 | Term | Definition |
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FLUID |
A substance that can flow and therefore can take the shape of its container. |
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SURFACE TENSION |
A force that tends to pull adjacent parts of a liquid's surface together, decreasing its surface area to the smallest size. |
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CAPILLARY ACTION |
The attraction of the surface of the liquid to the surface of a solid. |
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VAPORIZATION |
The process by which a liquid or solid changes to a gas. |
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EVAPORATION |
The process by which particles escape from the surface of a nonboiling liquid and enter the gas state. |
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FREEZING (SOLIDIFICATION) |
The physical change of a liquid to a solid by removal of heat. |
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CRYSTALLINE SOLID |
A solid made up of crystals. |
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CRYSTAL |
A substance in which the particles are arranged in an orderly, geometric, repeating pattern. |
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AMORPHOUS SOLID |
A soild in which the particles are arranged randomly. |
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MELTING |
The physical change of a solid to a liquid by the addition of heat. |
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MELTING POINT |
The temperature in which a solid becomes a liquid. |
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SUPERCOOLED LIQUIDS |
A substance that remains certain liquid properties even at temperatures at which they appear to be solid |
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CRYSTAL STRUCTURE |
The total three-dimensional arrangement of particles of crystals. |
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CRYSTAL LATTICE |
The arrangement of particles in the crystal that can be represented by a coordinate system. |
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UNIT CELL |
The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice. |
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EQUILIBRIUM |
Dynamic condition at which two opposing charges occur at equal rates in a closed system. |
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CLOSED SYSTEM |
Matter cannot enter or leave, but energy can. |
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OPEN SYSTEM |
Both matter and energy can escape or enter. |
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PHASE |
Any part of a system that has uniform composition and properties. |
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CONDENSATION |
The process by which a gas changes to a liquid. |
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LE CHÁTELIER'S PRINCIPLE |
When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress. |
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STRESS |
Typically a change in concentration, pressure, or temperature. |
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EQUILIBRIUM VAPOR PRESSURE |
The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature. |
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VOLATILE LIQUIDS |
Liquids that evaporate readily, have relatively weak attractive forces between particles. |
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NONVOLATILE LIQUIDS |
Liquids that evaporate slowly, have relatively strong attractive forces between particles. |
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BOILING |
The conversion of a liquid to a vapor within the liquid as its surface. |
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BOILING POINT |
The temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure. |
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MOLAR HEAT OF VAPORIZATION |
The amount of heat energy needed to vaporize one mole of liquid at its boiling point. |
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FREEZING POINT |
The temperature at which the solid and liquid are in equilibrium at 1 atm, 760 torr, 101.3 kPa pressure. |
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MOLAR HEAT OF FUSION |
The amount of heat energy required to melt one of solid at its melting point. |
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SUBLIMATION |
The change of state from a solid directly to a gas. |
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DEPOSITION |
The change of statee from a gas directly to a solid. |
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PHASE DIAGRAM |
A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist. |
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TRIPLE POINT |
Indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium. |
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CRITICAL POINT |
Indicates the critical temperature and critical pressure of a substance. |
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CRITICAL TEMPERATURE |
The temperature above which the substance cannot exist in the liquid state. |
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CRITICAL PRESSURE |
The lowest pressure at which the substance can exist as a liquid at the critical temperature. |
