What is metallic bonding and how does it occur?

Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons in a metal lattice.

In more detail, metallic bonding is a type of chemical bonding that arises from the electrostatic attractive force between conduction electrons (in the form of an electron cloud, also known as a 'sea of electrons') and positively charged metal ions. It is the main type of bond that holds metals together.

In a metal, the outer electrons of each atom are delocalised. This means they are not attached to any particular atom, but are free to move throughout the whole structure. These delocalised electrons are also known as conduction electrons, because they are responsible for the ability of metals to conduct electricity.

The positive metal ions are arranged in a regular pattern known as a lattice. The delocalised electrons are attracted to these positive ions, creating a strong bond between them. This is why metals are generally strong and have high melting and boiling points.

The 'sea of electrons' model also explains other properties of metals. For example, metals are malleable (they can be hammered into shape) and ductile (they can be drawn into a wire). This is because the layers of ions in the metal lattice can slide over each other without breaking the metallic bonds. The delocalised electrons can also move to new positions and maintain the attraction between the ions.

In summary, metallic bonding is a type of chemical bonding that involves the attraction between positive metal ions and delocalised electrons. This bonding gives metals their characteristic properties, such as strength, conductivity, malleability and ductility.