Question

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:

• A. Both Statements I and Statement II are incorrect
• B. Both Statement I and Statement II are correct
• C. Statement I is correct but Statement II is incorrect
• D. Statement I is incorrect but Statement II is correct

Answer 1

The Correct Option is C

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.