Question

Assertion :Bond angle of $H_{2}S$ is smaller than $H_{2}O$. Reason: As the electronegativity of the central atom increases, bond angle decreases.

• A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
• B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
• C. Assertion is correct but Reason is incorrect
• D. Both Assertion and Reason are incorrect

Answer 1

The correct option is C Assertion is correct but Reason is incorrect

Bond angle of $H_{2}S\left({92}^o\right)<H_{2}O\left({104}^{o}31\right)$.

As the electronegativity of the central atom decreases, bond angle decreases. In the present case, $S$ is less electronegative than oxygen. Thus bond pairs in $H_{2}S$ are more away from the central atom than in $H_{2}O$ and thu,s repulsive forces between bond pairs are smaller producing smaller bond angle.

Hence, assertion is correct but reason is incorrect.