Concept 3 - Metallic Bonds

What is a metallic bond?

A chemical attraction formed from a shared pool of valence electrons that holds metal atoms together.

In metallic bonds, do metals lose their valence electrons like in ionic bonds?

No, all metal atoms share their electrons from a "sea of electrons."

What are delocalized electrons?

Electrons that are not associated with a single atom or bond.

Why is the attraction of electrons lower in metals?

Because their electronegativity (EN) is low.

What structure do metals often form?

Lattices, similar to those seen with ionic bonds.

Why do metals create a "sea of electrons"?

Because metals are often bigger with overlapping orbitals.

What properties do metallic bonds give metals?

• Malleability (can be made into thin sheets)

• Ductility (can be made into wires)

• Electrical and thermal conductivity

• Strong absorption and reflection of light (metallic appearance)

How does the "sea of electrons" help in conductivity?

It allows electrons to flow through the material, producing an electric current.

What gives metals their shiny, metallic appearance?

Strong absorption and reflection of light.

What is an alloy?

A solution of two metals mixed together.

Why are alloys important?

Mixing metals in specific proportions can create materials with desirable properties.