb I Sr Rb

5.

Answer: A

1



6. Which of the following energy-level changes for an electron is most energetic?

A) 6 → 1

B) 4 → 1

C) 3 → 1

D) 5 → 1

E) All changes have the same energy.

6.

Answer: A

7. What is the systematic name for aqueous H3PO4?

A) hydrophosphorous acid

B) phosphorous acid

C) phosphoric acid

D) hydrophosphoric acid

E) none of the above

7.

Answer: C

8. Which of the following is the correct electron-dot structure for CS2?

A)

B)

C)

D)

E)

8.

Answer: A

9. What is the coefficient of hydrogen, H2, when the following equation is balanced?

Al (s) + H2SO4(aq) → Al2(SO4) 3 (aq) + ? H2 (g)

A) 1 B) 2 C) 3 D) 4 E) 5

9.

Answer: C

10. In a molecule with covalent bonding,

A) atoms of noble gases are held together by attractions between oppositely charged ions.

B) atoms of different metals form bonds.

C) atoms are held together by sharing electrons.

D) oppositely charged ions are held together by strong electrical attractions.

E) atoms of metals form bonds to atoms of nonmetals.

10.

Answer: C

2



11. How many grams of slaked lime [Ca(OH)2] are produced from 7.00 grams of quicklime (CaO),

according to the following balanced chemical equation?

CaO + H2O → Ca(OH)2

A) 5.30 g B) 518 g C) 9.25 g D) 9.50 g E) 7.00 g

11.

Answer: C

12. What is the name of SnCl2?

A) strontium chloride

B) tin dichloride

C) tin(II) chloride

D) ditin chloride

E) tin chloride

12.

Answer: C

13. Which statement about the boiling point of water is incorrect?

A) In a pressure cooker, shorter cooking times are required due to the change in boiling point.

B) The boiling point is less than 100*C for locations at low elevations.

C) The boiling point is greater than 100*C in a pressure cooker.

D) Boiling water at 1 atm will always have a temperature of 100*C.

13.

Answer: B

14. Which of the following names is paired with an incorrect formula?

A) Iron(III) chloride - FeCl3 B) Copper(II) nitride - Cu3N2

C) Lithium bromide - LiBr D) Copper(II) oxide - Cu2O

14.

Answer: D

15. How many centimeters are there in 57.0 in.?

A) 22 cm B) 22.4 cm C) 145 cm D) 0.0445 cm E) 140 cm

15.

Answer: C

16. The measurement 0.000 0043 m, expressed correctly using scientific notation, is

A) 4.3 x 10-6 m.

B) 4.3 x 10-7 m.

C) 4.3 x 106 m.

D) 4.3 m.

E) 0.43 x 10-5 m.

16.

Answer: A

3



17. What type of reaction is represented by the following equation?

AB + C → AC + B

A) decomposition

B) combustion

C) double displacement

D) single displacement

E) combination

17.

Answer: D

18. A thimble of water contains 4.0 x 1021 molecules. The number of moles of H2O is:

A) 6.6 x 10-23 B) 6.6 x 10-3 C) 2.4 x 1045 D) 2.4 x 1023

18.

Answer: B

19. A pure substance A is found to change upon heating into two new pure substances, B and C. C can bedecomposed by chemical means, B cannot be decomposed by chemical means. From this we mayconclude that ________.

A) A is an element, B and C are compounds B) A, B and C are all elements

C) A and C are compounds, B is an element D) A is a compound, B and C are elements

19.

Answer: C

20. Which of the following pairs of subatomic particles have charges of equal magnitude but opposite insign?

A) proton and electron B) electron and neutron

C) neutron and proton D) proton and positron

20.

Answer: A

21. The mass of a particular drop of water was determined to be 0.0521 g. How many water

molecules are in this drop of water?

A) 3.14 x 1021

B) 1.74 x 1021

C) 2.08 x 1026

D) 1.74 x 1022

E) 3.14 x 1022

21.

Answer: B

22. Which is an example of a homogeneous mixture?

A) chocolate chip cookie B) oil & vinegar salad dressing

C) a rock collection D) glucose solution

22.

Answer: D

4



23. Which of the following setups would convert centimeters to feet?

A) cm × 1 in.

2.54 cm ×

1 ft

12 in.

B) cm × 2.54 in.

1 cm ×

1 ft

12 in.

C) cm × 2.54 cm

1 in. ×

1 ft

12 in.

D) cm × 1 in.

2.54 cm ×

12 in.

1 ft

E) cm × 2.54 cm

1 in. ×

12 in.

1 ft

23.

Answer: A

24. Place the following elements in order of increasing electronegativity.

K Cs P

A) P < K < Cs

B) P < Cs < K

C) K < P < Cs

D) Cs < P < K

E) Cs < K < P

24.

Answer: E

25. 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) 6.77 g/mL

B) 1.00 g/mL

C) 0.0518 g/mL

D) 10.4 g/mL

E) 19.3 g/mL

25.

Answer: E

26. What is the chemical name of Pb3(PO4)4?

A) lead (III) phosphate B) lead triphosphide

C) lead (IV) phosphate D) lead phosphate

26.

Answer: C

27. Which group contains only elements which normally exist as diatomic molecules?

A) helium; neon, argon

B) nitrogen; sulfur, bromine

C) hydrogen; lithium, sodium

D) oxygen; phosphorus, germanium

E) nitrogen; oxygen, fluorine

27.

Answer: E

5



28. Calculate the number of moles of aspirin, C9H8O4, in a 4.0 gram tablet.

A) 0.022 B) 2.2 x 10-4 C) 2.2 D) 4.6 x 10-3

28.

Answer: A

29. The main group element E reacts with chlorine to form an ionic compound with the formula

ECl2. The element E is a member of what group in the Periodic Table?

A) 1A

B) 2A

C) 7A

D) 6A


29.

Answer: B

30. The elements in groups 1A, 7A and 8A are called, respectively:

A) alkali metals, chalcogens, halogens

B) alkaline earth metals, halogens, chalcogens

C) alkali metals, halogens, noble gases

D) alkaline earth metals, transition metals, halogens

30.

Answer: C

31. How many joules 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 0.450 J/g °C.

A) 350 J B) 160 J C) 35 J D) 10. J E) 16 J

31.

Answer: B

32. How many kilograms are in 452 mg?

A) 4.52 × 108 kg B) 4.52 × 10‐7 kg C) 4.52 × 10‐4 kg D) 0.452 kg

32.

Answer: C

33. For the equation given, how many grams of ammonia will result from 44.0 g of nitrogen (N2)

and sufficient hydrogen (H2)?

N2 (g) + 3H2 (g) → 2NH3 (g)

A) 107 g B) 53.4 g C) 214 g D) 88.0 g E) 26.7 g

33.

Answer: B

34. A beaker contains 0.964 grams of N2. How many moles of N2 does the beaker contain?

A) 0.0344 mol B) 0.0688 mol

C) 2.262 x 1023 mol D) 2.64 mol

34.

Answer: A

6



35. Which solution is the most concentrated? Each choice refers to the same solute and solvent.

A) 2.4 g solute in 5 mL solution

B) 30 g solute in 150 mL solution

C) 50 g solute in 175 mL solution

D) 2.4 g solute in 2 mL solution

E) 20 g solute in 50 mL solution

35.

Answer: D

36. Choose the best electron-dot structure for OCl2.

A)

B)

C)

D)

E)

36.

Answer: A

37. What is the correct formula that forms when calcium and sulfur react?

A) CaS B) CaSO4 C) CaSO3 D) Ca3S2

37.

Answer: A

38. The correct answer obtained from subtracting 1.2 from 123.96 contains ________.A) 5 significant figures B) 2 significant figuresC) 4 significant figures D) 3 significant figures

38.

Answer: C

39. The statement that best describes the formation of an ionic compound is:

A) Electrons are shared between two atoms and discrete molecules are formed.

B) Electrons are transferred from a non-metal to a metal, and the resulting charged particles

form a crystalline network.

C) Electrons move freely among a network of nuclei in fixed positions.

D) Electrons are transferred from a metal to a non-metal, and the resulting charged particles

form a crystalline network.

E) Each atom achieves an octet using electrons provided from an external electrical supply.

39.

Answer: D

40. The main type of interaction between molecules of hydrogen ( H2 ) are

A) dipole-dipole.

B) ionic bonds.

C) hydrogen bonds.

D) dispersion forces.

E) polar covalent.

40.

Answer: D

7



41. How many grams of sodium hydroxide (NaOH) are there in 0.150 mol?

A) 40.0 g B) 1.50 g C) 150. g D) 6.00 g E) 600. g

41.

Answer: D

42. Calculate the number of grams of sulfuric acid (H2SO4) in 6.00 mol.

A) 6.00 g B) 5.00 g C) 98.1 g D) 588 g E) 16.3 g

42.

Answer: D

43. What is the concentration, in (m/m) %, or (w/w)% of a solution prepared from 50.0 g NaCl and

150.0 g of water?

A) 25.0% B) 33.3% C) 40.0% D) 3.00% E) 0.250%

43.

Answer: A

44. Calculate the percent by mass sulfur in sulfuric acid, H2SO4.

A) 48.9% B) 32.7% C) 16.3% D) 8.16% E) 23.4%

44.

Answer: B

45. What is the correct formula for cobalt (II) cyanide?

A) Co(SCN)2 B) CoCN C) CoSCN D) Co(CN)2

45.

Answer: D

46. The energy of 4.72 kJ is the same as ________ cal.

A) 8.86 B) 1.13 C) 19 800 D) 4.184 E) 1130

46.

Answer: E

47. A pure substance has been isolated in the laboratory. Based on the two characteristics below, howcan the substance be classified?

I. The species can not be separated by physical means.

II. The species can be separated by chemical means.

A) a homogeneous mixture B) a heterogeneous mixture

C) an element D) a compound

47.

Answer: D

8



48. What is the balanced complete ionic equation for the following reaction in aqueous solution?

Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2 (s) + 2NaNO3 (aq)

A) Pb2+ + 2Cl- → PbCl2

B) Pb2+ + 2NO3- + 2Na+ + 2Cl- → Pb2+ + 2Cl- + 2Na+ + NO3-

C) Pb2+ + NO3- + 2Na+ + 2Cl- → PbCl2 + 2Na+ + NO3

-

D) Pb2+ + (NO3)2- + 2Na+ + Cl2- → PbCl2 + 2Na+ + (NO3)2-

E) Pb2+ + 2NO3- + 2Na+ + 2Cl- → PbCl2 + 2Na+ + 2NO3

-

48.

Answer: E

49. What is the mass percent oxygen in sodium carbonate, Na2CO3?

A) 43.4% B) 11.3% C) 56.6% D) 15.1% E) 54.7%

49.

Answer: A

50. If the following ions Ca2+, Cl-, Na+ and CO32- are placed in a test tube, the precipitate

formed is ________.

A) CaCO3 B) NaCl

C) CaCl2 D) no precipitate will be formed

50.

Answer: A

51. Identify the spectator ions in the following molecular equation.

KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)

A) Ag+ & Br-

B) K+ & Br-

C) Ag+ & NO3-

D) K+ & NO3-

E) There are no spectator ions in this reaction.

51.

Answer: D

52. What is the correct name for the following compound, (NH4)3PO4?A) ammonium phosphide B) ammonium phosphate

C) triammonium phosphate D) nitrogen tetrahydride phosphorous

52.

Answer: B

53. The calculator answer obtained from multiplying 21.08 x 1.9634 is 41.388472. The answer to the correctnumber of significant figures is ________.A) 41.3884 B) 41.4 C) 41.388 D) 41.39

53.

Answer: D

9



54. Which of the following ionic compounds is named without using a Roman numeral?

A) AuCl3 B) CuS C) Fe2O3 D) Ca(OH)2

54.

Answer: D

55. How many liters of a 0.0550 M KCl solution contain 0.163 moles of KCl?

A) 1.48 L B) 3.37 L C) 2.96 L D) 8.97 L E) 1.12 L

55.

Answer: C

56. What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution?

A) 2.0 M B) 0.029 M C) 34 M D) 1.0 M E) 0.50 M

56.

Answer: A

57. The chemical formula for heptasulfur dioxide is ________.

A) O2S B) SO2 C) S2O7 D) S7O2

57.

Answer: D

58. A solution with the same osmotic pressure as the blood is

A) molar to the blood.

B) isotonic to the blood.

C) nontonic to the blood.

D) hypertonic to the blood.

E) hypotonic to the blood.

58.

Answer: B

59. The Group 8A elements

A) react vigorously with water.

B) are unreactive and are rarely found in combination with other elements.

C) are liquids at room temperature.

D) melt at high temperatures.

E) are good conductors of electricity.

59.

Answer: B

60. A bond where the electrons are shared equally is called a(n) ________ bond.

A) coordinate covalent

B) ionic

C) pure (nonpolar) covalent

D) polar covalent


60.

Answer: C

10



61. According to the following balanced reaction, how many moles of NO are formed from 8.44

moles of NO2 if there is plenty of water present?

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

A) 1.83 moles NO

B) 25.3 moles NO

C) 8.44 moles NO

D) 5.50 moles NO

E) 2.81 moles NO

61.

Answer: E

62. How many moles of CO2 will be produced from the complete combustion of 0.956 moles of

C7H16 in the reaction below?

C7H16 + 11 O2 7 CO2 + 8 H2O

A) 6.69 moles B) 0.667 mole C) 3.50 moles D) 1.85 moles

62.

Answer: A

63. In which of the following pairs of elements is one element a metalloid and one element a nonmetal?

A) As and Si B) Pb and Bi C) Ge and F D) Sb and Ca

63.

Answer: C

64. You have been given 3.50 moles of ammonia, NH3. How many molecules of ammonia does it

contain?

A) 2.21 x 1024 B) 1.81 x 1024 C) 4.75 x 10-25 D) 2.21 x 10-24

64.

Answer: A

65. What is the formula for calcium phosphate?

A) Ca2PO4

B) Ca3(PO4)2

C) Ca2(PO3)3

D) Ca4(PO3)3

E) Ca3PO4

65.

Answer: B

11



66. The “set-up” for the problem “What is the mass, in grams, of 2.50 x 1022 atoms of Ca?” which

follows is correct, except numbers in the last conversion factor have been replaced by the

letters A and B. What are the numerical values of A and B, respectively?

A) 1 mole and 6.02 x 1023 atoms B) 6.02 x 1023 g and 1 atom

C) 40.08 mol and 6.02 x 1023 atoms D) 40.08 g and 1 mol

66.

Answer: D

67. Which of the following is a chemical property of aspirin?

A) It is a white crystalline solid in pure form at room temperature.

B) It can be compressed into tablets when mixed with cornstarch.

C) It melts at 135°C.

D) It does not readily dissolve in water.

E) It does not decompose when protected from moisture.

67.

Answer: E

68. What is the mass percent of carbon in methane, CH4?

A) 20.0% B) 25.2% C) 50.0% D) 74.9% E) 12.5%

68.

Answer: D

69. What is the correct name for Cl2O7?

A) chlorine oxide B) chloric acid

C) dichlorine heptoxide D) dichloride oxide

69.

Answer: C

70. Which of the following numbers contains three significant figures?A) 350 B) 85.967 C) 1.050 D) 8.90

70.

Answer: D

71. Which of the following compounds is soluble in water?

A) MgCO3

B) BaSO4

C) CaS

D) PbCl2

E) None of these compounds is soluble in water.

71.

Answer: C

12



72. The mass/volume percent concentration refers to

A) grams of solute in 1 L of solvent.

B) grams of solute in 100 mL of solvent.

C) grams of solute in 1 L of solution.

D) grams of solute in 100 mL of solution.

E) grams of solvent in 100 mL of solution.

72.

Answer: D

73. Which has the highest boiling point?

A) 0.1 M MgCl2

B) 0.1 M Na2SO4

C) 0.1 M glucose, C6H12O6

D) 0.1 M Al(NO3)3

E) pure water

73.

Answer: D

74. Which of the following statements is FALSE?

A) The rate of vaporization increases with increasing surface area.

B) The rate of vaporization increases with decreasing strength of intermolecular forces.

C) Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole

forces.

D) The rate of vaporization increases with increasing temperature.

E) None of the above are false.

74.

Answer: C

75. Which of the following is not a physical change?

A) dissolving Kool-aid B) liquefying oxygen

C) boiling water D) frying an egg

75.

Answer: D

76. Which of the following is the correct “set-up” for the problem “How many moles of C are

present in 25.00 grams of C6H12O6?”

A)

B)

C)

D)

76.

Answer: C

13



77. What are the coefficients for the balanced equation?

__Al2(SO4)3 (aq) + __KOH (aq) → __Al(OH)3 (s) + __K2SO4 (aq)

A) 1, 1, 1, 1 B) 1, 2, 3, 1 C) 1, 2, 1, 2 D) 1, 6 , 2, 3 E) 1, 2, 1, 3

77.

Answer: D

78. Which of the following statements about intermolecular forces is incorrect?

A) They occur within molecules rather than between molecules.

B) They are much weaker than intramolecular forces.

C) They must be overcome in order for molecules to escape from the liquid state into the vapor state.

D) They are electrostatic in origin.

78.

Answer: A

79. When a substance undergoes a chemical change it is always true that ________.

A) heat is absorbed B) new substances are formed

C) it changes state D) it condenses

79.

Answer: B

80. Which of the following represent the Lewis structure for Br⁻?

A) B) C) D) E)

80.

Answer: A

81. The mass percent of chlorine in Mg(ClO3)2 is:

A) 33.0 % B) 37.1 % C) 12.7 % D) 43.6 %

81.

Answer: B

82. One mol of particles of any substance contains how many particles?

A) 106

B) 3 × 1010

C) 6.022 × 10-23

D) 3 × 10-10

E) 6.022 × 1023

82.

Answer: E

83. The number of unpaired electrons present in a magnesium atom is ________.A) 1 B) 3 C) 5 D) 0

83.

Answer: D

14



84. Calculate the number of lithium atoms in 3.66 moles of lithium.

A) 3.54 x 1025 B) 6.23 x 1025 C) 2.20 x 1024 D) 8.97 x 1026

84.

Answer: C

85. The scientific principle which explains the observation that the amount of heat transfer

accompanying a change in one direction is numerically equal but opposite in sign to the

amount of heat transfer in the opposite direction is

A) Avogadroʹs Law.

B) the Law of Conservation of Mass and Energy.

C) the Law of Conservation of Mass.

D) the Law of Conservation of Energy.

E) the Law of Definite Proportions.

85.

Answer: D

86. Which of the following prototype equations corresponds to a double displacement type

reaction?

A) A + BC → ABC

B) A + BC → AC + B

C) AB + CD → AD + CB

D) AB + CD → AC + BD

E) AA + BB → BB + AA

86.

Answer: C

87. Which of the following pairs has an error in the formula or in the name? Formula Chemical Name

A) CoF3 cobalt fluoride B) CCl4 carbon tetrachloride

C) Cl2O7 dichlorine heptoxide D) Fe(ClO4)2 iron (II) perchlorate

87.

Answer: A

88. The number of cycles that pass through a stationary point is called

A) amplitude

B) frequency

C) median

D) wavelength

E) area

88.

Answer: B

89. Which of the following cannot have hydrogen bonds?

A) HF B) NH3 C) HCl D) CH3OH E) H2O

89.

Answer: C

15



90. The carbon dioxide molecule is linear. The electronegativities of C and O are 2.5 and 3.5,

respectively. Based on these values and on consideration of molecular geometry, the C-O

bond is ________ and the molecule is ________.

A) non-polar; polar

B) polar; polar

C) polar; non-polar

D) non-polar; non-polar


90.

Answer: C

91. Consider the molecule SiCl4. The electronegativity values for Si and Cl are 1.8 and 3.0,

respectively. Based on these values and on consideration of molecular geometry, the Si-Cl

bond is ________ and the molecule is ________.

A) non-polar; non-polar

B) polar; polar

C) non-polar; polar

D) polar; non-polar


91.

Answer: D

92. A temperature of 316 on the Kelvin scale is equivalent to ________.

A) 43 °C B) 589 °C C) 589 °C D) 104 °C

92.

Answer: A

93. What is the classification for this unbalanced reaction?

Fe (s) + HCl (aq) → FeCl3 (aq) + H2 (g)

A) single displacement

B) combustion

C) double displacement

D) decomposition

E) combination

93.

Answer: A

94. The energy of motion is referred to as ________.

A) kinetic energy

B) work

C) potential energy

D) freezing

E) specific heat

94.

Answer: A

16



95. Two atoms must represent the same element if they both have the same:A) atomic number B) number of electron shellsC) number of neutrons D) atomic mass

95.

Answer: A

96. Which element/classification pair is incorrectly matched? Element Classification

A) Cl Halogen B) Ca Transistion metal

C) Li Alkali metal D) Ne Noble gas

96.

Answer: B

97. How many grams of fluorine (F2) are required to produce 20.0 grams of FeF3 from the

reaction shown?

2 Fe + 3F2 → 2 FeF3

A) 10.1 g B) 20.2 g C) 5.05 g D) 6.74 g E) 4.49 g

97.

Answer: A

98. The number 1.987 x 106 in normal decimal notation is ________.A) 19,870,000 B) 19,870 C) 198,700 D) 1,987,000

98.

Answer: D

99. How many grams are present in 6.5 moles of Cu(NO3)2?

A) 124 g B) 1220 g C) 404 g D) 1080 g

99.

Answer: B

100. In a ________ reaction, two or more elements or compounds form one product.

A) combustion

B) single displacement

C) combination

D) double displacement

E) decomposition

100.

Answer: C

101. What is the atomic mass of B if 19.9% of all B atoms have a mass of 10.01 amu and 80.1% have a massof 11.01 amu?

A) 10.50 amu B) 10.81 amu C) 10.21 amu D) 10.63 amu

101.

Answer: B

17



102. According to the following balanced reaction, how many moles of KOH will be formed from

5.44 moles of H2O? Assume an excess of KO.

4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)

A) 8.33 moles KOH

B) 16.7 moles KOH

C) 10.9 moles KOH

D) 2.72 moles KOH

E) 4.87 moles KOH

102.

Answer: C

103. If the temperature is 18 °C then the reading on the Fahrenheit scale would be ________.

A) 40 °F B) 64 °F C) 12 °F D) 38 °F

103.

Answer: B

104. Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200 M NaCl to

250.0 mL.

A) 0.0160 M B) 0.160 M C) 0.00800 M D) 2.50 M E) 0.0320 M

104.

Answer: A

105. Calculate the number of iron atoms in 6.98 x 10−3 grams of iron.

A) 7.53 x 1019 atoms B) 3.24 x 1023 atoms

C) 9.37 x 1028 atoms D) 3.92 x 1019 atoms

105.

Answer: A

106. How many moles of iron are present in 3.15 x 1024 atoms of iron?

A) 1.90 moles

B) 0.523 moles

C) 5.23 moles

D) 292 moles

E) 1.90 x 1048 moles

106.

Answer: C

107. The correct name for the ionic compound SnS2 is ________.

A) tin (IV) sulfide B) selenium sulfide C) tin (II) sulfide D) tin sulfide

107.

Answer: A

108. Cobalt is atomic number 27. Cobalt-60 is used in the medical treatment of cancer. How many neutronsand protons are contained in the nucleus of this isotope?

A) 27 neutrons, 27 protons B) 27 neutrons, 33 protons

C) 33 neutrons, 33 protons D) 33 neutrons, 27 protons

108.

Answer: D

18



109. When the following equation is correctly balanced, what is the coefficient for aluminum?

Al (s) + O2 (g) → Al2O3 (s)

A) 2 B) 3 C) 6 D) 1 E) 4

109.

Answer: E

110. Given the electronegativity values of N (3.0) and O (3.5), illustrate the bond polarity in a

nitrogen monoxide molecule, NO, using delta notation.

A) (δ+) NO (δ-)

B) (δ-) NO (δ+)

C) (δ+) NO (δ+)

D) (δ-) NO (δ-)


110.

Answer: A

111. The strongest forces between HF molecules are ________.

A) dispersion forces

B) dipole-dipole attractions

C) ionic bonds

D) hydrogen bonds

E) nonpolar covalent bonds

111.

Answer: D

112. What is the chemical formula for hydrobromic acid?

A) HBr(aq)

B) HBrO3(aq)

C) HBrO2(aq)

D) HBrO(aq)


112.

Answer: A

113. The name of the compound with formula NaMnO4 is

A) sodium magnesium oxide.

B) sodium manganate.

C) sodium permanganate.

D) sodium manganese tetraoxide.

E) sodium magnesium tetraoxide.

113.

Answer: C

19



114. Aspirin (C9H8O4) can be made in the laboratory by reacting salicylic acid (C7H6O3) with

acetyl chloride (C2H3ClO).

C7H6O3 + C2H3ClO C9H8O4 + HCl

What mass of HCl is produced by the complete reaction of 36.0 g of acetyl chloride?

A) 16.7 g B) 8.69 g C) 108 g D) 58.1 g

114.

Answer: A

115. The physical state(s) present when a substance is melting is (are) ________.

A) gas

B) liquid + gas

C) solid + liquid

D) solid

E) liquid

115.

Answer: C

116. In which of the following sequences are the metric system prefixes listed in order of decreasing size?

A) hecto, kilo, deci B) kilo, centi, nano

C) nano, micro, milli D) micro, deca, centi

116.

Answer: B

117. Which transformation is evaporation?

A) solid → gas

B) solid → liquid

C) gas → solid

D) liquid → solid

E) liquid → gas

117.

Answer: E

118. Which compound listed below has a bond angle of 180° around the central atom?

A) CO2 B) NH3 C) H2O D) CC14

118.

Answer: A

119. The Roman numeral (II) in the name nickel (II) oxide indicates that ________.

A) there are two times as many nickel atoms present as oxygen atoms

B) there are two nickel atoms per formula unit

C) there are two oxygen atoms per formula unit

D) nickel atoms present are ions with a 2 charge

119.

Answer: D

20



120. Which of the following statements is TRUE?

A) An observation explains why nature does something.

B) A scientific law is fact.

C) A scientific law summarizes a series of related observations.

D) Once a theory is constructed, it is considered fact.

E) A hypothesis is speculation that is difficult to test.

120.

Answer: C

121. Which of the following electron configurations is impossible?

A) 1s22s42p63s23p3

B) 1s22s22p63s23p3

C) 1s22s22p63s23p6

D) 1s22s22p63s23p5

E) 1s22s22p63s23p1

121.

Answer: A

122. A molecule in which the central atom has no lone pairs and forms four single bonds is said to

have a ________ shape.

A) tetrahedral

B) planar

C) bent

D) pyramidal

E) linear

122.

Answer: A

123. Which element has the electron configuration [Kr]5s2 4d105p2?

A) Sn B) Pb C) Sb D) Ge

123.

Answer: A

124. Which of the following ions does not have the same electron configuration as the noble gas

neon?

A) F- B) Al3+ C) S2- D) Mg2+ E) O2-

124.

Answer: C

125. For the reaction: 2 P + 3 Cl2 2 PCl3 if 32.5 g of Cl2 reacts completely with excess P, how

many grams of PCl3 will be produced?

A) 42.0 g B) 62.9 g C) 83.9 g D) 94.4 g

125.

Answer: A

126. Iron pyrite (fool’s gold) is iron (II) sulfide. What is its formula?

A) FeSO3 B) FeS C) FeSO4 D) Fe2S3

126.

Answer: B

21



127. According to the United States Food and Drug Administration, the recommended daily

requirement of protein is 44 g. This is __________ of protein.

A) 320 000 oz B) 0.061 oz C) 1.6 oz D) 150 000 oz E) 1200 oz

127.

Answer: C

128. What is the molecular geometry of PH3?

A) tetrahedral

B) trigonal planar

C) bent

D) linear

E) trigonal pyramidal

128.

Answer: E

129. Which of the following statements concerning temperature change as a substance is heated is incorrect?

A) During the time a solid melts to a liquid the temperature remains constant.

B) As a solid is heated, its temperature rises until its melting point is reached.

C) As a liquid is heated, its temperature rises until its boiling point is reached.

D) During the time a liquid is changing to the gaseous state the temperature gradually increases whileall the liquid is changed.

129.

Answer: D


A) N2S3 dinitrogen trisulfide B) SrCl strontium chloride

C) BaSO3 barium sulfite D) ICl iodine monochloride

130.

Answer: B

131. Nitrogen gas has a(n) ________ volume and a(n) ________ shape.

A) indefinite; definite B) definite; definite

C) definite; indefinite D) indefinite; indefinite

131.

Answer: D

132. What is the systematic name for aqueous HC2H3O2?

A) dicarbonic acid

B) acetic acid

C) hydrogen carbonic acid

D) carbonic acid


132.

Answer: B

22



133. Which products would result from the double displacement reaction between MgCl2(aq) and

Na2CO3(aq)?

A) Na2Cl2(aq) and MgCO3(s)

B) NaCl(aq) and Mg2CO3(s)

C) MgNa2(aq) and CO3Cl2(aq)

D) NaCl(aq) and Mg(CO3)2(s)

E) NaCl(aq) and MgCO3(s)

133.

Answer: E

134. Which has the lowest boiling point?

A) 0.1 M MgCl2

B) 0.1 M Na2SO4

C) 0.1 M glucose, C6H12O6

D) pure water

E) 0.1 M Al(NO3)3

134.

Answer: D

135. A chemical ice pack gets cold when you mix the two chemicals within. The reaction that occurs

is

A) thermodynamic.

B) exothermic.

C) endothermic.

D) physical.


135.

Answer: C

136. Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO2.

A) eg=linear, mg=linear, nonpolar

B) eg=tetrahedral, mg=tetrahedral, nonpolar

C) eg=trigonal pyramidal, mg=trigonal pyramidal, polar

D) eg=tetrahedral, mg=bent, polar

E) eg=trigonal planar, mg=bent, polar

136.

Answer: E

137. The abbreviated electron configuration for the sulfur atom is ________.

A) [Ne] 3s2 3p4

B) [S] 3s2 3p4

C) [He] 3s2 3p4

D) [Ar] 3s2 3p4

E) [Ne] 3s2 3p6

137.

Answer: A

23



138. Which of the following statements does not describe a physical property?

A) Snow forms in the clouds via deposition.

B) Mercury is a liquid at room temperature.

C) A strip of magnesium metal weighs 7.49 grams.

D) Sparks are created when sodium metal is added to water.

138.

Answer: D

139. Perform the following mathematical operations. Express your answer to the proper number ofsignificant figures. (93.789 − 5.40) x 18.057 A) 1600 B) 1590 C) 1596 D) 1596.239

139.

Answer: C

140. What coefficient is placed in front of O2 to complete the balancing of the following equation?

C5H8 (l) + ? O2 (g) → 5CO2 (g) + 4H2O (g)

A) 7 B) 5 C) 1 D) 3 E) 9

140.

Answer: A

141. Considering 1.0 M solutions of each substance, which contains the largest concentration of

ions?

A) KCl B) NaOH C) FeCl3 D) NH3 E) K2SO4

141.

Answer: C

142. A bond where the electrons are shared unequally is called a(n) ________ bond.

A) ionic

B) polar covalent

C) coordinate covalent

D) non-polar covalent


142.

Answer: B

143. Which of the following is a general trend from left to right in the periodic table of elements?

A) atomic radius increases; metallic character increases

B) atomic radius decreases; metallic character decreases

C) atomic radius decreases; metallic character increases

D) atomic radius increases; metallic character decreases


143.

Answer: B

24



144. Place the following types of electromagnetic radiation in order of decreasing energy.

ultraviolet light radio waves microwaves

A) radio waves > ultraviolet light > microwaves

B) ultraviolet light > microwaves > radio waves

C) ultraviolet light > radio waves > microwaves

D) radio waves > microwaves > ultraviolet light

E) microwaves > radio waves > ultraviolet light

144.

Answer: B

145. How many mL of water should be added to 50.0 mL of a 15.0 M H2SO4 solution to give a final

concentration of 0.300 M?

A) 950 mL B) 2450 mL C) 2550 mL D) 1000 mL E) 2500 mL

145.

Answer: B

146. For the compound Cr2O3, what is the correct Roman numeral in the name, chromium (__) oxide?

A) III B) IV C) II D) VI

146.

Answer: A

147. The ability of an atom to attract the shared electrons in a covalent bond is its ________.

A) nonpolarity

B) electronegativity

C) ionic character

D) bonding ability

E) polarity

147.

Answer: B

148. Determine the electron geometry (eg) and molecular geometry (mg) of CO32⁻.

A) eg=trigonal planar, mg=bent

B) eg=tetrahedral, mg=trigonal planar

C) eg=tetrahedral, mg=trigonal pyramidal

D) eg=trigonal planar, mg=trigonal planar

E) eg=tetrahedral, mg=tetrahedral

148.

Answer: D

149. Determine the electron geometry, molecular geometry and polarity of N2O (O is terminal).

A) eg=trigonal planar, mg=bent, polar

B) eg=tetrahedral, mg=bent, polar

C) eg= linear, mg=linear, polar

D) eg=tetrahedral, mg=linear, nonpolar

E) eg=linear, mg=linear, nonpolar

149.

Answer: C

25



150. The atomic size of atoms

A) decreases going down within a group.

B) decreases going across a period (left to right).

C) increases going across a period (left to right).

D) does not change going across a period.

E) None of the above.

150.

Answer: B

151. What is the chemical formula for nitrous acid?

A) HNO2(aq)

B) HNO3(aq)

C) H2NO2(aq)

D) H2NO3(aq)


151.

Answer: A

152. Valence electrons are electrons located

A) in the outermost energy level of an atom.

B) throughout the atom.

C) in the nucleus of an atom.

D) in the first three energy levels of an atom.

E) in the first energy level of an atom.

152.

Answer: A

153. How many molecules of ethanol, C2H5OH, are contained in 150. gram sample?

A) 5.1 x 10-25 B) 1.96 x 1024 C) 6.02 x 1023 D) 46.0

153.

Answer: B

154. What fourth period element is represented by the dot structure shown?

A) Kr B) K C) Ca D) Br E) Mn

154.

Answer: D

155. How many molecules of water, H2O, are present in 75.0 g of H2O?

A) 75.0 molecules

B) 2.51 x 1024 molecules

C) 5.02 x 1024 molecules

D) 4.17 molecules

E) 7.53 x 1024 molecules

155.

Answer: B

26



156. How many of the following compounds are soluble in water?

Cu(OH)2 LiNO3 NH4Br K2S

A) 2 B) 4 C) 1 D) 0 E) 3

156.

Answer: E

157. The correct name for Fe2 (SO4)3 is

A) Iron (II) sulfate B) Iron (II) sulfide

C) Iron (III) sulfate D) Iron (III) sulfide

157.

Answer: C

158. The specific heat of copper is 0.385 J/g °C, and the specific heat of silver is 0.235 J/g °C. If the

same amount of heat is added to one g of each metal at 25 °C, what is the expected result?

A) The copper will reach a higher temperature.

B) The copper will reach a temperature lower than 25 °C.

C) The silver will soften.

D) The two samples will reach the same temperature.

E) The silver will reach a higher temperature.

158.

Answer: E

159. The surface temperature of the sun is 7530. °C. What is the surface temperature of the sun in degreesKelvins?

A) 10,400 K B) 420 K C) 273 K D) 7803 K

159.

Answer: D

160. The correct name for the ionic compound KClO3 is ________.

A) potassium chlorine oxide B) potassium chloride

C) potassium chlorite D) potassium chlorate

160.

Answer: D

161. Which of the following pairs is incorrectly matched?

Element Type of ElementA) silicon metalloid B) antimony metalC) arsenic metalloid D) nitrogen nonmetal

161.

Answer: B

162. The total number of valence electrons in a molecule of SOF2 is

A) 26 B) 20 C) 24 D) 18 E) 22

162.

Answer: A

27



163. What is the chemical formula for sulfuric acid?

A) HSO4(aq)

B) H2SO4(aq)

C) H2SO3(aq)

D) HSO3(aq)


163.

Answer: B

164. The average adult has approximately 9.0 pints of blood. If 20. drops of blood is equivalent to 1.0 mL,how many drops of blood does the average human contain?

A) 9.1 x 1011 drops B) 1100 drops C) 230,000 drops D) 85,000 drops

164.

Answer: D

165. What fourth period element is represented by the dot structure shown?

X:

A) Ca B) K C) As D) V E) Kr

165.

Answer: A

166. How many moles of water, H2O, are present in 75.0 g H2O?

A) 75.0 mol

B) 4.41 mol

C) 7.50 mol

D) 4.16 mol

E) 1.35 × 103 mol

166.

Answer: D

167. Which of the following does not contain 3.0 x 1024 atoms?

A) two moles of water B) 60 g of carbon

C) one mole of methane D) 160 g sulfur

167.

Answer: A

168. Which set of numbers will correctly balance the given equation?

___N2 (g) + ___O2 (g) → ___N2O5 (g)

A) 1, 5, 1 B) 1, 5, 2 C) 2, 5, 2 D) 2, 2, 5 E) 5, 2, 5

168.

Answer: C

169. The ʺdisappearanceʺ of mothballs is an example of ________.

A) condensation B) sublimation C) evaporation D) melting

169.

Answer: B

28



170. In exothermic reactions,

A) energy is converted to mass.

B) mass is conserved but energy is lost.

C) heat is taken in or absorbed.

D) energy is absorbed as mass is lost.

E) heat is liberated or released.

170.

Answer: E

171. In the reaction shown, how many moles of HCl are needed to react with 2.4 moles of Al?

2 Al + 6 HCl → 2 AlCl3 + 3 H2

A) 7.2 B) 6.4 C) 4.8 D) 0.8 E) 1.3

171.

Answer: A

172. Consider the following four liquids:

1. water: highly polar; H-bonding

2. hexanol: slightly polar; some H-bonding

3. chloroform: slightly polar; no H-bonding

4. octane: non-polar; no H-bonding

Which pair of liquids is immiscible?

A) water and octane

B) chloroform and octane

C) hexanol and chloroform

D) water and hexanol


172.

Answer: A

173. What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH?

A) 0.13 mL

B) 120 mL

C) 13 mL

D) 8.0 x 102 mL

E) 18 mL

173.

Answer: D

174. A molecule in which the central atom forms three single bonds and has one lone pair is said to

have a ________ shape.

A) trigonal pyramidal

B) tetrahedral

C) bent

D) planar

E) linear

174.

Answer: A

29



175. Elements constituting a period in the periodic table ________.

A) are called isotopes B) will always be in the same group

C) have consecutive atomic numbers D) have similar chemical properties

175.

Answer: C

176. What is the valence shell electron configuration of the ion formed from an atom of the halogen

family?

A) ns2np2 B) ns2np8 C) ns2 D) ns2np4 E) ns2np6

176.

Answer: E

177. The nucleus of an atom ________.

A) is negatively charged because of the presence of electrons

B) makes up more than 99.9% of the mass of the atom

C) contains all protons and electrons

D) is neutral since it contains only neutrons

177.

Answer: B

178. How many grams of glucose are needed to prepare 400. mL of a 2.0% (w/v) glucose solution?

A) 8.0 g B) 2.0 g C) 0.0050 g D) 800. g E) 200. g

178.

Answer: A

179. The formula for phosphorus pentafluoride is ________.

A) P5F B) (PF)5 C) PF5 D) P5F5 E) PF4

179.

Answer: C


A) SrBr2 strontium bromide

B) Zn(OH)2 zinc hydroxide

C) Ba3(PO4)2 barium phosphate

D) PCl3 phosphorous (III) chloride

180.

Answer: D

30



181. Which response includes all of the following that involve chemical changes and no physical changes?

I. burning charcoal

II. melting of gold

III. fermentation of grapes

IV. burning of natural gas

V. melting of ice

A) I, III, and IV B) I, II, and III C) II and V D) I and IV

181.

Answer: A

182. Which of the following is a chemical change?A) evaporation of gasoline B) cutting a copper wire into two piecesC) rusting of iron D) dissolving salt in water

182.

Answer: C

183. Mercury-202 has how many neutrons in its nucleus?

A) 102 B) 122 C) 22 D) 202

183.

Answer: B

184. 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) 5.00 x 102 mL

E) 1.00 x 104 mL

184.

Answer: B

185. What is the answer, with the correct number of significant figures, for this problem?

4.392 g + 102 .40 g + 2.51 g =

A) 109.302 g B) 109 g C) 109.30 g D) 109.3 g E) 110 g

185.

Answer: C

186. A red blood cell will undergo hemolysis in

A) 5% NaCl.

B) 5% glucose.

C) water.

D) 10% glucose.

E) 0.9% NaCl.

186.

Answer: C

31



187. What is the most likely charge on an ion formed by an element with a valence electron

configuration of ns2np4?

A) 2- B) 1- C) 4+ D) 2+ E) 6+

187.

Answer: A

188. How many unpaired electrons are there in a phosphorous atom?A) 2 B) 3 C) 1 D) 4

188.

Answer: B

189. Which transformation is sublimation?

A) gas → liquid

B) solid → liquid

C) solid → gas

D) liquid → solid

E) liquid → gas

189.

Answer: C

190. Which is a conclusion about the atom’s structure from Rutherford’s gold foil-alpha particleexperiments?

A) All alpha particles are affected the same way by the atoms in the gold foil.

B) The mass of an atom is distributed uniformly throughout the atom.

C) The positive charge of the atom is uniformly distributed throughout the atom.

D) The electrons occupy most of the total volume of an atom

190.

Answer: D

191. Which of the following terms does not involve the solid state?

A) melting B) sublimation C) freezing D) evaporation

191.

Answer: D

192. The typical volume of an aluminum can of soda is 355 mL. What is the equivalent volume in gallons?

A) 3.37 x 105 gal B) 5.75 gal C) 0.0938 gal D) 0.673 gal

192.

Answer: C

193. If a sample of carbon dioxide contains 3.8 moles of oxygen atoms, how many moles of carbon

dioxide are in the sample?

A) 3.8

B) 11.4

C) 1.9

D) 7.6


193.

Answer: C

32



194. A patient needs to receive 85 grams of glucose every 12 hours. What volume of a 5.0% (w/v)

glucose solution needs to be administered to the patient each 12 hours?

A) 1700 mL B) 17 mL C) 204 mL D) 6000 mL E) 60 mL

194.

Answer: A

195. Which of the following formulas in incorrect for a cobalt (III) compound?

A) CoCO3 B) Co2O3 C) CoPO4 D) CoCl3

195.

Answer: A

196. 4.34 quarts is equivalent to how many microliters?

A) 2.69 L B) 4.11 x 106 L C) 4.11 x 103 L D) 6.74 x 105 L

196.

Answer: B

197. In which of the following pairs of properties are both chemical properties?A) green in color, reacts violently with water B) has metallic luster, soluble in ammoniaC) has a high density, is very brittle D) flammable, reacts with acid

197.

Answer: D

198. Which ions are not spectator ions in the precipitation equation AgNO3 + NaCl → AgCl +

NaNO3?

A) Ag+ and NO3- B) Na+ and NO3- C) Ag+ and Cl- D) Na+ and Cl-

198.

Answer: C

199. In a Lewis dot structure the electrons which complete an octet but are not located/shared

between two atoms are referred to as

A) lone pairs.

B) bonding pairs.

C) filled shells.

D) delta minus electrons.

E) excess electrons.

199.

Answer: A

200. At maximum, an f subshell can hold _____ electrons, a d subshell can hold ____ electrons and a psubshell can hold ____ electrons.

A) 18, 8, 2 B) 2, 8, 18 C) 14, 10, 6 D) 2, 12, 21

200.

Answer: C

33



201. In this set of chemical reactions, which is a single displacement reaction?

A) CuSO4 (aq)+ BaCl2 (aq) → BaSO4 (s) + CuCl2 (aq)

B) K2SO4 (aq) + BaCl2 (aq) → BaSO4 (s) + 2KCl (aq)

C) AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)

D) Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2 (s) + 2NaNO3 (aq)

E) Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g)

201.

Answer: E

202. Which transformation is condensation?

A) liquid → solid

B) solid → liquid

C) gas → liquid

D) liquid → gas

E) solid → gas

202.

Answer: C

203. A red blood cell will undergo crenation in

A) 7% NaCl.

B) 0.5% NaCl.

C) water.

D) 3% glucose.

E) 5% glucose.

203.

Answer: A

204. The correct answer obtained by dividing 4.65 x 105 by 9.4 x 10−2 is ________.A) 2.02 x 10−7 B) 4.9 x 106 C) 4.95 x 106 D) 2.0 x 10−7

204.

Answer: B

205. Adding one proton to the nucleus of an atom:A) increases its atomic number by one unit but does not change its atomic massB) increases its atomic mass by one unit, but does not change its atomic numberC) does not change either its atomic number or its atomic massD) converts it to an atom of a different element

205.

Answer: D

206. The reaction 2AgNO3 (aq) + K2SO4 (aq) → 2KNO3 (aq) + Ag2SO4 (s) is an example of a(an)

________ reaction.

A) combustion

B) acid-base

C) oxidation-reduction

D) precipitation


206.

Answer: D

34



207. A solid substance is subjected to a number of tests and observations. Which of the following test resultswould not be classified as a physical property of the substance?A) Its density is 1.84 g/mL. B) It tastes sour.C) It reacts with base to form water. D) It is a white-colored solid.

207.

Answer: C

208. The numerical value for (5.6 x 104) ÷ (7.89 x 102) is equal to, with the proper number of significantfigures:A) 7.098 x 101 B) 71 C) 71.0 D) 70.976

208.

Answer: B

209. A polar covalent bond is found in which of these compounds?

A) F2 B) H2 C) NaCl D) N2 E) H2O

209.

Answer: E

210. Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield

750.0 mL of solution.

A) 0.130 M B) 2.30 M C) 1.50 M D) 0.768 M E) 1.18 M

210.

Answer: C

211. Acidic rain is caused by the reaction of sulfur oxides (produced when fossil fuels are burned)

with water, according to the reaction below. Classify the reaction shown below.

SO2 (g) + H2O (l) → H2SO3 (aq)

A) combination

B) combustion

C) decomposition

D) single displacement

E) double displacement

211.

Answer: A

212. Atomic emission spectra are due to electrons

A) being added to an atom.

B) in an atom dropping from one energy level to a lower one.

C) in an atom rising from one energy level to a higher one.

D) changing state from solid to liquid.

E) being removed from an atom.

212.

Answer: B

213. What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH?

A) 0.50 L B) 2.0 L C) 0.22 L D) 3.0 L E) 4.5 L

213.

Answer: B

35



214. When barium chloride is allowed to react with silver nitrate to give barium nitrate and silver

chloride, what are the coefficients for the balanced equation?

___BaCl2 (aq) + ___AgNO3 (aq) → ___AgCl (s) + ___ Ba(NO3)2 (aq)

A) 1, 2, 2, 1 B) 1, 1, 1, 1 C) 1, 1, 1, 2 D) 1, 1, 2, 1 E) 1, 2, 3, 1

214.

Answer: A

215. Which one of the following substances will float in gasoline, which has a density of 0.66 g/mL?

A) balsa wood (density = 0.16 g/mL)

B) mercury (density = 13.6 g/mL)

C) table salt (density = 2.16 g/mL)

D) aluminum (density = 2.70 g/mL)

E) sugar (density = 1.59 g/mL)

215.

Answer: A

216. Isotopes of a given element ________.

A) have the same atomic number but different chemical properties

B) have the same number of protons, but different mass numbers

C) have the same mass number but different chemical properties

D) have the same mass number but different numbers of protons

216.

Answer: B

217. According to dimensional analysis, which of the following is the correct set-up for the problem “Howmany milligrams are there in 67 kilograms?”

A) B)

C) D)

217.

Answer: C

218. All atoms of a given element may have different numbers of ________.

A) protons B) nucleons C) neutrons D) gamma rays

218.

Answer: C

36



219. What is the electron configuration for aluminum?

A) 1s2 2s2 2p6 3s2 3p6

B) 1s2 2s2 2p6 3s2 3p1

C) 1s2 2s2 2p6 3s2 3p8

D) 1s2 2s2 2p6 3s2 3p5

E) 1s2 2s2 2p6 3s2 3p3

219.

Answer: B

220. Automotive batteries generally are filled with sulfuric acid. If a battery has a volume of 1.86 L andcontains 3.42 x 103 grams of sulfuric acid, what is the density of sulfuric acid in g/mL?

A) 5.84 x 103 g/mL B) 1.84 g/mL C) 19.85 g/mL D) 5.43 x 10-4 g/mL

220.

Answer: B


configuration of ns1?

A) 1- B) 1+ C) 7+ D) 7- E) 0

221.

Answer: B

222. Give the correct name for FePO4.

A) iron phosphite

B) iron(III) phosphate

C) iron phosphate

D) phosphoiron

E) iron(II) phosphate

222.

Answer: B

223. The number 680 000 000 expressed correctly using scientific notation is

A) 680 x 106.

B) 0.68 x 106 .

C) 68 x 107 .

D) 6.8.

E) 6.8 x 108.

223.

Answer: E

224. A 15.5 gram sample of P2O5 contains how many grams of phosphorous?

A) 13.5

B) 3.38

C) 6.76

D) 1.69


224.

Answer: C

37



225. Which of the following statements is TRUE?

A) Vapor pressure increases with temperature.

B) Hydrogen bonds are stronger than covalent bonds.

C) Dispersion forces are generally stronger than dipole-dipole forces.

D) Intermolecular forces hold the atoms in molecules together.

E) None of the above are true.

225.

Answer: A

226. What is the mass number of a chromium isotope containing 28 neutrons?

A) 76 B) 24 C) 52 D) 28

226.

Answer: C

227. Which statement regarding balanced chemical equations is not true?

A) When no coefficient is written in front of a formula, the number ʺoneʺ is assumed.

B) Coefficients are used in front of formulas to balance the equation.

C) The number of each kind of atoms must be the same on each side.

D) Reactants are written to the left of the arrow.

E) Subscripts may be changed to make an equation simpler to balance.

227.

Answer: E

228. Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions

of Li2S and Cu(NO3)2 are mixed. (Make sure the equation is balanced.)

A) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq)

B) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s)

C) Li+ (aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq)

D) Li+ (aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq)

E) No reaction occurs.

228.

Answer: A

229. The correct name for CaCO3 is

A) Calcium monocarbonate B) Calcium carbon trioxide

C) Calcium carbonate D) Calcium monocarbon trioxide

229.

Answer: C

230. What is the molecular shape of a hydrogen sulfide molecule, H2S?

A) bent

B) linear

C) tetrahedral

D) trigonal pyramidal


230.

Answer: A

38



231. How many grams of carbon are present in 26.2 grams of H2CO3?

A) 11.60 g B) 16.8 g C) 5.07 g D) 47.3 g

231.

Answer: C

232. How many of the following compounds are insoluble in water?

KC2H3O2 CaSO4 SrS AlPO4

A) 1 B) 2 C) 0 D) 4 E) 3

232.

Answer: B

233. The formula for the compound chromium(II) nitrate is ________.

A) C2NO3 B) CrNO2 C) CrNO3 D) Cr(NO3)2 E) Cr2NO3

233.

Answer: D

234. How many moles of hydrogen (H2) are needed to react with 0.234 mol of oxygen (O2)

according to this equation?

2H2(g) + O2(g) → 2H2O(g)

A) 0.117 mol B) 0.936 mol C) 2.00 mol D) 0.468 mol E) 0.234 mol

234.

Answer: D

235. Raising the temperature of 10.0 g of water from 10.0 °C to 20.0 °C requires 418 J, while raising

the temperature of 10.0 g of aluminum from 10.0 °C to 20.0 °C requires 89.7 J. More joules are

required to heat the water because

A) ten grams of water occupies a larger volume than 10.0 g of aluminum.

B) 10.0 °C is closer to the melting point of water than to the melting point of aluminum.

C) water is a liquid and aluminum is a solid at 10.0 °C.

D) water has a greater potential energy than aluminum.

E) water has a larger specific heat than aluminum.

235.

Answer: E

236. Determine the number of moles of water produced when one mole of NH3 reacts according to

the balanced reaction shown.

4 NH3 + 5 O2 → 4 NO + 6 H2O

A) 1.25 B) 1.00 C) 1.33 D) 0.67 E) 1.50

236.

Answer: E

237. What is the mass of 36.0 mL of a liquid if its density is 2.70 g/mL?

A) 0.0750 g B) 0.748 g C) 13.3 g D) 97.2 g

237.

Answer: D

39



238. Give the approximate bond angle for a molecule with a tetrahedral shape.

A) 120° B) 180° C) 109.5° D) 105°

238.

Answer: C

239. Which of the following represent the Lewis structure for Ca2⁺?

A) B) C) D) E)

239.

Answer: B

240. The electron configuration shown below is for the element ________.

1s22s22p63s23p64s23d104p4

A) Se B) Br C) Ga D) As

240.

Answer: A

241. How many electrons are found in a Fe3+ ion?

A) 56 B) 29 C) 23 D) 26

241.

Answer: C

242. The number 3009.1 expressed in scientific notation to the correct number of significant figures becomes________.A) 3.0091 x 103 B) 3.0091 x 10−3 C) 3.01 x 103 D) 3.0091 x 104

242.

Answer: A

243. In the following list, which is the polar compound?

A) CCl4 B) N2 C) CO2 D) BF3 E) NH3

243.

Answer: E

244. Which one of the following compound names is paired with an incorrect formula?

A) ammonium carbonate - (NH4)2CO3 B) lithium acetate - LiC2H3O2

C) gold (I) sulfate - Au2SO4 D) potassium carbonate - KHCO3

244.

Answer: D

245. Of the elements: B, C, F, Li, and Na. The element with the largest atomic radius is

A) Li. B) C. C) B. D) Na. E) F.

245.

Answer: D

246. Which of the following type of matter/classification of matter pairs is incorrectly matched? type of matter classification of matter

A) pure gold elementB) concrete homogeneous mixtureC) saline solution homogeneous mixtureD) fruitcake heterogeneous mixture

246.

Answer: B

40



247. Density is an easy way to distinguish between gold (density: approx. 19 g/cm3), fool’s gold (density:approx. 4.5 g/cm3), and sand (density: approx. 2.5 g/cm3). If a large golden rock has a mass of 252 g anda volume of 56 cm3, which type of mineral is it?

A) sand B) fool’s gold C) gold D) none of these

247.

Answer: B

248. An element is a substance which ________.

A) can be broken down into simpler substances by chemical means.B) none of the above

C) cannot be broken down into simpler substances by physical or chemical means.

D) can be broken down into simpler substances by physical means.

248.

Answer: C

249. How many significant digits are in the volume measurement 4040.0 liters?

A) 2

B) 3

C) 4

D) 5


249.

Answer: D

250. What is the molecular shape of a silane molecule, SiH4?

A) bent

B) linear

C) tetrahedral



250.

Answer: C

251. Which of the following pairs of aqueous solutions will react when mixed?

A) Sr(C2H3O2)2 + Na2SO4

B) (NH4)2SO4 + LiCl

C) LiOH + Na2S

D) KNO3 + NaOH

E) None of the above solution pairs will produce a reaction.

251.

Answer: A

252. What is the systematic name of ICl3?

A) tri(iodine chloride)

B) iodine chloride

C) triiodine chloride

D) iodine trichloride

E) iodine(III) chloride

252.

Answer: D

41



253. In ionic compounds, ________ lose their valence electrons to form positively charged ________.

A) Testgen questions still do not copy to other applications.nonmetals, cations

B) metals, cations

C) nonmetals, anions

D) metals, polyatomic ions

E) metals, anions

253.

Answer: B

254. The correct name for the compound N2O4 is ________.

A) nitrooxide B) nitrogen oxide

C) dinitrogen tetroxide D) nitrogen (IV) oxide

254.

Answer: C

255. For the given reaction, how many moles of aluminum hydroxide are needed to react with 15.8

moles of sulfuric acid?

2Al(OH)3 (s) + 3H2SO4 (l) → Al2(SO4)3 (aq) + 6H2O (l)

A) 5.27 B) 10.5 C) 7.90 D) 15.8 E) 23.7

255.

Answer: B

256. Which of the following reactions below is a decomposition reaction?

A) 2 Cr (s) + 3 Cl2 (g) 2 CrCl3 (s)

B) 2 KClO3 (s) 2 KCl (s) + 3 O2 (g)

C) C7H8O2 (l) + 8 O2 (g) 7 CO2 (g) + 4 H2O (l)

D) 6 Li (s) + N2 (g) 2 Li3N (s)

256.

Answer: B

257. Silicon has ________ valence electrons.

A) 10 B) 4 C) 8 D) 2 E) 6

257.

Answer: B

For the following questions, consider the following equation.

2Mg(s) + O2(g) → 2MgO(s)

258. The number of moles of MgO produced when 0.200 mol of O2 reacts completely is ________.


258.

Answer: E

42



259. 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) 129 g B) 155 g C) 186 g D) 145 g E) 125 g

259.

Answer: C

260. Choose the bond below that is most polar.

A) C-N B) C-F C) C-C D) F-F E) C-O

260.

Answer: B

261. Which of the following is a property of both solids and liquids?

A) definite shape B) indefinite shape

C) definite volume D) indefinite volume

261.

Answer: C

262. The water molecule has a ________ molecular geometry because its central atom has ________

bonds and ________ lone pairs of electrons.

A) pyramidal; three; one

B) planar triangular; three; one

C) linear; two; two

D) bent; two; two

E) tetrahedral; four; zero

262.

Answer: D

263. 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) 0.100 M D) 6.67 M E) 0.200 M

263.

Answer: B

264. Which description best fits a solid?

A) definite volume; shape of container; no intermolecular attractions

B) definite shape and volume; strong intermolecular attractions

C) volume and shape of container; no intermolecular attractions

D) volume and shape of container; strong intermolecular attractions

E) definite volume; shape of container; moderate intermolecular attractions

264.

Answer: B

43



265. The following reaction takes place when an electric current is passed through water. It is an

example of a ________ reaction.

2H2O (l) electricity

2H2 (g) + O2 (g)

A) double displacement

B) single displacement

C) combustion

D) combination

E) decomposition

265.

Answer: E

266. Which description best fits a liquid?

A) definite shape and volume; strong intermolecular attractions

B) definite volume; shape of container; no intermolecular attractions

C) definite volume; shape of container; moderate intermolecular attractions

D) volume and shape of container; no intermolecular attractions

E) volume and shape of container; strong intermolecular attractions

266.

Answer: C

267. Which of the following is a physical process?

A) the rusting of iron B) the condensation of water vapor

C) the baking of a potato D) the explosion of nitroglycerin

267.

Answer: B

268. The correct answer for the calculation

where 126 and 135 are counted numbers and 1.364 and 0.8951 are measured numbers is ________.A) 1.422 B) 1.42 C) 1.4 D) 1.4220

268.

Answer: A

269. The smallest possible unit of a molecular compound is a(an)

A) atom.

B) cation.

C) molecule.

D) formula unit.

E) polyatomic ion.

269.

Answer: C

44



270. Atoms are neutral because ________.

A) all atoms contain neutrons

B) equal numbers of protons and neutrons are present

C) the atomic number equals the number of electrons

D) neutrons neutralize the () and (−) charges in the atom

270.

Answer: C

271. The Scientific Method

A) is just a theory.

B) is a framework for proving an argument you know to be true.

C) isnʹt used much in modern chemistry.

D) is based on continued observation and experiment.

E) is a strict set of rules and procedures that lead to inarguable fact.

271.

Answer: D

272. What is the mass of 9.44 × 1024 molecules of NO2?

A) 341 g B) 294 g C) 685 g D) 721 g E) 205 g

272.

Answer: D

273. A chemical bond formed when two atoms share two pairs of electrons is a ________ bond; it is

best described as ________.

A) single; covalent

B) double; ionic

C) triple; covalent

D) double; covalent

E) single; ionic

273.

Answer: D


configuration of ns2np5?

A) 2+ B) 5- C) 5+ D) 1+ E) 1-

274.

Answer: E

275. When the following reaction is balanced the coefficient in front of carbon dioxide is:

____ C5H12 + ____ O2 ____ CO2 + ____ H2O

A) 5 B) 6 C) 10 D) 7

275.

Answer: D

45



276. How many moles of carbon are in 3.5 moles of CaCO3?

A) 3.5

B) 100.09

C) 10.5

D) 7


276.

Answer: A

277. Which one of the following carries no electrical charge?

A) a neutron B) a proton C) an electron D) a cation

277.

Answer: A

278. 3.00 mol of NO2 has a mass of ________.

A) 46.0 g B) 30.0 g C) 45.0 g D) 138 g E) 90.0 g

278.

Answer: D

279. What is the systematic name for aqueous HI?

A) hydrogen iodide

B) hydroiodic acid

C) iodic acid

D) iodous acid


279.

Answer: B

280. Which statement best describes a sample of gas?

A) The volume and the shape of a gas are determined by its container.

B) A gas has a definite volume, but its shape is determined by its container.

C) The volume of a gas is determined by its container, but it has a definite shape.

D) A gas has a definite volume and a definite shape.

280.

Answer: A

281. What is the molecular shape of an ammonia molecule, NH3?

A) bent

B) linear

C) tetrahedral



281.

Answer: D

282. What volume of a solution with a density of 13.9 g/mL is needed to provide 155 grams of solution?

A) 106 mL B) 2150 mL C) 11.2 mL D) 0.185 mL

282.

Answer: C

46




A) PbO2 lead (IV) oxide B) Li2S lithium sulfide

C) CoO cobalt oxide D) Ag2CO3 silver (I) carbonate

283.

Answer: C

284. When 49.5 J of heat was transferred to 7.3 g iron at 22°C, the temperature of iron increases to

37°C. What is the specific heat of iron in J/g°C?

A) 4.5

B) 2.2

C) 24

D) 0.45


284.

Answer: D

285. The number 0.090804, when rounded off to 4 significant figures, would appear as ________.A) 0.0908 B) 0.091 C) 0.09080 D) 0.090

285.

Answer: C

286. The condensation of steam is an example of a ________.

A) sublimation B) change of state

C) extensive property D) chemical change

286.

Answer: B

287. A 50.0 mL sample of a 6.0 M solution of HCl is diluted to 200. mL. What is the new

concentration?

A) 2.10 M B) 1.50 M C) 6.0 M D) 2.00 M E) 24.0 M

287.

Answer: B

288. What is the final concentration if 100 mL of water is added to 25.0 mL of 6.0 M NaCl?

A) 6.0 M B) 24 M C) 1.2 M D) 30 M E) 1.5 M

288.

Answer: C

289. 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) 1.6 mg B) 0.59 mg C) 5.0 mg D) 19 mg E) 53 mg

289.

Answer: D

47



290. 2AgNO3(aq) + K2SO4(aq) → 2KNO3(aq) + Ag2SO4(s)

The net ionic equation for the balanced equation shown above is

A) 2 Ag+ + SO2-4 → Ag2SO4.

B) Ag+ + NO-3 → AgNO3.

C) K+ + NO-3 → KNO3.

D) H+ + OH- → H2O.

E) 2 K+ + SO2-4 → K2SO4.

290.

Answer: A

291. What is the strongest intermolecular force in a liquid containing molecules with nonpolar

bonds?

A) covalent bonds

B) hydrogen bonds

C) dipole forces

D) dispersion forces


291.

Answer: D

292. Which of the following measurements has three significant figures?

A) 0.510 m B) 5100 m C) 510 m D) 0.005 m E) 0.051 m

292.

Answer: A

293. On the electromagnetic spectrum, visible light is immediately between two other wavelengths.

Name them.

A) gamma ray and ultraviolet

B) radio and microwave

C) infrared and ultraviolet

D) microwave and x-ray

E) infrared and x-ray

293.

Answer: C

294. Why is water an extraordinary substance?

A) Water has strong hydrogen bonding.

B) Water has an exceptionally high specific heat capacity.

C) Water has a low molar mass, yet it is a liquid at room temperature.

D) Water is the main solvent within living organisms.

E) All of the above.

294.

Answer: E

48



295. Which of the following acids is named using the prefix hydro-?

A) HC2H3O2 B) HBr C) H2SO4 D) HNO2

295.

Answer: B

296. Calculate the mass (grams) of 0.750 moles of Al2(Cr2O7)3:

A) 486.0 g B) 526 g C) 702.0 g D) 270.0 g

296.

Answer: B

297. In the following reaction, how many grams of H2O are produced if 3.65 g of N2H4 react?

N2H4 + 3 O2 2NO2 + 2H2O

A) 4.10 g B) 1.47 g C) 11.2 g D) 10.5 g

297.

Answer: A

298. Place the following substances in order of decreasing strength of intermolecular forces.

H2O N2 CO

A) CO > H2O > N2

B) H2O > CO > N2

C) CO > N2 > H2O

D) N2 > H2O > CO

E) N2 > CO > H2O

298.

Answer: B

299. Of the elements: B, C, F, Li, and Na. The element with the smallest atomic radius is

A) Li. B) B. C) Na. D) F. E) C.

299.

Answer: D

300. In any balanced chemical equation, the number of each type of atom on both sides of the

equation is

A) doubled.

B) decreased by one.

C) dependent on the temperature.

D) increased by one.

E) the same.

300.

Answer: E

301. Water and vitamin C were added to a beaker. Calculate the mass of the beaker and its contents, andchoose the answer with the appropriate number of significant figures.

146.20 g beaker 23.1 g water 0.34 g vitamin C A) 169.64 g B) 169 g C) 169.6 g D) 160 g

301.

Answer: C

49



302. How many covalent bonds will a nitrogen atom normally make?

A) 1 B) 2 C) 3 D) 4 E) 6

302.

Answer: C

303. If the following ions Ca2+, NO3- , Na+ and SO42- are placed in a test tube, the precipitate

formed is ________.

A) CaSO4 B) Na2SO4 C) Ca(NO3)2 D) NaNO3

303.

Answer: A

304. When 0.0005760 is written in proper scientific notation with the correct number of significant figuresthe number is:A) 57.60 x 10-5 B) 5.760 x 104 C) 5.76 x 10-4 D) 5.760 x 10-4

304.

Answer: D

305. How many moles of water, H2O, are present in 75.0 g of H2O?

A) 4.17 moles

B) 4.41 moles

C) 75.0 moles

D) 7.50 moles

E) 1.35 x 103 moles

305.

Answer: A

306. What is the electron configuration for a magnesium ion, Mg2+?

A) 1s2 2s2 2p6 3s1

B) 1s2 2s2 2p6

C) 1s2 2s2 2p6 3s2 3p1

D) 1s2 2s2 2p6 3s2


306.

Answer: B

307. Three naturally occurring isotopes exist for the hypothetical element athenium. 2.50% of atheniumatoms have a relative mass of 26.0 amu, 75.0% of athenium atoms have a relative mass of 27.0 amu,and 22.5% of athenium atoms have a relative mass of 28.0 amu. What is the atomic mass of athenium?

A) 28.0 amu B) 27.2 amu C) 27.0 amu D) 26.8 amu

307.

Answer: B

308. The boiling point of a liquid is ________.

A) the temperature at which the vapor pressure of the liquid equals the pressure over the liquid

B) always 100*C or greater

C) the temperature at which liquid-vapor equilibrium is reached

D) the temperature at which the rate of condensation and evaporation are equal

308.

Answer: A

50



309. Which of the following is an oxidation-reduction reaction?

A) KOH + HNO3 → H2O + KNO3

B) Al2(SO4)3 + 6KOH → 2Al(OH)3 + 3K2SO4

C) N2 + O2 → 2NO

D) AgNO3 + NaCl → AgCl + NaNO3

E) CaCl2 + Na2SO4 → CaSO4 + 2NaCl

309.

Answer: C

310. Which of the following is a physical change?

A) Burning Coal

B) Smoking a cigarette

C) Synthesis of methane from carbon and hydrogen

D) Filtering muddy water

310.

Answer: D

311. How many unpaired electrons are there in a oxygen atom?

A) 3 B) 1 C) 2 D) 0

311.

Answer: C

312. For the given reaction, how many moles of pentane (C5H10) must have been burned if 97.50

moles of oxygen (O2) are consumed?

2C5H10 (l) + 15O2 (g) → 10CO2 (g) + 10H2O (g)

A) 97.50 B) 48.75 C) 195.0 D) 13.00 E) 6.500

312.

Answer: D

313. 4.00 mol of sodium has a mass of ________.

A) 44.0 g B) 4.60 g C) 23.0 g D) 128. g E) 92.0 g

313.

Answer: E

314. Red blood cells are placed in a solution and neither hemolysis nor crenation occurs. Therefore

the solution is

A) isotopic.

B) concentrated.

C) isotonic.

D) hypertonic.

E) hypotonic.

314.

Answer: C

51



315. How many protons and electrons are present in O2-?

A) 16 protons and 8 electrons.

B) 10 protons and 8 electrons.

C) 8 protons and 8 electrons.

D) 8 protons and 10 electrons.


315.

Answer: D

316. What is the percent by mass of oxygen in Na2SO4 ?

A) 45.0 B) 31.5 C) 39.5 D) 64.0 E) 9.88

316.

Answer: A

317. Place the following types of electromagnetic radiation in order of increasing wavelength.

ultraviolet light gamma rays radio waves

A) gamma rays < radio waves < ultraviolet light

B) ultraviolet light < gamma rays < radio waves

C) radio waves < ultraviolet light < gamma rays

D) radio waves < gamma rays < ultraviolet light

E) gamma rays < ultraviolet light < radio waves

317.

Answer: E

318. If object A weighs 24 grams and has a volume of 3 mL and object B weighs 14 g and has a volume of 7mL, ________.

A) A and B have equal densities B) B is half as dense as A

C) A is four times as dense as B D) B is more dense than A

318.

Answer: C

319. Which process is exothermic?

A) solid → liquid

B) solid → gas

C) liquid → gas

D) gas → liquid


319.

Answer: D

52



320. Which response contains all of the following that are physical changes and no chemical changes?

I. Candle wax melts.

II. Skin turns yellow when it comes in contact with nitric acid.

III. Milk curdles.

IV. Ice floats on water.

V. Windows fog when the temperature drops rapidly.

A) I, III, and V B) II and III C) II and IV D) I, IV, and V

320.

Answer: D

321. What element has the electron configuration 1s2 2s2 2p6 3s2 3p64s23d6 ?

A) Kr B) Fe C) Mn D) Ru E) Ni

321.

Answer: B

322. In liquid methanol,

CH3OH

which intermolecular forces are present?

A) Only dipole-dipole and ion-dipole forces are present.

B) Only hydrogen bonding forces are present.

C) Only dispersion and dipole-dipole forces are present.

D) Dispersion, hydrogen bonding and dipole-dipole forces are present.

322.

Answer: D

323. What is the electron configuration using core notation for P3-?

A) [Ne] 3s2 3p3

B) [Ar]

C) [Ne] 3s2

D) [Ne] 3p6


323.

Answer: B

324. When Geiger and Marsden conducted experiments, suggested by Rutherford, on the

bombardment of thin gold foil with alpha particles, they discovered that

A) all alpha particles were deflected, and none passed through.

B) all alpha particles were deflected, and none passed through.

C) the alpha particles were transmuted into electrons and protons.

D) most alpha particles passed through but, unexpectedly, some deflected.

E) most alpha particles were trapped in the gold.

324.

Answer: D

53



325. Which of the following statements about compounds and mixtures is correct?

A) Mixtures retain the properties of their individual components.

B) Since two or more simpler substances can be obtained from a compound, all compounds aremixtures.

C) Compounds always have properties that are identical to those of the elements used to producethem.

D) Compounds cannot be broken down into simpler substances by chemical means.

325.

Answer: A

326. Which is the correct formula for the ionic compound containing iron(III) ions and oxide ions?

A) FeO2 B) Fe2O2 C) Fe3O2 D) Fe2O3 E) FeO

326.

Answer: D

327. A neutral atom contains 12 neutrons and 14 electrons. The mass number and the number of protons forthis atom are, respectively, ________.

A) 26 and 14 B) 40 and 14 C) 26 and 12 D) 14 and 26

327.

Answer: A

328. Which of the following elements would exhibit chemical properties most similar to nitrogen?

A) Ne B) Ge C) Sb D) Zn

328.

Answer: C

329. The shape of the carbon dioxide (CO2 ) is

A) linear.

B) tetrahedral.

C) trigonal planar.

D) pyramidal.

E) bent.

329.

Answer: A

330. How many N2O4 molecules are contained in 76.3 g N2O4?

A) 1.38 × 1024 N2O4 molecules

B) 4.59 × 1025 N2O4 molecules

C) 7.26 × 1023 N2O4 molecules

D) 4.99 × 1023 N2O4 molecules

E) 5.54 × 1025 N2O4 molecules

330.

Answer: D

331. How many grams of Fe2O3 are there in 0.500 mol of Fe2O3?

A) 160. g B) 63.8 g C) 51.9 g D) 79.9 g E) 35.9 g

331.

Answer: D

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332. The correct electron dot symbol for a potassium atom is ________.

A) . P . B) . P C) . K . D) K : E) . K

332.

Answer: E

333. What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution?

A) 10. M B) 1.0 M C) 2.5 M D) 5.0 M E) 2.0 M

333.

Answer: C

334. According to the following balanced reaction, how many moles of HNO3 are formed from 8.44

moles of NO2 if there is plenty of water present?

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

A) 25.3 moles HNO3

B) 2.81 moles HNO3

C) 8.44 moles HNO3

D) 1.83 moles HNO3

E) 5.63 moles HNO3

334.

Answer: E

335. If ʺAʺ contains 2% NaCl and is separated by a semipermeable membrane from ʺBʺ which

contains 10% NaCl, which event will occur?

A) NaCl will flow from ʺAʺ to ʺBʺ.

B) NaCl will flow from ʺBʺ to ʺAʺ.

C) Water will flow from ʺAʺ to ʺBʺ.

D) Water will flow from ʺBʺ to ʺAʺ.


335.

Answer: C

336. Which of the following is an example of a heterogeneous mixture?

A) air B) vodka C) sugar water D) blood

336.

Answer: D

337. What is the concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution?

A) 0.160 M B) 0.250 M C) 0.125 M D) 0.0625 M E) 0.375 M

337.

Answer: B

338. What are the number of protons, neutrons, and electrons in

A) 9 protons, 10 neutrons, and 9 electrons B) 19 protons, 19 neutrons, and 19 electrons

C) 9 protons, 9 neutrons, and 19 electrons D) 9 protons, 9 neutrons, and 10 electrons

338.

Answer: A

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339. A nonvolatile liquid would ________.

A) have a high vapor pressure at room temperature

B) be a very “explosive” substance

C) have strong intermolecular forces between molecules

D) have weak intermolecular forces between molecules

339.

Answer: C

340. Which of the following formulas is paired with an incorrect name?

A) Ca3(PO4)2 - calcium phosphate B) SnCl2 - tin(II) chloride

C) CuCO3 - copper carbonate D) CrCl3 - chromium(III) chloride

340.

Answer: C

For the following questions, consider the following balanced equation.

Mg3N2(s) + 6H2O(l) → 3Mg(OH)2(s) + 2NH3(g)

341. When 2.50 mol of Mg3N2 are allowed to react, how many moles of H2O also react?


341.

Answer: A

342. Which of the following elements would be expected to have the least metallic character?A) Ba B) V C) F D) Ga

342.

Answer: C

343. Give the approximate bond angle for a molecule with a trigonal planar shape.

A) 180° B) 105° C) 120° D) 109.5°

343.

Answer: C

344. How many double bonds are there in a molecule of SF2?

A) 0 B) 1 C) 2 D) 3 E) 4

344.

Answer: A

345. Given the following: 41

19X,

39

19X,

41

20X, and

39

18X. Which are isotopes of each other?

A)41

19X,

39

19X,

41

20X, and

39

18X are isotopes of each other.

B)41

19X and

41

20X are isotopes of each other; and

39

19X and

39


C) 41

19X and

39


D) None are isotopes of each other.

345.

Answer: C

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346. Indicate which set of coefficients balances the equation

________NH3 + ________O2 ________NO + ________H2O

A) 2, 6, 3, 2 B) 6, 5, 4, 4 C) 3, 2, 1, 3 D) 4, 5, 4, 6

346.

Answer: D

347. Which of the following occur as the energy of a photon increases?

A) the wavelength increases

B) the speed increases.

C) the wavelength decreases.

D) the frequency decreases.

E) None of the above occur as the energy of a photon increases.

347.

Answer: C

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