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Ch 18 - L35 Chapter 18 Bonding in Transition Metals and...

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L35: Chapter 18 Bonding in Transition Metals and Coordination Complexes 18.1 Chemistry of Transition Metals 18.2 Formation of Coordination Complexes 18.3 Structure of Coordination Complexes 18.4 Crystal Field Theory and Magnetic Properties 18.5 The Spectrochemical Series and Ligand Field Theory 18.6 Organometallic Compounds and Catalysis Review Molecular Orbitals and Interaction of Molecules with Light (Chapters 15-17)
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Available Electronic Shells and Subshells and Their Energies Energy 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p
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Electronic Configurations of Many-Electron Atoms • Use the Aufbau (“Builiding up”) principle to predict “ground state” electronic structures: Rule #0: • Electrons go in one by one to the lowest available energy orbital Rule #1: • Every AO can hold at most 2 electrons. • When an orbital holds two electrons, the electrons must have opposite “spin” ( m s = ± ½) Rule #2 (Hund’s rule): • Electron with same spin avoid each other (Pauli principle)
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Transition metals - filling d - and f -orbitals, partially filled shells - can accept and donate electrons - many oxidation states -> tunable chemistry Mn: +2, +3, +4, +7 V: +2, +3, +4, +5 Fe: +2, +3 Cu: +1, +2 - catalysis (Pt, Ru, Cr, V) - added to modify properties of materials (e.g., steel) - materials (e.g., titanium utensils for mountaineering, bikes, etc) - important bio-molecules (enzymes, hemoglobin, vitamins)
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DEMO: oxidation states of Mn Mn 2+ : Mn 2+ (aq), MnSO4 Mn 3+ : Mn 3+ (aq) Mn 4+ : MnO 2 (s) Mn 5+ : [MnO 4 ] 2- Mn 6+ : [MnO 4 ] 3- Mn 7+ : MnO 4 - (aq), KMnO 4
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d -and f -orbitals: are not outer orbitals -> changes in properties along period are less drastic, e.g. they are all metals
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Ch 18 - L35 Chapter 18 Bonding in Transition Metals and...

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