Consider the redox reaction below.

Mg (s) + Fe2 + (aq) - >Mg2 + (aq) + Fe (s)

Which equation is a half reaction that describes the reduction that is taking place?

Fe2 + (aq) + 22 - > Fe (s)

Mg (s) - Mg2 + (aq) + 2e

Fe2 + (aq) - >Fe (s) + 2e-

Mg (s) + 2e--> Mg2 + (aq)

Fe2 + (aq) + 2e - > Fe (s)

Explanation:

Oxidation:

Oxidation involve the removal of electrons and oxidation state of atom of an element is increased.

Reduction:

Reduction involve the gain of electron and oxidation number is decreased.

Consider the following reaction:

Mg (s) + Fe2 + (aq) - >Mg2 + (aq) + Fe (s)

Magnesium loses its two valance electrons and oxidized while iron accept two electrons get reduced.

Magnesium is reducing agent while iron is oxidizing agent.

Oxidizing agents:

Oxidizing agents oxidize the other elements and itself gets reduced.

Reducing agents:

Reducing agents reduced the other element are it self gets oxidized.