Term
|
Definition
| Force of attraction between a liquid and another surface. |
|
|
Term
|
Definition
| Different forms of the same element in the same physical state. |
|
|
Term
|
Definition
| A noncrystalline solid with no well-defined, ordered structure. |
|
|
Term
|
Definition
| A series of very closely spaced, nearly continuous molecular orbitals that belong to the material as a whole. |
|
|
Term
|
Definition
| An energy separation between an insulator's highest filled electron energy band and the next higher-energy vacant band. |
|
|
Term
|
Definition
| A theory that accounts for the bonding and properties of metallic solids. |
|
|
Term
|
Definition
| The temperature at which the vapor pressure of a liquid is equal to the external pressure; also the condensation point. |
|
|
Term
|
Definition
| The drawing of a liquid up the inside of a small-bore tube when adhesive forces exceed cohesive forces, or the depression of the surface of the liquid when cohesive forces exceed adhesive forces. |
|
|
Term
| Clausius-Clapeyron equation |
|
Definition
| An equation that relates the change in vapor pressure of a liquid to the change in its temperature and its molar heat of vaporization. |
|
|
Term
|
Definition
| All the forces of attraction among particles of a liquid. |
|
|
Term
|
Definition
| The process by which a gas or vapor becomes a liquid; liquefaction. |
|
|
Term
|
Definition
| The liquid and solid phases; phases in which particles interact strongly. |
|
|
Term
|
Definition
| A partially filled band or a band of vacant energy levels just higher in energy than a filled band; a band within which, or into which, electrons must be promoted to allow electrical conduction to occur in a solid. |
|
|
Term
|
Definition
| In describing crystals, the number of nearest neighbors of an atom or ion. |
|
|
Term
|
Definition
| The combination of critical temperature and critical pressure of a substance. |
|
|
Term
|
Definition
| The pressure required to liquefy a gas (vapor) at its critical temperature. |
|
|
Term
|
Definition
| The temperature above which a gas cannot be liquefied; the temperature above which a substance cannot exhibit distinct gas and liquid phases. |
|
|
Term
|
Definition
| The pattern of arrangement of particles in a crystal. |
|
|
Term
|
Definition
| A solid characterized by a regular, ordered arrangement of particles. |
|
|
Term
|
Definition
| The direct solidification of a vapor by cooling; the reverse of sublimation. |
|
|
Term
| dipole-dipole interactions |
|
Definition
| Interactions between polar molecules, that is, between molecules with permanent dipoles. |
|
|
Term
| dipole-induced dipole interaction |
|
Definition
|
|
Term
| dispersion forces aka London forces |
|
Definition
| Very weak and very short-range attractive forces between short-lived temporary (induced) dipoles; also called London forces. |
|
|
Term
|
Definition
| The separation of a liquid mixture into its components on the basis of differences in boiling points. |
|
|
Term
|
Definition
| A situation in which two (or more) processes occur at the same rate so that no net change occurs. |
|
|
Term
| enthalpy of fusion aka heat of fusion |
|
Definition
| The amount of heat required to melt a specific amount of a solid at its melting point with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the molar heat of fusion. |
|
|
Term
| enthalpy of solidification aka heat of solidification |
|
Definition
| The amount of heat that must be removed from a specific amount of a liquid at its freezing point to freeze it with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the molar heat of solidification. |
|
|
Term
| evaporation aka vaporization |
|
Definition
| The process by which molecules on the surface of a liquid break away and go into the gas phase. |
|
|
Term
| freezing point aka the melting point |
|
Definition
| The temperature at which liquid and solid coexist in equilibrium; also the freezing point. |
|
|
Term
|
Definition
| The amount of heat that must be removed from a specific amount of a vapor at its condensation point to condense the vapor with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the molar heat of condensation. |
|
|
Term
| heat of fusion aka enthalpy of fusion |
|
Definition
| The amount of heat required to melt a specific amount of a solid at its melting point with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the molar heat of fusion. |
|
|
Term
| heat of solidification aka enthalpy of fusion |
|
Definition
| The amount of heat that must be removed from a specific amount of a liquid at its freezing point to freeze it with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the molar heat of solidification. |
|
|
Term
|
Definition
| The amount of heat required to vaporize a specific amount of a liquid at its boiling point with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the molar heat of vaporization. |
|
|
Term
|
Definition
| A fairly strong dipole-dipole interaction (but still considerably weaker than covalent or ionic bonds) between molecules containing hydrogen directly bonded to a small, highly electronegative atom, such as N, O, or F. |
|
|
Term
|
Definition
| A poor conductor of electricity and heat. |
|
|
Term
|
Definition
| Forces between individual particles (atoms, molecules, ions) of a substance. |
|
|
Term
|
Definition
| Forces between atoms (or ions) within molecules (or formula units). |
|
|
Term
|
Definition
| Refers to crystals having the same atomic arrangement. |
|
|
Term
|
Definition
| A system at equilibrium, or striving to attain equilibrium, responds in such a way as to counteract any stress placed upon it. |
|
|
Term
| London forces aka dispersion forces |
|
Definition
| ery weak and very short-range attractive forces between short-lived temporary (induced) dipoles; also called London forces. |
|
|
Term
| melting point aka the freezing point |
|
Definition
| The temperature at which liquid and solid coexist in equilibrium; also the freezing point. |
|
|
Term
|
Definition
| The upper surface of a liquid in a cylindrical container. |
|
|
Term
|
Definition
| Bonding within metals due to the electrical attraction of positively charged metal ions for mobile electrons that belong to the crystal as a whole. |
|
|
Term
| molar enthalpy of vaporization aka molar heat of vaporization |
|
Definition
| The amount of heat required to vaporize one mole of a liquid at its boiling point with no change in temperature; usually expressed in kJ/mol. See Heat of vaporization. |
|
|
Term
|
Definition
| The amount of heat necessary to raise the temperature of one mole of a substance one degree Celsius with no change in state; usually expressed in kJ/mol · °C. See Specific heat. |
|
|
Term
| molar heat of condensation |
|
Definition
| The amount of heat that must be removed from one mole of a vapor at its condensation point to condense the vapor with no change in temperature; usually expressed in kJ/mol. See Heat of condensation. |
|
|
Term
|
Definition
| The amount of heat required to melt one mole of a solid at its melting point with no change in temperature; usually expressed in kJ/mol. See Heat of fusion. |
|
|
Term
| molar heat of vaporization aka molar enthalpy of vaporization |
|
Definition
| The amount of heat required to vaporize one mole of a liquid at its boiling point with no change in temperature; usually expressed in kJ/mol. See Heat of vaporization. |
|
|
Term
|
Definition
| The temperature at which the vapor pressure of a liquid is equal to one atmosphere pressure. |
|
|
Term
|
Definition
| The melting (freezing) point at one atmosphere pressure. |
|
|
Term
|
Definition
| A diagram that shows equilibrium temperature-pressure relationships for different phases of a substance. |
|
|
Term
|
Definition
| Refers to substances that crystallize in more than one crystalline arrangement. |
|
|
Term
|
Definition
| A substance that does not conduct electricity well at low temperatures but that does at higher temperatures. |
|
|
Term
|
Definition
| The amount of heat necessary to raise the temperature of a specific amount of a substance one degree Celsius with no change in state; usually expressed in J/g · °C. See Molar heat capacity. |
|
|
Term
|
Definition
| The direct vaporization of a solid by heating without passing through the liquid state. |
|
|
Term
|
Definition
| A substance at a temperature above its critical temperature. A supercritical fluid cannot be described as either a liquid or gas, but has the properties of both. |
|
|
Term
|
Definition
| The result of inward intermolecular forces of attraction among liquid particles that must be overcome to expand the surface area. |
|
|
Term
|
Definition
| The point on a phase diagram that corresponds to the only pressure and temperature at which three phases (usually solid, liquid, and gas) of a substance can coexist at equilibrium. |
|
|
Term
|
Definition
| The smallest repeating unit showing all the structural characteristics of a crystal. |
|
|
Term
|
Definition
| The partial pressure of a vapor in equilibrium with its parent liquid or solid. |
|
|
Term
| vaporization aka evaporation |
|
Definition
| The process by which molecules on the surface of a liquid break away and go into the gas phase. |
|
|
Term
|
Definition
| The tendency of a liquid to resist flow; the inverse of its fluidity. |
|
|
Term
|
Definition
| The ease with which a liquid vaporizes. |
|
|
