Ligand Substitution Reactions: Rates and Mechanisms

1. Ligand Substitution Reactions: Rates and Mechanisms

2. Stoichiometric and Intimate Mechanisms • We can think of a reaction mechanism at two different levels. • – The reaction may occur through a series of distinct steps each of which can be written as a chemical equation. • » This series of steps is a stoichiometric mechanism. • – We can also consider what is happening during each of these individual steps. • » These details constitute the intimate mechanism of the reaction.

3. Stoichiometric Mechanism • Each step in the stoichiometric mechanism has a rate or equilibrium constant associated with it. • The stoichiometric mechanism looks at the reactants, products and intermediates that are involved in a reaction. • Each species considered exists in potential minimum along the reaction coordinate.

4. Stoichiometric mechanism: the sequence of elementary steps in a reaction 5 coordinate intermediate Dissociative Mechanism, D

5. 7 coordinate intermediate Associative Mechanism, A

6. In general, a D mechanism requires evidence for the existence (structural, spectroscopic) of an intermediate with reduced coordination number. An A mechanism requires evidence of an intermediate with increased coordination number.

7. If there is no identifiable intermediate, then we have to assume an interchange mechanism is operating transition state rather than an intermediate Interchange Mechanism, I

8. Intimate mechanism: this describes the nature of the process in the rate-determining step. If the rate is strongly dependent on the nature of the entering group, then the intimate mechanism is associative. We say the reaction is under associate activation. The symbol is a subscript a.

9. Suppose for the reaction [M(NH3)3(OH2)]n+ + Lm− → [M(NH3)3L](n-m)+ + H2O there is spectroscopic evidence for the existence of a 5 coordinate intermediate; the rate of the reaction is strongly dependent on the nature of L (for example, if L = H2O the reaction occurs 4 orders of magnitude slower than if L = CN−) • tells us that we are dealing with an A stoichiometric mechanism • tells us that the intimate mechanism is a The mechanism of the reaction is Aa

10. rate determining step

11. intermediate rate determining process

12. Whilst less common the situation could arise where the reaction proceeds through an intermediate of reduced coordination number (D) and this is followed by rate-determining attach of entering L on the intermediate (a). The mechanism would then be described as Da.

13. The mechanism would then be described as Da. Reversible formation of a 5 coordinate intermediate Product Rate-determining attack of entering ligand

14. rate determining step

15. In a Adreaction, formation of the intermediate of higher coordination number occurs relatively rapidly; the rate-determining step is the dissociation of a ligand from the intermediate

16. ‡ If there is no experimental evidence for an intermediate, then we have to assume an interchange, I, mechanism. In this mechanism, bond breaking and bond making occur simultaneously and there is no well-defined intermediate along the reaction coordinate.

17. ‡ An interchange, I, mechanism could be under either associative or dissociative activation, i.e., IaorId

18. ‡ If the rate of the reaction is strongly dependent on the nature of the entering group and is weakly dependent on the nature of the leaving group, then bond making is more important than bond breaking. The reaction is under associative activation. We say the mechanism is an Associative Interchange Mechanism, Ia

19. ‡ If the rate of the reaction is weakly dependent on the nature of the entering group and is strongly dependent on the nature of the leaving group, then bond breaking is more important than bond making in the approach to the transition state. The reaction is under dissociative activation. We say the mechanism is a Dissociative Interchange Mechanism, Id

20. Ia Id

21. inert labile Self-exchange reactions M(H2O)6 + H2O*  M(H2O)5(H2O*) + H2O (eg., from line shape analysis using 17O NMR)

22. Rate: • increases with ionic radius • decreases with an increase in ionic charge

23. Inertness  q __ r • Rate: • increases with ionic radius • decreases with an increase in ionic charge Inertness  ion  Self exchange reactions at metal centres are usually under dissociative activation

24. These two will exchange very rapidly because of the long (and therefore weak) M-L bonds. For the transition metals... • Inertness  ion • Jahn-Teller distortion of high spin d4 and d9 complexes imparts on them significant lability. This is an example of how a ground state structural effect can influence kinetics

25. There is a strong correlation between Ligand Field Stabilisation Energy (LFSE) and inertness For example, low spin Co3+ and Cr3+ are amongst the most inert transition metal ions

26. d3 LFSE = -12 Dq Cr(III) d6 (LS) -24Dq + 2P Co(III) d8 -12Dq Ni(II) d7 (HS) -8Dq Co(II) d9 -6Dq Cu(II) d10 0 Zn(II) Expected order of lability: Co(III) < Cr(III) = Ni(II) < Co(II) < Cu(II) < Zn(II)

27. more inert than expected more labile than expected Expected order of lability: Co(III) < Cr(III) = Ni(II) < Co(II) < Cu(II) < Zn(II) Observed order of lability: Cr(III) ~ Co(III) < Ni(II) < Co(II) < Zn(II) < Cu(II)

28. population of eg orbitals (which are antibonding) imparts lability to a metal ion. Thus Ni2+ (d8, t2g6eg2) is much more labile than d3 Cr3+ (t2g3) although it has the same LFSE more inert than expected more labile than expected J-T distortion of d9 ion Observed order of lability: Cr(III) ~ Co(III) < Ni(II) < Co(II) < Zn(II) < Cu(II)

29. Hence: LFSE (a thermodyamic parameter) is a rough guide to the rate of self-exchange reactions at metal centres (a kinetic parameter).

30. 2nd and 3rd transition series Usually very inert • High LFSE • Strong M-L bonds because of good overlap between ligand orbitals and the more expansive (compared to 3d) 4d and 5d orbitals

31. Ground state  Transition state LFSEGS LFSETS Clearly the LFSE contributes to the kinetic behaviour of a metal ion, i.e., there must be a ligand field contribution to the activation energy (LFAE) LFAE = LFSETS - LFSEGS

32. EXAMPLE [Cr(H2O)6]3+ {[Cr(H2O)5(H2O)]3+}‡ LFSEGS = -12Dq LFSETS • Assumptions: • the reaction is under dissociative activation • the departing ligand in the TS is far from the metal centre, i.e., that the TS is approximately 5-coordinate The LFSE of the TS will depend on the geometry of the TS, and two reasonable geometries can be envisaged, viz., square pyramidal (C4v) and trigonal bipyramidal (D3h)

33. The LFSE of the TS will depend on the geometry of the TS, and two reasonable geometries can be envisaged, viz., square pyramidal (C4v) and trigonal bipyramidal (D3h)

34. D3h In D3h the d orbitals transform as e” xz,yz e’ x2-y2, xy a1’ z2 Method of Krishnamurthy and Schaap to estimate LFSE of geometries that are neither Oh nor Td

35. Method of Krishnamurthy and Schaap axial ligand field equatorial ligand field

36. axial equatorial

37. axial equatorial

38. axial equatorial

39. axial equatorial

40. In D3h the d orbitals transform as e” xz,yz e’ x2-y2, xy a1’ z2 Symmetry requires the energies of these two oribitals to be the same axial equatorial Average of 2.93 and -4.57 is -0.82

41. In D3h the d orbitals transform as e” xz,yz e’ x2-y2, xy a1’ z2 axial equatorial

42. axial equatorial

43. LFSETS = 2(-2.71) – 0.82 = -6.24 Dq LFSEGS = -12Dq LFAE = -6.24 –(-12) Dq = 5.76 Dq

44. For Cr(III), Dq = 1760 cm-1 (from electronic spectroscopy), so LFAE= 10138 cm-1

45. From this kind of approach:

46. Predicted rate: Co(III) < Cr(III) < Ni(II) < Fe(III) < Mn(III)

47. Predicted rate: Co(III) < Cr(III) < Fe(III) < Ni(II) < Mn(III)

48. Predicted rate: Cr(III) < Mn(III) < Co(III) ~ Ni(II) < Fe(III)

49. Experimental rate: Cr(III) < Co(III) < Fe(III) < Ni(II) < Mn(III) Hence, probably a D mechanism, possibly with a C4v intermediate. There is other evidence to suggest that many Cr(III) reactions have a distinctly associative character, explaining the very inert nature of Cr(III) complexes