Question 1

What type(s)of intermolecular forces exist between PH3 and CO32-?

Accepted Answer

A) dispersion forces 
B) dispersion forces and ion-dipole 
C) dispersion forces, ion-dipole, and dipole-dipole 
D) dispersion forces and dipole-dipole 
E) dispersion forces, ion-dipole, dipole-dipole, and hydrogen bonds 
A) dispersion forces 
B) dispersion forces and ion-dipole 
C) dispersion forces, ion-dipole, and dipole-dipole 
D) dispersion forces and dipole-dipole 
E) dispersion forces, ion-dipole, dipole-dipole, and hydrogen bonds

Question 2

________ 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 3

In the ________ liquid crystalline phase, the component molecules exhibit only one dimensional ordering.

Accepted Answer

A) nematic 
B) smectic A 
C) smectic B 
D) smectic C 
E) cholesteric 
A) nematic 
B) smectic A 
C) smectic B 
D) smectic C 
E) cholesteric

Question 4

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 5

Heats of vaporization are greater than heats of fusion.

Accepted Answer

A) True 
 B)False

Question 6

Which of the following statements is false?

Accepted Answer

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. 
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.

Question 7

The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 J/mol ∙ K. The conversion of 50.0 g of ice at 0.00 °C to liquid water at 0.00°C requires ________ kJ of heat.

Accepted Answer

A) 6.01 
B) 16.7 
C) 75.3 
D) 17.2 
E) Insufficient data are given. 
A) 6.01 
B) 16.7 
C) 75.3 
D) 17.2 
E) Insufficient data are given.

Question 8

London Dispersion Forces tend to ________ in strength with increasing molecular weight.

Accepted Answer

The answer of London Dispersion Forces tend to ________ in...

Question 9

In the smectic A liquid-crystalline phase, ________.

Accepted Answer

A) the molecules are aligned along their long axes, with no ordering with respect to the ends of the molecules 
B) the molecules are arranged in sheets, with their long axes parallel and their ends aligned as well 
C) the molecules are aligned with their long axes tilted with respect to a line perpendicular to the plane in which the molecules are stacked 
D) disk-shaped molecules are aligned through a stacking of the disks in layers 
E) the molecules are oriented in a totally random fashion 
A) the molecules are aligned along their long axes, with no ordering with respect to the ends of the molecules 
B) the molecules are arranged in sheets, with their long axes parallel and their ends aligned as well 
C) the molecules are aligned with their long axes tilted with respect to a line perpendicular to the plane in which the molecules are stacked 
D) disk-shaped molecules are aligned through a stacking of the disks in layers 
E) the molecules are oriented in a totally random fashion

Question 10

Of the following substances, only ________ has London dispersion forces as its only intermolecular force.

Accepted Answer

A) CCl4 
B) SnF3 
C) CH3OH 
D) HI 
E) H2O 
A) CCl4 
B) SnF3 
C) CH3OH 
D) HI 
E) H2O

Question 11

What types of intermolecular forces exist between NH3 and H2S?

Accepted Answer

A) dispersion forces and dipole-dipole forces 
B) dispersion forces 
C) dispersion forces and hydrogen bonds 
D) dispersion forces, hydrogen bonds, and dipole-dipole forces 
E) dispersion forces, hydrogen bonds, and ion-dipole forces 
A) dispersion forces and dipole-dipole forces 
B) dispersion forces 
C) dispersion forces and hydrogen bonds 
D) dispersion forces, hydrogen bonds, and dipole-dipole forces 
E) dispersion forces, hydrogen bonds, and ion-dipole forces

Question 12

Of the following, ________ is the most volatile.

Accepted Answer

A) C2H6 
B) C2I6 
C) C2Br6 
D) C2Cl6 
E) C2F6 
A) C2H6 
B) C2I6 
C) C2Br6 
D) C2Cl6 
E) C2F6

Question 13

On a phase diagram, the melting point is the same as ________.

Accepted Answer

A) the triple point 
B) the critical point 
C) the freezing point 
D) the boiling point 
E) the vapor-pressure curve 
A) the triple point 
B) the critical point 
C) the freezing point 
D) the boiling point 
E) the vapor-pressure curve

Question 14

What is the predominant intermolecular force in HCN?

Accepted Answer

A) dipole-dipole attraction 
B) ion-dipole attraction 
C) ionic bonding 
D) hydrogen bonding 
E) London dispersion forces 
A) dipole-dipole attraction 
B) ion-dipole attraction 
C) ionic bonding 
D) hydrogen bonding 
E) London dispersion forces

Question 15

Of the following substances, ________ has the highest boiling point.

Accepted Answer

A) HOCH2CH2CH2OH 
B) CH3CH2OH 
C) C4H10 
D) N2 
E) Cl2 
A) HOCH2CH2CH2OH 
B) CH3CH2OH 
C) C4H10 
D) N2 
E) Cl2

Question 16

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/g-K and 2.3 J/g-K, respectively. How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -60 °C?

Accepted Answer

A) 207.3 
B) -13.3 
C) 6.34 
D) 3617 
E) 8.63 
A) 207.3 
B) -13.3 
C) 6.34 
D) 3617 
E) 8.63

Question 17

-The phase diagram of a substance is given above. This substance is a ________ at 30 °C and 0.5 atm.

Accepted Answer

A) liquid 
B) gas 
C) solid 
D) supercritical fluid 
E) crystal 
A) liquid 
B) gas 
C) solid 
D) supercritical fluid 
E) crystal

Question 18

The predominant intermolecular force in (CH3)2NH is ________.

Accepted Answer

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

Question 19

The enthalpy change for converting 1.00 mol of ice at -25.0 °C to water at 50.0 °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) 6.27 
C) 10.71 
D) 4709 
E) 8.83 
A) 12.28 
B) 6.27 
C) 10.71 
D) 4709 
E) 8.83

Question 20

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

Exam 11: Liquids and Intermolecular Forces

What type(s)of intermolecular forces exist between PH3 and CO32-?

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

In the ________ liquid crystalline phase, the component molecules exhibit only one dimensional ordering.

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

Heats of vaporization are greater than heats of fusion.

Which of the following statements is false?

The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 J/mol ∙ K. The conversion of 50.0 g of ice at 0.00 °C to liquid water at 0.00°C requires ________ kJ of heat.

London Dispersion Forces tend to ________ in strength with increasing molecular weight.

In the smectic A liquid-crystalline phase, ________.

Of the following substances, only ________ has London dispersion forces as its only intermolecular force.

What types of intermolecular forces exist between NH3 and H2S?

Of the following, ________ is the most volatile.

On a phase diagram, the melting point is the same as ________.

What is the predominant intermolecular force in HCN?

Of the following substances, ________ has the highest boiling point.

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/g-K and 2.3 J/g-K, respectively. How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -60 °C?

-The phase diagram of a substance is given above. This substance is a ________ at 30 °C and 0.5 atm.

The predominant intermolecular force in (CH3)2NH is ________.

The enthalpy change for converting 1.00 mol of ice at -25.0 °C to water at 50.0 °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.

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 ________.

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

What type(s)of intermolecular forces exist between PH₃ and CO₃²^-?

What types of intermolecular forces exist between NH₃ and H₂S?

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/g-K and 2.3 J/g-K, respectively. How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -60 °C?

The predominant intermolecular force in (CH₃)₂NH is ________.

The enthalpy change for converting 1.00 mol of ice at -25.0 °C to water at 50.0 °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.