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(A) $1$. Determine the oxidation state of the metal ion in each complex:- In $[Mn(H_2O)_6]^{2+}$,$Mn$ is in $+2$ oxidation state. The electronic confi

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$[Mn(H_2O)_6]^{2+}$

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(A) $1$. Determine the oxidation state of the metal ion in each complex:- In $[Mn(H_2O)_6]^{2+}$,$Mn$ is in $+2$ oxidation state. The electronic configuration of $Mn^{2+}$ $(Z=25)$ is $[Ar] 3d^5$.- In $[Fe(H_2O)_6]^{2+}$,$Fe$ is in $+2$ oxidation state. The electronic configuration of $Fe^{2+}$ $(Z=26)$ is $[Ar] 3d^6$.- In $[Co(NH_3)_6]^{3+}$,$Co$ is in $+3$ oxidation state. The electronic configuration of $Co^{3+}$ $(Z=27)$ is $[Ar] 3d^6$.- In $[Ni(H_2O)_6]^{2+}$,$Ni$ is in $+2$ oxidation state. The electronic configuration of $Ni^{2+}$ $(Z=28)$ is $[Ar] 3d^8$.$2$. Apply Crystal Field Theory $(CFT)$ for octahedral complexes:- $H_2O$ is a weak field ligand,so it does not cause pairing of electrons in $d$-orbitals.- For $Mn^{2+}$ $(d^5)$,the electrons fill the orbitals as $t_{2g}^3 e_g^2$ (high spin).- For $Fe^{2+}$ $(d^6)$,the electrons fill as $t_{2g}^4 e_g^2$.- For $Co^{3+}$ $(d^6)$,$NH_3$ is a strong field ligand,causing pairing: $t_{2g}^6 e_g^0$.- For $Ni^{2+}$ $(d^8)$,the electrons fill as $t_{2g}^6 e_g^2$.$3$. Conclusion: The configuration $t_{2g}^3 e_g^2$ corresponds to $[Mn(H_2O)_6]^{2+}$.

In which one of the following complexes does the metal ion have a $t_{2g}^3 e_g^2$ configuration?

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