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adhesive force

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Force of attraction between a liquid and another surface.

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allotropes

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Different forms of the same element in the same physical state.

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amorphous solid

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A noncrystalline solid with no well-defined, ordered structure.

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band

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A series of very closely spaced, nearly continuous molecular orbitals that belong to the material as a whole.

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band gap

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An energy separation between an insulator's highest filled electron energy band and the next higher-energy vacant band.

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band theory of metals

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A theory that accounts for the bonding and properties of metallic solids.

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boiling point

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The temperature at which the vapor pressure of a liquid is equal to the external pressure; also the condensation point.

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capillary action

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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.

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Clausius-Clapeyron equation

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An equation that relates the change in vapor pressure of a liquid to the change in its temperature and its molar heat of vaporization.

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cohesive forces

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All the forces of attraction among particles of a liquid.

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condensation

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The process by which a gas or vapor becomes a liquid; liquefaction.

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condensed phases

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The liquid and solid phases; phases in which particles interact strongly.

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conduction band

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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.

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coordination number

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In describing crystals, the number of nearest neighbors of an atom or ion.

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critical point

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The combination of critical temperature and critical pressure of a substance.

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critical pressure

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The pressure required to liquefy a gas (vapor) at its critical temperature.

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critical temperature

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The temperature above which a gas cannot be liquefied; the temperature above which a substance cannot exhibit distinct gas and liquid phases.

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crystal lattice

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The pattern of arrangement of particles in a crystal.

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crystalline solid

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A solid characterized by a regular, ordered arrangement of particles.

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deposition

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The direct solidification of a vapor by cooling; the reverse of sublimation.

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dipole-dipole interactions

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Interactions between polar molecules, that is, between molecules with permanent dipoles.

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dipole-induced dipole interaction

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See Dispersion forces.

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dispersion forces aka London forces

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Very weak and very short-range attractive forces between short-lived temporary (induced) dipoles; also called London forces.

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distillation

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The separation of a liquid mixture into its components on the basis of differences in boiling points.

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dynamic equilibrium

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A situation in which two (or more) processes occur at the same rate so that no net change occurs.

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enthalpy of fusion aka heat of fusion

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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.

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enthalpy of solidification aka heat of solidification

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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.

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evaporation aka vaporization

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The process by which molecules on the surface of a liquid break away and go into the gas phase.

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freezing point aka the melting point

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The temperature at which liquid and solid coexist in equilibrium; also the freezing point.

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heat of condensation

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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.

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heat of fusion aka enthalpy of fusion

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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.

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heat of solidification aka enthalpy of fusion

answer

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.

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heat of vaporization

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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.

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hydrogen bond

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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.

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insulator

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A poor conductor of electricity and heat.

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intermolecular forces

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Forces between individual particles (atoms, molecules, ions) of a substance.

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intramolecular forces

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Forces between atoms (or ions) within molecules (or formula units).

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isomorphous

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Refers to crystals having the same atomic arrangement.

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LeChatelier's Principle

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A system at equilibrium, or striving to attain equilibrium, responds in such a way as to counteract any stress placed upon it.

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London forces aka dispersion forces

answer

ery weak and very short-range attractive forces between short-lived temporary (induced) dipoles; also called London forces.

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melting point aka the freezing point

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The temperature at which liquid and solid coexist in equilibrium; also the freezing point.

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meniscus

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The upper surface of a liquid in a cylindrical container.

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metallic bonding

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Bonding within metals due to the electrical attraction of positively charged metal ions for mobile electrons that belong to the crystal as a whole.

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molar enthalpy of vaporization aka molar heat of vaporization

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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.

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molar heat capacity

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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.

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molar heat of condensation

answer

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.

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molar heat of fusion

answer

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.

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molar heat of vaporization aka molar enthalpy of vaporization

answer

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.

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normal boiling point

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The temperature at which the vapor pressure of a liquid is equal to one atmosphere pressure.

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normal melting point

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The melting (freezing) point at one atmosphere pressure.

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phase diagram

answer

A diagram that shows equilibrium temperature-pressure relationships for different phases of a substance.

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polymorphous

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Refers to substances that crystallize in more than one crystalline arrangement.

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semiconductor

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A substance that does not conduct electricity well at low temperatures but that does at higher temperatures.

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specific heat

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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.

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sublimation

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The direct vaporization of a solid by heating without passing through the liquid state.

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supercritical fluid

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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.

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surface tension

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The result of inward intermolecular forces of attraction among liquid particles that must be overcome to expand the surface area.

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triple point

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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.

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unit cell

answer

The smallest repeating unit showing all the structural characteristics of a crystal.

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vapor pressure

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The partial pressure of a vapor in equilibrium with its parent liquid or solid.

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vaporization aka evaporation

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The process by which molecules on the surface of a liquid break away and go into the gas phase.

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viscosity

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The tendency of a liquid to resist flow; the inverse of its fluidity.

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volatility

answer

The ease with which a liquid vaporizes.

Chesnut Chem 1212k Ch 13 Vocabulary – Flashcards

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