Why are metals conductive?

Metals are conductive primarily because their electrons are loosely bound to the nuclei, which allows them to be highly mobile. This characteristic of metals is a result of their atomic structure. In a metallic lattice, metal atoms share a "sea of electrons," which are free to move throughout the structure. This mobility enables the conduction of electricity as electrons can flow easily in response to an electric field.

The conductivity of metals is a fundamental property that arises from their electronic configuration, particularly the presence of valence electrons that are not tightly held by the atomic nuclei. Because these electrons can move freely, they can carry an electric charge, making metals excellent conductors of electricity.

Other characteristics of metals, such as having a metallic luster, their position on the periodic table, or their typical valence states, do not directly contribute to their conductivity in the same way. While these factors may influence some physical properties of metals, it is the mobility of the loosely bound electrons that is the core reason behind their excellent conductivity.