Q: Which equation correctly represents the relationship between heat, mass, specific heat, and temperature change for heating a substance?

$q = m \times C_s \times \Delta T$

Question 1

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

Accepted Answer

Ice has a lower density than liquid water because its molecules form an open, hexagonal structure due to hydrogen bonding.

Question 2

Which intermolecular force is present in all substances, regardless of their polarity?

Accepted Answer

Dispersion forces (London forces)

Question 3

A liquid is placed in a narrow glass tube and forms a concave meniscus. What does this indicate about the relative strengths of adhesive and cohesive forces?

Accepted Answer

Adhesive forces are stronger than cohesive forces.

Question 4

Which of the following molecules can form hydrogen bonds?

Accepted Answer

NH3

Question 5

Why do n-pentane and neopentane, which have the same molar mass, have different boiling points?

Accepted Answer

n-Pentane has more surface-to-surface contact, leading to stronger dispersion forces.

Question 6

Which equation correctly represents the relationship between heat, mass, specific heat, and temperature change for heating a substance?

Accepted Answer

$q = m 	imes C_s 	imes \Delta T$

Question 7

Which of the following best describes the process of vaporization?

Accepted Answer

It is an endothermic process where molecules gain enough energy to escape the liquid phase.

Question 8

Which factor does NOT increase the rate of vaporization of a liquid?

Accepted Answer

Increasing the strength of intermolecular forces

Question 9

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

Accepted Answer

CH3OH

Question 10

What is the main reason that water is a liquid at room temperature while methane (CH4) is a gas?

Accepted Answer

Water molecules form hydrogen bonds, which are much stronger than the dispersion forces in methane.

Question 11

Which of the following best describes the effect of increasing molecular size on the strength of dispersion forces?

Accepted Answer

Dispersion forces increase as molecular size and electron cloud volume increase.

Question 12

Which of the following is true about the boiling point of a liquid at high altitude (lower external pressure)?

Accepted Answer

The boiling point decreases.

Question 13

Which intermolecular force is responsible for the solubility of ionic compounds in water?

Accepted Answer

Ion-dipole forces

Question 14

Which of the following statements about viscosity is correct?

Accepted Answer

Viscosity decreases as temperature increases.

Question 15

A sample of liquid is heated until it reaches its boiling point. What happens to the temperature of the liquid as it boils?

Accepted Answer

The temperature remains constant until all the liquid has vaporized.

Question 16

Which of the following best describes a crystalline solid?

Accepted Answer

A solid with particles arranged in a regular, repeating geometric pattern.

Question 17

Which of the following is NOT a factor that affects the magnitude of dispersion forces?

Accepted Answer

Polarity of the molecule

Question 18

Which process is exothermic?

Accepted Answer

Condensation

Question 19

Which of the following best explains why water has a high surface tension?

Accepted Answer

Water molecules form strong hydrogen bonds, resulting in high cohesive forces.

Question 20

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

Liquids, Solids, and Intermolecular Forces: Chapter 12 Study Notes

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