| A | B |
|---|
| Absolute Zero | the lowest possible temperature; the temperature at which all particle movement stops; -273?C or 0 K. |
| Avogadro’s Law | gases at the same temperature |
| (Normal) Boiling Point | the temperature at which a phase change between liquid and gas occurs at 1 atm or 101.3 kPa; the temperature at which the vapor pressure of a liquid is equal to the atmospheric pressure. |
| Compound | pure substance composed of two or more different elements chemically combined. |
| Cooling Curve | diagram showing phase changes for a substance as it loses energy and |
| Deposition | phase change from gas to solid. |
| Energy | the capacity to do work. |
| Element | pure substance composed of one species of atoms. |
| Evaporation | phase change from liquid to gas. |
| Extensive (property) | a physical property that depends on sample size or amount |
| (Ex: mass | length). |
| Heat | form of energy measured in Joules (J). |
| Heat of Fusion | energy required to change 1 g of a substance from solid to liquid. |
| Heat of Vaporization | energy required to change 1 g of a substance from liquid to gas. |
| Heating Curve | diagram showing phase changes for a substance as it gains energy and goes from solid phase all the way to gas phase. |
| Heat Transfer | energy transferred from a substance with more (hotter) to a |
| Intensive (property) | a physical property that does NOT depend on sample size or amount (Ex: melting point |
| Kinetic Energy | energy of motion; energy associated with a change in temperature. |
| Lattice | the unique crystal structure associated with any given solid. |
| Matter | anything that has mass and takes up space. |
| Melting Point | the temperature at which a phase change between solid and liquid occurs. |
| Mixture | two or more pure substances physically combined. |
| Potential (AKA Physical) Energy | energy of position; energy associated with a phase change. |
| Sublimation | phase change from solid to gas. |
| Temperature | a measure of average kinetic energy. |
