Inorganic Spectoscopy-UV-Vis
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Transcript of Inorganic Spectoscopy-UV-Vis
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UV-visible spectroscopyUV-visible spectroscopy
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the Period 4 transition metals
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Colors of representative compounds of the Period 4 transition metals
titanium oxide
sodium chromate
potassium ferricyanide
nickel(II ) nitrate hexahydrate
zinc sulfate heptahydrate
scandium oxide
vanadyl sulfate dihydrate
manganese(II ) chloride
tetrahydrate cobalt(II ) chloride
hexahydrate
copper(II ) sulfate
pentahydrate
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Aqueous oxoanions of transition elements
Mn(II) Mn(VI) Mn(VII)
One of the most characteristic chemical properties of these elements is the occurrence of multiple oxidation states.
Mn(II) Mn(VI) Mn(VII)
V(V)Cr(VI)
Mn(VII)
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Effects of the metal oxidation state and of ligand identity on color
[V(H2O)6]2+ [V(H2O)6]3+
[Cr(NH3)6]3+ [Cr(NH3)5Cl ]2+
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Linkage isomers
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Complementary colour
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The five d-orbitals in an octahedral field of ligands
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Splitting of d-orbital energies by an octahedral field of ligands
∆ is the splitting energy
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The effect of ligand on splitting energy
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Electronic Spectroscopy of Transition Metal Complexes
Chemistry 412 Experiment 1
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What is electronic spectroscopy?
Absorption
Absorption of radiation leading to electronic transitions within a molecule or complex
Absorption[Ru(bpy)3]2+ [Ni(H2O)6]2+
10104
UV = higher energy transitions - between ligand orbitals
visible = lower energy transitions - between d-orbitals of transition metals
- between metal and ligand orbitals
UV
400
λ / nm (wavelength)
200 700
visible
~14 000 50 00025 000
UVvisible
ν / cm-1 (frequency)−
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Absorption maxima in a visible spectrum have three important characteristics
1. number (how many there are)
This depends on the electron configuration of the metal centre
2. position (what wavelength/energy)
This depends on the ligand field splitting parameter, ∆oct or ∆tet and on the degree This depends on the ligand field splitting parameter, ∆oct or ∆tet and on the degree
of inter-electron repulsion
3. intensity
This depends on the "allowedness" of the transitions which is described by two
selection rules
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Selection Rules
In electronic spectroscopy there are three selection rules which determine whether or not transitions are formally allowed:
1. Spin selection rule: ∆S = 0
allowed transitions: singlet → singlet or triplet → tripletforbidden transitions: singlet → triplet or triplet → singlet
Changes in spin multiplicity are forbiddenChanges in spin multiplicity are forbidden
Singlet state: All electrons in the molecule are spin-pairedTriplet state: One set of electron spins is unpaired Usama El-Ayaan
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Selection rules
2. Laporte selection rule: there must be a change in the parity (symmetry) of the complex
Laporte-allowed transitions: g → uLaporte-forbidden transitions: g → g or u → u
Transition metal complexes get around this rule through M-L vibrations, which temporarily removes the center of symmetry
g stands for gerade – compound with a center of symmetryu stands for ungerade – compound without a center of symmetry
3. Selection rule of ∆ℓ = ± 1 (ℓ is the azimuthal or orbital quantum number, where ℓ = 0 (s orbital), 1 (p orbital), 2 (d orbital), etc.)
allowed transitions: s → p, p → d, d → f, etc.forbidden transitions: s → s, d → d, p → f, etc.
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Energy of transitions
molecular rotationslower energy (0.01 - 1 kJ mol-1)microwave radiation
electron transitionshigher energy (100 - 104 kJ mol-1)visible and UV radiation
Ground State
Excited State
molecular vibrationsmedium energy (1 - 120 kJ mol-1)IR radiation
During an electronic transition
the complex absorbs energy
electrons change orbital
the complex changes energy stateUsama El-Ayaan
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[Ti(OH2)6]3+ = d1 ion, octahedral complex
white light400-800 nm
blue: 400-490 nm
yellow-green: 490-580 nm
red: 580-700 nm
3+
Ti
Absorption of light
A
λ / nm
This complex has a light purple colour in
solution because it absorbs green light
λmax = 510 nmUsama El-Ayaan
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eg
t2g
∆o
hν
The energy of the absorption by [Ti(OH2)6]3+ is the ligand-field splitting, ∆o
GS
ES
GS
ES
eg
t2g
d-d transition
[Ti(OH2)6]3+ λmax = 510 nm ∆o is ∴ 243 kJ mol-1
20 300 cm-1
An electron changes orbital; the ion changes energy state
complex in electronic Ground State (GS)
complex in electronic excited state (ES)
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Electron-electron repulsiond2 ion
eg
t2g
xy xz yz
z2 x2-y2eg
t2g
xy xz yz
z2 x2-y2
xz + z2 xy + z2xz + z2 xy + z2
lobes overlap, large electron repulsion lobes far apart, small electron repulsion
x
z
x
z
yy
These two electron configurations do not have the same energyUsama El-Ayaan
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Deriving term symbols in a free ion
- an electron is completely defined by 4 quantum numbers
n = 1,2,3… (energy and distance from the nucleus ie. what shell)
Electron configurations of the same energy are collected together into terms
l = 0, 1, 2…orbital angular momentum (what sort {shape} of orbital, s, p, d…)
ml = -l…+l component of l (what kind of orbital, eg. for d: xy, xz…)
ms = spin angular momentum (contribution from unpaired electrons, spin 1/2)
- an ion can be defined using ionic quantum numbers made up of contributions
from all the electrons in the ion…..
..…these define the whole ionUsama El-Ayaan
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Russel Saunders Coupling
L = 0, 1, 2…total orbital angular momentum (term)
ML = -L…+L component of L (ML = Σ ml)
S = total spin quantum number (S = Σ s)
Ionic quantum numbers:
Each electronic state has its own term symbol
2S+1
Lspin multiplicity L = 0 S term
L = 1 P termL = 2 D termL = 3 F term
Within each term, there can be several degenerate microstates with different ML and MS
Ms = -S….+S component of S (MS = Σ ms)
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Microstates e.g. for a free d2 ion
10 ways of arranging 2 electrons in 5 degenerate d-orbitals (Hund's rules apply)
etc
low repulsion (7 microstates) high repulsion (3 microstates)
xy + z2 xy + xz x2-y2 + z2 xz + z2
xy + yz x2-y2 + yz yz + z2
xz + yz x2-y2 + xz xy + x2-y2
2S+1
Lspin multiplicity
orbital angular momentum
xz + yz x -y + xz xy + x -y
ML = -3, -2, -1, 0, 1, 2, 3 ML = -1, 0, 1
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low repulsion (7 microstates) high repulsion (3 microstates)
ML = ∑ ml
For d-orbitals ml = -2 -1 0 1 2
x2-y2 yz z2 xz xy
For ML = -3….3 L = 3 F term
For ML = -1….1 L = 1 P term
xy + z2 xy + xz x2-y2 + z2 xz + z2
xy + yz x2-y2 + yz yz + z2
xz + yz x2-y2 + xz xy + x2-y2
ML = -3, -2, -1, 0, 1, 2, 3 ML = -1, 0, 1
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For a free d2 ion with two parallel spins there are two terms
Total spin S = no. of electrons x spin on an electron2 x 1/2 ∴ S = 1
Spin multiplicity = (2S + 1) = 3
2S+1
L F and P?
For a free d2 ion with two parallel spins there are two terms
3F 3Plow energy high energy
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3P
3F
∆ E
∆ E = 15 B
States of the same spin multiplicity
Which is the Ground State?
B is the Racah parameter and is a measure of inter-electron repulsion
within the whole ion
Relative strength of coupling interactions:
MS = Σ ms > ML = Σ ml > ML - MSUsama El-Ayaan
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1. States with the highest spin multiplicity (2S+1) will be lowest in energy
(S = no. of e- x spin 1/2)
e.g. for a d5 ion 6S < 4G
Deriving the Ground State Term (Hund's rules)
2. Of two states with the same S, the one with higher L is of lower energy2. Of two states with the same S, the one with higher L is of lower energy
L = 0, S term; L = 1, P term; L = 2, D term; L = 3, F term
e.g. for a d2 ion 3F < 3P
These rules are only applicable to the ground state
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What are the ground state terms for the configurations p2 and d2?
p2: 1D 3P 1S
The ground state must be 3P because this has the largest spin multiplicity
d2: 1G 3F 1D 3P 1S
The ground state is either 3F or 3P because these have the largest spin multiplicity
Of the two, 3F must be the ground state because it has the largest value of L
(when L = 2, P term; when L = 3, F term)
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Ground States in free ions
d4 -2 -1 0 1 25D
ML = -2…2 L = 2 D term
MS = 4/2 2S+1 = 5
d3 -2 -1 0 1 24F
ML = -3…3 L = 3 F term
MS = 3/2 2S+1 = 4
d5 -2 -1 0 1 26S
ML = 0 L = 0 S term
MS = 5/2 2S+1 = 6
d6 -2 -1 0 1 25D
ML = -2….2 L = 2 D term
MS = 2 2S+1 = 5Usama El-Ayaan
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Ground States in free ions
d7 -2 -1 0 1 24F
d8 -2 -1 0 1 2
ML = -3….3 L = 3 F term
MS = 3/2 2S+1 = 4
d8 -2 -1 0 1 23F
d9 -2 -1 0 1 22D
ML = -3….3 L = 3 F term
MS = 2/2 2S+1 = 3
ML = -2…2 L = 2 D term
MS = 1/2 2S+1 = 2Usama El-Ayaan
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Ground State Terms for all electron configurations
Ground State
d1 d9 2D
d2 d8 3F 3P
d3 d7 4F 4P
d4 d6 5D
d5 6Sd5 6S
d-d transitions in high spin complexes
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2Eg
Effect of a crystal field on the free ion term of a d1 complex
tetrahedral field free ion octahedral field
d1 ≅≅≅≅ d6
2T2g
2T2
2E
6 Dq
4 Dq
2D
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∆∆∆∆
2Eg
2D
Energy
Energy level diagram for d1 ions in an Oh field
2T2g
2D
ligand field strength, ∆oct
For d6 ions in an Oh field, the splitting is the same, but the multiplicity of the states is 5,
ie 5Eg and 5T2gUsama El-Ayaan
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A
ν / cm-1-
30 00020 00010 000
d1 oct [Ti(OH2)6]3+
Orgel diagram for d1, d4, d6, d9
2Eg �2T2g
2Eg
2T2g
2D∆∆∆∆
E
LF strength
Orgel diagram for d , d , d , d
0 ∆∆
D
d4, d9 tetrahedral
T2g or T2
T2g or T2
d4, d9 octahedral
Eg or E
d1, d6 tetrahedral
Eg or E
d1, d6 octahedral
∆∆∆∆
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The Jahn-Teller Distortion: Any non-linear molecule in a degenerate electronic state
will undergo distortion to lower it's symmetry and lift the degeneracy
d3 4A2gd5 (high spin) 6A1gd6 (low spin) 1A1gd8 3A2g
Degenerate electronic ground state: T or E
Non-degenerate ground state: A
A
ν / cm-1-30 00020 00010 000
[Ti(H2O)6]3+, d1
2T2g
2Eg
2B1g
2A1g
Usama El-Ayaan
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Racah Parameters
d7 tetrahedral complex
15 B' = 10 900 cm-1
B' = 727 cm-1
[CoCl4]2-[Co(H2O)6]2+
d7 octahedral complex
15 B' = 13 800 cm-1
B' = 920 cm-1
Free ion [Co2+]: B = 971 cm-1
B' = 0.95B
B' = 0.75B
Nephelauxetic ratio, ββββ
ββββ is a measure of the decrease in electron-electron repulsion on complexationUsama El-Ayaan
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- some covalency in M-L bonds – M and L share electrons
-effective size of metal orbitals increases
-electron-electron repulsion decreases
cloud expandingThe Nephelauxetic Effect
Nephelauxetic series of ligands
F- < H2O < NH3 < en < [oxalate]2- < [NCS]- < Cl- < Br- < I-
Nephelauxetic series of metal ions
Mn(II) < Ni(II) Co(II) < Mo(II) > Re (IV) < Fe(III) < Ir(III) < Co(III) < Mn(IV)
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Selection Rules
Transition εεεε complexes
Spin forbidden 10-3 – 1 Many d5 Oh cxsLaporte forbidden [Mn(OH2)6]2+
Spin allowedLaporte forbidden 1 – 10 Many Oh cxs
[Ni(OH2)6]2+
10 – 100 Some square planar cxs[PdCl ]2-[PdCl4]2-
100 – 1000 6-coordinate complexes of low symmetry, many square planar cxs particularly with organic ligands
Spin allowed 102 – 103 Some MLCT bands in cxs with unsaturated ligandsLaporte allowed
102 – 104 Acentric complexes with ligands such as acac, or with P donor atoms
103 – 106 Many CT bands, transitions in organic speciesUsama El-Ayaan
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eg
t 2g
eg
t 2g
I- < Br- < S2- < SCN- < Cl-< NO3- < F- < OH- < ox2-
< H2O < NCS- < CH3CN < NH3 < en < bpy
< phen < NO2- < phosph < CN- < CO
The Spectrochemical Series
∆ ∆
weak field ligands
e.g. H2O
high spin complexes
strong field ligands
e.g. CN-
low spin complexes
The Spin Transition
Usama El-Ayaan
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Tanabe-Sugano diagrams
E/B
2T2g
4A1g, 4E
4T2g
4T1g
2A1g
4T2g
2Eg
2T1g
2A1g
4EgAll terms included
Ground state assigned to E = 0
Higher levels drawn relative to GS
Energy in terms of B
High-spin and low-spin configurations
d5
∆/B
4T2g
4T1g
2T2g
6A1g
Eg
4A2g, 2T1g Critical value of ∆
WEAK FIELD STRONG FIELDUsama El-Ayaan
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Tanabe-Sugano diagram for d2 ions
E/B
[V(H2O)6]3+: Three spin allowed transitions
νννν1 = 17 800 cm-1 visible
νννν2 = 25 700 cm-1 visible
νννν = obscured by CT transition in UV
10 000
ε
30 000ν / cm-1−
10
20 000
5
∆/B
νννν3 = obscured by CT transition in UV
25 700 = 1.44
17 800
∆/B = 32
νννν3 = 2.1νννν1 = 2.1 x 17 800
∴ νννν3 = 37 000 cm-1
= 32 Usama El-Ayaan
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E/B
νννν1 = 17 800 cm-1
νννν2 = 25 700 cm-1
νννν1
νννν2E/B = 43 cm-1
E/B = 30 cm-1
∆/B = 32
νννν1E/B = 30 cm-1
E/B = 43 cm-1 E = 25 700 cm-1
B = 600 cm-1
∆o / B = 32
∆o = 19 200 cm-1
Usama El-Ayaan
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Tanabe-Sugano diagram for d3 ions
E/B
[Cr(H2O)6]3+: Three spin allowed transitionsνννν1 = 17 400 cm-1 visible
νννν2 = 24 500 cm-1 visible
νννν3 = obscured by CT transition
24 500 = 1.41
17 400
∆/B = 24
∆/B
νννν3 = 2.1νννν1 = 2.1 x 17 400
∴ νννν3 = 36 500 cm-1
= 24 Usama El-Ayaan
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Calculating ν3
E/B
νννν1 = 17 400 cm-1
νννν2 = 24 500 cm-1
When νννν1 = E =17 400 cm-1
E/B = 24
so B = 725 cm-1
When νννν2 = E =24 500 cm-1
E/B = 34
∆/B = 24
E/B = 34 cm-1
E/B = 24 cm-1
E/B = 34
so B = 725 cm-1
If ∆/B = 24
∆ = 24 x 725 = 17 400 cm-1
Usama El-Ayaan
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TiF4 d0 ion
TiCl4 d0 ion
TiBr4 d0 ion
TiI4 d0 ion
d0 and d10 ion have no d-d transitions
Zn2+ d10 ion
d0 and d10 ions
white
white
orange
dark brown
white
[MnO4]- Mn(VII) d0 ion
[Cr2O7]- Cr(VI) d0 ion
[Cu(MeCN)4]+ Cu(I) d10 ion
[Cu(phen)2]+ Cu(I) d10 ion
extremely purple
bright orange
colourless
dark orange
Charge Transfer TransitionsUsama El-Ayaan
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Charge Transfer Transitions
Ligand-to-metal charge transfer
LMCT transitions
Metal-to-ligand charge transfer
MLCT transitions
Lπ∗
t *
eg*
d-d transitions
MdLπ
Lσ
t2g*
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Transition Metals, Compounds and Complexesor
Electronic Spectroscopy of Transition Metal Complexes
Dr. E.R. Schofield
Lecture 3: Interpretation of weak field spectraLecture 3: Interpretation of weak field spectra
Electronic spectra from Orgel diagrams
Orgel diagram for d2, d3, d7, d8 ions
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Energy
d1 ≡≡≡≡ d6 d4 ≡≡≡≡ d9
Orgel diagram for d1, d4, d6, d9
D
or E
T2g or T2
Eg
ligand field strength
0 ∆∆d4, d9 tetrahedral
or T2
Eg or
d4, d9 octahedral
E
d1, d6 tetrahedral
T2g
d1, d6 octahedral
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A
ν / cm-1-
30 00020 00010 000
d1 oct [Ti(OH2)6]3+
Orgel diagram for d1, d4, d6, d9
2Eg �2T2g
2Eg
2T2g
2D∆∆∆∆
E
LF strength
Orgel diagram for d , d , d , d
0 ∆∆
D
d4, d9 tetrahedral
T2g or T2
T2g or T2
d4, d9 octahedral
Eg or E
d1, d6 tetrahedral
Eg or E
d1, d6 octahedral
∆∆∆∆
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Effect of a ligand field on Ground State Terms
GS
d1 d9 2D
d2 d8 3F 3P
d3 d7 4F 4P
d4 d6 5D
d5 6S
D T2(g) and E(g)
free ion ligand field
d S
GS
d1 d9 2D
d2 d8 3F 3P
d3 d7 4F 4P
d4 d6 5D
d5 6S
P
F
free ion ligand field
?
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Octahedral d2 complex
3P: high repulsion
In a LF, these orbitals are unaffected
3F: low repulsion
In a LF, orbitals in the t2g set go down in energy, orbitals in the eg set go up in energy
xz + z2
yz + z2
xy + x2-y2
3T1g
d2 ≅≅≅≅ d7
x2-y2 + z2
x2-y2 + yzx2-y2 + xzxy + z2
xy + xzxy + yzxz + yz
3A2g
3T2g
3T1g
eg eg singly degenerate, high energy
eg t2g triply degenerate, medium energy
t2g t2g triply degenerate, low energy
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Octahedral d3 complex
4P: high repulsion
In a LF, these orbitals are unaffected � 4T1g
4F: low repulsion
The order of energy levels is the opposite to that for a d2 ion �
d3 ≅≅≅≅ d8(same terms, different spin)
The order of energy levels is the opposite to that for a d2 ion �
4T1g
4T2g
4A2g
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Energy
Orgel diagram for d2, d3, d7, d8 ionsQuantum Mixing
F
PT1 or T1g
T1 or T1g
A2 or A2g
T1 or T1gT2 or T2g
Ligand field strength (Dq)
d2, d7 tetrahedral d2, d7 octahedral
d3, d8 octahedral d3, d8 tetrahedral
0
T2 or T2g
A2 or A2g
T1 or T1g
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P
Energy level diagram for oct d2, d7, tet d3, d8
15 B'15 B
15 B > 15 B'
x
10 Dq
T1(g)
A2(g)
F
x
10 Dq
6 Dq
2 Dq
T1(g)
T2(g)
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Calculating B' and x d7 octahedral complex
4A2g
4T1g
10 Dq
x
15 B'
A
[Co(H2O)6]2+
νννν2
νννν3
25 000 20 000 15 000 10 000
νννν1νννν2
νννν3
v / cm-1
4T1g
4T2g
6 Dq
2 Dq
x
νννν1
25 000 20 000 15 000 10 000
νννν1 = 8 000 cm-1
νννν2 = 16 000 cm-1
νννν3 = 19 400 cm-1
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F
P
Energy
Orgel diagram for d2, d3, d7, d8 ions
A2 or A2g
T1 or T1gT2 or T2g
T1 or T1gT1 or T1g
Ligand field strength (Dq)
d2, d7 tetrahedral d2, d7 octahedral
d3, d8 octahedral d3, d8 tetrahedral
0
T2 or T2g
A2 or A2g
T1 or T1g
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Px 10 Dq
T1(g)
A2(g)
Energy level diagram for oct d2, d7, tet d3, d8νννν1: x + 8 Dq
νννν2: 2 x + 6 Dq + 15 B'
νννν3: x + 18 Dq
νννν2
νννν3
νννν1: T2(g) � T1(g)
νννν2: T1(g)(P) � T1(g)
νννν3: A2(g) � T1(g)
F
15 B'15 B
x
6 Dq
2 Dq
T1(g)
T2(g)
νννν1
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Transition Metal Complexes
Housecroft and Sharpe, p. 20
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Metal d orbitals – octahedral metal complexes
M = metal
L = ligand
Housecroft and Sharpe, p. 453
t2g orbitals – point between the ligands – π symmetry
eg orbitals – point at the ligands – σ symmetry
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UV-visible spectra of transition metal complexes
Transition metal complexes commonly exhibit UV-visible spectra containing both weak “d-d” (ε < 100) and strong “charge-transfer” (ε > 1000) bands which are characteristic of the nature of both the metal and the ligand(s)of both the metal and the ligand(s)
Shriver, Langford & Atkins (2nd ed), p. 582Usama El-Ayaan
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Selection Rules
In electronic spectroscopy there are three selection rules which determine whether or not transitions are formally allowed:
1. Spin selection rule: ∆S = 0
allowed transitions: singlet → singlet or triplet → tripletforbidden transitions: singlet → triplet or triplet → singletforbidden transitions: singlet → triplet or triplet → singlet
Changes in spin multiplicity are forbidden
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Selection rules
2. Laporte selection rule: there must be a change in the parity (symmetry) of the complex
Laporte-allowed transitions: g → uLaporte-forbidden transitions: g → g or u → u
Transition metal complexes get around this rule through M-L vibrations, which temporarily removes the center of symmetry
g stands for gerade – compound with a center of symmetryu stands for ungerade – compound without a center of symmetry
3. Selection rule of ∆ℓ = ± 1 (ℓ is the azimuthal or orbital quantum number, where ℓ = 0 (s orbital), 1 (p orbital), 2 (d orbital), etc.)
allowed transitions: s → p, p → d, d → f, etc.forbidden transitions: s → s, d → d, p → f, etc.
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Crystal field theory – d orbitals split into two sets
eg
t2g
Housecroft and Sharpe, p. 455
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Crystal Field Splitting
Housecroft and Sharpe, p. 456
To promote an electron from the lower d orbital to the higher d orbital requires energy equal to ∆oct, the “crystal field splitting energy”Usama El-Ayaan
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Spectrochemical Series
Spectrochemical Series (the effect of the ligand set on the magnitude of ∆o)
I- < Br- < Cl- < F- < O2- < OH- < H2O < NH3 < NO2- < CN- < PR3 < CO
σ-donor ligands
π-donor ligands increase the energy of the t2g orbitals
π-acceptor ligands decrease the energy of the t2g orbitals
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Visible spectra of octahedral Ni(II) complexes
[Ni(NH3)6]2+
1000 300 nm
[Ni(H2O)6]2+
Housecroft and Sharpe, p. 471
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Tanabe-Sugano diagrams
d3d2
excited
Shriver, Langford & Atkins
ground state
excited states
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UV-visible spectrum of a Chromium(III) complex
Spin-allowed transitions
Quartet → Quartet
Spin-forbidden transitions
Shriver, Langford & Atkins (2nd ed), p. 582
Spin-forbidden transitions
Quartet → Doublet
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d-d transitions in d3 metal complexes
For a d3 metal ion, such as Cr3+
there is one electron in each of the three t2g orbitals, while the eg orbitals are empty
eg
d3
Shriver, Langford & Atkins (2nd ed), p. 594
t2g
eg
t2g
eg
d-d transition
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Excitation of d electrons
y
z z
y
Electron goes from the dxyorbital into a
Electron goes from the dxzorbital into a d orbital
Shriver, Langford & Atkins (2nd ed), p. 590
x x
dz2 orbital
*requires a change in planes (xy to z)
dz2 orbital
*much less relocation of the electron
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Tanabe-Sugano diagram – d2 ion
Tanabe-Sugano diagram for a d2
ion, such as V2+
3T1g → 3T2g
3T1g
3T1g(F) → 3T1g(P)
3T1g → 3A2g
Housecroft and Sharpe, p. 472
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Jahn-Teller distortions
e.g. [Ti(H2O)6]3+ d1 electronic configuration
When a set of degenerate orbitals are unevenly filled, then a perturbation of the molecular structure will occur so that the degeneracy is removed
eg
t2g
dz2
dxz, dyz
dxy
dx2-y2
ν1 ν2d
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[Ti(H2O)6]3+ visible spectrum
ν1ν2
500 400600
[Ti(H2O)6]3+
λ, nm
Housecroft and Sharpe, p. 456
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Visible spectrum of [Mn(H2O)6]2+ (1 M solution)
Mn(H2O)62+ is a “high-spin” d5 ion (t2g
3 eg2) and
therefore all d-d transitions are spin-forbidden
All of the transitions have ε values of << 1, (very weak)
Brisdon, p. Usama El-Ayaan
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Charge-Transfer
Ligand-to-Metal Charge Transfer
(LMCT)
Shriver, Langford & Atkins (2nd ed), p. 595
Metal-to-Ligand Charge Transfer
(MLCT)
Charge transfer bands are allowed transitions, with εvalues > 10,000
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Ligand-to-Metal Charge Transfer
• Occurs with metals in high oxidation states (few d electrons) complexed by ligands which are good electron-donors
O
MnO
O
O
Permanganate anion
Manganese(VII) has no d electrons, while the O2- (oxide) ligands donate lone pairs of electrons to form double bonds
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UV-Visible spectrum of MnO4-
Lπ → M(t2g)
Lπ → M(eg)
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Metal-to-Ligand Charge Transfer (MLCT)
• Occurs with metals in low oxidation states (lots of d electrons) complexed by ligands which are good electron-acceptors
Ruthenium(II) has 6 d e-
Housecroft and Sharpe, p. 208Ru(2,2’-bipyridine)3
2+
has 6 d e-
2,2’-bipyridine is a good π-acceptor ligand
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Visible spectrum of Ru(2,2’-bipyridine)32+
[Ru(bpy)3]2+ MLCT
λmax = 452 nm ε = 14,600 M-1 cm-1
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Coordination ChemistryElectronic Spectra of Metal ComplexesElectronic Spectra of Metal Complexes
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Electronic configurations of multi-electron atomsRussell-Saunders (or LS) coupling
For each 2p electronn = 1; l = 1
ml = -1, 0, +1ms = ± 1/2
For the multi-electron atomL = total orbital angular momentum quantum numberS= total spin angular momentum quantum number
Spin multiplicity = 2S+1
ML = ∑ml (-L,…0,…+L)ML = ∑ml (-L,…0,…+L)MS = ∑ms (S, S-1, …,0,…-S)
ML/MS define microstatesand L/S define states(collections of microstates)
Groups of microstates with the same energy are called terms
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before we did:
p2
ML & M S
MicrostateTable
States (S, P, D)Spin multiplicity
Terms3P, 1D, 1S
Ground state term3P
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For metal complexes we need to considerd1-d10
d2
3F, 3P, 1G, 1D, 1S
For 3 or more electrons, this is a long tedious process
But luckily this has been tabulated before…
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Transitions between electronic terms will give rise to spectra
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Selection rules(determine intensities)
Laporte rule
g → g forbidden (that is, d-d forbidden)
but g → u allowed (that is, d-p allowed)
Spin rule
Transitions between states of different multiplicities forbidden
Transitions between states of same multiplicities allowed
These rules are relaxed by molecular vibrations, and spin-orbit coupling
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Group theory analysis of term splitting
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High Spin Ground Statesdn Free ion GS Oct. complex Tet complex
d0 1S t2g0eg
0 e0t20
d1 2D t2g1eg
0 e1t20
d2 3F t2g2eg
0 e2t20
d3 4F t2g3eg
0 e2t21
d4 5D t2g3eg
1 e2t22
An e electron superimposed on a spherical
distribution energies reversed because
tetrahedral
d5 6S t2g3eg
2 e2t23
d6 5D t2g4eg
2 e3t23
d7 4F t2g5eg
2 e4t23
d8 3F t2g6eg
2 e4t24
d9 2D t2g6eg
3 e4t25
d10 1S t2g6eg
4 e4t26
Holes: dn = d10-n and neglecting spin dn = d5+n; same splitting but reversed energies because positive.
A t2 hole in d5, reversed energies,
reversed again relative to
octahedral since tet.
Holes in d5
and d10, reversingenergies relative to
d1
Expect oct d1 and d6 to behave same as tet d4 and d9
Expect oct d4 and d9 (holes), tet d1 and d6 to be reverse of oct d1Usama El-Ayaan
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Energy
d1 ≡≡≡≡ d6 d4 ≡≡≡≡ d9
Orgel diagram for d1, d4, d6, d9
D
or E
T2g or T2
Eg
ligand field strength
0 ∆∆d4, d9 tetrahedral
or T2
Eg or
d4, d9 octahedral
E
d1, d6 tetrahedral
T2g
d1, d6 octahedral
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F
P
Energy
Orgel diagram for d2, d3, d7, d8 ions
A2 or A2g
T1 or T1gT2 or T2g
T1 or T1gT1 or T1g
Ligand field strength (Dq)
d2, d7 tetrahedral d2, d7 octahedral
d3, d8 octahedral d3, d8 tetrahedral
0
T2 or T2g
A2 or A2g
T1 or T1g
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d2
3F, 3P, 1G, 1D, 1S
Real complexesUsama El-Ayaan
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Tanabe-Sugano diagrams
d2
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Electronic transitions and spectra
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Other configurations
d1 d9
d3
d2 d8
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Other configurations
d3
The limit betweenhigh spin and low spin
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Determining ∆o from spectra
d1d9
One transition allowed of energy ∆o
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mixing
Determining ∆o from spectra
Lowest energy transition = ∆o
mixing
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Ground statemixing
E (T1g→A2g) - E (T1g→T2g) = ∆o
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The d5 case
All possible transitions forbiddenVery weak signals, faint color
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Some examples of spectra
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Charge transfer spectra
LMCT
Ligand character
Metal character
MLCTMetal character
Ligand character
Much more intense bandsUsama El-Ayaan