Metallic solids

Definition

Metallic solids are types of solids composed of metal atoms held together by a sea of delocalized electrons. They typically exhibit high electrical and thermal conductivity, malleability, and ductility.

5 Must Know Facts For Your Next Test

1. Metallic bonding involves the attraction between free-floating electrons and positively charged metal ions.
2. Metallic solids have high melting and boiling points due to strong metallic bonds.
3. They are good conductors of electricity because the delocalized electrons can move freely.
4. The malleability and ductility of metallic solids arise from their ability to deform under stress without breaking bonds.
5. Examples include elements like iron, copper, and gold.

Review Questions

• What type of bonding is found in metallic solids?
• Why do metallic solids have high electrical conductivity?
• How do the properties of malleability and ductility manifest in metallic solids?

Related terms

Ionic Solids: Solids composed of ions held together by electrostatic forces; they typically have high melting points and are brittle.

Covalent Network Solids: Solids where atoms are connected by covalent bonds in a continuous network; they usually have very high melting points.

Amorphous Solids: Solids that lack a well-defined, long-range crystal structure; examples include glass and plastics.