Metallic Bonding

1. Metallic Bonding Topic 4.4

2. Metallic Bonding • Metals are on the left side of the Periodic Table. • Metals have a small number of electrons in their outer shell. • Metals have low ionization energies and typically react with other elements by losing their valence electrons and forming positive ions.

3. Metallic Bonding • In the elemental state, when there is no other element present to accept the electrons and form an ionic compound, the valence electrons become delocalized. • This means that the electrons are no longer associated closely with any one metal nucleus, but instead, spread themselves through the metal structure.

4. Metallic Bonding • The metal atoms without these electrons become positively charged ions and form a regular lattice structure through which these electrons can move freely.

5. Metallic Bonding • So, there is force of electrostatic attraction between the lattice of positive ions and the delocalized electrons – this is known as metallic bonding.

6. Metallic Bonding • Metals are good conductors of electricity because the delocalized electrons are highly mobile and can move through the metal structure in response to an applied voltage. • The mobility of the electrons also makes metals good conductors of heat.

7. Metallic Bonding • Metals are malleable and ductile • Malleable refers to ease of reshaping (e.g. turning flat slabs into tubes without cracking or breaking) and ductile refers to the ability to be drawn out, as into wires. Granite is not very malleable or ductile. Copper is.

8. Metallic Bonding • Applying pressure on the metal makes very little difference in the over all structure.