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(A) To determine the oxidation state of nickel $(Ni)$ in each compound:$1$. In $Ni(CO)_4$,$CO$ is a neutral ligand,so the oxidation state of $Ni$ is $

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$Ni(CO)_4$

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(A) To determine the oxidation state of nickel $(Ni)$ in each compound:$1$. In $Ni(CO)_4$,$CO$ is a neutral ligand,so the oxidation state of $Ni$ is $0$.$2$. In $(CH_3COO)_2Ni$,the acetate ion $(CH_3COO^-)$ has a charge of $-1$,so $Ni + 2(-1) = 0$,which gives $Ni = +2$.$3$. In $NiO$,oxygen $(O)$ has a charge of $-2$,so $Ni + (-2) = 0$,which gives $Ni = +2$.$4$. In $NiCl_2(PPh_3)_2$,$Cl$ has a charge of $-1$ and $PPh_3$ is a neutral ligand,so $Ni + 2(-1) + 2(0) = 0$,which gives $Ni = +2$.Comparing these values,$Ni(CO)_4$ has the lowest oxidation state of $0$.

The compound in which nickel has the lowest oxidation state is

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