Honors Chemistry Semester 2 Finals

Front 1

volume

Back 1

the total amount of space taken up of a container
(in Liters, L)

Front 2

temperature

Back 2

energy of gas particles
(Kelvin, K)

Front 3

pressure

Back 3

collision of gas particles w/ container
(in atmospheres- atms)

Front 4

moles

Back 4

number of gas particles
(mol, n)

Front 5

Boyle's Law

Back 5

P and V are inversely proportional
Pi x Vi = Pf x Vf

Front 6

Charles' Law

Back 6

T and V are directly proportional
Vi/Ti = Vf/Tf

Front 7

Avogadro's Law

Back 7

relationship between n & V
n/v = constant

Front 8

molar volume of a gas

Back 8

amt of space a gas will occupy @ STP

Front 9

___torr = ___ atm

Back 9

760 torr = 1 atm

Front 10

Dalton's Law of Partial Pressure

Back 10

the overall pressure of a mixture of gases is equal to the sum of the pressures for the individual gases
Ptot = P1+P2+P3

Front 11

solubility

Back 11

maximum amount of solute that be dissolved in a solvent

Front 12

saturated

Back 12

maximum amt of solute dissolved in solvent

Front 13

how are solubility and temperature related for solids?

Back 13

solubility of solids increases with increasing temperature.

Front 14

unsaturated solution

Back 14

less than the maximum amount of solute is dissolved in the solvent

Front 15

how are solubility and T related for gases?

Back 15

solubility decreases w/ increasing T. increases with increasing P

Front 16

concentration

Back 16

amount of solute in a given amt of solvent

Front 17

Molarity (M)

Back 17

mols solute
---------------
L solution

Front 18

3 steps for making solution from a solid

Back 18

1. calculate the # of grams needed
2. measure out the solid and addit to the volumetric flask
3. add water to the line- total V

Front 19

3 steps for making solution from stock solution

Back 19

1) calculate the volume of stock solution needed
2) measure stock solution and add to volumetric flask
3) add solvent to the line

Front 20

dilution equal equasion

Back 20

M1 x V1 = M2 x V2

Front 21

vapor pressure

Back 21

pressure due to evaporation of solvent particles
liquid <----> gas

Front 22

dynamic equilibrium (for gas/liquid)

Back 22

same amt of liquid particles becoming a gas as of gas particles becoming a liquid

Front 23

boiling temperature

Back 23

100.0 C. temp when vapor pressure = atmospheric pressure

Front 24

colligative properties

Back 24

properties that depend on the quantity of solute present not the identity (it doesn't matter WHAT just HOW MUCH solute)

Front 25

boiling point elevation

Back 25

bp of a solution is higher than the bp of a pure solvent
aka >100.0 C

Front 26

freezing point depression

Back 26

fp of a soln is lower than the freezing pt of a pure solvent

Front 27

bp equasion

Back 27

BPsoln = BPsolvent + change in Tb

Front 28

fp equasion

Back 28

FPsoln = FPsolv - change in Tf

Front 29

molality (m)

Back 29

mol solute
---------------
kg solvent

Front 30

change in T depends on...

Back 30

1) identity of solvent (k)
2) molality of solute (conc)

Front 31

change in Tf equation

Back 31

[delta]Tf = i x Kf x m
i = number of ions the substance breaks into

Front 32

change in Tb equation

Back 32

[delta]Tb = i x Kb x m

Front 33

kinetics

Back 33

the study of rxn rates

Front 34

reaction mechanism

Back 34

series of steps to go from reactants to product

Front 35

substitution rxn

Back 35

one atom/group of atoms replaces another

Front 36

find the change in the energy of a reaction (equation)

Back 36

[delta]Hrxn = [delta]H( bonds broken) - [delta]H(bonds formed)

Front 37

relationship between forward and reverse enthalpy changesq

Back 37

[delta]Hforward = -[delta]Hreverse

Front 38

transition state

Back 38

structure(s) in between reactants and product

Front 39

bond enthalpy

Back 39

energy required to break a bond
always +

Front 40

enthalpy

Back 40

the amount of energy available

Front 41

Collision theory (3)

Back 41

in order for a rxn to occur, molecules
1) must collide
2) w/ the proper orientation
3) and sufficient energy

Front 42

catalyst

Back 42

a molecule/compound that speeds upa rxn that is not consumed in the rxn

Front 43

ezymes

Back 43

biological catalysts

Front 44

how do enzymes work? (2)

Back 44

1) lowering activation energy
2) &/or orienting molecules

Front 45

concentration and rate relationship

Back 45

a higher conc of solute increases the rate

Front 46

rate law

Back 46

equation used to describe the effect of concentration on rate

rate = k[A]^x *[B]^y

Front 47

Hess's Law

Back 47

if a series of rxns can be added to give an overall rxn, then the energies of the rxns can be added to give the energy of the overall rxn

Front 48

how to do Hess's Law probs (3 steps)

Back 48

1. flip rxns as needed to organize the rxns to be added so that the reactnats are on the reactant side & products are on the product side (location of compounds match the overall equasion)
2. make coeffiecients in the rxns to be added match the coefficients in the overall rxn by muliplying by same #
3. add rxns together

Front 49

average rate

Back 49

change in conc over a period of time
[delta][A]
--------------
[delta]t

Front 50

instantaneous rate

Back 50

how the conc is changing at a specific time

Front 51

inital rate

Back 51

instantaneous rate at the beginning of a rxn

Front 52

what can rate laws not be determined by?

Back 52

rate laws cannot be determined by stoichiometry. only get it by experiment

Front 53

reaction orders

Back 53

tells how a change in specific conc affects the rate

Front 54

ORDERS: 0

Back 54

0th: x=0
--2x => no change in rate
--4x => no change in rate

Front 55

ORDERS: 1

Back 55

1st: x=1
--2x conc => 2x rate
--4x conc => 4x rate

Front 56

ORDER: 2

Back 56

2nd: x= 2
change in conc has a squared change in rate
--2x conc =>4x rate
--4x conc =>16x rate

Front 57

rate law- determining
2 main steps

Back 57

1) determine rxn orders
--choose 2 experiments where only 1 conc changes
2) determine the rate constant
--plugging in experimental values

Front 58

rxn mechanics

Back 58

a series of steps that occur to get from reactants to products
--sum of the steps in a mechanism must give the overall rxn
-only valid if it matches the experimental rate law

Front 59

rate determining step

Back 59

slowest step in a rxn.
-determines the rate for the entire rxn

Front 60

intermediates

Back 60

substance made in the step & used in a later step
=> doesn't appear in overall equation

Front 61

dynamic equilibrium

Back 61

rate of forward rxn = rate of reverse rxn
-rxn doesnt stop, but the conc of reactants & prod.s stop changing

Front 62

Keq =

Back 62

Keq = Kfor [products]
---------- = ---------------
Krev [reactants]

Front 63

what phases are included in Keq?

Back 63

aqueous (aq)
gas (g)
NOT
solids (s)
liquids (l)

Front 64

when is Keq product/reactant favored?

Back 64

if Keq <1 then it is a reactant favored rxn
if Keq>1 it is a product favored rxn

Front 65

Le Chatelier's Principle

Back 65

if a rxn at equilibrium is distrubed then the rxn will shift to minimize the effect of the disturbance & reachieve equilibrium

Front 66

adding products?

Back 66

shift to left-reactants

Front 67

removing reactants?

Back 67

shifts left-reactants

Front 68

remove products?

Back 68

shifts right- products

Front 69

add reactants?

Back 69

shifts right-products

Front 70

GAS EQ
decrease V = increase P

Back 70

shift to side w/ fewer moles of gas

Front 71

GAS EQ
increase V = decrease P

Back 71

shift to side with more moles of gas

Front 72

[delta]H = + (positive)
heat/energy as a ______

Back 72

reactant.
increase T, shift to right, K will get bigger
decrease T, shift to left, K will get smaller

Front 73

[delta]H = - (negative)
heat/energy as a ____

Back 73

product
increase T, shift to left, K will get smaller.
decrease T, shift to right, K will get bigger

Front 74

q = mc[delta]T
variables?

Back 74

q=heat (J)
m=mass (g)
c=specific heat capacity (J/g x degrees Celsius)
[delta]T=change in temp (K or C)

Front 75

specific heat capacity

Back 75

energy required to raise the temp of 1g of a substance by 1`C

Front 76

1st law of thermodynamics (law of cons. of energy)

Back 76

energy cannot be created or destroyed therefore
q(hot) = --q(cold)

Front 77

to find [delta]Hrxn
(3 steps)

Back 77

1) q(water) q=mc[delta]T
2) q(rx) q(rxn)=--q(water)
3) [delta]Hrxn = q(rxn)
--------------
n (limit.react.)

Front 78

electrolytes

Back 78

dissolve in H2O and produce ions
-conduct electricity
--ionic compounds

Front 79

non-electrolytes

Back 79

dissolve in H2O but no ions
-doesn't conduct electricity
--covalent compounds

Front 80

strong electrolyte

Back 80

completely dissociates
product favored

Front 81

weak electrolyte

Back 81

partially dissociates
reactant favored

Front 82

7 strong acids

Back 82

1) HCl - hydro chloric acid
2) HBr - hydrobromic acid
3) HI - hydroiodic acid
4) HNO3 - nitric acid
5) H2SO4 - sulfuric acid
6) HClO4 - perchloric acid
7) HClO3 - chloric acid

Front 83

3 defining aspects of ACIDS

Back 83

1. sour taste
2. turns litmus red
3. reacts w/ metal to produce H2

Front 84

3 defining aspects of BASES

Back 84

1. bitter taste
2. turns litmus blue
3. aqueous solutions feel slippery

Front 85

Arrhenius def. acid

Back 85

produces H+ ions in H20

Front 86

Arrhenius def. bases

Back 86

produces OH- ions in H20

Front 87

strong bases?

Back 87

group 1 hydroxides
soluble hydroxides group 2 (Ca, Sr, Ba)

Front 88

monoprotic acids

Back 88

--lose 1 H+
(all strongs acids but H2SO4)

Front 89

diprotic acids

Back 89

lose 2 H+
(only H2SO4)

Front 90

pH

Back 90

measure of the amt of H+
pH = --log[H+]

Front 91

Kw ?

Back 91

the auto-ionization constant for water

Front 92

buffers

Back 92

solns that resist a change in pH
composed of a conjugate acid/base pair

Front 93

radioactivity

Back 93

spontaneous emissions of energy &/or particles from the nucleus

Front 94

e- capture

Back 94

the nucleus snags an electron from 1 of lower energy orbitals
particle as a reactant

Front 95

gamma radiation

Back 95

high energy radiation
causes no change to the nucleus
usually accompanies another type of decay

Front 96

polymers

Back 96

long chain of molecules made of smaller molecules

Front 97

monomers

Back 97

small molecules that react to form long chains

Front 98

addition polymers

Back 98

monomers bond together to make one chain

Front 99

condensation polymers

Back 99

polymerization creates a small molecule as a byproduct

Front 100

what 5 things affect rxn rate?

Back 100

rate, k, Ea, orientation, concentration

Front 101

Bronsted-Lowry def. acid

Back 101

anything that donates a proton

Front 102

Bronsted-Lowry def. base

Back 102

anything that accepts a proton

Front 103

Kw =

Back 103

[OH-] x [H3O+]
10^-7

Front 104

intermolecular forces def. &
3 types?

Back 104

attraction between molecules
1) London Dispersion forces- nonpolar molecules
2) dipole-dipole forces - polar molecules
3) hydrogen bonding (VERYstrong, but not a bond)

Front 105

London Dispersion Forces

Back 105

condensed states are formed by (the domino effect) attraction of e- in other molecules to the instantaneous dipole

Front 106

instantaneous dipole

Back 106

momentary uneven distribution of e-

Front 107

dipole-dipole

Back 107

uneven sharing of e- creating partial charges
attraction of partial charges on polar molecules

Front 108

hydrogen bonding

Back 108

-very strong dipole force
-NOT a bond
-must have an H bonded to an N, O, F
-attracted to a N,O,F in another molecule

Front 109

kinetic molecular theory of gases
(4)

Back 109

1. the V of a gas molecule is small compared to the distance between molecules
2. gases experience no IMFs
--gases neither attract nor repel each other
3. gases are in constant, rapid, random motion & their collisions are elastic
4. the average kinetic energy of a gas is proportional to its T (K)