Chemistry 2000 - OverviewReview: Concepts from chem. 1000 important to chem. 2000

Chapter 13 - Intermolecular forces

Chapter 14 – Solutions and their behaviour

Dipole-dipole, dipole-induced dipole and london forces

Hydrogen bonding and surface tension

Properties of liquids: vapour pressure boiling points

Properties of Solids: melting points, crystallinity, types of solids

Concentration: Morality, molality, mole fraction and weight percent

Phase diagrams

Colligative properties: b.p. elevation, f.p depression and osmotic pressure

Chapter 22 Transition metals and Coordination Compounds

Lewis acids and Lewis bases

ligands (monodentate, bidentate, chelating)

co-ordination number

naming co-ordination complexes and complex salts

Chapter 15 – Chemical Kinetics

Chapter 16 – Chemical Equilibrium

Chemistry 2000

Rate constant, and rate equations

Zero-, first-, and second-order rate laws

Collision theory and Arrhenius law

Reaction co-ordinates, intermediates and transition states

Mechanisms, catalysts, rate determining steps

Dynamic equilibrium

Equilibrium Constants

Le Châtelier’s principle and reaction quotient

Problem solving

Chapter 17 – Acids and bases

Chapter 18 – Other aspects of aqueous equilibria

Chemistry 2000

Lewis, Brønsted and Arrhenius definition

Conjugate acid-base pairs, acid-base properties and reactions

Ionization constants- Ka, Kb, Kw – and thier expressions

pH, pOH, pKw, pKa and pKb

More problem solving

Titrations and Buffers

Solubility rules, Ksp and effects on solubility

Henderson-Hasselbach equation

Indicators

Equivalence point vs. end poin

Even more problem solving

Chapter 6 – Energy and chemical reactions

Chapter 19 – Entropy and Free energy

Chapter 20 – Electron transfer reactions

Chemistry 2000Energy, stability and chemical reactions

Exothermic vs. endothermic

System vs. surroundings – movement of heat - “thermodynamics”

Calorimetry

Enthalpy calculations

Laws of thermodynamics

Enthalpy, entropy, and Gibbs free energy

Gibbs free energy and equilibrium

Temperature and equilibrium constants

Oxidation states, half- reactions and balancing redox reactions

Voltaic cells, electrolytic cells (batteries) and cell potentials

Fuels cells and energy efficiency

Chemistry 1000 ReviewRelevant chemical concepts and related ideas Kotz 6th ed

Units and significant figures Ch 1

Atomic theory of matter; element symbols and names Ch 2

Writing chemical formulae; empirical, molecular, structural and condensed structural formulae

Ch3

Naming common molecular and ionic compounds Ch 3

Recognize common ions; ionic compounds and dissociation of ionic compounds in solution

Ch 3 & 5

Strong and weak electrolytes; basic solubility rules for ionic compounds Ch 5

Recognize common strong and weak acids and bases; acid dissociation; base dissociation

Ch 5

Classification of reactions; assigning oxidation states and recognizing oxidation reduction reactions

Ch 5

Stoichiometry: moles, balancing equations, limiting reagents, percent yield Ch 2 & 4

A basic understanding of periodicity and the underpinnings of atomic and molecular structure.

Ch 2 and 7-10

Molecular shape and molecular polarity Ch 9

Ideal gases; gas pressure ; gas stoichiometry; partial pressures; kinetic molecular theory

Ch12

Common Formulae from Chem 1000

mn

M

The mole

Density md

V

Ideal Gases

PV nRT T ii

P pi i Tp X P i

ii

i

nX

n

2

nP a V bn nRT

V

212E mv rms

3RTv

M

Kinetic Theory of gases

Waves

hcE h

c

h

mv h

x mv4

Quantum mechanics

2E mc

Nuclear Chemistry

22 2

22 2

1 1

1 1

final initialfinal initial

final initial

E E E RhcZn n

Ry Zn n

o

Nln k t

N

1/ 2

0.693t

k

Wavefunctions of H

Hydrogen Orbitals

Radial Probability Density Plot

P Orbitals

D Orbitals

F Orbitals

The Orbitals of the Hydrogen Atom

0 nodes

1 node

2 nodes

Radial nodes

1 planar node 2 planar nodes

Atoms with more than one electron

Aufbau order and Energy Levels

Traditional aufbau sequence diagram

1.008

H 1

2

13

14

15

16

17

4.003

He 2

6.939

Li 3

9.012

Be 4

10.811

B 5

12.011

C 6

14.007

N 7

15.999

O 8

18.998

F 9

20.183

Ne 10

22.990

Na 11

24.312

Mg 12

3

4

5

6

7

8

9

10

11

12

26.982

Al 13

28.086

Si 14

30.974

P 15

32.064

S 16

35.453

Cl 17

39.948

Ar 18

39.102

K 19

40.08

Ca 20

44.956

Sc 21

47.90

Ti 22

50.942

V 23

51.996

Cr 24

54.938

Mn 25

55.847

Fe 26

58.933

Co 27

58.71

Ni 28

63.546

Cu 29

65.37

Zn 30

69.72

Ga 31

72.59

Ge 32

74.922

As 33

78.96

Se 34

79.904

Br 35

83.80

Kr 36

85.47

Rb 37

87.62

Sr 38

88.905

Y 39

91.22

Zr 40

92.906

Nb 41

95.94

Mo 42

(98)

Tc 43

101.07

Ru 44

102.90

Rh 45

106.4

Pd 46

107.87

Ag 47

112.40

Cd 48

114.82

In 49

118.69

Sn 50

121.75

Sb 51

127.60

Te 52

126.90

I 53

131.30

Xe 54

132.91

Cs 55

137.33

Ba 56

138.91

La 57

178.49

Hf 72

180.95

Ta 73

183.85

W 74

186.21

Re 75

190.22

Os 76

192.2

Ir 77

195.09

Pt 78

196.97

Au 79

200.59

Hg 80

204.38

Tl 81

207.19

Pb 82

208.98

Bi 83

(209)

Po 84

(210)

At 85

(222)

Rn 86

(223)

Fr 87

226.025

Ra 88

227.029

Ac 89

(261)

Rf 104

(262)

Ha 105

(263)

Sg 106

(262)

Ns 107

(265)

Hs 108

(266)

Mt 109

new 110

new 111

140.12

Ce 58

140.91

Pr 59

144.24

Nd 60

(145)

Pm 61

150.36

Sm 62

151.97

Eu 63

157.25

Gd 64

158.93

Tb 65

162.50

Dy 66

164.93

Ho 67

167.26

Er 68

168.93

Tm 69

173.04

Yb 70

174.97

Lu 71

232.04

Th 90

231.04

Pa 91

238.03

U 92

237.05

Np 93

(244)

Pu 94

(243)

Am 95

(247)

Cm 96

(247)

Bk 97

(251)

Cf 98

(252)

Es 99

(257)

Fm 100

(258)

Md 101

(259)

No 102

(260)

Lr 103

s block

d block

p block

f block

Afbau sequence from Periodic Table

Electron Dot Structures

Bond polarity and electronegativity

F-Li+ F F

d

Pauling Electronegativity

General trend in element electronegativity

Lewis diagrams and Molecular Shape

The 5 Shape Families

General Shape Families AX2 & AX3

Shape Family AX4 Lone pairs and shape: 4 Electron Pairs

Linear

Hydrogen Fluoride, HF1 bond pair3 lone pairs

X

Shape Family AX5: Five Electron Pairs

Shape Family AX5: Five Electron Pairs

The AX6 Family :Six Electron Pairs

Special features of VSEPR

Geometry of Large Molecules

Shape and Polarity

Permanent Dipole Moments

Simple Molecular Orbitals

Energy Levels of LCAO-Molecular Orbitals

H2

He2

21MO configuration: ( )s

2 * 21 1MO configuration: ( ) ( )s s

LCAO From Atomic P Orbitals: σ-MO’s

LCAO From Atomic P Orbitals: π-MO’s

The complete energy level diagram

Li2 – bond order 1

Be2 - fills the σ2s* orbital, BO = 0

B2 - partially fills π2p levels, BO = 1

-2 e’s parallel i.e. paramagnetic

C2 - fills π2p, - BO = 2

- diamagnetic

O2 - partially fills π2p* levels, BO = 2

- paramagnetic

F2 - fills π2p* levels - BO = 1

Ne2 – fills σ2p*, BO = O, does not exist

N2 - fills σ2p - BO = 3 - diamangetic

Electron Configurations of diatomic molecules

BeH2 and sp Hybridization

unhybridzed2

2( )

p

sp

2

2

p

s

Be 2 H

sp hybrids

1s 1s

2 Be-H bonds

2 Be-H "antibonds"

2px 2py 2px 2py

BH3 and sp2 Hybridization

unhybridzed

2

2

2( )

p

sp

2

2

p

s

B 3 H

sp2 hybrids1s 1s 1s

3 B-H bonds

3 B-H "antibonds"

2py 2py

CH4 and sp3 Hybridization

no unhybridzed orbitals in 2nd shell

3

2( )sp

2

2

p

s

C 4 H

sp3 hybrids1s 1s 1s 1s

4 C-H bonds

4 C-H "antibonds"

H2O and sp3 Hybridization

no unhybridzed orbitals in 2nd shell

3

2( )sp

2

2

p

s

O 2 H

sp3 hybrids1s 1s

2 C-H

2 LP’s

Bonding in Large Molecules

sp3

sp3

sp3

sp3

sp3

sp2

sp2

Chapter 22

Transition Metal Coordination Compounds

FeOO

O

O

O

O

C

C

C

C

O

O

O

O

O

O

C

C

K3 + 3 H2O

Synthesis and Analysis of an Iron Complex

1 18

1.0079

H 1

2

13

14

15

16

17

4.0026

He 2

6.941

Li 3

9.0122

Be 4

10.811

B 5

12.011

C 6

14.0067

N 7

15.9994

O 8

18.9984

F 9

20.1797

Ne 10

22.9898

Na 11

24.3050

Mg 12

3

4

5

6

7

8

9

10

11

12

26.9815

Al 13

28.0855

Si 14

30.9738

P 15

32.066

S 16

35.4527

Cl 17

39.948

Ar 18

39.0983

K 19

40.078

Ca 20

44.9559

Sc 21

47.88

Ti 22

50.9415

V 23

51.9961

Cr 24

54.9380

Mn 25

55.847

Fe 26

58.9332

Co 27

58.693

Ni 28

63.546

Cu 29

65.39

Zn 30

69.723

Ga 31

72.61

Ge 32

74.9216

As 33

78.96

Se 34

79.904

Br 35

83.80

Kr 36

85.4678

Rb 37

87.62

Sr 38

88.9059

Y 39

91.224

Zr 40

92.9064

Nb 41

95.94

Mo 42

(98)

Tc 43

101.07

Ru 44

102.906

Rh 45

106.42

Pd 46

107.868

Ag 47

112.411

Cd 48

114.82

In 49

118.710

Sn 50

121.757

Sb 51

127.60

Te 52

126.905

I 53

131.29

Xe 54

132.905

Cs 55

137.327

Ba 56

La-Lu

178.49

Hf 72

180.948

Ta 73

183.85

W 74

186.207

Re 75

190.2

Os 76

192.22

Ir 77

195.08

Pt 78

196.967

Au 79

200.59

Hg 80

204.383

Tl 81

207.19

Pb 82

208.980

Bi 83

(210)

Po 84

(210)

At 85

(222)

Rn 86

(223)

Fr 87

226.025

Ra 88

Ac-Lr

(261)

Rf 104

(262)

Db 105

(263)

Sg 106

(262)

Bh 107

(265)

Hs 108

(266)

Mt 109

(281)

Dt 110

138.906

La 57

140.115

Ce 58

140.908

Pr 59

144.24

Nd 60

(145)

Pm 61

150.36

Sm 62

151.965

Eu 63

157.25

Gd 64

158.925

Tb 65

162.50

Dy 66

164.930

Ho 67

167.26

Er 68

168.934

Tm 69

173.04

Yb 70

174.967

Lu 71

227.028

Ac 89

232.038

Th 90

231.036

Pa 91

238.029

U 92

237.048

Np 93

(240)

Pu 94

(243)

Am 95

(247)

Cm 96

(247)

Bk 97

(251)

Cf 98

(252)

Es 99

(257)

Fm 100

(258)

Md 101

(259)

No 102

(260)

Lr 103

The Transition Metals

Variable Oxidation States

CuH2O

OH2

OH2

OH2

CuH3N

NH3

NH3

NH3

FeOH2

H2O

H2O

OH2

OH2

OH2

FeOO

O

O

O

O

C

C

C

C

O

O

O

O

O

O

C

C

2+ 2+ 3+

3-

Perspective line drawings of some coordination complexes encountered in Chemistry 2000

Chelating Ligands

Six-Coordinate Metals Complexed byThree Bidentate Ligands

Electronic Structure and Colour of Transition Metal Coordination Compounds

D orbitals in an octahedral ligand field

Origin of Colour

Spectrophotometer

Lewis acids and Lewis bases

ligands (monodentate, bidentate, chelating)

co-ordination number

naming co-ordination complexes and complex salts

electron configurations of cations

d electrons and crystal field splitting

why co-ordination complexes are often coloured

spectrophotometry (especially for labs!)

Important Concepts from Chapter 22