Why are metallic compounds good conductors?

1 Answer
anor277
May 16, 2018

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....

Related questions
See all questions in Metallic Compounds
Impact of this question
5321 views around the world
You can reuse this answer
Creative Commons License