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(C) The electronic configuration of $Fe$ $(Z=26)$ is $[Ar] 3d^6 4s^2$. Thus,$Fe$ has $6$ electrons in the $d$ orbital.Electronic configurations of the

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$i, iii$ only

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(C) The electronic configuration of $Fe$ $(Z=26)$ is $[Ar] 3d^6 4s^2$. Thus,$Fe$ has $6$ electrons in the $d$ orbital.Electronic configurations of the given elements:$Mg$ $(Z=12)$: $1s^2 2s^2 2p^6 3s^2$. Total '$s$' electrons = $2+2+2 = 6$.$Cl$ $(Z=17)$: $1s^2 2s^2 2p^6 3s^2 3p^5$. Total '$p$' electrons = $6+5 = 11$.$Ne$ $(Z=10)$: $1s^2 2s^2 2p^6$. Total '$p$' electrons = $6$.Comparing these values,the number of $d$ electrons in $Fe$ $(6)$ is equal to the total '$s$' electrons of $Mg$ $(6)$ and the total '$p$' electrons of $Ne$ $(6)$.Therefore,statements $(i)$ and $(iii)$ are correct.

The number of $d$ electrons in $Fe$ is equal to which of the following?
$i$. Total number of '$s$' electrons of $Mg$
$ii$. Total number of '$p$' electrons of $Cl$
$iii$. Total number of '$p$' electrons of $Ne$
The correct option is

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The number of $d$ electrons in $Fe$ is equal to which of the following?$i$. Total number of '$s$' electrons of $Mg$$ii$. Total number of '$p$' electrons of $Cl$$iii$. Total number of '$p$' electrons of $Ne$The correct option is