Final answer:
A metallic bond is the attraction between delocalized electrons and metal cations, forming within metals and leading to properties such as conductivity and malleability.
Step-by-step explanation:
A metallic bond is a bond between localized electrons and metal cations. This is found within metals where the metal atoms release some outermost electrons, forming a sea of electrons that move freely around the metal cations. The metal atoms exist as positive ions (cations) arranged in a consistent 3D pattern known as a crystal lattice. The delocalized electrons are not bound to any one atom but are free to move throughout the metal structure. These free-moving electrons in the presence of cations lead to the formation of a metallic bond, which is the electrostatic attraction between the positively charged atomic nuclei of metal atoms and the delocalized electrons. This unique bonding grants metals their characteristic properties such as electrical conductivity, malleability, and ductility.