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(C) The enthalpy of atomisation depends on the number of unpaired electrons available for metallic bonding. Among the given transition metals ($Cr$,$C

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$6$

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(C) The enthalpy of atomisation depends on the number of unpaired electrons available for metallic bonding. Among the given transition metals ($Cr$,$Co$,$Fe$,$Ni$),$Cr$ has the lowest enthalpy of atomisation because it has a stable $d^5$ configuration,which limits the number of electrons participating in metallic bonding compared to others.For $Cr$ $(Z=24)$,the electronic configuration is $[Ar] 3d^5 4s^1$.The total number of valence electrons is the sum of electrons in the outermost $s$ and $d$ orbitals.Valence electrons = $5 (d) + 1 (s) = 6$.

The number of valence electrons present in the metal among $Cr$,$Co$,$Fe$,and $Ni$ which has the lowest enthalpy of atomisation is

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