What gives metals their ability to conduct electricity?

Metals conduct electricity primarily due to the presence of delocalized electrons. In metallic structures, atoms are arranged in a lattice where some of the electrons are not bound to any specific atom. Instead, these delocalized electrons are free to move throughout the metal. This movement of electrons allows for the transfer of electrical charge when a potential difference is applied.

When you connect a metal to a power source, these delocalized electrons can flow easily, resulting in the conduction of electricity. The sea of electrons model helps illustrate how this electron mobility contributes to the overall electrical conductivity of metals.

In contrast, fixed electrons refer to electrons that are bound to specific atoms and do not contribute to conductivity. Atomic nuclei themselves do not conduct electricity; they are positively charged centers that provide structural integrity to the metal but do not facilitate charge movement. Insulating layers, typically found in non-metallic materials, prevent the flow of electricity, which is the opposite of what allows metals to conduct electricity.