Consider a galvanic cell in which Al 3 + Al3+ is reduced to elemental aluminum and magnesium metal is oxidized to Mg 2 + Mg2+ . Write the balanced half-cell reactions that take place at the cathode and at the anode.

Anode:

3Mg(s) > 3Mg2+(aq) + 6e

Cathode:

2Al3+(aq) +6e > 2Al(s)

Explanation:

Anode:

3Mg(s) > 3Mg2+(aq) + 6e

Cathode:

2Al3+(aq) +6e > 2Al(s)

Magnesium is more electro positive than aluminum hence it functions as the anode. Six electrons are lost/gained in the redox process as shown in the oxidation and reduction half reaction equations above. Magnesium is oxidized to magnesium ion while aluminum is reduced to elemental aluminum.

it takes on an electronical energy