Ap Chemistry

Front 1

Aufbau Principle

Back 1

as protons are added one by one electrons are also added to the orbitals

Front 2

Pauli Exclusion Principle

Back 2

No two electrons can have the same set of quantum numbers, each orbital has two with opposites spins

Front 3

Hunds Rule

Back 3

to minimize energy of an atom, maximize the spin

Front 4

Quantum Numbers - 1

Back 4

Principle quantum number - rows on the periodic table
"n" integral values 1,2,3. a) orbital size increases
b) spend ore time away nucleus. c) less tightly bound to the nucleus, ore apt to leave.

Front 5

Quantum Numbers - 2

Back 5

Angular Momentum Quantum Number Azimuthal -
l - integral values from 0
0 -s (sphere 1) 1-p (dumbell 3) 2-d (clover 5) 3-f (double clover 7)

Front 6

Quantum Number -3

Back 6

Magnetic Quantum Number - m(sub L) -l - +l integral values related to the orientations of orbitals in space
s-2
p-6
d-10
f-14

Front 7

Quantum -4

Back 7

electron Spin Quantum - M(sub s) +1/2 -1/2

Front 8

Orbital Box vs Standard

Back 8

boxes vs. configuration

Front 9

Atomic Radii

Back 9

Size Increases as you go down and decreases as you go right.

Front 10

ionization energy

Back 10

as you go further from the nucleus, there is less attraction as you go down, ionization decreases as you go right, ionization increases

Front 11

electron affinity

Back 11

energy associated with each added electron as you go up and right it increases

Front 12

Electromagnetic Spectrum

Back 12

Radio Micro Infrared Visible Ultraviolet X-Ray Gamma
Red Long 700 nm - Violet Short 400 nm

Front 13

λf=c

Back 13

λ = wavelength in meters
f = frequncy in hz of s^-1
c- 3 x 10 ^8 m/s

Front 14

E=hf

Back 14

E= energy in a single proton (-19 visible)
h= Plank's Constant
f = frequncy in hz of s^-1

Front 15

λ= h/mv

Back 15

DeBrogle-the wavelength is inversely proportional to the momentum of a particle
λ= wavelength in meters
h= Plank's
m= mass in kg
v= velocity m/s

Front 16

Chemical Equilibrium

Back 16

the state where the concentrations of all reactants and products remain constant

Front 17

Forward Reaction A + B =C + D

Back 17

----->

Front 18

Reverse Reaction A + B =C + D

Back 18

<------

Front 19

Equilibrium Constant

Back 19

K...Kc...Keq
law of mass action K = [products]^mols/ [Reactants] ^ mols

Front 20

If a reaction is reversed... then the value is

Back 20

Inversed

Front 21

if a balanced equation is multiplied by a factor "n"

Back 21

raise the original to "n" power

Front 22

if Keq is large (greater than one)

Back 22

it has more products, products favored, shift right

Front 23

If Keq is small (less than one)

Back 23

more reactants, reactants favored, shift left

Front 24

What are the Standard states of equilibrium

Back 24

25C and 1 atm

Front 25

Equilibrium in pressure

Back 25

with gases use partial pressure Kp = (P products) / (P reactants)

Front 26

Find Kp

Back 26

Kp = Keq (RT) ^change in "n"
T- temp in Kelvins
n - coefficient of products- reactants

Front 27

What is Hetero-genius Equlibria - importance?

Back 27

reactants and products are in different phases/ do not include solids and pure liquids when finding the Keq

Front 28

Reactant Quotient

Back 28

Q .... if Q= K its in equilibrium no shift
Q > K shifts left products consumed reactants are formed
Q < K shifts right products are formed
IF NO INITIAL PRODUCT SHIFT RIGHT

Front 29

How to do an equilibrium Problem

Back 29

1. write balanced equation
2. write equilibrium equation law of mass action
3. List initial concentrations
4. Calculate Q
5. Define the change needed
6. Define Equilibrium concentrations
7. Substitute the equilibrium expression and solve
Check Your K Value

Front 30

LeChatalier's Principle

Back 30

if a stress is applied to a system at equilibrium the system will shift if possible in the direction that completely or least partially alleviates the stress
Keq wont Change because temp doesnt

Front 31

LeChat- how do you change pressure?

Back 31

adding or removing gas or increase or decrease temperature

Front 32

How can a system decrease its own pressure

Back 32

by shifting in the are where there are fewer gas particles

Front 33

When pressure changes..

Back 33

amounts of reactants and products change, not concentrations Keq doesn't change
Only count gas molecules to determine shift

Front 34

When pressure increases

Back 34

volume decreases

Front 35

endothermic

Back 35

absorbs heat

Front 36

exothermic

Back 36

releases heat

Front 37

Arrheneus Concept

Back 37

acids produce H+ and bases produce OH - in aqueous solutions

Front 38

Bronstad Lowry Model

Back 38

an acid H+ donator and a base is a proton acceptor water is a B-L base
Acid + base = conjugate acid and conjugate base

Front 39

Ka of a strong acid...

Back 39

lies to the right/ wants to get rid of H+
most of original acid dissociates

Front 40

A strong acid makes...

Back 40

a weak conjugate base

Front 41

Ka of weak acid..

Back 41

lies to the left/ wants H+
most of the original acid stays

Front 42

monoprotic acid-

Back 42

acid who donates one H+

Front 43

diprotic/ triprotic

Back 43

acid who donates two/three H+

Front 44

Amphoteric

Back 44

water acts as an acid or base

Front 45

Neutral
Acid
Base

Back 45

[H+] = [OH-]
[H+] > [OH-]
[H+] < [OH -]

Front 46

Kw=

Back 46

1.0 x 10^-14

Front 47

Soren Sorenson

Back 47

PH Scale

Front 48

PH is..

Back 48

the power of a hydrogen ion
measured in a log scale base 10

Front 49

1 PH increase is...
PH of four =

Back 49

an increase in H+ by 10
1 x 10^-4 M acidity

Front 50

Explain PH Scale

Back 50

0 acid
7 neutral
14 base

Front 51

how do you find PH? POH?

Back 51

pH= -log [H+]
pOH = -log {OH -}

Front 52

major species vs minor species

Back 52

major components in large amounts in a solution
minor- components in small amounts

Front 53

pH --> concentration
concentration --> pH

Back 53

log
antilog

Front 54

Lewis Structures Rules

Back 54

Be or B can have less than 8
Nitrogen can have less than 8 and odd numbers
1st and 2nd row cant exceed octet

Front 55

Types of Chemical Bonds-

Back 55

ionic polar covalent
ionic pairs have lower energies than separated ions

Front 56

Coulombs Law

Back 56

relationship between charge and distance - less energy to be together -- charge (Q1Q2)/(Radius)

Front 57

bond length

Back 57

distance where energy is a minimum

Front 58

polar

Back 58

sharing but one atom attracts an electron more

Front 59

electronegativity

Back 59

the ability of an atom in a molecule to attract right increase down decrease
0 -> .4 covalent
.5 -> 1.9 polar covalent

Front 60

dipole moments

Back 60

a molecule which has an end which has a center of positive charge and a center negative charge

Front 61

If central atom is less than outer atoms

Back 61

no dipole

Front 62

ion size

Back 62

down increase right decrease

Front 63

Isoelectron

Back 63

same amount of electons

Front 64

Lattice energy

Back 64

energy required to break up molecules. the change in energy that takes place when separated gaseous ions are packed together to form an ionic shield k(QQ/R)

Front 65

when bonds are broken...

Back 65

endothermic
DeltaH bonds broken- bonds formed

Front 66

Hybridization

Back 66

the mixing of normal orbitals to form new ones to get maximum bond energy and minimize repulson

Front 67

2 electron pairs

Back 67

linear sp

Front 68

3 electron pairs

Back 68

trigonal planar sp2

Front 69

4 electron pairs

Back 69

tetrahedral sp3

Front 70

5 electron pairs

Back 70

trigonal bipyramidal dsp3

Front 71

6 pairs

Back 71

octahedral d2sp3

Front 72

Sigma

Back 72

every bond. single bonds double and trible

Front 73

pi

Back 73

every double bond one. triple bond two

Front 74

Peromagnetism

Back 74

causes a substance to be repelled by a magnetic field due to unpaired electrons

Front 75

diamagnetism

Back 75

causes a substance to be attracted by magnetic fields due to paired electrons

Front 76

intramoleculer bonding

Back 76

bonding between atoms in a molecule

Front 77

intermolecule bonding

Back 77

occurs between molecules

Front 78

dipole forces

Back 78

attractive forces resulting when polar molecules line up so that positive and negative ends are close - 1% as strong as covalent

Front 79

intra < or > or = inter

Back 79

>

Front 80

Hydrogen Bond

Back 80

special dipole dipole force NOF highly electronegativity
H- bonding increase in boiling point

Front 81

LDF London Dispersion Forces

Back 81

in all covalent bonds exists between nonpolar (noble gases too) molecules that involve an accidental dipole & momentary dipole - form because of nonsymmetry electron distribution

Front 82

Liquids have

Back 82

high density compared to gases

Front 83

Droplets-

Back 83

sphere minimizes the surface area. interior molecules surrounded by molecule surface molecules pulled to one side

Front 84

surface tension

Back 84

the resistence of a liquid to an increase in the surface area

Front 85

Capillary action

Back 85

- spontaneous rising of a liquid through a narrow tube

Front 86

adhesive force

Back 86

between water molecutes and side of container... concave u .... adhesive greater than conhesive polar

Front 87

conhesive force

Back 87

between water molecules cohesive greater than adhesive o convex non polar

Front 88

Heating curves

Back 88

q= mcΔt then
q2= ΔH x mols

Front 89

Phase Diagram

Back 89

Solid Liquid Gas. triple point
critcal point

Front 90

solid to gas

Back 90

sublimation

Front 91

gas to solid

Back 91

deposition

Front 92

solid to liquid

Back 92

melting

Front 93

liquid to solid

Back 93

freezing

Front 94

liquid to gas

Back 94

vaporization

Front 95

gas to liquid

Back 95

condensation

Front 96

molality

Back 96

moles solute / kg solvent

Front 97

normalty

Back 97

equivilalents number of h or oh x molarity

Front 98

like dissolves

Back 98

like

Front 99

Vitamin A

Back 99

fat soluble nonpolar

Front 100

Vitamin C

Back 100

water soluble polar

Front 101

Pressure affects solubiltiy

Back 101

effects gases

Front 102

Henry's Law

Back 102

the amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the solution C=KP

Front 103

Temperature affecting solubility

Back 103

dissolving a solid in a solvent is more rapid at higher temperatures
solubility of a gas decreased with higher temperatures

Front 104

Non volatile substances...

Back 104

lower vapor pressure of a solid .. decreases the number of solvent molecules per volume

Front 105

Raoult's Law

Back 105

P=XPs
x mol fraction of solvent
Ps solvent
P pressure

Front 106

Colligative Properties

Back 106

properties of a solution that depend on the number not on the identity of solute particles

Front 107

in a nonvolatile solute lowers the vapor pressure.. then

Back 107

the solution must be heated at a higher temperaure

Front 108

When you add a substance pressure _____ and the boiling point ____

Back 108

decreases; increases

Front 109

ΔT= KbMsolutei

Back 109

Kb constant
M molality of a solute
i van hoff

Front 110

Half Life-

Back 110

time it takes for half of a material to decay

Front 111

Alpha Decay

Back 111

4/2 He

Front 112

Beta

Back 112

electron 0/-1 e product side

Front 113

Electron Capture

Back 113

0/-1 e on reactant side

Front 114

positron emission

Back 114

0/1 e on product side