Final answer:
Metallic bonding is the force between conduction electrons in a sea of electrons and the positively charged metal ions, is unique to metals, and is responsible for their distinctive properties such as conductivity and malleability.
Step-by-step explanation:
Metallic bonding is a type of chemical bonding that arises from the electrostatic attractive force between the conduction electrons (in the form of a sea of electrons) and the positively charged metal ions. In metallic bonding, the valence electrons from the metal atoms are delocalized, meaning they can move freely throughout the metal structure. This delocalisation of electrons contributes to the high electrical and thermal conductivity of metals.
The correct answer to the question would be (d) It involves a "sea of electrons" moving freely among metal ions. Metallic bonds are characterized by an array of positive ions, or cations, surrounded by this sea of mobile valence electrons. Unlike ionic bonding, which involves the complete transfer of electrons from one atom to another and typically occurs between a metal and a non-metal, or covalent bonding, where electrons are shared between atoms, metallic bonding is unique to metallic elements.
Metallic crystals are formed when these bonds create a lattice-like structure that holds the ions in a clear crystalline pattern. This leads to the unique properties of metals, such as malleability, ductility, and the ability to conduct electricity and heat.