1. Lecture 294/5/06

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

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

5. Complex formation can change physical and chemical properties Ag + (aq) + e -  Ag (s) E° = 0.799 V [Ag(CN) 2 ] - + e-  Ag (s) + 2CN - (aq)E° = - 0.31 V

7. Coordination # 2 4 6 Geometry

8. Naming complex compounds

9. 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

10. 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?