Question 1

Na Cl crystallizes in a cubic unit cell with Cl- ions on each corner and each face. How many Na+ and Cl- ions are in each unit cell of Na Cl?

Accepted Answer

A)  1 Na+ ion and 1 Cl- ion 
B)  2 Na+ ions and 2 Cl- ions 
C)  4 Na+ ions and 4 Cl- ions 
D)  8 Na+ ions and 8 Cl- ions 
A)  1 Na+ ion and 1 Cl- ion 
B)  2 Na+ ions and 2 Cl- ions 
C)  4 Na+ ions and 4 Cl- ions 
D)  8 Na+ ions and 8 Cl- ions

Question 2

Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.076 bar is

Accepted Answer

A)  0 
B)  40 
C)  50 
D)  20 
E)  60 
A)  0 
B)  40 
C)  50 
D)  20 
E)  60

Question 3

Identify the substance with the highest viscosity in the liquid phase.

Accepted Answer

A)  gasoline 
B)  water 
C)  corn syrup 
D)  motor oil 
E)  tea 
A)  gasoline 
B)  water 
C)  corn syrup 
D)  motor oil 
E)  tea

Question 4

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

Accepted Answer

A)  C6H14 and C10H20 
B)  LiBr and C5H12 
C)  N2O4 and NH4Cl 
D)  C6H14 and H2O 
E)  None of the pairs above will form a homogeneous solution. 
A)  C6H14 and C10H20 
B)  LiBr and C5H12 
C)  N2O4 and NH4Cl 
D)  C6H14 and H2O 
E)  None of the pairs above will form a homogeneous solution.

Question 5

What is the strongest type of intermolecular force present in H2?

Accepted Answer

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

Question 6

Which of the following is considered an atomic solid?

Accepted Answer

A)  Br2 
B)  CsCl 
C)  N2 
D)  Nb 
E)  None of these is an atomic solid. 
A)  Br2 
B)  CsCl 
C)  N2 
D)  Nb 
E)  None of these is an atomic solid.

Question 7

Match the following.
-CH3CH3

Accepted Answer

A) dipole-dipole forces 
B) ion-dipole forces 
C) H2 + H2O 
D) dispersion forces 
E) hydrogen bonding
F)ionic bond 
A) dipole-dipole forces 
B) ion-dipole forces 
C) H2 + H2O 
D) dispersion forces 
E) hydrogen bonding
F)ionic bond

Question 8

How much energy is required to heat 36.0 g H2O from a liquid at 65 °C to a gas at 115 °C? The following physical data may be useful: ΔvapH = 40.7 kJ mol-1
Cliq = 4.18 J g-1 °C-1
Cgas = 2.01 J g-1 °C-1
Csol = 2.09 J g-1 °C-1
Tmelting = 0 ∘C
Tboiling = 100 ∘C

Accepted Answer

A)  63.5 kJ 
B)  87.7 kJ 
C)  10.9 kJ 
D)  52.7 kJ 
E)  91.7 kJ 
A)  63.5 kJ 
B)  87.7 kJ 
C)  10.9 kJ 
D)  52.7 kJ 
E)  91.7 kJ

Question 9

Match the following.
-LiI

Accepted Answer

A) dipole-dipole forces 
B) ion-dipole forces 
C) H2 + H2O 
D) dispersion forces 
E) hydrogen bonding
F)ionic bond 
A) dipole-dipole forces 
B) ion-dipole forces 
C) H2 + H2O 
D) dispersion forces 
E) hydrogen bonding
F)ionic bond

Question 10

Place the following substances in order of decreasing boiling point. He Ar H2

Accepted Answer

A)  He > H2 > Ar 
B)  H2 > He > Ar 
C)  He > Ar > H2 
D)  Ar > He > H2 
E)  H2 > Ar > He 
A)  He > H2 > Ar 
B)  H2 > He > Ar 
C)  He > Ar > H2 
D)  Ar > He > H2 
E)  H2 > Ar > He

Question 11

Which substance below has the strongest intermolecular forces?

Accepted Answer

A)  A2X, ΔvapH = 39.6 kJ mol-1 
B)  BY2, ΔvapH = 26.7 kJ mol-1 
C)  C3X2, ΔvapH = 36.4 kJ mol-1 
D)  DX2, ΔvapH = 23.3 kJ mol-1 
E)  EY3, ΔvapH = 21.5 kJ mol-1 
A)  A2X, ΔvapH = 39.6 kJ mol-1 
B)  BY2, ΔvapH = 26.7 kJ mol-1 
C)  C3X2, ΔvapH = 36.4 kJ mol-1 
D)  DX2, ΔvapH = 23.3 kJ mol-1 
E)  EY3, ΔvapH = 21.5 kJ mol-1

Question 12

Identify triple point.

Accepted Answer

A)  the temperature, pressure, and density for a gas 
B)  the temperature at which the boiling point equals the melting point 
C)  the temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium 
D)  the temperature that is unique for a substance 
E)  the temperature at which the solid and liquid coexist 
A)  the temperature, pressure, and density for a gas 
B)  the temperature at which the boiling point equals the melting point 
C)  the temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium 
D)  the temperature that is unique for a substance 
E)  the temperature at which the solid and liquid coexist

Question 13

The freezing 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 14

Choose the substance with the highest viscosity in the liquid phase.

Accepted Answer

A)  SbCl3 
B)  AsCl5 
C)  ICl2 
D)  BeCl2 
E)  OCl2 
A)  SbCl3 
B)  AsCl5 
C)  ICl2 
D)  BeCl2 
E)  OCl2

Question 15

Lithium crystallizes in a body-centred cubic structure. What is the coordination number of each atom?

Accepted Answer

A)  4 
B)  6 
C)  8 
D)  12 
A)  4 
B)  6 
C)  8 
D)  12

Question 16

Match the following.
-CH3OH

Accepted Answer

A) dipole-dipole forces 
B) ion-dipole forces 
C) H2 + H2O 
D) dispersion forces 
E) hydrogen bonding
F)ionic bond 
A) dipole-dipole forces 
B) ion-dipole forces 
C) H2 + H2O 
D) dispersion forces 
E) hydrogen bonding
F)ionic bond

Question 17

At atmospheric pressure, dry ice ________.

Accepted Answer

A)  freezes 
B)  deposits 
C)  sublimes 
D)  melts 
E)  boils 
A)  freezes 
B)  deposits 
C)  sublimes 
D)  melts 
E)  boils

Question 18

The energy required to increase the surface area of a liquid by a unit amount is called ________.

Accepted Answer

A)  viscosity 
B)  surface tension 
C)  dipole-dipole force 
D)  hydrogen bonding 
E)  capillary action 
A)  viscosity 
B)  surface tension 
C)  dipole-dipole force 
D)  hydrogen bonding 
E)  capillary action

Question 19

How much energy is required to heat 87.1 g acetone (molar mass = 58.08 g mol-1) from a solid at -154.0 °C to a liquid at -42. 0°C? The following physical data may be useful: ΔfusH = 7.27 kJ mol-1
Cliq = 2.16 J g-1 °C-1
Cgas = 1.29 J g-1 °C-1
Csol = 1.65 J g-1 °C-1
Tmelting = -95.0 °C

Accepted Answer

A)  8.48 kJ 
B)  18.5 kJ 
C)  32.2 kJ 
D)  29.4 kJ 
E)  9.97 kJ 
A)  8.48 kJ 
B)  18.5 kJ 
C)  32.2 kJ 
D)  29.4 kJ 
E)  9.97 kJ

Question 20

Place the following compounds in order of decreasing strength of intermolecular forces. HF O2 CO2

Accepted Answer

A)  HF > CO2 > O2 
B)  HF > O2 > CO2  
C)  O2 > CO2 > HF 
D)  CO2 > HF > O2 
E)  CO2 > O2 > HF 
A)  HF > CO2 > O2 
B)  HF > O2 > CO2  
C)  O2 > CO2 > HF 
D)  CO2 > HF > O2 
E)  CO2 > O2 > HF

Exam 11: Liquids, Solids, and Intermolecular Forces

Na Cl crystallizes in a cubic unit cell with Cl- ions on each corner and each face. How many Na+ and Cl- ions are in each unit cell of Na Cl?

Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.076 bar is

Identify the substance with the highest viscosity in the liquid phase.

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

What is the strongest type of intermolecular force present in H2?

Which of the following is considered an atomic solid?

Match the following. -CH3CH3

How much energy is required to heat 36.0 g H2O from a liquid at 65 °C to a gas at 115 °C? The following physical data may be useful: ΔvapH = 40.7 kJ mol-1 Cliq = 4.18 J g-1 °C-1 Cgas = 2.01 J g-1 °C-1 Csol = 2.09 J g-1 °C-1 Tmelting = 0 ∘C Tboiling = 100 ∘C

Match the following. -LiI

Place the following substances in order of decreasing boiling point. He Ar H2

Which substance below has the strongest intermolecular forces?

Identify triple point.

The freezing point of water is ________.

Choose the substance with the highest viscosity in the liquid phase.

Lithium crystallizes in a body-centred cubic structure. What is the coordination number of each atom?

Match the following. -CH3OH

At atmospheric pressure, dry ice ________.

The energy required to increase the surface area of a liquid by a unit amount is called ________.

How much energy is required to heat 87.1 g acetone (molar mass = 58.08 g mol-1) from a solid at -154.0 °C to a liquid at -42. 0°C? The following physical data may be useful: ΔfusH = 7.27 kJ mol-1 Cliq = 2.16 J g-1 °C-1 Cgas = 1.29 J g-1 °C-1 Csol = 1.65 J g-1 °C-1 Tmelting = -95.0 °C

Place the following compounds in order of decreasing strength of intermolecular forces. HF O2 CO2

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

Na Cl crystallizes in a cubic unit cell with Cl^- ions on each corner and each face. How many Na⁺ and Cl^- ions are in each unit cell of Na Cl?

What is the strongest type of intermolecular force present in H₂?

Match the following. -CH₃CH₃

How much energy is required to heat 36.0 g H₂O from a liquid at 65 °C to a gas at 115 °C? The following physical data may be useful: Δ_vapH = 40.7 kJ mol^-1 C_liq = 4.18 J g^-1 °C^-1 C_gas= 2.01 J g^-1 °C^-1 C_sol = 2.09 J g^-1 °C^-1 T_melting= 0 ^∘C T_boiling = 100 ^∘C

Place the following substances in order of decreasing boiling point. He Ar H₂

Match the following. -CH₃OH

Place the following compounds in order of decreasing strength of intermolecular forces. HF O₂CO₂