| A | B |
|---|
| intermolecular forces | forces between molecules, not as strong as within molecule (covalent & ionic) |
| vander waals forces | dispersion forces |
| dipole | slightly polar |
| hydrogen bonding | very polar- strongest |
| KE formula | KE = 1/2(mass)(velocity)^2 |
| temperature | average of KE |
| true solids | particles are arranged in orderly, repeating pattern. |
| member | one particle (of true solid) |
| unit cell | simplest repeating unit; retains shape |
| crystal lattice | 3 dimensional arrangement of unit cells repeated over & over |
| anhydrous | compound containing no water of hydration |
| hydrate | compound w/water molecules attatched (CuSo4 * 6H2O) |
| hydroscopic | absorbs water from surroundings (packets in vitamin bottles) |
| deliquescent | absorbs enough water from surroundings to become a liquid (NaOH) |
| efflorescent | releases H20 to surroundings (bread) |
| amorphous | solis, no definite repeating pattern. No true melting point. No plateau. (Glass, butter, tar, plastic) |
| polymorphous | many forms of the same substance |
| isomorphous | two substances that have the same structure |
| pressure | measure of forces w/which gas molecules hit the side of a container |
| Normal atmospheric pressure | 760 torrs |
| vapor pressure | pressure excerted by vapor molecules above a liquid when dynamic equilibrium is reached |
| dynamic equilibrium | two opposite processes ocurring at the same rate |
| volatility | how easily a liquid evaporates |
| very volatile | high vapor pressure, low inter-molecular forces, low boiling point |
| not volatile | low vapor pressure, strong inter-molecular forces, high boiling point |
| sublimation | solid changes directly to gas w/o going through liquid phaser |
| melting/freezing | solid to liquid/liquid to solid |
| vaporization | liquid to gas |
| evaporization | occurs only on surface; room temperaturel cooling process;sweat |
| boiling | occurs throughout the liquid; requires energy |
| boiling point | vapor pressure = atmospheric pressure |
| water properties | high BP, MP Cp, high surface tension (needle floats), ice is less dense than water because the hydrogen bonds stifen and spread apart |
| phase diagrams | graphs that show conditions (tem & press) under which a substance will exist as a solid, liquid or gas |
| triple point | all 3 states are in equilibrium |
| critical temperature and pressure | a gas cannot be liquified above this point |
| melting <--> freezing pnt | solid <--> liquid |
| boiling <--> condensation pnt | liquid <--> gas |
| deposition <--> sublimation | solid <-->gas |
| energy transfered from one body to another because of a difference in temp | heat |
| calories, joules | heat |
| degrees (C, F, K) | temp |
| measured indirectly w/a calorimeter | heat |
| measured w/a thermometer | temp |
| specific heat or heat capacity | amount of heat needed to raise 1 gram of a substance 1*C |
| Calorie | amount of heat needed to raise 1 gram of water 1*C |
| heat of fusion (HF) | amount of heat needed to melt 1 gram of a substance at its melting point |
| heat of vaporization | amount of heat needed to vaporize 1 gram of a substance at its boiling point |
