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(B) The atom has a valence electronic configuration of $3d^6$ in its $+3$ oxidation state. This corresponds to the $Co^{3+}$ ion $(Z=27)$.To find the

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$3$

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(B) The atom has a valence electronic configuration of $3d^6$ in its $+3$ oxidation state. This corresponds to the $Co^{3+}$ ion $(Z=27)$.To find the ground state configuration of the neutral atom $(Co)$,we add back the $3$ electrons removed during oxidation.The neutral $Co$ atom has the configuration $[Ar] 3d^7 4s^2$.In the $3d^7$ subshell,there are $5$ orbitals. According to Hund's rule,the $7$ electrons are filled as follows: $5$ electrons occupy the orbitals singly,and $2$ electrons pair up.This leaves $5 - 2 = 3$ unpaired electrons in the $3d$ subshell.Therefore,the number of unpaired electrons in the ground state of the atom is $3$.

How many unpaired electrons will be present in the ground state of an atom which has valence electronic configuration $3d^6$ in its $+3$ oxidation state?

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