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Step 2: Write the oxidation and reduction half-reactions.
Step 3: Balance the atoms in each half-reaction.
Step 4: Balance the charges in each half-reaction.
Step 5: Make sure that the number of electrons lost in oxidation equals the number of electrons gained in reduction. (Multiply by a coefficient.)
Use oxidation numbers to determine which element was oxidized and which element was reduced.
Write the oxidation and reduction half-reactions. (You may need to break apart any compounds that contain either of the elements undergoing oxidation or reduction.)
Oxidation half-reaction:
Na → Na + e− Reduction half-reaction: Br2 + e− → Br
Balance the atoms in each half-reaction. The sodium atoms are balanced. The bromine atoms need to be balanced.
Na → Na + e−
Br2 + e− → 2Br
Balance the charges in each half-reaction. The sodium charges are balanced. The bromine charges need to be balanced.
Na → Na + e−
Br2 + 2e− → 2Br
Make sure that the number of electrons lost in oxidation equals the number of electrons gained in reduction. Do this by multiplying by a coefficient, in this case 2, so that the number of electrons lost by sodium equals the number of electrons gained by bromine.
2Na → 2Na + 2e−
Br2 + 2e− → 2Br
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