The species having tetrahedral shape is

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(D) The hybridization of $[NiCl_4]^{2-}$ is $sp^3$. The shape of $[NiCl_4]^{2-}$ is tetrahedral. The oxidation state of $Ni$ in this complex is $+2$.

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$[NiCl_4]^{2-}$

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(D) The hybridization of $[NiCl_4]^{2-}$ is $sp^3$. The shape of $[NiCl_4]^{2-}$ is tetrahedral. The oxidation state of $Ni$ in this complex is $+2$. The electronic configuration of $Ni^{2+}$ is $3d^8$. Since the chloride ion $(Cl^-)$ is a weak field ligand,it does not cause electron pairing in the $3d$ orbitals. Therefore,one $4s$ orbital and three $4p$ orbitals hybridize to form four $sp^3$ hybrid orbitals,which overlap with the orbitals of the four $Cl^-$ ligands,resulting in a tetrahedral geometry.

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