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.

List-$I$ (Element)	List-$II$ (Block)
$A$. $Cd$	$I$. $f$-block
$B$. $Eu$	$II$. $s$-block
$C$. $Se$	$III$. $d$-block
$D$. $Ba$	$IV$. $p$-block

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Which of the following ions indicates the maximum magnetic moment?

Match the following:
List-$I$ (Element) List-$II$ (Block)
$A$. $Cd$ $I$. $f$-block
$B$. $Eu$ $II$. $s$-block
$C$. $Se$ $III$. $d$-block
$D$. $Ba$ $IV$. $p$-block

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