Chemistry – Metals - Properties of metals | e-Consult

Thermal Conductivity: Metals generally have much higher thermal conductivities than non-metals. This is because the delocalised electrons in metals can efficiently transfer kinetic energy throughout the material. When one part of a metal is heated, the free electrons gain energy and move rapidly, colliding with other electrons and atoms, thus transferring the heat energy. Non-metals, lacking delocalised electrons, rely on lattice vibrations for heat transfer, which is a much less efficient process.

Electrical Conductivity: Similarly, metals are excellent conductors of electricity. The delocalised electrons in metals form an 'electron sea' that can easily move under the influence of an electric field. This allows electric current to flow readily. Non-metals have tightly bound electrons and do not have a significant number of free electrons, making them poor conductors of electricity (insulators). Some non-metals, like graphite, can conduct electricity, but this is due to delocalised electrons within the covalent network structure, not the typical metallic conduction mechanism.

Why Metals are Good Conductors: The key reason metals are good conductors is the presence of delocalised electrons. These electrons are not bound to individual atoms and can move freely throughout the metallic structure. This allows for both the efficient transfer of kinetic energy (heat) and the easy flow of electric charge.