11 - reaction mechanisms
TRANSCRIPT
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Reaction mechanisms of Coordination
Compounds
Advanced Inorganic Chemistry
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The Kinetic Model - Transition State
Theory Molecules obtain sufficient energy to
reach a state intermediate between
reactants and products This intermediate state is called the
activated complex
There is then a 50% probability of theactivated complexes decaying to productsor reactants
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Principle of microscopic
reversibility Molecules can proceed along the reaction
coordinate in either direction
It is required that at equilibriumbothforward and reverse reactions proceed at
equal rates along the reaction coordinate
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Consequences
the route of entry for the new ligand must
be just the reverse of that for the loss of the
leaving ligand Insofar as the entering group Y resembles
the leaving group X, the mechanism for
replacement of X by X (exchange) mustresemble replacement of X by Y
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Inert and labile
Inertness is a kinetic stability
As we discussed earlier, it reflect the rate at which
the ligands of the complex exchange places withthose molecules in the outer sphere
Thermodynamic stability is described by n
A complex can be thermodynamically stable
(large n), but kinetically unstable (labile)
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Langford and Gray Classification
Class I; (diffusion controlled) k 108s-1
alkali metals, alkaline earths (except Be2+
and Mg2+), Cd2+, Hg2+, Cr2+, Cu2+, sometrivalent lanthanides
Class II; 104< k < 108s-1
divalent first transition series elements(except V2+, Cr2+, Cu2+), Ti3+, Mg2+, othertrivalent lanthanides
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Langford and Gray
Class III; 1 < k < 104s-1
Be2+, V2+, Al3+, Ga3+, several trivalent
lanthanides
Class IV; 10-6< k < 10-2s-1.
Cr3+, Co3+, Rh3+, Ir3+, Ru2+, Pt2+,
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Lability and electron
configuration Inert configurations
d3, low spin d4, d5, d6
d8is borderline (really only weak field Ni2+
complexes)
Strong field d8complexes are square planar
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Mechanisms for ligand
substitution reacts, Oh systems X- leaving group; Y - entering group
Leaving group usually listed last
e.g.
L5MX + Y L5MY + X
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Two issues
intimate mechanism - whether the main
factor controlling the activation energy is
the breaking of the M-X bond (dissociative,d) or making of the M-Y bond (associative,
a)
stoichiometric mechanism - what is thesequence of elementary steps leading from
reactants to products
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Dissociative (D) mechanism
Bond-breaking most important. Complex is
surrounded by solvent molecules, Y and other
molecules that may be present L5M intermediate must be observed to verify D
L5MX
k1
k-1
L5M + X
L5M + Yk2
L5MY + X
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Id- Interchange dissociative
primary contribution to activation energy is bond-
breaking, but L5M is not detectable
M-X is breaking, but M-Y is starting to form
L5MX + YK
(L5MX,Y)
(L5
MX,Y)k
(L5MY,X)
(L5MY,X)fast
L5MY + X
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Experimental parameters
Can control [Y]o, [L5MX]o
rate = kobs[L5MX]
Note [L5MX]o= [L5MX] + K[L5MX][Y]
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Associative (A) mechanism
No firmly established A mechanisms for
octahedral complexes since seven
coordinate intermediate has never beenobserved conclusively
rate = kobs[L5MX][Y]
D, Id, and Iaall lead to the same rate law, soadditional tests of mechanism are needed
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Experimental tests of mechanism
No mechanism is actually proven
Easiest thing to distinguish is the intimate
mechanism
Most data is know for inert complexes
(CoIII, CrIII, RhIII, IrIII, PtII, NiII)
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Reactions studied - ligand
exchange Aquation (often termed acid hydrolysis)
L5MXn++ H2O L5M(OH2)
(n+1)++ X-
AnationL5M(OH2)
(n+1)++ X-L5MXn++ H2O
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Sensitivity to the Nature of the
Entering or Leaving Group Consider Table 11.3 - rates of aquation of
[Co(NH3)5X]n+
Rates depend heavily on nature of X (sixorders of magnitude)
Relatively little sensitivity to Y
Therefore, breaking M-X bond is more
important
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Sensitivity to the Nature of the
Entering or Leaving Group One problem is that in water, no direct
replacement of X-occurs, rather aquation
followed by anation Conversely, [Ti(OH2)6]
3+shows a rate
variation with entering groups ~ 104(Table
11.5)
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Electronic effects of inert ligands
for cis-[Co(en)2LX]n+(Table 11.6)
When X leaves, the orbital of the d2sp3hybrid isempty
If the cis L is a good -donor, it can supplyelectrons to the electron deficient CoIII.
This stabilizes the transition state and lowers the
activation energy Therefore, cis complexes with good -donors,
react more rapidly than cis complexes with -acceptor ligands (CN-) or -only donors (NH3)
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Electronic effects of inert ligands
with L trans to X, no stabilization can takeplace unless the complex rearranges to
trigonal bipyramidal. this rearrangement raises Eaand lowers the
rate relative to the corresponding ciscomplex
These observations would be hard toreconcile with an a intimate mechanism
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Comparison of rates for Anation
and Water Exchange Since water (or any solvent) concentration cannot
be varied, so its presence in the transition state
cannot be discerned kinetically Can use 18OH2as X
L5M(18OH2) + H2O L5M(OH2) +
18OH2
Mechanism is Id, since K[H2O]>>1, so kobsis
identified with the rate for dissociative interchangeof H2O between the inner and outer sphere
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Comparison of rates for Anation
and Water Exchange Similar limiting rate laws can be observed if [Y] is
high enough
Reaction is then 1st order in L5MX and k
obsis in
units in s-1
at low [Y], 2nd order kinetics are observed
at high [Y], 1st order (saturation) kinetics are
observed plots of kobsvs [Y] will help. Limiting first order
behavior may not be observed if k2or K is toosmall
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Effect of charge on reaction rate
Increased positive charge should make
bond-breaking more difficult
rate would decrease with increasingpositive charge for d intimate mechanism
true for main group elements
for TMI, CFSE overlay the charge effects
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Activation parameters
G= H- TS
H- energy requirements for reaching the
transition state
S- change in ordering on reaching the
transition state
Activation parameters can often revealdifferences masked by similar values of kobs
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Activation parameters
also have V- volumes of activation
kobsexp(-PV/RT)
a plot of ln kobsvs P gives a straight line of
slope -V/RT
Data more complex than expected
V= Vinstrinsic+ Vsolvent(latter term
more important for charged ligands
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V> 0 when anionic ligands leaveanionic complexes
See Table 11.12 for summary