Foundation Level (Fail → Pass)

1. Define oxidation and reduction in simple terms.

2. State what happens at the anode and the cathode.

3. Identify the direction of electron flow in a galvanic cell.

4. What is a salt bridge and why is it needed?

5. Define redox reaction.

6. Give one example of an oxidation half‑equation.

7. State one example of a reduction half‑equation.

8. What is a galvanic (voltaic) cell?

9. What is an electrolytic cell?

10. State the meaning of E° (standard electrode potential).

Intermediate Level (Pass → Credit)

1. Write the balanced half‑equations for Zn/Cu electrochemical cell.

2. Explain how a salt bridge maintains electrical neutrality.

3. Calculate E°cell from given half‑cell potentials.

4. Explain how concentration affects electrode potential.

5. Compare galvanic and electrolytic cells.

6. Explain the role of inert electrodes.

7. Use the electrochemical series to predict spontaneity.

8. Write the overall redox equation for a given cell.

9. Explain what happens to mass of electrodes during electrolysis.

10. State Faraday’s First Law of Electrolysis.

Advanced Level (Credit → Distinction)

1. Derive E°cell using reduction potentials.

2. Use the Nernst equation to calculate electrode potential.

3. Explain how temperature affects redox equilibria.

4. Analyse the mechanism of metal deposition during electroplating.

5. Predict reaction feasibility using E° values and Gibbs energy.

6. Compare different types of industrial electrochemical cells.

7. Evaluate competing electrode reactions in aqueous electrolysis.

8. Interpret complex cell diagrams with multiple half‑cells.

9. Assess the effect of pH on electrode potential.

10. Design an experiment to measure an unknown metal’s electrode potential.