States of Matter
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Created by:
MissWilliamsladybug on March 26, 2012
Subjects:
Description:
Chemistry vocab
Classes:
Chem, ASTEC Chemistry Students
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57 terms
Terms | Definitions |
|---|---|
 diffusion | Spontaneous mixing of the particles of two substances caused by their random motion |
| effusion | Process by which gas particles under pressure pass through a tiny opening |
| elastic collision | Collision between gas particles and between particles and container walls. These collisions have no net loss of kinetic energy |
| fluid | Gas particles glide easily past one another. Both liquids and gases flow so they are both considered this. These take the shape of their container. |
| ideal gas | An imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory. |
| kinetic-molecular theory | Particles of matter are always in motion. |
| real gas | A gas that does not behave completely according to the assumptions of the kinetic-molecular theory |
| atmosphere of pressure | Exactly 760 mm Hg. |
| barometer | Device used to measure atmospheric pressure. |
| millimeter of mercury | A common unit of pressure, symbolized by mm Hg. |
| newton | It is the force that will increase the speed of one kilogram mass by one meter per second each second it is applied. It is the SI unit of force. |
| pascal | The pressure exerted by a force of one newton (1N) acting on an area of one square meter. |
| standard temperature and pressure | For purposes of comparison, scientists have agreed on standard conditions of exactly 1 atm pressure and 0°C. These conditions are commonly abbreviated STP. |
| absolute zero | -273.15°C or 0 K. The theoretical lowest temperature possible to achieve. |
| Boyle's law | The volume of a fixed mass of gas varies inversely with the pressure at constant temperature. (simply - when volume goes up the pressure goes down, and when volume goes down the pressure goes up when temperature is kept constant) |
| Charles's Law | The volume of a fixed mass at constant pressure varies directly with the Kelvin temperature (simply - when the temperature goes up the volume goes up, when the temperature goes down, the volume goes down if pressure is constant) |
| combined gas law | Expresses the relationship between pressure, volume, and temperature of a fixed amount of gas. |
| Dalton's Law of partial pressures | The total pressure of a mixture of gasses is equal to the sum of the partial pressures. |
| gas laws | Simple mathematical relationships between the volume, temperature, pressure, and quantity of a gas. |
| Gay-Lussac's Law | The pressure of a fixed mass of gas at constant volume varies directly with the Kelvin Temperature. (simply - pressure goes up with the temperature, and down with temperature if volume is kept constant) |
| partial pressure | The pressure of each gas in a mixture. |
| Avogadro's law | Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. |
| Gay-Lussac's law of combining volumes of gases | At constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers |
| standard molar volume of a gas | The volume occupied by one mole of a gas at STP. This has been found to be 22.41410 L. |
| ideal gas constant | The constant R. |
| ideal gas law | The mathematical relationship of pressure, volume, temperature, and the number of moles of a gas. |
| capillary action | The attraction of the surface of a liquid to the surface of a solid. |
| evaporation | The process by which particles escape from the surface of a nonboiling liquid and enter the gas state. |
| surface tension | A force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface area to the smallest possible size. |
| amorphous solid | The particles are arranged randomly. |
| crystal structure | The total three-dimensional arrangement of particles of a crystal. |
| melting | The physical change of a solid to a liquid by the addition of heat. |
| supercooled liquid | Substances that retain certain liquid properties even at temperatures at which they appear to be solid. |
| freezing | The physical change of a liquid to a solid by removal of heat. |
| vaporization | The process by which a liquid or solid changes to a gas. |
| crystal | A substance in which the particles are arranged in an orderly, geometric, repeating pattern. |
| crystalline solid | Most solids are this. They consist of crystals. |
| melting point | The temperature at which a solid becomes a liquid. |
| unit cell | The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice. |
| boiling | The conversion of a liquid to a vapor within the liquid as well as at its surface. It occurs when the equilibrium vapor pressure of the liquid equals the atmospheric pressure. |
| boiling point | The temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure. |
| condensation | The process by which a gas changes to a liquid. |
| critical point | Indicates the critical temperature and critical pressure. |
| critical pressure | The lowest pressure at which the substance can exist as a liquid at the critical temperature. |
| critical temperature | The temperature above which the substance cannot exist in the liquid state. |
| deposition | The change of state from a gas directly to a solid. |
| equilibrium | A dynamic condition in which two opposing changes occur at equal rates in a closed system. |
| equilibrium vapor pressure | The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature. |
| freezing point | The temperature at which the solid and liquid are in equilibrium at 1 atm pressure. |
| Le Chatelier's principle | When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress. |
| Molar heat of fusion | The amount of heat energy required to melt one mole of solid at its melting point. |
| molar heat of vaporization | The amount of heat energy needed to vaporize one mole of liquid at its boiling point. |
| phase | Any part of a system that has uniform composition and properties. |
| phase diagram | A graph of pressure versus temperature that shows the conditions under which the phases of as substance exist. |
| sublimation | The change of state from a solid directly to a gas. |
| triple point | Indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium. |
| volatile liquid | Liquids that evaporate readily. |
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