Metals are excellent conductors of electricity due to the presence of a 'sea' of delocalised electrons. In a metallic lattice, the metal atoms are arranged in a regular, repeating pattern, forming a giant lattice of positive ions. These positive ions are held together by the electrostatic attraction to the delocalised electrons.

When an electric field is applied, the delocalised electrons are free to move throughout the entire metal structure. This movement of charge constitutes an electric current. Because there are many free electrons available, metals can conduct electricity very efficiently.

Diagram:

In a solid metal, metal ions (positive ions) are arranged in a regular, repeating lattice structure. This lattice is surrounded by a "sea" of delocalised electrons that are free to move throughout the entire structure.

Electrical Conductivity: The delocalised electrons are the key to good electrical conductivity. When a voltage is applied, these electrons are easily displaced and flow in a specific direction, forming an electric current. The lattice provides a framework for these electrons to move through with minimal resistance.

Malleability and Ductility: The metallic bond, formed by the interaction between the positive metal ions and the delocalised electrons, is non-directional. This means that the metal ions can slide past each other without breaking the bonds. The delocalised electrons facilitate this movement by allowing the ions to rearrange themselves into new, stable positions under stress. This ability to deform without fracturing is what gives metals their malleability and ductility.

Metallic bonding is a type of chemical bond that occurs between metal atoms. It arises from the electrostatic attraction between the positively charged metal ions (cations) and a 'sea' of delocalised electrons. The delocalised electrons are not associated with any particular atom but are free to move throughout the entire metallic lattice.

This 'sea' of electrons is crucial to the properties of metals. The electrostatic attraction between the positive ions and the delocalised electrons results in:

• High electrical conductivity: The delocalised electrons are free to move throughout the metal, allowing them to carry an electric current.
• High thermal conductivity: The delocalised electrons can efficiently transfer kinetic energy throughout the metal, leading to high thermal conductivity.
• Malleability and ductility: The delocalised electrons allow the metal ions to slide past each other without breaking the bonds, making metals malleable (able to be hammered into sheets) and ductile (able to be drawn into wires).
• Luster: The delocalised electrons readily absorb and re-emit light, giving metals their characteristic shiny appearance.