| Term | Definition |
|---|
| 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 |
| equilibrium | dynamic condition in which two opposing changes occur at equal rates in a closed system |
| condensation | the process by which a gas changes to a liquid |
| equilibrium vapor pressure | pressure exerted by a vapor in equilibrium; with its corresponding liquid at a given temperature |
| volatile | liquids that evaporated readily |
| sublimation | change of state from a solid directly to a gas |
| deposition | change of state from a gas directly to a solid |
| phase diagram | a graph of pressure versus temperature that shows the conditions under which the phases of a substance exist |
| triple point | indicates the temperature and pressure conditions at which the solid, liquid and vapor of the substance can coexist at equilibrium |
| properties of water | boils at 100 degress Celsius, low density, floats, polar compound with bent shape, high molar heat of fusion, high molar heat of vaporization, expands when freezes |
| solute | substance dissolved in a solution |
| solvent | dissolving medium in a solution |
| solution | homogeneous mixture of two or more substances in a single phase |
| saturation | the amount of dissolved solute |
| dissociation | separation of ions that occurs when an ionic compound dissolves |
| colligative properties | properties that depend on the concentration of solute particles but not on their identity |
| molarity | the number of moles of solute in one liter of solution |
| molality | the concentration of a solution expressed in moles of solute per kilogram of solvent |
| weak electrolyte | any compound whose dilute aqueous solutions conduct electricity poorly |
| strong electrolyte | any compound whose dilute aqueous solutions conduct electricity well |
| concentrated | relatively large amount of solute in a solvent |
| diluted | relatively small amount of solute in a solvent |
| Avogadro's Law | equal volumes of gases at the same temperature and pressure contain the same number of molecules |
| Kinetic-Molecular Theory | particles of matter are always in motion |
| Boyle's Law | relates pressure and volume of a gas V1P1=V2P2 |
| Charles's Law | relates the temperature and volume of a gas V1/T1=V2/T2 |
| Gay-Lussac's Law | pressure of a gas is directly proportional to the Kelvin temperature if the volume is kept constant P1/T1=P2/T2 |
| combined gas law | P1V1/T1=P2V2/T2 |
| Dalton's law of partial pressure | in the absence of a chemical reaction the pressure of a gas mixture is the sum of the individual pressures of each gas alone Ptotal=P1+P2+P3+... |
| partial pressure | pressure of each gas in a mixture |
| diffusion | spontaneous mixing of particles of two substances (gases) cased by their random motion |
| effusion | process by which gases pass thorugh a tiny opening |
| barometer | measures pressure |
| measure of pressure | torr, kPa, atm |
| standard molar volume of a gas | volume occupied by one mole of a gas at STP |
| ideal gas law | PV=nRT where P is pressure, V is volume, n is the # of moles, R is the constant, and T is the temperature |
| R | ideal gas constant |
| Molar mass | M=mRT/PV where M is the molar mass, m is the mass of gas, R is the constant, T is the temperature, P is the pressure, and V is the volume |
| Density | D=MP/RT where D is the density, M is the molar mass, P is the pressure, R is the constant, and T is the temperature |
| Arrhenius | acids produce higher concentration of H+ or H3O+; bases produce higher concentration of OH- |
| Bronsted-Lowry | acids donate proton; bases accept proton |
| amphoteric | any species that can react as either an acid or base |
| acid | compounds with H+ or H3O+ ions |
| base | compounds with OH- ions |
| conjugate acid | species that is formed with a base gains a proton |
| conjugate base | species that is formed with an acid loses a proton |
| monoprotic | donates one proton |
| polyprotic | donates more than one proton |
| endpoint | the point in a titration at which an indicator changes color |
| equivalence point | the point at which the two solutions used in a titration are present in chemically equivalent amounts |
| Lewis | acids accept electron pair and bases donate election pair |
Combine with other sets
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