# Why are metallic compounds good conductors?

May 16, 2018

#### Answer:

Well, how do we describe $\text{metallic bonding....?}$

#### Explanation:

$\text{Metallic bonding}$ 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: $\text{positive ions in a sea of electrons}$.

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: $\text{malleability}$, the ability to beaten into a sheet (cf. Latin $\text{malleus"="hammer}$); and $\text{ductility}$, 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....