Question 1

Which of the following best describes the change that occurs when liquid water evaporates, as shown in the first two images?

Accepted Answer

A physical change occurs, with water molecules moving farther apart and entering the gas phase.

Question 2

Refer to the third image (two circles with particles). Which circle best represents the arrangement of water molecules in the gas phase after evaporation?

Accepted Answer

The left circle, where particles are far apart and move freely.

Question 3

A balloon is filled with helium gas. What happens to the mass and volume of the balloon compared to when it was empty?

Accepted Answer

The mass increases and the volume increases.

Question 4

Which of the following gases is colorless, odorless, and flammable at room temperature, as shown in the table of common gases?

Accepted Answer

Methane ($$\mathrm{CH_4$})$$

Question 5

Which of the following elements are diatomic gases at standard temperature and pressure (STP)?

Accepted Answer

Hydrogen ($$\mathrm{H_2$}$$), Nitrogen ($$\mathrm{N_2$}$$), Oxygen ($$\mathrm{O_2$}$$), Fluorine ($$\mathrm{F_2$}$$), and Chlorine ($$\mathrm{Cl_2$})$$

Question 6

A barometer is used to measure atmospheric pressure. Why is mercury used instead of water in a barometer?

Accepted Answer

Mercury is much denser than water, so the column is much shorter and more practical.

Question 7

According to Boyle’s Law, what happens to the volume of a gas if the pressure is doubled at constant temperature?

Accepted Answer

The volume is halved.

Question 8

A sample of gas occupies 4.00 L at 1.00 atm and 300 K. What will be its volume at 2.00 atm and 300 K?

Accepted Answer

$$2.00\ \mathrm{L}$$

Question 9

Which of the following statements is NOT an assumption of the Kinetic Molecular Theory of Gases?

Accepted Answer

Gas particles have strong attractive forces between them.

Question 10

Which intermolecular force is present in all molecular compounds, regardless of polarity?

Accepted Answer

London Dispersion Forces

Question 11

Which of the following compounds can form hydrogen bonds with water?

Accepted Answer

Ammonia ($$\mathrm{NH_3$})$$

Question 12

Which of the following best explains why water has a higher boiling point than methane ($$\mathrm{CH_4$}$$)?

Accepted Answer

Water forms hydrogen bonds, which are much stronger than the London dispersion forces in methane.

Question 13

Which type of intermolecular force is primarily responsible for the solubility of NaCl in water?

Accepted Answer

Ion-dipole interactions

Question 14

Which of the following statements best describes the 'like dissolves like' rule?

Accepted Answer

Polar solutes dissolve in polar solvents, and nonpolar solutes dissolve in nonpolar solvents.

Question 15

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

Accepted Answer

Oil is nonpolar and water is polar, so they do not have compatible intermolecular forces.

Question 16

Which of the following best describes an amphipathic molecule?

Accepted Answer

A molecule with both hydrophilic (polar) and hydrophobic (nonpolar) regions.

Question 17

Why are fats solid and oils liquid at room temperature?

Accepted Answer

Fats have more saturated hydrocarbon chains, allowing stronger London dispersion forces and tighter packing.

Question 18

Which of the following best describes the structure of a cell membrane?

Accepted Answer

A bilayer of phospholipids with hydrophilic heads facing outward and hydrophobic tails facing inward.

Question 19

What is the primary role of cholesterol in the cell membrane?

Accepted Answer

It modulates membrane fluidity by interacting with both saturated and unsaturated phospholipid tails.

States of Matter and Their Attractive Forces: Gas Laws, Solubility, and Applications to the Cell Membrane

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