States Of Matter

Front 1

Kinetic-molecular theory

Back 1

the idea that particles of matter are always in motion

Front 2

Ideal gas

Back 2

a hypothetical gas that fits all the assumptions of the kinetic-molecular theory

Front 3

Elastic collision

Back 3

a collision where there is no net loss of total kinetic energy

Front 4

Diffusion

Back 4

spontaneous mixing of the particles of two substances caused by their random motion

Front 5

Effusion

Back 5

a process by which gas particles pass through a tiny opening

Front 6

Real gas

Back 6

a gas that does not behave completely according to the Kinsthetic-molecular theory

Front 7

Fluid

Back 7

a substance that flows and takes the shape of its container

Front 8

Surface tension

Back 8

a force that pulls adjacent particles of a liquids surface together, decreasing surface area to the smallest possible size

Front 9

Capillary action

Back 9

the attraction of the surface of a liquid to the surface of a solid

Front 10

Vaporization

Back 10

liquid or solid to a gas

Front 11

Evaporation

Back 11

process of nonboiling liquid changing to a gas

Front 12

Freezing

Back 12

liquid to solid by removal of energy as heat

Front 13

Crystalline solid

Back 13

a solid made up of crystals (geometric repeating pattern)

Front 14

Crystal

Back 14

substance with orderly, geometric patterned particles

Front 15

Amorphous solid

Back 15

solid with randomly arranged particles

Front 16

Melting

Back 16

solid to liquid by adding energy as heat

Front 17

Melting point

Back 17

temp. that a solid becomes a liquid (kinetic nrgs of solid particles overcome the forces holding the together)

Front 18

Supercooled liquids

Back 18

substances that retain certain liquid properties even at temperatures where they appear to be solid

Front 19

Crystal structure

Back 19

3-D arrangement of crystal particles

Front 20

Unit cell

Back 20

smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice

Front 21

Phase

Back 21

any part of a system that has uniform composition and properties

Front 22

Condensation

Back 22

gas to liquid

Front 23

Equilibrium

Back 23

2 opposing changes occur at equal rates in a closed system

Front 24

Equilibrium vapor pressure

Back 24

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

Front 25

Volatile liquids

Back 25

liquids that evaporate readily and have relatively weak forces of attraction between their particles

Front 26

Boiling

Back 26

conversion of liquid to a vapor within the liquid as well as at its surface

Front 27

Boiling point

Back 27

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

Front 28

Molar enthalpy of vaporization

Back 28

amt. of energy neende to baporize one mol of liquid at the liquids boiling point at constant pressure

Front 29

Freezing point

Back 29

temp at which the particles of liquid and solid have the same avg kinsthetic nrg

Front 30

Molar enthalpy of fusion

Back 30

amt. of nrg as heat needed to melt one mol of a solid at the solids meltiong pt.

Front 31

Sublimination

Back 31

solid directly to a gas

Front 32

Deposition

Back 32

gas directly to a solid

Front 33

Phase diagram

Back 33

graph of pressure v. temp. that shows conditions under which the phases of a substance exist. (shows how phases change w/temp or pressure)

Front 34

Triple point

Back 34

indicates temp. and pressure conditions where the solid, liquid, and gas states can coexist at equilibrium

Front 35

Critical Point

Back 35

indicates the critical temp. and critical pressure

Front 36

Critical temperature

Back 36

temp. above which the substance cannot exist in the liquid state

Front 37

Critical pressure

Back 37

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