Test 4 review - Ch 19 Test 4 Review Suggestions(quiz 4 review suggestions(typos corrected and some additional suggestions Oxidation States Recall

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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 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 e - Multiply thru as needed to get e - on product side (ox) to equal e - on reactant side (red) Sum to get balanced overall, simplifying where possible If specified as in basic solution: neutralize any H + with an equal # of OH - (added to both sides); simplify ex/ Write out oxidation and reduction ½ reactions for the following to get a balanced overall in basic conditions MnO 4 - + I - MnO 2 + I 2 ex/ Write out oxidation and reduction ½ reactions for the following to get a balanced overall in acidic conditions
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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.

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Test 4 review - Ch 19 Test 4 Review Suggestions(quiz 4 review suggestions(typos corrected and some additional suggestions Oxidation States Recall

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