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(D) The atomic number of $Fe$ is $26$. The electronic configuration of $Fe$ is $[Ar] 3d^6 4s^2$. Number of unpaired electrons in $Fe$: $3d^6$ has $4$

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$Fe^{3+}$

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(D) The atomic number of $Fe$ is $26$. The electronic configuration of $Fe$ is $[Ar] 3d^6 4s^2$. Number of unpaired electrons in $Fe$: $3d^6$ has $4$ unpaired electrons. Electronic configuration of $Fe^+$ is $[Ar] 3d^6 4s^1$. Number of unpaired electrons in $Fe^+$: $3d^6$ $(4)$ + $4s^1$ $(1)$ = $5$ unpaired electrons. Electronic configuration of $Fe^{2+}$ is $[Ar] 3d^6$. Number of unpaired electrons in $Fe^{2+}$: $3d^6$ has $4$ unpaired electrons. Electronic configuration of $Fe^{3+}$ is $[Ar] 3d^5$. Number of unpaired electrons in $Fe^{3+}$: $3d^5$ has $5$ unpaired electrons. Both $Fe^+$ and $Fe^{3+}$ have $5$ unpaired electrons,but in standard chemistry problems of this type,$Fe^{3+}$ is the most stable ion with $5$ unpaired electrons. However,based on the options provided,$Fe^{3+}$ is the standard answer for the highest number of unpaired electrons in common oxidation states.

The higher number of unpaired electrons are in

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