2.1.5 Metallic Bonding

In this lesson, we will explore the unique nature of metallic bonding in metals. We will understand how metals consist of giant structures of atoms and how the delocalisation of electrons leads to the formation of strong metallic bonds.

Giant Structures of Metal Atoms

Metals are characterised by their giant structures of atoms arranged in a regular pattern. This regular arrangement allows for the efficient packing of metal atoms, resulting in a closely bonded metallic latticeHighly organised structure of repeating atoms/molecules that forms a crystalline structure.. Examples of metals include iron, copper, and aluminium.

Delocalised Electrons

In metallic bonding, the electrons in the outer shell of metal atoms are not tightly bound to individual atoms. Instead, they are delocalised or free to move throughout the entire structure of the metal. Delocalisation occurs because the outer electrons are not strongly attracted to any specific nucleusA membrane-bound organelle in eukaryotic cells that contains DNA., but rather to the positive metal ions as a whole.

Formation of Metallic Bonds

The delocalised electrons in metals form a "sea" of mobile electrons that surround the positively charged metal ions. This sea of electrons is responsible for the strong metallic bonds between metal atoms. The positive metal ions are held together by the attraction between the metal cations and the shared delocalised electrons.

Strength of Metallic Bonds

The sharing of delocalised electrons in metallic bonding gives rise to strong metallic bonds. These bonds are responsible for the high melting points, high electrical and thermal conductivity, and malleability of metals. The mobility of the delocalised electrons allows for efficient transfer of electric current and thermal energy.

Conclusion

In conclusion, metallic bonding occurs in metals, which consist of giant structures of atoms arranged in a regular pattern. The delocalisation of electrons in the outer shell of metal atoms gives rise to strong metallic bonds. The sharing of these delocalised electrons allows for unique properties such as high electrical and thermal conductivity, malleability, and high melting points.