In which of the following molecules the centr | vedclass

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(B) The number of hybrid orbitals $(H)$ is calculated using the formula: $H = \frac{1}{2} [V + M - C + A]$,where $V$ is the number of valence electron

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$SF_4$

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(B) The number of hybrid orbitals $(H)$ is calculated using the formula: $H = \frac{1}{2} [V + M - C + A]$,where $V$ is the number of valence electrons of the central atom,$M$ is the number of monovalent atoms,$C$ is the total positive charge,and $A$ is the negative charge.For $CH_4$: $H = \frac{1}{2} [4 + 4 - 0 + 0] = 4$,which corresponds to $sp^3$ hybridization.For $SF_4$: $H = \frac{1}{2} [6 + 4 - 0 + 0] = 5$,which corresponds to $sp^3d$ hybridization.For $BF_4^-$: $H = \frac{1}{2} [3 + 4 - 0 + 1] = 4$,which corresponds to $sp^3$ hybridization.For $NH_4^+$: $H = \frac{1}{2} [5 + 4 - 1 + 0] = 4$,which corresponds to $sp^3$ hybridization.Thus,the central atom in $SF_4$ does not have $sp^3$ hybridization.

In which of the following molecules the central atom does not have $sp^3$ hybridization?

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