Final answer:
The properties of metals such as conductivity, malleability, ductility, and luster are due to the metallic bond, which involves a 'sea' of delocalized electrons allowing free electron flow and the creation of cations.
Step-by-step explanation:
The metallic bond formed in metallic bonding is responsible for the characteristic properties of metals such as high electrical and thermal conductivity, malleability, ductility, and luster. In metallic solids, like crystals of copper, aluminum, and iron, metal atoms create a structure often described as a uniform distribution of atomic nuclei within a 'sea' of delocalized electrons. This 'sea' allows electrons to flow freely, which explains why metals are excellent conductors of electricity and heat. When metals are subjected to light, their electrons absorb and re-emit energy, creating the distinctive luster associated with metals. The malleability and ductility of metals are due to the ability of their atomic layers to slide over each other without breaking the metallic bond.
Furthermore, the ease with which metals can lose their valence electrons to form cations plays a significant role in their high conductivity. The unique characteristics of metallic bonding contribute to the varied and useful bulk properties of metallic solids, making them indispensable in numerous industrial and technological applications.