Among the following elements, which one exhib | vedclass

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(B) $1$. The melting point and boiling point of metals depend on the strength of metallic bonding, which is determined by the number of unpaired elect

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$Hg$

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(B) $1$. The melting point and boiling point of metals depend on the strength of metallic bonding, which is determined by the number of unpaired electrons available for delocalization.$2$. $Cr$, $Cu$, and $Au$ are transition elements with partially filled $d$-orbitals, allowing for strong metallic bonding.$3$. $Hg$ has a completely filled $d$-orbital configuration $([Xe] 4f^{14} 5d^{10} 6s^2)$.$4$. Due to the lack of unpaired electrons, the interatomic metallic forces in $Hg$ are very weak, resulting in it being a liquid at room temperature with a melting point of $234 \ K$.

Among the following elements, which one exhibits the lowest melting point $(M.P.)$ and boiling point $(B.P.)$? Note: While $Hg$ is often discussed alongside transition elements, it is technically not a transition element due to its completely filled $d$-orbitals.

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