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Coordination Chemistry II: Ligand Field Theory
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  1. Coordination Chemistry II: Ligand Field Theory • Chapter 10 • Friday, November 22, 2013

  2. Metal valence orbitals: Ligand frontier orbital: 4s 5s 6s 3d 4d 5d 5p 6p 4p Sc – Zn For now we will only consider σ-bonding with the ligands Y – Cd La – Hg Ligand Field Theory • In LFT we use metal valence orbitals and ligand frontier orbitals to make metal–ligand molecular orbitals • Oh first! • We already did this: see 10/18 lecture.

  3. xy (n+1)s z2 x s xz y yz nd z x2–y2 (n+1)p A1g T1u T2g Eg Oh σ-MOs for Octahedral Complexes • We use group theory to understand how metal and σ-ligand orbitals interact in a complex: symmetries (irr. reps.) of the metal valence orbitals are obtained directly from the character table We need to determine the reducible representation for the σ-ligand orbitals in Oh: C2′ C4 S4 the total ligand representation (Γ6L) can be decomposed as we learned in 4.4.2 C2 σh irreducible representations 6 0 0 2 2 0 0 0 4 2 A1g + Eg + T1u

  4. xy nd (n+1)p (n+1)s z2 x s xz y yz z x2–y2 a1g* eg* t2g t1u* M non-bonding A1g T1u T2g Eg Eg A1g T1u anti-bonding M–L σ* bonding M–L σ eg a1g t1u σ-ML6Octahedral MO Diagram Δo

  5. M–L σ* t1u* ∆O M–L σ* a1g* frontier orbitals M–L σ* eg* M nb t2g M–L σ t1u a1g M–L σ eg M–L σ MO Pictures • It is also helpful to visualize the MOs so we understand the electron distribution within a coordination complex

  6. Adding Metal Electrons • Metal ions typically have some valence electrons that can be accommodated in the metal d orbitals • d0 ions – Ti4+, Zr4+, V5+, Ta5+, Cr6+, Mo6+, etc. • d1 ions – Ti3+, V4+, Ta4+, Cr5+, Mo5+, etc. • d2 ions – V3+, Ta3+, Cr4+, Mo4+, etc. • d3 ions – V2+, Ta2+, Cr3+, Mo3+, Mn4+, etc. • d4-d7 – hold on • d8 ions – Co1+, Ni2+, Cu3+, etc. • d9 ions – Ni1+, Cu2+, etc. • d10 ions – Cu1+, Zn2+, etc. t1u* a1g* eg* t2g t1u a1g eg

  7. HIGH SPIN LOW SPIN High Spin and Low Spin • The situation is a little more complicated for d4-d7metals: • d4 ions – Cr2+, Mo2+, Mn3+, Fe4+, Ru4+, etc. • d5 ions – Mn2+, Re2+, Fe3+, Ru3+, etc. • d6 ions – Fe2+, Ru2+, Co3+, Rh3+, Pt4+, etc. • d7 ions – Fe1+, Ru1+, Co2+, Rh2+, Ni3+, etc. • For d4-d7 electron counts: • when ∆o> Πtotal ➙ low spin • when ∆o< Πtotal ➙ high spin t1u* t1u* a1g* a1g* eg* eg* t2g t2g t1u t1u a1g a1g eg eg

  8. High Spin and Low Spin Electron configurations for octahedral complexes, e.g. [M(H2O)6]+n. Only the d4 through d7 cases can be either high-spin or low spin. Δ < Π Δ > Π • Weak-field ligands: • - Small Δ, High spin complexes • Strong-field ligands: • - Large Δ, Low spin complexes

  9. d4 HS d6 LS d8 eg* eg* eg* Πe only counts for electrons at the same energy! t2g t2g t2g Electron Pairing Energy • The total electron pairing energy, Πtotal, has two components, Πc and Πe • Πc is a destabilizing energy for the Coulombicrepulsion associated with putting two electrons into the same orbital • Πe is a stabilizing energy for electron exchange associated with two electrons having parallel spin

  10. High Spin Low Spin eg* eg* t2g t2g Using LFSE and Π Is the complex high spin or low spin? Fe2+, d6 Δ < Π Aqua is a weak field ligand; hexaaqua complexes almost always high spin

  11. π-MOs for Octahedral Complexes The reducible representation for the π-ligand orbitals in Oh: x and y axes on each ligand irreducible representations 0 0 0 0 T1g+ T2g+ T1u + T2u 12 0 -4 0 0 0 The non-bonding t2g orbitals of an octahedral metal complex are oriented perfectly to form π-bonds with ligands

  12. π Donor vs π Acceptor Ligands • The nature of the metal ligand π interaction is dependent on the type of ligand. • π-donor ligands are ligands with one or more lone pairs of electrons in p orbitals on the donor atom that can donate to empty orbitals on the metal. • preferred for metals with high oxidation states and low d electron count (d0-d3) • π-acceptor ligands (π-acidic ligands) are ligands with empty π* orbitals on the donor atom that can accept electrons from the metal. • preferred for metals with low oxidation states and high d electron count (d6 or higher) • donation of electron density from the metal to the ligand π* orbital results in weakening of the multiple ligand bond Examples: Cl–, Br–, I–, OR–, SR–, NR2–, O2–, NR2–, N3– Examples: CO, NO, CN-, pyridine • “π back bonding”

  13. π-acceptor M–L π* M–L π* π-donor t1u* eg* t2g* t2g* adding d electrons populates the M–L π orbital adding d electrons populates the M–L π* orbital ∆o t2g ∆o a1g* ∆o M–L π t2g M–L π t2g* t2g t1u a1g eg π-Effects in Octahedral Complexes σ-only increasing ∆O eg* eg* M nb t2g

  14. π-Effects in Octahedral Complexes strong field, low spin weak field, high spin

  15. I– < Br– < Cl– < OH– < RCO2– < F– < H2O < NCS– < NH3 < en < NO2– < phen < CN– ≅ CO • weak-field ligands • high-spin complexes for 3d metals* • strong-field ligands • low-spin complexes for 3d metals* π donor ligands σ only ligands π acceptor ligands Spectrochemical Series • The trend in ∆O that arises from π-donor, σ-only, and π-acceptor ligands is the basis for the Spectrochemical Series. For [ML6]n+complexes: increasing ∆O The value of Δo also depends systematically on the metal: 1. Δo increases with increasing oxidation number. 2. Δo increases down a group. → both trends are due to stronger metal-ligand bonding. * Due to effect #2, octahedral 3d metal complexes can be low spin or high spin, but 4d and 5d metal complexes are always low spin.

  16. xy (n+1)s z2 x s xz y yz nd z x2–y2 (n+1)p A1 T2 T2 E T2 A1 σ-MOs for Tetrahedral Complexes • Four-coordinate tetrahedral complexes are ubiquitous throughout the transition metals. the irr. reps. of the metal valence orbitals are obtained directly from the character table Td For the ligand orbitals we need to consider how the Lewis base pairs transform in the Td point group. The result is: Γσ= A1 + T2

  17. xy (n+1)s (n+1)p z2 x s xz y yz z x2–y2 2a1 2t2 3t2 ∆t A1 T2 T2 E bonding M–L σ 1a1 1t2 σ-ML4Tetrahedral MO Diagram M d orbitals very weakly M–L σ* M non-bonding e nd A1 T2

  18. very weakly M–L σ* strongly M–L σ* t2* eg* ∆t ∆o M non-bonding e M non-bonding t2g Tetrahedral Complexes • Metal d orbitals are split into a non-bonding E set and a very weakly anti-bond T2 set • tetrahedral geometry can accommodate all d electron counts, from d0 to d10 • Δtis small compared to Δo: • All tetrahedral complexes of the 3d transition metals are HIGH SPIN! • Tetrahedral complexes of the heavier transition metals are low spin.

  19. Tetrahedral Crystal Field Splitting opposite splitting of octahedral field L t2 orbitals point more directly at ligands and are destabilized. z L y M L x L barycenter (spherical field) e orbitals point less directly at ligands and are stabilized. Δt < Δo because only 4 ligands and d orbitals point between ligands