Question 1

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 2

A metal crystallizes in a face-centred cubic structure and has a density of 11.9 g cm-3.If the radius of the metal atom is 138 pm,what is the identity of the metal?

Accepted Answer

A) At 
B) Pd 
C) Mn 
D) Fe 
E) Cr 
A) At 
B) Pd 
C) Mn 
D) Fe 
E) Cr

Question 3

Which of the following statements is TRUE?

Accepted Answer

A) Vapour pressure increases with temperature. 
B) Hydrogen bonds are stronger than covalent bonds. 
C) Intermolecular forces hold the atoms in molecules together. 
D) Dispersion forces are generally stronger than dipole-dipole forces. 
A) Vapour pressure increases with temperature. 
B) Hydrogen bonds are stronger than covalent bonds. 
C) Intermolecular forces hold the atoms in molecules together. 
D) Dispersion forces are generally stronger than dipole-dipole forces.

Question 4

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 5

Define sublimation.

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 6

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 7

Which of the following statements is FALSE?

Accepted Answer

A) The rate of vaporization increases with increasing surface area. 
B) The rate of vaporization increases with decreasing strength of intermolecular forces. 
C) The rate of vaporization increases with increasing temperature. 
D) Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces. 
A) The rate of vaporization increases with increasing surface area. 
B) The rate of vaporization increases with decreasing strength of intermolecular forces. 
C) The rate of vaporization increases with increasing temperature. 
D) Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces.

Question 8

Define dynamic equilibrium between the liquid and gaseous phases.

Accepted Answer

Dynamic equilibrium

Question 9

Choose the substance with the lowest boiling point.

Accepted Answer

A) H2S 
B) NBr3 
C) F2 
D) CF2H2 
E) H2O2 
A) H2S 
B) NBr3 
C) F2 
D) CF2H2 
E) H2O2

Question 10

Which has the smallest dipole-dipole forces?

Accepted Answer

A) CH3Cl  
B) HBr  
C) O2 
D) NO  
A) CH3Cl  
B) HBr  
C) O2 
D) NO

Question 11

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$\sqrt{2}$ 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 12

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

Accepted Answer

A) Fe 
B) Ne 
C) Xe 
D) N2 
E) CO 
A) Fe 
B) Ne 
C) Xe 
D) N2 
E) CO

Question 13

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 14

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 15

Identify the characteristics of a liquid.

Accepted Answer

A) indefinite shape and volume 
B) indefinite shape,but definite volume 
C) definite shape and volume 
D) definite shape and indefinite volume 
A) indefinite shape and volume 
B) indefinite shape,but definite volume 
C) definite shape and volume 
D) definite shape and indefinite volume

Question 16

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 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 vapour pressure at a given temperature. 
SF6 $\quad$SiH4 $\quad$SF4

Accepted Answer

A) SF6 4 4 
B) SiH4 4 6 
C) SF6 4 4 
D) SF4 6 4 
E) SiH4 6 4 
A) SF6 4 4 
B) SiH4 4 6 
C) SF6 4 4 
D) SF4 6 4 
E) SiH4 6 4

Question 19

Place the following compounds in order of increasing strength of intermolecular forces. 
CH4 $\quad$CH3CH2CH3 $\quad$CH3CH3

Accepted Answer

A) CH3CH2CH3 4 3CH3 
B) CH3CH2CH3 3CH3 4 
C) CH3CH3 4 3CH2CH3 
D) CH4 3CH2CH3 3CH3 
E) CH4 3CH3 3CH2CH3 
A) CH3CH2CH3 4 3CH3 
B) CH3CH2CH3 3CH3 4 
C) CH3CH3 4 3CH2CH3 
D) CH4 3CH2CH3 3CH3 
E) CH4 3CH3 3CH2CH3

Question 20

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

Accepted Answer

A) HOCH2CH2OH 
B) CH2F2 
C) CH3CH2F 
D) CH3CH2OH 
E) CH3CH2CH3 
A) HOCH2CH2OH 
B) CH2F2 
C) CH3CH2F 
D) CH3CH2OH 
E) CH3CH2CH3

Exam 11: Liquids, solids, and Intermolecular Forces

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

A metal crystallizes in a face-centred cubic structure and has a density of 11.9 g cm-3.If the radius of the metal atom is 138 pm,what is the identity of the metal?

Which of the following statements is TRUE?

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

Define sublimation.

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.

Which of the following statements is FALSE?

Define dynamic equilibrium between the liquid and gaseous phases.

Choose the substance with the lowest boiling point.

Which has the smallest dipole-dipole forces?

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 2\sqrt{2}2​ r.

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

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

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

Identify the characteristics of a liquid.

The melting point of water is ________.

Which type of bonding does Sr form upon solidification?

Place the following substances in order of increasing vapour pressure at a given temperature. SF6 \quad SiH4 \quad SF4

Place the following compounds in order of increasing strength of intermolecular forces. CH4 \quad CH3CH2CH3 \quad CH3CH3

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

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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

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Gibbs Energy and Thermodynamics

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Chemistry of the Nonmetals

Metals and Metallurgy

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Filters

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

A metal crystallizes in a face-centred cubic structure and has a density of 11.9 g cm^-3.If the radius of the metal atom is 138 pm,what is the identity of the metal?

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.

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 $\sqrt{2}$ r.

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 increasing vapour pressure at a given temperature. SF₆ $\quad$ SiH₄ $\quad$ SF₄

Place the following compounds in order of increasing strength of intermolecular forces. CH₄ $\quad$ CH₃CH₂CH₃ $\quad$ CH₃CH₃