What force describes the attraction between free moving electrons and positive metal ions?

The attraction between free-moving electrons and positive metal ions is best described by the concept of a metallic bond. In metallic bonding, metal atoms lose some of their electrons, which become delocalized and create a "sea of electrons" that is free to move throughout the structure. This electron mobility is critical, as it allows metals to conduct electricity and heat effectively. The positively charged metal ions are held together by the electrostatic attraction to these delocalized electrons, which is what constitutes a metallic bond.

This type of bonding imparts various properties to metals, including malleability, ductility, and electrical conductivity, all of which are essential characteristics of metallic elements. These features arise from the strong attraction between the delocalized electrons and the positively charged ions, enabling the metallic structure to maintain its integrity while allowing movement of atoms.

In contrast, covalent bonds involve the sharing of electron pairs between atoms, typically occurring between nonmetals, while ionic bonds result from the electrostatic force between charged ions (positive and negative) that are not free-moving as in metals. Hydrogen bonds are relatively weak attractions between molecules or parts of molecules with a hydrogen atom bonded to a more electronegative atom, primarily influencing intermolecular interactions rather than bonding within a metallic