Can someone teach me how to balance redox reactions?

Balancing Oxidation-Reduction Half-Equations:
The process of writing fully balanced oxidation-reduction equations must be split into two separate half equations.
One half-equation is used to show the oxidising processes, while the other is used to show the reducing processes.
- The reduction half-equation shows the oxidant being reduced to a product.
- The oxidation half-equation shows the reductant being oxidised to a product. Half-Equations are written and balanced using the following method:
- The reactant is shown changing to its product:
Reactant Product
- The species undergoing the change in ON is balanced.
- The oxygen atoms in the reaction are balanced by adding water to the side opposite of the oxygen atoms.
- The hydrogen atoms in the reaction are balanced by adding hydrogen ions to the side opposite the hydrogen atoms.
- The charge in the reaction is balanced by adding electrons the most positive side.

Balancing Oxidation-Reduction Full-Equations:
Oxidation-Reduction Full equations are made by merging two half-equations together; the oxidation half-equation and the reduction half-equation.
Full-Equations are written using the following method:
- Either one or both of the half-equations must be multiplied by a number(s) so that the amount of electrons in both equations is the same. The number(s) used must be chosen so that the amount of products and reactants in the equations are as simplified as possible.
- The two half-equations are merged together so that the reactants and products of both equations are on the same sides of the full-equation.
- The ions, molecules and electrons that are common to both sides are canceled.
- As a final check, the charges, ions and molecules of both sides of the full-equation are checked to see if they equal.

not sure of the oxidation state method though

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Can someone teach me how to balance redox reactions?

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