Question 1

Why do O, F and N, when bonded to H, form such strong intermolecular attractions to neighbouring molecules? Make sure to be specific.

Accepted Answer

Oxygen, fluorine, and nitrogen are all v

Question 2

Vanadium crystallizes in a body-centred cubic structure and has an atomic radius of 131 pm. Determine the density of vanadium if the edge length of a bcc structure is 4r/   .

Accepted Answer

A) 3.06 g cm-3 
B) 12.2 g cm-3 
C) 6.11 g cm-3 
D) 2.77 g cm-3 
E) 8.46 g cm-3 
A) 3.06 g cm-3 
B) 12.2 g cm-3 
C) 6.11 g cm-3 
D) 2.77 g cm-3 
E) 8.46 g cm-3

Question 3

Identify the compound that does not have dipole-dipole forces as its strongest force.

Accepted Answer

A) CH2Cl2 
B) CH3OCH3 
C) CH3Br 
D) HCCl3 
E) CO2 
A) CH2Cl2 
B) CH3OCH3 
C) CH3Br 
D) HCCl3 
E) CO2

Question 4

What is the edge length of a face-centred cubic unit cell made up of atoms having a radius of 128 pm?

Accepted Answer

A) 181 pm 
B) 362 pm 
C) 512 pm 
D) 1020 pm 
A) 181 pm 
B) 362 pm 
C) 512 pm 
D) 1020 pm

Question 5

Identify the compound that does not have hydrogen bonding.

Accepted Answer

A) (CH3)3N 
B) H2O 
C) CH3OH 
D) HF 
E) CH3NH2 
A) (CH3)3N 
B) H2O 
C) CH3OH 
D) HF 
E) CH3NH2

Question 6

Place the following substances in order of decreasing boiling point. H2O N2 CO

Accepted Answer

A) CO > H2O > N2 
B) N2 > CO > H2O 
C) H2O > CO > N2 
D) CO > N2 > H2O 
E) N2 > H2O > CO 
A) CO > H2O > N2 
B) N2 > CO > H2O 
C) H2O > CO > N2 
D) CO > N2 > H2O 
E) N2 > H2O > CO

Question 7

Define boiling.

Accepted Answer

A) A liquid becomes a gas. 
B) A gas becomes a liquid. 
C) A gas becomes a solid. 
D) A solid becomes a gas. 
E) A solid becomes a liquid. 
A) A liquid becomes a gas. 
B) A gas becomes a liquid. 
C) A gas becomes a solid. 
D) A solid becomes a gas. 
E) A solid becomes a liquid.

Question 8

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 9

Which of the following substances would you predict to have the highest ΔvapH?

Accepted Answer

A) Xe 
B) C6H6 
C) SiF4 
D) Br2 
E) N2 
A) Xe 
B) C6H6 
C) SiF4 
D) Br2 
E) N2

Question 10

The melting 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 11

Place the following substances in order of decreasing boiling point. N2 O2 H2

Accepted Answer

A) O2 > H2 > N2 
B) N2 > H2 > O2 
C) N2 > O2 > H2 
D) O2 > N2 > H2 
E)  H2 > N2 > O2 
A) O2 > H2 > N2 
B) N2 > H2 > O2 
C) N2 > O2 > H2 
D) O2 > N2 > H2 
E)  H2 > N2 > O2

Question 12

Identify the type of solid for diamond.

Accepted Answer

A) metallic atomic solid 
B) ionic solid 
C) nonbonding atomic solid 
D) molecular solid 
E) networking atomic solid 
A) metallic atomic solid 
B) ionic solid 
C) nonbonding atomic solid 
D) molecular solid 
E) networking atomic solid

Question 13

Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ mol-1. How much heat could be removed by 20.0 g of ethyl chloride?

Accepted Answer

A) 8.18 kJ 
B) 341 kJ 
C) 528 kJ 
D) 3410 kJ 
A) 8.18 kJ 
B) 341 kJ 
C) 528 kJ 
D) 3410 kJ

Question 14

Determine the vapour pressure (in mbar)of a substance at 29 °C, whose normal boiling point is 76 °C and has a ΔvapH of 38.7 kJ mol-1.

Accepted Answer

A) 80 mbar 
B) 13 mbar 
C) 21 mbar 
D) 48 mbar 
E) 128 mbar 
A) 80 mbar 
B) 13 mbar 
C) 21 mbar 
D) 48 mbar 
E) 128 mbar

Question 15

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 16

Ethanol (C2H5OH)melts at -114 °C. The enthalpy of fusion is 5.02 kJ mol-1. The specific heats of solid and liquid ethanol are 0.97 J g-1 °C-1 and 2.3 J g-1 °C-1, respectively. How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50 °C?

Accepted Answer

A) 207.3 kJ 
B) -12.7 kJ 
C) 6.91 kJ 
D) 4192 kJ 
E) 9.21 kJ 
A) 207.3 kJ 
B) -12.7 kJ 
C) 6.91 kJ 
D) 4192 kJ 
E) 9.21 kJ

Question 17

Which type of bonding does Sr form upon solidification?

Accepted Answer

A) covalent network 
B) ionic 
C) metallic 
D) molecular 
A) covalent network 
B) ionic 
C) metallic 
D) molecular

Question 18

Place the following substances in order of increasing boiling point. CH3CH2OH Ar CH3OCH3

Accepted Answer

A) Ar 3OCH3 3CH2OH 
B) CH3CH2OH 3OCH3 
C) CH3CH2OH 3OCH3 3OCH3 3CH2OH 
E) Ar 3CH2OH 3OCH3  
A) Ar 3OCH3 3CH2OH 
B) CH3CH2OH 3OCH3 
C) CH3CH2OH 3OCH3 3OCH3 3CH2OH 
E) Ar 3CH2OH 3OCH3

Question 19

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

Accepted Answer

A) Cl2 
B) CO 
C) HF 
D) NaCl 
E) All of these have intermolecular forces stronger than dispersion. 
A) Cl2 
B) CO 
C) HF 
D) NaCl 
E) All of these have intermolecular forces stronger than dispersion.

Question 20

Define volatile.

Accepted Answer

Liquids th

Exam 11: Liquids, Solids, and Intermolecular Forces

Why do O, F and N, when bonded to H, form such strong intermolecular attractions to neighbouring molecules? Make sure to be specific.

Vanadium crystallizes in a body-centred cubic structure and has an atomic radius of 131 pm. Determine the density of vanadium if the edge length of a bcc structure is 4r/ .

Identify the compound that does not have dipole-dipole forces as its strongest force.

What is the edge length of a face-centred cubic unit cell made up of atoms having a radius of 128 pm?

Identify the compound that does not have hydrogen bonding.

Place the following substances in order of decreasing boiling point. H2O N2 CO

Define boiling.

Define freezing.

Which of the following substances would you predict to have the highest ΔvapH?

The melting point of water is ________.

Place the following substances in order of decreasing boiling point. N2 O2 H2

Identify the type of solid for diamond.

Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ mol-1. How much heat could be removed by 20.0 g of ethyl chloride?

Determine the vapour pressure (in mbar)of a substance at 29 °C, whose normal boiling point is 76 °C and has a ΔvapH of 38.7 kJ mol-1.

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

Ethanol (C2H5OH)melts at -114 °C. The enthalpy of fusion is 5.02 kJ mol-1. The specific heats of solid and liquid ethanol are 0.97 J g-1 °C-1 and 2.3 J g-1 °C-1, respectively. How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50 °C?

Which type of bonding does Sr form upon solidification?

Place the following substances in order of increasing boiling point. CH3CH2OH Ar CH3OCH3

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

Define volatile.

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. H₂O N₂ CO

Which of the following substances would you predict to have the highest Δ_vapH?

Place the following substances in order of decreasing boiling point. N₂ O₂ H₂

Ethyl chloride, C₂H₅Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ mol^-1. How much heat could be removed by 20.0 g of ethyl chloride?

Determine the vapour pressure (in mbar)of a substance at 29 °C, whose normal boiling point is 76 °C and has a Δ_vapHof 38.7 kJ mol^-1.

Ethanol (C₂H₅OH)melts at -114 °C. The enthalpy of fusion is 5.02 kJ mol^-1. The specific heats of solid and liquid ethanol are 0.97 J g^-1 °C^-1 and 2.3 J g^-¹ °C^-1, respectively. How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50 °C?

Place the following substances in order of increasing boiling point. CH₃CH₂OH Ar CH₃OCH₃