Oxidation and Reduction Subtitle

Definition Oxidation Reduction Reaction (Redox): A reaction in which electrons are transferred from one substance to another.

Definition of Redox Reaction Oxidation cannot occur without reduction Definition of Oxidized: 1. Losing of electrons (LEO) 2. Increasing the ox. number, ie: 0 to +1 -2 to -1 3. Gaining oxygen Definition of Reduced: 1. Gaining of electrons (GER) 2. Reducing the ox. number, ie: -1 to -2 1 to 0 3. Losing oxygen Becoming more positive Becoming more negative

LEO goes GER Oxidation Reduction Is Is Losing Gaining

Example of an electron transfer reaction 2Mg + O2  2MgO Mg atom transfers two electrons to each oxygen atom. As a result 2 Mg atoms become Mg2+ and two oxygen atoms become O2- Mg loses two electrons O gains two electrons

Example of an electron transfer reaction

Examples of Oxidation Reduction When an electron is lost (An electron is found on the product side) there is oxidation X0  X+1 + e- When an electron is gained (An electron is found on the reactant side) there is reduction e- +Y+1  Y0

Examples: +1e- (LEO)oxidized 1e-+ (GER)reduced +1e- (LEO)oxidized start finish Ex5 Na0Na+1 Ex6 Fe+3Fe+2 Ex7 N+1N+2 Ex8 Mg+2Mg0 +1e- (LEO)oxidized 1e-+ (GER)reduced +1e- (LEO)oxidized (GER)reduced 2e-+

Vocabulary Whatever is oxidized is called the reducing agent Whatever is reduced is called the oxidizing agent

Real Examples: oxidized +1e- reducing agent reduced 1e-+ start finish Ex5 Na0Na+1 Ex6 Fe+3Fe+2 Ex7 N+1N+2 Ex8 Mg+2Mg0 oxidized +1e- reducing agent reduced 1e-+ oxidizing agent oxidized +1e- reducing agent reduced 2e-+ oxidizing agent