Final answer:
Metallic bonds are formed between positively charged metal cations and a sea of delocalized electrons, allowing for the movement of these electrons and giving metals their characteristic properties.
Step-by-step explanation:
The statement that metallic bonds are formed between positively charged atoms (cations) with mobile electrons shared between them describes a fundamental aspect of the structure of metals. Metallic bonding involves the electrostatic attraction between the positively charged atomic nuclei of metal atoms, often referred to as cations, and a 'sea' of delocalized electrons. These electrons are free to move throughout the metal, not belonging to any single atom, which allows for the distinctive properties of metals such as electrical conductivity and malleability.
The positive metal ion and the valence electrons form a lattice-like structure where the delocalized electrons can move freely. This freedom of movement contributes to the strong nature of metallic bonds, as they involve the attraction of these stationary metal cations to the surrounding mobile delocalized electrons.
Metals such as copper, iron, and aluminum exhibit metallic bonding, with each metal bonded to several neighboring atoms and bonding electrons being free to move throughout the crystal lattice. This results in the formation of metallic crystals that are conductive, malleable, and characterized by a low ionization energy and low electronegativity.