Which of the following is NOT tetrahedral in | vedclass

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(C) To determine the shape,we calculate the hybridization and number of lone pairs for each species:$1$. $NH_4^+$: Central atom $N$ has $5$ valence el

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$SF_4$

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(C) To determine the shape,we calculate the hybridization and number of lone pairs for each species:$1$. $NH_4^+$: Central atom $N$ has $5$ valence electrons. $H = (5+4-1)/2 = 4$. Hybridization is $sp^3$ with $0$ lone pairs,so it is tetrahedral.$2$. $SiCl_4$: Central atom $Si$ has $4$ valence electrons. $H = (4+4)/2 = 4$. Hybridization is $sp^3$ with $0$ lone pairs,so it is tetrahedral.$3$. $SF_4$: Central atom $S$ has $6$ valence electrons. $H = (6+4)/2 = 5$. Hybridization is $sp^3d$ with $1$ lone pair. Due to the presence of a lone pair,its shape is see-saw,not tetrahedral.$4$. $SO_4^{2-}$: Central atom $S$ has $6$ valence electrons. $H = (6+0+2)/2 = 4$. Hybridization is $sp^3$ with $0$ lone pairs,so it is tetrahedral.Thus,$SF_4$ is the molecule that is not tetrahedral.

List-$I$ (molecule/ion)	List-$II$ (Number of lone pairs of electrons on the central atom)
$(A)$ $XeF_2$	$(I)$ $2$
$(B)$ $XeO_3$	$(II)$ $0$
$(C)$ $XeF_4$	$(III)$ $3$
$(D)$ $PF_6^-$	$(IV)$ $1$

Which of the following is $NOT$ tetrahedral in shape?

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