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) + Cl 2 (aq)  2 KCl (aq) + Br 2 (aq) Net ionic Equation: 2Br - (aq) + Cl 2 (aq)  Br 2 (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 1.Al → Al 3+ + 3e- 2.Cu 2+ + e- → Cu + 3. Fe 3+ → Fe 2+