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Coordination Compounds Colorful world of transition metals [Co(NH3)5Cl]Cl2 • Complex ion: can be cation or anion; contains the transition metal and usually is in brackets. • Ligands: neutral molecule or ion having a lone pair of electrons that forms a coordinate covalent bond to a metal ion; usually dissociate when aqueous. Ligands in the spectrochemical series show which ones can replace others. [Co(NH3)5Cl]Cl2 • Counter ion: anion or cation needed to make complex ion neutral. Use it to find variable charges of transition metals • Oxidation Number: (primary valence), refers to the ability to form ionic bonds with anions [Co(NH3)5Cl]Cl2 • Coordination number (secondary valence): refers to number of bonds formed between the metal ion & ligands in complex ion. Ligands • Mono/unidentate: one attachment site • Bidentate: two attachment sites (unbonded pair of electrons) • Polydentate: multiple attachment sites; EDTA, dien Nomenclature [Ir(NH3)4(H2O)2](NO3)3 • Determine oxidation # of metal • Ligands are named first, alphabetically with prefixes: mono-, di-, tri-, tetra-, penta-, hexa-. Prefixes DO NOT affect order. • Anion ligands end in “o” chloro, fluoro • First name end with metal + variable charge (romans #s) • Second name = counter ions/anion • If complex ion is anion the ending changes to the Latin name and – ate suffix Name, coordination # and oxidation # • K4[Fe(CN)6] • Na[PtCl3(NH3)] • Dichloroethylenediamminecadmium • Tris(en)cobalt (III) tris (oxalato)ferrate