Unit 2: Gases, Liquids, & Solutions

Flashcards covering key concepts of gases, liquids, and solutions, including theories, laws, and properties.

Kinetic Molecular Theory

A model that assumes gas particles are perfect point masses with no volume or intermolecular forces.

Partial Pressure

The pressure exerted by a single component of a mixture of gases.

Dalton’s Law

The principle stating that the total pressure of a gas mixture is the sum of the partial pressures of each individual gas.

Intermolecular Forces (IMFs)

Forces between molecules that affect physical properties such as boiling point and viscosity.

London Dispersion Forces (LDF)

Weakest intermolecular force present in all molecules; increases with molar mass.

Dipole-Dipole Forces

Attractive forces between the positive end of one polar molecule and the negative end of another.

Hydrogen Bonding

A strong type of dipole-dipole interaction occurring when hydrogen is bonded to nitrogen, oxygen, or fluorine.

Ion-Dipole Forces

Attractive forces between an ion and a polar molecule, strongest of the intermolecular forces.

Vapor Pressure

The pressure exerted by a vapor in equilibrium with its liquid or solid phase at a given temperature.

Boiling Point

The temperature at which a liquid's vapor pressure equals the external pressure.

Phase Diagrams

Graphs that show the state of a substance at varying temperatures and pressures.

Critical Point

The end of a phase equilibrium line; above this point, distinct liquid and gas phases do not exist.

Henry's Law

The principle stating that the amount of gas dissolved in a liquid is proportional to its pressure above the liquid.

Colligative Properties

Properties that depend on the number of solute particles in a solution, not their identity.

Vapor Pressure Lowering (Raoult's Law)

The principle that the addition of a solute decreases the vapor pressure of the solvent.

Boiling Point Elevation

The increase in boiling point that occurs when a solute is added to a solvent.

Freezing Point Depression

The decrease in freezing point that occurs when a solute is added to a solvent.

Van 't Hoff Factor ($i$)

A factor that indicates the number of particles a solute breaks into in solution, significant for colligative properties.