How do metal atoms bond with each other?

Metal atoms bond with each other through metallic bonding, which involves the sharing of free electrons among a lattice of positive ions.

Metallic bonding is a type of chemical bonding that arises from the electrostatic attractive force between conduction electrons and positively charged metal ions. It is responsible for many physical properties of metals, such as their high electrical conductivity, thermal conductivity, malleability, and ductility.

In a metal, the outer electrons of each atom are delocalised. Rather than being attached to individual atoms, these electrons are free to move throughout the structure. This is often described as a 'sea' of electrons. 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.

The strength of the metallic bond is determined by the number of electrons which each atom can contribute to the 'sea' of electrons, and the size and charge of the cation. The more electrons an atom can contribute, the stronger the bond. Similarly, the smaller and more charged the cation, the stronger the bond.

This type of bonding results in a structure that is often solid at room temperature, with high melting and boiling points due to the strong attractions between the ions and the sea of electrons. The delocalised electrons also allow metals to conduct electricity and heat. Furthermore, the layers of ions in the lattice can slide over each other, making metals malleable (they can be shaped) and ductile (they can be drawn into wires).

In summary, metallic bonding is a unique type of bonding that gives metals their characteristic properties. It involves the sharing of free electrons among a lattice of positive ions, creating a strong bond.