Chem Chapter 10 vocab

Kinetic-molecular Theory

Idea that particles of matter are always in motion

Ideal Gas

Hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory

Elastic Collision

No net loss of total kinetic energy

Diffusion

Spontaneous mixing of particles of two substances caused by their random motion

Effusion

Process by which gas particles pass through a tiny opening into a vacuum

Real Gas

Does not behave completely according to the assumptions of the kinetic-molecular theory

Fluid

Substance that can flow & therefore take the shape of its container

Surface Tension (Property of all liquids)

Force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface are to the smallest possible size

Capillary Action

Attraction of the surface of a liquid to the surface of a solid, is a property closely related to surface tension

Vaporization

Liquid or solid changing to a gas

Evaporation

Process of particles escaping from the surface of a non-boiling liquid & enter the gas state

Freezing

Physical change of a liquid to a solid & Physical change of a liquid to a solid by removal of energy as heat

Crystalline Solid

Consisting of crystals

Crystal

Substance which the particles are arranged in an orderly, geometric, repeating pattern

Amorphous Solid

Particles that are arranged randomly

Melting

Physical CHange of a solid to a liquid by the addition of energy as heat

Melting Point

Temperature of when a solid becomes a liquid

Supercoded Liquids

Substances that retain certain liquid properties even at temps at which they appear to be solid

Crystal Structure

The total 3-dimensional arrangements of particles of a crystal

Unit Cell

Smallest portion of a crystal lattice that shows the 3-Dimensional pattern of the entire lattice

Phase

Any part of a system that has uniform composition & properties

Condensation

The process when gas changes to a liquid

Equilibrium

A dynamic condition in which two opposing changes occur at equal rates in a closed system

Equilibrium Vapor Liquids

The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature

Volatile Liquids

Liquids that evaporate readily, have relatively weak forces of attraction between their particles

Boiling

Conversion of the liquid to a vapor within the liquid as well as its surface

Boiling Point

Temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure

Molar Enthalpy of Vaporization

The amount of energy as heat that is needed to vaporize one mole of liquid at the liquid's boiling point at constant pressure

Freezing Point

Temperature at which solid & liquid are in equilibrium @ 1 ATM Pressure

Molar Enthalpy of Fusion

Amount of energy as heat required to melt one mole of solid at the solid's melting point

Sublimation

Change of state from a solid directly to a gas

Phase Diagram

Graph of pressure vs. temperature that shows the conditions under which the phases of a substance exist. It also reveals how the states of a system change with changing temperature or pressure.

Triple Point

Indicated the temperature & pressure conditions at which the solid, liquid, & vapor of the substance can coexist at equilibrium

Critical Point

Indicated the critical temperature & critical pressure

Critical Temperature

The temperature above which the substance cannot exist in the liquid state

Critical Pressure

The lowest pressure at which the substance can exist as a liquid at the critical temperature.

Deposition

The Change of state from a gas directly to a solid