In which of the following is the metallic bon | vedclass

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(D) The strength of a metallic bond depends upon the number of unpaired electrons in the $d$-orbitals. As the number of unpaired electrons increases,t

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$Cr$

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(D) The strength of a metallic bond depends upon the number of unpaired electrons in the $d$-orbitals. As the number of unpaired electrons increases,the metallic bond strength increases. $Cr$ (Chromium) has the electronic configuration $[Ar] 3d^5 4s^1$,which contains $6$ unpaired electrons. Due to the maximum number of unpaired electrons,$Cr$ exhibits the strongest metallic bonding among the given options.

In which of the following is the metallic bond strongest?

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