Question | Answer |
spontaneous mixing of the particles of two substances due to their random motion | diffusion |
process by which gas particles pass through a tiny opening | effusion |
collision between gas particles and container walls in which there is no net loss of kinetic energy | elastic collision |
substance that can flow and therefore take the shape of its container; a liquid or gas | fluid |
imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory | ideal gas |
based on the idea that the particles of matter are in constant motion | kinetic-molecular theory |
gas that does not behave completely according to the assumptions of the kinetic-molecular theory | real gas |
the attraction of the surface of a liquid to the surface of a solid | capillary action |
process by which particles escape from the surface of a nonboiling liquid and enter the gas state | evaporation |
physical change of a liquid to a solid by removal of heat | freezing |
force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface area to the smallest possible size | surface tension |
process by which a liquid or solid changes to a gas | vaporization |
solid in which the particles are arranged randomly | amorphous |
substance in which the particles are arranged in an orderly, geometric, repeating pattern | crystal |
total three-dimensional arrangement of particles of a crystal | crystal structure |
solid made up of crystals | crystalline |
physical change of a solid to a liquid by the addition of heat | melting |
temperature at which a solid becomes a liquid | melting point |
substances that retain certain liquid properties even at temperatures at which they appear to be solid | supercooled liquids |
smallest portion of a crystal lattice that slows the three-dimensional pattern of the entire lattice | unit cell |
the conversion of a liquid to a vapor within the liquid as well as at its surface | boiling |
the temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure | boiling point |
the process by which a gas changes to a liquid | condensation |
indicates the critical pressure and critical temperature | critical point |
the lowest pressure at which the substance can exist as a liquid at the critical temperature | critical pressure |
temperature above which the substance cannot exist in the liquid state | critical temperature |
change of state of a gas directly to a solid | deposition |
dynamic condition in which two opposing changes occur at equal rates in a closed system | equilibrium |
the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature | equilibrium vapor pressure |
temperature at which a solid and liquid are in equilibrium at 1 atm of pressure | freezing point |
when a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress | LeChatlier's principle |
amount of heat energy required to melt one mole of solid at its melting point | molar enthalpy of fusion |
amount of heat energy needed to vaporize one mole of liquid at its boiling point | molar enthalpy of vaporization |
any part of a system that has uniform composition and properties | phase |
graph of pressure versus temperature that shows the conditions under which the phases of a substance exist | phase diagram |
change of state from a solid directly to a gas | sublimation |
indicates the temperature and pressure conditions at which the solid, liquid, and vapor of a substance can coexist at equilibrium | triple point |
liquids that evaporate readily | volatile |