Chemistry: A Molecular Approach: 3rd Edition Test Bank - Tro

Chemistry: A Molecular Approach: 3rd Edition Test Bank – Tro

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Chemistry: A Molecular Approach: 3rd Edition Test Bank – Tro
What: TEST BANK
Year Published: 2013
Authors: Tro
Edition: 3rd

Product Description

Chemistry: A Molecular Approach: 3rd Edition Test Bank – Tro

 

Chemistry: A Molecular Approach: 3rd Edition Test Bank – Tro

 

Sample

 

Chemistry: A Molecular Approach, 3e (Tro)
Chapter 11 Liquids, Solids, and Intermolecular Forces

Multiple Choice Questions

1) Identify the characteristics of a liquid.
A) indefinite shape and volume
B) indefinite shape, but definite volume
C) definite shape and volume
D) none of the above
E) all of the above
Answer: B
Diff: 1 Page Ref: 11.2

2) Identify the characteristics of a gas.
A) indefinite shape and volume
B) indefinite shape, but definite volume
C) definite shape and volume
D) none of the above
E) all of the above
Answer: A
Diff: 1 Page Ref: 11.2

3) Which one of the following has a low density?
A) gas
B) liquid
C) solid
D) none of the above
E) all of the above
Answer: A
Diff: 1 Page Ref: 11.2

4) Which one of the following has a definite shape and volume?
A) gas
B) liquid
C) solid
D) none of the above
E) all of the above
Answer: C
Diff: 1 Page Ref: 11.2

5) Give the change in condition to go from a liquid to a gas.
A) increase heat or reduce pressure
B) increase heat or increase pressure
C) cool or reduce pressure
D) cool or increase pressure
E) none of the above
Answer: A
Diff: 1 Page Ref: 11.2

6) The forces between polar molecules is known as ________.
A) hydrogen bonding
B) ion-dipole forces
C) dipole-dipole forces
D) dispersion forces
E) ionic forces
Answer: C
Diff: 1 Page Ref: 11.3

7) Which of the following statements is TRUE?
A) Intermolecular forces are generally stronger than bonding forces.
B) The potential energy of molecules decrease as they get closer to one another.
C) Energy is given off when the attraction between two molecules is broken.
D) Increasing the pressure on a solid usually causes it to become a liquid.
E) None of the above are true.
Answer: B
Diff: 1 Page Ref: 11.3

8) What is the strongest type of intermolecular force present in NH2CH3?
A) dispersion
B) dipole-dipole
C) hydrogen bonding
D) ion-dipole
E) none of the above
Answer: C
Diff: 1 Page Ref: 11.3

9) The two strands in DNA are held together by ________.
A) dispersion forces
B) dipole-dipole forces
C) hydrogen bonding
D) ion-dipole forces
Answer: C
Diff: 1 Page Ref: 11.3

10) How many compounds, of the ones listed below, have hydrogen bonding?

CH3CH2CH2NH2 CH3CH2NHCH2CH3 (CH3CH2)2NCH2CH3
A) 2
B) 3
C) 1
D) 0
Answer: A
Diff: 2 Page Ref: 11.3
11) Place the following compounds in order of increasing strength of intermolecular forces.

CH4 CH3CH2CH3 CH3CH3

A) CH3CH2CH3 < CH4 < CH3CH3
B) CH3CH2CH3 < CH3CH3 < CH4
C) CH3CH3 < CH4 < CH3CH2CH3
D) CH4 < CH3CH2CH3 < CH3CH3
E) CH4 < CH3CH3 < CH3CH2CH3
Answer: E
Diff: 2 Page Ref: 11.3

12) Place the following compounds in order of decreasing strength of intermolecular forces.

I. CH3CH2CH2CH2CH2CH3 II. (CH3)3CCH3 III. (CH3)3CCH2CH3

A) III > II > I
B) I > III > II
C) I > II > III
D) II > III > I
E) III > I > II
Answer: B
Diff: 2 Page Ref: 11.3

13) Identify the compound that does not have hydrogen bonding.
A) (CH3)3N
B) H2O
C) CH3OH
D) HF
E) CH3NH2
Answer: A
Diff: 2 Page Ref: 11.3

14) In a liquid, the energy required to increase the surface of the area by a unit amount is called ________.
A) viscosity
B) surface tension
C) dipole-dipole force
D) hydrogen bonding
E) capillary action
Answer: B
Diff: 1 Page Ref: 11.4
15) Choose the substance with the lowest viscosity.
A) Cl3CCCl3
B) Cl2CHCH2Cl
C) Cl2CHCHCl2
D) ClCH2CH2Cl
E) Cl3CCHCl2
Answer: D
Diff: 2 Page Ref: 11.4

16) Choose the substance with the highest viscosity.
A) SbCl3
B) AsCl5
C) ICl2
D) BeCl2
E) OCl2
Answer: D
Diff: 2 Page Ref: 11.4

17) Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.
A) capillary action
B) viscosity
C) surface tension
D) density
E) none of the above
Answer: A
Diff: 2 Page Ref: 11.4

18) Describe sweating in humans.
A) It is an endothermic reaction.
B) The sweat evaporates absorbing heat from the body.
C) The skin is cooled.
D) None of the above.
E) All of the above.
Answer: E
Diff: 2 Page Ref: 11.5

19) Which of the following statements is TRUE?
A) Vapor pressure increases with temperature.
B) Hydrogen bonds are stronger than covalent bonds.
C) Intermolecular forces hold the atoms in molecules together.
D) Dispersion forces are generally stronger than dipole-dipole forces.
E) None of the above are true.
Answer: A
Diff: 1 Page Ref: 11.5
20) Identify the place which has the lowest boiling point of water.
A) Death Valley, 282 feet below sea level
B) A pressurized passenger jet, 35,000 feet
C) New Orleans, sea level
D) Mt. Everest, 29,035 feet
E) Denver, Colorado, 5280 feet
Answer: D
Diff: 1 Page Ref: 11.5

21) Identify the place which has the highest boiling point of water.
A) Death Valley, 282 feet below sea level
B) A pressurized passenger jet, 35,000 feet
C) New Orleans, sea level
D) Mt. Everest, 29035 feet
E) Denver, Colorado, 5280 feet
Answer: A
Diff: 1 Page Ref: 11.5

22) Which of the following statements is FALSE?
A) The rate of vaporization increases with increasing surface area.
B) The rate of vaporization increases with decreasing strength of intermolecular forces.
C) The rate of vaporization increases with increasing temperature.
D) Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces.
E) None of the above are false.
Answer: D
Diff: 1 Page Ref: 11.5

23) Which substance below has the strongest intermolecular forces?
A) A2X, ΔHvap= 39.6 kJ/mol
B) BY2, ΔHvap= 26.7 kJ/mol
C) C3X2, ΔHvap= 36.4 kJ/mol
D) DX2, ΔHvap= 23.3 kJ/mol
E) EY3, ΔHvap= 21.5 kJ/mol
Answer: A
Diff: 1 Page Ref: 11.5

24) Define boiling.
A) A liquid becomes a gas.
B) A gas becomes a liquid.
C) A gas becomes a solid.
D) A solid becomes a gas.
E) A solid becomes a liquid.
Answer: A
Diff: 1 Page Ref: 11.5
25) Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.
A) absolute temperature
B) definite temperature
C) fluid temperature
D) critical temperature
E) solid temperature
Answer: D
Diff: 1 Page Ref: 11.5

26) Choose the substance with the highest vapor pressure at a given temperature.
A) SiS2
B) RbCl
C) CH3SCH3
D) BF3
E) SbH3
Answer: D
Diff: 2 Page Ref: 11.5

27) Which of the following substances would you predict to have the highest ΔHvap?
A) CH3Cl
B) HCl
C) HOCH2CH2OH
D) CH3CH2OH
E) CH3CH2CH2CH3
Answer: C
Diff: 2 Page Ref: 11.5

28) How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2) at its boiling point, if its ΔHvap is 31.6 kJ/mol?
A) 31.2 kJ
B) 6.49 kJ
C) 55.1 kJ
D) 15.4 kJ
E) 18.1 kJ
Answer: E
Diff: 3 Page Ref: 11.5

29) How much energy is required to vaporize 98.6 g of ethanol (C2H5OH) at its boiling point, if its ΔHvap is 40.5 kJ/mol?
A) 86.7 kJ
B) 11.5 kJ
C) 18.9 kJ
D) 52.8 kJ
E) 39.9 kJ
Answer: A
Diff: 3 Page Ref: 11.5
30) Place the following substances in order of increasing vapor pressure at a given temperature.

SF6 SiH4 SF4

A) SF6 < SiH4 < SF4
B) SiH4 < SF4 < SF6
C) SF6 < SF4 < SiH4
D) SF4 < SF6 < SiH4
E) SiH4 < SF6 < SF4
Answer: D
Diff: 4 Page Ref: 11.5

31) Place the following substances in order of decreasing vapor pressure at a given temperature.

PF5 BrF3 CF4

A) BrF3 > PF5 > CF4
B) BrF3 > CF4 > PF5
C) PF5 > BrF3 > CF4
D) CF4 > BrF3 > PF5
E) CF4 > PF5 > BrF3
Answer: E
Diff: 4 Page Ref: 11.5

32) Place the following substances in order of increasing vapor pressure at a given temperature.

NF3 NH3 BCl3

A) NH3 < NF3 < BCl3
B) NF3 < NH3 < BCl3
C) BCl3 < NF3 < NH3
D) NH3 < BCl3 < NF3
E) BCl3 < NH3 < NF3
Answer: A
Diff: 4 Page Ref: 11.5

33) Place the following substances in order of decreasing vapor pressure at a given temperature.

BeF2 CH3OH OF2

A) CH3OH > OF2 > BeF2
B) BeF2 > OF2 > CH3OH
C) OF2 > CH3OH > BeF2
D) OF2 > BeF2 > CH3OH
E) BeF2 > CH3OH > OF2
Answer: C
Diff: 4 Page Ref: 11.5

34) Place the following substances in order of decreasing boiling point.

H2O N2 CO

A) CO > H2O > N2
B) N2 > CO > H2O
C) H2O > CO > N2
D) CO > N2 > H2O
E) N2 > H2O > CO
Answer: C
Diff: 4 Page Ref: 11.5

35) Place the following substances in order of decreasing boiling point.

N2 O2 H2

A) O2 > H2 > N2
B) N2 > H2 > O2
C) N2 > O2 > H2
D) O2 > N2 > H2
E) H2 > N2 > O2
Answer: D
Diff: 4 Page Ref: 11.5

36) Determine ΔHvap for a compound that has a measured vapor pressure of 24.3 torr at 273 K and 135 torr at 325 K.
A) 41 kJ/mol
B) 79 kJ/mol
C) 24 kJ/mol
D) 13 kJ/mol
E) 34 kJ/mol
Answer: C
Diff: 5 Page Ref: 11.5

37) Determine the normal boiling point of a substance whose vapor pressure is 55.1 mm Hg at 35°C and has a ΔHvap of 32.1 kJ/mol.
A) 255 K
B) 368 K
C) 412 K
D) 390. K
E) 466 K
Answer: D
Diff: 5 Page Ref: 11.5
38) Determine the vapor pressure (in mm Hg) of a substance at 29°C, whose normal boiling point is 76°C and has a ΔHvap of 38.7 kJ/mol.
A) 80 mm Hg
B) 13 mm Hg
C) 21 mm Hg
D) 48 mm Hg
E) 96 mm Hg
Answer: E
Diff: 5 Page Ref: 11.5

39) Determine the vapor pressure (in torr) of a substance at 36°C, whose normal boiling point is 84°C and has a ΔHvap of 22.1 kJ/mol.
A) 239 torr
B) 31.8 torr
C) 41.8 torr
D) 147 torr
E) 98 torr
Answer: A
Diff: 5 Page Ref: 11.5

40) Define deposition.
A) A liquid becomes a gas.
B) A gas becomes a liquid.
C) A gas becomes a solid.
D) A solid becomes a gas.
E) A solid becomes a liquid.
Answer: C
Diff: 1 Page Ref: 11.6

41) Define sublimation.
A) the phase transition from solid to gas
B) the phase transition from gas to solid
C) the phase transition from gas to liquid
D) the phase transition from liquid to gas
E) the phase transition from liquid to solid
Answer: A
Diff: 1 Page Ref: 11.6

42) Define freezing.
A) the phase transition from solid to gas
B) the phase transition from gas to solid
C) the phase transition from gas to liquid
D) the phase transition from liquid to gas
E) the phase transition from liquid to solid
Answer: E
Diff: 1 Page Ref: 11.6
43) Define fusion.
A) the phase transition from solid to liquid
B) the phase transition from gas to solid
C) the phase transition from gas to liquid
D) the phase transition from liquid to gas
E) the phase transition from liquid to solid
Answer: A
Diff: 1 Page Ref: 11.6

44) At atmospheric pressure, dry ice ________.
A) freezes
B) deposits
C) sublimes
D) melts
E) boils
Answer: C
Diff: 1 Page Ref: 11.6

45) At atmospheric pressure, ice ________.
A) freezes
B) deposits
C) sublimes
D) melts
E) boils
Answer: D
Diff: 1 Page Ref: 11.6

46) How much energy is required to heat 36.0 g H2O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful.

ΔHvap = 40.7 kJ/mol
Cliq = 4.18 J/g∘C
Cgas = 2.01 J/g∘C
Csol = 2.09 J/g∘C
Tmelting = 0∘C
Tboiling = 100∘C

A) 63.5 kJ
B) 87.7 kJ
C) 10.9 kJ
D) 52.7 kJ
E) 91.7 kJ
Answer: B
Diff: 5 Page Ref: 11.7
47) How much energy must be removed from a 125 g sample of benzene (molar mass= 78.11 g/mol) at 425.0 K to liquify the sample and lower the temperature to 335.0 K? The following physical data may be useful.

ΔHvap = 33.9 kJ/mol
ΔHfus = 9.8 kJ/mol
Cliq = 1.73 J/g°C
Cgas = 1.06 J/g°C
Csol = 1.51 J/g°C
Tmelting = 279.0 K
Tboiling = 353.0 K

A) 38.9 kJ
B) 95.4 kJ
C) 67.7 kJ
D) 54.3 kJ
E) 74.4 kJ
Answer: C
Diff: 5 Page Ref: 11.7

48) How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C to a liquid at -42.0°C? The following physical data may be useful.

ΔHfus = 7.27 kJ/mol
Cliq = 2.16 J/g°C
Cgas = 1.29 J/g°C
Csol = 1.65 J/g°C
Tmelting = -95.0°C

A) 8.48 kJ
B) 18.5 kJ
C) 32.2 kJ
D) 29.4 kJ
E) 9.97 kJ
Answer: D
Diff: 5 Page Ref: 11.7
49) How much energy must be removed from a 94.4 g sample of benzene (molar mass= 78.11 g/mol) at 322.0 K to solidify the sample and lower the temperature to 205.0 K? The following physical data may be useful.

ΔHvap = 33.9 kJ/mol
ΔHfus = 9.8 kJ/mol
Cliq = 1.73 J/g°C
Cgas = 1.06 J/g°C
Csol = 1.51 J/g°C
Tmelting = 279.0 K
Tboiling = 353.0 K

A) 17.6 kJ
B) 11.8 kJ
C) 70.2 kJ
D) 10.5 kJ
E) 29.4 kJ
Answer: E
Diff: 5 Page Ref: 11.7

50) Define triple point.
A) The temperature, pressure, and density for a gas.
B) The temperature at which the boiling point equals the melting point.
C) The temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium.
D) The temperature that is unique for a substance.
E) The temperature at which the solid and liquid co-exist.
Answer: C
Diff: 1 Page Ref: 11.8
51) Consider the phase diagram shown. Choose the statement below that is TRUE.
A) The triple point of this substance occurs at a temperature of 31°C.
B) At 10 atm of pressure, there is no temperature where the liquid phase of this substance would exist.
C) The solid phase of this substance is higher in density than the liquid phase.
D) The line separating the solid and liquid phases represents the ΔHvap.
E) None of the above are true.
Answer: C
Diff: 1 Page Ref: 11.8

52) Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500°C, what phase changes will occur (in order of increasing temperature)?
A) condensation, followed by vaporization
B) sublimation, followed by deposition
C) vaporization, followed by deposition
D) fusion, followed by vaporization
E) No phase change will occur under the conditions specified.
Answer: D
Diff: 1 Page Ref: 11.8

53) Why is water an extraordinary substance?
A) Water has a low molar mass, yet it is a liquid at room temperature.
B) Water is the main solvent within living organisms.
C) Water has an exceptionally high specific heat capacity.
D) Water has strong hydrogen bonding.
E) All of the above.
Answer: E
Diff: 1 Page Ref: 11.9

54) Identify the compound with the highest boiling point.
A) CH4
B) NH3
C) HF
D) H2S
E) H2O
Answer: E
Diff: 1 Page Ref: 11.9

55) Determine the radius of an Al atom (in pm) if the density of aluminum is 2.71 g/cm3. Aluminum crystallizes in a face centered cubic structure with an edge length of 2 r.
A) 143 pm
B) 227 pm
C) 96 pm
D) 172 pm
E) 193 pm
Answer: A
Diff: 5 Page Ref: 11.11

56) A metal crystallizes in a face centered cubic structure and has a density of 11.9 g/cm3. If the radius of the metal atom is 138 pm, what is the identity of the metal?
A) At
B) Pd
C) Mn
D) Fe
E) Cr
Answer: B
Diff: 5 Page Ref: 11.11

57) Vanadium crystallizes in a body centered cubic structure and has an atomic radius of 131 pm. Determine the density of vanadium, if the edge length of a bcc structure is 4r/ .
A) 3.06 g/cm3
B) 12.2 g/cm3
C) 6.11 g/cm3
D) 2.77 g/cm3
E) 8.46 g/cm3
Answer: C
Diff: 5 Page Ref: 11.11

58) Identify the type of solid for AgCl.
A) metallic atomic solid
B) ionic solid
C) nonbonding atomic solid
D) molecular solid
E) networking atomic solid
Answer: B
Diff: 1 Page Ref: 11.12

59) Identify the type of solid for ice.
A) metallic atomic solid
B) ionic solid
C) nonbonding atomic solid
D) molecular solid
E) networking atomic solid
Answer: D
Diff: 1 Page Ref: 11.12

60) Identify the type of solid for gold.
A) metallic atomic solid
B) ionic solid
C) nonbonding atomic solid
D) molecular solid
E) networking atomic solid
Answer: A
Diff: 1 Page Ref: 11.12

61) Identify the type of solid for diamond.
A) metallic atomic solid
B) ionic solid
C) nonbonding atomic solid
D) molecular solid
E) networking atomic solid
Answer: E
Diff: 1 Page Ref: 11.12

62) Identify the type of solid for argon.
A) metallic atomic solid
B) ionic solid
C) nonbonding atomic solid
D) molecular solid
E) networking atomic solid
Answer: C
Diff: 1 Page Ref: 11.12
Algorithmic Questions

1) Which has the smallest dipole-dipole forces?
A) CH3Cl
B) HBr
C) O2
D) NO
Answer: C
Diff: 2 Page Ref: 11.3

2) Which is expected to have the largest dispersion forces?
A) C3H8
B) C12H26
C) F2
D) Be Cl2
Answer: B
Diff: 2 Page Ref: 11.3

3) Which of the following compounds exhibits hydrogen bonding?
A) CH3I
B) HBr
C) CH3OCH3
D) CH3NH2
Answer: D
Diff: 2 Page Ref: 11.3

4) List the compounds in decreasing boiling point order.

CH3CH2CH3 Ar CH3CN
A) CH3CH2CH3 > CH3CN > Ar
B) Ar > CH3CH2CH3 > CH3CN
C) CH3CH2CH3 > Ar > CH3CN
D) CH3CN > CH3CH2CH3 > Ar
E) Ar > CH3CN > CH3CH2CH3
Answer: D
Diff: 2 Page Ref: 11.3

5) In liquid propanol,
CH3CH2CH2OH
which intermolecular forces are present?
A) Dispersion, hydrogen bonding and dipole-dipole forces are present.
B) Only dipole-dipole and ion-dipole forces are present.
C) Only dispersion and dipole-dipole forces are present.
D) Only hydrogen bonding forces are present.
Answer: A
Diff: 3 Page Ref: 11.3
6) Which of the following compounds exhibits only dipole-dipole intermolecular interactions?
A) Br2
B) CH3Br
C) CBr4
D) BrCH2CH2OH
Answer: B
Diff: 3 Page Ref: 11.3

7) The normal boiling point for H2Se is higher than the normal boiling point for H2S . This can be explained by
A) larger dipole-dipole forces for H2Se .
B) larger dispersion forces for H2Se .
C) larger hydrogen-bond forces for H2Se .
D) larger dipole-dipole forces, larger dispersion forces, and larger hydrogen-bond forces for H2Se .
Answer: B
Diff: 3 Page Ref: 11.3

8) What is the strongest type of intermolecular force present in Cl2?
A) ion-dipole
B) dipole-dipole
C) dispersion
D) hydrogen bonding
E) none of the above
Answer: C
Diff: 1 Page Ref: 11.3

9) What is the strongest type of intermolecular force present in CHBr3?
A) ion-dipole
B) dispersion
C) hydrogen bonding
D) dipole-dipole
E) none of the above
Answer: D
Diff: 1 Page Ref: 11.3

10) What type of intermolecular force causes the dissolution of KF in water?
A) hydrogen bonding
B) dipole-dipole forces
C) ion-dipole force
D) dispersion forces
E) none of the above
Answer: C
Diff: 1 Page Ref: 11.3
11) Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.
A) O2
B) CO
C) HF
D) NaCl
E) All of these have intermolecular forces stronger than dispersion.
Answer: A
Diff: 2 Page Ref: 11.3

12) Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force.
A) H2
B) SO2
C) NH3
D) CF4
E) BCl3
Answer: B
Diff: 2 Page Ref: 11.3

13) Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force.
A) SBr2
B) C2H6
C) CH3OH
D) CH2Br2
E) None of the above compounds exhibit hydrogen bonding.
Answer: C
Diff: 2 Page Ref: 11.3

14) Place the following compounds in order of increasing strength of intermolecular forces.

CS2 I2 NH2CH3

A) NH2CH3 < CS2 < I2
B) I2 < NH2CH3 < CS2
C) NH2CH3 < I2 < CS2
D) I2 < CS2 < NH2CH3
E) CS2 < NH2CH3 < I2
Answer: D
Diff: 2 Page Ref: 11.3
15) Place the following compounds in order of decreasing strength of intermolecular forces.

HF H2 CO2

A) HF > CO2 > H2
B) HF > H2 > CO2
C) H2 > CO2 > HF
D) CO2 > HF > H2
E) CO2 > H2 > HF
Answer: A
Diff: 2 Page Ref: 11.3

16) Identify the compound that does not have dipole-dipole forces as its strongest force.
A) CH2Br2
B) CH3OCH3
C) CH3Cl
D) HCBr3
E) CO2
Answer: E
Diff: 2 Page Ref: 11.3

17) Identify the compound that has hydrogen bonding.
A) (CH3)3N
B) N2
C) CH3CH3
D) HI
E) H2O
Answer: E
Diff: 2 Page Ref: 11.3

18) Choose the pair of substances that are most likely to form a homogeneous solution.
A) KI and Hg
B) LiCl and C6H14
C) C3H8 and C2H5OH
D) F2 and PF3
E) NH3 and CH3OH
Answer: E
Diff: 2 Page Ref: 11.3

19) Choose the pair of substances that are most likely to form a homogeneous solution.
A) C6H14 and C10H20
B) KCl and C5H12
C) N2O4 and NH4I
D) C6H14 and H2O
E) None of the pairs above will form a homogeneous solution.
Answer: A
Diff: 2 Page Ref: 11.3

20) Choose the pair of substances that are most likely to form a homogeneous solution.
A) CBr4 and SF2
B) NF3 and SO2
C) CO and C6H6
D) NH2CH3 and CH4
E) None of the pairs above will form a homogeneous solution.
Answer: B
Diff: 2 Page Ref: 11.3

21) Choose the substance with the highest surface tension.
A) HOCH2CH2OH
B) CH2Br2
C) CH3CH2Cl
D) CH3CH2OH
E) CH3CH2CH3
Answer: A
Diff: 2 Page Ref: 11.4

22) Choose the substance with the lowest surface tension.
A) CH3OH
B) CH3CH2CH2CH3
C) C6H6
D) H2O
E) (CH3)2CO
Answer: B
Diff: 2 Page Ref: 11.4

23) Choose the substance with the highest viscosity.
A) (CH3CH2)2CO
B) C2H4Cl2
C) HOCH2CH2CH2CH2OH
D) CCl4
E) C6H14
Answer: C
Diff: 2 Page Ref: 11.4

24) Identify the substance with the highest viscosity.
A) gasoline
B) water
C) maple syrup
D) motor oil
E) coffee
Answer: C
Diff: 2 Page Ref: 11.4

25) Based on the figure above, the boiling point of diethyl ether under an external pressure of 1.32 atm is ________°C.
A) 10
B) 20
C) 30
D) 40
E) 0
Answer: D
Diff: 3 Page Ref: 11.5

26) Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.0724 atm is ________°C.
A) 80
B) 60
C) 70
D) 40
E) 20
Answer: E
Diff: 3 Page Ref: 11.5

27) Based on the figure above, the boiling point of water under an external pressure of 0.316 atm is ________°C.
A) 70
B) 40
C) 60
D) 80
E) 90
Answer: A
Diff: 3 Page Ref: 11.5
28) Which of the following compounds has the highest boiling point?
A) H2O
B) H Cl
C) H2S
D) N H3
Answer: A
Diff: 4 Page Ref: 11.5

29) Choose the substance with the lowest vapor pressure at a given temperature.
A) CO2
B) CaI2
C) BF3
D) Ar
E) PF5
Answer: B
Diff: 2 Page Ref: 11.5

30) Place the following substances in order of increasing boiling point.

Ne I2 N2

A) Ne < I2 < N2
B) I2 < N2 < Ne
C) N2 < I2 < Ne
D) I2 < Ne < N2
E) Ne < N2 < I2
Answer: E
Diff: 2 Page Ref: 11.5

31) Place the following substances in order of increasing boiling point.

CH3CH2OH He CH3OCH3

A) He < CH3OCH3 < CH3CH2OH
B) CH3CH2OH < He < CH3OCH3
C) CH3CH2OH < CH3OCH3 < He
D) CH3OCH3 < He < CH3CH2OH
E) He < CH3CH2OH < CH3OCH3
Answer: A
Diff: 2 Page Ref: 11.5
32) Choose the substance with the highest boiling point.
A) CH4
B) KI
C) CS2
D) HF
E) I2
Answer: B
Diff: 2 Page Ref: 11.5

33) Choose the substance with the lowest boiling point.
A) H2S
B) NBr3
C) O2
D) CI2H2
E) H2O2
Answer: C
Diff: 2 Page Ref: 11.5

34) Which of the following substances would you predict to have the highest ΔHvap?
A) Xe
B) C6H6
C) SiF4
D) F2
E) N2
Answer: B
Diff: 2 Page Ref: 11.5

35) How much energy is required to vaporize 158 g of butane (C4H10) at its boiling point, if its ΔHvap is 24.3 kJ/mol?
A) 15.1 kJ
B) 66.1 kJ
C) 41.9 kJ
D) 2.60 kJ
E) 38.4 kJ
Answer: B
Diff: 3 Page Ref: 11.5
36) Place the following substances in order of decreasing boiling point.

He Rn H2

A) He > H2 > Rn
B) H2 > He > Rn
C) He > Rn > H2
D) Ar > Rn > H2
E) H2 > Ar > Rn
Answer: D
Diff: 4 Page Ref: 11.5

37) The boiling point of water is ________.
A) 0 K
B) 32°C
C) 212 K
D) 100oC
E) 273°C
Answer: D
Diff: 1 Page Ref: 11.5

38) The melting point of water is ________.
A) 32oF
B) 32oC
C) 212oC
D) 100°C
E) 273°C
Answer: A
Diff: 1 Page Ref: 11.6

39) The freezing point of water is ________.
A) 32oF
B) 32oC
C) 212oC
D) 100°C
E) 273°C
Answer: A
Diff: 1 Page Ref: 11.6
40) The heat of vaporization of water at 100°C is 40.66 kJ/mol. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100°C.
A) 20.3 kJ of heat are absorbed.
B) 20.3 kJ of heat are released.
C) 81.3 kJ of heat are absorbed.
D) 81.3 kJ of heat are released.
Answer: B
Diff: 4 Page Ref: 11.7

41) Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 35.0°C to gaseous CCl4 at 76.8°C (the normal boiling point for CCl4). The specific heat of CCl4(l) is
0.857 J/(g ∙ °C), its heat of fusion is 3.27 kJ/mol, and its heat of vaporization is 29.82 kJ/mol.
A) 0.896 kJ
B) 1.43 kJ
C) 5.74 kJ
D) 6.28 kJ
Answer: C
Diff: 4 Page Ref: 11.7

42) The enthalpy change for converting 1.00 mol of ice at -50.0°C to water at 70.0°C is ________ kJ. The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ/mol.
A) 12.28
B) 6.41
C) 13.16
D) 7154
E) 9.40
Answer: C
Diff: 4 Page Ref: 11.7

43) The enthalpy change for converting 10.0 g of ice at -25.0°C to water at 80.0°C is ________ kJ. The specific heats of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ/mol.
A) 12.28
B) 6.16
C) 3870
D) 7.21
E) 9.88
Answer: D
Diff: 4 Page Ref: 11.7
44) The fluorocarbon C2Cl3F3 has a normal boiling point of 47.6°C. The specific heats of C2Cl3F3 (l) and C2Cl3F3 (g) are 0.91 J/gK and 0.67 J/gK, respectively. The heat of vaporization of the compound is 27.49 kJ/mol. The heat required to convert 50.0 g of the compound from the liquid at 5.0°C to the gas at 80.0°C is ________ kJ.
A) 8.19
B) 1454
C) 30.51
D) 3031
E) 10.36
Answer: E
Diff: 4 Page Ref: 11.7

45) Ethanol (C2H5OH) melts at -114°C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/gK and 2.3 J/gK, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135°C to liquid ethanol at -50°C?
A) 207.3 kJ
B) -12.7 kJ
C) 6.91 kJ
D) 4192 kJ
E) 9.21 kJ
Answer: C
Diff: 4 Page Ref: 11.7

46) Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ/mol. How much heat could be removed by 20.0 g of ethyl chloride?
A) 8.18 kJ
B) 341 kJ
C) 528 kJ
D) 3410 kJ
Answer: A
Diff: 4 Page Ref: 11.7

47) How much heat is released when 105 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ∙ °C), and the molar heat capacity of ice is
36.4 J/(mol ∙ °C).
A) 54.8 kJ
B) 273 kJ
C) 319 kJ
D) 347 kJ
Answer: C
Diff: 4 Page Ref: 11.7
48) Assign the appropriate labels to the phase diagram shown below.
A) A = liquid, B = solid, C = gas, D = critical point
B) A = gas, B = solid, C = liquid, D = triple point
C) A = gas, B = liquid, C = solid, D = critical point
D) A = solid, B = gas, C = liquid, D = triple point
E) A = liquid, B = gas, C = solid, D = critical point
Answer: B
Diff: 1 Page Ref: 11.8

49) Give the coordination number for a body-centered cubic cell.
A) 0
B) 6
C) 8
D) 10
E) 12
Answer: C
Diff: 1 Page Ref: 11.11

50) What is the edge length of a face-centered cubic unit cell made up of atoms having a radius of 128 pm?
A) 181 pm
B) 362 pm
C) 512 pm
D) 1020 pm
Answer: B
Diff: 5 Page Ref: 11.11
51) Nickel has a face-centered cubic structure and has a density of 8.90 g/cm3. What is its atomic radius?
A) 125 pm
B) 249 pm
C) 353 pm
D) 997 pm
Answer: A
Diff: 5 Page Ref: 11.11

52) Gold crystallizes in a face-centered cubic structure. What is the edge length of the unit cell if the atomic radius of gold is 144 pm?
A) 204 pm
B) 288 pm
C) 333 pm
D) 407 pm
Answer: D
Diff: 5 Page Ref: 11.11

53) Cesium has a radius of 272 pm and crystallizes in a body-centered cubic structure. What is the edge length of the unit cell?
A) 314 pm
B) 385 pm
C) 544 pm
D) 628 pm
Answer: D
Diff: 5 Page Ref: 11.11

54) Lithium crystallizes in a body-centered cubic structure. What is the coordination number of each atom?
A) 4
B) 6
C) 8
D) 12
Answer: C
Diff: 5 Page Ref: 11.11

55) NaCl crystallizes in a cubic unit cell with Cl- ions on each corner and each face. How many Na+ and Cl- ions are in each unit cell of NaCl?
A) 1 Na+ ion and 1 Cl- ion
B) 2 Na+ ions and 2 Cl- ions
C) 4 Na+ ions and 4 Cl- ions
D) 8 Na+ ions and 8 Cl- ions
Answer: C
Diff: 5 Page Ref: 11.11
56) How many H- ions are around each Na+ ion in NaH, which has a cubic unit cell with H- ions on each corner and each face?
A) 1
B) 4
C) 6
D) 8
Answer: C
Diff: 5 Page Ref: 11.11

57) Which of the following forms a molecular solid?
A) CaO
B) C10H22
C) C, graphite
D) gold
Answer: B
Diff: 1 Page Ref: 11.12

58) Which of the following forms an ionic solid?
A) Ag
B) C7H15NH2
C) Rb I
D) S O3
Answer: C
Diff: 1 Page Ref: 11.12

59) Which type of bonding does Sr form upon solidification?
A) covalent network
B) ionic
C) metallic
D) molecular
Answer: C
Diff: 2 Page Ref: 11.12

60) Which of the following is considered a molecular solid?
A) Au
B) NH4NO3
C) I2
D) Rn
E) None of these is a molecular solid.
Answer: C
Diff: 1 Page Ref: 11.12
61) Which of the following is considered an ionic solid?
A) (NH4)2CO3
B) CBr4
C) SeBr2
D) XeF4
E) None of these is an ionic solid.
Answer: A
Diff: 1 Page Ref: 11.12

62) Which of the following is considered an atomic solid?
A) F2
B) CsBr
C) N2
D) Nb
E) None of these is an atomic solid.
Answer: D
Diff: 1 Page Ref: 11.12

63) Which of the following is considered a nonbonding atomic solid?
A) Ne
B) Cu
C) I2
D) Ca
E) K
Answer: A
Diff: 1 Page Ref: 11.12

64) Which of the following substances should have the highest melting point?
A) CO2
B) SrS
C) Kr
D) F2
E) MgO
Answer: E
Diff: 1 Page Ref: 11.12

65) Which of the following substances should have the highest melting point?
A) Fe
B) Ne
C) Xe
D) N2
E) CO
Answer: A
Diff: 1 Page Ref: 11.12
Matching Questions

Match the following.

A) ionic bond
B) dipole-dipole forces
C) hydrogen bonding
D) ion-dipole forces
E) dispersion forces
1) LiI
Diff: 1 Page Ref: 11.3

2) CH3OH
Diff: 1 Page Ref: 11.3

3) CH3CH3
Diff: 1 Page Ref: 11.3

4) CH2F2 F) H2 + H2O
Diff: 1 Page Ref: 11.3

5) LiI + H2O
Diff: 1 Page Ref: 11.3

Answers: 1) A 2) C 3) E 4) B 5) D

Short Answer Questions

1) Why do O, F and N, when bonded to H, form such strong intermolecular attractions to neighboring molecules? Make sure to be specific.
Answer: Oxygen, fluorine and nitrogen are all very small and highly electronegative elements. When they bond to hydrogen they form extremely polar bonds. These extremely polar bonds formed between small atoms can get very close to interact with other molecules. The closer the molecules get, the more strongly they can interact. In addition, these three elements usually have lone pair electrons which make the attractions to other molecules even stronger.
Diff: 1 Page Ref: 11.3

2) Define viscosity.
Answer: Viscosity is the resistance of a liquid to flow.
Diff: 2 Page Ref: 11.4

3) Why does the temperature of a substance stay constant during a phase change such as vaporization?
Answer: The energy added to the substance is not used to raise the kinetic energy of the substance. Instead it is “used up” in breaking the intermolecular attractions between particles to take them from a liquid (with intermolecular attractions) to a gas (with no intermolecular attractions).
Diff: 1 Page Ref: 11.5

4) Define volatile.
Answer: Liquids that vaporize easily.
Diff: 1 Page Ref: 11.5

5) Define boiling point of a liquid.
Answer: The temperature at which the vapor pressure equals the external pressure.
Diff: 1 Page Ref: 11.5

6) Define dynamic equilibrium.
Answer: Dynamic equilibrium is when the rate of condensation equals the rate of vaporization.
Diff: 2 Page Ref: 11.5

7) Why is the ΔHvap higher than ΔHfus for a given compound?
Answer: Vaporizing a substance requires the complete “breaking” of all intermolecular attractions, whereas the melting of a substance only requires the breaking of a portion of the intermolecular attractions.
Diff: 1 Page Ref: 11.6

8) Sketch the phase diagram of benzene. Make sure to label the axes and the different phases of benzene. Use the physical data provided below.

melting point = 279 K
boiling point = 353 K
Tc = 562 K
Pc = 48.4 atm
Triple Point = 0.05 atm, 279 K

Answer: Sketch should include all given information showing fusion and vaporization curves.
Diff: 3 Page Ref: 11.8

9) Give the edge length in terms of r for a simple cubic cell.
Answer: 2r
Diff: 1 Page Ref: 11.9

10) Describe the difference between the conduction band and the valence band.
Answer: The valence band is the group of highest energy occupied orbitals in the solid. The conduction band is the set of empty orbitals that are higher in energy than the valence band. In metals the difference in energy between the valence band and conduction band is fairly small, making it easy for electrons to move from the valence band to the conduction band.
Diff: 2 Page Ref: 11.12

Chemistry: A Molecular Approach: 3rd Edition Test Bank – Tro

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