Yes, metallic bonding does conduct electricity. This is primarily due to the presence of free-moving electrons within the metallic structure.
In metals, atoms are arranged in a lattice structure, and they release some of their electrons into a “sea of electrons” that are not bound to any specific atom. These delocalized electrons can move freely throughout the metal. When an electric field is applied, these free electrons can drift through the metal, allowing electric current to flow.
Additionally, the tightly packed arrangement of metal atoms and the presence of positive ions also contribute to the cohesive strength of metallic bonds, making them ideal for conducting electricity. This is why metals like copper and aluminum are widely used in electrical wiring and components.