Zinc metal; copper (II) sulfate solution

(a) Molecular equation:

(b) Total ionic equation:

(c) Net ionic equation:

A = Zn (s) + CuSO₄ (aq) → ZnSO₄ (aq) + Cu (s)

B = Zn (s) + Cu²⁺ (aq) + SO₄²⁻ (aq) → Zn²⁺ (aq) + SO₄²⁻ (aq) + Cu (s)

C = Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)

Explanation:

The reactivity of zinc is higher than than copper. That's why when zinc is added into the copper (ii) sulfate it displace the copper and form zinc sulfate solution.

Molecular equation:

Zn (s) + CuSO₄ (aq) → ZnSO₄ (aq) + Cu (s)

It is redox reaction. The copper is reduced because its oxidation number reduced from + 2 to zero and zinc is oxidize its oxidation state increase from zero to + 2.

Ionic equation:

Zn (s) + Cu²⁺ (aq) + SO₄²⁻ (aq) → Zn²⁺ (aq) + SO₄²⁻ (aq) + Cu (s)

Net ionic equation:

Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)

The SO₄²⁻ are spectator ions that's why these are not written in net ionic equation.

Spectator ions:

These ions are same in both side of chemical reaction. These ions are cancel out. Their presence can not effect the equilibrium of reaction that's why these ions are omitted in net ionic equation.