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Review: Balancing Redox Reactions

1 review : Balancing Redox Reactions Determine which species is oxidizedand which species is reduced Oxidation corresponds to an increase inthe oxidation number of an element Reduction corresponds to a decrease inthe oxidation number of an element Write half Reactions for oxidation andreduction processes Oxidation reaction will have e- s on theright side of equation Reduction reaction will have e- s on theleft side of the equationReview: Balancing Redox Reactions Balance half Reactions includingcharge balance Multiply each half reaction by a factorso that the total number of e- stransferred in each reaction are equal Add the resulting half reactionstogether to get the overall balancedredox equation2 review : Balancing Redox ReactionsExample:F2(g) + Al(s) F-(aq) + Al3+(aq)oxid. state 0 0 -1 +3 Fluorine is reduced (0 -1)Aluminum is oxidized (0 +3) Half Reactions :oxidation:Al(s) Al3+(aq) + 3 e-reduction:F2(g) + 2 e- 2 F-(aq) review : Balancing Redox ReactionsExample:F2(g) + Al(s) F-(aq) + Al3+(aq) Balance e- s transferred:multiply oxidation rxn by 22 Al(s) 2 Al3+(aq) + 6 e-multiply reduction rxn by 33 F2(g) + 6 e- 6 F-(aq) Add half reaction to get net reaction:2 Al(s) + 3 F2(g) 2 Al3+(aq) + 6 F-(aq) Check atom and charge balance:3 review : Balancing Redox ReactionsEx

Balancing Redox Reactions Balance half reactions including charge balance Multiply each half reaction by a factor so that the total number of e-’s transferred in each reaction are equal Add the resulting half reactions together to get the overall balanced redox equation. 2 Review:

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