AP CHEMISTRY Test Booklet

Units 1-6 MCQ revision

1. A 2 L container will hold about 4 g of which of the following gases at 0°C and 1 atm?
(A) SO2
(B) N2
(C) CO2
(D) C4H8
(E) NH3

2. Which of the following best helps to account for the fact that the F- ion is smaller than the O2- ion?
(A) F- has a larger nuclear mass than O2- has.
(B) F- has a larger nuclear charge than O2- has.
(C) F- has more electrons than O2- has.
(D) F- is more electronegative than O2- is.
(E) F- is more polarizable than O2- is.

3. When the actual gas volume is greater than the volume predicted by the ideal gas law, the explanation lies in the
fact that the ideal gas law does NOT include a factor for molecular.
(A) volume
(B) mass
(C) velocity
(D) attractions
(E) shape

4. At standard temperature and pressure, a 0.50 mol sample of H2 gas and a separate 1.0 mol sample of O2 gas have
the same
(A) average molecular kinetic energy
(B) average molecular speed
(C) volume
(D) effusion rate
(E) density

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5.

A Lewis diagram for the molecule is shown above. In the actual molecule, the bond angles
are closest to
(A)
(B)
(C)
(D)

6.
3 C2H2(g) → C6H6(g)

What is the standard enthalphy change ΔHo, for the reaction represented above?

(ΔHof of C2H2(g) is 230 kJ mol-1;

(ΔHof of C6H6(g) is 83 kJ mol-1;)

(A) -607 kJ
(B) -147 kJ
(C) -19 kJ
(D) +19 kJ
(E) +773 kJ

7. Which of the following describes the changes in forces of attraction that occur as H2O changes phase from a liquid
to a vapor?
(A) H – O bonds break as H – H and O – O bonds form.
(B) Hydrogen bonds between H2O molecules are broken.
(C) Covalent bonds between H2O molecules are broken.
(D) Ionic bonds between H+ ions and OH- ions are broken.
(E) Covalent bonds between H+ ions and H2O molecules become more effective.

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8. If 200. mL of 0.60 M MgCl2(aq) is added to 400. mL of distilled water, what is the concentration of Mg2+(aq) in
the resulting solution? (Assume volumes are additive).
(A) 0.20 M
(B) 0.30 M
(C) 0.40 M
(D) 0.60 M
(E) 1.2 M

9. When 70. milliliter of 3.0-molar Na2CO3 is added to 30. milliliters of 1.0-molar NaHCO3 the resulting
concentration of Na+ is
(A) 2.0 M
(B) 2.4 M
(C) 4.0 M
(D) 4.5 M
(E) 7.0 M

10. A 40.0 mL sample of 0.25 M KOH is added to 60.0 mL of 0.15 M Ba(OH)2. What is the molar concentration of
OH-(aq) in the resulting solution? (Assume that the volumes are additive.)
(A) 0.10 M
(B) 0.19 M
(C) 0.28 M
(D) 0.40 M
(E) 0.55 M

11. Under which of the following conditions of temperature and pressure would 1.0 mol of the real gas CO2(g) behave
most like an ideal gas?

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Temperature(K) Pressure(atm)

(A)
100 0.1

Temperature(K) Pressure(atm)
(B)
100 100

Temperature(K) Pressure(atm)
(C)
800 0.1

Temperature(K) Pressure(atm)
(D)
800 1

Temperature(K) Pressure(atm)
(E)
800 100

Refer to three gases in identical rigid containers under the conditions given in the table below.

12. The average kinetic energy of the gas molecules is

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(A) greatest in container A

(B) greatest in container B
(C) greatest in container C
(D) the same in all three containers

13. If the pressure of each gas is increased at constant temperature until condensation occurs, which gas will condense
at the lowest pressure?
(A) Methane
(B) Ethane
(C) Butane
(D) All the gases will condense at the same pressure.

14. The density of the gas, in g/L, is

(A) greatest in container A
(B) greatest in container B
(C) greatest in container C
(D) the same in all three containers

Refer to the following diatomic species

(A) Li2

(B) B2

(C) N2

(D) O2

(E) F2

15. Contains 1 sigma (σ) and 2 pi (π) bonds

(A) Li2
(B) B2
(C) N2
(D) O2
(E) F2

16. Has a bond order of 2

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(A) Li2
(B) B2
(C) N2
(D) O2
(E) F2

17. Has the largest bond-dissociation energy

(A) Li2
(B) B2
(C) N2
(D) O2
(E) F2

18.

The photoelectron spectra above show the energy required to remove a 1s electron from a nitrogen atom and from
an oxygen atom. Which of the following statements best accounts for the peak in the upper spectrum being to the
right of the peak in the lower spectrum?
(A) Nitrogen atoms have a half-filled p subshell.
(B) There are more electron-electron repulsions in oxygen atoms than in nitrogen atoms.
Electrons in the p subshell of oxygen atoms provide more shielding than electrons in the p subshell of
(C)
nitrogen atoms.
(D) Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

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19. The London (dispersion) forces are weakest for which of the following gases under the same conditions of
temperature and pressure?
(A) H2
(B) O2
(C) Xe
(D) F2
(E) N2

20. When a sample of oxygen gas in a closed container of constant volume is heated until its absolute temperature is
doubled, which of the following is also doubled?
(A) The density of the gas
(B) The pressure of the gas
(C) The average velocity of the gas molecules
(D) The number of molecules per cm3
(E) The potential energy of the molecules

21.

Based on the results of the paper chromatography experiment shown above, which of the following can be
concluded about the dye?
(A) It has a small molar mass.
(B) It has weak intermolecular forces.
(C) It has a weaker attraction for the stationary phase that it has for the mobile phase.
(D) It has a stronger attraction for the stationary phase than it has for the mobile phase.

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22. A 100g sample of a metal was heated to 100oC and then quickly transferred to an insulated container holding 100g
of water at 22oC. The temperature of the water rose to reach a final temperature of 35oC. Which of the following
can be concluded?
The metal temperature changed more than the water temperature did; therefore the metal lost more thermal
(A)
energy than the water gained.
The metal temperature changed more than the water temperature did, but the metal lost the same amount of
(B)
thermal energy as the water gained.
The metal temperature changed more than the water temperature did; therefore the heat capacity of the metal
(C)
must be greater than the heat capacity of the water.
The final temperature is less than the average starting temperature of the metal and the water; therefore the
(D)
total energy of the metal and water decreased.

23. A→X

The enthalpy change for the reaction represented above is ΔHT. This reaction can be broken down into a series of
steps as shown in the diagram:

A relationship that must exist among the various enthalpy changes is

(A) ΔHT – ΔH1 – ΔH2 – ΔH3 = 0
(B) ΔHT + ΔH1 + ΔH2 + ΔH3 = 0
(C) ΔH3 – (ΔH1 + ΔH2) = ΔHT
(D) ΔH2 – (ΔH3 + ΔH1) = ΔHT
(E) ΔHT + ΔH2 = ΔH1 + ΔH3

Directions: Each set of lettered choices below refers to the numbered statements immediately following it. Select the one
lettered choice that best fits each statement. A choice may be used once, more than once, or not at all in each set.

(A) A network solid with covalent bonding

(B) A molecular solid with zero dipole moment
(C) A molecular solid with hydrogen bonding
(D) An ionic solid
(E) A metallic solid

24. Solid ethyl alcohol, C2H5OH

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(A) A network solid with covalent bonding

(B) A molecular solid with zero dipole moment
(C) A molecular solid with hydrogen bonding
(D) An ionic solid
(E) A metallic solid

25.

Consider the molecules represented above and the data in the table below.

Nonane and 2,3,4-trifluoropentane have almost identical molar masses, but nonane has a significantly higher boiling
point. Which of the following statements best helps explain this observation?
(A) The C-F is easier to break than the C-H bond.
(B) The C-F is more polar than the C-H bond.
(C) The carbon chains are longer in nonane than they are in 2,3,4-trifluoropentane.
(D) The carbon chains are farther apart in a sample of nonane than they are in 2,3,4-trifluoropentane.

26.

To make Au stronger and harder, it is often alloyed with other metals, such as Cu and Ag. Consider two alloys, one
of Au and Cu and one of Au and Ag, each with the same mole fraction of Au. If the Au/Cu alloy is harder than the
Au/Ag alloy, then which of the following is the best explanation based on the information in the table above?
(A) Cu has two common oxidation states, but Ag has only one.
(B) Cu has a higher melting point than Au has, but Ag has a lower melting point than Au has.
(C) Cu atoms are smaller than Ag atoms, thus they interfere more with the displacement of atoms in the alloy.
(D) Cu atoms are less polarizable than are Au or Ag atoms, thus Cu has weaker interparticle forces.

27. The geometry of the SO3 molecule is best described as

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(A) trigonal planar

(B) trigonal pyramidal
(C) square pyramidal
(D) bent
(E) tetrahedral

28.

Based on the data in the tables above, which of the following statements provides the best prediction for the boiling
point of NaCl?
NaCl will have a lower boiling point than NaF because the coulombic attractions are weaker in NaCl than in
(A)
NaF.
NaCl will have a boiling point between that of NaF and MgO because the covalent character of the bonds in
(B)
NaCl is intermediate between that of MgO and NaF.
(C) NaCl will have a higher boiling point than MgO because the ions are spaced farther apart in NaCl.
NaCl will have a higher boiling point than MgO because the energy required to transfer electrons from the
(D)
anion to the cation is larger in NaCl than in MgO.

29. Which of the following pieces of laboratory glassware should be used to most accurately measure out a 25.00 mL
sample of a solution?
(A) 5 mL pipet
(B) 25 mL pipet
(C) 25 mL beaker
(D) 25 mL Erlenmeyer flask
(E) 50 mL graduated cylinder

30. A student wishes to prepare 2.00 liters of 0.100–molar KIO3 (molecular weight 214). The proper procedure is to
weigh out
(A) 42.8 grams of KIO3 and add 2.00 kilograms of H2O
(B) 42.8 grams of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters
(C) 21.4 grams of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters
(D) 42.8 grams of KIO3 and add 2.00 liters of H2O
(E) 21.4 grams of KIO3 and add 2.00 liters of H2O

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31. Two flexible containers for gases are at the same temperature and pressure. One holds 0.50 gram of hydrogen and
the other holds 8.0 grams of oxygen. Which of the following statements regarding these gas samples is FALSE?
(A) The volume of the hydrogen container is the same as the volume of the oxygen container.
The number of molecules in the hydrogen container is the same as the number of molecules in the oxygen
(B)
container.
(C) The density of the hydrogen sample is less than that of the oxygen sample.
The average kinetic energy of the hydrogen molecules is the same as the average kinetic energy of the
(D)
oxygen molecules.
(E) The average speed of the hydrogen molecules is the same as the average speed of the oxygen molecules.

32. H2Se(g) + 4 O2F2(g) → SeF6(g) + 2 HF(g) + 4 O2(g)

Which of the following is true regarding the reaction represented above?

(A) The oxidation number of O does not change.
(B) The oxidation number of H changes from -1 to +1.
(C) The oxidation number of F changes from +1 to -1.
(D) The oxidation number of Se changes from -2 to +6.
(E) It is a disproportionation reaction for F.

The following questions relate to the graph below. The graph shows the temperature of a pure substance as it is heated at a
constant rate in an open vessel at 1.0 atm pressure. The substance changes from the solid to the liquid to the gas phase.

33. The substance is at its normal freezing point at time

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(A) t1
(B) t2
(C) t3
(D) t4
(E) t5

34. Which of the following best describes what happens to the substance between t4 and t5?
(A) The molecules are leaving the liquid phase.
(B) The solid and liquid phases coexist in equilibrium.
(C) The vapor pressure of the substance is decreasing.
(D) The average intermolecular distance is decreasing.
(E) The temperature of the substance is increasing.

35.

The liquefied hydrogen halides have the normal boiling points given above. The relatively high boiling point of HF
can be correctly explained by which of the following?
(A) HF gas is more ideal.
(B) HF is the strongest acid.
(C) HF molecules have a smaller dipole moment.
(D) HF is much less soluble in water.
(E) HF molecules tend to form hydrogen bonds.

36. On the basis of strength of intermolecular forces, which of the following elements would be expected to have the
highest melting point?
(A) Br2
(B) Cl2
(C) F2
(D) Kr
(E) N2

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37.

The hybridization of the carbon atoms in the molecule represented above can be described as
(A) sp
(B) sp2
(C) sp3
(D) dsp2
(E) d2sp

38.
H-C≡C-H

What is the hybridization of the carbon atoms in a molecule of ethyne, represented above?
(A) sp
(B) sp2
(C) sp3
(D) dsp2
(E) d2sp

39. In solid methane, the forces between neighboring CH4 molecules are best characterized as
(A) ionic bonds
(B) covalent bonds
(C) hydrogen bonds
(D) ion-dipole forces
(E) London (dispersion) forces

40. Which of the following represents a process in which a species is reduced?

(A) Ca(s) → Ca2+(aq)
(B) Hg(l) → Hg22+(aq)
(C) Fe2+(aq) → Fe3+(aq)
(D) NO3-(aq) → NO(g)
(E) SO32-(aq) → SO42-(aq)

41. Forms monatomic ions with 2– charge in solutions

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(A) F
(B) S
(C) Mg
(D) Ar
(E) Mn

K(s)+ ½ Cl2(g) → KCl(s) ΔH° = -437kJ/molrxn

The elements K and Cl react directly to form the compound KCl according to the equation above. Refer to the information
above and the table below to answer the questions that follow.

42. Cl2(g) + 2e- → 2Cl-(g)

Which of the following expressions is equivalent to ΔHo for the reaction represented above?
(A) x + y
(B) x-y
(C) x + 2y
(D)

43. How much heat is released or absorbed when 0.050 mol of Cl2(g) is formed from KCl(s)?
(A) 87.4 kJ is released
(B) 43.7 kJ is released
(C) 43.7 kJ is absorbed
(D) 87.4 kJ is absorbed

44. Which of the values of ∆Ho for a process in the table is (are) less than zero (i.e., indicate(s) an exothermic process)?

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(A) z only
(B) y and z only
(C) x, y, and z only
(D) w, x, y, and z

45.

The ionization energies for element X are listed in the table above. On the basis of the data, element X is most likely
to be
(A) Na
(B) Mg
(C) Al
(D) Si
(E) P

46. Approximately what mass of CuSO4 • 5H2O (250 g mol-1) is required to prepare 250 mL of 0.10 M copper(II)
sulfate solution?
(A) 4.0 g
(B) 6.2 g
(C) 34 g
(D) 85 g
(E) 140 g

47. A 360. mg sample of aspirin, C9H8O4, (molar mass 180. g), is dissolved in enough water to produce 200. mL of
solution. What is the molarity of aspirin in a 50. mL sample of this solution?
(A) 0.0800 M
(B) 0.0400 M
(C) 0.0200 M
(D) 0.0100 M
(E) 0.00250 M

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Directions: Each set of lettered choices below refers to the numbered statements immediately following it. Select the one
lettered choice that best fits each statement. A choice may be used once, more than once, or not at all in each set.

The following questions refer to the below molecules:

(A) CO2
(B) H2O
(C) CH4
(D) C2H4
(E) PH3

48. The molecule with the largest dipole moment

(A) CO2
(B) H2O
(C) CH4
(D) C2H4
(E) PH3

49. The molecule with only one double bond

(A) CO2
(B) H 2O
(C) CH4
(D) C2H4
(E) PH3

50. The molecule that has trigonal pyramidal geometry

(A) CO2
(B) H2O
(C) CH4
(D) C2H4
(E) PH3

51. For which of the following molecules are resonance structures necessary to describe the bonding satisfactorily?
(A) H2S
(B) SO2
(C) CO2
(D) OF2
(E) PF3

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52. Which of the following molecules has an angular (bent) geometry that is commonly represented as a resonance
hybrid of two or more electron-dot structures?
(A) CO2
(B) O3
(C) CH4
(D) BeF2
(E) OF2

53. Of the following molecules, which has the largest dipole moment?
(A) CO
(B) CO2
(C) O2
(D) HF
(E) F2

54. Has molecules with a pyramidal shape

(A) NH3(g)
(B) BH3(g)
(C) H2(g)
(D) H2S(g)
(E) HBr(g)

55. Of the following compounds, which is the most ionic?

(A) SiCl4
(B) BrCl
(C) PCl3
(D) Cl2O
(E) CaCl2

56. The boiling points of the elements helium, neon, argon, krypton, and xenon increase in that order. Which of the
following statements accounts for this increase?
(A) The London (dispersion) forces increase.
(B) The hydrogen bonding increases.
(C) The dipole-dipole forces increase.
(D) The chemical reactivity increases.
(E) The number of nearest neighbors increases.

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57.
2 MnO4-(aq) + 10 Br-(aq) + 16 H+(aq) → 2 Mn2+(aq) + 5 Br2(aq) + 8 H2O(l)

How many electrons are transferred in the reaction represented by the balanced equation above?
(A) 2
(B) 4
(C) 5
(D) 8
(E) 10

58. Of the following single bonds, which is the LEAST polar?

(A) N—H
(B) H—F
(C) O—F
(D) I—F
(E) O—H

59. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the temperature of
the system remains constant, which of the following statements about the partial pressure of gas X is correct?
(A) It is equal to ⅓ the total pressure
(B) It depends on the intermolecular forces of attraction between molecules of X, Y, and Z.
(C) It depends on the relative molecular masses of X, Y, and Z.
(D) It depends on the average distance traveled between molecular collisions.
(E) It can be calculated with knowledge only of the volume of the container.

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60.

The diagram above represents H2(g) and N2(g) in a closed container. Which of the following diagrams would
represent the results if the reaction shown below were to proceed as far as possible?

N2(g) + 3 H2(g) → 2 NH3(g)

(A)

(B)

(C)

(D)

(E)

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61. Which of the following particulate diagrams best shows the formation of water vapor from hydrogen gas and
oxygen gas in a rigid container at 125oC?

(A)

(B)

(C)

(D)

62. Pi (π) bonding occurs in each of the following species EXCEPT

(A) CO2
(B) C2H4
(C) CN–
(D) C6H6
(E) CH4

63. The pressure, in atm, exerted by 1.85 mol of an ideal gas placed in a 3.00 L container at 35.0°C is given by which of
the following expressions?
(A)

(B)

(C)

(D)

(E)

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64. A sealed vessel contains 0.200 mol of oxygen gas, 0.100 mol of nitrogen gas, and 0.200 mol of argon gas. The total
pressure of the gas mixture is 5.00 atm. The partial pressure of the argon is
(A) 0.200 atm
(B) 0.500 atm
(C) 1.00 atm
(D) 2.00 atm
(E) 5.00 atm

65. A flask contains 0.25 mole of SO2(g), 0.50 mole of CH4(g), and 0.50 mole of O2(g). The total pressure of the gases
in the flask is 800 mm Hg. What is the partial pressure of the SO2(g) in the flask?
(A) 800 mm Hg
(B) 600 mm Hg
(C) 250 mm Hg
(D) 200 mm Hg
(E) 160 mm Hg

66. Equal numbers of moles of He(g), Ar(g), and Ne(g) are placed in a glass vessel at room temperature. If the vessel
has a pinhole-sized leak, which of the following will be true regarding the relative values of the partial pressures of
the gases remaining in the vessel after some of the gas mixture has effused?
(A) PHe < PNe < PAr
(B) PHe < PAr < PNe
(C) PNe < PAr < PHe
(D) PAr < PHe < PNe
(E) PHe = PAr = PNe

67.
CH3—CH2—CH2—CH2—CH3CH3—CH2—CH2—CH2—OHHO—CH2—CH2—CH2—OH

X Y Z

Based on concepts of polarity and hydrogen bonding, which of the following sequences correctly lists the
compounds above in the order of their increasing solubility in water?
(A) Z < Y < X
(B) Y<Z<X
(C) Y<X<Z
(D) X < Z < Y
(E) X<Y<Z

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Directions: Each set of lettered choices below refers to the numbered statements immediately following it. Select the one
lettered choice that best fits each statement. A choice may be used once, more than once, or not at all in each set.

The following questions refer to the reactions represented below.

(A) H2SeO4(aq) + 2 Cl-(aq) + 2 H+(aq) → H2SeO3(aq) + Cl2(g) + H2O(l)

(B) S8(s) + 8 O2(g) → 8 SO2(g)
(C) 3 Br2(aq) + 6 OH-(aq) → 5 Br-(aq) + BrO3-(aq) + 3 H2O(l)
(D) Ca2+(aq) + SO42-(aq) → CaSO4(s)
(E) PtCl4(s) + 2 Cl-(aq) → PtCl62-(aq)

68. A precipitation reaction

(A) H2SeO4(aq) + 2 Cl-(aq) + 2 H+(aq) → H2SeO3(aq) + Cl2(g) + H2O(l)
(B) S8(s) + 8 O2(g) → 8 SO2(g)
(C) 3 Br2(aq) + 6 OH-(aq) → 5 Br-(aq) + BrO3-(aq) + 3 H2O(l)
(D) Ca2+(aq) + SO42-(aq) → CaSO4(s)
(E) PtCl4(s) + 2 Cl-(aq) → PtCl62-(aq)

69. A reaction in which the same reactant undergoes both oxidation and reduction
(A) H2SeO4(aq) + 2 Cl-(aq) + 2 H+(aq) H2SeO3(aq) + Cl2(g) + H2O(l)
(B) S8(s) + 8 O2(g) 8 SO2(g)
(C) 3 Br2(aq) + 6 OH-(aq) 5 Br-(aq) + BrO3-(aq) + 3 H2O(l)
(D) Ca2+(aq) + SO42-(aq) CaSO4(s)
(E) PtCl4(s) + 2 Cl-(aq) PtCl62-(aq)

70. A precipitation reaction

(A) 2 Mg(s) + O2(g) → 2 MgO(s)
(B) Pb2+(aq) + CrO42-(aq) → PbCrO4(s)
(C) SO3(g) + 2 H2O(l) → H3O+(aq) + HSO4-(aq)
(D) 2 H2O(g) → 2 H2(g) + O2(g)
(E) Ag+(aq) + 2 NH3(aq) → [Ag(NH3)2]+(aq)

71. At constant temperature, the behavior of a sample of a real gas more closely approximates that of an ideal gas as its
volume is increased because the

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(A) collisions with the walls of the container become less frequent
(B) average molecular speed decreases
(C) molecules have expanded
(D) average distance between molecules becomes greater
(E) average molecular kinetic energy decreases

72. In which of the following species does sulfur have the same oxidation number as it does in H2SO4?
(A) H2SO3
(B) S2O32-
(C) S2-
(D) S8
(E) SO2Cl2

73. Which of the following molecules has the shortest bond length?
(A) N2
(B) O2
(C) Cl2
(D) Br2
(E) I2

74. Sodium chloride is LEAST soluble in which of the following liquids?

(A) H2O
(B) CCl4
(C) HF
(D) CH3OH
(E) CH3COOH

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75.

On the basis of the solubility curves shown above, the greatest percentage of which compound can be recovered by
cooling a saturated solution of that compound from 90°C to 30°C?
(A) NaCl
(B) KNO3
(C) K2CrO4
(D) K2SO4
(E) Ce2(SO4)3

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76.
Material Initial Temperature Mass Specific Heat
Cup
of Spoon of Spoon of Spoon Capacity
Aluminum
Ceramic
Steel
Silver

Four identical cups of coffee, originally at , were stirred with four different spoons, as listed in the
table above. In which cup will the temperature of the coffee be highest at thermal equilibrium? (Assume that the
heat lost to the surroundings is negligible.)
(A) Cup
(B) Cup
(C) Cup
(D) Cup

77. Which of the following techniques is most appropriate for the recovery of solid KNO3 from an aqueous solution of
KNO3?
(A) Paper chromatography
(B) Filtration
(C) Titration
(D) Electrolysis
(E) Evaporation to dryness

78.

The cooling curve above shows how the temperature of a sample varies with time as the sample goes through phase
changes. The sample starts as a gas, and heat is removed at a constant rate. At which time does the sample contain
the most liquid?

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(A) t1
(B) t2
(C) t3
(D) t4
(E) t5

79. Which of the following properties generally decreases across the periodic table from sodium to chlorine?
(A) First ionization energy
(B) Atomic mass
(C) Electronegativity
(D) Maximum value of oxidation number
(E) Atomic radius

80. The volume of distilled water that should be added to 10.0 mL of 6.00 M HCl(aq) in order to prepare a 0.500 M
HCl(aq) solution is approximately
(A) 50.0 mL
(B) 60.0 mL
(C) 100. ML
(D) 110. ML
(E) 120. mL

81. How many mL of 10.0 M HCl are needed to prepare 500. mL of 2.00 M HCl ?
(A) 1.00 mL
(B) 10.0 mL
(C) 20.0 mL
(D) 100. mL
(E) 200. mL

82. According to the VSEPR model, the progressive decrease in the bond angles in the series of molecules CH4, NH3,
and H2O is best accounted for by the
(A) increasing strength of the bonds
(B) decreasing size of the central atom
(C) increasing electronegativity of the central atom
(D) increasing number of unshared pairs of electrons
(E) decreasing repulsion between hydrogen atoms

83. A rigid metal tank contains oxygen gas. Which of the following applies to the gas in the tank when additional
oxygen is added at constant temperature?

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(A) The volume of the gas increases.

(B) The pressure of the gas decreases.
(C) The average speed of the gas molecules remains the same.
(D) The total number of gas molecules remains the same.
(E) The average distance between the gas molecules increases.

84. The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of
electrons on the central atom?
(A) H2S
(B) NH3
(C) CH4
(D) HCN
(E) CO2

85. The melting point of MgO is higher than that of NaF. Explanations for this observation include which of the
following?

I. Mg2+ is more positively charged than Na+.

II. O2- is more negatively charged than F-.

III. The O2- ion is smaller than the F- ion.

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

86. Which of the following gases deviates most from ideal behavior?
(A) SO2
(B) Ne
(C) CH4
(D) N2
(E) H2

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87. A sample of an ideal gas is cooled from 50.0oC to 25.0oC in a sealed container of constant volume. Which of the
following values for the gas will decrease?

I. The average molecular mass of the gas

II. The average distance between the molecules

III. The average speed of the molecules

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

88. Which of the following is a nonpolar molecule that contains polar bonds?
(A) F2
(B) CHF3
(C) CO2
(D) HCl
(E) NH3

89. Which of the following has a zero dipole moment?

(A) HCN
(B) NH3
(C) SO2
(D) NO2
(E) PF5

90. Which of the following ions has the same number of electrons as Br - ?
(A) Ca2+
(B) K+
(C) Sr2+
(D) I-
(E) Cl-

91. Which of the following species is NOT planar?

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(A) CO32-
(B) NO3-
(C) ClF3
(D) BF3
(E) PCl3

92. In which of the following processes are covalent bonds broken?

(A) I2(s) → I2(g)
(B) CO2(s) → CO2(g)
(C) NaCl(s) → NaCl(l)
(D) C(diamond) → C(g)
(E) Fe(s) → Fe(l)

93. N2 molecules absorb ultraviolet light but not visible light. I2 molecules absorb both visible and ultraviolet light.
Which of the following statements explains the observations?
(A) More energy is required to make N2 molecules vibrate than is required to make I2 molecules vibrate.
More energy is required to remove an electron from an I2 molecule than is required to remove an electron
(B)
from a N2 molecule.
Visible light does not produce transitions between electronic energy levels in the N2 molecule but does
(C)
produce transitions in the I2 molecule.
(D) The molecular mass of I2 is greater than the molecular mass of N2.

94. A 0.10 M aqueous solution of sodium sulfate, Na2SO4 , is a better conductor of electricity than a 0.10 M aqueous
solution of sodium chloride, NaCl. Which of the following best explains this observation?
(A) Na2SO4 is more soluble in water than NaCl is.
(B) Na2SO4 has a higher molar mass than NaCl has.
To prepare a given volume of 0.10 M solution, the mass of Na2SO4 needed is more than twice the mass of
(C)
NaCl needed.
More moles of ions are present in a given volume of 0.10 M Na2SO4 than in the same volume of 0.10 M
(D)
NaCl.
(E) The degree of dissociation of Na2SO4 in solution is significantly greater than that of NaCl.

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