Thermal and electrical conductivity. Why are metals good conductors of heat and electricity? Electric current is the flow of electrons in a wire. They are no longer firmly held by a specific atom, but instead they can move freely through the lattice of positive metal ions.
Moreover, why do metals bend easily and conduct electricity?
Metals form giant structures in which electrons in the outer shells of the metal atoms are free to move. The metallic bond is the force of attraction between these free electrons and metal ions. Metals are good conductors of electricity and heat. This is because the free electrons can move throughout the metal.
Why do metals conduct electricity and heat?
First, let me explain why metals generally conduct heat better than other solids do. In metals, some of the electrons (often one per atom) are not stuck to individual atoms but flow freely among the atoms. Of course, that's why metals are such good conductors of electricity.
How is the electrical conductivity of a metal explained by a metallic bond?
"Metallic bonding is the force of attraction between valence electrons and the metal ions. The metallic bond causes many of the traits of metals, such as strength, malleability, ductility, luster, conduction of heat and electricity. Because the electrons move freely, the metal has some electrical conductivity.