1. High electrical and thermal conductivity: Because the valence electrons in metals are not strongly bound to any particular atom, they can move freely throughout the metal lattice. This allows metals to conduct electricity and heat very well.

2. Luster: The free valence electrons in metals also contribute to their luster, or shininess. When light strikes a metal surface, the electrons absorb the energy and then re-emit it in all directions, giving the metal a shiny appearance.

3. Malleability and ductility: Metals are malleable, meaning they can be hammered into thin sheets, and ductile, meaning they can be drawn into thin wires. This is because the strong metallic bonds allow the atoms in metals to slide past each other easily.