1. Oxidation and Reduction
Subtitle

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

3. 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

4. LEO goes GER
Oxidation Reduction
Is Is
Losing Gaining

5. 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

6. Example of an electron transfer reaction

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

8. 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-+

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

10. Real Examples: oxidized +1e- reducing agent reduced 1e-+
start finish
Ex 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