1. Oxidation/Reduction
Oxidation is the process whereby a reactant loses one or more electrons.
Reduction is the process whereby a reactant gains one or more electrons.
These two always occur together, you can not have on without the other.

2. The oxidizing agent is reduced.
The reducing agent is oxidized.

3. 2Na + Cl2  2NaCl 2Na  2Na+ + 2e- oxidation
Cl2 + 2e-  2Cl reduction
The above are called ½ reactions
Because Na causes the reduction of Cl2, the Na is acting as the reducing agent.
Because Cl2 causes the oxidation of Na, Cl2 is acting as the oxidizing agent.

4. Oxidation/Reduction Oxidation Ionic state becomes more positive.
Loses electrons.
Gains oxygen.
Loses hydrogen.
Reduction
Ionic state becomes more negative.
Gains electrons.
Loses oxygen.
Gains hydrogen.

5. CH4 + 2O2  2CO2 + 2H2O
Is carbon oxidized or reduced?
Why?

6. Black/White Film
The film is coated with a gel containing microcrystal's of AgBr.
Light causes the Br to oxidize.
Br-  Br + e- Oxidation
Ag+ + e-  Ag Reduction

7. Electrochemistry is the study of the relationship between electrical energy and chemical change.
Electrode is any material that conducts electrons into or out of a medium.

8. Voltaic cell
Voltaic cell is a set-up to harness electrical energy from an oxidation-reduction reaction.
A self contained voltaic cell is called a battery.

9. Type of batteries
Disposable battery has a relatively short life because the electron producing chemicals are consumed.