Q: A sample of gas is collected over water at 25$^ \circ$C. The total pressure is 755 mmHg, and the vapor pressure of water at this temperature is 24 mmHg. What is the pressure of the dry gas?

$755\ \text{mmHg} - 24\ \text{mmHg} = 731\ \text{mmHg}$

Q: A 2.00 L container holds 0.082 mol of an ideal gas at 300 K. What is the pressure inside the container? (Use $R = 0.08206\ \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K}$)

$P = \frac{nRT}{V} = \frac{0.082 \times 0.08206 \times 300}{2.00} \approx 1.01\ \text{atm}$

Question 1

Which of the following substances would you expect to have the strongest London dispersion forces (LDFs)?

Accepted Answer

n-Pentane

Question 2

Which of the following statements best explains why ionic solids are brittle?

Accepted Answer

When the lattice is struck, like charges are forced to touch, causing repulsion and the lattice to shatter.

Question 3

Which of the following intermolecular forces is present in all molecules, regardless of their polarity?

Accepted Answer

London dispersion forces

Question 4

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

Accepted Answer

NH$_3$

Question 5

A sample of gas is collected over water at 25$^
\circ$C. The total pressure is 755 mmHg, and the vapor pressure of water at this temperature is 24 mmHg. What is the pressure of the dry gas?

Accepted Answer

$755\ 	ext{mmHg} - 24\ 	ext{mmHg} = 731\ 	ext{mmHg}$

Question 6

Which of the following best describes the difference between crystalline and amorphous solids?

Accepted Answer

Crystalline solids have an ordered 3D lattice, while amorphous solids have a disordered structure.

Question 7

Which of the following is NOT an assumption of the ideal gas law?

Accepted Answer

Gas particles have strong intermolecular forces.

Question 8

Which of the following solids is characterized by a 'sea of valence electrons' that allows for electrical conductivity?

Accepted Answer

Metallic solids

Question 9

Which of the following would increase the strength of London dispersion forces in a molecule?

Accepted Answer

Increasing the size of the electron cloud (more electrons)

Question 10

Which of the following best explains why water has an unusually high boiling point compared to other group 16 hydrides?

Accepted Answer

Water forms strong hydrogen bonds due to its two hydrogen atoms bonded to a highly electronegative oxygen atom.

Question 11

A 2.00 L container holds 0.082 mol of an ideal gas at 300 K. What is the pressure inside the container? (Use $R = 0.08206\ 	ext{L} \cdot 	ext{atm} / 	ext{mol} \cdot 	ext{K}$)

Accepted Answer

$P = \frac{nRT}{V} = \frac{0.082 	imes 0.08206 	imes 300}{2.00} \approx 1.01\ 	ext{atm}$

Question 12

Which of the following best describes a covalent network solid?

Accepted Answer

A solid in which atoms are held together by a continuous network of covalent bonds.

Question 13

Which of the following statements about hydrogen bonding is TRUE?

Accepted Answer

Hydrogen bonding occurs when hydrogen is bonded to F, O, or N.

Question 14

Which of the following is a property of molecular solids?

Accepted Answer

They have low melting points and are generally poor conductors of electricity.

Question 15

Which of the following best explains why metallic solids are good conductors of electricity?

Accepted Answer

They have a 'sea' of delocalized valence electrons that can move freely.

Question 16

Which of the following is the correct relationship described by Boyle's Law?

Accepted Answer

$P_1 V_1 = P_2 V_2$

Question 17

Which of the following would most likely have the highest boiling point?

Accepted Answer

A substance with strong hydrogen bonding

Question 18

Which of the following is TRUE about the average kinetic energy of an ideal gas?

Accepted Answer

It is proportional to the absolute temperature of the gas.

Question 19

Which of the following best describes an interstitial alloy?

Accepted Answer

A mixture where small atoms fill the spaces between larger metal atoms in the lattice.

Intermolecular Forces, Types of Solids, and Properties of Gases: Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards