What type of bonding do metals exhibit?

Metals exhibit metallic bonding, which is characterized by a unique arrangement of atoms. In metallic bonding, metal atoms release some of their electrons to form a 'sea of electrons' that are free to move around. This delocalization of electrons allows the atoms to be held together by strong electrostatic forces of attraction between the positively charged metal ions and the negatively charged electron cloud. This bonding structure gives metals their distinctive properties, such as electrical conductivity, malleability, and ductility, as the electrons can move easily throughout the metal lattice.

This is distinct from ionic bonding, which involves the transfer of electrons from one atom to another, forming oppositely charged ions that attract each other. Covalent bonding involves the sharing of electrons between atoms, typically nonmetals, leading to the formation of discrete molecules. Hydrogen bonding is a weak intermolecular force that occurs between molecules containing hydrogen atoms bonded to electronegative atoms like nitrogen, oxygen, or fluorine.