Which of the following has square planar geometry?

[PtCl₄]^2- has +2 oxidation state of Pt. In the presence of weak field ligand, the splitting is:

$t_{2g}^6{e}_g^2$

in eg, there are ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2} \mathrm{and} {\mathrm{d}}_{{\mathrm{z}}^2.}$ Out of two, the energy of ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}$ is higher than ${\mathrm{d}}_{{\mathrm{z}}^2}.$ Therefore, the further splitting is:

${\mathrm{t}}_{2\mathrm{g}}^6({\mathrm{d}}_{\mathrm{xy}}^2, {\mathrm{d}}_{\mathrm{yz}}^2, {\mathrm{d}}_{\mathrm{zx}}^2), {\mathrm{e}}_{\mathrm{g}}^2({\mathrm{d}}_{{\mathrm{z}}^2}^2, {\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}^0).$

Its causes pairing despite of weak field ligand and makes one d-orbital vacant. Hence, [PtCl₄]^2- has dsp² hybridization and forms a complex having square planar geometry.