Identify the element having the highest entha | vedclass

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(B) The enthalpy of atomization of transition elements depends on the strength of metallic bonding,which is directly related to the number of unpaired

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$Fe$ $(Z=26)$

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(B) The enthalpy of atomization of transition elements depends on the strength of metallic bonding,which is directly related to the number of unpaired electrons in the $d$-orbital.More unpaired electrons lead to stronger metallic bonding and higher enthalpy of atomization.Let us analyze the number of unpaired electrons in the given elements:$Sc$ $(Z=21)$: $[Ar] 3d^1 4s^2$ ($1$ unpaired electron)$Fe$ $(Z=26)$: $[Ar] 3d^6 4s^2$ ($4$ unpaired electrons)$Cu$ $(Z=29)$: $[Ar] 3d^{10} 4s^1$ ($1$ unpaired electron)$Zn$ $(Z=30)$: $[Ar] 3d^{10} 4s^2$ ($0$ unpaired electrons)Among the given options,$Fe$ has the maximum number of unpaired electrons $(4)$,resulting in the strongest metallic bonding and the highest enthalpy of atomization.

$E^{\Theta }$	$V$	$Cr$	$Mn$	$Fe$	$Co$	$Ni$	$Cu$
$(M^{2+}/M)$	$-1.18$	$-0.91$	$-1.18$	$-0.44$	$-0.28$	$-0.25$	$+0.35$

Identify the element having the highest enthalpy of atomization from the following.

Similar Questions

For the first row transition metals,the $E^{\Theta }$ values are:

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$(M^{2+}/M)$ $-1.18$ $-0.91$ $-1.18$ $-0.44$ $-0.28$ $-0.25$ $+0.35$

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