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22 Cards in this Set

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Liquid
one of three states of matter, it is characterized by, limited expansion, lack of shape, maintenance of volume, slight compressibility, high density, and mixing in other liquids.
Condensation
conversion of vapor (gas) molecules to a liquid.
Evaporation
Escape of molecules from the surface of a liquid to form a vapor in the surrounding space above the liquid.
Dynamic equilibrium
a situation in which the rate of a forward process is equal to the rate of the reverse process occurring simultaneously as when the rate of evaporation is equal to the rate of condensation for a liquid in a closed container.
Vapor pressure
in a closed container, the pressure exerted by a vapor in dynamic equilibrium with its liquid state.
Boiling point
temperature at which the vapor pressure of a liquid is equal to the external pressure above the surface of the liquid.
Endothermic change of state
any change in the state of matter in which heat energy is absorbed.
Exothermic change of state
any change in the state of matter in which heat is released.
Heat of vaporization
quantity of heat required to evaporate 1 g of a given liquid at its boiling point and at constant pressure.
Heat of condensation
quantity of heat released in order to condense 1 g of a gas to a liquid at its boiling point and at constant pressure.
Distillation
purifying of a liquid by heating it to the boiling point and cooling the vapors in a condenser.
Surface tension
property of a liquid that tends to draw the surface molecules into the body of the liquid and hence to reduce the surface to a minimum.
Viscosity
property of a liquid that describes the resistance of a liquid to flow.
Solid
one of three states of matter; it is characterized by lack of expansion, definite shape, constant volume, lack of compressibility, high density, and severely limited mixing.
Crystalline solid
any solid that consists of particles arranged in a definite geometric shape or form that is distinctive for that solid.
Amorphous solid
any solid that consists of particles arranged in an irregular manner and thus lacks the regular structure of a crystalline solid.
Freezing point
temperature at which the particles of a liquid begin to form crystals or irregular particles of a solid.
Melting point
temperature at which the kinetic energy of some of the particles in a solid matches the attractive forces in the solid and the solid begins to liquefy.
Heat of fusion
quantity of heat required to convert 1 g of a solid to liquid at the melting point of the substance.
Heat of solidification (crystallization)
quantity of heat released by 1 g of a liquid as it becomes a solid at the melting point of the substance.
Sublimation
direct conversion of a solid to a vapor without passing through the liquid state; it is an endothermic change of state.
Deposition
direct conversion of a vapor to a solid without passing through the liquid state; it is an exothermic change of state.