Why are metallic compounds good conductors?
Well, how do we describe
The formally positively charged metal nuclei can move with respect to each other WITHOUT disrupting the metallic bond. And this gives rise to typical metallic properties:
But the free electrons are delocalized across the entire lattice, and thus they give rise to two other bulk properties: the capacity to conduct electrical charge and heat. Most metals are excellent conductors. The free electrons are competent to conduct both charge and heat....