Final answer:
Metallic bonding is characterized by the electrostatic attraction between the positively charged metal ions and the shared pool of delocalised electrons, allowing for free electron movement and leading to metal's distinctive properties.
Step-by-step explanation:
The electrostatic nature of metallic bonding is due to the attraction between the positively charged atomic nuclei of metal atoms, often referred to as cations, and the delocalised electrons that are free to move about the metal lattice. This kind of bonding is distinct because rather than having electrons localized between atoms, as in covalent bonds, or transferred between atoms, as in ionic bonds, the electrons in metallic bonds are shared collectively in a 'sea of electrons'. These electrons are not associated with any one atom, allowing them to move freely through the metallic structure, which leads to many of the unique properties of metals, such as conductivity, malleability, and luster.