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Transcript
2009 Chemistry I: Modern Chemistry Holt, Rinehart, & Winston Unit 3 Chapter 10 – States of Matter, pp 329-351 1 amorphous solid; 2 boiling; 3 boiling point; 4 capillary action; 5 condensation; 6 critical point; 7 critical pressure; 8 critical temperature; 9 crystal; 10 crystalline solids; 11 crystal structure; 12 deposition; 13 diffusion; 14 effusion; 15 elastic collision; 16 equilibrium; 17 equilibrium vapor pressure; 18 evaporation; 19 fluid; 20 freezing point; 21 ideal gas; 22 kinetic-molecular theory; 23 melting; 24 melting point; 25 molar enthalpy of fusion; 26 molar enthalpy of vaporization; etc… 1 solids in which the particles are arranged randomly 2 a change of a liquid to bubbles of vapor that appear throughout the liquid as well as at its surface 3 temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure 4 attraction of surface of a liquid to the surface of a solid 5 process by which a gas changes to a liquid 6 the critical temperature & critical pressure of a substance 7 the lowest pressure at which the substance can exist as a liquid at the critical temperature 8 temperature above which a substance cannot exist in the liquid state 9 substance in which particles are arranged in an orderly, geometric, repeating pattern 10 solids consisting of crystals 11 the total 3-dimensional arrangement of particles of a crystal 12 change of state from a gas directly to a solid 13 spontaneous mixing of the particles of 2 substances caused by their random motion 14 process by which gas particles pass through a tiny opening 15 a collision in which there is no net loss of total kinetic energy 16 dynamic condition in which 2 opposing changes occur at equal rates in a closed system 17 pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature 18 process by which particles escape from the surface of a non-boiling liquid & enter the gas state 19 substance that can flow and will take the shape of its container 20 temperature/ pressure at which the liquid & solid of a substance are at equilibrium 21 a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory 22 an explanation for the properties & behavior of solids, liquids, & gases in terms of energy & forces 23 physical change of a solid to a liquid by addition of thermal energy 24 the temperature/ pressure at which a solid becomes a liquid 25 amount of thermal energy required to melt 1 mole of solid at the solid’s melting point 26 amount of thermal energy needed to vaporize 1 mol of liquid at its boiling point at constant pressure (cont.) 27 phase; 28 phase diagram; 29 real gas; 30 sublimation; 31 supercooled liquids; 32 surface tension; 33 triple point; 34 unit cell; 35 vaporization; 36 volatile liquids 27 any part of a system that has uniform composition and properties 28 graph of pressure vs. temperature showing the conditions under which phases of a substance exist 29 gas that does not behave completely according to the assumptions of the kinetic-molecular theory 30 change of state from a solid directly to a gas 31 substances that retain liquid properties even at temperatures at which they appear to be solid 32 force tending to pull adjacent parts of a liquid’s surface together, decreasing surface area maximally 33 temperature & pressure at which the solid, liquid, & vapor of a substance can coexist at equilibrium 34 the smallest portion of a crystal lattice that shows the 3-D pattern of the entire lattice 35 process by which a liquid or solid changes to a gas 36 liquids that evaporate readily Chapter 11 – Gases, pp 361-388 1 absolute zero; 2 atmosphere of pressure; 3 Avogadro’s law; 4 barometer; 5 Boyle’s law; 6 Charles’ law; 7 combined gas law; 8 Dalton’s law of partial pressures; 9 Gay-Lussac’s law; 10 Gay-Lussac’s law of combining volumes of gases; 11 Graham’s law of effusion; 12 ideal gas constant; 13 ideal gas law; 14 millimeters of mercury; 15 newton; 16 partial pressure; etc… 1 the temperature –273.15oC, equal to 0 Kelvin 2 pressure exactly equivalent to 760 mm Hg 3 equal volumes of gases at the same temperature & pressure contain equal #s of molecules 4 device used to measure atmospheric pressure 5 the volume of a fixed mass of gas varies inversely with the pressure at constant temperature 6 the volume of a fixed amount of gas at constant pressure varies directly with Kelvin temperature 7 an expression of the relationship between pressure, volume, & temperature of a fixed amount of gas 8 the total pressure of a gas mixture is the sum of the partial pressures of the component gases 9 the pressure on a fixed mass of gas at a constant volume varies directly with the Kelvin temperature 10 at constant temperature & pressure, the volume of gaseous reactants & products can be expressed as ratio of small whole numbers 11 the rates of effusion of gases at the same temperature & pressure are inversely proportional to the square roots of their molar masses 12 the constant R in the equation PV = nRT 13 mathematical relationship among temperature, volume, pressure, & # of moles of a gas 14 common unit of pressure symbolized by mm Hg 15 the force that will increase the speed of 1 kg by 1 meter per second each second the force is applied 16 the pressure of each gas in a mixture (cont) 17 pascal; 18 pressure; 19 standard molar volume of gas 17 the pressure exerted by a force of 1 Newton acting on a surface area of 1 square meter 18 force per unit area on a surface 19 the volume occupied by 1 mole of gas at STP Chapter 12: Solutions, pp 401-425 1 colloid; 2 concentration; 3 effervescence; 4 electrolyte; 5 enthalpy of solution; 6 Henry’s Law; 7 hydration; 8 immiscible; 9 miscible; 10 molality; 11 molarity; 12 nonelectrolyte; 13 saturated solution; 14 solubility; 15 soluble; 16 solute; 17 solution; 18 solution equilibrium; 19 solvated; 20 solvent; 21 supersaturated solution; 22 suspension; 23 Tyndall effect; 24 unsaturated solution 1 mixtures in which particles are of intermediate size between those in solution & in suspensions 2 measure of the amount of solute in a given amount of solvent or solution 3 the rapid escape of gas from a liquid in which it is dissolved 4 substance in aqueous solutions that allows electrical conductivity 5 net amount of energy absorbed as heat by the sol’n when specific am’t of solute dissolves in solvent 6 solubility of gas in liquid is directly proportional to partial pressure of that gas on surface of liquid 7 solution process with water as the solvent 8 liquids that are not soluble in each other 9 liquids that dissolve freely in one another in any proportion 10 number of moles of solute in one kilogram of solvent 11 number of moles of solute in one liter of solution 12 substance in aqueous solution that does not permit electrical conductivity 13 solution containing maximum amount of dissolved solute 14 am’t of substance required to form saturated sol’n with specific am’t of solvent at specified temp. 15 capable of being dissolved 16 substance dissolved in a solution 17 homogeneous mixture of 2 or more substances in a single phase 18 physical state in which opposing processes of solute dissolution/crystallization occur at equal rates 19 solute particle that is surrounded by solvent molecules 20 the dissolving medium in a solution 21 solution containing more dissolved solute than a saturated solution under the same conditions 22 mixture in which particles in a solvent are so large that they settle out unless constantly agitated 23 property by which light is scattered by particles in heterogeneous mixtures 24 solution containing less than the maximum amount of solute under existing conditions Chapter 13: Ions in Aqueous Solutions & Colligative Properties, pp 434-457. 1 boiling-point elevation; 2 colligative properties; 3 dissociation; 4 freezing-point depression; 5 hydronium ion; 6 ionization; 7 molal boiling-point constant; 8 molal freezing-point constant; 9 net ionic equation; 10 nonvolatile substance; 11 osmosis; 12 osmotic pressure; 13 semipermeable membrane; 14 spectator ions; 15 strong electrolyte; 16 weak electrolyte 1. difference between the boiling points of the pure solvent & a solution of nonelectrolyte in that solvent & is directly proportional to the molal concentration of that solute 2. properties depending on the concentration but not the identity of solute particles 3. the separation of ions when an ionic compound dissolves in an aqueous solution 4. difference between the freezing points of the pure solvent & a solution of nonelectrolyte in that solvent & is directly proportional to the molal concentration of that solute 5. the H3O+ ion 6. process by which ions are formed from solute molecules by the action of the solvent 7. boiling-point elevation of the solvent in a 1-molal solution of a nonvolatile, nonelectrolyte solute 8. freezing-point depression of the solvent in a 1-molal solution of a nonvolatile, nonelectrolyte solute 9. equation including only those compounds & ions undergoing a chemical change in aqueous solution 10. substances that have little tendency to become a gas under existing conditions 11. movement of water through a semipermeable membrane from the area of low solute concentration to the area of high solute concentration 12. the external pressure that must be applied to stop osmosis 13. a membrane that allows the passage of some particles while blocking the passage of others 14. ions not taking part in a chemical reaction & are found in solution both before & after the reaction 15. any compound whose dilute aqueous solution conducts electricity well 16. any compound whose dilute aqueous solution conducts electricity poorly