Question 1

Which of the following statements best distinguishes between intermolecular and intramolecular forces?

Accepted Answer

Intramolecular forces are the forces that hold atoms together within a molecule, while intermolecular forces are the forces between molecules.

Question 2

Which of the following molecules can form hydrogen bonds with itself?

Accepted Answer

NH3

Question 3

Why does water expand upon freezing, unlike most other substances?

Accepted Answer

Because the hydrogen bonds in ice arrange the molecules in a more open structure, increasing the volume.

Question 4

Which of the following best explains why hydrogen bonding leads to higher boiling points in substances like H2O and HF?

Accepted Answer

Hydrogen bonds are stronger than both London dispersion and dipole-dipole forces, requiring more energy to break.

Question 5

Which of the following compounds would you expect to have the highest surface tension at room temperature?

Accepted Answer

Water (H2O)

Question 6

A solution of NaCl in water is an example of which type of intermolecular force being most significant?

Accepted Answer

Ion-dipole forces

Question 7

Which of the following best describes the trend in viscosity for a series of hydrocarbons as their molar mass increases?

Accepted Answer

Viscosity increases because stronger London dispersion forces make it harder for molecules to move past each other.

Question 8

Which of the following is NOT a requirement for hydrogen bonding to occur between molecules?

Accepted Answer

The molecule must be ionic.

Question 9

Which of the following best explains why H2O has a much higher boiling point than H2S, even though both are group 6A hydrides?

Accepted Answer

H2O forms strong hydrogen bonds, while H2S does not.

Question 10

Which of the following best describes the effect of increasing temperature on the surface tension of a liquid?

Accepted Answer

Surface tension decreases because increased kinetic energy allows molecules to overcome intermolecular forces more easily.

Question 11

Which of the following molecules exhibits only London dispersion forces as its intermolecular force?

Accepted Answer

I2

Question 12

Which of the following best explains why CCl4 has a higher boiling point than CH3F, even though CH3F is polar?

Accepted Answer

CCl4 has a much higher molar mass, resulting in stronger London dispersion forces.

Question 13

Which of the following is the strongest type of intermolecular force present in a mixture of NaCl dissolved in water?

Accepted Answer

Ion-dipole forces

Question 14

Which of the following best describes capillary action?

Accepted Answer

The rising of a liquid through a narrow tube due to the competition between cohesive and adhesive forces.

Question 15

Which of the following is a real-life example of hydrogen bonding playing a critical biological role?

Accepted Answer

The double-helix structure of DNA is stabilized by hydrogen bonds between base pairs.

Question 16

Which of the following statements about the viscosity of water is correct based on the data provided?

Accepted Answer

Viscosity decreases as temperature increases.

Question 17

Which of the following molecules can form the greatest number of hydrogen bonds with neighboring molecules?

Accepted Answer

H2O

Question 18

Which of the following best explains why glycerin (C3H8O3) is a liquid at room temperature while CS2 and Br2 are not?

Accepted Answer

Glycerin can form hydrogen bonds, which are much stronger than the London dispersion forces present in CS2 and Br2.

Question 19

Which of the following is the correct order of increasing strength of intermolecular forces?

Accepted Answer

London dispersion < dipole-dipole < hydrogen bonding < ion-dipole

Question 20

Which of the following best explains why surface tension is higher in water than in ethanol?

Accepted Answer

Water forms more extensive hydrogen bonding networks than ethanol.

Solids, Liquids, and Intermolecular Forces: Study Guide

Study Guide - Practice Questions