Question 1

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 bondingF) C) and D)
G) A) and C)

Question 2

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

Accepted Answer

A)  density
B)  viscosity
C)  vapor pressure
D)  surface tension
E)  hydrogen bondingF) A) and B)
G) A) and E)

Question 3

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

Accepted Answer

A)  NBr3
B)  CH3COOH
C)  SiCl4
D)  HBr
E)  Cl2OF) B) and D)
G) C) and E)

Question 4

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)  crystalF) A) and C)
G) All of the above

Question 5

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 forcesF) A) and B)
G) B) and E)

Question 6

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 forcesF) A) and E)
G) None of the above

Question 7

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

Accepted Answer

A)  CI4
B)  CBr4
C)  CCl4
D)  CF4
E)  CH4F) A) and D)
G) A) and E)

Question 8

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 waterF) A) and E)
G) A) and D)

Question 9

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 equilibriumF) C) and D)
G) A) and E)

Question 10

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, oneF) A) and C)
G) B) and D)

Question 11

Which molecule is the least volatile?

Accepted Answer

A)  CH3Cl
B)  CH3I
C)  CH3F
D)  CH4
E)  CH3BrF) A) and B)
G) All of the above

Question 12

-  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)  2TF) B) and E)
G) D) and E)

Question 13

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)  BCF) A) and C)
G) B) and C)

Question 14

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)  8.83F) B) and E)
G) None of the above

Question 15

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 zF) B) and D)
G) D) and E)

Question 16

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 liquidF) B) and D)
G) D) and E)

Question 17

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 aboveF) None of the above
G) A) and D)

Question 18

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 temperatureF) C) and D)
G) B) and D)

Question 19

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 2O,Δ   = 6.01 kJ/mol and Δ   = 40.67 kJ/mol. A) 64.8 B) 75.9 C) 11100 D) 12000 E) 112" class="answers-bank-image d-inline" rel="preload" > = 6.01 kJ/mol and Δ 2O,Δ   = 6.01 kJ/mol and Δ   = 40.67 kJ/mol. A) 64.8 B) 75.9 C) 11100 D) 12000 E) 112" class="answers-bank-image d-inline" rel="preload" > = 40.67 kJ/mol.

Accepted Answer

A)  64.8
B)  75.9
C)  11100
D)  12000
E)  112F) B) and E)
G) D) and E)

Question 20

Which molecule has hydrogen bonding as the predominant intermolecular force?

Accepted Answer

A)  CH4
B)  C6H6
C)  CH3OH
D)  CO2
E)  C4H10F) D) and E)
G) None of the above

Exam 11: Liquids and Intermolecular Forces

What types of intermolecular forces exist between NH3 and H2O?

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Hydrogen bonding is a special case of ________.

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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?

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

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Which molecule has hydrogen bonding as the predominant intermolecular force?

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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.

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On a phase diagram,the critical pressure is ________.

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

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

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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 .

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

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

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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.

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

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What is the predominant intramolecular force in NaNO3?

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

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

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Which molecule is the least volatile?

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

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

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What types of intermolecular forces exist between NH₃ and H₂O?

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

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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.

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What is the predominant intramolecular force in NaNO₃?

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