What is a characteristic result of a metallic bond?

A metallic bond is characterized by the sharing of free electrons among a lattice of positively charged metal ions. This delocalization of electrons allows metals to conduct heat and electricity efficiently. When a metal is heated or when an electric current is applied, the free electrons can move easily, leading to high thermal and electrical conductivity. This is a fundamental property of metals and is a direct result of their atomic structure and the metallic bonding present within them.

In contrast, materials with low conductivity, high reactivity with other elements, or formation of rigid structures do not exemplify the key features of metallic bonding. These characteristics are more aligned with other types of bonding or materials rather than those that exhibit metallic characteristics.