3.11 Describe the bonding in metals. Explain on the atomic/molecular level why metals are malleable (you can make them into different shapes), ductile (you can draw them out into wires), shiny, and conduct electricity.

What type of bonding occurs in metals?

Metallic bonding, where valence electrons are delocalized and move freely through the metal lattice.

What is the electron sea model of metallic bonding?

In the electron sea model, delocalized electrons form a "sea" that flows freely between positively charged metal ions.

How are atoms arranged in metals?

Metal atoms are arranged in a regular, closely packed structure, often in patterns like BCC, FCC, or HCP.

Why are metals malleable (able to be shaped into different forms)?

Metals are malleable because layers of metal ions can slide past each other without breaking metallic bonds, aided by delocalized electrons.

Why are metals ductile (able to be drawn into wires)?

Metals are ductile because delocalized electrons allow the metal ions to move past one another when stretched, forming thin wires without breaking.

Why do metals appear shiny?

Metals are shiny because delocalized electrons reflect visible light effectively, giving metals their characteristic luster.

Why do metals conduct electricity?

Metals conduct electricity because delocalized electrons can move freely in response to an electric field, carrying electrical charge through the material.

What is the relationship between metallic bonding and the macroscopic properties of metals?

• Malleability: Due to sliding layers of metal ions and mobile electrons.

• Ductility: Delocalized electrons allow ions to move without breaking the bond, forming wires.

• Shiny Appearance: Caused by reflection of light by delocalized electrons.

• Electrical Conductivity: Delocalized electrons move freely, allowing current to pass through the metal.