Strength of The Bond
The atoms in metals have a strong attractive force between them. Much energy is required to overcome it. Therefore, metals often have high boiling points, with tungsten (5828 K) being extremely high. A remarkable exception are the elements of the zinc group: Zn, Cd, and Hg. Their electron configuration ends in ...ns2 and this comes to resemble a noble gas configuration like that of helium more and more when going down in the periodic table because the energy distance to the empty np orbitals becomes larger. These metals are therefore relatively volatile, and are avoided in ultra-high vacuum systems.
Otherwise, metallic bonding can be very strong, even in molten metals, such as Gallium. Even though gallium will melt from the heat of one's hand just above room temperature, its boiling point is not far from that of copper. Molten gallium is therefore a very nonvolatile liquid thanks to its strong metallic bonding.
The latter also exemplifies that metallic bonding due to its delocalization in all directions is often not very particular about the directionality of the bonding. There is typically a preference for close packing of the atoms, such as face or body centered cubic arrangements, but in the case of liquid gallium the stacking is not regular, at least not at long range and bond angles are easily changed.
Given high enough cooling rates and appropriate alloy composition, metallic bonding can occur even in glasses with an amorphous structure.
Much biochemistry is mediated by the weak interaction of metal ions and biomolecules. Such interactions and their associated conformational change has been measured using dual polarisation interferometry.
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