Which of the following characteristics is NOT typically associated with metallic bonding?

Metallic bonding is characterized by a unique arrangement of atoms in metals, where electrons are not associated with individual atoms but are instead delocalized across the entire metal structure. This delocalization allows metals to conduct electricity effectively, giving rise to high electrical conductivity. Additionally, the ability of metal atoms to slide past each other, while maintaining their cohesive forces, contributes to the malleability observed in metals.

Brittleness is generally not a characteristic of metallic bonding. While some materials, such as certain alloys, may exhibit brittleness, most pure metals are known for their ductility and malleability, which enable them to deform under stress rather than break. The presence of delocalized electrons allows the metallic structure to maintain its integrity even when subjected to mechanical forces, thereby explaining why brittleness is not typically associated with metallic bonding.