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Redox REactions

Redox REactions. 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 ) + Cl 2 ( aq )  2 KCl ( aq ) + Br 2 ( aq )

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Redox REactions

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  1. Redox REactions

  2. 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-

  3. 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

  4. Oxidation Reactions • Oxidation is defined as the loss of electrons from atoms of a substance • Reactions that LOSE ELECTRONS (LEO- “Loss of Electrons”-Oxidation)

  5. Reduction Reactions • Reactions that GAIN ELECTRONS (GER- “Gaining Electrons- Reduction)

  6. Practice: • Identify as oxidation or reduction • Al → Al3+ + 3e- • Cu2+ + e- → Cu+ 3. Fe3+ → Fe2+

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