States of Matter: Liquids and Solids Chapter

Chapter 11 - States of Matter: Liquids and Solids
1. Which of the following statements concerning liquids is incorrect?
A) The volume of a liquid changes very little with pressure.
B) Liquids are relatively incompressible.
C) Liquid molecules move slowly compared to solids.
D) Non-volatile liquids have low vapor pressures at room temperature.
E) The molecules of a liquid are in constant random motion.
ANS: C PTS: 1 DIF: easy REF: 11.1
OBJ: Compare a gas, a liquid, and a solid using a kinetic-molecular theory description.
TOP: phases | liquid KEY: properties of liquids
MSC: general chemistry
2. Which of the following statements concerning solids, liquids and gases is/are correct?
1. The close contact of the particles in a solid prevents all possible motion,
including vibrational motion.
2. Liquids and gases are both considered fluids.
3. The postulate from kinetic-molecular theory that the particles in a gas are in
constant random motion is equally applicable to liquids, except the particles
are more tightly packed in a gas.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 2 and 3
ANS: B PTS: 1 DIF: easy REF: 11.1
OBJ: Compare a gas, a liquid, and a solid using a kinetic-molecular theory description.
TOP: phases | liquid
3. What is the name for the following phase change?
I2(s) → I2(g)
A) sublimation
B) freezing
C) vaporization
D) condensation
E) melting
ANS: A PTS: 1 DIF: easy REF: 11.2
OBJ: Define melting, freezing, vaporization, sublimation, and condensation.
TOP: phases | phase transitions MSC: general chemistry
Test Bank General Chemistry, 10th
edition 1

4. Which of the following processes is endothermic?
A) melting of ice
B) condensation of water
C) deposition of carbon dioxide
D) freezing of water
E) condensation of ammonia
ANS: A PTS: 1 DIF: moderate REF: 11.2
TOP: phases | phase transitions
5. The process represented by the equation C10H8(s) → C10H8(g) is
A) melting.
B) liquefaction.
C) sublimation.
D) condensation.
E) fusion.
6. When a solid undergoes a phase change to a gas, the process is called
A) fusion.
B) condensation.
C) melting.
D) vaporization.
E) sublimation.
ANS: E PTS: 1 DIF: easy REF: 11.2
7. A bottle is filled with a small amount of a volatile liquid and sealed. Sometime later it is
observed that no liquid is evident in the sealed bottle. Which of the following statements
would explain this observation?
A) More time is needed to establish equilibrium.
B) Liquid and vapor are at equilibrium in the bottle.
C) Too little liquid was added to achieve a liquid vapor equilibrium in the closed
system.
D) The vapor state is favored when equilibrium is established.
E) The liquid has undergone sublimation.
ANS: C PTS: 1 DIF: moderate REF: 11.2
OBJ: Define vapor pressure. TOP: phases | phase transitions
KEY: vapor pressure MSC: general chemistry
edition 2

8. Enough of a volatile liquid is placed in a closed container to achieve a liquid-vapor
equilibrium at a fixed temperature. Which of the following statements regarding this system
is/are correct once equilibrium is established?
1. Liquid molecules are no longer evaporating.
2. The number of vapor molecules remains essentially constant.
3. The partial pressure exerted by the vapor molecules is called the vapor
pressure of the liquid.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 2 and 3
ANS: E PTS: 1 DIF: moderate REF: 11.2
9. Enough of a volatile liquid is placed in a closed container to achieve a liquid-vapor
equilibrium. Which of the following statements regarding this system is/are correct once
equilibrium is established?
1. The rate of condensation is equal to the rate of evaporation.
2. The fraction of molecules with enough energy to escape the liquid surface
depends on the liquid surface area.
3. The vapor pressure is independent of the temperature.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
10. If more ice is added to an ice-water mixture at equilibrium,
A) the temperature will increase somewhat.
B) the vapor pressure of the water will decrease.
C) the temperature will decrease somewhat.
D) the vapor pressure of the water will rise.
E) the vapor pressure of the water will remain constant.
OBJ: Describe the process of reaching a dynamic equilibrium that involves the
vaporization of a liquid and condensation of its vapor.
TOP: phases | phase transitions KEY: vapor pressure
edition 3

11. Which of the following involves a change in temperature during the phase transition?
A) condensation of water
B) fusion of ethanol
C) vaporization of water
D) all of the above
E) none of the above
OBJ: Describe the process of reaching a dynamic equilibrium that involves the
vaporization of a liquid and condensation of its vapor.
12. The boiling point of a liquid is
A) always the temperature at which the vapor pressure equals 760 mmHg (1 atm).
B) always the temperature at which the liquid phase of a substance is in equilibrium
with the vapor phase.
C) always the temperature at which the vapor pressure equals the pressure exerted on
the liquid.
D) always equal to the vapor pressure of the liquid at a given temperature.
E) independent of the pressure exerted on the liquid.
OBJ: Define boiling point. TOP: phases | phase transitions
13. Which one of the following liquids would you expect to have the highest vapor pressure at
room temperature? (all boiling points are normal boiling points)
A) n-pentane, b.p. = 36.1°C
B) methanol, b.p. = 65.0°C
C) carbon tetrachloride, b.p. = 76.7°C
D) acetic acid, b.p. = 118°C
E) mercury, b.p. = 357°C
OBJ: Define boiling point. TOP: phases | phase transitions
14. In which of the following processes will energy be evolved as heat?
A) crystallization
B) melting
C) sublimation
D) vaporization
E) none of these
OBJ: Define heat (enthalpy) of fusion and heat (enthalpy) of vaporization.
TOP: phases | phase transitions KEY: phase transition enthalpy change
edition 4

15. Which of the following phase changes are endothermic?
A) vaporization
B) freezing
C) liquifaction
D) crystallization
E) condensation
OBJ: Define heat (enthalpy) of fusion and heat (enthalpy) of vaporization.
16. The enthalpy of fusion of sodium is 2.60 kJ/mol. How many grams of sodium can be melted
by adding 81.7 kJ of energy to the metal at its melting point?
A) 7.22 × 10
2
g
B) 9.24 g
C) 3.55 g
D) 31.4 g
E) 1.50 × 10
3
g
OBJ: Calculate the heat required for a phase change of a given mass of substance.
(Example 11.1) TOP: phases | phase transitions
17. Assume 12,500 J of energy is added to 2.0 moles (36 grams) of H2O as an ice sample at
0°C. The molar heat of fusion is 6.02 kJ/mol. The specific heat of liquid water is 4.18 J/g
°C. The molar heat of vaporization is 40.6 kJ/mol. The resulting sample contains which of
the following?
A) water and water vapor
B) ice and water
C) only water
D) only water vapor
E) only ice
KEY: phase transition enthalpy change MSC: general chemistry
18. How much heat is released at constant pressure if a 14.0-L tank containing 56.0 atm of
hydrogen sulfide gas condenses at its boiling point of -60.0o
C? The enthalpy of
vaporization of hydrogen sulfide is 18.7 kJ/mol at -60.0o
C. (R = 0.0821 L • atm/(K • mol))
A) 1.17 × 102
J
B) 2.98 × 106
J
C) 4.17 × 102
J
D) 1.87 × 104
J
E) 8.38 × 105
J
edition 5

19. What is the value of q when 8.21 g of water vaporizes at 373 K? The enthalpy of
condensation of water at 373 K is –40.7 kJ/mol.
A) –334 kJ
B) –18.5 kJ
C) 18.5 kJ
D) 334 kJ
E) 0.202 kJ
20. The vapor pressure of a liquid increases with increasing temperature. Which of the
following statements best explains this relationship?
A) All the molecules have greater kinetic energies.
B) The number of gaseous molecules above the liquid remains constant, but these
molecules have greater average kinetic energy.
C) The faster-moving molecules in the liquid exert a greater pressure.
D) The intermolecular forces between the molecules decrease at higher temperatures.
E) The average kinetic energy of molecules is greater; thus more molecules can enter
the gaseous state.
OBJ: Describe the general dependence of the vapor pressure (in P) on the temperature (T).
21. The vapor pressure of a given liquid will increase if
A) the liquid is moved to a container in which its surface is very much larger.
B) the volume of the liquid is increased.
C) the temperature is increased.
D) the volume of the vapor phase is increased.
E) a more volatile liquid is added to the given liquid.
OBJ: Describe the general dependence of the vapor pressure (in P) on the temperature (T).
edition 6

22. A particular compound has an enthalpy of vaporization of 28300 J/mol. At 281 K it has a
vapor pressure of 101 mmHg. What is its vapor pressure at 301 K? (R = 8.31 J/(K· mol))
A) 98.8 mmHg
B) 123 mmHg
C) 45.2 mmHg
D) 226 mmHg
E) 103 mmHg
ANS: D PTS: 1 DIF: moderate REF: 11.2
OBJ: Calculate the vapor pressure at a given temperature. (Example 11.2)
TOP: phases | phase transitions KEY: Clausius-Clapeyron equation
23. A liquid has an enthalpy of vaporization of 30.8 kJ/mol. At 275 K it has a vapor pressure of
117 mmHg. What is the normal boiling point of this liquid? (R = 8.31 J/(K· mol))
A) 293 K
B) 319 K
C) 275 K
D) 259 K
E) 241 K
ANS: B PTS: 1 DIF: moderate REF: 11.2
24. In a certain mountain range, water boils at 94°C. What is the atmospheric pressure under
these conditions? The enthalpy of vaporization of water at 100°C is 40.7 kJ/mol.
(R = 8.31 J/(K · mol))
A) 1760 mmHg
B) 324 mmHg
C) 613 mmHg
D) 942 mmHg
E) 329 mmHg
25. For a particular liquid, raising its temperature from 319 K to 337 K causes its vapor pressure
to double. What is the enthalpy of vaporization of this liquid? (R = 8.31 J/(K · mol))
A) 34.4 kJ/mol
B) 320 kJ/mol
C) 2.01 kJ/mol
D) 228 kJ/mol
E) 104 kJ/mol
edition 7

ANS: A PTS: 1 DIF: difficult REF: 11.2
OBJ: Calculate the heat of vaporization from vapor pressure. (Example 11.3)
26. Knowing that ∆Hvap for water is 40.7 kJ/mol, calculate Pvap of water at 37°C.
A) 52.7 torr
B) 25.4 torr
C) 18.7 torr
D) 12.4 torr
E) 6.90 torr
27. What is the enthalpy of vaporization of a compound that has a vapor pressure of 131 mmHg
at 211 K and 2.23 mmHg at 177 K? (R = 8.31 J/(K· mol))
A) 996 kJ/mol
B) 1.15 kJ/mol
C) 3.31 kJ/mol
D) 37.2 kJ/mol
E) 368 kJ/mol
28. In the accompanying phase diagram, a liquid can be present at combinations of temperature
and pressure corresponding to points
A) A, C, G, and D.
B) A, C, D, and F.
C) A, B, C, and G.
D) A and C only.
E) G, C, D, and E.
edition 8

OBJ: Define phase diagram. TOP: phases | phase transitions
KEY: phase diagram MSC: general chemistry
29. Which of the following statements concerning the accompanying phase diagram is false?
A) The solid is more dense than the liquid.
B) Point C is the critical point of the substance.
C) Point A is the triple point of the substance.
D) The normal boiling point is above the triple point.
E) The curve AD divides the solid region from the gas region.
30. Given the accompanying phase diagram, under what conditions will liquid be found in
equilibrium with either solid or gas?
A) Anywhere along curve AB.
B) Anywhere along curve AC.
C) Anywhere along curve AD.
D) Anywhere along curve AB and AC.
E) Anywhere along curve AB and AD.
edition 9

31. Choose the correct statement about the diagram below.
A) The diagram shows the triple point above 1 atm pressure.
B) The diagram is qualitatively correct for water.
C) The diagram shows that the melting point of the solid increases with increasing
pressure.
D) The diagram could represent the phase diagram of CO2.
E) None of the above statements is correct.
32. From a consideration of the phase diagram below, a change from point M to point N
corresponds to
A) sublimation.
B) liquefaction.
C) evaporation.
D) condensation.
E) freezing.
edition 10

33. The triple point of iodine is at 90 torr and 115°C. This means that liquid I2
A) cannot have a vapor pressure less than 90 torr.
B) is more dense than I2(s).
C) cannot exist at 1 atmosphere pressure.
D) cannot exist above 115°C.
E) can exist at pressure of 10 torr.
OBJ: Define triple point. TOP: phases | phase transitions
34. The critical point of CCl4 is 283°C and 45 atm pressure. Liquid CCl4 has a vapor pressure of
10.0 atm at 178°C. Which of the following statements must be true?
A) Vapor and liquid can only be in equilibrium at one temperature—the normal
boiling point.
B) Liquid CCl4 can exist at temperatures greater than 283°C if the pressure is greater
than 45 atm.
C) Liquid and solid can only be in equilibrium at one temperature—the freezing point.
D) The triple point of CCl4 must be less than 178°C.
E) The normal boiling point of CCl4 must be greater than 178°C.
KEY: phase diagram | triple point MSC: general chemistry
35. Below is a phase diagram for a substance.
What is the name for point X on the diagram?
A) boiling point
B) normal boiling point
C) triple point
D) melting point
E) critical point
KEY: phase diagram | triple point MSC: general chemistry
edition 11

Which line represents the melting-point curve of the substance?
A) R-X
B) S-X
C) X-Z
D) S-Z
E) M-N
OBJ: Describe the melting-point curve and the vapor-pressure curves (for the liquid and
the solid) in a phase diagram. TOP: phases | phase transitions
KEY: phase diagram | melting-point curve MSC: general chemistry
Which line represents the vapor-pressure curve of the substance?
A) S-Z
B) X-Z
C) S-X
D) M-N
E) R-X
KEY: phase diagram | vapor pressure curve MSC: general chemistry
edition 12

38. If the liquid of a pure substance has a lower density than the solid, what is the effect on the
pressure-temperature phase diagram?
A) The vapor-pressure curve arches upward.
B) The normal melting point is above room temperature.
C) The melting-point curve has a negative slope.
D) The vapor-pressure curve arches downward.
E) The melting-point curve has a positive slope.
KEY: phase diagram | melting-point curve MSC: general chemistry
What is the name for point Z on the diagram?
A) normal boiling point.
B) critical point.
C) melting point.
D) boiling point.
E) triple point.
OBJ: Define critical temperature and critical pressure.
TOP: phases | phase transitions KEY: phase diagram
40. Which explanation best describes surface tension?
A) Molecules at the surface of a liquid experience a net force towards the liquid's
interior.
B) Molecules at the edges of a liquid adhere to the surface of the liquid's container.
C) Molecules of a liquid tend to form a concave meniscus.
D) Molecules of a liquid tend to resist flow.
E) Molecules of a liquid have a very low vapor pressure.
OBJ: Define surface tension. TOP: phases | liquid
KEY: properties of liquids | surface tension MSC: general chemistry
edition 13

41. If the diameter of a spherical water droplet is 100.0 µm, how much energy is required to
increase the diameter of the water droplet by 3.0 µm? The surface tension of water is
1.0 × 10-3
J/m2
.
A) 3.1 × 10–11
J
B) 1.9 × 10–12
J
C) 2.8 × 10–14
J
D) 7.7 × 10–12
J
E) 3.3 × 10–11
J
OBJ: Define surface tension. TOP: phases | liquid
42. Which is the best reason for why water in a glass capillary has a concave meniscus, while
mercury in a glass capillary has a convex meniscus?
A) Mercury has a greater dispersion force than water.
B) The water is attracted more strongly to the glass than the mercury is attracted to the
glass.
C) The mercury is attracted more strongly to the glass than the water is attracted to the
glass.
D) Water is a molecular compound while mercury is a metallic element.
E) Water has a greater dispersion force than mercury.
OBJ: Describe the phenomenon of capillary rise. TOP: phases | liquid
43. Which of the following forces is/are responsible for capillary action, a property of liquids?
1. attractive forces between the liquid and the capillary material
2. surface tension of the liquid
3. viscosity of the liquid
A) 1
B) 2
C) 3
D) 1 and 2
E) 1, 2, and 3
ANS: D PTS: 1 DIF: easy REF: 11.4
KEY: properties of liquids MSC: general chemistry
44. Which of the following concerning surface tension and viscosity is/are correct?
1. A molecule at the surface of a liquid experiences a net attractive force toward
the interior of the liquid.
2. The surface tension of a liquid is unaffected by substances dissolved in the
liquid.
edition 14

3. The viscosity of a liquid is determined in part by the strength of
intermolecular forces.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1 and 3
45. The measure of the resistance to flow of a liquid is
A) London forces.
B) van der Waals forces.
C) viscosity.
D) vapor pressure.
E) surface tension.
OBJ: Define viscosity. TOP: phases | liquid
KEY: properties of liquids | viscosity MSC: general chemistry
46. In which of the following substances are intermolecular forces of attraction absent?
A) HF(l)
B) CCl4(l)
C) NaCl(l)
D) H2O(l)
E) N2(l)
OBJ: Define London (dispersion) forces. TOP: phases | liquid
47. Which one of the following decreases as the strength of the attractive intermolecular forces
increases?
A) The normal boiling temperature.
B) The vapor pressure of a liquid.
C) The extent of deviations from the ideal gas law.
D) The heat of vaporization.
E) The sublimation temperature of a solid.
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid KEY: intermolecular forces
edition 15

48. Which of the following compounds has the highest normal boiling point?
A) CH3CH2CH2CH3
B) CH3Cl
C) CH3CH2OH
D) CH3OCH3
E) CH3CH2CH3
KEY: intermolecular forces | hydrogen bonding MSC: general chemistry
49. Which of the following compounds has the highest vapor pressure at 25°C?
A) CH3CH2OH
B) CH3CH2CH2CH3
C) CH3OCH3
D) CH3CH2CH3
E) CH3CH2CH2Cl
50. Which of the following pure substances has the lowest normal boiling point?
A) H2S
B) NH3
C) H2O
D) H2Te
E) H2Se
51. Methane (CH4) is able to be liquefied at low temperatures due to which intermolecular
force?
A) ionic bonding
B) covalent bonding
C) hydrogen bonding
D) dipole–dipole
E) London dispersion
edition 16

52. Which compound has the lowest standard enthalpy of vaporization at 25°C?
A) C6H14
B) C8H16
C) C5H12
D) C8H18
E) C7H16
TOP: phases | liquid KEY: intermolecular forces | London forces
53. Which of the following indicates the existence of strong intermolecular forces of attraction
in a liquid?
A) a very low critical temperature
B) a very low boiling point
C) a very low vapor pressure
D) a very low viscosity
E) a very low enthalpy of vaporization
54. Which of the following compounds has the lowest normal boiling point?
A) CH3CH2CH2NH2
B) CH3CH2CH2F
C) CH3CH2CH2OH
D) CH3CH2COOH
E) CH3CH(OH)CH3
55. Which of the following compounds is expected to have the lowest vapor pressure?
A) CH3OCH3
B) CH3CH2F
C) CH3CH2OH
D) CH3CH2CH2CH3
E) CH3CH2CH3
edition 17

56. Which of the following pure substances has the highest normal boiling point?
A) HI
B) HCl
C) HF
D) H2S
E) HBr
57. Why does hydrogen fluoride have an unusually high normal boiling point compared to the
other hydrogen halides?
A) The H-F bond in hydrogen fluoride is very strong.
B) Hydrogen fluoride has very strong London dispersion forces.
C) Hydrogen fluoride is capable of forming hydrogen bonds.
D) Hydrogen fluoride is ionic.
E) Hydrogen fluoride is covalent.
58. Which of the following pure substances has the lowest vapor pressure at 25°C?
A) SbH3
B) NH3
C) PH3
D) AsH3
E) H2O
59. Which of the following pure substances has the highest vapor pressure at room temperature?
A) Si3H8
B) Si2H6
C) Si2Cl6
D) Si4H10
E) SiH4
edition 18

60. Which of the following pure substances has the highest standard enthalpy of vaporization at
25°C?
A) H2O
B) NH3
C) PH3
D) AsH3
E) SbH3
61. At 25°C, the vapor pressure of diethyl ether, (CH3CH2)2O, is higher than the vapor pressure
of its isomer n-butanol, CH3CH2CH2CH2OH, because
A) diethyl ether has a higher density than n-butanol.
B) diethyl ether has weaker intermolecular forces than n-butanol.
C) diethyl ether has a lower critical temperature than n-butanol.
D) diethyl ether has a higher surface tension than n-butanol.
E) diethyl ether has weaker intramolecular forces than n-butanol.
62. Which of the following pure substances has an unusually high normal boiling point?
A) CH3OCH3
B) CH3SH
C) HCl
D) CH3NH2
E) CH3Cl
63. Rank the following molecules in order of increasing normal boiling point: CH3CH2OH,
CH3CH2CH2OH, CH3CH2OCH3.
A) lowest CH3CH2CH2OH, CH3CH2OCH3, CH3CH2OH highest.
B) lowest CH3CH2OH, CH3CH2OCH3, CH3CH2CH2OH highest.
C) lowest CH3CH2CH2OH, CH3CH2OH, CH3CH2OCH3 highest.
D) lowest CH3CH2OCH3, CH3CH2OH, CH3CH2CH2OH highest.
E) lowest CH3CH2OCH3, CH3CH2CH2OH, CH3CH2OH highest.
edition 19

64. Rank the following in order of increasing normal boiling point: N2, O2, Br2, Xe.
A) N2 < O2 < Xe < Br2
B) O2 < N2 < Xe < Br2
C) Br2 < Xe < N2 < O2
D) N2 < O2 < Br2 < Xe
E) Xe < Br2 < N2 < O2
65. Which of the following concerning intermolecular forces is/are correct?
1. Intermolecular forces depend in part on the shape of a molecule.
2. London forces contribute to the net forces of attraction found in all molecular
solids and liquids.
3. Hydrogen bonding is a special category of dipole-dipole attractions.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
66. In an experiment, 40.0 mmol of helium gas is collected over water. The total volume of gas
collected is 0.224 L. Under similar conditions, the gas is collected over two other liquids, A
and B. The total volume of gas collected over A and B are 0.222 L and 0.227 L,
respectively. Which of the following statements is false?
A) Liquid B boils at a higher temperature than water
B) Liquid A boils at a higher temperature than water
C) The vapor pressure of B is higher than that of A
D) The vapor pressure of B is higher than that of water
E) Liquid A boils at a temperature higher than B
edition 20

67. When two water molecule form a hydrogen bond, which atoms are involved in the
interaction?
A) Two hydrogens from one molecule and one hydrogen from the other molecule
B) An oxygen from one molecule and an oxygen from the other molecule
C) Two hydrogens from one molecule and one oxygen from the other molecule
D) A hydrogen from one molecule and a hydrogen from the other molecule
E) A hydrogen from one molecule and an oxygen from the other molecule
OBJ: Define hydrogen bonding. TOP: phases | liquid
68. What is the maximum number of hydrogen bonds in which a water molecule could
participate?
A) 2
B) 4
C) 3
D) 6
E) 5
69. Which pure substance exhibits hydrogen bonding?
A) HNF2
B) B2H6
C) HBr
D) H2S
E) CaH2
70. Which of the following substances has the weakest intermolecular forces?
A) I2
B) C8H18
C) SiH4
D) CH3CH2CH2CH2OH
E) SbCl3
OBJ: Identify the intermolecular forces in a substance. (Example 11.5)
edition 21

71. Which of the following best describes carbon dioxide (CO2) at room temperature and
pressure?
A) ionic solid
B) nonpolar molecular gas
C) metallic solid
D) polar molecular gas
E) covalent network solid
TOP: phases | gas MSC: general chemistry
72. Which of the following pure substances may exhibit hydrogen bonding?
A) CH3Cl
B) CH3OCH3
C) H2CO
D) N(CH3)3
E) H2NNH2
73. The strongest intermolecular forces present in a sample of pure I2 are
A) London forces.
B) dipole–dipole forces.
C) metallic bonds.
D) covalent network bonds.
E) covalent bonds.
74. The strongest intermolecular forces between molecules of PH3 are
A) hydrogen bonds.
B) covalent bonds.
C) ionic bonds.
D) London forces.
E) dipole–dipole attractions.
edition 22

75. The molecules in a sample of solid SO2 are attracted to each other by a combination of
A) H-bonding and ionic bonding.
B) covalent bonding and dipole-dipole interactions.
C) London forces and H-bonding.
D) London forces and dipole-dipole interactions.
E) none of these
76. Which of the following best describes silane (SiH4) at room temperature and pressure?
A) ionic solid
B) covalent network solid
C) nonpolar molecular gas
E) metallic solid
TOP: phases | gas MSC: general chemistry
77. Which of the following is the strongest intermolecular force present in dry ice, CO2(s)?
A) covalent bonding
B) hydrogen bonding
C) ionic bonding
D) London forces
E) metallic bonding
78. A solid has a very high melting point, is hard, and in the molten state is a non-conductor.
The solid is most likely
A) a covalent network solid.
B) a metallic solid.
C) an amorphous solid.
D) a molecular solid.
E) an ionic solid.
OBJ: Define molecular solid, metallic solid, ionic solid, and covalent network solid.
TOP: phases | solid
edition 23

79. Van der Waals forces must be broken to melt this type of solid.
A) A covalent network solid.
B) A metallic solid.
C) A molecular solid.
D) An ionic solid.
E) none of the above
TOP: phases | solid
80. Which substance can be described as cations bonded together by mobile electrons?
A) S8(s)
B) Ag(s)
C) HCl(l)
D) KCl(s)
E) Kr(l)
TOP: phases | solid KEY: classification of solids
81. Which of the following best describes calcium hydride (CaH2) at room temperature and
pressure?
A) nonpolar molecular gas
B) metallic solid
C) ionic solid
E) covalent network solid
OBJ: Identify types of solids. (Example 11.7) TOP: phases | solid
KEY: classification of solids MSC: general chemistry
82. Which of the following is not a covalent network solid?
A) diamond
B) silicon carbide
C) quartz
D) iron
E) graphite
edition 24

83. Which of the following is a molecular solid?
A) NaCl
B) CH4
C) SiO2
D) C(graphite)
E) C(diamond)
84. Which of the following is an ionic solid?
A) SiO2(s)
B) Ne(s)
C) Na(s)
D) CsF(s)
E) CO2(s)
85. Which bonding interaction best describes the strongest intermolecular forces in AlH3?
A) dipole–dipole forces
B) metallic bonding
C) ionic bonding
D) London dispersion forces
E) primarily hydrogen bonding
86. Which of the following is a molecular solid?
A) carborundum, SiC
B) quartz
C) glass
D) hydrogen chloride
E) potassium
87. Which of the following pure substances has the highest normal melting point?
A) KF
B) KI
C) NaF
D) NaCl
E) NaI
edition 25

OBJ: Relate the melting point of a solid to its structure. TOP: phases | solid
KEY: properties of solids | melting point MSC: general chemistry
88. Which of the following pure substances has the lowest melting point?
A) LiF
B) RbF
C) CsF
D) KF
E) NaF
89. Which of the following pure substances has the lowest melting point?
A) Cs2O
B) CsCl
C) CsBr
D) CsI
E) CsF
90. Which of the following pure substances has the highest melting point?
A) CCl4
B) AlCl3
C) NCl3
D) LiCl
E) MgCl2
91. Which of the following pure substances has the highest melting point?
A) KBr
B) NaCl
C) NaF
D) CsI
E) LiF
edition 26

92. A low melting solid readily dissolves in water to give a nonconducting solution. The solid is
most likely a
A) molecular solid.
B) ionic solid.
C) covalent network solid.
D) weak base.
E) metallic solid.
93. Which of the following pure substances is a solid at room temperature and pressure?
A) NH3
B) PH3
C) SiH4
D) CH4
E) AlH3
OBJ: Determine relative melting points based on types of solids. (Example 11.8)
TOP: phases | solid KEY: properties of solids | melting point
A) NO2
B) SiO2
C) CO2
D) P4O10
E) N2O5
A) P4O10
B) P4O6
C) CO2
D) CaO
E) Na2O
edition 27

96. Which of the following pure substances has the highest normal boiling point?
A) H2O
B) CF4
C) CsF
D) CaF2
E) KF
TOP: phases | solid KEY: properties of solids
97. A certain solid substance that is very hard, has a high melting point, and is nonconducting
unless melted is most likely to be:
A) CO2
B) I2
C) H2O
D) NaCl
E) Cu
OBJ: Relate the hardness and electrical conductivity of a solid to its structure.
98. A solid crystal of NaCl is
A) soft, low melting, a poor electrical conductor.
B) soft, low melting, a good electrical conductor.
C) hard, high melting, a good electrical conductor.
D) hard, high melting, a poor electrical conductor.
E) soft, high melting, a poor electrical conductor.
OBJ: Relate the hardness and electrical conductivity of a solid to its structure.
99. Which of the following concerning the 2-D lattice provided below is/are correct?
1. One possible unit cell contains a single Α and a single •.
2. More than one unit cell which reproduces this lattice is possible.
3. One possible unit cell contains four Α’s and four •’s.
edition 28

A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
OBJ: Define crystal lattice and unit cell of a crystal lattice. TOP: phases | solid
100. For a given pure metal which of the following cubic unit cells would result in the highest
metal density?
A) It depends on the identity of the metal.
B) The density would be identical for all these cells if the edge length of each cell
were the same.
C) A face-centered cubic cell.
D) A simple cubic cell.
E) A body-centered cubic cell.
OBJ: Define simple cubic unit cell, body-centered cubic unit cell, and face-centered cubic
unit cell. TOP: phases | solid
KEY: crystalline solids | cubic unit cell MSC: general chemistry
101. In any cubic lattice an atom lying at the corner of a unit cell is shared equally by how many
unit cells?
A) 1
B) 16
C) 2
D) 4
E) 8
KEY: crystalline solids | cubic unit cell MSC: general chemistry
102. The space-filling representation of a crystalline polonium provided below is an example of a
_____ unit cell, which contains the equivalent of _____ atom(s) within a single unit cell.
edition 29

A) simple cubic, 1 atom
B) body centered cubic, 2 atoms
C) face centered cubic, 4 atoms
D) simple cubic, 8 atoms
E) body centered cubic, 3 atoms
103. The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an
anion in the center, and a cation at the center of each face. The unit cell contains a net:
A) 2 anions and 3 cations.
B) 2 anions and 2 cations.
C) 5 anions and 3 cations.
D) 3 anions and 4 cations.
E) 5 anions and 6 cations.
OBJ: Determine the number of atoms in a unit cell. (Example 11.9)
TOP: phases | solid KEY: crystalline solids | cubic unit cell
104. How many atoms are there in a cubic close-packed unit cell of aluminum?
A) 4
B) 6
C) 1
D) 8
E) 2
TOP: phases | solid
KEY: structures of crystalline solids | metallic solid MSC: general chemistry
105. How many atoms are there in a body-centered cubic unit cell of vanadium?
A) 4
B) 8
C) 6
D) 2
E) 1
TOP: phases | solid
edition 30

106. A metal crystallizes in a face-centered cubic lattice. The radius of the atom is 196 pm and
the density of the element is 1.55 g/cm3
. How many atoms are there per unit cell?
A) 4
B) 6
C) 8
D) 1
E) 2
TOP: phases | solid
107. Which one of the following statements about solid Cu (face-centered cubic unit cell) is
incorrect?
A) It will conduct electricity.
B) The length of a face diagonal is four times the Cu radius.
C) The number of atoms surrounding each Cu atom is 12.
D) The solid has a cubic closest-packed structure.
E) There are two atoms per unit cell.
OBJ: Note the common structures (face-centered cubic and body-centered cubic) of
metallic solids. TOP: phases | solid
108. Lithium chloride crystallizes in a face-centered cubic structure. The unit cell length is
5.14 × 10-8
cm. The chloride ions are touching each other along the face diagonal of the unit
cell. The lithium ions fit into the holes between the chloride ions. How many chloride ions
are there in this unit cell?
A) 4
B) 3
C) 1
D) 8
E) 2
OBJ: Describe the three types of cubic structures of ionic solids.
TOP: phases | solid
KEY: structures of crystalline solids | ionic solid MSC: general chemistry
109. Assuming the following metals all have the same unit cell structure, which of the following
would be expected to have the highest density: Sc, Ti, Mn, or Co?
A) Mn
B) Ti
C) Co
D) Sc
E) cannot be determined from the information given.
edition 31

OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10)
TOP: phases | solid KEY: calculations with unit cell dimensions
110. The metal palladium crystallizes in a face-centered cubic lattice with an edge length of
388.8 pm. What is the density of palladium?
A) 0.752 g/cm3
B) 3.01 g/cm3
C) 1.50 g/cm3
D) 6.01 g/cm3
E) 12.0 g/cm3
ANS: E PTS: 1 DIF: difficult REF: 11.9
111. The metal gold, with an atomic radius of 144.2 pm, crystallizes in a face-centered cubic
lattice. What is the density of gold?
A) 9.65 g/cm3
B) 1.21 g/cm3
C) 4.82 g/cm3
D) 2.41 g/cm3
E) 19.3 g/cm3
. What is the identity of the metal?
A) Cu
B) Ca
C) Sr
D) Ni
E) Yb
TOP: phases | solid KEY: structures of crystalline solids
edition 32

113. Calcium crystallizes in a face-centered cubic lattice. The density of the element is 1.55
g/cm3
. What is the volume of a single unit cell?
A) 1.72 × 10
−22
cm3
B) 4.13 × 10
−22
cm3
C) 1.07 × 10
−25
cm3
D) 4.29 × 10
−23
cm3
E) 1.03 × 10
−22
cm3
TOP: phases | solid
114. Ytterbium crystallizes in a face-centered cubic lattice. The radius of ytterbium is 198 pm.
What is the edge length of the unit cell?
A) 560 pm
B) 396 pm
C) 792 pm
D) 420 pm
E) 198 pm
OBJ: Calculate unit-cell dimension given radius and unit cell. TOP: phases | solid
5.14 × 10-8
cell. The lithium ions fit into the holes between the chloride ions. What is the mass of LiCl
in a unit cell?
A) 5.63 × 10-22
g
B) 1.41 × 10-22
g
C) 4.22 × 10-22
g
D) 7.04 × 10-23
g
E) 2.82 × 10-22
g
5.14 × 10-8
cell. The lithium ions fit into the holes between the chloride ions. What is the density of the
lithium chloride?
A) 0.520 g/cm3
B) 2.82 g/cm3
C) 2.08 g/cm3
D) 3.11 g/cm3
E) 3.78 g/cm3
edition 33

ANS: C PTS: 1 DIF: difficult REF: 11.9
117. The metal iron crystallizes in a body-centered cubic lattice. If the density of iron is
7.87 g/cm3
, what is the unit cell edge length?
A) 287 pm
B) 77.6 pm
C) 75.0 pm
D) 61.6 pm
E) 228 pm
OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11)
118. The metal barium crystallizes in a body-centered cubic lattice. If the radius of barium is
222 pm, what is the unit cell edge length?
A) 513 pm
B) 444 pm
C) 296 pm
D) 222 pm
E) 96.1 pm
TOP: phases | solid
119. The metal cesium crystallizes in a body-centered cubic lattice. If the density of cesium is
1.88 g/cm3
, what is the unit cell volume?
A) 1.77 × 106
pm3
B) 2.35 × 104
pm3
C) 2.35 × 108
pm3
D) 1.17 × 108
pm3
E) 4.70 × 104
pm3
edition 34

120. Sodium crystallizes in the body-centered cubic system. If the edge of the unit cell is 430 pm,
what is the radius of a sodium atom in picometers?
A) 186 pm
B) 744 pm
C) 992 pm
D) 859 pm
E) 80.5 pm
OBJ: Calculate unit-cell dimension from unit-cell type and edge-length. (Example 11.11)
TOP: phases | solid
121. Copper crystallizes with a face-centered cubic unit cell. If the edge length of the unit cell is
362 pm, what is the radius of a copper atom in picometers?
A) 128 pm
B) 512 pm
C) 1020 pm
D) 296 pm
E) 45.3 pm
OBJ: Calculate unit-cell dimension from unit-cell type and edge-length. (Example 11.11)
TOP: phases | solid
122. What is the simplest formula of the compound represented by the unit cell provided below?
A) AB3
B) AB2
C) AB
D) A2B4
E) A2B6
TOP: phases | solid
edition 35

. What is the volume of the unit cell?
A) 8.18 × 106
pm3
B) 1.12 × 109
pm3
C) 4.42 × 107
pm3
D) 1.95 × 106
pm3
E) 3.27 × 107
pm3
ANS: C PTS: 1 DIF: difficult REF: 11.9
. What is the molar volume of the metal?
A) 98.9 cm3
/mol
B) 24.7 cm3
/mol
C) 86.6 cm3
/mol
D) 33.4 cm3
/mol
E) 0.380 cm3
/mol
ANS: D PTS: 1 DIF: difficult REF: 11.9
125. The metal cesium crystallizes in a body-centered cubic lattice. If the density of cesium is
1.88 g/cm3
, what is the atomic volume of cesium?
A) 1.60 × 104
pm3
B) 7.99 × 103
pm3
C) 3.99 × 107
pm3
D) 6.01 × 105
pm3
E) 7.98 × 107
pm3
126. The metal barium crystallizes in a body-centered cubic lattice. If the density of barium is
3.51 g/cm3
, what is the atomic radius of barium?
A) 15.1 pm
B) 174 pm
C) 42.5 pm
D) 19.0 pm
E) 219 pm
edition 36

5.14 × 10-8
cell. The lithium ions fit into the holes between the chloride ions. What is the radius of the
chloride ion?
A) 2.52 × 10-8
cm
B) 1.82 × 10-8
cm
C) 2.56 × 10-8
cm
D) 1.45 × 10-8
cm
E) 2.82 × 10-8
cm
ANS: B PTS: 1 DIF: difficult REF: 11.9
128. Which of the following statements concerning the determination of crystal structure by x-
ray diffraction is incorrect?
A) X-rays are reflected from the repeating planes of an ordered crystal lattice.
B) A diffraction pattern reveals the locations of the electrons in a crystal.
C) Analysis of a diffraction pattern reveals the structure of a crystal.
D) X-rays undergo constructive and destructive interference upon reflection in a
crystal lattice.
E) A diffraction pattern from a crystal depends on the incident angle of the x-rays.
OBJ: Note that diffraction of x rays from a crystal gives information about the positions of
atoms in the crystal. TOP: phases | solid KEY: x-ray diffraction
edition 37

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