Question 1

Hydrogen bonding is a special case of __________.

Accepted Answer

A) London-dispersion forces 
B) ion-dipole attraction 
C) dipole-dipole attractions 
D) ion-ion interactions 
E) none of the above 
A) London-dispersion forces 
B) ion-dipole attraction 
C) dipole-dipole attractions 
D) ion-ion interactions 
E) none of the above

Question 2

Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point?

Accepted Answer

A) CH3CH2CH3 
B) CH3OCH3 
C) CH3Cl 
D) CH3CHO 
E) CH3CN 
A) CH3CH2CH3 
B) CH3OCH3 
C) CH3Cl 
D) CH3CHO 
E) CH3CN

Question 3

__________ is the energy required to expand the surface area of a liquid by a unit amount of area.

Accepted Answer

A) Viscosity 
B) Surface tension 
C) Volatility 
D) Meniscus 
E) Capillary action 
A) Viscosity 
B) Surface tension 
C) Volatility 
D) Meniscus 
E) Capillary action

Question 4

Which of the following has dispersion forces as its only intermolecular force?

Accepted Answer

A) CH4 
B) HCl 
C) C6H13NH2 
D) NaCl 
E) CH3Cl 
A) CH4 
B) HCl 
C) C6H13NH2 
D) NaCl 
E) CH3Cl

Question 5

Which compound has the strongest intermolecular forces?

Accepted Answer

A) CBr4 
B) C12H26 
C) CI4 
D) N2 
E) O2 
A) CBr4 
B) C12H26 
C) CI4 
D) N2 
E) O2

Question 6

When the phase diagram for a substance has a solid-liquid phase boundary line that has a negative slope (leans to the left), the substance __________.

Accepted Answer

A) can go from solid to liquid, within a small temperature range, via the application of pressure 
B) sublimes rather than melts under ordinary conditions 
C) cannot go from solid to liquid by application of pressure at any temperature 
D) cannot be liquefied above its triple point 
E) melts rather than sublimes under ordinary conditions 
A) can go from solid to liquid, within a small temperature range, via the application of pressure 
B) sublimes rather than melts under ordinary conditions 
C) cannot go from solid to liquid by application of pressure at any temperature 
D) cannot be liquefied above its triple point 
E) melts rather than sublimes under ordinary conditions

Question 7

The phase diagram of a substance is shown above. The area labeled __________ indicates the solid phase for the substance.

Accepted Answer

A) w 
B) x 
C) y 
D) z 
E) y and z 
A) w 
B) x 
C) y 
D) z 
E) y and z

Question 8

Of the following, __________ should have the highest critical temperature.

Accepted Answer

A) CBr4 
B) CCl4 
C) CF4 
D) CH4 
E) H2 
A) CBr4 
B) CCl4 
C) CF4 
D) CH4 
E) H2

Question 9

The property responsible for the "beading up" of water is __________.

Accepted Answer

A) density 
B) viscosity 
C) vapor pressure 
D) surface tension 
E) hydrogen bonding 
A) density 
B) viscosity 
C) vapor pressure 
D) surface tension 
E) hydrogen bonding

Question 10

Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.0724 atm is __________°C.

Accepted Answer

A) 80 
B) 60 
C) 70 
D) 40 
E) 20 
A) 80 
B) 60 
C) 70 
D) 40 
E) 20

Question 11

Cholesteric liquid crystals are colored because __________.

Accepted Answer

A) each molecule is a chromophore 
B) of the slight twist between layers 
C) of the large spacing between layers 
D) of the large number of conjugated bonds 
E) all of the molecules contain multiple benzene rings 
A) each molecule is a chromophore 
B) of the slight twist between layers 
C) of the large spacing between layers 
D) of the large number of conjugated bonds 
E) all of the molecules contain multiple benzene rings

Question 12

A volatile liquid is one that __________.

Accepted Answer

A) is highly flammable 
B) is highly viscous 
C) is highly hydrogen-bonded 
D) is highly cohesive 
E) readily evaporates 
A) is highly flammable 
B) is highly viscous 
C) is highly hydrogen-bonded 
D) is highly cohesive 
E) readily evaporates

Question 13

__________ are particularly polarizable.

Accepted Answer

A) Small nonpolar molecules 
B) Small polar molecules 
C) Large nonpolar molecules 
D) Large polar molecules 
E) Large molecules, regardless of their polarity, 
A) Small nonpolar molecules 
B) Small polar molecules 
C) Large nonpolar molecules 
D) Large polar molecules 
E) Large molecules, regardless of their polarity,

Question 14

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/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ/mol

Accepted Answer

A) 12.28 
B) 6.16 
C) 3870 
D) 7.21 
E) 9.88 
A) 12.28 
B) 6.16 
C) 3870 
D) 7.21 
E) 9.88

Question 15

Some things take longer to cook at high altitudes than at low altitudes because __________.

Accepted Answer

A) water boils at a lower temperature at high altitude than at low altitude 
B) water boils at a higher temperature at high altitude than at low altitude 
C) heat isn't conducted as well in low density air 
D) natural gas flames don't burn as hot at high altitudes 
E) there is a higher moisture content in the air at high altitude 
A) water boils at a lower temperature at high altitude than at low altitude 
B) water boils at a higher temperature at high altitude than at low altitude 
C) heat isn't conducted as well in low density air 
D) natural gas flames don't burn as hot at high altitudes 
E) there is a higher moisture content in the air at high altitude

Question 16

The normal boiling point of the substance with the phase diagram shown above is __________°C.

Accepted Answer

A) 10 
B) 20 
C) 30 
D) 40 
E) 50 
A) 10 
B) 20 
C) 30 
D) 40 
E) 50

Question 17

Molecules containing only single bonds do not exhibit liquid-crystal behavior because free rotation can occur around single bonds making these molecules flexible.

Accepted Answer

A) True 
 B)False

Question 18

C12H26 molecules are held together by __________.

Accepted Answer

A) ion-ion interactions 
B) hydrogen bonding 
C) ion-dipole interactions 
D) dipole-dipole interactions 
E) dispersion forces 
A) ion-ion interactions 
B) hydrogen bonding 
C) ion-dipole interactions 
D) dipole-dipole interactions 
E) dispersion forces

Question 19

According to the phase diagram shown above, the normal boiling point of this substance is __________°C.

Accepted Answer

A) -3 
B) 10 
C) 29 
D) 38 
E) 0 
A) -3 
B) 10 
C) 29 
D) 38 
E) 0

Question 20

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)__________.

Accepted Answer

A) plasma 
B) gas 
C) liquid 
D) amorphous solid 
E) supercritical fluid and gas 
A) plasma 
B) gas 
C) liquid 
D) amorphous solid 
E) supercritical fluid and gas

Exam 11: Liquids and Intermolecular Forces

Hydrogen bonding is a special case of __________.

Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point?

__________ is the energy required to expand the surface area of a liquid by a unit amount of area.

Which of the following has dispersion forces as its only intermolecular force?

Which compound has the strongest intermolecular forces?

When the phase diagram for a substance has a solid-liquid phase boundary line that has a negative slope (leans to the left), the substance __________.

The phase diagram of a substance is shown above. The area labeled __________ indicates the solid phase for the substance.

Of the following, __________ should have the highest critical temperature.

The property responsible for the "beading up" of water is __________.

Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.0724 atm is __________°C.

Cholesteric liquid crystals are colored because __________.

A volatile liquid is one that __________.

__________ are particularly polarizable.

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/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ/mol

Some things take longer to cook at high altitudes than at low altitudes because __________.

The normal boiling point of the substance with the phase diagram shown above is __________°C.

Molecules containing only single bonds do not exhibit liquid-crystal behavior because free rotation can occur around single bonds making these molecules flexible.

C12H26 molecules are held together by __________.

According to the phase diagram shown above, the normal boiling point of this substance is __________°C.

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)__________.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

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/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H₂O, ΔH_fus = 6.01 kJ/mol, and ΔH_vap = 40.67 kJ/mol

C₁₂H₂₆ molecules are held together by __________.