Question 1

In liquid ethanol, CH3CH2OH 
Which intermolecular forces are present?

Accepted Answer

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. 
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.

Question 2

What is the packing efficiency in body-centred cubic unit cells?

Accepted Answer

A)  74% 
B)  86% 
C)  68% 
D)  52% 
E)  24% 
A)  74% 
B)  86% 
C)  68% 
D)  52% 
E)  24%

Question 3

Which of the following substances should have the lowest melting point?

Accepted Answer

A)  HF 
B)  HCI 
C)  HI 
D)  HBr 
A)  HF 
B)  HCI 
C)  HI 
D)  HBr

Question 4

Place the following compounds in order of decreasing strength of intermolecular forces. I. CH3CH2CH2CH2CH2CH3 II. (CH3)3CCH3 III. (CH3)3CCH2CH3

Accepted Answer

A)  III > II > I 
B)  I > III > II 
C)  I > II > III 
D)  II > III > I 
E)  III > I > II 
A)  III > II > I 
B)  I > III > II 
C)  I > II > III 
D)  II > III > I 
E)  III > I > II

Question 5

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)?

Accepted Answer

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. 
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.

Question 6

Choose the pair of substances that are most likely to form a homogeneous solution.

Accepted Answer

A)  NaCl and Hg 
B)  LiF and C6H14 
C)  C3H8 and C2H5OH 
D)  Br2 and PF3 
E)  NH3 and CH3OH 
A)  NaCl and Hg 
B)  LiF and C6H14 
C)  C3H8 and C2H5OH 
D)  Br2 and PF3 
E)  NH3 and CH3OH

Question 7

Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

Accepted Answer

A)  Cl2 
B)  NH3 
C)  HF 
D)  NaCl 
A)  Cl2 
B)  NH3 
C)  HF 
D)  NaCl

Question 8

Define volatile.

Accepted Answer

Liquids th

Question 9

What is the strongest type of intermolecular force present in NH2CH3?

Accepted Answer

A)  dispersion 
B)  dipole-dipole 
C)  hydrogen bonding 
D)  ion-dipole 
E)  none of the above 
A)  dispersion 
B)  dipole-dipole 
C)  hydrogen bonding 
D)  ion-dipole 
E)  none of the above

Question 10

Why is water an extraordinary substance?

Accepted Answer

A)  Water has a low molar mass, yet it is a liquid at room temperature. 
B)  The phase diagram for water has three triple points. 
C)  Water has an exceptionally low specific heat capacity. 
D)  Water has no hydrogen bonding. 
A)  Water has a low molar mass, yet it is a liquid at room temperature. 
B)  The phase diagram for water has three triple points. 
C)  Water has an exceptionally low specific heat capacity. 
D)  Water has no hydrogen bonding.

Question 11

The normal boiling point of water is ________.

Accepted Answer

A)  0 °C 
B)  32 °C 
C)  212 °C 
D)  100 °C 
E)  273 °C 
A)  0 °C 
B)  32 °C 
C)  212 °C 
D)  100 °C 
E)  273 °C

Question 12

The fluorocarbon       has a normal boiling point of 47.6 °C. The specific heats of   and       (g) are 0.91 J g-1 °C-1 and 0.67 J g-1 °C-1, respectively. The heat of vaporization of the compound is 27.49 kJ mol-1. The heat required to convert 50.0 g of the compound from the liquid at   to the gas at 70.0 °C is ________ kJ.

Accepted Answer

A)  10.07 
B)  2742 
C)  30.22 
D)  9.86 
E)  4.60 
A)  10.07 
B)  2742 
C)  30.22 
D)  9.86 
E)  4.60

Question 13

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?

Accepted Answer

A)  1 
B)  4 
C)  6 
D)  8 
A)  1 
B)  4 
C)  6 
D)  8

Question 14

Based on the figure above, the boiling point of water under an external pressure of 0.316   is

Accepted Answer

A)  50 
B)  30 
C)  80 
D)  70 
E)  40 
A)  50 
B)  30 
C)  80 
D)  70 
E)  40

Question 15

Choose the substance with the lowest surface tension in the liquid phase.

Accepted Answer

A)  CH3SH 
B)  CH3CH2CH2CH3 
C)  C6H6 
D)  H2O 
E)  (CH3)2CO 
A)  CH3SH 
B)  CH3CH2CH2CH3 
C)  C6H6 
D)  H2O 
E)  (CH3)2CO

Question 16

Define freezing.

Accepted Answer

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 
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

Question 17

Which of the following is considered a molecular solid?

Accepted Answer

A)  Cu 
B)  NH4NO3 
C)  I2 
D)  Xe 
E)  None of these is a molecular solid. 
A)  Cu 
B)  NH4NO3 
C)  I2 
D)  Xe 
E)  None of these is a molecular solid.

Question 18

Define viscosity.

Accepted Answer

Viscosity

Question 19

The normal boiling point for H2Se  is higher than the normal boiling point for H2S . This can be explained by ________.

Accepted Answer

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  
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

Question 20

Which of the following statements is TRUE?

Accepted Answer

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 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 is true.

Exam 11: Liquids, Solids, and Intermolecular Forces

In liquid ethanol, CH3CH2OH Which intermolecular forces are present?

What is the packing efficiency in body-centred cubic unit cells?

Which of the following substances should have the lowest melting point?

Place the following compounds in order of decreasing strength of intermolecular forces. I. CH3CH2CH2CH2CH2CH3 II. (CH3)3CCH3 III. (CH3)3CCH2CH3

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)?

Choose the pair of substances that are most likely to form a homogeneous solution.

Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

Define volatile.

What is the strongest type of intermolecular force present in NH2CH3?

Why is water an extraordinary substance?

The normal boiling point of water is ________.

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?

Based on the figure above, the boiling point of water under an external pressure of 0.316 is

Choose the substance with the lowest surface tension in the liquid phase.

Define freezing.

Which of the following is considered a molecular solid?

Define viscosity.

The normal boiling point for H2Se is higher than the normal boiling point for H2S . This can be explained by ________.

Which of the following statements is TRUE?

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

In liquid ethanol, CH₃CH₂OH Which intermolecular forces are present?

Place the following compounds in order of decreasing strength of intermolecular forces. I. CH₃CH₂CH₂CH₂CH₂CH₃ II. (CH₃)₃CCH₃ III. (CH₃)₃CCH₂CH₃

What is the strongest type of intermolecular force present in NH₂CH₃?

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?

The normal boiling point for H₂Se is higher than the normal boiling point for H₂S. This can be explained by ________.