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Unformatted text preview: • Oxidation States – Recall from chapter 4 the rules for assigning oxidation states (in order to ID re/dox ½ rxns.) • Element by itself: ox # = 0 • Oxygen is -2 unless in H 2 O 2 or with more electroneg atom like F, Cl • H is +1 unless with metals like LiH • Groups I and II are +1, +2 (NaOH, MgCl 2 ) • Neutral compounds sum to 0; polyatomic ions sum to overall charge • Identifying oxidation and reduction ½ reactions (from unbalanced equation, description in words, line notation) ex/ If you had a flask filled with Cl 2 ( g ), and you introduced some molten Na ( s ), you’d see a violent reaction ( http://youtu.be/Ftw7a5ccubs ). Write out oxidation and reduction ½ reactions and sum to a balanced overall. • Balancing redox reactions • ID and write out oxidation and reduction ½ reactions • Achieve mass balance and charge balance for each • Use stoichiometry for atoms other than O and H • Assume acidic aqueous rxn – get O mass balance via H 2 O; get H mass balance via H + • Get charge balance by neutralizing + charge imbalance with added...
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This note was uploaded on 05/15/2011 for the course CHM 116 taught by Professor Matchett during the Fall '11 term at Grand Valley State University.
- Fall '11