9.Molecular Orbitals and Bonding in Inorganic Complexes.pdf...

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Molecular Orbitals and Bonding in Inorganic Complexes * With a few metal complexes to set the stage (like PtCl 6 2– ), we're starting to get some idea of what a metal–ligand bond means * Best demonstrated by the contrast between the organic and inorganic conceptions of bonding M–H: The organic chemist homolyzes covalent bonds: M–H M · + H · Inorganic chemists heterolyze covalent bonds (giving e ligand): M–H M + + H M–NH 3 (organic chemists assign formal charges to "dative" bonds, inorganic chemists don't): * Both of these conceptions are approximations. For many metal complexes, the ligands are much more electronegative than the central metal, so it is an appropriate simplification to assign all of the electrons for drawn bonds to the ligand. * All of the above only apply to σ -only ligands (they don't consider π effects). For completeness, we need to consider the possibility that ligands can either donate or accept electrons with π -symmetry orbitals.
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