The correct statement about iron includes:I) | vedclass

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(A) $I$) In $K_2FeO_4$,iron is in the $+ 6$ oxidation state,which is its highest oxidation state.$II$) The electronic configuration of $Fe$ is $[Ar] 3

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$I, II, III$

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(A) $I$) In $K_2FeO_4$,iron is in the $+ 6$ oxidation state,which is its highest oxidation state.$II$) The electronic configuration of $Fe$ is $[Ar] 3d^6 4s^2$. In the $+ 2$ oxidation state $(Fe^{2+})$,it loses two $4s$ electrons,leaving $3d^6$ configuration,which has six electrons in the $3d$ orbitals.$III$) The electronic configuration of $Fe^{3+}$ is $[Ar] 3d^5$. This has five unpaired electrons in the $3d$ orbital,making it a common and stable oxidation state due to the half-filled $d$-subshell.Thus,all three statements are correct.

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.

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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.