Chem135 Final Exam Review

Front 1

Aluminum

Back 1

Al 3+

Front 2

Ammonium

Back 2

NH4+

Front 3

Barium

Back 3

Ba 2+

Front 4

Bismuth

Back 4

Bi 3+

Front 5

Calcium

Back 5

Ca 2+

Front 6

Cesium

Back 6

Cs+

Front 7

Chromium(II)

Back 7

Cr 2+

Front 8

Chromium(III)

Back 8

Cr 3+

Front 9

Cobalt

Back 9

Co 2+

Front 10

Copper(I)

Back 10

Cu+

Front 11

Copper(II)

Back 11

Cu 2+

Front 12

Hydrogen

Back 12

H+

Front 13

Hydronium

Back 13

H3O+

Front 14

Iron(II)

Back 14

Fe2+

Front 15

Iron(III)

Back 15

Fe 3+

Front 16

Lead(II)

Back 16

Pb 2+

Front 17

Lithium

Back 17

Li+

Front 18

Magnesium

Back 18

Mg2+

Front 19

Manganese

Back 19

Mn 2+

Front 20

Mercury(I)

Back 20

Hg2 2+

Front 21

Mercury(II)

Back 21

Hg 2+

Front 22

Nickel

Back 22

Ni 2+

Front 23

Potassium

Back 23

K+

Front 24

Rubidium

Back 24

Rb+

Front 25

Silver

Back 25

Ag+

Front 26

Sodium

Back 26

Na+

Front 27

Strontium

Back 27

Sr 2+

Front 28

Tin(II)

Back 28

Sn 2+

Front 29

Tin(IV)

Back 29

Sn 4+

Front 30

Zinc

Back 30

Zn 2+

Front 31

Acetate

Back 31

CH3CO2 -

Front 32

Arsenate

Back 32

AsO4 3-

Front 33

Bromide

Back 33

Br -

Front 34

Carbonate

Back 34

CO3 2-

Front 35

Hydrogen carbonate

Back 35

HCO3 -

Front 36

Chlorate

Back 36

ClO3 -

Front 37

Chloride

Back 37

Cl-

Front 38

Chlorite

Back 38

ClO2 -

Front 39

Chromate

Back 39

CrO4 2-

Front 40

Cyanide

Back 40

CN-

Front 41

Dichromate

Back 41

Cr2O7 2-

Front 42

Fluoride

Back 42

F-

Front 43

Hydroxide

Back 43

OH-

Front 44

Hypochlorite

Back 44

ClO-

Front 45

Iodide

Back 45

I-

Front 46

Nitrate

Back 46

NO3 -

Front 47

Nitride

Back 47

N 3-

Front 48

Nitrite

Back 48

NO2 -

Front 49

Oxalate

Back 49

C2O4 2-

Front 50

Oxide

Back 50

O 2-

Front 51

Perchlorate

Back 51

ClO4 -

Front 52

Permanganate

Back 52

MnO4 -

Front 53

Peroxide

Back 53

O2 2-

Front 54

Phosphate

Back 54

PO4 3-

Front 55

Monohydrogen Phosphate

Back 55

HPO4 2-

Front 56

Dihydrogen Phosphate

Back 56

H2PO4 -

Front 57

Sulfate

Back 57

SO4 2-

Front 58

Hydrogen sulfate

Back 58

HSO4 -

Front 59

Sulfide

Back 59

S2 -

Front 60

Hydrogen sulfide

Back 60

HS -

Front 61

Thiocyanate

Back 61

SCN-

Front 62

Thiosulfate

Back 62

S2O3 2-

Front 63

What was the experiment in which the electron was discovered because rays were deflected towards the positive side?

Back 63

Thomson's cathode ray experiment

Front 64

What was the experiment in which electrons were shown to be very light, electrons and protons are now known to exist, and alpha, beta, and gamma particles were revealed?

Back 64

Radioactive experiment

Front 65

What was the experiment that led to atomic theory and discovered that the atom is mostly empty space?

Back 65

Rutherford's gold foil experiment

Front 66

Natural abundance of isotopes

Back 66

Sum of: (fraction of naturally occurring n * mass of n) = atomic mass of element

Front 67

Nomenclature for naming ionic compoinds

Back 67

Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca

Front 68

Prefixes for carbon backbone nomenclature

Back 68

Meth
Eth
Prop
But
Pent
Hex
Hept
Oct
Non
Dec

Front 69

Priorities for nomenclature (high to low)

Back 69

Carboxylic acid
Ester
Amide
Aldehyde
Ketone
Alcohol
Amine
Hydrocarbon

Front 70

Hydrocarbon

Back 70

C and H only
-e

Front 71

Amine

Back 71

N w/only carbons or NH2, NH
-amine

Front 72

Alcohol

Back 72

-OH
-ol

Front 73

Ketone

Back 73

=O
-one

Front 74

Aldehyde

Back 74

-H and =O
-al

Front 75

Amide

Back 75

=O and N
-amide

Front 76

Ester

Back 76

=O and O
-oate

Front 77

Carboxylic acid

Back 77

=O and -OH
-oic acid

Front 78

Priorities for benzenes (high to low)

Back 78

Analine
Phenol
Anasole
Toluene
Chlorobenzene
Styrene
Benzoic acid
Nitrobenzene

Front 79

Analine

Back 79

NH2

Front 80

Phenol

Back 80

OH

Front 81

Anasole

Back 81

OCH3

Front 82

Toluene

Back 82

CH3

Front 83

Chlorobenzene

Back 83

Cl

Front 84

Styrene

Back 84

C=C

Front 85

Benzoic acid

Back 85

COOH

Front 86

Nitrobenzene

Back 86

NO2

Front 87

How do you name benzenes?

Back 87

1 carbon - parent
2nd carbon - ortho (o-)
3rd carbon - meta (m-)
4th carbon - para (p-)

Front 88

How to calculate enthalpy changes from the heating or cooling curve

Back 88

sloped part: q=m(kg)*Cs*deltaT = kJ
Hvap or Hfus: #mol*Hvap or Hfus (kJ/mol) = kJ

Front 89

Ideal gas law

Back 89

pv=nRT

Front 90

Substitutions possible in Ideal gas law

Back 90

n = (g/MM)
v = (g/d)

Front 91

Energy/wavelength equality

Back 91

E (J/photon) = hV = hc/T

T = wavelength in meters
V = frequency (1/sec or Hz)

Front 92

Rydberg's equation

Back 92

1/T = R(1/n^2 - 1/m^2)
n < m

Front 93

Balmer/Rydberg series

Back 93

shell 2

Front 94

Lyman series

Back 94

shell 1

Front 95

What is vanderwaals/dispersion forces?

Back 95

fluctuation of e- and temporary dipole (weakest!!!)

Front 96

What is dipole-dipole force?

Back 96

Always present: ex O=<
partial negative charge on O, partial positive charge on C.

Front 97

What is a hydrogen bond intermolecular force?

Back 97

F,O,N form them with H, and they are very strong

Front 98

When does the behavior of a gas become non-ideal?

Back 98

Low temperatures, high pressures because these cause attractive forces

Front 99

What does the wave-particle duality entail?

Back 99

Light is both waves and particles (photons)

Front 100

What is the photoelectric effect?

Back 100

Proves bundles of photons exist and that a certain amount of energy is required to knock out an electron; also shows that light is a particle.

Front 101

Does going OUT a shell take energy or release energy?

Back 101

Takes energy

Front 102

What is the quantum number n?

Back 102

The principle quantum number: denotes shell and distance from nucleus

Front 103

What is the quantum number l?

Back 103

The azimuthal quantum number: describes shape of orbital.
(0,1...(n-1))
0 = s
1 = p
2 = d
3 = f

Front 104

What is the quantum number ml?

Back 104

Magnetic quantum number
-l..0..+l
Describes orientation of orbital

Front 105

What is the quantum number ms?

Back 105

Spin
+/- 1/2

Front 106

What is z-effective?

Back 106

# protons - core electrons, so how much positive charge is felt by the outer electrons from the nucleus

Front 107

What is shielding?

Back 107

When core electrons shield outer electrons from the nucleus' charge

Front 108

What does the Aufbau principle say?

Back 108

Electrons fill lower energy orbitals first

Front 109

What does the Pauli exclusion principle say?

Back 109

Only two electrons will go per orbital and they will have opposite signs

Front 110

What does Hund's rule say?

Back 110

One electron will go in each orbital until orbitals are 1/2 filled

Front 111

Atomic radius increases...

Back 111

Down and Left

Front 112

Ionization energy increases

Back 112

Up and Right

Front 113

Electron affinity becomes more negative

Back 113

Up and Right

Front 114

When metals ionize, where do they lose electrons from first?

Back 114

Their outer shell (highest n value)

Front 115

Energy of photon*frequency = binding energy

Back 115

hV = O
h=Planck's constant
V = frequency (Hz)
O = binding energy (J)

Front 116

Core electrons

Back 116

# of electrons of previous noble gas; for group C elements add 10 to include transition metals

Front 117

Outer electrons

Back 117

Always number of electrons in the shell with the highest n value

Front 118

Valence electrons

Back 118

Number of electrons n the highest n value shell but add the d electrons in the orbital you're in the process of filling for transition metals

Front 119

Electronegativity

Back 119

FONClBr

Front 120

How to draw resonance hybrid

Back 120

Draw sigma bonds
Draw electrons common to all structures
Draw dotted bonds for where pi bonds could be
Partial charges

Front 121

Electron pair geometries

Back 121

2-Linear
3-Trigonal Planar
4-Tetrahedral
5-Trigonal bipyramidal
6-Octahedral

Front 122

Molecular geometries

Back 122

2-Trigonal Planar-Bent
4-Tetrahedral-Trigonal pyramidal-Bent
5-Trigonal bipyramidal-seesaw-T-shaped-Linear
6-Octahedral-Square pyramidal-square planar-T-shaped-Linear

Front 123

Combustion reaction format

Back 123

C,H,maybe O +O2 --> CO2 + H2O

Front 124

Arrhenius acid

Back 124

Produce H3O+ in solution

Front 125

Bronsted-Lowry acid

Back 125

Proton donor

Front 126

Lewis acid

Back 126

Electron pair acceptor

Front 127

Arrhenius base

Back 127

Produces OH- in aqueous solvent

Front 128

Bronsted-Lowry base

Back 128

Proton acceptor

Front 129

Lewis base

Back 129

Electron donor

Front 130

Conjugate acid/base

Back 130

The acid - H
The base + H

Front 131

What are the diatomic elements?

Back 131

BrINClHOF

Front 132

What happens in organic chemistry reactions of alkenes, alkynes, ketones, and aldehydes?

Back 132

The pi bond reacts to create two new sigma bonds

Front 133

Which o-chem reaction is it if it's a benzene?

Back 133

Substitution: substituted for H

Front 134

Which o-chem reaction involves an alkane, halide, and heat?

Back 134

Substitution

Front 135

Which o-chem reaction involves a strong acid or strong base as the solvent?

Back 135

Elimination (the reverse of addition)

Front 136

Which o-chem reaction involves alcohols -OH going to =O?

Back 136

Oxidizing

Front 137

Which o-chem reaction involves LiAl4, and =O going to -OH?

Back 137

Reduction

Front 138

Compounds of group I are

Back 138

soluble :)

Front 139

Compounds of nitrates are

Back 139

soluble :)

Front 140

Compounds of acetates are

Back 140

soluble :)

Front 141

Compounds of chlorates are

Back 141

soluble :)

Front 142

Compounds of the halogens with metals are

Back 142

soluble, EXCEPT:
Ag
Hg
I
Pb
(HALI)

Front 143

Compounds of sulfates are

Back 143

soluble, EXCEPT:
Ba2+
Sr2+
Ca2+
Pb2+
Ag+
Hg+

Front 144

Compounds of carbonates are

Back 144

insoluble :(

Front 145

compounds of hydroxides are

Back 145

insoluble :(

Front 146

compounds of oxides are

Back 146

insoluble :(

Front 147

compounds of silicates are

Back 147

insoluble :(

Front 148

Compounds of phosphates are

Back 148

insoluble :(

Front 149

Compounds of sulfides are

Back 149

insoluble, EXCEPT:
Ba2+
Sr2+
Ca2+
Mg
Na+
K+
NH4+

Front 150

Coffee cup calorimeter

Back 150

-q=m*Cs*deltaT

Front 151

Bomb calorimeter

Back 151

-q=C*deltaT(bomb) + m*Cs*deltaT(surr)

Front 152

How do you get Erxn per mole of a particular reactant?

Back 152

Divide qrxn by the number of moles that reacted

Front 153

Hess's Law

Back 153

Hrxn = Sum of Hfproducts*mol - Sum of Hfreactants*mol

Front 154

Reaction coordinate diagram Delta H?

Back 154

Delta H = Sum of bonds broken - Sum of bonds formed

Front 155

1st order rate law

Back 155

ln[A]t = -kt + ln[A]o

Front 156

2nd order rate law (integrated)

Back 156

1/[A]t = kt + 1/[A]o

Front 157

How do you know which step is the rate determining step?

Back 157

Smaller rate constant, greater activation energy

Front 158

What does a large K or a small K indicate?

Back 158

Large K: high concentration of products, low concentration of reactants

Small K: low concentration of products, high concentration of reactants

Front 159

What does it mean for a reaction to be in dynamic equilibrium?

Back 159

Rate of forward reaction = rate of reverse reaction

Front 160

What does Keq equal?

Back 160

[C]^c[D]^d/[A]^a[B]^b

Front 161

When do you negate x?

Back 161

When the k value is very small, or when the initial concentration divided by k is greater than 400?

Front 162

If Q<K

Back 162

Reaction goes to right

Front 163

If Q>K

Back 163

Reaction goes to left

Front 164

If Q=K

Back 164

Reaction is at equilibrium

Front 165

Strong acids

Back 165

HI
HBr
HCl
H2SO4
HNO3

Front 166

Strong bases

Back 166

LiOH
NaOH
KOH

Front 167

Ka = ?

Back 167

[H3O+][A-]/[HA]

Front 168

pH = ?

Back 168

-log[H3O+]

Front 169

pKa = ?

Back 169

-logKa

Front 170

Ka x Kb = ?

Back 170

Kw = 1x10^-14

Front 171

Reduction happens at the _____, oxidation happens at the ______

Back 171

cathode, anode

Front 172

Which half of the electrochemistry reaction will be the reduction half which is spontaneous?

Back 172

The half-reaction with a more + Ecell

Front 173

Ecell (entire redox) =

Back 173

E(1/2 cell cathode) - E(1/2 cell anode)

Front 174

Delta G =

Back 174

-nFEcell