The hybridization of the central atom of ClF_ | vedclass

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(B) To determine the hybridization,we calculate the steric number $(SN)$ using the formula: $SN = 	ext{number of sigma bonds} + 	ext{number of lone

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$sp^3d, sp^3, sp^2$

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(B) To determine the hybridization,we calculate the steric number $(SN)$ using the formula: $SN = 	ext{number of sigma bonds} + 	ext{number of lone pairs}$.$1$. For $ClF_3$: The central atom $Cl$ has $3$ bond pairs and $2$ lone pairs. $SN = 3 + 2 = 5$,which corresponds to $sp^3d$ hybridization.$2$. For $NH_3$: The central atom $N$ has $3$ bond pairs and $1$ lone pair. $SN = 3 + 1 = 4$,which corresponds to $sp^3$ hybridization.$3$. For $SO_3$: The central atom $S$ has $3$ bond pairs and $0$ lone pairs. $SN = 3 + 0 = 3$,which corresponds to $sp^2$ hybridization.Thus,the hybridizations are $sp^3d, sp^3, sp^2$ respectively.

The hybridization of the central atom of $ClF_3$,$NH_3$,and $SO_3$ are respectively:

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