L07 Chem 151 Lecture 8: Complexes
8 Nov 2016
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Central metal cation with empty orbitals that can accept electron pairs (a lewis acid) Surrounded by some number of neutral/anion ligands that can donate a pair of electrons (a lewis base) Coordinate covalent bond all electrons come from the ligands, none from the central metal. When coordination compounds are dissolved in water, the complexes remain intact. H2o, cn-, co, nh3, cl-, o2 monodentate (occupy one binding site) Ethylenediamine bidentate (polydentate ligands are called chelating agents) Coordination number number of ligand sites around central atom in a complex. Depends on nature of central metal and the ligands. Agoh + 2nh3 -> [ag(nh3)2]oh complex formation. When a reagent capable of acting as a ligand is added to a ppt and the ppt dissolves, a complex is formed. Ml6 + y -> ml5y + l (if added ligand has greater affinity) Ml5y + y -> ml4y2 + l, this continues step by step.
