The species having tetrahedral shape is

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(D) The electronic configuration of $Ni^{2+}$ is $3d^8$. In $[NiCl_4]^{2-}$,$Cl^-$ is a weak field ligand,so it does not cause pairing of electrons. T

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$[NiCl_4]^{2-}$

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(D) The electronic configuration of $Ni^{2+}$ is $3d^8$. In $[NiCl_4]^{2-}$,$Cl^-$ is a weak field ligand,so it does not cause pairing of electrons. Thus,the hybridization is $sp^3$,which results in a tetrahedral geometry. In contrast,$[PdCl_4]^{2-}$,$[Ni(CN)_4]^{2-}$,and $[Pd(CN)_4]^{2-}$ involve $4d$ or $5d$ metals or strong field ligands,leading to $dsp^2$ hybridization and square planar geometry.

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