Question 1

Which type of intermolecular force is primarily responsible for the high boiling point of water compared to other molecules of similar size?

Accepted Answer

Hydrogen bonding

Question 2

Refer to the images of water molecules in different arrangements. Which image best represents the solid phase (ice) of water, and why?

Accepted Answer

The image with water molecules arranged in a regular, open lattice due to hydrogen bonding, resulting in lower density.

Question 3

Which of the following best explains why ice floats on liquid water?

Accepted Answer

Ice has a lower density than liquid water because its hydrogen-bonded structure forms an open lattice.

Question 4

The diagram showing two HCl molecules with a dashed line between them illustrates which concept?

Accepted Answer

A dipole-dipole intermolecular force

Question 5

Which of the following statements about intermolecular forces (IMFs) is correct?

Accepted Answer

IMFs are responsible for the existence of solids and liquids.

Question 6

Which type of intermolecular force is present in all molecules, regardless of polarity?

Accepted Answer

London dispersion forces

Question 7

Why does n-pentane have a higher boiling point than neopentane, even though they have the same molar mass?

Accepted Answer

n-Pentane has a more extended shape, allowing greater surface area for dispersion forces.

Question 8

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

Accepted Answer

HF

Question 9

What is the primary intermolecular force between I2 molecules in the solid state?

Accepted Answer

London dispersion forces

Question 10

Which of the following best describes the interaction between Na+ ions and water molecules in an aqueous solution?

Accepted Answer

Ion-dipole interaction, with the oxygen atom of water oriented toward the Na+ ion.

Question 11

Which of the following statements about the boiling points of formaldehyde (CH2O) and ethane (C2H6) is correct?

Accepted Answer

Formaldehyde has a higher boiling point due to dipole-dipole interactions.

Question 12

Which of the following best explains why O2 can dissolve in water, even though O2 is nonpolar?

Accepted Answer

A dipole-induced dipole interaction occurs, where water induces a temporary dipole in O2.

Question 13

Which of the following is the strongest type of intermolecular force?

Accepted Answer

Ion-dipole forces

Question 14

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

Accepted Answer

Viscosity decreases with increasing temperature.

Question 15

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

Accepted Answer

Water is polar and pentane is nonpolar, so their intermolecular forces are not compatible.

Question 16

Which of the following molecules would you expect to have the highest boiling point?

Accepted Answer

CH3OH

Question 17

Which of the following is a correct order of increasing boiling points for the following substances: CH4, CH3OH, H2?

Accepted Answer

H2 < CH4 < CH3OH

Question 18

Which of the following best describes the relationship between intermolecular forces and vapor pressure?

Accepted Answer

Stronger intermolecular forces result in lower vapor pressure.

Question 19

Which of the following best describes the effect of molecular shape on the magnitude of dispersion forces?

Accepted Answer

Straight-chain molecules have higher boiling points due to greater surface-to-surface contact.

Question 20

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

Accepted Answer

The molecule must be ionic

Intermolecular Forces and Their Effects on Properties of Solids, Liquids, and Solutions

Study Guide - Practice Questions