2random, medium speed, limited distances
liquid
3random, fast, cover large distances
gas
4attractive forces between polar molecules
dipole dipole interaction
5occurs in molecules that have H atoms bonded in N, O, F
6measure of elastic force in the surface of a liquid
surface tension
7tendency of a liquid to rise in narrow tubes
capillary action
8attraction between like molecules
cohesion
9attraction between unlike molecules
adhesion
10measure of a fluids resistance to flow
viscosity
11pressure exhibited by vapor present above a liquid surface
vapor pressure
12energy required to vaporize 1 mole of liquid at a given temperature
molar heat of vaporization
13temperature when liquid turns into gas
boiling pont
14three areas in the phase diagram
solid, liquid, gas
15three lines in phase diagram
melting/freezing, vaporization/condensation, sublimation/deposition
16two points in phase diagram
triple point, critical point
17all phases at equilibrium
triple point
18terminates liquidas phase line, also called supercritical fluid
critical point
19a plot of the temperature versus time
heating curve
20show how temperature changes as substance is cooled down
cooling curve
21way f describing solution composition
mole fraction
22mole of component/total mole of all component
mole fraction of component
23moles of solute/L solution
molarity
24properties of a solution that depend ONLY on number and NOT on identity
colligative properties
25direct measure of escaping tendency of molecules
vapor pressure lowering
26P=XP⁰
vapor pressure lowering
27increase in boiling point temperature from adding non volatile solute to a solvent
boiling point elevation
28∆B=Kbm
boiling point elevation
29decrease in freezing point temperature
freezing point depression
30∆Tf=Kfm
freezing point depression
31study of heat and energy changes that accompan physical ang chemical processes
thermochemistry
32first law of thermodynamics
law of conservation of energy
33gives off heat to it's surroundings
exothermic
36heat released by the system
exothermic
37work done by the system
exothermic
38absorbs heat from the surrounding
endothermic
41heat absorbed by the system
endothermic
42wor done on the system
endothermic
43states that change in enthalpy for any chemica reaction remains constant whether it occurs in one or several steps
Hess's Law
44energy contained within the system
internal energy
45sum of kinetic and potential energy of all components of the system
internal energy
46denoted by "E"
internal energy
47effect of temperature
increase in temperature causes reactant particles to move rapidly resulting to more collision
48effect of concentration
when concentration increases, the frequency of collisions is increased and reaction is sped up
49effect of particle size
tinier particles have greater surface area and provide much greater contact and effect more collision
50effect of catalyst
substance that speeds up the reaction process
51biological catalyst
enzyme
52measured by a change in concentration of reactants and products per unit time
rates of reaction
53rate of reaction remains the same regardless of an increase in the concentration of reactants
zero order reaction
54r=k[A]⁰
zero order reaction
55rate of reaction is directly proportional to the product of concentration of reactants raised to the first power
first order reaction
56r=k[A]
first order reaction
57energy needed for the formation of an activated complex
activation energy
58"Particles can only react if they collide with enough energy for the reaction to take place."
collision theory
59ineffective collision
-not properly oriented -slow moving particles
60effective collision
fast moving and correctly oriented
61increase the rate of a chemical reaction
positive catalyst
62decrease the rate of reaction
negative catalyst
63the product f a reaction is the catalyst itself
auto catalyst