Considering H_2O as a weak field ligand,the n | vedclass

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(D) The atomic number of $Mn$ is $25$. The electronic configuration of $Mn$ is $[Ar] 3d^5 4s^2$.In the complex $[Mn(H_2O)_6]^{2+}$,the oxidation state

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$5$

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(D) The atomic number of $Mn$ is $25$. The electronic configuration of $Mn$ is $[Ar] 3d^5 4s^2$.In the complex $[Mn(H_2O)_6]^{2+}$,the oxidation state of $Mn$ is $+2$. Thus,the configuration of $Mn^{2+}$ is $[Ar] 3d^5$.Since $H_2O$ is a weak field ligand,it does not cause pairing of electrons in the $d$-orbitals.Therefore,the $5$ electrons in the $3d$ subshell remain unpaired.Hence,the number of unpaired electrons is $5$.

Considering $H_2O$ as a weak field ligand,the number of unpaired electrons in $[Mn(H_2O)_6]^{2+}$ will be (Atomic number of $Mn = 25$).

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