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Account for the following : The melting and boiling points of Zn, Cd, and Hg are low.
Account for the following : The melting and boiling points of Zn, Cd, and Hg are low.
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- Fully filled d-orbitals weaken metallic bonding.
- Strong metallic bonding requires unpaired d-electrons.
Updated On: Jan 13, 2026
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Solution and Explanation
The low melting and boiling points of Zn, Cd, and Hg are attributed to the absence of unpaired electrons in their d-orbitals, which results in weak metallic bonding. Electronic Configuration and Bonding - As Group 12 elements, Zn, Cd, and Hg exhibit a complete d\(^{10}\) electronic configuration. - This absence of unpaired d-electrons diminishes the strength of metallic bonding, leading to these metals being soft with low melting and boiling points.
Weak Interatomic Forces - In typical transition metals, strong metallic bonding is facilitated by the overlap of d-orbitals. - However, for Zn, Cd, and Hg, their fully filled d-orbitals do not participate in bonding, thereby causing weak interatomic forces and consequently, low melting and boiling points.
Weak Interatomic Forces - In typical transition metals, strong metallic bonding is facilitated by the overlap of d-orbitals. - However, for Zn, Cd, and Hg, their fully filled d-orbitals do not participate in bonding, thereby causing weak interatomic forces and consequently, low melting and boiling points.
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