Metallic bonding is the attraction between positively charged atomic nuclei of metal atoms and delocalised electrons, forming weaker bonds than ionic or covalent bonds.
Metallic bonding occurs as a result of the electrostatic attraction between the positively charged atomic nuclei of metal atoms and the delocalised electrons in the metal. This bond is responsible for the formation of metallic crystals where valence electrons are free to move throughout the crystal.
Metallic bonds are weaker than ionic or covalent bonds, with dissociation energies ranging from 1 to 3 eV. The attraction between +ions and the sea of free moving electrons is what holds the atoms together in a piece of metal.
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