Level 1 – Basic Recall (1–10)

1. What are p-block elements?

2. Which groups belong to the p-block?

3. Name any three halogens.

4. Name two noble gases.

5. What are allotropes?

6. Give two allotropes of carbon.

7. State the oxidation state of halogens.

8. What is the electron configuration of Group 17?

9. Name one acidic oxide from the p-block.

10. List one property of halogens.

Level 2 – Understanding (11–20)

11. Explain why halogens are good oxidising agents.

12. Describe a halogen displacement reaction.

13. Why does reactivity decrease down Group 17?

14. Explain why noble gases are inert.

15. Compare acidic strength of HF, HCl, HBr and HI.

16. Explain why F₂ is the strongest oxidizing agent among halogens.

17. Why does metallic character increase down the groups?

18. Describe the structure of graphite.

19. Explain why CO₂ is an acidic oxide.

20. Describe thermal stability trends of hydrogen halides.

Level 3 – Application (21–30)

21. Predict whether Cl₂ will displace I₂ from KI solution.

22. Explain why SiO₂ is a giant covalent structure.

23. Compare bonding in diamond vs silicon.

24. Write the reaction between SO₂ and water.

25. Predict whether SO₃ or SO₂ is a stronger acid anhydride.

26. Explain the use of helium in balloons.

27. Predict the observation when chlorine is passed through KI solution.

28. Compare the volatility of Group 17 elements using Van der Waals forces.

29. Explain why aluminium oxide is amphoteric.

30. Write the reaction: P₄O₁₀ + H₂O → ?

Level 4 – Analysis (31–40)

31. Analyse the inert pair effect in Group 13 and 14.

32. Explain why nitrogen forms stable covalent bonds but phosphorus forms P₄.

33. Compare oxidation states in Group 14 elements.

34. Evaluate the acidity of oxides across Period 3.

35. Predict the structure of XeF₆ using VSEPR theory.

36. Explain why HF has unusually high boiling point.

37. Analyse the trend in oxidizing ability of halogens.

38. Explain why BCl₃ is a Lewis acid.

39. Compare thermal stability of carbonates in Group 14.

40. Evaluate how electron shielding affects p-block reactivity.

Level 5 – Exam/Challenge (41–50)

41. Explain why ICl₅ forms despite iodine being less electronegative than chlorine.

42. Predict the shapes of various p-block molecules using hybridization.

43. Analyse halogen displacement reactions using electrode potentials.

44. Explain bonding in ozone using resonance.

45. Compare acidity of H₂SO₃ vs H₂SO₄ using oxidation states.

46. Justify why SiO₂ is insoluble in water while CO₂ dissolves easily.

47. Explain the trend in basicity of amines across the p-block.

48. Predict the stability of higher oxidation states in heavier p-block elements.

49. Analyse environmental impacts of NO₂ and SO₂ using redox chemistry.

50. Evaluate why Group 15 hydrides show decreasing stability down the group.