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Coordination Chemistry ligands bonding to metals
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Donor-Acceptor Complexes
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Definitions Lewis Acid = acceptor = usually a transition metal cation Lewis Base = donor = ligand = usually something with a lone electron pair Coordination number = # of metal-ligand attachments Denticity = # of attachments a ligand makes
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Common Ligands Monodentate Ligands: Halides: F -, Cl -, Br -, I - O 2-, S 2-, OH -, CN - NH 3, H 2 O, CO Bidentate Ligands:Polydentate Ligands: heme, salen
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Monodentate complexes
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Bidentate ligand complexes Ni(DMG) 2 Co(en) 2 Cl 2
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Bidentate complexes Co(en) 3 2+ Fe(phen) 3 2+
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Polydentate complexes Co(salen) + chlorophyll
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Fe-heme
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Polydentate complexes Fe-heme O 2 -Fe-heme
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Determining Metal Oxidation States [Ag(NH 3 ) 2 ]NO 3 K 2 [NiCl 4 ] [Co(en) 2 Cl 2 ]Cl [Cr(H 2 O) 4 CO 3 ]Br
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Isomerization in Coordination Compounds Do for octahedral Complexes
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Inner and Outer Spheres [Co(NH 3 ) 4 Cl 2 ]Cl H 2 O [Co(NH 3 ) 4 (H 2 O)Cl]Cl 2
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All compounds Structural (constitutional) Stereo linkage ionization hydration geometric optical [Co(NH 3 ) 5 Cl]NO 2 [Co(NH 3 ) 5 NO 2 ]Cl [Co(NH 3 ) 4 Cl(H 2 O)]Cl 2 [Co(NH 3 ) 4 Cl 2 ]Cl H 2 O [Co(NH 3 ) 5 SCN] 2+ [Co(NH 3 ) 5 NCS] 2+
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Linkage Isomers
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Ionization Isomers
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Hydration Isomers
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Optical Isomers: enantiomers (mirror images) key to recognizing: no mirror planes of symmetry Type 1. arrangement of monodentate ligands Type 2. arrangement of bidentate ligands
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Geometric isomerism: like cis-trans
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Geometric isomerism Fac- isomer Mer- isomer
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Geometric Isomers: predicting numbers Use shorthand: M = metal a, b, c, etc. are different ligands Example 1: Co(NH 3 ) 4 Cl 2
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Example 2: Co(NH 3 ) 3 BrCl 2
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Example 3: Co(NH 3 ) 3 enBr 2+
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