Download Chem Unit 3 Vocabulary

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