6.4 Metallic Bonds and Properties of Metals

Formed when small holes in a metallic crystal are filled with smaller atoms (bicycle frame)

• Interstitial Alloys

• Substitutional Alloys

• Covalent Compounds

• Ionic Compounds

Some of the atoms in the original metal are replaced by other metals of similar atomic size

• Substitutional Alloys

• Interstitial Alloys

• Covalent Alloys

• Metallic Alloys

Metal atoms do not share their valence electrons with neighboring atoms, nor do they lose their valence electrons in this..

• Metallic Lattice

• Ionic Bonding

• Covalent Bonding

• Van der Waals Forces

The ability of metals to be drawn into wires

• Malleability

• Ductility

• Brittleness

• Conductivity

The ability of metals to be hammered into thin sheets

• Ductility

• Malleability

• Brittleness

• Conductivity

All the metal atoms in a metallic solid contribute their valence electrons to form a ¨sea¨ of electrons that surrounds the metal cations in the lattice.

• Electron Sea Model

• Covalent Bonding Theory

• Ionic Bonding Concept

• Metallic Bonding Principle

The property of metals that allows them to conduct electricity

• Thermal Conductivity

• Electrical Conductivity

• Magnetic Conductivity

• Optical Conductivity

The attraction of a metallic cation for delocalized electrons

• Ionic Bond

• Covalent Bond

• Metallic Bond

• Hydrogen Bond

When the atom´s outer electrons move freely throughout the solid, a metallic cation is formed

• Delocalized Electrons

• Localized Electrons

• Ionized Electrons

• Fixed Electrons

What are made up of charged particles arranged in a lattice structure?

• Metals

• Nonmetals

• Gases

• Liquids