Which of the following is not tetrahedral?

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Question

(A) To determine the geometry,we calculate the hybridization and number of lone pairs for each species:$1$. $SCl_4$: Sulfur has $6$ valence electrons.

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$SCl_4$

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(A) To determine the geometry,we calculate the hybridization and number of lone pairs for each species:$1$. $SCl_4$: Sulfur has $6$ valence electrons. It forms $4$ bonds with $Cl$ and has $1$ lone pair. The steric number is $5$ ($sp^3d$ hybridization),resulting in a see-saw geometry.$2$. $SO_4^{2-}$: Sulfur has $6$ valence electrons,plus $2$ from the charge. It forms $4$ bonds with $O$ atoms. The steric number is $4$ ($sp^3$ hybridization),resulting in a tetrahedral geometry.$3$. $Ni(CO)_4$: Nickel is in the $0$ oxidation state $(3d^8 4s^2)$. $CO$ is a strong field ligand,causing pairing of electrons. The hybridization is $sp^3$,resulting in a tetrahedral geometry.$4$. $NiCl_4^{2-}$: Nickel is in the $+2$ oxidation state $(3d^8)$. $Cl^-$ is a weak field ligand,so no pairing occurs. The hybridization is $sp^3$,resulting in a tetrahedral geometry.Therefore,$SCl_4$ is the only species that is not tetrahedral.

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