Level 1 — Basic Recall (1–10)

1. What is oxidation?

2. What is reduction?

3. Define redox reaction.

4. What is an oxidizing agent?

5. What is a reducing agent?

6. State the oxidation number of oxygen in most compounds.

7. State the oxidation number of hydrogen in most compounds.

8. What is an electrolytic cell?

9. What is a galvanic (voltaic) cell?

10. Define electrode.

Level 2 — Understanding (11–20)

11. Explain why oxidation and reduction always occur together.

12. Distinguish between oxidation number and charge.

13. Explain the purpose of a salt bridge in a galvanic cell.

14. Why is the anode negative in a galvanic cell?

15. Why is the anode positive in an electrolytic cell?

16. Describe how electrons flow in an electrochemical cell.

17. Explain the term “standard electrode potential (E°).”

18. Why does a more positive E° value indicate a stronger oxidizing agent?

19. Explain how concentration affects cell voltage (conceptual).

20. Why do electrolytic cells require an external power supply?

Level 3 — Application (21–30)

21. Assign oxidation numbers to nitrogen in NH₃, NO₂, and NO₃⁻.

22. Balance a redox equation using the ion–electron method.

23. Predict the anode and cathode in a Zn–Cu galvanic cell.

24. Write the half-equations for the Daniell cell (Zn/Cu).

25. Calculate the cell potential using given E° values.

26. Predict whether a redox reaction is spontaneous using E° values.

27. Determine which ion is discharged first during electrolysis of aqueous NaCl.

28. Predict products of electrolysis of molten PbBr₂.

29. Identify the oxidizing agent in a given reaction.

30. Write the overall cell reaction for Mg|Mg²⁺ || Cu²⁺|Cu.

Level 4 — Analysis (31–40)

31. Analyse why concentration changes shift electrode potentials.

32. Compare galvanic and electrolytic cells in terms of function and electron flow.

33. Explain selective discharge of ions using electrode potentials.

34. Analyse how electroplating works using electrochemistry principles.

35. Predict the effect of mixing solutions of ions with different E° values.

36. Compare strengths of oxidizing agents using E° tables.

37. Analyse why water is often reduced/oxidized instead of electrolytes in aqueous solutions.

38. Evaluate the effect of increasing or decreasing ion concentration on EMF.

39. Explain how standard hydrogen electrode is used as reference.

40. Compare metals' positions in the electrochemical series with their reactivity.

Level 5 — Exam/Challenge (41–50)

41. Use E° values to determine feasibility of a complex redox reaction.

42. Derive the full balanced redox equation from given half-equations.

43. Explain corrosion of iron using electrochemical principles.

44. Evaluate methods of corrosion prevention (galvanizing, sacrificial protection).

45. Predict cell potential under non-standard conditions qualitatively using Nernst effect.

46. Calculate EMF of a cell using the formula E°cell = E°cathode – E°anode.

47. Analyse a concentration cell and explain how EMF is generated.

48. Predict products of electrolysis in a multi-ion mixture.

49. Explain the role of ligands on altering electrode potentials (qualitative).

Evaluate industrial applications of electrochemistry (electrolysis of brine, metal purification, batteries).