Question 1

Which of the following statements best explains why oil and water do not mix?

Accepted Answer

Oil is nonpolar and water is polar, so their intermolecular forces are incompatible.

Question 2

Which intermolecular force is primarily responsible for the liquefaction of noble gases at low temperatures?

Accepted Answer

London dispersion forces

Question 3

Which of the following molecules would exhibit hydrogen bonding?

Accepted Answer

NH$_3$

Question 4

Why does water have a higher boiling point than hydrogen sulfide (H$_2$S)?

Accepted Answer

Water forms strong hydrogen bonds, while H$_2$S does not.

Question 5

Which of the following best describes the effect of molecular size on London dispersion forces?

Accepted Answer

Larger and heavier molecules exhibit stronger dispersion forces.

Question 6

Which of the following is an example of an ion-dipole interaction?

Accepted Answer

Na$^+$ ions surrounded by water molecules

Question 7

Which of the following statements about dispersion forces is FALSE?

Accepted Answer

Dispersion forces only occur in polar molecules.

Question 8

Which of the following best explains why n-pentane has a higher boiling point than neopentane?

Accepted Answer

n-Pentane has a greater surface area, leading to stronger dispersion forces.

Question 9

Which of the following is NOT a van der Waals force?

Accepted Answer

Ion-dipole interaction

Question 10

Which of the following scenarios involves a dipole-induced dipole interaction?

Accepted Answer

Oxygen gas dissolving in water

Question 11

Which of the following is a necessary condition for hydrogen bond formation?

Accepted Answer

A hydrogen atom bonded to a highly electronegative atom such as F, O, or N

Question 12

Which of the following best explains why ice is less dense than liquid water?

Accepted Answer

Ice forms a cage-like structure due to hydrogen bonding, creating more open space.

Question 13

Which of the following best describes the process of solution formation?

Accepted Answer

It involves breaking solute-solute and solvent-solvent attractions (endothermic) and forming solute-solvent attractions (exothermic).

Question 14

If the sum of the endothermic terms in solution formation is greater than the exothermic term, what is the sign of $\Delta H_{solution}$ and what drives the process?

Accepted Answer

$\Delta H_{solution}$ is positive (endothermic), and increased entropy can still drive solution formation.

Question 15

Which of the following is the correct expression for the enthalpy of solution?

Accepted Answer

$\Delta H_{solution} = \Delta H_{solute} + \Delta H_{solvent} + \Delta H_{mix}$

Question 16

Which of the following best explains why sodium chloride dissolves in water?

Accepted Answer

The ion-dipole interactions between Na$^+$, Cl$^-$ and water molecules are strong enough to overcome the lattice energy.

Question 17

Which of the following is TRUE about the solubility of gases in water as temperature increases?

Accepted Answer

The solubility of gases in water decreases with increasing temperature.

Question 18

According to Henry's Law, which equation correctly relates the solubility of a gas to its partial pressure?

Accepted Answer

$S_{gas} = k_H P_{gas}$

Question 19

Which of the following best describes the effect of pressure on the solubility of gases in liquids?

Accepted Answer

Increasing the pressure of a gas above a liquid increases its solubility in the liquid.

Intermolecular Forces and Solution Formation: Chapter 13 Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards