chemistry 2000 - overview
DESCRIPTION
Chemistry 2000 - Overview. Review: Concepts from chem. 1000 important to chem. 2000. 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. - PowerPoint PPT PresentationTRANSCRIPT
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