Question 1

What is the predominant intramolecular force in NaNO3?

Accepted Answer

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

Question 2

The vapor pressure of any substance at its normal boiling point is ________.

Accepted Answer

A) 1 Pa 
B) 1 torr 
C) 1 atm 
D) equal to atmospheric pressure 
E) equal to the vapor pressure of water 
A) 1 Pa 
B) 1 torr 
C) 1 atm 
D) equal to atmospheric pressure 
E) equal to the vapor pressure of water

Question 3

What intermolecular force is responsible for the fact that ice is less dense than liquid water?

Accepted Answer

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

Question 4

What types of intermolecular forces exist between NH3 and H2O?

Accepted Answer

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

Question 5

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 6

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

Accepted Answer

A) NBr3 
B) CH3COOH 
C) SiCl4 
D) HBr 
E) Cl2O 
A) NBr3 
B) CH3COOH 
C) SiCl4 
D) HBr 
E) Cl2O

Question 7

On a phase diagram,the critical pressure is ________.

Accepted Answer

A) the pressure required to melt a solid 
B) the pressure below which a substance is a solid at all temperatures 
C) the pressure above which a substance is a liquid at all temperatures 
D) the pressure at which a liquid changes to a gas 
E) the pressure required to liquefy a gas at its critical temperature 
A) the pressure required to melt a solid 
B) the pressure below which a substance is a solid at all temperatures 
C) the pressure above which a substance is a liquid at all temperatures 
D) the pressure at which a liquid changes to a gas 
E) the pressure required to liquefy a gas at its critical temperature

Question 8

Which molecule is the least volatile?

Accepted Answer

A) CH3Cl 
B) CH3I 
C) CH3F 
D) CH4 
E) CH3Br 
A) CH3Cl 
B) CH3I 
C) CH3F 
D) CH4 
E) CH3Br

Question 9

-   is the slope of a plot of the natural log of the vapor pressure of a substance versus ________.

Accepted Answer

A) -1/T 
B) -T 
C) 1/T 
D) T 
E) 2T 
A) -1/T 
B) -T 
C) 1/T 
D) T 
E) 2T

Question 10

The enthalpy change for converting 1.00 mol of ice at -25.0 °C to water at 50.0 °C is   The specific heats of ice,water,and steam are     and   respectively.For   O,Δ   = 6.01 kJ/mol,and   .

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 11

At 1 atm,an unknown sample melts at 49.9 °C and boils at 209.5 °C.If the temperature is 0°C,what is the state of matter for the sample?

Accepted Answer

A) solid and liquid in equilibrium 
B) liquid 
C) gas 
D) solid 
E) liquid and gas in equilibrium 
A) solid and liquid in equilibrium 
B) liquid 
C) gas 
D) solid 
E) liquid and gas in equilibrium

Question 12

Which one of the following derivatives of methane has the highest boiling point?

Accepted Answer

A) CI4 
B) CBr4 
C) CCl4 
D) CF4 
E) CH4 
A) CI4 
B) CBr4 
C) CCl4 
D) CF4 
E) CH4

Question 13

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 14

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

Accepted Answer

A) nematic, one 
B) smectic A, one 
C) nematic, two 
D) nematic, three 
E) smectic B, one 
A) nematic, one 
B) smectic A, one 
C) nematic, two 
D) nematic, three 
E) smectic B, one

Question 15

On the phase diagram shown above,segment ________ corresponds to the conditions of temperature and pressure under which the solid and the gas of the substance are in equilibrium.

Accepted Answer

A) AB 
B) AC 
C) AD 
D) CD 
E) BC 
A) AB 
B) AC 
C) AD 
D) CD 
E) BC

Question 16

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 17

Which molecule has hydrogen bonding as the predominant intermolecular force?

Accepted Answer

A) CH4 
B) C6H6 
C) CH3OH 
D) CO2 
E) C4H10 
A) CH4 
B) C6H6 
C) CH3OH 
D) CO2 
E) C4H10

Question 18

How high a liquid will rise up a narrow tube as a result of capillary action depends on ________.

Accepted Answer

A) the magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the tube, and gravity 
B) gravity alone 
C) only the magnitude of adhesive forces between the liquid and the tube 
D) the viscosity of the liquid 
E) only the magnitude of cohesive forces in the liquid 
A) the magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the tube, and gravity 
B) gravity alone 
C) only the magnitude of adhesive forces between the liquid and the tube 
D) the viscosity of the liquid 
E) only the magnitude of cohesive forces in the liquid

Question 19

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 20

Calculate the enthalpy change (in kJ)associated with the conversion of 25.0 grams of ice at -4.00 °C to water vapor at 109.0 °C.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,Δ   = 6.01 kJ/mol and Δ   = 40.67 kJ/mol.

Accepted Answer

A) 64.8 
B) 75.9 
C) 11100 
D) 12000 
E) 112 
A) 64.8 
B) 75.9 
C) 11100 
D) 12000 
E) 112

Exam 11: Liquids and Intermolecular Forces

What is the predominant intramolecular force in NaNO3?

The vapor pressure of any substance at its normal boiling point is ________.

What intermolecular force is responsible for the fact that ice is less dense than liquid water?

What types of intermolecular forces exist between NH3 and H2O?

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

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

On a phase diagram,the critical pressure is ________.

Which molecule is the least volatile?

- is the slope of a plot of the natural log of the vapor pressure of a substance versus ________.

The enthalpy change for converting 1.00 mol of ice at -25.0 °C to water at 50.0 °C is The specific heats of ice,water,and steam are and respectively.For O,Δ = 6.01 kJ/mol,and .

At 1 atm,an unknown sample melts at 49.9 °C and boils at 209.5 °C.If the temperature is 0°C,what is the state of matter for the sample?

Which one of the following derivatives of methane has the highest boiling point?

Hydrogen bonding is a special case of ________.

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

On the phase diagram shown above,segment ________ corresponds to the conditions of temperature and pressure under which the solid and the gas of the substance are in equilibrium.

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

Which molecule has hydrogen bonding as the predominant intermolecular force?

How high a liquid will rise up a narrow tube as a result of capillary action depends on ________.

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

Calculate the enthalpy change (in kJ)associated with the conversion of 25.0 grams of ice at -4.00 °C to water vapor at 109.0 °C.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,Δ = 6.01 kJ/mol and Δ = 40.67 kJ/mol.

Introduction: Matter, energy, and Measurement

Atoms, molecules, and Ions

Chemical Reactions and Reaction Stoichiometry

Reactions in Aqueous Solution

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 is the predominant intramolecular force in NaNO₃?

What types of intermolecular forces exist between NH₃ and H₂O?

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

Calculate the enthalpy change (in kJ)associated with the conversion of 25.0 grams of ice at -4.00 °C to water vapor at 109.0 °C.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,Δ = 6.01 kJ/mol and Δ = 40.67 kJ/mol.