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Chapter 13Intermolecular Forces,
Liquids, and Solids
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Which of the following molecules can hydrogen bond with itself?
1. 1, 22. 2, 33. 3, 44. 1, 2, 35. 1, 2, 3, 4
CH2F2 NH3 CH3-O-H CH3C CH3
O
1 2 3 4
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Which of the following molecules can hydrogen bond with itself?
1. 1, 22. 2, 33. 3, 44. 1, 2, 35. 1, 2, 3, 4
CH2F2 NH3 CH3-O-H CH3C CH3
O
1 2 3 4
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Arrange the following according to increasing melting point.
1. O2 < He < I2 < Kr
2. He < O2 < I2 < Kr
3. He < O2 < Kr < I2
4. I2 < Kr < O2 < He
5. I2 < Kr < He < O2
Kr I2 O2 He
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Arrange the following according to increasing melting point.
1. O2 < He < I2 < Kr
2. He < O2 < I2 < Kr
3. He < O2 < Kr < I2
4. I2 < Kr < O2 < He
5. I2 < Kr < He < O2
Kr I2 O2 He
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Arrange the following according to increasing melting point.
1. MgO < H2O < CO2 < O2
2. O2 < CO2 < H2O < MgO
3. O2 < H2O < CO2 < MgO
4. H2O < O2 < MgO < CO2
5. O2 < CO2 < H2O < MgO
MgO CO2 O2 H2O
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Arrange the following according to increasing melting point.
1. MgO < H2O < CO2 < O2
2. O2 < CO2 < H2O < MgO
3. O2 < H2O < CO2 < MgO
4. H2O < O2 < MgO < CO2
5. O2 < CO2 < H2O < MgO
MgO CO2 O2 H2O
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Arrange the following according to increasing vapor pressure.
1. NH3 < I2 < Br2 < CH4
2. I2 < Br2 < NH3 < CH4
3. NH3 < CH4 < I2 < Br2
4. NH3 < I2 < CH4 < Br2
5. CH4 < NH3 < Br2 < I2
NH3 I2 Br2 CH4
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Arrange the following according to increasing vapor pressure.
1. NH3 < I2 < Br2 < CH4
2. I2 < Br2 < NH3 < CH4
3. NH3 < CH4 < I2 < Br2
4. NH3 < I2 < CH4 < Br2
5. CH4 < NH3 < Br2 < I2
NH3 I2 Br2 CH4
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Which does not represent close packing?
1. ABABAB2. ABCABC3. ABACBAC 4. AABCABB5. CACBABC
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Which does not represent close packing?
1. ABABAB2. ABCABC3. ABACBAC 4. AABCABB5. CACBABC
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Which statement is true?
1. Boiling point ~120°C2. Boiling point ~95°C 3. Boiling point ~75°C4. Melting point ~95°C5. Melting point ~75°C
0
200
400
600
800
Vap
or
Pre
ssu
re (
mm
Hg
)
25 50 75 100Temperature (° C)
0
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Which statement is true?
1. Boiling point ~120°C2. Boiling point ~95°C 3. Boiling point ~75°C4. Melting point ~95°C5. Melting point ~75°C
0
200
400
600
800
Vap
or
Pre
ssu
re (
mm
Hg
)
25 50 75 100Temperature (° C)
0
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Lead crystallizes in a face-centered cubic unit cell. How many lead atoms are in one unit cell?
1. 12. 23. 44. 105. 14
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Lead crystallizes in a face-centered cubic unit cell. How many lead atoms are in one unit cell?
1. 12. 23. 44. 105. 14
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1. 22. 43. 64. 85. 14
How many tetrahedral holes are in a face- centered cubic unit cell?
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1. 22. 43. 64. 85. 14
How many tetrahedral holes are in a face- centered cubic unit cell?
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Of the following substances, predict which has the highest boiling point based on intermolecular forces.
1. Propane, C3H8
2. Dimethyl ether, CH3OCH3
3. Methyl chloride, CH3Cl4. Acetaldehyde, CH3CHO5. Acetonitrile, CH3CN
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Of the following substances, predict which has the highest boiling point based on intermolecular forces.
1. Propane, C3H8
2. Dimethyl ether, CH3OCH3
3. Methyl chloride, CH3Cl4. Acetaldehyde, CH3CHO5. Acetonitrile, CH3CN
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Correct Answer:
Each of these molecules has almost the same molecular weight; however, acetonitrile has the largest dipole moment (3.9 D) and hence the largest dipole-dipole forces. Thus it has the highest boiling point.
1. Propane, C3H8
2. Dimethyl ether, CH3OCH3
3. Methyl chloride, CH3Cl4. Acetaldehyde, CH3CHO5. Acetonitrile, CH3CN
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Of the following substances, predict which has the lowest boiling point based on London dispersion forces.
1. He2. Ne3. Ar4. Kr5. Xe
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Correct Answer:
More massive species have more polarizability and stronger London dispersion forces; consequently, amongst the noble gases He has the lowest boiling point.
1. He2. Ne3. Ar4. Kr5. Xe
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Of the following substances, predict which has the highest boiling point based upon intermolecular forces?
1. CH4
2. H2O3. H2S4. SiH4
5. H2Se
NH ……. O=C
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Correct Answer:
Of these, only H2O has any hydrogen bonding. Hydrogen bonding substantially increases the intermolecular forces, and hence the boiling point.
1. CH4
2. H2O3. H2S4. SiH4
5. H2Se
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Which one of the following phase changes is an exothermic process?
1. Sublimation2. Vaporization3. Condensation4. Melting
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Correct Answer:
All the other phase-change processes listed are endothermic.
1. Sublimation2. Vaporization3. Condensation4. Melting
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How much energy is required to raise the temperature of 1800. g ice at 0°C to 10°C? Hfus = 6.01 kJ/mol, heat capacity of water is 75.2 J/mol-K.
1. 60.1 kJ2. 75.2 kJ3. 135 kJ4. 601 kJ5. 676 kJ
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Correct Answer:
There are 100 moles of ice, so the enthalpy of fusion is:H =(6.01 kJ/mol)(100 mol) = 601 kJ.To raise the water temperature 10°C requires q = (75.2 J/mol-K)(100 mol)(10°C ) = 75.2 kJ. Total energy = 601 kJ +75 kJ = 676 kJ
1. 60.1 kJ2. 75.2 kJ3. 135 kJ4. 601 kJ5. 676 kJ
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Temperature
Pre
ssu
reAA
DD
CC
BB
In the unlabeled phase diagram below, the line segment from A to B separates which two phases?
1. Gas-liquid2. Liquid-solid3. Solid-gas
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Correct Answer:
1. Gas-liquid2. Liquid-solid3. Solid-gas
Temperature
Pre
ssu
reAA
DD
CC
BB
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Quartz is an example of which type of solid: crystalline or amorphous?
1. Crystalline2. Amorphous
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Correct Answer:
In quartz, the SiO bonds are arranged in regular, defined arrays.
1. Crystalline2. Amorphous
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What are the net number of Na+ and Cl ions in the NaCl unit cell represented below?
1. 4 Na+, 4 Cl
2. 2 Na+, 1 Cl
3. 2 Na+, 2 Cl
4. 1 Na+, 2 Cl
5. 1 Na+, 1 Cl
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Correct Answer:
There are 4 Na+ resulting from: (1/4 Na+/edge)(12 edges) = 3 Na+
(1 Na+/center)(1 center) = 1 Na+
There are 4 Cl− resulting from:
(1/8 Cl/corner)(8 corners) = 1 Cl
(1/2 Cl/face)(6 faces) = 3 Cl
1. 4 Na+, 4 Cl
2. 2 Na+, 1 Cl
3. 2 Na+, 2 Cl
4. 1 Na+, 2 Cl
5. 1 Na+, 1 Cl
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The NaCl crystal shown below is an example of which type of cubic lattice?
1. Primitive cubic2. Body-centered
cubic3. Face-centered
cubic
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Correct Answer:
NaCl is an example
of a face-centered
crystalline lattice.
1. Primitive cubic2. Body-centered
cubic3. Face-centered
cubic
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Diamond and graphite are examples of which type of crystalline solids?
1. Molecular2. Covalent network3. Ionic4. Metallic
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Correct Answer:
Diamond and graphite are both forms of carbon, and consist of a network of covalent bonds (hence covalent network).
1. Molecular2. Covalent network3. Ionic4. Metallic
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Correct Answer:
Each of these molecules has almost the same molecular weight; however, acetonitrile has the largest dipole moment (3.9 D) and hence the largest dipole-dipole forces. Thus it has the highest boiling point.
1. Propane, C3H8
2. Dimethyl ether, CH3OCH3
3. Methyl chloride, CH3Cl4. Acetaldehyde, CH3CHO5. Acetonitrile, CH3CN
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Of the following substances, predict which has the lowest boiling point based on London dispersion forces.
1. He2. Ne3. Ar4. Kr5. Xe
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Correct Answer:
More massive species have more polarizability and stronger London dispersion forces; consequently, amongst the noble gases He has the lowest boiling point.
1. He2. Ne3. Ar4. Kr5. Xe
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Of the following substances, predict which has the highest boiling point based upon intermolecular forces?
1. CH4
2. H2O3. H2S4. SiH4
5. H2Se
NH ……. O=C
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Correct Answer:
Of these, only H2O has any hydrogen bonding. Hydrogen bonding substantially increases the intermolecular forces, and hence the boiling point.
1. CH4
2. H2O3. H2S4. SiH4
5. H2Se
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Which one of the following phase changes is an exothermic process?
1. Sublimation2. Vaporization3. Condensation4. Melting
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Correct Answer:
All the other phase-change processes listed are endothermic.
1. Sublimation2. Vaporization3. Condensation4. Melting
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How much energy is required to raise the temperature of 1800. g ice at 0°C to 10°C? Hfus = 6.01 kJ/mol, heat capacity of water is 75.2 J/mol-K.
1. 60.1 kJ2. 75.2 kJ3. 135 kJ4. 601 kJ5. 676 kJ
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Correct Answer:
There are 100 moles of ice, so the enthalpy of fusion is:H =(6.01 kJ/mol)(100 mol) = 601 kJ.To raise the water temperature 10°C requires q = (75.2 J/mol-K)(100 mol)(10°C ) = 75.2 kJ. Total energy = 601 kJ +75 kJ = 676 kJ
1. 60.1 kJ2. 75.2 kJ3. 135 kJ4. 601 kJ5. 676 kJ
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Temperature
Pre
ssu
reAA
DD
CC
BB
In the unlabeled phase diagram below, the line segment from A to B separates which two phases?
1. Gas-liquid2. Liquid-solid3. Solid-gas
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Correct Answer:
1. Gas-liquid2. Liquid-solid3. Solid-gas
Temperature
Pre
ssu
reAA
DD
CC
BB
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Quartz is an example of which type of solid: crystalline or amorphous?
1. Crystalline2. Amorphous
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Correct Answer:
In quartz, the SiO bonds are arranged in regular, defined arrays.
1. Crystalline2. Amorphous
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What are the net number of Na+ and Cl ions in the NaCl unit cell represented below?
1. 4 Na+, 4 Cl
2. 2 Na+, 1 Cl
3. 2 Na+, 2 Cl
4. 1 Na+, 2 Cl
5. 1 Na+, 1 Cl
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Correct Answer:
There are 4 Na+ resulting from: (1/4 Na+/edge)(12 edges) = 3 Na+
(1 Na+/center)(1 center) = 1 Na+
There are 4 Cl− resulting from:
(1/8 Cl/corner)(8 corners) = 1 Cl
(1/2 Cl/face)(6 faces) = 3 Cl
1. 4 Na+, 4 Cl
2. 2 Na+, 1 Cl
3. 2 Na+, 2 Cl
4. 1 Na+, 2 Cl
5. 1 Na+, 1 Cl
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The NaCl crystal shown below is an example of which type of cubic lattice?
1. Primitive cubic2. Body-centered
cubic3. Face-centered
cubic
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Correct Answer:
NaCl is an example
of a face-centered
crystalline lattice.
1. Primitive cubic2. Body-centered
cubic3. Face-centered
cubic
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Diamond and graphite are examples of which type of crystalline solids?
1. Molecular2. Covalent network3. Ionic4. Metallic
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Correct Answer:
Diamond and graphite are both forms of carbon, and consist of a network of covalent bonds (hence covalent network).
1. Molecular2. Covalent network3. Ionic4. Metallic