The most stable oxidation state of iron is:

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(B) The electronic configuration of $Fe$ $(Z=26)$ is $[Ar] 3d^6 4s^2$.When $Fe$ loses two electrons,it forms $Fe^{2+}$ with a configuration of $[Ar] 3

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$+3$

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(B) The electronic configuration of $Fe$ $(Z=26)$ is $[Ar] 3d^6 4s^2$.When $Fe$ loses two electrons,it forms $Fe^{2+}$ with a configuration of $[Ar] 3d^6$.When $Fe$ loses three electrons,it forms $Fe^{3+}$ with a configuration of $[Ar] 3d^5$.The $3d^5$ configuration is half-filled,which provides extra stability to the $Fe^{3+}$ ion.Therefore,the $+3$ oxidation state is more stable than the $+2$ oxidation state.

Similar Questions

The correct statement about iron includes:
$I$) The highest oxidation state of iron is $+ 6$ in $K_2FeO_4$.
$II$) The iron shows $+ 2$ oxidation state with six electrons in the $3d$ orbitals.
$III$) The common oxidation state of iron is $+ 3$ with five unpaired electrons in the $3d$ orbital.

Which one of the following statements is not correct?

Arrange the following ions in the increasing order of their magnetic moments: $(i) \, V^{4+}$,$(ii) \, Mn^{4+}$,$(iii) \, Fe^{3+}$,$(iv) \, Ni^{2+}$. $[V = 23, Mn = 25, Fe = 26, Ni = 28]$

Variable valency is shown by

Which of the following pairs of elements have one electron in the $5d$-subshell in their observed electronic configuration?

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