$\text{Surface Tension} = \frac{\text{Energy}}{\text{Area}}$

Question 1

Which of the following molecules is capable of forming hydrogen bonds with water molecules?

Accepted Answer

CH3NH2

Question 2

Why does water have a higher boiling point than hydrogen sulfide (H2S), despite both being group 6A hydrides?

Accepted Answer

Water forms extensive hydrogen bonds, which are stronger than the intermolecular forces in H2S.

Question 3

Which intermolecular force is primarily responsible for the high melting and boiling points of glycerin?

Accepted Answer

Hydrogen bonding

Question 4

A solution of sodium chloride in water is stabilized by which type of intermolecular force?

Accepted Answer

Ion-dipole forces

Question 5

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

Accepted Answer

Hydrogen bonding in ice creates an open, hexagonal structure with more empty space.

Question 6

Which intermolecular forces are present in formaldehyde (CH2O)?

Accepted Answer

London dispersion and dipole-dipole forces

Question 7

Which equation describes the energy required to increase the surface area of a liquid by a unit amount?

Accepted Answer

$	ext{Surface Tension} = \frac{	ext{Energy}}{	ext{Area}}$

Question 8

Which of the following best describes the relationship between viscosity and temperature for liquid water?

Accepted Answer

Viscosity decreases as temperature increases.

Question 9

Which of the following molecules can form four hydrogen bonds per molecule in the solid state?

Accepted Answer

Water ($	ext{H}_2	ext{O}$)

Question 10

Which intermolecular force is responsible for the attraction between the base pairs in DNA?

Accepted Answer

Hydrogen bonding

Question 11

Which of the following statements about hydrogen bonding is TRUE?

Accepted Answer

Hydrogen bonding is an intermolecular force that occurs when hydrogen is bonded to F, O, or N.

Question 12

Which of the following substances will have the highest surface tension at room temperature?

Accepted Answer

Water ($	ext{H}_2	ext{O}$)

Question 13

Which of the following best explains why n-nonane has a higher viscosity than n-pentane?

Accepted Answer

n-Nonane has a higher molar mass, leading to stronger London dispersion forces.

Question 14

Which of the following is NOT a factor affecting the strength of ion-dipole interactions?

Accepted Answer

Number of hydrogen bonds formed

Question 15

Which of the following best describes capillary action in water?

Accepted Answer

Adhesive forces are stronger than cohesive forces, resulting in a concave meniscus.

Question 16

Which of the following molecules will have the strongest London dispersion forces?

Accepted Answer

CCl4

Question 17

Which of the following is a correct statement about the boiling points of group 4A and group 6A hydrides?

Accepted Answer

Group 6A hydrides have higher boiling points than group 4A hydrides because of hydrogen bonding in water.

Question 18

Which of the following molecules is liquid at room temperature due to hydrogen bonding?

Accepted Answer

Hydrogen peroxide

Question 19

Which intermolecular force is present in all molecules and atoms, regardless of their polarity?

Accepted Answer

London dispersion forces

Question 20

Which of the following best explains why motor oil must maintain proper viscosity at both high and low temperatures?

Accepted Answer

To provide effective lubrication by preventing the oil from becoming too thin or too thick.

Solids, Liquids, and Intermolecular Forces: Study Guide

Study Guide - Practice Questions