Question 1

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 2

Determine the vapour pressure (in mbar)of a substance at 36 °C whose normal boiling point is 84 °C and has a ΔvapH of 22.1 kJ mol-1.

Accepted Answer

A) 319 mbar 
B) 31.8 mbar 
C) 41.8 mbar 
D) 147 mbar 
E) 98 mbar 
A) 319 mbar 
B) 31.8 mbar 
C) 41.8 mbar 
D) 147 mbar 
E) 98 mbar

Question 3

Choose the substance with the highest vapour pressure at a given temperature.

Accepted Answer

A) SiS2 
B) RbCl 
C) CH3SCH3 
D) BF3 
E) SbH3 
A) SiS2 
B) RbCl 
C) CH3SCH3 
D) BF3 
E) SbH3

Question 4

Assign the appropriate labels to the phase diagram shown below.

Accepted Answer

A) A = liquid, B = solid, C = gas, D = critical point 
B) A = gas, B = solid, C = liquid, D = triple point 
C) A = gas, B = liquid, C = solid, D = critical point 
D) A = solid, B = gas, C = liquid, D = supercritical fluid 
E) A = liquid, B = gas, C = solid, D = triple point 
A) A = liquid, B = solid, C = gas, D = critical point 
B) A = gas, B = solid, C = liquid, D = triple point 
C) A = gas, B = liquid, C = solid, D = critical point 
D) A = solid, B = gas, C = liquid, D = supercritical fluid 
E) A = liquid, B = gas, C = solid, D = triple point

Question 5

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 6

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 7

Match the following.

-CH2F2

Accepted Answer

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

Question 8

Give the change in condition to go from a liquid to a gas.

Accepted Answer

A) increase heat or reduce pressure 
B) increase heat or increase pressure 
C) cool or reduce pressure 
D) cool or increase pressure 
E) none of the above 
A) increase heat or reduce pressure 
B) increase heat or increase pressure 
C) cool or reduce pressure 
D) cool or increase pressure 
E) none of the above

Question 9

Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l)at 35.0 °C to gaseous CCl4 at 76.8 °C (the normal boiling point for CCl4). The specific heat of CCl4(l)is 0.857 J g-1 °C-1, its heat of fusion is 3.27 kJ mol-1, and its heat of vaporization is 29.82 kJ mol-1.

Accepted Answer

A) 0.896 kJ 
B) 1.43 kJ 
C) 5.74 kJ 
D) 6.28 kJ 
A) 0.896 kJ 
B) 1.43 kJ 
C) 5.74 kJ 
D) 6.28 kJ

Question 10

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 11

Based on the figure above, the boiling point of water under an external pressure of 0.316 bar is ________ °C.

Accepted Answer

A) 70 
B) 40 
C) 60 
D) 80 
E) 90 
A) 70 
B) 40 
C) 60 
D) 80 
E) 90

Question 12

NaCl 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 NaCl?

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 13

Determine the radius of an Al atom (in pm)if the density of aluminum is 2.71 g cm-3. Aluminum crystallizes in a face-centred cubic structure with an edge length of 2   r.

Accepted Answer

A) 143 pm 
B) 227 pm 
C) 96 pm 
D) 172 pm 
E) 193 pm 
A) 143 pm 
B) 227 pm 
C) 96 pm 
D) 172 pm 
E) 193 pm

Question 14

Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.

Accepted Answer

A) capillary action 
B) viscosity 
C) surface tension 
D) density 
E) none of the above 
A) capillary action 
B) viscosity 
C) surface tension 
D) density 
E) none of the above

Question 15

Based on the figure above, the boiling point of diethyl ether under an external pressure of 1.32 bar is ________ °C.

Accepted Answer

A) 10 
B) 20 
C) 30 
D) 40 
E) 0 
A) 10 
B) 20 
C) 30 
D) 40 
E) 0

Question 16

How much energy is required to vaporize 158 g of butane (C4H10)at its boiling point if its ΔvapH is 24.3 kJ mol-1?

Accepted Answer

A) 15.1 kJ 
B) 66.1 kJ 
C) 89.4 kJ 
D) 11.2 kJ 
E) 38.4 kJ 
A) 15.1 kJ 
B) 66.1 kJ 
C) 89.4 kJ 
D) 11.2 kJ 
E) 38.4 kJ

Question 17

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 18

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

Accepted Answer

A) (CH3CH2)2CO 
B) C2H4Cl2 
C) HOCH2CH2CH2CH2OH 
D) CF4 
E) C6H14 
A) (CH3CH2)2CO 
B) C2H4Cl2 
C) HOCH2CH2CH2CH2OH 
D) CF4 
E) C6H14

Question 19

Which of the following compounds exhibits only dispersion and dipole-dipole intermolecular interactions?

Accepted Answer

A) H2 
B) HI  
C) CO2 
D) CH3NH2 
A) H2 
B) HI  
C) CO2 
D) CH3NH2

Question 20

Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.197 bar is ________ °C.

Accepted Answer

A) 80 
B) 70 
C) 60 
D) 20 
E) 40 
A) 80 
B) 70 
C) 60 
D) 20 
E) 40

Exam 11: Liquids, Solids, and Intermolecular Forces

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

Determine the vapour pressure (in mbar)of a substance at 36 °C whose normal boiling point is 84 °C and has a ΔvapH of 22.1 kJ mol-1.

Choose the substance with the highest vapour pressure at a given temperature.

Assign the appropriate labels to the phase diagram shown below.

Which of the following is considered a molecular solid?

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

Match the following. -CH2F2

Give the change in condition to go from a liquid to a gas.

Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l)at 35.0 °C to gaseous CCl4 at 76.8 °C (the normal boiling point for CCl4). The specific heat of CCl4(l)is 0.857 J g-1 °C-1, its heat of fusion is 3.27 kJ mol-1, and its heat of vaporization is 29.82 kJ mol-1.

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

Based on the figure above, the boiling point of water under an external pressure of 0.316 bar is ________ °C.

NaCl 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 NaCl?

Determine the radius of an Al atom (in pm)if the density of aluminum is 2.71 g cm-3. Aluminum crystallizes in a face-centred cubic structure with an edge length of 2 r.

Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.

Based on the figure above, the boiling point of diethyl ether under an external pressure of 1.32 bar is ________ °C.

How much energy is required to vaporize 158 g of butane (C4H10)at its boiling point if its ΔvapH is 24.3 kJ mol-1?

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?

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

Which of the following compounds exhibits only dispersion and dipole-dipole intermolecular interactions?

Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.197 bar is ________ °C.

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 Metallury

Transition Metals and Coordination Compounds

Filters

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

Determine the vapour pressure (in mbar)of a substance at 36 °C whose normal boiling point is 84 °C and has a Δ_vapHof 22.1 kJ mol^-1.

Match the following. -CH₂F₂

NaCl 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 NaCl?

Determine the radius of an Al atom (in pm)if the density of aluminum is 2.71 g cm^-3. Aluminum crystallizes in a face-centred cubic structure with an edge length of 2 r.

How much energy is required to vaporize 158 g of butane (C₄H₁₀)at its boiling point if its Δ_vapH is 24.3 kJ mol^-1?

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?