chem312_Coordination_complex_lecture_12

chem312_Coordination_complex_lecture_12 - Electronic...

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h ! excited state h ! ground state Electronic Spectrum of [Ni(H 2 O) 6 ] +2 ! ( nm) " absorption of a photon causes an electron to be promoted into a higher energy orbital the photon energy corresponds to visible light d z2 d xy d x2-y2 d xz d yz Bare M +n degenerate degenerate M +n surrounded by spherical distribution of L q- 6 L q- L q- L q- L q- d z2 d xy d x2-y2 d xz d yz degeneracy has been lifted splitting corresponds to the wavelength of visible light less coulombic repulsion d xz d z2 z more coulombic repulsion M +n interacting with 6 L q- fixed along the axes Fix L q- along axes L q- L q- L q- x z x d xz d yz d xy Why do the d–orbitals split when ligands bind to metal ions? valence electrons coulombic repulsion d z2 h ! excited state h ! ground state Electronic Spectrum of [Ni(H 2 O) 6 ] +2 ! ( nm) " absorption of a photon causes an electron to be promoted into a higher energy orbital d z2 d xz d z2 An alternative way to explain the splitting between the d–orbitals is to use Molecular Orbital Theory. L L L L M L L x y z L L L L L L x y z ! –type orbitals L L L L M L L x y z L L L L M L L x y z (3d z2 , 3d x2–y2 ) (4pz,4px, 4py) 4s O h symmetry recall SF 6 …….
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The d–orbitals point along the axes point between the axes ! –type orbitals " –type orbitals d z2 , d x2-y2 d xz , d xy , d yz Notice: the d–orbitals are not all degenerate Thus, symmetry arguments alone tell us that the
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This note was uploaded on 03/06/2010 for the course CHEM 312 taught by Professor Staff during the Winter '08 term at University of Washington.

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chem312_Coordination_complex_lecture_12 - Electronic...

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