Advanced Placement Chemistry

1989 Multiple Choice Questions

Notes

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Use these answers for questions 1 - 3.

(A) O
(B) La
(C) Rb
(D) Mg
(E) N

1. What is the most electronegative element of the above?

2. Which element exhibits the greatest number of different oxidation states?

3. Which of the elements above has the smallest ionic radius for its most commonly found ion?

Use these answers for questions 4 - 7.

(A) 1s² 2s²2p⁵ 3s²3p⁵
(B) 1s² 2s²2p⁶ 3s²3p⁶
(C) 1s² 2s²2p⁶2d¹⁰ 3s²3p⁶
(D) 1s² 2s²2p⁶ 3s²3p⁶3d⁵
(E) 1s² 2s²2p⁶ 3s²3p⁶3d³ 4s²

4. An impossible electronic configuration

5. The ground-state configuration for the atoms of a transition element

6. The ground-state configuration of a negative ion of a halogen

7. The ground-state configuration of a common ion of an alkaline earth element

Use these answers for questions 8 - 10.

(A) a solution with a pH less than 7 that is not a buffer solution
(B) a buffer solution with a pH between 4 and 7
(C) a buffer solution with a pH between 7 and 10
(D) a solution with a pH greater than 7 that is not a buffer solution
(E) a solution with a pH of 7

Ionization Constants

CH₃COOH = 1.8 x 10¯⁵
NH₃ = 1.8 x 10¯⁵
H₂CO₃; K₁ = 4 x 10¯⁷
H₂CO₃; K₂ = 4 x 10¯¹¹

8. A solution prepared to be initially 1 M in NaCl and 1 M in HCl.

9. A solution prepared to be initially 1 M in Na₂CO₃ and 1 M in CH₃COONa

10. A solution prepared to be initially 0.5 M in CH₃COOH and 1 M in CH₃COONa

Use these answers for questions 11 - 14.

(A) hydrogen bonding
(B) hybridization
(C) ionic bonding
(D) resonance
(E) van der Waals forces (London dispersion forces)

11. Is used to explain why iodine molecules are held together in the solid state

12. Is used to explain why the boiling point of HF is greater than the boiling point of HBr

13. Is used to explain the fact that the four bonds in methane are equivalent

14. Is used to explain the fact that the carbon-to-carbon bonds in benzene, C₆H₆, are identical

15. The weight of H₂SO₄ (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar solution is

(A) 3.10 grams
(B) 12.0 grams
(C) 29.4 grams
(D) 294 grams
(E) 300. grams

16. A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.50 mole of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?

(A) 0.13 atm
(B) 0.27 atm
(C) 0.63 atm
(D) 0.90 atm
(E) 6.3 atm

17. The Lewis dot structure of which of the following molecules shows only one unshared pair of valence electron?

(A) Cl₂
(B) N₂
(C) NH₃
(D) CCl₄
(E) H₂O₂

18. For the types of radiation given, which of the following is the correct order of increasing ability to penetrate a piece of lead?

(A) Alpha particles < gamma rays < beta particles
(B) Alpha particles < beta particles < gamma rays
(C) Beta particles < alpha particles < gamma rays
(D) Beta particles < gamma rays < alpha particles
(E) Gamma rays < alpha particles < beta particles

19. In the titration of a weak acid of unknown concentration with a standard solution of a strong base, a pH meter was used to follow the progress of the titration. Which of the following is true for this experiment?

(A) The pH is 7 at the equivalence point.
(B) The pH at the equivalence point depends on the indicator used.
(C) The graph of pH versus volume of base added rises gradually at first and then much more rapidly.
(D) The graph of pH versus volume of base added shows no sharp rise.
(E) The [H⁺] at the equivalence point equals the ionization constant of the acid.

20. 6 I¯ + 2 MnO₄¯ + 4 H₂O(l) ---> 3 I₂(s) + 2 MnO₂(s) + OH¯

Which of the following statements regarding the reaction represented by the equation above is correct?

(A) Iodide ion is oxidized by hydroxide ion.
(B) MnO₄¯ is oxidized by iodide ion.
(C) The oxidation number of manganese changes from +7 to +2.
(D) The oxidation number of manganese remains the same.
(E) The oxidation number of iodine changes from -1 to 0.

21. Which of the following is true at the triple point of a pure substance?

(A) The vapor pressure of the solid phase always equal the vapor pressure of the liquid phase.
(B) The temperature is always 0.01 K lower that the normal melting point.
(C) The liquid and gas phases of the substance always have the same density and are therefore indistinguishable.
(D) the solid phase always melts if the pressure increases at constant temperature.
(E) The liquid phase always vaporizes if the pressure increases at constant temperature.

22. __ Cr₂O₇²¯ + __ e¯ + __ H⁺ ---> __ Cr³⁺ + __ H₂O(l) When the equation for the half reaction above is balanced with the lowest whole-number coefficients, the coefficient for H₂O is

(A) 2
(B) 4
(C) 6
(D) 7
(E) 14

23. How many grams of calcium nitrate, Ca(NO₃)₂, contains 24 grams of oxygen atoms?

(A) 164 grams
(B) 96 grams
(C) 62 grams
(D) 50. grams
(E) 41 grams

24. The mass of element Q found in 1.00 mole of each of four different compounds is 38.0 grams, 57.0 grams, 76.0 grams, and 114 grams, respectively. A possible atomic weight of Q is

(A) 12.7
(B) 19.0
(C) 27.5
(D) 38.0
(E) 57.0

25. The simplest formula for an oxide of nitrogen that is 36.8 percent nitrogen by weight is

(A) N₂O
(B) NO
(C) NO₂
(D) N₂O₃
(E) N₂O₅

26. How many milliliters of 11.6-molar HCl must be diluted to obtain 1.0 liter of 3.0-molar HCl?

(A) 3.9 mL
(B) 35 mL
(C) 260 mL
(D) 1,000 mL
(E) 3,900 mL

27.

I. Difference in temperature between freezing point of solvent and freezing point of solvent and freezing point of solution
II. Molal freezing point depression constant, K_f, for solvent

In addition to the information above, which of the following gives the minimum data required to determine the molecular mass of a nonionic substance by the freezing point depression technique?

(A) No further information is necessary.
(B) Mass of solute
(C) Mass of solute and mass of solvent
(D) Mass of solute and volume of solvent
(E) Mass of solute, mass of solvent, and vapor pressure of solvent

28. Which of the following is probably true for a solid solute with a highly endothermic heat of solution when dissolved in water?

(A) The solid has a low lattice energy.
(B) As the solute dissolves, the temperature of the solution increases.
(C) The resulting solution is ideal.
(D) The solid is more soluble at higher temperatures.
(E) the solid has a high energy of hydration.

29. In which of the following systems would the number of moles of the substances present at equilibrium NOT be shifted by a change in the volume of the system at constant temperature?

(A) CO(g) + NO(g) <===> CO₂(g) + 1/2 N₂(g)
(B) N₂(g) + 3 H₂(g) <===> 2 NH₃(g)
(C) N₂(g) + 2 O₂(g) <===> 2 NO₂(g)
(D) N₂O₄(g) <===> 2 NO₂(g)
(E) NO(g) + O₃(g) <===> NO₂(g) + O₂(g)

30. Hydrogen gas is collected over water at 24 °C. The total pressure of the sample is 755 millimeters of mercury. At 24 °C, the vapor pressure of water is 22 millimeters of mercury. What is the partial pressure of the hydrogen gas?

(A) 22 mm Hg
(B) 733 mm Hg
(C) 755 mm Hg
(D) 760 mm Hg
(E) 777 mm Hg

31. The structural isomers C₂H₅OH and CH₃OCH₃ would be expected to have the same values for which of the following? (Assume ideal behavior.)

(A) Gaseous densities at the same temperature and pressure
(B) Vapor pressures at the same temperature
(C) Boiling points
(D) Melting points
(E) Heats of vaporization

32. A 2.00-liter sample of nitrogen gas at 27 °C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged, the final temperature of the gas is

(A) 68 °C
(B) 120 °C
(C) 477 °C
(D) 677 °C
(E) 950. °C

33. Which of the following conclusions can be drawn from J. J. Thomson's cathode ray experiments?

(A) Atoms contain electrons.
(B) Practically all the mass of an atom is contained in its nucleus.
(C) Atoms contain protons, neutrons, and electrons.
(D) Atoms have a positively charged nucleus surrounded by an electron cloud.
(E) No two electrons in one atom can have the same four quantum numbers.

34. All of the following species can function as Brönsted-Lowry bases in solution EXCEPT

(A) H₂O
(B) NH₃
(C) S²¯
(D) NH₄⁺
(E) HCO₃¯

35. When phenolphthalein is used as the indicator in a titration of an HCl solution with a solution of NaOH, the indicator undergoes a color change from clear to red at the end point of the titration. This color change occurs abruptly because

(A) phenolphthalein is a very strong acid that is capable of rapid dissociation
(B) the solution being titrated undergoes a large pH change near the end point of the titration
(C) phenolphthalein undergoes an irreversible reaction in basic solution
(D) OH¯ acts as a catalyst for the decomposition of phenolphthalein
(E) phenolphehalein is involved in the rate-determining step of the reaction between H₃O⁺ and OH¯

36. Appropriate laboratory procedures include which of the following?

I. Rinsing a buret with distilled water just before filling it with the titrant for the first titration
II. Lubricating glass tubing before inserting it into a stopper
III. For accurate results, waiting until warm or hot objects have reached room temperature before weighing them

(A) II only
(B) I and II only
(C) I and III only
(D) II and III only
(E) I, II, and III

37. __ CH₃CH₂COOH(l) + __ O₂(g) ---> __ CO₂(g) + __ H₂O(l)

How many moles of O₂ are required to oxidize 1 mole of CH₃CH₂COOH according to the reaction represented above?

(A) 2 moles
(B) 5/2 moles
(C) 3 moles
(D) 7/2 moles
(E) 9/2 moles

38. 98-Cf-251 ---> 2n + 54-Xe-131 + __

What is the missing product in the nuclear reaction represented above?

(A) 42-Mo-118
(B) 44-Ru-118
(C) 42-Mo-120
(D) 44-Ru-120
(E) 46-Pd-122

39. When a hydrate of Na₂CO₃ is heated until all the water is removed, it loses 54.3 percent of its mass. The formula of the hydrate is

(A) Na₂CO₃ ^. 10 H₂O
(B) Na₂CO₃ ^. 7 H₂O
(C) Na₂CO₃ ^. 5 H₂O
(D) Na₂CO₃ ^. 3 H₂O
(E) Na₂CO₃ ^. H₂O

40. 2 K + 2 H₂O ---> 2 K⁺ + 2 OH¯ + H₂

When 0.400 mole of potassium reacts with excess water at standard temperature and pressure as shown in the equation above, the volume of hydrogen gas produced is

(A) 1.12 liters
(B) 2.24 liters
(C) 3.36 liters
(D) 4.48 liters
(E) 6.72 liters

41. Which of the following reactions has the largest positive value of DS per mole of Cl₂

(A) H₂(g) + Cl₂(g) ---> 2 HCl(g)
(B) Cl₂(g) + 1/2 O₂(g) ---> Cl₂O(g)
(C) Mg(s) + Cl₂(g) ---> MgCl₂(s)
(D) 2 NH₄Cl(s) ---> N₂(g) + 4 H₂(g) + Cl₂(g)
(E) Cl₂(g) ---> 2 Cl(g)

42. The SbCl₅ molecule has trigonal bipyramid structure. Therefore, the hybridization of Sb orbitals should be

(A) sp²
(B) sp³
(C) dsp²
(D) dsp³
(E) d²sp³

43. Which of the following does NOT behave as an electrolyte when it is dissolved in water?

(A) CH₃OH
(B) K₂CO₃
(C) NH₄Br
(D) HI
(E) Sodium acetate, CH₃COONa

44. The metal calcium reacts with molecular hydrogen to form a compound. All of the following statements concerning this compound are true EXCEPT:

(A) Its formula is CaH₂.
(B) It is ionic.
(C) It is solid at room temperatur(E)
(D) When added to water, it reacts to produce H₂ gas.
(E) When added to water, it forms an acidic solution.

45. A measured mass of an unreactive metal was dropped into a small graduated cylinder half filled with water. The following measurements were made.

Mass of metal = 19.611 grams
Volume of water before addition of metal = 12.4 milliliters
Volume of water after addition of metal = 14.9 milliliters

The density of the metal should be reported as

(A) 7.8444 grams per mL
(B) 7.844 grams per mL
(C) 7.84 grams per mL
(D) 7.8 grams per mL
(E) 8 grams per mL

46. As the number of oxygen atoms increases in any series of oxygen acids, such as HXO, HXO₂, HXO₃, ...., which of the following is generally true?

(A) The acid strength varies unpredictably.
(B) The acid strength decreases only if X is a nonmetal.
(C) The acid strength decreases only if X is a metal.
(D) The acid strength decreases whether X is a nonmetal or a metal.
(E) The acid strength increases.

47. CCl₄, CO₂, PCl₃, PCl₅, SF₆ Which of the following does not describe any of the molecules above?

(A) Linear
(B) Octahedral
(C) Square planar
(D) Tetrahedral
(E) Trigonal pyramidal

48.Which of the following is a graph that describes the pathway of reaction that is endothermic and has high activation energy?

(A)		(B)
(C)		(D)
(E)

Use the following diagram for questions 49-51.

49. The normal boiling point of the substanced represented by the phase diagram above is

(A) -15 °C
(B) -10 °C
(C) 140 °C
(D) greater than 140 °C
(E) not determinable from the diagram

50. The phase diagram above provides sufficient information for determining the

(A) entropy change on vaporization
(B) conditions necessary for sublimation
(C) deviations from ideal gas behavior of the gas phase
(D) latent heat of vaporization
(E) latent heat of fusion

51. For the substance represented in the diagram, which of the phases is most dense and which is least dense at - 15 °C.

52. The test for the presence of Ag⁺ in an unknown solution involves the treatment of the solver-ammonia complex with dilute hydrochloric acid. The appearance of a white precipitate at this point indicates the presence of silver ion in the original sample. The net ionic equation that represents this test is

(A) Ag(NH₄)₄⁺ + 4 H⁺ <===> Ag(s) + 4 NH₄⁺
(B) Ag(NH₄)₄⁺ + Cl¯ <===> AgCl(s) + 4 NH₄⁺
(C) Ag(NH₃)₄⁺ + 4 HCl <===> AgCl(s) + 4 NH₄⁺ + 3 Cl#175;
(D) Ag(NH₃)₄⁺ + Cl¯ <===> Ag(NH₃)₂Cl(s)
(E) Ag(NH₃)₄⁺ + 2 H⁺ + Cl#175; <===> AgCl(s) + 2 NH₄⁺

53. Which of the following must be true for a reaction that proceeds spontaneously from initial standard state conditions?

(A) DG° > 0 and K_eq > 1
(B) DG° > 0 and K_eq < 1
(C) DG° < 0 and K_eq > 1
(D) DG° < 0 and K_eq > 1
(E) DG° = 0 and K_eq = 1

54. Which of the following is the correct equilibrium expression for the hydrolysis of CO₃²¯ ?

(A) K = [HCO₃¯ ] / ( [CO₃²¯ ] [H₃O⁺] )
(B) K = ( [HCO₃¯] [OH¯] ) / [CO₃²¯]
(C) K = ( [CO₃²¯ ] [OH¯] ) / [HCO₃¯]
(D) K = [CO₃²¯ ] / ( [CO₂] [OH¯]² )
(E) K = ( [CO₃²¯ ] [H₃O⁺] ) / [HCO₃¯]

55.

H₂PO₄¯ + HBO₃²¯ <===> HPO₄²¯ + H₂BO₃¯

The equilibrium constant for the reaction represented by the equation above is greater than 1.0. Which of the following gives the correct relative strengths of the acids and bases in the reaction?

56. A 0.20-molar solution of a weak monoprotic acid, HA, has a pH of 3.00. The ionization constant of this acid is

(A) 5.0 x 10¯⁷
(B) 2.0 x 10¯⁷
(C) 5.0 x 10¯⁶
(D) 5.0 x 10¯³
(E) 2.0 x 10¯³

57. rate = k[X]

For the reaction whose rate law is given above, a plot of which of the following is a straight line?

(A) [X] versus time
(B) log [X] versus time
(C) 1/[X] versus time
(D) [X] versus 1/time
(E) log [X] versus 1/time

58.

(CH₃)₃CCl(aq) + OH¯ ---> (CH₃)₃COH(aq) + Cl¯

For the reaction represented above, the experimental rate law is given as follows.

Rate = k [(CH₃)₃CCl]

If some solid sodium solid hydroxide is added to a solution that is 0.010-molar in (CH₃)₃CCl and 0.10-molar in NaOH, which of the following is true? (Assume the temperature and volume remain constant.)

(A) Both the reaction rate and k increase.
(B) Both the reaction rate and k decrease.
(C) Both the reaction rate and k remain the same.
(D) The reaction rate increases but k remains the same.
(E) The reaction rate decreases but k remains the same.

59. Which of the following compounds is ionic and contains both sigma and pi covalent bonds?

(A) Fe(OH)₃
(B) HClO
(C) H₂S
(D) NO₂
(E) NaCN

60.

The standard reduction potentials for two half reactions are given above. The Nernst equation for a galvanic cell at 25° C in which Fe(s) reduces Ni²⁺ is the following.

E = E° - 0.059/2 log [Fe²⁺] / [Ni²⁺]

What is the equilibrium constant for the reaction below?

Fe(s) + Ni²⁺ ---> Fe²⁺ + Ni(s)

(A) 1.9 x 10¯²³
(B) 7.6 x 10¯⁸
(C) 3.6 x 10⁺³
(D) 1.3 x 10⁺⁷
(E) 5.2 x 10⁺²²

61. When acidified K₂Cr₂O₇ solution is added to Na₂S solution, green Cr³⁺ ions and free S are formed. When acidified K₂Cr₂O₇ solution is added to NaCl, no change occurs. Of the substances involved in these reactions, which is the best reducing agent?

(A) K₂Cr₂O₇
(B) Na₂S
(C) Cr³⁺
(D) S
(E) NaCl

62. As the temperature is raised from 20 ° C to 40 ° C, the average kinetic energy of neon atoms changes by a factor of

(A) 1/2
(B) [square root of](313/293)
(C) 313/293
(D) 2
(E) 4

63. Which of the following characteristics is common to elemental sulfur, chlorine, nitrogen, and carbon?

(A) They are gaseous elements at room temperature.
(B) They have oxides that are acid anhydrides.
(C) They have perceptible color at room temperature.
(D) They form ionic oxides.
(E) They react readily with hydrogen at room temperature.

64. A solution is known to contain an inorganic salt of one of the following elements. The solution is colorless. The solution contains a salt of

(A) Cu
(B) Mn
(C) Fe
(D) Ni
(E) Zn

65. The solubility of CuI is 2 x 10¯⁶ molar. What is the solubility product constant, K_sp, for CuI?

(A) 1.4 x 10¯³
(B) 2 x 10¯⁶
(C) 4 x 10¯¹²
(D) 2 x 10¯¹²
(E) 8 x 10¯¹⁸

66. MnS(s) + 2 H⁺ <===> Mn²⁺ + H₂S(g)

At 25 °C the solubility product constant, K_sp, for MnS in 5 x 10¯¹⁵ and the acid dissociation constants K₁ and K₂ for H₂S are 1 x 10¯⁷ and 1 x 10¯¹³, respectively. What is the equilibrium constant for the reaction represented by the equation above at 25 °C?

(A) 1 x 10¯¹³ / 5 x 10¯¹⁵
(B) 5 x 10¯¹⁵ / 1 x 10¯⁷
(C) 1 x 10¯⁷ / 5 x 10¯²⁰
(D) 5 x 10¯¹⁵ / 1 x 10¯²⁰
(E) 1 x 10¯²⁰ / 5 x 10¯¹⁵

67. BrO₃¯ + 5 Br¯ + 6 H⁺ <===> 3 Br₂ + 3 H₂O

If 25.0 milliliters of 0.200-molar BrO₃¯ is mixed with 30.0 milliliters of 0.450-molar Br¯ solution that contains a large excess of H⁺, the amount of Br₂ formed, according to the equation above, is

(A) 5.00 x 10¯³ mole
(B) 8.10 x 10¯³ mole
(C) 1.35 x 10¯² mole
(D) 1.50 x 10¯² mole
(E) 1.62 x 10¯² mole

68. The specific rate constant k for radioactive element X is 0.023 min -1. What weight of X wsa originally present in a sample if 40. grams is left after 60. minutes?

(A) 10. grams
(B) 20. grams
(C) 80. grams
(D) 120 grams
(E) 160 grams

69. A white solid is observed to be insoluble in water, insoluble in excess ammonia solution, and soluble in dilute HCl. Which of the following compounds could the solid be?

(A) CaCO₃
(B) BaSO₄
(C) Pb(NO₃)₂
(D) AgCl
(E) Zn(OH)₂

70. H₂O(s) ---> H₂O(l) When ice melts at its normal melting point, 273.16 K and 1 atmosphere, which of the following is true for the process shown above?

(A) DH < 0, DS > 0, DV > 0
(B) DH < 0, DS < 0, DV > 0
(C) DH > 0, DS < 0, DV < 0
(D) DH > 0, DS > 0, DV > 0
(E) DH > 0, DS > 0, DV < 0

71. A solution of toluene (molecular weight 92.1) in benzene (molecular weight 78.1) is prepared. The mole fraction of toluene in the solution is 0.100. What is the molality of the solution?

(A) 0.100 m
(B) 0.703 m
(C) 0.921 m
(D) 1.28 m
(E) 1.42 m

72. How many moles of solid Ba(NO₃)₂ should be added to 300. milliliters of 0.20-molar Fe(NO₃)₃ to increase the concentration of the NO₃¯ ion to 1.0-molar? (Assume that the volume of the solution remains constant.)

(A) 0.060 mole
(B) 0.12 mole
(C) 0.24 mole
(D) 0.30 mole
(E) 0.40 mole

73. Adding water to some chemicals can be dangerous because large amounts of heat are liberated. Which of the following does NOT liberate heat when water is added to it?

(A) KNO₃
(B) NaOH
(C) CaO
(D) H₂SO₄
(E) Na

74. Equal volumes of 0.10-molar H₃PO₄ and 0.20-molar KOH are mixed. After equilibrium is established, the type of ion an solution in largest concentration, other than the K⁺ ion, is

(A) H₂PO₄¯
(B) HPO₄²¯
(C) PO₄³¯
(D) OH¯
(E) H₃O⁺

75. If a copper sample containing some zinc impurity is to be purified by electrolysis, the anode and the cathode must be which of the following?

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