Which of the following species has a pyramida | vedclass

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(A) To determine the shape,we calculate the number of electron pairs around the central atom using the formula: $	ext{Number of electron pairs} = \fr

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$PCl_3$

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(A) To determine the shape,we calculate the number of electron pairs around the central atom using the formula: $	ext{Number of electron pairs} = \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.For $PCl_3$: $V=5$ (for $P$),$M=3$ (for $Cl$). $	ext{Electron pairs} = \frac{1}{2} [5 + 3] = 4$. This corresponds to $sp^3$ hybridization with one lone pair and three bond pairs,resulting in a pyramidal shape.For $SO_3$: $V=6$ (for $S$),$M=0$. $	ext{Electron pairs} = \frac{1}{2} [6] = 3$. This corresponds to $sp^2$ hybridization with zero lone pairs,resulting in a trigonal planar shape.For $CO_3^{2-}$: $V=4$ (for $C$),$M=0$,$A=2$. $	ext{Electron pairs} = \frac{1}{2} [4 + 2] = 3$. This corresponds to $sp^2$ hybridization,resulting in a trigonal planar shape.For $NO_3^-$: $V=5$ (for $N$),$M=0$,$A=1$. $	ext{Electron pairs} = \frac{1}{2} [5 + 1] = 3$. This corresponds to $sp^2$ hybridization,resulting in a trigonal planar shape.Therefore,only $PCl_3$ has a pyramidal shape.

Which of the following species has a pyramidal shape?

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