What is the definition of metallic bonding?

Metallic bonding is characterized by the electrostatic attraction between positive metal ions and delocalised electrons. In a metallic structure, metal atoms lose some of their electrons, which then become delocalised, allowing them to move freely throughout the metal lattice. This delocalization creates a 'sea of electrons' that are not tied to any specific atom, facilitating conductivity and malleability of metals.

The attraction between these negatively charged delocalised electrons and the positively charged metal ions is what holds the structure together, contributing to properties such as electrical conductivity, thermal conductivity, and ductility that are characteristic of metals. This fundamental understanding of metallic bonding illustrates the unique behavior of metals compared to other types of bonding, such as covalent or ionic bonding.