Exam 1

Of the following, a 0.1 M aqueous solution of _____ will have the lowest freezing point. A. NaCl B. Al(NO₃)₃ C. K₂CrO₄ D. Na₂SO₄ E. Sucrose

B. Al(NO₃)₃

The dissolution of water in octane (C₈H₁₈) is prevented by __________. A. London dispersion forces between octane molecules B. Hydrogen bonding between water molecules C. Dipole Dipole attraction between water molecules D. Ion dipole attraction between water and octane molecules E. Repulsion between like-charged water and octane molecules

B. Hydrogen bonding between water molecules

________ solids consist of atoms or molecules held together by dipole-dipole forces, London dispersion forces, and/or hydrogen bonds. A. Ionic B. Molecular C. Metallic D. Covalent Network E. Metallic and Covalent Network

B. Molecular

The phrase "like dissolves like" refers to the fact that _____. A. Gases can only dissolve other gases. B. Polar solvents dissolve polar solutes and non-polar solvents dissolve non-polar solutes. C. Solvents can only dissolve solutes of similar molar mass. D. Condensed phases can only dissolve other condensed phases. E. Polar solvents dissolve non-polar solutes and vice versa.

B. Polar solvents dissolve polar solutes and non-polar solvents dissolve non-polar solutes.

Which of the following statements is false? A. Non-polar liquids tend to be insoluble in polar liquids. B. The weaker the attraction between the solute and solvent molecules, the greater the solubility. C. Substances with similar intermolecular attractive forces tend to be soluble in one another. D. The solubility of a gas increases in direct proportion to its partial pressure above the solution. E. The solubility of gases in water decreases with increasing temperature.

B. The weaker the attraction between the solute and solvent molecules, the greater the solubility.

Hydrogen bonding is a special case of _____. A. London-dispersion forces B. Ion-dipole attraction C. Dipole-dipole attraction D. Ion-ion interactions E. None of the above

C. Dipole-dipole attraction

The process of solute particles being surrounded by solvent particles is known as _______. A. Salutation B. Agglomeration C. Solvation D. Agglutination E. Dehydration

C. Solvation

Which of the following is not a type of solid? A. Ionic B. Molecular C. Supercritical D. Metallic E. Covalent-Network

C. Supercritical

The shape of a liquid's meniscus is determined by ____. A. The viscosity of the liquid. B. The type of material the container is made of. C. The relative magnitude of cohesive forces in the liquid and adhesive forces between the liquid and its container. D. The amount of hydrogen bonding in the liquid. E. The volume of the liquid.

C. The relative magnitude of cohesive forces in the liquid and adhesive forces between the liquid and its container.

The ideal value of i (van't Hoff factor) for (NH₄)₃PO₄ A. 1 B. 2 C. 3 D. 4 E. 5

D. 4

In which of the following molecules is hydrogen bonding likely to be the most significant component of the total intermolecular forces? A. CH₄ B. C₅H₁₁OH C. C₆H₁₃NH₂ D. CH₃OH E. CO₂

D. CH₃OH

Of the following substances, only ____ has London dispersion force: A. CH₃OH B. NH₃ C. H₂S D. CH₄ E. HCl

D. CH₄

Which of the following substances would be most soluble in CCl₄? A. CH₃CH₂OH B. H₂O C. NH₃ D. C₁₀H₂₂ E. NaCl

D. C₁₀H₂₂

As the concentration of a solute in a solution increases, the freezing point of the solution ______ and the vapor pressure of the solution _____. A. Increases, increases B. Increases, decreases C. Decreases, increases D. Decreases, decreases E. Decreases, is unaffected

D. Decreases, decreases

Molality is defined as the _______. A. moles solute/moles solvent B. Moles solute/liters solution C. Moles solute/kg solution D. Moles solute/kg solvent E. None (dimensionless)

D. Moles solute/kg solvent

Which one of the following should have the lowest boiling point? A. PH₃ B. H₂S C. HCl D. SiH₄ E. H₂O

D. SiH₄

In a saturated solution of salt in water, ______. A. the rate of crystallization > the rate of dissolution B. The rate of dissolution > the rate of crystallization C. Seed crystal addition may case massive crystallization. D. The rate of crystallization = the rate of dissolution. E. Addition of more water causes massive crystallization.

D. The rate of crystallization = the rate of dissolution.

Which of the following is most soluble in water? A. CH₃OH B. CH₃CH₂CH₂OH C. CH₃CH₂OH D. CH₃CH₂CH₂CH₂OH E. CH₃CH₂CH₂CH₂CH₂OH

A. CH₃OH

Pressure has an appreciable effect on the solubility of _______ in liquids. A. Gases B. Solids C. Liquids D. Salts E. Solids and Liquids

A. Gases

The substance with the largest heat of vaporization is ____. A. I₂ B. Br₂ C. Cl₂ D. F₂ E. O₂

A. I₂

What is the predominant intermolecular force in CBr₄? A. London-dispersion forces B. Ion-dipole attraction C. Ionic bonding D. Dipole-dipole attraction E. Hydrogen bonding

A. London-dispersion forces

Pairs of liquids that ill mix in all proportions are called _____ liquids. A. Miscible B. Unsaturated C. Polar Liquids D. Saturated E. Supersaturated

A. Miscible

The dissolution of gases in water is virtually always exothermic because ______. A. One of the two endothermic steps (separation of solute particles) in the solution formation process is unnecessary. B. The exothermic step in the solution-formation process is unnecessary. C. Gases react exothermically with water. D. Neither of the two endothermic steps in the solution formation process is necessary. E. All three steps in the solution formation process are exothermic.

A. One of the two endothermic steps (separation of solute particles) in the solution formation process is unnecessary.

Which Statements about viscosity are true? (i) viscosity increases as temperature decreases. (ii) viscosity increases as molecular weight increases. (iii) viscosity increases as intermolecular forces increase. A. (i) B. (i) and (iii) C. (ii) and (iii) D. none E. All

E. All

Large intermolecular forces in a substance are manifested by _________: A. Low vapor pressure B. High boiling point C. High heats of fusion and vaporization D. High critical temperatures and pressures E. All of the above

E. All of the above

In liquids, the attractive intermolecular forces are ______. A. Very weak compared with kinetic energies of the molecules. B. Strong enough to hold the molecules relatively close together. C. Strong enough to keep the molecules confined to vibrating about their fixed lattice positions. D. Not strong enough to keep molecules from moving past each other. E. Strong enough to hold molecules relatively close together but not strong enough to keep the molecules from moving past each other.

E. Strong enough to hold molecules relatively close together but not strong enough to keep the molecules from moving past each other.

Colligative properties of solutions include all of the following except _______. A. Depression of vapor pressure upon addition of a solute to a solvent. B. Elevation of the boiling point of a solution upon addition of a solute to a solvent. C. Depression of the freezing point of a solution upon addition of a solute to a solvent. D. An increase in the osmotic pressure of a solution upon the addition of more solute. E. The increase of reaction rates with increase in temperature.

E. The increase of reaction rates with increase in temperature.