Level 1 – Basic Recall (1–10)

1. What are s-block elements?

2. Which groups belong to the s-block?

3. State the general electron configuration of Group 1.

4. State the general electron configuration of Group 2.

5. Name any three alkali metals.

6. Name any three alkaline earth metals.

7. State the oxidation states of Group 1 and 2 elements.

8. Why are alkali metals stored in oil?

9. Write the equation for sodium + water.

10. State one physical property common to all Group 1 metals.

Level 2 – Understanding (11–20)

11. Explain why Group 1 metals increase in reactivity down the group.

12. Compare Group 1 and Group 2 in terms of hardness.

13. Explain why Group 2 metals have higher melting points than Group 1.

14. Why do Group 1 compounds tend to be highly soluble?

15. Describe the trend in solubility of Group 2 hydroxides.

16. Describe the trend in solubility of Group 2 sulfates.

17. Why do Group 2 carbonates decompose more easily than Group 1 carbonates?

18. Explain why magnesium reacts slowly with cold water.

19. Why are ionic compounds formed by Group 1 metals usually white solids?

20. Explain why beryllium shows anomalous properties.

Level 3 – Application (21–30)

21. Write the balanced equation for potassium burning in oxygen.

22. Predict the reactivity of Rb compared to Na.

23. Explain why lithium carbonate decomposes easily on heating.

24. Compare flame colours of Li, Na, K.

25. Predict the solubility trend for Group 2 sulfates using ionic radius.

26. Write the reaction: CaO + H₂O → ?

27. Explain why Mg²⁺ forms more stable complexes than Ca²⁺.

28. Use Fajan’s rules to compare polarising power of Group 1 vs Group 2.

29. Predict whether MgCO₃ or BaCO₃ decomposes more easily.

30. Explain why alkali metals form strong alkaline hydroxides.

Level 4 – Analysis (31–40)

31. Analyse the trend in hydration enthalpies of Group 1 ions.

32. Compare the thermal stability of nitrates in Group 1 vs Group 2.

33. Discuss how the large ionic radius of Cs⁺ affects its chemistry.

34. Explain why BeCl₂ shows covalent character while BaCl₂ is ionic.

35. Predict lattice enthalpy changes down Group 2.

36. Compare electronegativities of Group 1 vs Group 2.

37. Analyse reactivity trends using ionisation energy.

38. Explain why alkali metals form peroxides and superoxides down the group.

39. Compare trends in flame colours with ionization energy.

40. Explain the diagonal relationship between lithium and magnesium.

Level 5 – Exam/Challenge (41–50)

41. Predict the effect of increasing nuclear charge on Group 2 solubility.

42. Explain the anomalous behaviour of lithium in terms of polarising power.

43. Discuss the stability of bicarbonates in Group 2.

44. Compare the chemistry of Na⁺ and K⁺ in biological systems.

45. Explain how size/charge ratio affects Group 2 carbonate stability.

46. Justify why Ca²⁺ hardens water but Na⁺ does not.

47. Predict whether Mg(OH)₂ or Ba(OH)₂ is more basic.

48. Analyse the energetics of thermal decomposition of Group 1/2 nitrates.

49. Evaluate why Group 2 metals act as better reducing agents than Group 1 in some reactions.

50. Use periodic trends to justify differences between s-block and p-block reactivity.