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Chemistry: The Central Science, 12e (Brown et al.)
Chapter 11 Liquids and Intermolecular Forces
11.1 Multiple-Choice Questions
1) Crystalline solids __________.
A) have their particles arranged randomly
B) have highly ordered structures
C) are usually very soft
D) exist only at high temperatures
E) exist only at very low temperatures
2) In liquids, the attractive intermolecular forces are __________.
A) very weak compared with kinetic energies of the molecules
B) strong enough to hold molecules relatively close together
C) strong enough to keep the molecules confined to vibrating about their fixed lattice points
D) not strong enough to keep molecules from moving past each other
E) strong enough to hold molecules relatively close together but not strong enough to keep molecules
from moving past each other
3) As a solid element melts, the atoms become __________ and they have __________ attraction for
one another.
A) more separated, more
B) more separated, less
C) closer together, more
D) closer together, less
E) larger, greater
4) As a gaseous element condenses, the atoms become __________ and they have __________
attraction for one another.
A) more separated, more
B) more separated, less
C) closer together, more
D) closer together, less
E) larger, greater
5) A gas is __________ and assumes __________ of its container whereas a liquid is __________ and
assumes __________ of its container.
A) compressible, the volume and shape, not compressible, the shape of a portion
B) compressible, the shape, not compressible, the volume and shape
C) compressible, the volume and shape, compressible, the volume
D) condensed, the volume and shape, condensed, the volume and shape
E) condensed, the shape, compressible, the volume and shape
6) Together, liquids and solids constitute __________ phases of matter.
A) the compressible
B) the fluid
C) the condensed
D) all of the
E) the disordered
7) Which statement is true about liquids but not true about solids?
A) They flow and are highly ordered.
B) They are highly ordered and not compressible.
C) They flow and are compressible.
D) They assume both the volume and the shape of their containers.
E) They flow and are not compressible.
8) The strongest interparticle attractions exist between particles of a __________ and the weakest
interparticle attractions exist between particles of a __________.
A) solid, liquid
B) solid, gas
C) liquid, gas
D) liquid, solid
E) gas, solid
9) Which one of the following exhibits dipole-dipole attraction between molecules?
A) XeF4
B) AsH3
C) CO2
D) BCl3
E) Cl2
10) Which one of the following exhibits dipole-dipole attraction between molecules?
A) PH3
B) CCl4
C) Br2
D) CO2
E) C10H22
11) Of the following substances, only __________ has London dispersion forces as its only
intermolecular force.
A) CH3OH
B) NH3
C) H2S
D) CH4
E) HCl
12) Of the following substances, only __________ has London dispersion forces as its only
intermolecular force.
A) H2O
B) CCl4
C) HF
D) CH3COOH
E) PH3
13) Of the following substances, only __________ has London dispersion forces as the only
intermolecular force.
A) CH3OH
B) NH3
C) H2S
D) Kr
E) HCl
14) Which one of the following should have the lowest boiling point?
A) PH3
B) H2S
C) HCl
D) SiH4
E) H2O
15) Which one of the following should have the lowest boiling point?
A) CH3OH
B) H2S
C) NH3
D) HCl
E) CH4
16) Of the following substances, __________ has the highest boiling point.
A) H2O
B) CO2
C) CH4
D) Kr
E) NH3
17) Of the following substances, __________ has the highest boiling point.
A) CH3CH2OH
B) C2H6
C) N2
D) F2
E) HOCH2CH2OH
18) Of the following, __________ has the highest boiling point.
A) N2
B) Br2
C) H2
D) Cl2
E) O2
19) In which of the following molecules is hydrogen bonding likely to be the most significant
component of the total intermolecular forces?
A) CH4
B) C5H11OH
C) C6H13NH2
D) CH3OH
E) CO2
20) Which of the following has dispersion forces as its only intermolecular force?
A) CH4
B) HCl
C) C6H13NH2
D) NaCl
E) CH3Cl
21) When NaCl dissolves in water, aqueous Na+ and Cl- ions result. The force of attraction that exists
between Na+ and H2O is called a(n) __________ interaction.
A) dipole-dipole
B) ion-ion
C) hydrogen bonding
D) ion-dipole
E) London dispersion force
22) __________ are particularly polarizable.
A) Small nonpolar molecules
B) Small polar molecules
C) Large nonpolar molecules
D) Large polar molecules
E) Large molecules, regardless of their polarity,
23) The ease with which the charge distribution in a molecule can be distorted by an external electrical
field is called the __________.
A) electronegativity
B) hydrogen bonding
C) polarizability
D) volatility
E) viscosity
24) Which one of the following derivatives of ethane has the highest boiling point?
A) C2Br6
B) C2F6
C) C2I6
D) C2Cl6
E) C2H6
25) What is the predominant intermolecular force in CBr4?
A) London-dispersion forces
B) ion-dipole attraction
C) ionic bonding
D) dipole-dipole attraction
E) hydrogen-bonding
26) What is the predominant intermolecular force in CH3CH2OH?
A) London-dispersion forces
B) ion-dipole attraction
C) ionic bonding
D) induced dipole-dipole attraction
E) hydrogen-bonding
27) The intermolecular force(s) responsible for the fact that CH4 has the lowest boiling point in the set
CH4, SiH4, GeH4, SnH4 is/are __________.
A) hydrogen bonding
B) dipole-dipole interactions
C) London dispersion forces
D) mainly hydrogen bonding but also dipole-dipole interactions
E) mainly London-dispersion forces but also dipole-dipole interactions
28) Elemental iodine (I2) is a solid at room temperature. What is the major attractive force that exists
among different I2 molecules in the solid?
A) London dispersion forces
B) dipole-dipole rejections
C) ionic-dipole interactions
D) covalent-ionic interactions
E) dipole-dipole attractions
29) Hydrogen bonding is a special case of __________.
A) London-dispersion forces
B) ion-dipole attraction
C) dipole-dipole attractions
D) ion-ion interactions
E) none of the above
30) Which one of the following substances will have hydrogen bonding as one of its intermolecular
forces?
A)
B)
C)
D)
E)
31) Which one of the following substances will not have hydrogen bonding as one of its intermolecular
forces?
A)
B)
C)
D)
E)
32) What intermolecular force is responsible for the fact that ice is less dense than liquid water?
A) London dispersion forces
B) dipole-dipole forces
C) ion-dipole forces
D) hydrogen bonding
E) ionic bonding
33) The predominant intermolecular force in (CH3)2NH is __________.
A) London dispersion forces
B) ion-dipole forces
C) ionic bonding
D) dipole-dipole forces
E) hydrogen bonding
34) The predominant intermolecular force in AsH3 is __________.
A) London dispersion forces
B) ion-dipole forces
C) ionic bonding
D) dipole-dipole forces
E) hydrogen bonding
35) C12H26 molecules are held together by __________.
A) ion-ion interactions
B) hydrogen bonding
C) ion-dipole interactions
D) dipole-dipole interactions
E) dispersion forces
36) Which of the following molecules has hydrogen bonding as its only intermolecular force?
A) HF
B) H2O
C) C6H13NH2
D) C5H11OH
E) None, all of the above exhibit dispersion forces.
37) Which of the following molecules has hydrogen bonding as its only intermolecular force?
A) NH3
B) H2O
C) C3H7OH
D) HOCH2CH2OH
E) None, all of the above exhibit dispersion forces.
38) What types of intermolecular forces exist between HI and H2S?
A) dipole-dipole and ion-dipole
B) dispersion forces, dipole-dipole, and ion-dipole
C) dispersion forces, hydrogen bonding, dipole-dipole, and ion-dipole
D) dispersion forces and dipole-dipole
E) dispersion forces, dipole-dipole, and ion-dipole
39) What type(s) of intermolecular forces exist between Br2 and CCl4?
A) dispersion forces
B) dispersion forces and ion-dipole
C) dispersion forces and dipole-dipole
D) dispersion forces, ion-dipole, and dipole-dipole
E) None. Since both are gases at room temperature, they do not interact with each other.
40) What type(s) of intermolecular forces exist between Cl2 and CO3-2?
A) dispersion forces
B) dispersion forces and ion-dipole
C) dispersion forces, ion-dipole, and induced dipole - induced dipole
D) dispersion forces and ion-induced dipole
E) dispersion forces, ion-dipole, dipole-dipole, and ion-induced dipole
41) What types of intermolecular forces exist between NH3 and CBr4?
A) dispersion forces and dipole-dipole forces
B) dispersion forces and dipole-induced dipole forces
C) dispersion forces and hydrogen bonds
D) dispersion forces, hydrogen bonds, and induced dipole-induced dipole forces
E) dispersion forces, hydrogen bonds, and dipole-induced dipole forces
42) What types of intermolecular forces exist between PH3 and N2?
A) dispersion forces and dipole-dipole forces
B) dispersion forces and dipole-induced dipole forces
C) dispersion forces and hydrogen bonds
D) dispersion forces, hydrogen bonds, and induced dipole-induced dipole forces
E) dispersion forces, hydrogen bonds, and dipole-induced dipole forces
43) __________ is the energy required to expand the surface area of a liquid by a unit amount of area.
A) Viscosity
B) Surface tension
C) Volatility
D) Meniscus
E) Capillary action
44) Which statements about viscosity are true?
(i) Viscosity increases as temperature decreases.
(ii) Viscosity increases as molecular weight increases.
(iii) Viscosity increases as intermolecular forces increase.
A) (i) only
B) (ii) and (iii)
C) (i) and (iii)
D) none
E) all
45) The shape of a liquid's meniscus is determined by __________.
A) the viscosity of the liquid
B) the type of material the container is made of
C) the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its
container
D) the amount of hydrogen bonding in the liquid
E) the volume of the liquid
46) Viscosity is __________.
A) the "skin" on a liquid surface caused by intermolecular attraction
B) the resistance to flow
C) the same as density
D) inversely proportional to molar mass
E) unaffected by temperature
47) How high a liquid will rise up a narrow tube as a result of capillary action depends on __________.
A) the magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the tube,
and gravity
B) gravity alone
C) only the magnitude of adhesive forces between the liquid and the tube
D) the viscosity of the liquid
E) only the magnitude of cohesive forces in the liquid
48) The property responsible for the "beading up" of water is __________.
A) density
B) viscosity
C) vapor pressure
D) surface tension
E) hydrogen bonding
49) Heat of sublimation can be approximated by adding together __________ and __________.
A) heat of fusion, heat of condensation
B) heat of fusion, heat of vaporization
C) heat of freezing (solidification), heat of condensation
D) heat of freezing (solidification), heat of vaporization
E) heat of deposition, heat of vaporization
50) Which of the following statements is false?
A) The absolute value of the heat of sublimation is equal to the absolute value of the heat of deposition.
B) The heat of sublimation is equal to the sum of the heat of vaporization and the heat of melting.
C) The heat of sublimation is equal to the sum of the heat of vaporization and the heat of freezing.
D) The absolute value of the heat of sublimation is equal to the absolute value of the sum of the heat of
condensation and the heat of freezing.
E) The absolute value of the heat of deposition is equal to sum of the absolute value of the heat of
vaporization and the absolute value of the heat of freezing.
51) The phase changes B → C and D → E are not associated with temperature increases because the
heat energy is used up to __________.
A) increase distances between molecules
B) break intramolecular bonds
C) rearrange atoms within molecules
D) increase the velocity of molecules
E) increase the density of the sample
52) Based on the following information, which compound has the strongest intermolecular forces?
Substance ΔHvap(kJ/mol)
Argon (Ar) 6.3
Benzene (C6H6) 31.0
Ethanol (C2H5OH) 39.3
Water (H2O) 40.8
Methane (CH4) 9.2
A) Argon
B) Benzene
C) Ethanol
D) Water
E) Methane
53) Which compound has the strongest intermolecular forces?
A) CBr4
B) C12H26
C) CI4
D) N2
E) O2
54) Large intermolecular forces in a substance are manifested by __________.
A) low vapor pressure
B) high boiling point
C) high heats of fusion and vaporization
D) high critical temperatures and pressures
E) all of the above
55) A substance that expands to fill its container yet has a density approaching that of a liquid, and that
can behave as a solvent is called a(n) __________.
A) plasma
B) gas
C) liquid
D) amorphous solid
E) supercritical fluid and gas
56) The critical temperature and pressure of CS2 are 279°C and 78 atm, respectively. At temperatures
above 279°C and pressures above 78 atm, CS2 can only occur as a __________.
A) solid
B) liquid
C) liquid and gas
D) gas
E) supercritical fluid
57) The substance with the largest heat of vaporization is __________.
A) I2
B) Br2
C) Cl2
D) F2
E) O2
58) Of the following, __________ is an exothermic process.
A) melting
B) subliming
C) freezing
D) boiling
E) All of the above are exothermic.
59) Of the following, __________ should have the highest critical temperature.
A) CBr4
B) CCl4
C) CF4
D) CH4
E) H2
60) Of the following, __________ is the most volatile.
A) CBr4
B) CCl4
C) CF4
D) CH4
E) C6H14
61) Of the following, __________ is the least volatile.
A) CBr4
B) CCl4
C) CF4
D) CH4
E) C6H14
62) A volatile liquid is one that __________.
A) is highly flammable
B) is highly viscous
C) is highly hydrogen-bonded
D) is highly cohesive
E) readily evaporates
63) In general, the vapor pressure of a substance increases as __________ increases.
A) surface tension
B) molecular weight
C) hydrogen bonding
D) viscosity
E) temperature
64) The vapor pressure of any substance at its normal boiling point is
A) 1 Pa
B) 1 torr
C) 1 atm
D) equal to atmospheric pressure
E) equal to the vapor pressure of water
65) Volatility and vapor pressure are __________.
A) inversely proportional to one another
B) directly proportional to one another
C) not related
D) the same thing
E) both independent of temperature
