1. Metallic Bonding

2. Cation Formation Recall that metals are more stable when they lose electrons to obtain a full valence shell.

3. Metallic Bonding If no nonmetal is present to accept the extra valence electrons, metals release the electrons to freely travel throughout the collection of metal ions.

4. Metallic Properties The delocalized electrons explain many properties of metals. Electrons have a clear path through the solid so metals have high electrical conductivity.

5. Metallic Properties Metals are also able to conduct heat via the mobile electrons.

6. Metallic Properties Layers of metal are held tightly by the sea of electrons so they are hard to pull apart and are tough, but the individual atoms can slip past each other easily so metals are ductile.

7. Metallic Properties The characteristic “shine” of many metals is attributed to the mobile electrons reflecting light.