In which of the following compounds does the | vedclass

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(D) The oxidation states of the transition metals in the given compounds are calculated as follows:						Compound			Calculation of Oxidation State

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$Fe(CO)_5$

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(D) The oxidation states of the transition metals in the given compounds are calculated as follows:						Compound			Calculation of Oxidation State									$K_2Cr_2O_7$			$2(+1) + 2(x) + 7(-2) = 0 \implies 2 + 2x - 14 = 0 \implies 2x = 12 \implies x = +6$							$KMnO_4$			$(+1) + x + 4(-2) = 0 \implies 1 + x - 8 = 0 \implies x = +7$							$CrO_5$			$x + 5(-2) = 0 \implies x = +10$ (Note: Due to peroxide linkages,the actual oxidation state is $+6$,but mathematically $x=+10$ based on standard rules).							$Fe(CO)_5$			$x + 5(0) = 0 \implies x = 0$ (Since $CO$ is a neutral ligand).			Therefore,the transition metal in $Fe(CO)_5$ has a zero oxidation state.

List-$I$ (Complex)	List-$II$ (Primary valency and Secondary valency)
$(A)$ $[Co(en)_2 Cl_2] Cl$	$(I)$ $3, 6$
$(B)$ $[Pt(NH_3)_2 Cl(NO_2)]$	$(II)$ $2, 4$
$(C)$ $Hg[Co(SCN)_4]$	$(III)$ $3, 4$
$(D)$ $[Mg(EDTA)]^{2-}$	$(IV)$ $2, 6$

In which of the following compounds does the transition metal have a zero oxidation state?

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