Comprehensive Chemistry: States, Mixtures, Thermodynamics, and Kinetic Theory

Kinetic Molecular Theory (KMT)

a model that describes the behaviors of gas as being point sized, having perfectly elastic collisions, and constant motion

Heat

Energy transferred due to a temperature difference.

State of Matter

Physical forms: solid, liquid, gas, plasma, and superatom.

Mixture

Combination of substances; can be homogeneous (uniform, like solution) or heterogeneous (not uniform, like suspension or colloid).

Resilient

Ability of particles to bounce without losing energy.

Thermodynamics

Study of energy transfer and transformation.

Suspension

A heterogeneous mixture with visible particles that settle.

Colloid

A mixture with small particles that do not settle.

Solution

Homogeneous mixture of solute + solvent.

Solute

Substance dissolved in a solvent.

Solvent

Substance that dissolves the solute.

Equilibrium

State where forward and reverse processes occur at the same rate.

Compound

Substance made of two or more elements chemically combined.

Element

Substance made of only one type of atom.

Kinetics

Study of the rate of chemical reactions.

Phase Diagram

Graph showing state of matter at various temperatures and pressures.

Phase Change

Transition from one state of matter to another.

Heat Capacity (C)

Energy required to raise 1 g of a substance by 1°C.

Heat of Fusion (ΔHfus)

Energy needed to melt a solid at its melting point.

Heat of Vaporization (ΔHvap)

Energy needed to vaporize a liquid at its boiling point.

Calorimetry

Technique to measure heat changes in reactions.

Solid, Liquid, Gas, Plasma, Superatom

Different states of matter.

Amorphous Solid

Solid without a definite shape or crystal structure.

Absolute Zero (0 K)

Theoretical temperature where particles have minimal kinetic energy.

Pressure (P)

Force per unit area.

Partial Pressure

Pressure contributed by a single gas in a mixture.

Kinetic Energy (KE)

Energy of motion; depends on mass and velocity.