In which scenario would a metallic bond not be observed?

Metallic bonding occurs when metal atoms collectively share their delocalized electrons within a lattice structure. This type of bonding is characteristic of metals and their alloys, where the atoms are arranged in a way that allows for these free-moving electrons, contributing to properties like ductility and electrical conductivity.

The scenario where metallic bonding would not be observed involves interactions between different types of elements. When a metal bonds with a non-metal, ionic or covalent bonding is typically observed instead. In ionic bonding, the metal donates electrons to the non-metal, resulting in the formation of charged ions, while covalent bonding involves the sharing of electrons between non-metals. Hence, in a relationship involving a metal and a non-metal, the metallic bond is not a relevant factor, as the bonding nature shifts to ionic or covalent.

In contrast, solid metal lattices and alloys are characterized by metallic bonds due to the presence of closely packed metal atoms each contributing to the delocalized electron cloud that defines metallic bonding. Likewise, a gas of metal atoms does not form metallic bonds because the atoms are too far apart to share electrons in a bonding pattern typical of metallic structures. However, if these metal atoms were to condense into a solid state, they would most likely exhibit