(D) The charge on the complex ion is equal to the sum of the oxidation state of the metal and the charge on the ligands.Let the oxidation state of $Pt

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(D) The charge on the complex ion is equal to the sum of the oxidation state of the metal and the charge on the ligands.Let the oxidation state of $Pt$ be $x$.The charge on the $Cl^-$ ligand is $-1$.Therefore,$x + 6 \times (-1) = -2$.$x - 6 = -2$.$x = +4$.Thus,the oxidation state of $Pt$ in $[PtCl_6]^{2-}$ is $+4$.