the photo chemistry of ligand field is very important to have an idea for the intrinsic properties of different coordination compound, and the electronic properties such as, LMCT,LLCT, MLCH etc..........
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photo chemistry of ligand in coordination compound
1. Addis Ababa University
Department of Chemistry
PhD Program
Photochemistry of Ligand Field
Transition
presenter: Masresha Amare
Adviser: Prof V.J .T Raju
Dr. Yonas Chebude
2. Introduction
What is Photochemistry about?
concerned with the changes in chemical and
physical behaviour of molecules following
absorption of one (or more) photons
Primarily consider absorption of visible/UV
although IR absorption may also change chemical
behaviour
Mainly concerned with electronic excitation
3. Cont………
Electronic excitation
change of molecular orbital occupancy
increased energy
change of bonding characteristics and possibly geometry
change of charge distribution
possible changes of resultant electron spin, orbital
symmetry
4. Cont………….
AB*
Fates of photoexcited species
Physical quenching
AB
BA
Isomerization
A + B
Dissociation
AB+
+ e-
Ionization
Luminescence
AB + hν
AB + CD‡
Intermolecular
energy transfer
AB†
Intramolecular
energy transfer
(radiationless
transition)
AB + E or ABE
Direct reaction
AB⋅
+
+ E⋅
-
or AB⋅
-
+ E⋅
+
Charge transfer
+ M
+ CD
+ E
5. Electronic Transitions
Three types of electronic transitions may be
distinguished
transitions between MOs mainly localized on the
central metal.
the metal d orbitals (e.g., the t2g(π) and eg MOs
d–d transitions or ligand-field transitions
6. Cont…………
Octahedral complexes Cr(III)
ground state of these complexes,4
A2g, belongs
to the configuration t2g
3
.
Spin allowed 4
A2g(t2g
3
) → 4
T2g(t2g
2
eg1
) and
4
A2g → 4
T1g correspond to the promotion of an
electron from the t2g to eg orbitals.
9. Cont……….
Effect of T2g → eg
(1) an increase in the metal–ligand repulsion
some lengthening of metal-ligand distances
breaking of a metal-ligand bond
rearrangement of the molecule toward a
more-stable structure (isomerization
10. Cont…………..
(2) a decrease of electron density in some
directions between the ligands
Facilitate a nucleophilic attack on the central
metal by solvent molecules or other ligands
present in the solution (substitution reaction)
12. Cont…………
Transitions between MOs mainly localized on the
ligands and MOs mainly localized on the central
metal.
This transition are called CT or optical electron
transfer
LMCT or MLCT, transitions can occur.
13. Cont………..
Transitions between MOs mainly localized on
the ligands.
only involve ligand orbitals which are almost
unaffected by coordination to the metal
Transitions of such a type are called ‘ligand-
centered’ (LC) or ‘intra-ligand transitions.’
15. Absorption Bands
MC (Ligand-Field) Bands
Consider a d1
octahedral complex such as
[Ti (H2O)6]2+
.
all the orbitals lying below the t2g(π*) orbitals t2g
orbital are filed
the t2g(π*) orbitals contain one electron, the
eg(σ*) orbitals are empty
16. Cont………
the ground electronic configuration of a
d1
complex gives rise to only one state (2
T2g)
and the excited electronic configuration also
has one state (2
Eg)
only one d–d band may be present in the
spectrum of [Ti(H2O)6]3+
In a state diagram it Corresponds to the
2
T2g → 2
Egtransition
18. Cont………..
complexes containing more than one d-
electron, the situation is complicated by the
interelectronic repulsions
the ground-electronic configuration of a d2
(3
F)
octahedral complex give rises to the 3
T1g,3
T2g
3
A2g,
state (field free ion)
absorption bands could then arise from the
transitions3
T1g → 3
T2g, 3
T1g → 3
A2g, and
3
T1g → 3
T1g(P)
19. Cont………..
Therefore, three transitions correspond to the
t2g
2
→ eg
2
promotion (Transitions from the
ground state 3
T1g to each one of the excited
states described above are symmetry
forbidden )
a d2
system, such as [V(H2O)6]3+
only two
transition are allowed
3
T1g (t2g
2
) → 3
T2g(t2geg) and 3
T1g(t2g
2
)
→ 3
T1g(t2geg) (give bands of sufficient intensity
)
21. Charge-transfer bands
the movement of electrons between orbitals
that are predominantly ligand in character and
orbitals that are predominantly metal in
character
high intensity and the sensitivity of their
energies to solvent polarity.
electron migrates between orbitals that are
predominantly ligand in character and orbitals
that are predominantly metal in character
23. Cont………….
LMCT
observed in the visible region of the spectrum
when the metal is in a high oxidation state
and ligands contain nonbonding electrons.
In octahedral complex we may distinguish
four types of LMCT
πL → πM*(t2g), πL→σM*(eg) ,σL→ πM* t2g) and σL →
σM*(eg)
[IrCl6]2-
24. Cont………..
MLCT transitions
likely to happen in complexes with central
atoms having small ionization potentials and
ligands with easily available empty π*
ligands such as CN–
, CO, SCN–
etc
MLCT transitions will be favored when the
metal has a low oxidation state
bands in the visible range of [Ru(bpy)3]2+
due to
MLCT while [Ru(bpy)3]3+
is due to LMCT
25. Cont………
ion-pair charge-transfer
the ion pairs formed by a coordinatively
saturated complex cation and a polarizable
anion-like iodide .
ion-pair charge-transfer bands are due to
intermolecular CT transitions from the anion
to the antibonding d- orbitals of the central
metal.
26. Cont………..
The intensity of these bands depends on the
formation constant of the ion pair and on the
concentration of the two ions.
Intermolecular CT transitions of the inverse
type (i.e. from the complex to an outer
species) is called CTTS.
exhibited by some negative complex ions such
as [Fe(CN)6]4-
.
27. Cont…………
LLCT Or (Intra-Ligand) Bands
due to transitions between two MOs both of
which are principally localized on the ligand
system .
such bands may be found at relatively low
energy in complexes containing ligands which
have π-systems of their own
Aromatic Ligands such as bipyridine and
phenanthroline belong to this group
28. Effect of Solvent Polarity on CT Spectra
• only occurs if the species being studied is an
ion pair
• The position of the CT band is reported as a
transition energy and depends on the
solvating ability of the solvent
• Polar solvent molecules align their dipole
moments maximally or perpendicularly with
the ground state or excited state dipoles
29. Cont………………..
Both the ground state and the excited state
are neutral.
When both the ground state and the excited
state are neutral a shift in wavelength is not
observed
No change occurs.
Like dissolves like and a polar solvent won’t be
able to align its dipole with a neutral ground
and excited state.
30. Cont……….
The excited state is polar, but the ground
state is neutral
It will align its dipole with the excited state
and lower its energy by solvation.
This will shift the wavelength to higher
wavelength and lower frequency.
32. Cont………..
The ground state and excited state is polar
the polar solvent will align its dipole moment
with the ground state
Maximum interaction will occur and the energy
of the ground state will be lowered
The dipole moment of the excited state would be
perpendicular to the dipole moment of the
ground state, since the polar solvent dipole
moment is aligned with the ground state
This interaction will raise the energy of the polar
excited state
34. Cont……..
The ground state is polar and the excited
state is neutral
the ground state is polar the polar solvent will
align its dipole moment with the ground state
Maximum interaction will occur and the
energy of the ground state will be lowered
the excited state is neutral no change in
energy will occur
35. Cont…………
• Like dissolves like and a polar solvent won't be
able to align its dipole with a neutral excited
state.
• Overall you would expect an increase in
energy because the ground state is lower in
energy (decrease wavelength, increase
frequency, increase energy).
37. • Conclusion
• the excited state properties of coordination and
organometallic compounds play important roles
in many research fields, including
nanotechnology, solar energy conversion, and
environmental issues.
• We hope that the present article can be useful as
a source of information and a possible starting
point for future developments. For a related
chapter in this Comprehensive, we refer to
Editor's Notes
Electronic excitation
change of molecular orbital occupancy
increased energy
change of bonding characteristics and possibly geometry
change of charge distribution
possible changes of resultant electron spin, orbital symmetry
A luminescent complex is one that re-emits radiation after it has been electronically excited. Fluorescence occurs when there is no change in multiplicity, whereas phosphorescence occurs when an excited state undergoes intersystem crossing to a state of different multiplicity and then undergoes radiative decay.
electron transitions occurring between ‘metal’ d- orbital.
the ground state of complexes is usually stable toward intramolecular oxidation–reduction processes.
The angular rearrangement of the metal electrons can cause ligand substitution or isomerization reactions
Factor Influencing CT excited states in Redox processes
the stability of upper and lower oxidation states of the metal and ligands.
the effective amount of CT induced by irradiation
whether or not the CT is localized between one particular ligand and the metal
(X M CT states in MLn-1X complexes)
environnemental conditions (cage effect, solvent reactivity.)
Depending on whether the excited electron is originally located on the ligands or on the central metal, ligand-to-metal or metal-to-ligand charge-transfer (LMCT or MLCT, respectively) transitions can occur.
For example, the configuration d2in the field free ion V3+has these terms (in order of increasing energy):3F(ground state)1D,3P,1G, and 1S.
In the octahedral symmetry, the free ion terms split as follows:
3F :3T1g (ground state) 3T2g , 3A2g
1D :1T2g,1Eg
3P :3T1g
1G :1A1g,1T2g,1T1g,1Eg
1S :1A1g
Charge-transfer bands in the visible region of the spectrum (and hence contributing to the intense colours of many complexes) may occur if the ligands have lone pairs of relatively high energy (as in sulfur and selenium) or if the metal atom has low-lying empty orbitals.
LMCT bands are usually in the UV region; however, they can extend to the visible spectral region, particularly for complexes containing highly reducing ligands such
as I-, and Br– oxalate2– it is a common observation that the wavenumber of these bands decreases as the central ion becomes more oxidizing and the ligands more reducing.
.
where πL and σL are MOs mainly localized on the ligands, and πM* (t2g) and σM*(eg) are the MOs which receive the most important contribution from the two groups of metal d orbital note that in the low-spin d6octahedral complexes, such as those of Co(III) the ‘metal’ t2g orbitals are filled, so that the πL----πM* ( t2g) and σL--------- πM* (t2g) transitions cannot occur as a consequence, these complexes cannot exhibit LMCT bands at low energy
Ligands such as CN–, CO, SCN–, and especially the conjugated carbon-containing molecules possess empty π* orbitals suited for such transitions. Regarding the central atoms, it is obvious that MLCT transitions will be favored when the metal has a low oxidation state .forexample, the bands in the visible range of [Ru(bpy)3]2+
(bpy=2,2-bipyridine) are due to MLCT transitions, while those of [Ru(bpy)]3+ are due to LMCT transitions.
A typical example of an intermolecular CT band is given by the intense new band which appears in the spectrum of aqueous solutions of [Co (NH3)6]3+ salts when the concentration of iodide ion is increased. these types of CT bands have the same nature of CT bands found in supramolecular, compounds made of organic donor and acceptor subunits. Intermolecular CT transitions of the inverse type (i.e., from the complex to an outer species) are the so-called charge transfer-to-solvent (CTTS) transitions exhibited by some negative complex ions such as [Fe(CN)6]4-
The first LLCT that was assigned was a near-UV band in the absorption spectra of [Be(bipy)(X2)] complexes.8The LLCT bands red-shifted in the order of the increasing reducing strength of the halide, consistent with an assignment of a halide orbital
to bipy antibonding orbital charge transfer.
some bands of complexes containing aromatic ligands, such as bipyridine, terpyridine, and phenanthroline, surely belong to this class. generally it is possible to identify bands as intra-ligand or CT in nature by observing their energy shifts in a series of complexes of a given ligand with a variety of different metals.
more specifically, it should also be considered that: (1) the MLCT transitions increase the positive charge of the metal, so that a nucleophilic attack by outer ligands could be facilitated, and (2) in most LMCT transitions, the transferred electron goes into a metal orbital which points in the direction of the ligands (i.e., in a eg
σ-antibonding orbital): a metal–ligand repulsion could then result, analogously to what happens in the case of the ligand-field excited state. moreover, CT transitions are expected to cause a strong change in the acid strength of complexes which contain ‘protogenic’ ligands, such as H2O, NH3, and cyano ligands.