Question

Which of the following statements is false about oxygen and sulphur?

• A. Atoms of oxygen and sulphur consist two unpaired electrons in valence shell.
• B. Oxygen and sulphur show -2, +4 and +6 oxidation states.
• C. Oxygen is gas while sulphur is solid at room temperature.
• D. Hydride of oxygen is more stable than hydride of sulphur.

Hint:

The absence of vacant d-orbitals is the primary reason why second-period elements (N, O, F) exhibit anomalous behavior compared to their heavier group members! Oxygen's maximum covalency is restricted strictly to 4.

Answer 1

The Correct Option is B

Step 1: Understanding the Concept:
Oxygen and Sulphur belong to Group 16. While they share similar valence electron counts, their chemistry differs due to the absence of d-orbitals in oxygen.

Step 2: Formula Application:
Electronic configuration: Oxygen ($2s^2 2p^4$): No d-orbitals. Sulphur ($3s^2 3p^4 3d^0$): Vacant d-orbitals available.

Step 3: Explanation:
Oxygen cannot show +4 and +6 oxidation states because it lacks d-orbitals to expand its octet. It primarily shows -2 (except in $OF_2$ and peroxides). Sulphur, however, can expand its valency to show +4 and +6.

Step 4: Final Answer:
Statement (b) is false because oxygen does not exhibit +4 and +6 oxidation states.