Chem chapter 10 and 11

Kinetic Molecular Theory (KMT)

A theory stating that particles of matter are in constant motion and their kinetic energy depends on temperature.

Solid

A state of matter with definite shape and volume; particles vibrate in fixed positions.

Liquid

A state of matter with definite volume but no definite shape; particles can flow past one another.

Gas

A state of matter with no definite shape or volume; particles move freely and are far apart.

Plasma

A high-energy state of matter consisting of ionized particles.

Intermolecular Forces

Attractive forces between molecules that influence physical properties.

Dipole-Dipole Forces

Attractions between polar molecules.

Hydrogen Bonding

A strong type of dipole-dipole attraction involving hydrogen bonded to N, O, or F.

London Dispersion Forces

Weak attractions caused by temporary dipoles in molecules.

Surface Tension

The resistance of a liquid to an increase in surface area.

Viscosity

A liquid's resistance to flow.

Vaporization

The process by which a liquid changes into a gas.

Evaporation

Vaporization occurring only at the surface of a liquid.

Boiling

Vaporization throughout a liquid when vapor pressure equals atmospheric pressure.

Condensation

The change of a gas into a liquid.

Freezing

The change of a liquid into a solid.

Melting

The change of a solid into a liquid.

Sublimation

The change of a solid directly into a gas.

Deposition

The change of a gas directly into a solid.

Vapor Pressure

The pressure exerted by a vapor above its liquid at equilibrium.

Phase Diagram

A graph showing the phases of a substance at different temperatures and pressures.

Triple Point

The condition where solid, liquid, and gas phases coexist.

Critical Point

The temperature and pressure beyond which a gas cannot be liquefied.

Atmospheric Pressure

Pressure caused by the weight of air above a surface.

Barometer

A device used to measure atmospheric pressure.

Manometer

An instrument used to measure gas pressure.

Pascal (Pa)

The SI unit of pressure.

Standard Temperature and Pressure (STP)

0°C (273 K) and 1 atm.

Kelvin Scale

An absolute temperature scale where 0 K is absolute zero.

Boyle's Law

Pressure and volume are inversely related at constant temperature.

Charles's Law

Volume and temperature are directly related at constant pressure.

Gay-Lussac's Law

Pressure and temperature are directly related at constant volume.

Combined Gas Law

A law combining Boyle's, Charles's, and Gay-Lussac's laws.

Ideal Gas Law

PV = nRT; relates pressure, volume, moles, and temperature.

Ideal Gas

A theoretical gas that perfectly follows gas laws.

Real Gas

A gas that deviates from ideal behavior due to intermolecular forces and particle volume.

Diffusion

The movement of gas particles from high to low concentration.

Effusion

The movement of gas particles through a tiny opening without pressure buildup.

Graham's Law

The rate of effusion or diffusion is inversely proportional to the square root of molar mass.

Elastic Collision

A collision in which kinetic energy is conserved.

Partial Pressure

The pressure exerted by one gas in a mixture.

Dalton's Law of Partial Pressures

Total pressure equals the sum of the partial pressures of all gases.

Molar Volume of a Gas

At STP, one mole of gas occupies 22.4 L.