Lecture 294/5/06. Recap Balancing Redox reactions Electrochemical cells Batteries Standard Reduction Potential table Corrosion Nernst equation Electrolysis.

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Presentation transcript:

Lecture 294/5/06

Recap Balancing Redox reactions Electrochemical cells Batteries Standard Reduction Potential table Corrosion Nernst equation Electrolysis Molten aqueous Counting electrons

Central metal and ligands Complex ions vs. Coordination complexes Complex ions and Coordination complexes

Complex formation can change physical and chemical properties Ag + (aq) + e -  Ag (s) E° = V [Ag(CN) 2 ] - + e-  Ag (s) + 2CN - (aq)E° = V

Coordination # Geometry

Naming complex compounds

bonds NH 3 Ammine1 COCarbonyl1 H2OH2OAqua1 Br - Bromo1 Cl - Chloro1 CN - Cyano1 F-F- Fluoro1 NO 2 - Nitro1 OH - Hydroxo1 NCS - Isothicyanto1 SCN - Thiocyanato1 CO 3 2- Carbanato2 C 2 O 4 2- Oxalato2 H 2 NCH 2 CH 2 NH 2 (en)Ethylenediamine2 EDTA 4- Ethylenediaminetetraacetic acid6

Co(NH 3 ) 3 (OH) 3 K[Cr(NH 3 ) 2 (C 2 O 4 ) 2 ] diamminetriaquahydroxochromium (III) nitrate Potassium tetrachloroplatinate (II) Name, coordination number, and geometry?