What is the strongest attractive force in a metallic lattice?

In a metallic lattice, the strongest attractive force comes from the electrostatic attraction between delocalized electrons and metal ions. Metals consist of positive metal ions that are surrounded by a "sea" of delocalized electrons. These electrons are not bound to any specific ion but are free to move throughout the structure, creating a lattice of positive ions.

This interaction is a result of the nature of metallic bonding, where these delocalized electrons act as a glue that holds the positively charged metal ions together. The strong electrostatic attraction between the negatively charged delocalized electrons and the positively charged metal ions is what gives metals their characteristic properties, such as electrical conductivity, malleability, and ductility.

The other forces mentioned, such as covalent bonds, Van der Waals forces, and hydrogen bonds, are not the primary forces at play in a metallic lattice. Covalent bonds form between specific atoms sharing electrons, while Van der Waals forces and hydrogen bonds are much weaker intermolecular forces that play a role in different types of materials, particularly in non-metallic compounds. Thus, the presence of the strong electrostatic forces in metallic lattices distinctly defines their structural integrity and metallic properties.