Electronic Structure and Angular Momentum of Transition Metal Complexes

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Electronic Structure and Angular Momentum of Transition Metal Complexes Electronic Structure and Angular Momentum of Transition Metal Complexes © K. S. Suslick, 2013 Angular Momentum vs. Number of Electron Spins To understand the energy of paramagnetic systems (i.e., ones with unpaired electrons), we must describe them in terms of their angular momentum. S = 0 Singlet Total Angular Momentum: S = 1/2 Doublet S = 1 Triplet J = Ms + ML S = 3/2 Quartet S = 2 Quintet Total Multiplicity: (2S+1)(2L+1) L = 0 “S term” singly orb. deg. Each “microstate” has the same L = 1 “P term” triply L and S, but different J. L = 2 “D term” pentuply L = 3 “F term” L = 4 “G term” © K. S. Suslick, 2013 1 Spin For the Total Spin of an atom or molecule the rules apply: 1. Doubly occupied orbitals do NOT contribute to the total Spin 2. Singly occupied orbitals can be occupied with either spin-up or spin-down e- 3. Unpaired e- can be coupled parallel or antiparallel, giving a total spin S 4. For a state with total spin S there are 2S+1 “components” with M = S,S-1,...,-S. Hence terms singlet, doublet, triplet, … 5. The MS quantum number is always the sum of all individual ms QNs. © K. S. Suslick, 2013 Spin Names “Russell-Saunders” Term Symbols for atoms; Irr Rep Mulliken for molecules Examples for dn configurations: Atoms Molecules doublet 2H sextet 6A triplet 3 l=1 or 3 © K. S. Suslick, 2013 2 L–S Coupling L-S Coupling = Russell-Saunders Coupling If coupling of the spin angular momentum and orbital angular momentum is relatively weak (and it usually is), then L and S remain “good” Quantum Numbers and can be treated independently of each other. Each electronic state has its own term symbol spin multiplicity 2S+1 L = 0 “S term” singly orb. deg. L = 1 “P term” triply L L = 2 “D term” pentuplicately L = 3 “F term” L = 4 “G term” (Within each term, there can be several degenerate microstates with different ML and MS.) © K. S. Suslick, 2013 L–S Coupling L = 0, 1, 2…total orbital angular momentum (“term”) ML = 0, 1, 2, L components of L (ML = ml for each e). For example, for L = 1, there are three ML values: 1, 0, -1. (analogous to l = 1 and its three ml values: 1, 0, -1) # of ML states is 2L+1 = orbital degeneracy S = total spin angular momentum Ms = S, S-1, ….-S components of S (MS = ms). For example, for S = 1, there are three Ms values, 1, 0, -1. Each electronic state has its own term symbol spin multiplicity 2S+1 L = 0 “S term” singly orb. deg. L = 1 “P term” triply L L = 2 “D term” pentuplicately L = 3 “F term” L = 4 “G term” (Within each term, there can be several degenerate microstates with different ML and MS.) © K. S. Suslick, 2013 3 Hund’s Rules 1. The ground state (GS ‘term’) has the highest spin multiplicity (S). 2. If two or more terms have the same spin multiplicity, then the GS will have the highest value of L. 3. For subshells less than half-filled (e.g., p2), lowest J is preferred; for subshells more than half-filled, highest J is preferred. Of all the states possible from degenerate orbitals, the lowest energy one will have the highest spin multiplicity (i.e., most unpaired spins). For states with the same spin multiplicity, the highest orbital degeneracy will be lowest in energy. © K. S. Suslick, 2013 The Problem: Electron-Electron Repulsion. d2 Consider as an example, 2 d electrons, one in z2 e e z2 x2-y2 g z2 x2-y2 g t2g t2g xy xz yz xy xz yz z z xz + z2 xy + z2 y y x x overlapping lobes, lobes far apart, large inter-electron repulsion small inter-electron repulsion These two electron configurations differ in energy. © K. S. Suslick, 2013 4 Microstates and Spin Orbit Coupling For a given L, the allowed values of ML and Ms are called microstates. 2N from spin (2No)! o # of microstates = up vs. down (2No –Ne)! Ne! Where No = degeneracy of orbitals in set of subshell and Ne = number of electrons e.g., for free atoms/ions, No for d orbitals = 5 © K. S. Suslick, 2013 Microstates and Spin Orbit Coupling 2N from spin (2No)! o up vs. down (2No –Ne)! Ne! Pauli X etc. etc. for 25 for 20 more © K. S. Suslick, 2013 5 Microstates and Spin Orbit Coupling Shorthand way to describe determinantal Wave Functions, e.g., for 2 electrons: mS of electron #1 mL of electron #1 2 e- in p orbitals: ml = -1, 0, +1, ms = -½ or +½ ( 1- 0+ ) mL = 1 0 -1 © K. S. Suslick, 2013 Microstates and Spin Orbit Coupling To find all the terms for a specific configuration: 3) Repeat #2 for microstates remaining with next greater ML etc. © K. S. Suslick, 2013 6 Microstates and Spin Orbit Coupling: p3 p3 examples: © K. S. Suslick, 2013 Microstates and Spin Orbit Coupling: d2 Ms mL M L 1G 3F 3P 1D 1S So, the allowed terms states for d2 are 1G, 3F, 3P, 1D, and 1S. What’s the GS?! Hund’s Rules. © K. S. Suslick, 2013 7 Hund’s Rules 1. The ground state (GS ‘term’) has the highest spin multiplicity (S). 2. If two or more terms have the same spin multiplicity, then the GS will have the highest value of L. 3. For subshells less than half-filled (e.g., p2), lowest J is preferred; for subshells more than half-filled, highest J is preferred. Of all the states possible from degenerate orbitals, the lowest energy one will have the highest spin multiplicity (i.e., most unpaired spins). For states with the same spin multiplicity, the highest orbital degeneracy will be lowest in energy. © K. S. Suslick, 2013 Microstates and Spin Orbit Coupling The allowed terms states for d2 are 1G, 3F, 3P, 1D, and 1S. What’s the GS? Hund’s Rules. G.S. is 3F. What’s the lowest excited state? Hund’s Rules DO NOT TELL YOU THAT!! (the XS energies you get from Condon-Shortley or Racah Parameters). © K. S. Suslick, 2013 8 Energy Separations of Free Ion States © K. S. Suslick, 2013 Microstates and Spin Orbit Coupling, d2 © K. S. Suslick, 2013 9 Spin Orbit Coupling © K. S. Suslick, 2013 Size of Spin Orbit Coupling For a single electron, the strength of Spin-Orbit Coupling (SOC) in a particular microstate is measured by For the whole Term State, SOC is measured by © K. S. Suslick, 2013 10 Energy Separations of Free Ion States But there is a fine structure within these states due to SOC! © K. S. Suslick, 2013 Energy Separations of Free Ion States “Lande Interval Rule” Furthermore, with L-S approximation, Spin-Orbit Coupling must preserve the “center of gravity” of the energy of the term state. (n.b., degeneracies of the J states must be counted.) © K. S. Suslick, 2013 11 Energy Separations of Free Ion States “center of gravity preserved” © K. S. Suslick, 2013 Energy Separations of Free Ion States microstates: © K. S. Suslick, 2013 12 Energy Separations of Free Ion States SOC magnitude from center of gravity L=3, S=1 J = 4, 3, 2 Degeneracy = 2J+1 © K. S. Suslick, 2013 Spin Orbit Coupling, d23F ground state SOC magnitude from center of gravity L=3, S=1, J = 4, 3, 2 Degeneracy = 2J+1 © K. S. Suslick, 2013 13 Energy Separations of Free Ion States = 9-fold degenerate 7-fold degenerate 5-fold degenerate © K. S. Suslick, 2013 Energy Separations of Free Ion States The inter-electron repulsion integrals can be broken into 3 radially and angular forms: © K. S. Suslick, 2013 14 Energy Separations of Free Ion States The inter-electron repulsion integrals can be broken into 3 radially and angular forms: (more later on Tanabe-Sugano Diagrams) © K. S. Suslick, 2013 Energy Separations of Free Ion States: d2 © K. S. Suslick, 2013 15 © K. S. Suslick, 2013 Hole Formalism Eletrons vs. holes: dn and d10-n will have the same possible term states! Their energies of interaction with the environment, however, will have opposite signs. © K. S. Suslick, 2013 16 Spin Orbit Coupling: J-J Coupling If spin-orbit coupling is very strong, then it can no longer be treated as just a perturbation. mL and ms are no longer "good" quantum numbers. Only j = mL + ms is valid. For multi-electron systems, applies only (not L and S). Applies to Lanthanides, Actinides and 3rd row metals. © K. S. Suslick, 2013 Size of Spin Orbit Coupling 120 cm–1 for Ti2+ to 830 cm–1 for Cu2+ (3d) 300 cm–1 for Y2+ to 1600 cm–1 for Pd2+(4d), 640 cm–1 for Ce3+ to 2950 cm–1 for Tb3+ (4f). © K. S. Suslick, 2013 17 Effect of Ligands on State Energies Simplest approach: “Crystal Field Theory” 1. metal d-electron Term States 2. Perturbation by point charges (i.e., ligands) 3. No consideration of other (non-d) electrons. 4. No covalency (added as an empirical correction in Ligand Field Theory) 5. Useful for optical spectra magnetism EPR Mössbauer © K. S. Suslick, 2013 Approximations in CFT kinetic coulombic inter-electron repulsion spin-orbit coupling ligand field comparable magnitudes = net pt. charge on ligand, . l = distance between ith electron and ligand, . l = ligand or crystal field © K. S. Suslick, 2013 18 Approximations in CFT 1. Free ion with SOC: 2. Weak field 3. Strong field © K. S. Suslick, 2013 Approximations in CFT So, how do we assign states in each of these conditions and how do they correlate? © K.
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