What type of bonding is primarily exhibited by metals?

Metals primarily exhibit metallic bonding, which is characterized by the presence of a "sea of electrons." In this type of bonding, atoms in a metal lattice release some of their electrons, allowing them to move freely within the structure. This delocalization of electrons results in several key properties associated with metals, such as electrical conductivity, malleability, ductility, and a shiny appearance.

In metallic bonding, the positive metal ions are held together by the electrostatic attraction to the delocalized electrons, creating a strong bond that allows the metal to maintain its structure while also enabling the electrons to move throughout the lattice. This is why metals can conduct electricity; the free-moving electrons can easily carry an electrical charge. Moreover, the ability of metals to be deformed without breaking (malleability) is a direct result of the nature of metallic bonding, as the atoms can slide past one another while still being held together by the electron sea.

Understanding metallic bonding is essential for explaining the unique properties of metals compared to other types of bonds, such as ionic or covalent bonding, which do not exhibit the same free movement of electrons or the same physical properties.