Question

Why are metallic compounds good conductors?

Answer 1

Well, how do we describe `"metallic bonding....?"`

Explanation:

`"Metallic bonding"` consists of an array of close-packed metal atoms, which each contribute one or two or more electrons to the overall metallic lattice. And the result is the familiar description of metals: `"positive ions in a sea of electrons"`.

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: `"malleability"`, the ability to beaten into a sheet (cf. Latin `"malleus"="hammer"`); and `"ductility"`, the ability to be drawn into a wire.

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....