The species having a pyramidal shape is

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(D) To determine the shape,we calculate the hybridization and number of lone pairs for each species:$1$. $SO_3$: The central $S$ atom has $3$ bond pai

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$OSF_2$

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(D) To determine the shape,we calculate the hybridization and number of lone pairs for each species:$1$. $SO_3$: The central $S$ atom has $3$ bond pairs and $0$ lone pairs. It has $sp^2$ hybridization and a trigonal planar shape.$2$. $BrF_3$: The central $Br$ atom has $3$ bond pairs and $2$ lone pairs. It has $sp^3d$ hybridization and a $T$-shaped geometry.$3$. $SiO_3^{2-}$: The central $Si$ atom has $3$ bond pairs and $0$ lone pairs. It has $sp^2$ hybridization and a trigonal planar shape.$4$. $OSF_2$ (Thionyl fluoride): The central $S$ atom has $3$ bond pairs (one double bond to $O$ and two single bonds to $F$) and $1$ lone pair. The total steric number is $4$ ($3$ bond pairs + $1$ lone pair),which corresponds to $sp^3$ hybridization. Due to the presence of one lone pair,the geometry is pyramidal.

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