Which type of bonding results from the attraction between metal atoms and a sea of electrons?

Metallic bonding occurs when metal atoms are surrounded by a "sea of electrons." In this type of bonding, the outermost electrons are not bound to any particular atom and can move freely throughout the metallic structure. This electron mobility allows metals to conduct electricity and heat efficiently. The positive metal ions are held together by the electrostatic attraction to the negatively charged electrons that are delocalized over the entire metallic lattice. This unique bonding mechanism accounts for many characteristic properties of metals, including malleability, ductility, and luster. In contrast to covalent bonding, where atoms share electrons, or ionic bonding, which involves the transfer of electrons between atoms, metallic bonding is distinct in its reliance on this delocalized electron sea. Hydrogen bonding, on the other hand, involves attractive forces between hydrogen and highly electronegative atoms, which is not relevant in the context of metals.