Metal Displacement Reactions
The Dance Partner Bully — when a stronger metal crashes the party.
🎭 The Analogy
Imagine Copper is happily dancing with Sulfate in a blue solution. Then Zinc walks in — stronger, more reactive, desperate to bond. Zinc shoves Copper aside, grabs Sulfate, and poor Copper is ejected onto the floor as a brown solid. The solution turns colourless. That's displacement.
⚗️ Virtual Lab — Watch the Reaction
🔮 Displacement Predictor
Based on the Reactivity Series: K › Na › Ca › Mg › Al › Zn › Fe › Pb › H › Cu › Ag › Au
🔬 Net Ionic Equation Builder
Watch how we strip the spectator ion to reveal the REAL electron transfer.
Full Ionic Equation
Start with all ions in solution.
Zn(s) + Cu²⁺(aq) + SO₄²⁻(aq) → Zn²⁺(aq) + SO₄²⁻(aq) + Cu(s)
⚡ Redox Analysis — Who Loses, Who Gains?
⚠️ Examiner Traps — Don't Lose Marks!
- ❌ "Zinc is more reactive so it reacts" — too vague. Say: "Zinc displaces copper because zinc is higher in the reactivity series and loses electrons more readily."
- ❌ Forgetting state symbols — always write (s), (aq), (g), (l) in equations.
- ❌ Saying the solution "turns colourless" without explaining WHY — say: "Blue colour fades as Cu²⁺ ions are removed from solution."
- ❌ Calling copper deposit "rust" or "red solid" — it is a brown solid (pure copper).
- ❌ Confusing oxidation and reduction — remember OIL RIG: Oxidation Is Loss, Reduction Is Gain.
📋 Key Summary
A more reactive metal displaces a less reactive metal from its aqueous salt solution. In Zn + CuSO₄, the blue colour fades (Cu²⁺ removed), a brown solid forms (Cu deposited), and zinc dissolves (Zn²⁺ formed). Zinc is oxidised (loses electrons); copper ions are reduced (gain electrons). The net ionic equation strips the spectator ion SO₄²⁻ to reveal the true electron transfer: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s).
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