Redox reactions involve the transfer of electrons between atoms or molecules. During redox, oxidation and reduction occur simultaneously. Oxidation is the loss of electrons by an atom, increasing its oxidation state, while reduction is the gain of electrons by an atom, decreasing its oxidation state. Metals typically undergo oxidation by losing electrons, while nonmetals gain electrons through reduction. The oxidation states of elements in compounds can be determined based on established rules and used to balance redox reactions.

1. REDOX REACTIONS
Erick Martini andYeshua Pasarell

2. REDOX
 REDOX breaks up to reduction and oxidation.
These are very common types reactions.
 They involve the exchange of electrons, so
any ionic bond is made by a REDOX reaction.

3. Oxidation
 Oxidation happens when an atom loses
electrons and its oxidation number increases.
 In a REDOX reaction, metals are usually the
ones that oxidize.

4. Reduction
 Reduction is when an atom gains electrons
and its oxidation number reduces.
 In REDOX, nonmetals are the ones reduced.

5. Oxidation and Reduction
 These events always occur at the same time,
because when an atom is oxidized or loses
electrons, another one is reduced or gained
those electrons.

6. Oxidation Number
 The oxidation number of an element in a
compound is the charge of the individual
atom of that element in a compound.

7. Oxidation Number Rules
 Oxygen is always -2 except in peroxides, were it’s -1.
 Hydrogen is always +1 except in metallic bonds.
 An uncombined element is 0.
 Elements in groups 1 and 2 are +1 and +2.
 Aluminum is +3.
 The sum of the charges in a neutral compound is 0.
 The sum on the charges in a polyatomic ion is the
charge of the ion.

8. REDOX Balancing
 The REDOX balancing method uses the
oxidation number of the elements to balance
the reaction.

9. Balancing
 First, you write all the oxidation numbers of the
elements in the full reaction.
 Then, you see which one oxidized and which one
reduced.
 You write the amount of electrons won or lost.
 You make them equal with coefficients.
 You write that coefficient in the reaction in the
where the element is present.
 You finish balancing with the conventional method.

10. Activity!
Compound
Element
Ox.
Number
Ox.
Number
Renata’s Ripoff

11. CO2
C
+4 +2
5 Secs.

12. Fe3O2
Fe
+2 +3

13. SO4
2-
S
+6 +7

14. Ca3(PO4)2
P
+5 +6
10 Secs.

15. HNO3
N
+6 +5

16. (NH4)3PO4
N
-4 -3

17. NH4NO3
N
+5 -3

18. (H3O)2SO3
S
+4 +5