Which of the following complex ions has 0 d-e | vedclass

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(A) To find the number of $d$-electrons,we determine the oxidation state of the central metal atom:$1$. For $[MnO_4]^-$,$Mn + 4(-2) = -1 \implies Mn =

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$[MnO_4]^-$

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(A) To find the number of $d$-electrons,we determine the oxidation state of the central metal atom:$1$. For $[MnO_4]^-$,$Mn + 4(-2) = -1 \implies Mn = +7$. Electronic configuration of $Mn$ $(Z=25)$ is $[Ar] 3d^5 4s^2$. $Mn^{7+}$ is $[Ar] 3d^0 4s^0$. It has $0$ $d$-electrons.$2$. For $[Co(NH_3)_6]^{3+}$,$Co + 6(0) = +3 \implies Co = +3$. $Co$ $(Z=27)$ is $[Ar] 3d^7 4s^2$. $Co^{3+}$ is $[Ar] 3d^6$. It has $6$ $d$-electrons.$3$. For $[Fe(CN)_6]^{3-}$,$Fe + 6(-1) = -3 \implies Fe = +3$. $Fe$ $(Z=26)$ is $[Ar] 3d^6 4s^2$. $Fe^{3+}$ is $[Ar] 3d^5$. It has $5$ $d$-electrons.$4$. For $[Cr(H_2O)_6]^{3+}$,$Cr + 6(0) = +3 \implies Cr = +3$. $Cr$ $(Z=24)$ is $[Ar] 3d^5 4s^1$. $Cr^{3+}$ is $[Ar] 3d^3$. It has $3$ $d$-electrons.Thus,$[MnO_4]^-$ has $0$ $d$-electrons.

Which of the following complex ions has $0$ $d$-electrons in the central metal atom? (Atomic numbers: $Cr = 24, Mn = 25, Fe = 26, Co = 27$)

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