The species having pyramidal shape is

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(A) To determine the shape,we calculate the hybridization and number of lone pairs using the formula: $H = \frac{1}{2}(V + M - C + A)$,where $V$ is th

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$SO_3^{2-}$

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(A) To determine the shape,we calculate the hybridization and number of lone pairs using 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 $SO_3^{2-}$: $H = \frac{1}{2}(6 + 0 - 0 + 2) = 4$ ($sp^3$ hybridization). It has $3$ bond pairs and $1$ lone pair,resulting in a pyramidal shape.$2$. For $SO_3$: $H = \frac{1}{2}(6 + 0 - 0 + 0) = 3$ ($sp^2$ hybridization). It has $3$ bond pairs and $0$ lone pairs,resulting in a trigonal planar shape.$3$. For $CO_3^{2-}$: $H = \frac{1}{2}(4 + 0 - 0 + 2) = 3$ ($sp^2$ hybridization). It has $3$ bond pairs and $0$ lone pairs,resulting in a trigonal planar shape.$4$. For $ClF_3$: $H = \frac{1}{2}(7 + 3 - 0 + 0) = 5$ ($sp^3d$ hybridization). It has $3$ bond pairs and $2$ lone pairs,resulting in a $T$-shaped geometry.Therefore,the species with a pyramidal shape is $SO_3^{2-}$.

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