# Redox Equation and Half equation

2Mg+ O_{2} → 2MgO

0 0 +2 -2

The diagram above shows that Mg to Mg ^{2}+ is oxidation (reducing agent)

O_{2} to O^{2}– reduction occurs (oxidizing agent)

Half equation

Some reactions maybe written in 2 halves (the oxidation half and the reduction half). The 2 parts are called the half equations.

2Mg+ O_{2} → 2MgO

**Oxidation ** ** reduction **

2Mg -4e- → 2Mg^{2}+ O_{2} +4e- → 2O^{2}–

Electrons are lost electrons are gained

Redox Reaction

Zn + CuSO_{4 }→ ZnSO_{4} +Cu

0 +2 +2 0

Half equations

Oxidation: Zn -2e- → Zn ^{2}+ reducing agent

Reduction: Cu ^{2}+ +2e- → Cu oxidizing agent

Try:

Zn + H_{2}SO_{4 } → ZnSO_{4} +H_{2}