Chapter 10 Chemistry

kinetic-molecular theory

based on the idea that particles of matter are always in motion

ionic

to have to do with ions/charged molecules

ideal gas

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

elastic collision

one in which there is no net loss of total kinetic energy

kinetic energy

energy of motion

real gas

At a gas that does not behave completely according to the assumptions of the kinetic-molecular the

diffusion

such spontaneous mixing of the particles of two substances cause by their random motion

effusion

a gas that does not behave completely according to the assumptions of the kinetic-molecular theory.

fluid

a substance that can flow and therefore take the shape of its container

surface tension

a force that tends to pull adjacent parts of liquids surface together, thereby decreasing surface are to the smallest possible size

capillary action

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

freezing

the physical change of a liquid to a solid by removal of energy as heat

evaporation

the process by which particles escape from the surface of a nonboiling liquid and enter the gas state.

vaporization

the process by which a liquid or solid changes to a gas

crystalline solids

they consist of crystals

crystal

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

amorphous solids

ones in which the particles are arranged randomly

supercooled liquids

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

melting point

the temperature at which a solid becomes a liquid

melting

the physical change of a solid to a liquid by the addition of energy as heat.

unit cell

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

crystal structure

the total three-dimensional arrangement of particles of a crystal

phase

any part of a system that has uniform composition and properties

condensation

the process by which a gas changes to a liquid

equilibrium

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

equilibrium vapor pressure

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

volatile liquids

liquids that evaporate readily

equilibrium vapor pressure

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

boiling point

the temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure.

boiling

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

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

normal freezing point

the temperature at which the solid and liquid are in equilibrium at 1 atm

molar enthalpy of fusion

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

phase diagram

a graph of pressure versus temperature that shows the condition under which the phases of substance exist

sublimation

the change of state from a solid directly to a gas

deposition

the change of state from a gas directly to solid

triple point

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

critical point

the critical temperature and 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