Which of the following is a square planar com | vedclass

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(D) $Pt^{2+}$ is a $5d$ transition metal ion with a $d^8$ electronic configuration. Complexes of $Pt(II)$ typically undergo $dsp^2$ hybridization,whic

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(D) $Pt^{2+}$ is a $5d$ transition metal ion with a $d^8$ electronic configuration. Complexes of $Pt(II)$ typically undergo $dsp^2$ hybridization,which results in a square planar geometry. In $[PtCl_4]^{2-}$,the central $Pt^{2+}$ ion is coordinated to four ligands in a square planar arrangement. Similarly,$[PtClBr(H_2O)_2]$ and $[Pt(NH_3)(Py)(H_2O)I]^{+}$ also involve $Pt(II)$ centers,which maintain the square planar geometry due to the strong crystal field splitting associated with $5d$ metals. Therefore,all the given complexes exhibit square planar geometry.

Which of the following is a square planar complex ion?

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