Final answer:
Metallic bonds contribute to the characteristic properties of metals such as electrical and heat conductivity, malleability, ductility, luster, high melting points, and density due to the free movement of valence electrons and the strong attraction between metal ions and these electrons.
Step-by-step explanation:
The Relationship Between Metallic Bonds and Metal Properties
Metallic bonds are the force of attraction between positively charged metal ions and the valence electrons that surround them. This creates a lattice-like structure where electrons are free to move. This electrical conductivity is due to electrons being able to flow through the metal, allowing it to carry an electric current. Similarly, the close packing of positive nuclei in metals enables efficient heat conduction.
Metallic bonds also give metals their malleability (the ability to be hammered into sheets) and ductility (the capacity to be stretched into wires), because the layers of atoms can slide past each other without breaking the metallic bonds. The sharing of valence electrons among a sea of metal ions also accounts for the metals' characteristic luster, as electrons absorb and re-emit light energy.
Due to the strength of the metallic bonds, metals typically exhibit high melting points. The tight packing of the atomic structure, resultant from these bonds, also explains the high density commonly associated with metallic substances. Furthermore, metals often form cations in compounds due to the ease with which they can lose valence electrons, a trait that is tied to their metallic bonding nature.