Lecture 9 Slides - Printer-friendly.pdf - Homework Reminder Exercise Set 7 Practice Quiz 7 Course Content Video#7 Pre-lab 7 Help session today(5-6 pm in

Lecture 9 Slides - Printer-friendly.pdf - Homework Reminder...

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1 Lecture 9 Introduction to Coordination Chemistry 1. Complexes and Coordination Compounds 2. Monodentate Ligands and Polydentate Ligands 3. Coordination Numbers and the Geometries of Complexes 4. Complex Formation Reactions and Ligand Substitution Reactions 5. Exp. 7: Chemistry of Iron, Copper, and Cobalt Complexes Homework Reminder: Exercise Set 7 Practice Quiz 7 Course Content Video #7 Pre-lab 7 Help session today (5-6 pm in Wrighton 250) Coordination Complexes Central metal (ion) n+ M surrounded by certain numbers of ligands :L M n+ is the central metal ion which has empty orbitals that can accept electron pairs (a Lewis acid). L are the ligands. They can be anions or neutral molecules that contain at least one atom that is capable of donating a pair of electrons (a Lewis base) to the central metal to form a coordinate-covalent bond. (Dative bond) A complex can be a cation, an anion, or a neutral molecule [Co(NH 3 ) 6 ] SO 4 K 2 [CoCl 4 ] Pt(NH 3 ) 2 Cl 2 A coordination cpd is a cpd containing complex ion(s) Complex cation + Simple anion Simple cation + Complex anion Complex cation + Complex anion A complex neutral molecule [Co(NH 3 ) 6 ] [CoCl 4 ] When coordination compounds dissolve in water, the complex ions usually remain in tact. K 2 [CoCl 4 ] 2 K + + CoCl 4 2- [Co(NH 3 ) 6 ] SO 4 Co(NH 3 ) 6 2+ + SO 4 2- e.g.
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