Question 1

Which of the following best explains why substances with strong intermolecular forces generally have higher boiling points?

Accepted Answer

Because more energy is required to overcome the attractive forces between molecules.

Question 2

Which type of intermolecular force is primarily responsible for the high boiling point of water ($$\mathrm{H_2O}$$)?

Accepted Answer

Hydrogen bonding

Question 3

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

Accepted Answer

$$\mathrm{NH_3$}$$

Question 4

Which statement best describes London dispersion forces?

Accepted Answer

They are temporary attractions caused by momentary uneven electron distributions.

Question 5

Which of the following molecules is nonpolar and only exhibits London dispersion forces?

Accepted Answer

$$\mathrm{H_2$}$$

Question 6

Given the molecules $$\mathrm{CH_3F}$$ and $$\mathrm{CH_4$}$$, which has a higher boiling point and why?

Accepted Answer

$$\mathrm{CH_3F}$$, because it has dipole-dipole interactions in addition to London dispersion forces.

Question 7

Which of the following best explains why ethanol ($$\mathrm{C_2H_5OH}) is $$soluble in water?

Accepted Answer

Ethanol can form hydrogen bonds with water molecules.

Question 8

Which molecule would you expect to have the lowest boiling point: $$\mathrm{C_2H_6}$$, $$\mathrm{C_2H_5OH}$$, $$\mathrm{CH_3F}$$, or $$\mathrm{H_2O}$$?

Accepted Answer

$$\mathrm{C_2H_6}$$

Question 9

Which of the following statements about the boiling points of methane ($$\mathrm{CH_4$}$$), ethane ($$\mathrm{C_2H_6}$$), and propane ($$\mathrm{C_3H_8}) is $$correct?

Accepted Answer

Boiling point increases as the number of carbon atoms increases due to stronger London dispersion forces.

Question 10

Which of the following best describes why oil does not dissolve in water?

Accepted Answer

Oil is nonpolar and water is polar, so there are no significant intermolecular attractions between them.

Question 11

Which of the following molecules can exhibit hydrogen bonding: $$\mathrm{HF}$$, $$\mathrm{HCl}$$, $$\mathrm{HBr}$$, $$\mathrm{HI}$$?

Accepted Answer

$$\mathrm{HF}$$

Question 12

Which of the following best explains why $$\mathrm{$$CCl_4$$} is $$nonpolar even though it contains polar bonds?

Accepted Answer

The molecule is symmetrical, so the bond dipoles cancel out.

Question 13

Which of the following molecules is most likely to be soluble in hexane ($$\mathrm{C_6H_{14}}$$)?

Accepted Answer

$$\mathrm{$$CCl_4$$}$$

Question 14

Which of the following best describes the intermolecular forces present in $$\mathrm{CO_2$}$$?

Accepted Answer

London dispersion forces only

Question 15

Which of the following molecules is polar: $$\mathrm{CO_2$}$$, $$\mathrm{H_2O}$$, $$\mathrm{$$CCl_4$$}$$, $$\mathrm{CH_4$}$$?

Accepted Answer

$$\mathrm{H_2O}$$

Question 16

Which of the following best explains why propane ($$\mathrm{C_3H_8}) $$has a lower boiling point than ethanol ($$\mathrm{C_2H_5OH}$$)?

Accepted Answer

Propane only has London dispersion forces, while ethanol can form hydrogen bonds.

Intermolecular Forces, Liquids, and Boiling Points: Study Guide

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