AP Chemistry Rapid Review — Concepts + Practice Problems

These flashcards cover key concepts and practice problems from AP Chemistry, focusing on gas laws, intermolecular forces, and chemical reactions.

Explain how Boyle’s Law illustrates the relationship between pressure and volume in gases.

Boyle's Law shows that pressure and volume are inversely related; as the volume of a gas decreases (at constant temperature), the pressure increases due to particles being compressed and colliding with the walls of the container more frequently.

If a gas occupies a volume of 3.00 L at a pressure of 2.00 atm, what will be its volume at a pressure of 1.00 atm?

6.00 L (Use Boyle's Law: P1V1 = P2V2. Hence, (2.00 atm)(3.00 L) = (1.00 atm)(V2), solving gives V2 = 6.00 L. Hint: Remember to keep temperature constant when using this law!)

Discuss the relationship between temperature and average kinetic energy of particles.

As temperature increases, the average kinetic energy of particles also increases because temperature is a measure of the average energy of their motion; higher temperature means more energy, hence faster particles.

A gas has an average kinetic energy of 100 J at 300 K. What will be its average kinetic energy at 600 K?

400 J (Average kinetic energy is directly proportional to temperature. If the temperature doubles, the average kinetic energy will also double. Hint: Use the relationship KE ∝ T.)

Define a polar covalent bond and explain why it occurs.

A polar covalent bond occurs when two atoms with different electronegativities share electrons unevenly, resulting in partial positive and negative charges on the atoms.

If hydrogen and oxygen form a polar bond, what is the dipole moment and how does it manifest in water?

The dipole moment in water is significant due to the bent shape of the molecule, causing it to have a partial negative charge near the oxygen and a partial positive charge near the hydrogens, leading to strong hydrogen bonding. (There’s no numeric answer; focus on molecular structure.)

What is the significance of hydrogen bonding in terms of water's properties?

Hydrogen bonding is responsible for water's high boiling and melting points, its high specific heat, and its solvent capabilities, allowing it to dissolve many ionic and polar substances.

Calculate the boiling point elevation when 0.25 mol of a non-volatile solute is added to 1.00 kg of water. (K_b for water is approximately 0.512 °C kg/mol)

The boiling point elevation is 0.128 °C (ΔT = iK_b m; here, i = 1 since it’s a non-volatile solute and m = 0.25 mol/kg). Hint: Always check for van 't Hoff factor in different solutes!

State Avogadro’s Law and provide an example of its application in gas stoichiometry.

Avogadro's Law states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. Example: 2.0 L of hydrogen gas will contain the same number of molecules as 2.0 L of oxygen gas at the same conditions.

If 5.00 L of gas A is at 1.00 atm, how many liters of gas B at the same pressure will contain 0.50 mol if gas B is at the same conditions?

5.00 L (Using Avogadro’s law, if 5.00 L contains about 0.50 mol of gas B, then at 1.00 atm, the volume of gas B would also be 5.00 L. Hint: Ensure you compare under the same conditions.)