Given below are two statements:
Statement I: SO\(_2\) and H\(_2\)O both possess V-shaped structures.
Statement II: The bond angle of SO\(_2\) is less than that of H\(_2\)O. In the light of the above statements, choose the most appropriate answer from the options given below:
Given below are two statements:
Statement I: SO\(_2\) and H\(_2\)O both possess V-shaped structures.
Statement II: The bond angle of SO\(_2\) is less than that of H\(_2\)O. In the light of the above statements, choose the most appropriate answer from the options given below:
- Both Statements I and Statement II are incorrect
- Both Statement I and Statement II are correct
- Statement I is correct but Statement II is incorrect
- Statement I is incorrect but Statement II is correct
The Correct Option is C
Solution and Explanation
1. Statement I: Both SO\(_2\) and H\(_2\)O possess V-shaped (bent) structures due to the presence of lone pairs on the central atom. - SO\(_2\): The central sulfur atom forms two double bonds with oxygen and has one lone pair of electrons. - H\(_2\)O: The central oxygen atom forms two single bonds with hydrogen and has two lone pairs of electrons. Thus, this statement is correct.
2. Statement II: The bond angle of SO\(_2\) is approximately 119.5° (sp\(^2\) hybridization), while the bond angle of H\(_2\)O is 104.5° (sp\(^3\) hybridization). - The larger bond angle in SO\(_2\) is due to the greater repulsion caused by the double bonds in SO\(_2\), compared to the single bonds in H\(_2\)O. Thus, this statement is incorrect. \[ \text{SO}_2: \angle \text{O-S-O} \approx 119.5^\circ \quad \text{H}_2\text{O}: \angle \text{H-O-H} \approx 104.5^\circ \]
Conclusion: Statement I is correct, but Statement II is incorrect.
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