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

If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion

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If Assertion is correct but Reason is incorrect

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Assertion is correct but Reason is incorrect

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If Assertion is incorrect but Reason is correct

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Solution

The correct option is C Assertion is correct but Reason is incorrect
Bond angle of $H_{2} S (92^{o}) < H_{2} O (104^{o} 31)$ .
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 thus repulsive forces between bond pairs are smaller producing smaller bond angle.

Thus, Assertion is correct but Reason is incorrect

Hence, the correct option is $C$

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Similar questions

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Assertion :Bond angle of H2S is smaller than H2O. Reason: Electronegativity of the central atom increases, bond angle decreases.

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