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REDOX REACTIONS
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Oxidation-Reduction reactions• A reaction in which electrons are transferred from one atom to another
• Chemists often refer to oxidation-reactions as redox reactions
• Example: • Complete chemical equation: • 2 KBr (aq) + Cl2 (aq) 2 KCl (aq) + Br2 (aq)• Net ionic Equation: 2Br- (aq) + Cl2 (aq) Br2 (aq) + 2 Cl-
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Vocabulary• Half reactions- part of the redox reaction where it shows either
the oxidation reaction or the reduction reaction• Electrons are usually present in either side of the half reaction• Oxidation half-reactions has electrons on the product side (losing
electrons)• Reduction half-reactions has electrons on the reactant side (gaining
electrons)
• Oxidizing agent- a chemical species that Accepts (gains) electrons from an oxidized species• Reducing species = Oxidizing agent
• Reducing agent- a chemical species that Donates (lose) electrons from a reduced species• Oxidizing species = Reducing agent
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Oxidation Reactions• Oxidation is defined as the loss of electrons from atoms of a substance• Reactions that LOSE ELECTRONS (LEO- “Loss of Electrons”-Oxidation)
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Reduction Reactions• Reactions that GAIN ELECTRONS (GER- “Gaining Electrons- Reduction)
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Practice: • Identify as oxidation or reduction
1. Al → Al3+ + 3e-
2. Cu2+ + e- → Cu+
3. Fe3+ → Fe2+