How do you write oxidation reduction half reactions?

Writing oxidation-reduction (redox) half-reactions involves balancing the gain and loss of electrons that occur during the oxidation and reduction processes. Here's a step-by-step guide to writing them:

Steps to Write Redox Half-Reactions:
Identify the Oxidation and Reduction Reactions:

Oxidation: The reaction where a species loses electrons.
Reduction: The reaction where a species gains electrons.
Write the Unbalanced Half-Reactions:

Start with the oxidation half-reaction: Write the species that is oxidized and indicate the loss of electrons.
Then, write the reduction half-reaction: Write the species that is reduced and indicate the gain of electrons.
Balance the Atoms Except for Hydrogen and Oxygen:

Balance the atoms of each element except for hydrogen and oxygen in each half-reaction.
Balance Oxygen Atoms by Adding H₂O:

Add water molecules (H₂O) to balance oxygen atoms if necessary. Place them on the side that needs more oxygen atoms.
Balance Hydrogen Atoms by Adding H⁺ Ions:

Add hydrogen ions (H⁺) to balance hydrogen atoms if necessary. Place them on the side that needs more hydrogen atoms.
Balance Charge by Adding Electrons:

Add electrons (e⁻) to balance the charges on both sides of each half-reaction. Electrons are added to the side that has a higher positive charge to balance it with the side that has a higher negative charge.
Equalize the Number of Electrons in Both Half-Reactions:

Multiply the entire half-reactions by appropriate integers so that the number of electrons lost in the oxidation half-reaction equals the number gained in the reduction half-reaction.
Combine the Half-Reactions:

Add the balanced half-reactions together. The electrons should cancel out in the combined equation.