AP Chemistry Flashcards: Solids Liquids And Gases

What this deck covers

This deck focuses on Solids Liquids And Gases, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: What is the main difference between crystalline and amorphous solids?

Answer: Crystalline solids have ordered structures; amorphous do not. Structural organization distinguishes these two solid types.

Flashcard 2: What is the Kinetic Molecular Theory?

Answer: Theory explaining the behavior of gases in terms of particle motion. Model treating gases as point particles in constant random motion.

Flashcard 3: State the unit of the gas constant $R$ in the ideal gas law.

Answer: L·atm/(mol·K). Units derived from $PV = nRT$ rearranged to solve for $R$.

Flashcard 4: What determines the boiling point of a liquid?

Answer: Intermolecular forces and atmospheric pressure. Stronger intermolecular forces require higher temperature to overcome.

Flashcard 5: What is the formula for the ideal gas law?

Answer: $PV = nRT$. Fundamental equation relating pressure, volume, moles, and temperature for ideal gases.

Flashcard 6: What is the definition of a volatile substance?

Answer: A substance that readily vaporizes at low temperature. High vapor pressure leads to easy evaporation.

Flashcard 7: What is the primary component of air?

Answer: Nitrogen. Comprises approximately 78% of Earth's atmospheric composition.

Flashcard 8: Find the density of a gas with molar mass 44 g/mol at 2 atm and 273 K.

Answer: 3.92 g/L. Using $d = \frac{PM}{RT}$ with given values yields this density.

Flashcard 9: What is Henry's law?

Answer: The solubility of a gas is proportional to its partial pressure. Gas solubility increases linearly with increasing partial pressure.

Flashcard 10: What is the unit of pressure in the SI system?

Answer: Pascal (Pa). Base SI unit equivalent to $N/m^2$ or $kg/(m \cdot s^2)$.

Flashcard 11: What is the Kinetic Molecular Theory?

Answer: Theory explaining the behavior of gases in terms of particle motion. Model treating gases as point particles in constant random motion.

Flashcard 12: What is an ideal gas?

Answer: A hypothetical gas that perfectly fits the ideal gas law. Theoretical model with no intermolecular forces or molecular volume.

Flashcard 13: Define 'freezing point depression'.

Answer: Decrease in freezing point due to solute addition. Colligative property that lowers the temperature at which freezing occurs.

Flashcard 14: What is Avogadro's law?

Answer: $\frac{V_1}{n_1} = \frac{V_2}{n_2}$ (constant $P$ and $T$). States that volume is directly proportional to amount of gas.

Flashcard 15: Define the term 'molarity'.

Answer: Molarity is moles of solute per liter of solution. Standard concentration unit expressed as $mol/L$ or $M$.

Flashcard 16: What is Boyle's law?

Answer: $P_1V_1 = P_2V_2$ (constant $T$ and $n$). Describes inverse relationship between pressure and volume at constant temperature.

Flashcard 17: Define 'surface tension'.

Answer: Surface tension is the energy required to increase surface area of a liquid. Results from unequal intermolecular forces at liquid-gas interface.

Flashcard 18: What is the Kinetic Molecular Theory?

Answer: Theory explaining the behavior of gases in terms of particle motion. Model treating gases as point particles in constant random motion.

Flashcard 19: What is the formula for calculating partial pressure?

Answer: $P_i = X_i \times P_{\text{total}}$. Partial pressure equals mole fraction times total pressure.

Flashcard 20: What is the normal boiling point of a liquid?

Answer: The boiling point at 1 atm pressure. Standard reference temperature for comparing boiling points.

Flashcard 21: What is Charles's law?

Answer: $\frac{V_1}{T_1} = \frac{V_2}{T_2}$ (constant $P$ and $n$). Shows direct proportionality between volume and absolute temperature.

Flashcard 22: What is the critical point of a substance?

Answer: The temperature and pressure above which a gas cannot be liquefied. Beyond this point, distinct liquid and gas phases cannot exist.

Flashcard 23: What is the cohesive force in liquids?

Answer: The force of attraction between molecules in a liquid. Intermolecular attractions that hold liquid molecules together.

Flashcard 24: What is the relationship between temperature and vapor pressure?

Answer: Vapor pressure increases with temperature. Higher temperature provides more kinetic energy for molecules to escape liquid phase.

Flashcard 25: Define 'sublimation'.

Answer: The transition of a substance directly from solid to gas. Phase change that occurs when vapor pressure exceeds atmospheric pressure.

Flashcard 26: What is the boiling point of water at 1 atm in Celsius?

Answer: 100°C. Standard boiling point of pure water at standard atmospheric pressure.

Flashcard 27: What is the standard atmospheric pressure in atm?

Answer: 1 atm. Standard reference pressure at sea level.

Flashcard 28: Define 'enthalpy of fusion'.

Answer: The change in enthalpy when 1 mole of solid melts to liquid. Energy needed to break intermolecular forces during melting process.

Flashcard 29: What is the term for the transition from solid to gas?

Answer: Sublimation. Direct phase transition bypassing the liquid phase entirely.

Flashcard 30: Calculate the number of moles in 22.4 L of gas at STP.

Answer: 1 mole. At STP, 22.4 L equals one molar volume of any ideal gas.

Flashcard 31: Define the term 'vapor pressure'.

Answer: The pressure exerted by a vapor in equilibrium with its liquid. Represents dynamic equilibrium between evaporation and condensation.

Flashcard 32: What is Raoult's law?

Answer: Vapor pressure of solution is proportional to mole fraction of solvent. Describes how solutes reduce vapor pressure of solutions.

Flashcard 33: What is Dalton's law of partial pressures?

Answer: Total pressure is the sum of partial pressures of gases. Each gas contributes independently to total system pressure.

Flashcard 34: What is the main difference between crystalline and amorphous solids?

Answer: Crystalline solids have ordered structures; amorphous do not. Structural organization distinguishes these two solid types.

Flashcard 35: What is the critical temperature of a substance?

Answer: The temperature above which a gas cannot be liquefied. Above this temperature, no amount of pressure can create liquid phase.

Flashcard 36: Identify the phase change from liquid to gas.

Answer: Vaporization. Phase transition requiring energy input to overcome intermolecular forces.

Flashcard 37: What is the enthalpy of vaporization?

Answer: The heat required to vaporize 1 mole of liquid. Energy required to convert liquid molecules to gas phase.

Flashcard 38: What is Gay-Lussac's law?

Answer: $\frac{P_1}{T_1} = \frac{P_2}{T_2}$ (constant $V$ and $n$). Describes direct relationship between pressure and absolute temperature.

Flashcard 39: What is the boiling point elevation?

Answer: Increase in boiling point due to solute addition. Colligative property dependent on solute particle concentration.

Flashcard 40: Define the term 'viscosity'.

Answer: Viscosity is a measure of a fluid's resistance to flow. Property that determines how easily a fluid flows or moves.

Flashcard 41: What is the triple point of a substance?

Answer: The condition where all three phases coexist in equilibrium. Unique temperature and pressure where solid, liquid, and gas phases coexist.

Flashcard 42: What is the main difference between crystalline and amorphous solids?

Answer: Crystalline solids have ordered structures; amorphous do not. Structural organization distinguishes these two solid types.