In which of the following species is the hybr | vedclass

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(A) To determine the hybridization of the central atom,we use the formula: $H = \frac{1}{2}(V + M - C + A)$,where $V$ is the number of valence electro

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$SO_2, SO_3$

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(A) To determine the hybridization of the central atom,we use the formula: $H = \frac{1}{2}(V + M - C + A)$,where $V$ is the number of valence electrons,$M$ is the number of monovalent atoms,$C$ is the cationic charge,and $A$ is the anionic charge.$1$. For $SO_2$: $V=6, M=0$. $H = \frac{1}{2}(6+0) = 3$ ($sp^2$ hybridization).$2$. For $SO_3$: $V=6, M=0$. $H = \frac{1}{2}(6+0) = 3$ ($sp^2$ hybridization).$3$. For $SO_4^{2-}$: $V=6, M=0, A=2$. $H = \frac{1}{2}(6+2) = 4$ ($sp^3$ hybridization).$4$. For $SO_3^{2-}$: $V=6, M=0, A=2$. $H = \frac{1}{2}(6+2) = 4$ ($sp^3$ hybridization).$5$. For $CH_4$: $V=4, M=4$. $H = \frac{1}{2}(4+4) = 4$ ($sp^3$ hybridization).$6$. For $HCOOH$: The central carbon atom is bonded to $H$,$OH$,and double-bonded to $O$. It has $3$ sigma bonds and $0$ lone pairs,so $H=3$ ($sp^2$ hybridization).Comparing the options:$A$. $SO_2$ $(sp^2)$ and $SO_3$ $(sp^2)$. Both have the same hybridization.Therefore,the correct option is $A$.

In which of the following species is the hybrid state of the central atom the same?

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