1. Oxidation Reduction Chemisty: Redox Chemistry
Oxidation and Reduction reactions always take place simultaneously.
Loss of electrons – oxidation (Increase in Oxidation Number)
Ex:Na > Na+1 + e-1
Gain of electrons - reduction ( Decrease in Oxidation Number)
Cl2 + 2 e > 2 Cl-1

3. Oxidation occurs when a molecule does any of the following:  
Loses electrons
Loses hydrogen
Gains oxygen
If a molecule undergoes oxidation, it has
been oxidized and it is the reducing agent
(aka reductant).

4. Reduction occurs when a molecule does any of the
following:
Gains electrons
Gains hydrogen
Loses oxygen
If a molecule undergoes reduction, it has been reduced and it is the oxidizing agent (aka oxidant).

6. zinc is being oxidized while the copper is being reduced. Why?

7. Redox reactions involve electron transfer:
Lose e - =Oxidation
Cu (s) + 2 Ag + (aq) Cu 2+ (aq) + 2 Ag(s)
Gain e - =Reduction

8. Oxidation Numbers Rules for Assigning Oxidation States
The oxidation state of an atom in an uncombined element is 0.
The oxidation state of a monatomic ion is the same as its charge.
Oxygen is assigned an oxidation state of –2 in most of its covalent compounds. Important exception: peroxides (compounds containing the O2 2- group), in which each oxygen is assigned an oxidation state of –1)
In its covalent compounds with nonmetals, hydrogen is assigned an oxidation state of +1
For a compound, sum total of ON s is zero.
For an ionic species (like a polyatomic ion), the sum of the oxidation states must equal the overall charge on that ion.

9. Redox: Reduction occurs when an atom gains one or more electrons. Ex:
Oxidation occurs when an atom or ion loses one or more electrons.
LEO goes GER
Copper metal reacts with silver nitrate to form silver metal and copper nitrate:
Cu + 2 Ag(NO3)  2 Ag + Cu(NO3)2.

10. Identifying OX, RD, SI Species
Ca0 + 2 H+1Cl-1  Ca+2Cl-12 + H20
Oxidation = loss of electrons. The species becomes more positive in charge. For example, Ca0  Ca+2, so Ca0 is the species that is oxidized.
Reduction = gain of electrons. The species becomes more negative in charge. For example, H+1  H0, so the H+1 is the species that is reduced.
Spectator Ion = no change in charge. The species does not gain or lose any electrons. For example, Cl-1  Cl-1, so the Cl-1 is the spectator ion.

11. Writing Half-Reactions
Ca0 + 2 H+1Cl-1  Ca+2Cl-12 + H20
Oxidation: Ca0  Ca+2 + 2e-
Reduction: 2H+1 + 2e-  H20
The two electrons lost by Ca0 are gained by the two H+1 (each H+1 picks up an electron).
PRACTICE SOME!

12. Practice Half-Reactions
Don’t forget to determine the charge of each species first!
4 Li + O2  2 Li2O
Oxidation Half-Reaction:
Reduction Half-Reaction:
Zn + Na2SO4  ZnSO4 + 2 Na