© 2015 pearson education, inc. chapter 12 liquids, solids, and intermolecular forces laurie leblanc...

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Chapter 12

Liquids, Solids, and Intermolecular

Forces

Laurie LeBlancCuyamaca College

Clicker Questions

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A. intramolecular.B. intermolecular.C. molecular.D. covalent.E. ionic.

A force that occurs between molecules is called

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A. intramolecular.B. intermolecular.C. molecular.D. covalent.E. ionic.

A force that occurs between molecules is called

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A. intramolecular.B. ionic.C. covalent.D. All of the aboveE. Two of the above

A force that occurs between atoms within a compound might be

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A. intramolecular.B. ionic.C. covalent.D. All of the aboveE. Two of the above

A force that occurs between atoms within a compound might be

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A. Carbon dioxideB. WaterC. Rubbing alcoholD. Table sugarE. Gasoline

Which pure compound has the highest total intermolecular forces per molecule at 25 °C?

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A. Carbon dioxideB. WaterC. Rubbing alcoholD. Table sugarE. Gasoline

Which pure compound has the highest total intermolecular forces per molecule at 25 °C?

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A. The molecules are close together.B. The density is higher than its gas.C. It is not compressed easily.D. It assumes the shape of its container.E. All of the above

Which property describes a molecular liquid?

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Which property describes a molecular liquid?

A. The molecules are close together.B. The density is higher than its gas.C. It is not compressed easily.D. It assumes the shape of its container.E. All of the above

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A. The solid has a lower density than gas.B. The solid has a lower average kinetic energy than gas

at the same temperature.C. The solid is easy to compress.D. The solid does not assume the shape of its container.E. All of the above

Which property best describes a molecular solid?

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A. The solid has a lower density than gas.B. The solid has a lower average kinetic energy than gas

at the same temperature.C. The solid is easy to compress.D. The solid does not assume the shape of its container.E. All of the above

Which property best describes a molecular solid?

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A. It is less dense than water.B. It is more dense than water.C. The repulsive forces override the attractive forces.D. There are strong intermolecular forces between the

water and the metal.E. The molecules of water

attract each other and keep it from sinking.

Why doesn’t a paper clip sink when the clip is placed gently on water?

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A. It is less dense than water.B. It is more dense than water.C. The repulsive forces override the attractive forces.D. There are strong intermolecular forces between the

water and the metal.E. The molecules of water

attract each other and keep it from sinking.

Why doesn’t a paper clip sink when the clip is placed gently on water?

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A. Oxygen gasB. Pancake syrupC. Running waterD. Liquid heliumE. Rubbing alcohol

Which of the following has the highest viscosity?

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A. Oxygen gasB. Pancake syrupC. Running waterD. Liquid heliumE. Rubbing alcohol

Which of the following has the highest viscosity?

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A. condensation.B. evaporation.C. sublimation.D. vaporization.E. Two of the above

The transformation from a liquid to a gas is called

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A. condensation.B. evaporation.C. sublimation.D. vaporization.E. Two of the above

The transformation from a liquid to a gas is called

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A. It remains unchanged. B. It decreases.C. It increases.D. None of the aboveE. All of the above

What happens to the kinetic energy of gaseous water molecules during condensation?

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A. It remains unchanged. B. It decreases.C. It increases.D. None of the aboveE. All of the above

What happens to the kinetic energy of gaseous water molecules during condensation?

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A. Gold B. Vegetable oilC. WaterD. Motor oilE. Fingernail polish remover

Which of the following is the most volatile?

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A. Gold B. Vegetable oilC. WaterD. Motor oilE. Fingernail polish remover

Which of the following is the most volatile?

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A. The boiling point increases with higher pressure.B. The boiling point increases with lower pressure.C. The boiling point decreases with higher pressure.D. The boiling point decreases with lower pressure.E. Two of the above

What is the relationship between the external pressure and the boiling point of a compound?

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A. The boiling point increases with higher pressure.B. The boiling point increases with lower pressure.C. The boiling point decreases with higher pressure.D. The boiling point decreases with lower pressure.E. Two of the above

What is the relationship between the external pressure and the boiling point of a compound?

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A. OxygenB. Water vaporC. NothingD. HydrogenE. Nitrogen

What is the gas found within a bubble of boiling water?

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A. OxygenB. Water vaporC. NothingD. HydrogenE. Nitrogen

What is the gas found within a bubble of boiling water?

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A. BoilingB. FreezingC. CondensationD. Both a and bE. Both b and c

Which of the following processes are exothermic?

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A. BoilingB. FreezingC. CondensationD. Both a and bE. Both b and c

Which of the following processes are exothermic?

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A. 5 grams of water at 100 °CB. 5 grams of water at 75 °CC. 5 grams of steam at 100 °CD. 5 grams of water at 0 °CE. 5 grams of ice at 0 °C

Which of the following contains the most thermal energy?

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A. 5 grams of water at 100 °CB. 5 grams of water at 75 °CC. 5 grams of steam at 100 °CD. 5 grams of water at 0 °CE. 5 grams of ice at 0 °C

Which of the following contains the most thermal energy?

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A. 1.85 × 103 kJB. 1.12 kJC. 103 kJD. 2.52 kJE. 40.6 kJ

How much energy is required to boil 45.5 g of water at 100 °C at sea level? The molar heat of vaporization of water is 40.6 kJ/mol.

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A. 1.85 × 103 kJB. 1.12 kJC. 103 kJD. 2.52 kJE. 40.6 kJ

How much energy is required to boil 45.5 g of water at 100 °C at sea level? The molar heat of vaporization of water is 40.6 kJ/mol.

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A. 27.1 kJB. 6.02 kJC. 1.34 kJD. 1.50 kJE. 30.5 kJ

How much energy is required to melt 4.50 mol of ice at 0 °C? The molar heat of fusion of water is 6.02 kJ/mol.

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A. 27.1 kJB. 6.02 kJC. 1.34 kJD. 1.50 kJE. 30.5 kJ

How much energy is required to melt 4.50 mol of ice at 0 °C? The molar heat of fusion of water is 6.02 kJ/mol.

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A. The rate of freezing is faster.B. The rate of melting is faster.C. The ice will always melt.D. The water will always freeze.E. The rates of freezing and melting are equal.

Which statement is most likely true concerning an ice/water mixture kept at 0 °C?

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A. The rate of freezing is faster.B. The rate of melting is faster.C. The ice will always melt.D. The water will always freeze.E. The rates of freezing and melting are equal.

Which statement is most likely true concerning an ice/water mixture kept at 0 °C?

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A. CovalentB. Dipole–dipoleC. Hydrogen bondingD. MolecularE. Dispersion

Which type of intermolecular force is the strongest?

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A. CovalentB. Dipole–dipoleC. Hydrogen bondingD. MolecularE. Dispersion

Which type of intermolecular force is the strongest?

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A. IonicB. Dipole–dipoleC. Hydrogen bondingD. DispersionE. Covalent

Which intermolecular force allows water to bead on a surface?

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A. IonicB. Dipole–dipoleC. Hydrogen bondingD. DispersionE. Covalent

Which intermolecular force allows water to bead on a surface?

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A. CH3CH2CH3

B. CH3CH2NH2

C. CH3OCH3

D. CH4

E. CH3CH2OH

Which of the following has the highest boiling point?

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A. CH3CH2CH3

B. CH3CH2NH2

C. CH3OCH3

D. CH4

E. CH3CH2OH

Which of the following has the highest boiling point?

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A. CH3CH2CH3

B. CH3CH2NH2

C. CH3OCH3

D. H2O

E. CH3CH2OH

Which of the following is least soluble in water?

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A. CH3CH2CH3

B. CH3CH2NH2

C. CH3OCH3

D. H2O

E. CH3CH2OH

Which of the following is least soluble in water?

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A. Dipole–dipoleB. Hydrogen bondingC. DispersionD. IonicE. Covalent

What type of intermolecular force causes today’s Saran Wrap to stick to itself?

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A. Dipole–dipoleB. Hydrogen bondingC. DispersionD. IonicE. Covalent

What type of intermolecular force causes today’s Saran Wrap to stick to itself?

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A. NaCl, Ar, CO2, H2O

B. Ar, NaCl, H2O, CO2

C. H2O, CO2, NaCl, Ar

D. Ar, CO2, H2O, NaCl

E. CO2, H2O, Ar, NaCl

Arrange the following in order of increasing melting point:

CO2, Ar, H2O, NaCl

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A. NaCl, Ar, CO2, H2O

B. Ar, NaCl, H2O, CO2

C. H2O, CO2, NaCl, Ar

D. Ar, CO2, H2O, NaCl

E. CO2, H2O, Ar, NaCl

Arrange the following in order of increasing melting point:

CO2, Ar, H2O, NaCl

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A. MolecularB. IonicC. AtomicD. AmorphousE. None of the above

What type of crystalline solid is formed by potassium iodide?

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A. MolecularB. IonicC. AtomicD. AmorphousE. None of the above

What type of crystalline solid is formed by potassium iodide?

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A. C6H12O6

B. HClC. S8

D. NaClE. None of the above

Which of the following is an example of an atomic solid?

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A. C6H12O6

B. HClC. S8

D. NaClE. None of the above

Which of the following is an example of an atomic solid?

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A. The density of a liquid is greater than its solid.B. Solids have a definite shape; liquids do not.C. Liquids and solids are easily compressed.D. None of the aboveE. All of the above

Which of the following is/are true?

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A. The density of a liquid is greater than its solid.B. Solids have a definite shape; liquids do not.C. Liquids and solids are easily compressed.D. None of the aboveE. All of the above

Which of the following is/are true?

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A. Substances with stronger intermolecular forces are less viscous than those with more.

B. Molecules with greater length have greater viscosity.C. Substances with stronger intermolecular forces are more

viscous than those with less.D. Both a and b are true.E. Both b and c are true.

Which of the following is/are true of viscosity?

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A. Substances with stronger intermolecular forces are less viscous than those with more.

B. Molecules with greater length have greater viscosity.C. Substances with stronger intermolecular forces are more

viscous than those with less.D. Both a and b are true.E. Both b and c are true.

Which of the following is/are true of viscosity?

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A. Although water has a low molar mass, its boiling point is relatively high.

B. Because water is so polar, it is able to dissolve some ionic compounds.

C. Ice is less dense than liquid water.D. Hydrogen bonding is responsible for

many of water’s unique properties.E. None of the above

Which of the following is NOT true of water?

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A. Although water has a low molar mass, its boiling point is relatively high.

B. Because water is so polar, it is able to dissolve some ionic compounds.

C. Ice is less dense than liquid water.D. Hydrogen bonding is responsible for

many of water’s unique properties.E. None of the above

Which of the following is NOT true of water?

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A. 791.0 kJB. 43.9 kJC. 393 kJD. 297 kJE. 87.65 kJ

How much heat is required to melt 131.4 g of ice at 0.0 °C? (ΔHfus for H2O is 6.02 kJ/mol.)

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A. 791.0 kJB. 43.9 kJC. 393 kJD. 297 kJE. 87.65 kJ

How much heat is required to melt 131.4 g of ice at 0.0 °C? (ΔHfus for H2O is 6.02 kJ/mol.)

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A. C3H8

B. CO2

C. CH2O

D. Br2

E. CS2

Which of the following molecules have dipole–dipole forces?

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A. C3H8

B. CO2

C. CH2O

D. Br2

E. CS2

Which of the following molecules have dipole–dipole forces?