| Term | Definition |
|---|
| amorphous solid | a solid in which the particles are not arranged with periodicity or order |
| boiling | the conversion of a liquid to a vapor at a specific temperature and pressure; occurs when the vapor pressure of the liquid equals the atmospheric pressure |
| boiling point | the temperature and pressure at which a liquid and a gas are in equilibrium |
| capillary action | the attraction of the surface of a liquid to the surface of a solid, which causes the liquid to rise or fall |
| condensation | the change of state from a gas to a liquid |
| critical point | the temperature and pressure at which the gas and liquid states of a substance become identical and form one phase |
| crystal | a solid whose atoms, ions, or molecules are arranged in a definite pattern |
| crystalline solid | a solid that consists of crystals |
| deposition | the change of state from a gas directly to a solid |
| diffusion | the movement of particles from regions of higher density to regions of lower density |
| effusion | the passage of a gas under pressure through a tiny opening |
| elastic collision | a collision between ideally elastic bodies in which the final and initial kinetic energies are the same |
| equilibrium | in chemistry, the state in which a chemical reaction and the reverse chemical reaction occur at the same rate such that the concentrations of reactants and products do not change |
| equilibrium vapor pressure | the vapor pressure of a system at equilibrium |
| evaporation | the change of a substance from a liquid to a gas |
| fluid | a nonsolid state of matter in which the atoms or molecules are free to move past each other, as in a gas or liquid |
| freezing | the change of state in which a liquid becomes a solid as heat is removed |
| freezing point | the temperature at which a solid and liquid are in equilibrium at 1 atm pressure; the temperature at which a liquid substance freezes |
| ideal gas | an imaginary gas whose particles are infinitely small and do not interact with each other |
| kinetic-molecular theory | a theory that explains that the behavior of physical systems depends on the combined actions of the molecules constituting the system |
| melting | he change of state in which a solid becomes a liquid by adding heat or changing pressure |
| melting pointthe temperature and pressure at which a solid becomes a liquidmolar enthalpy of fusion | the amount of energy as heat required to change 1 mol of a substance from solid to liquid at constant temperature and pressure |
| phase | in chemistry, one of the four states or conditions in which a substance can exist: solid, liquid, gas, or plasma; a part of matter that is uniform |
| phase diagram | a graph of the relationship between the physical state of a substance and the temperature and pressure of the substance |
| real gas | a gas that does not behave completely like a hypothetical ideal gas because of the interactions between the gas molecules |
| sublimation | the process in which a solid changes directly into a gas (the term is sometimes also used for the reverse process) |
| supercooled liquid | a liquid that is cooled below its normal freezing point without solidifying |
| surface tension | the force that acts on the surface of a liquid and that tends to minimize the area of the surface |
| triple point | the temperature and pressure conditions at which the solid, liquid, and gaseous phases of a substance coexist at equilibrium |
| unit cell | the smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice |
| vaporization | the process by which a liquid or solid changes to a gas |
| volatile liquid | a liquid that evaporates readily or at a low temperature |
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