Chapter 11 Review
Student: ___________________________________________________________________________
1.
Helium atoms do not combine to form He2 molecules, yet He atoms do attract one another weakly through
A. dipole-dipole forces.
B. ion-dipole forces.
C. dispersion forces.
D. dipole-induced dipole forces.
E. hydrogen bonding.
2.
The molecular property related to the ease with which the electron density in a neutral atom or molecule can be distorted is
called
A. a dipole moment.
B. polarizability.
C. a dispersion force.
D. surface tension.
E. a van der Waals force.
3.
Which one of the following substances will have both dispersion forces and dipole-dipole forces?
A. HCl
B. BCl3
C. Br2
D. H2
E. CO2
4.
Which one of the following substances should exhibit hydrogen bonding in the liquid state?
A. PH3
B. H2
C. H2S
D. CH4
E. NH3
5.
Which two properties are more typical of molecular compounds than of ionic compounds?
1. They are gases or liquids at room temperature.
2. They have high melting points.
conduct electricity, but liquids do.
4. Atoms share electrons.
A. 1 and 4
B. 1 and 3
C. 2 and 3
D. 2 and 4
E. 3 and 4
6.
Which of the following substances should have the highest boiling point?
A. CH4
B. Cl2
C. Kr
D. CH3Cl
E. N2
7.
Which of the following liquids would have the highest viscosity at 25°C?
A. CH3OCH3
B. CH2Cl2
C. C2H5OH
D. CH3Br
E. HOCH2CH2OH
8.
Which one of the following substances should exhibit hydrogen bonding in the liquid state?
A. SiH4
B. H2
C. H2S
D. CH4
E. CH3NH2
3. Solids do not
9.
Which of the following properties indicates the presence of weak intermolecular forces in a liquid?
A. a high heat of vaporization
B. a high critical temperature
C. a high vapor pressure
D. a high boiling point
E. none of these
10. Which of the following properties indicates the presence of strong intermolecular forces in a liquid?
A. a low heat of vaporization
B. a low critical temperature
C. a low vapor pressure
D. a low boiling point
E. none of these
11. For which of the following species are the intermolecular interactions entirely due to dispersion forces?
A. C2H6
B. CH3OCH3
C. NO2
D. H2S
E. CaNO3
12. For which of the following species are the dispersion forces strongest?
A. C4H10
B. C5H12
C. C6H14
D. C7H16
E. C8H18
13. Each of the following substances is a liquid at -50°C. Place these liquids in order of increasing vapor pressure.
dimethyl ether (CH3OCH3), propane (C3H8), ethanol (CH3CH2OH)
A. ethanol < propane < dimethyl ether
B. ethanol < dimethyl ether < propane
C. propane < dimethyl ether < ethanol
D. dimethyl ether < ethanol < propane
E. propane < ethanol < dimethyl ether
14. Which of the following would be expected to have the highest vapor pressure at room temperature?
A. ethanol, bp = 78°C
B. methanol, bp = 65°C
C. water, bp = 100°C
D. acetone, bp = 56°C
15. Which of the following would be expected to have the lowest vapor pressure at room temperature?
A. ethanol, bp = 78°C
B. methanol, bp = 65°C
C. water, bp = 100°C
D. acetone, bp = 56°C
16. Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point?
A. ethanol, bp = 78°C
B. methanol, bp = 65°C
C. water, bp = 100°C
D. benzene, bp = 80°C
E. The vapor pressure of each of the liquids at its normal boiling point would be the same.
17. Choose the response that lists the member of each of the following pairs that has the higher boiling point.
(I) H2O or KI
(II) HF or HI
(III) Cl2 or Br2
A. H2O, HF, and Cl2
B. KI, HF, and Br2
C. KI, HI, and Br2
D. H2O, HI, and Cl2
E. KI, HF, and Cl2
18. Arrange the following in order of increasing boiling point: RbCl, CH3Cl, CH3OH, CH4.
A. CH3OH < CH3Cl < RbCl < CH4
B. CH3OH < CH4 < CH3Cl < RbCl
C. RbCl < CH3Cl < CH3OH < CH4
D. CH4 < CH3OH < CH3Cl < RbCl
E. CH4 < CH3Cl < CH3OH < RbCl
19. Krypton has a higher melting point than argon because of its
A. hydrogen bonding.
B. stronger dispersion forces.
C. permanent dipole moment.
D. ionic bonds.
E. greater ionization energy.
20. Which one of the following substances should exhibit hydrogen bonding in the liquid state?
A. PH3
B. He
C. H2S
D. CH4
E. CH3OH
21. Which of the responses includes all of the following that can form hydrogen bonds with water molecules?
Na+
(2) CH3COOH
(3) C2H6
(4) CH3NH2
A. (1) and (2)
B. (1) and (3)
C. (2) and (3)
D. (2) and (4)
E. (3) and (4)
(1)
22. Which of the following atoms does not participate in hydrogen bonding?
A. S
B. O
C. F
D. N
23. Each of the following substances is a gas at 25°C and 1 atmosphere pressure. Which one will liquefy most easily when
compressed at a constant temperature?
A. F2
B. H2
C. HF
D. SiH4
E. Ar
24. Which of the following is not true with regard to water?
A. Water has a high heat capacity.
B. Water has an unusually high boiling point.
C. Water can form hydrogen bonds.
D. Ice is more dense than liquid water.
E. Water is a polar molecule.
25. Which property of water allows a razor blade to float on it without sinking?
A. viscosity
B. surface tension
C. density
D. specific heat
E. triple point
26. An example of a covalent network solid is
A. diamond.
B. potassium.
C. iodine.
D. sodium chloride.
E. none of these.
27. Which one of the following is an example of a covalent network solid?
A. SiO2
B. K
C. I2
D. CaCl2
E. none of these
28. The structural form of the element Ge closely resembles the structure of
A. C (diamond).
B. N (diatomic).
C. As (tetrahedral).
D. S (S8 ring).
E. Kr (monatomic).
29. Which one of the following substances crystallizes as a molecular solid?
A. KI
B. SiO2
C. Sn
D. CH3OH
E. Al2(SO4)3
30. Butter melts over a range of temperature, rather than with a sharp melting point. Butter is classified as a/an
A. metallic crystal.
B. covalent solid.
C. molecular crystal.
D. amorphous solid.
E. ionic crystal.
31. Which one of the following substances crystallizes as a covalent crystal?
A. CaO
B. SiO2
C. CO2
D. Pb
E. KMnO4
32. Which one of the following crystallizes in a metallic lattice?
A. C
B. NaMnO4
C. K
D. LiClO4
E. K2Cr2O7
33. The number of atoms in a body-centered cubic unit cell is
A. 1.
B. 2.
C. 3.
D. 4.
E. 8.
34. The number of atoms in a face-centered cubic unit cell is
A. 1.
B. 2.
C. 3.
D. 4.
E. 8.
35. Potassium crystallizes in a body-centered cubic lattice. How many atoms are there per unit cell?
A. 1
B. 2
C. 4
D. 6
E. 8
36. A liquid boils when its
A. vapor pressure is exactly 1 atmosphere.
B. vapor pressure is equal to, or greater than, the external pressure pushing on it.
C. temperature is equal to 273 K (standard temperature).
D. temperature is greater than room temperature.
37. The heat capacity of liquid water is 4.18 J/g·°C and the heat of vaporization is 40.7 kJ/mol. How many kilojoules of heat must
be provided to convert 1.00 g of liquid water at 67°C into 1.00 g of steam at 100°C?
A. 22.7 kJ
B. 40.8 kJ
C. 2.2 kJ
D. 2,400 J
E. 40.8 J
38. Use the graph of vapor pressure to determine the normal boiling point of CHCl3.
A. 19°C
B. 52°C
C. 60°C
D. 64°C
E. 70°C
39. Which of the following is not an endothermic process?
A. melting of a solid
B. vaporization
C. raising the temperature of a gas
D. condensation of water vapor
E. sublimation of dry ice
40. Use the graph of vapor pressure to determine the normal boiling point of O2.
A. 92 K
B. 90 K
C. 88 K
D. 84 K
E. O2 doesn't boil because it is always a gas.
41. Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20°C to convert it to liquid water at 60.0°C. Given:
Specific heat (ice) = 2.1 J/g·°C
Specific heat (water) = 4.18 J/g·°C
ΔHfus = 6.0 kJ/mol
A. 420 J
B. 2,900 J
C. 6,300 J
D. 63 kJ
E. 7.5 J
42. Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1,809 K), given that: ΔH = 13.80 kJ/
fus
mol.
A. 494 kJ
B. 27,600 kJ
C. 27.6 kJ
D. 27,600 J
E. 25,000 kJ
43. The vapor pressure of a liquid in a closed container depends upon
A. the amount of liquid.
B. the surface area of the liquid.
C. the volume of the container.
D. the temperature.
E. none of these.
44. 3.59 g of water was introduced into an evacuated 1.50 L flask at 30°C. What mass of water will evaporate? (Vapor pressure of
water at 30°C is 31.82 mmHg.)
A. 0.0455 g
B. 0.455 g
C. 0.04187 g
D. 2.52 × 10-3 g
E. 0.4187 g
45. Which one of the following elements would have the lowest melting point?
A. Kr
B. Br2
C. S8
D. Ca
E. K
46. Which of the following gases would have the highest critical temperature?
A. CH4
B. O2
C. CO2
D. NH3
E. Ne
47. Octane is a liquid component of gasoline. Given the following vapor pressures of octane at various temperatures, estimate the
boiling point of octane in Leadville, Colorado, where the atmospheric pressure is 496 mmHg.
400 mmHg @ 104°C, 500 mmHg @ 111°C, 600 mmHg @ 117°C,
700 mmHg @ 122°C, 760 mmHg @ 125°C
A. 125°C
B. 120°C
C. 115°C
D. 110°C
E. 105°C
48. The vapor pressure of ethanol is 400 mmHg at 63.5°C. Its molar heat of vaporization is 39.3 kJ/mol. What is vapor pressure of
ethanol, in mmHg, at 34.9°C?
A. 1,510 mmHg
B. 100 mmHg
C. 200 mmHg
D. 0.0099 mmHg
E. 4.61 mmHg
Chapter 11 Review Key
1.
Helium atoms do not combine to form He2 molecules, yet He atoms do attract one another weakly through
A. dipole-dipole forces.
B. ion-dipole forces.
C. dispersion forces.
D. dipole-induced dipole forces.
E. hydrogen bonding.
Difficulty: Medium
Raymond - 011 Intermolecular... #1
2.
The molecular property related to the ease with which the electron density in a neutral atom or molecule can be distorted is
called
A. a dipole moment.
B. polarizability.
C. a dispersion force.
D. surface tension.
E. a van der Waals force.
Difficulty: Easy
Raymond - 011 Intermolecular... #2
3.
Which one of the following substances will have both dispersion forces and dipole-dipole forces?
A. HCl
B. BCl3
C. Br2
D. H2
E. CO2
Difficulty: Medium
Raymond - 011 Intermolecular... #3
4.
Which one of the following substances should exhibit hydrogen bonding in the liquid state?
A. PH3
B. H2
C. H2S
D. CH4
E. NH3
Difficulty: Medium
Raymond - 011 Intermolecular... #4
5.
Which two properties are more typical of molecular compounds than of ionic compounds?
1. They are gases or liquids at room temperature.
2. They have high melting points.
conduct electricity, but liquids do.
4. Atoms share electrons.
A. 1 and 4
B. 1 and 3
C. 2 and 3
D. 2 and 4
E. 3 and 4
3. Solids do not
Difficulty: Medium
Raymond - 011 Intermolecular... #5
6.
Which of the following substances should have the highest boiling point?
A. CH4
B. Cl2
C. Kr
D. CH3Cl
E. N2
Difficulty: Medium
Raymond - 011 Intermolecular... #6
7.
Which of the following liquids would have the highest viscosity at 25°C?
A. CH3OCH3
B. CH2Cl2
C. C2H5OH
D. CH3Br
E. HOCH2CH2OH
Difficulty: Medium
Raymond - 011 Intermolecular... #7
8.
Which one of the following substances should exhibit hydrogen bonding in the liquid state?
A. SiH4
B. H2
C. H2S
D. CH4
E. CH3NH2
Difficulty: Medium
Raymond - 011 Intermolecular... #21
9.
Which of the following properties indicates the presence of weak intermolecular forces in a liquid?
A. a high heat of vaporization
B. a high critical temperature
C. a high vapor pressure
D. a high boiling point
E. none of these
Difficulty: Easy
Raymond - 011 Intermolecular... #9
10.
Which of the following properties indicates the presence of strong intermolecular forces in a liquid?
A. a low heat of vaporization
B. a low critical temperature
C. a low vapor pressure
D. a low boiling point
E. none of these
Difficulty: Easy
Raymond - 011 Intermolecular... #10
11.
For which of the following species are the intermolecular interactions entirely due to dispersion forces?
A. C2H6
B. CH3OCH3
C. NO2
D. H2S
E. CaNO3
Difficulty: Medium
Raymond - 011 Intermolecular... #11
12.
For which of the following species are the dispersion forces strongest?
A. C4H10
B. C5H12
C. C6H14
D. C7H16
E. C8H18
Difficulty: Medium
Raymond - 011 Intermolecular... #12
13.
Each of the following substances is a liquid at -50°C. Place these liquids in order of increasing vapor pressure.
dimethyl ether (CH3OCH3), propane (C3H8), ethanol (CH3CH2OH)
A. ethanol < propane < dimethyl ether
B. ethanol < dimethyl ether < propane
C. propane < dimethyl ether < ethanol
D. dimethyl ether < ethanol < propane
E. propane < ethanol < dimethyl ether
Difficulty: Medium
Raymond - 011 Intermolecular... #13
14.
Which of the following would be expected to have the highest vapor pressure at room temperature?
A. ethanol, bp = 78°C
B. methanol, bp = 65°C
C. water, bp = 100°C
D. acetone, bp = 56°C
Difficulty: Medium
Raymond - 011 Intermolecular... #14
15.
Which of the following would be expected to have the lowest vapor pressure at room temperature?
A. ethanol, bp = 78°C
B. methanol, bp = 65°C
C. water, bp = 100°C
D. acetone, bp = 56°C
Difficulty: Medium
Raymond - 011 Intermolecular... #15
16.
Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point?
A. ethanol, bp = 78°C
B. methanol, bp = 65°C
C. water, bp = 100°C
D. benzene, bp = 80°C
E. The vapor pressure of each of the liquids at its normal boiling point would be the same.
Difficulty: Medium
Raymond - 011 Intermolecular... #16
17.
Choose the response that lists the member of each of the following pairs that has the higher boiling point.
(I) H2O or KI
(II) HF or HI
(III) Cl2 or Br2
A. H2O, HF, and Cl2
B. KI, HF, and Br2
C. KI, HI, and Br2
D. H2O, HI, and Cl2
E. KI, HF, and Cl2
Difficulty: Medium
Raymond - 011 Intermolecular... #17
18.
Arrange the following in order of increasing boiling point: RbCl, CH3Cl, CH3OH, CH4.
A. CH3OH < CH3Cl < RbCl < CH4
B. CH3OH < CH4 < CH3Cl < RbCl
C. RbCl < CH3Cl < CH3OH < CH4
D. CH4 < CH3OH < CH3Cl < RbCl
E. CH4 < CH3Cl < CH3OH < RbCl
Difficulty: Medium
Raymond - 011 Intermolecular... #18
19.
Krypton has a higher melting point than argon because of its
A. hydrogen bonding.
B. stronger dispersion forces.
C. permanent dipole moment.
D. ionic bonds.
E. greater ionization energy.
Difficulty: Medium
Raymond - 011 Intermolecular... #19
20.
Which one of the following substances should exhibit hydrogen bonding in the liquid state?
A. PH3
B. He
C. H2S
D. CH4
E. CH3OH
Difficulty: Medium
Raymond - 011 Intermolecular... #20
21.
Which of the responses includes all of the following that can form hydrogen bonds with water molecules?
Na+
(2) CH3COOH
(3) C2H6
(4) CH3NH2
A. (1) and (2)
B. (1) and (3)
C. (2) and (3)
D. (2) and (4)
E. (3) and (4)
(1)
Difficulty: Medium
Raymond - 011 Intermolecular... #22
22.
Which of the following atoms does not participate in hydrogen bonding?
A. S
B. O
C. F
D. N
Difficulty: Easy
Raymond - 011 Intermolecular... #23
23.
Each of the following substances is a gas at 25°C and 1 atmosphere pressure. Which one will liquefy most easily when
compressed at a constant temperature?
A. F2
B. H2
C. HF
D. SiH4
E. Ar
Difficulty: Medium
Raymond - 011 Intermolecular... #25
24.
Which of the following is not true with regard to water?
A. Water has a high heat capacity.
B. Water has an unusually high boiling point.
C. Water can form hydrogen bonds.
D. Ice is more dense than liquid water.
E. Water is a polar molecule.
Difficulty: Medium
Raymond - 011 Intermolecular... #26
25.
Which property of water allows a razor blade to float on it without sinking?
A. viscosity
B. surface tension
C. density
D. specific heat
E. triple point
Difficulty: Medium
Raymond - 011 Intermolecular... #27
26.
An example of a covalent network solid is
A. diamond.
B. potassium.
C. iodine.
D. sodium chloride.
E. none of these.
Difficulty: Medium
Raymond - 011 Intermolecular... #28
27.
Which one of the following is an example of a covalent network solid?
A. SiO2
B. K
C. I2
D. CaCl2
E. none of these
Difficulty: Medium
Raymond - 011 Intermolecular... #29
28.
The structural form of the element Ge closely resembles the structure of
A. C (diamond).
B. N (diatomic).
C. As (tetrahedral).
D. S (S8 ring).
E. Kr (monatomic).
Difficulty: Medium
Raymond - 011 Intermolecular... #30
29.
Which one of the following substances crystallizes as a molecular solid?
A. KI
B. SiO2
C. Sn
D. CH3OH
E. Al2(SO4)3
Difficulty: Medium
Raymond - 011 Intermolecular... #31
30.
Butter melts over a range of temperature, rather than with a sharp melting point. Butter is classified as a/an
A. metallic crystal.
B. covalent solid.
C. molecular crystal.
D. amorphous solid.
E. ionic crystal.
Difficulty: Medium
Raymond - 011 Intermolecular... #32
31.
Which one of the following substances crystallizes as a covalent crystal?
A. CaO
B. SiO2
C. CO2
D. Pb
E. KMnO4
Difficulty: Medium
Raymond - 011 Intermolecular... #33
32.
Which one of the following crystallizes in a metallic lattice?
A. C
B. NaMnO4
C. K
D. LiClO4
E. K2Cr2O7
Difficulty: Medium
Raymond - 011 Intermolecular... #34
33.
The number of atoms in a body-centered cubic unit cell is
A. 1.
B. 2.
C. 3.
D. 4.
E. 8.
Difficulty: Medium
Raymond - 011 Intermolecular... #35
34.
The number of atoms in a face-centered cubic unit cell is
A. 1.
B. 2.
C. 3.
D. 4.
E. 8.
Difficulty: Medium
Raymond - 011 Intermolecular... #36
35.
Potassium crystallizes in a body-centered cubic lattice. How many atoms are there per unit cell?
A. 1
B. 2
C. 4
D. 6
E. 8
Difficulty: Medium
Raymond - 011 Intermolecular... #39
36.
A liquid boils when its
A. vapor pressure is exactly 1 atmosphere.
B. vapor pressure is equal to, or greater than, the external pressure pushing on it.
C. temperature is equal to 273 K (standard temperature).
D. temperature is greater than room temperature.
Difficulty: Medium
Raymond - 011 Intermolecular... #50
37.
The heat capacity of liquid water is 4.18 J/g·°C and the heat of vaporization is 40.7 kJ/mol. How many kilojoules of heat
must be provided to convert 1.00 g of liquid water at 67°C into 1.00 g of steam at 100°C?
A. 22.7 kJ
B. 40.8 kJ
C. 2.2 kJ
D. 2,400 J
E. 40.8 J
Difficulty: Medium
Raymond - 011 Intermolecular... #51
38.
Use the graph of vapor pressure to determine the normal boiling point of CHCl3.
A.
B.
C.
D.
E.
19°C
52°C
60°C
64°C
70°C
Difficulty: Medium
Raymond - 011 Intermolecular... #52
39.
Which of the following is not an endothermic process?
A. melting of a solid
B. vaporization
C. raising the temperature of a gas
D. condensation of water vapor
E. sublimation of dry ice
Difficulty: Easy
Raymond - 011 Intermolecular... #53
40.
Use the graph of vapor pressure to determine the normal boiling point of O2.
A.
B.
C.
D.
E.
92 K
90 K
88 K
84 K
O2 doesn't boil because it is always a gas.
Difficulty: Medium
Raymond - 011 Intermolecular... #55
41.
Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20°C to convert it to liquid water at 60.0°C. Given:
Specific heat (ice) = 2.1 J/g·°C
Specific heat (water) = 4.18 J/g·°C
ΔHfus = 6.0 kJ/mol
A. 420 J
B. 2,900 J
C. 6,300 J
D. 63 kJ
E. 7.5 J
Difficulty: Medium
Raymond - 011 Intermolecular... #56
42.
Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1,809 K), given that: ΔHfus = 13.80 kJ/
mol.
A. 494 kJ
B. 27,600 kJ
C. 27.6 kJ
D. 27,600 J
E. 25,000 kJ
Difficulty: Medium
Raymond - 011 Intermolecular... #57
43.
The vapor pressure of a liquid in a closed container depends upon
A. the amount of liquid.
B. the surface area of the liquid.
C. the volume of the container.
D. the temperature.
E. none of these.
Difficulty: Medium
Raymond - 011 Intermolecular... #60
44.
3.59 g of water was introduced into an evacuated 1.50 L flask at 30°C. What mass of water will evaporate? (Vapor
pressure of water at 30°C is 31.82 mmHg.)
A. 0.0455 g
B. 0.455 g
C. 0.04187 g
D. 2.52 × 10-3 g
E. 0.4187 g
Difficulty: Medium
Raymond - 011 Intermolecular... #63
45.
Which one of the following elements would have the lowest melting point?
A. Kr
B. Br2
C. S8
D. Ca
E. K
Difficulty: Easy
Raymond - 011 Intermolecular... #64
46.
Which of the following gases would have the highest critical temperature?
A. CH4
B. O2
C. CO2
D. NH3
E. Ne
Difficulty: Medium
Raymond - 011 Intermolecular... #65
47.
Octane is a liquid component of gasoline. Given the following vapor pressures of octane at various temperatures, estimate
the boiling point of octane in Leadville, Colorado, where the atmospheric pressure is 496 mmHg.
400 mmHg @ 104°C, 500 mmHg @ 111°C, 600 mmHg @ 117°C,
700 mmHg @ 122°C, 760 mmHg @ 125°C
A. 125°C
B. 120°C
C. 115°C
D. 110°C
E. 105°C
Difficulty: Medium
Raymond - 011 Intermolecular... #67
48.
The vapor pressure of ethanol is 400 mmHg at 63.5°C. Its molar heat of vaporization is 39.3 kJ/mol. What is vapor
pressure of ethanol, in mmHg, at 34.9°C?
A. 1,510 mmHg
B. 100 mmHg
C. 200 mmHg
D. 0.0099 mmHg
E. 4.61 mmHg
Difficulty: Medium
Raymond - 011 Intermolecular... #61
Chapter 11 Review Summary
Category
Difficulty: Easy
Difficulty: Medium
Raymond - 011 Intermolecular...
# of Questions
6
42
48