Solids, Liquids, and Gases - AP Chemistry

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

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

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

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

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

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

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

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

1 atm. Standard reference pressure at sea level.

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

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

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

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

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

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

Sublimation. Direct phase transition bypassing the liquid phase entirely.

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

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

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

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

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

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

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

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

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

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

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

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

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