In which of the following compounds,the trans | vedclass

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(B) To determine the oxidation state of the transition metal,we consider the charge of the ligands:$1$. In $[Fe(H_2O)_3(OH)_3]$,$Fe + 3(0) + 3(-1) = 0

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$[Ni(CO)_4]$

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(B) To determine the oxidation state of the transition metal,we consider the charge of the ligands:$1$. In $[Fe(H_2O)_3(OH)_3]$,$Fe + 3(0) + 3(-1) = 0 \implies Fe = +3$.$2$. In $[Ni(CO)_4]$,$Ni + 4(0) = 0 \implies Ni = 0$. Here,$CO$ (carbonyl) is a neutral ligand.$3$. In $[Fe(H_2O)_6]SO_4$,$Fe + 6(0) = +2 \implies Fe = +2$.$4$. In $[Co(NH_3)_6]Cl_3$,$Co + 6(0) = +3 \implies Co = +3$.Thus,the transition metal with an oxidation state of zero is in $[Ni(CO)_4]$.

In which of the following compounds,the transition metal is in an oxidation state of zero?

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