L35_TransMetals2

L35_TransMetals2 - Transition metals Available Electronic...

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Transition metals
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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 goes 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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3d anomalies: Cr: 4s 1 3d 5 (same in Mo); Cu: 4s 1 3d 10 (same in Ag and Au)
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Electron configuration in ions: 3d orbitals are lower than 4s! Thus, electrons are removed from 4s first. Example: Mn: [Ar]4s 2 3d 5 Mn 2+ : [Ar]3d 5
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KMnO 4 , potassium permanganate, is extremely strong oxidant 1. Rxn of KMnO 4 with HCl: KMnO 4 + HCl -> MnO 2 + Cl 2 + . ... 2. Oxidative properties of KMnO
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This note was uploaded on 07/22/2008 for the course CHEM 115b taught by Professor Reisler during the Spring '08 term at USC.

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L35_TransMetals2 - Transition metals Available Electronic...

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