1. Sodium chloride NaCl : The bonding in sodium chloride is ionic. This type of bonding occurs when there is a transfer of electrons between a metal and a non-metal atom. In the case of NaCl, sodium Na is a metal and chlorine Cl is a non-metal. Sodium loses one electron to achieve a stable electron configuration, forming a positively charged ion Na+ , while chlorine gains one electron to achieve a stable electron configuration, forming a negatively charged ion Cl- . The electrostatic attraction between these oppositely charged ions results in the formation of an ionic bond. Sodium chloride forms a crystalline lattice structure, which gives it a high melting and boiling point, and it is soluble in water due to the polar nature of water molecules.2. Graphite: The bonding in graphite is covalent with some delocalized electrons. Graphite is an allotrope of carbon, which is a non-metal. In graphite, each carbon atom is covalently bonded to three other carbon atoms, forming a hexagonal planar structure. These covalent bonds result from the sharing of electrons between carbon atoms. The fourth electron of each carbon atom is delocalized and free to move throughout the structure, which gives graphite its electrical conductivity and lubricating properties. The layers of hexagonal carbon structures are held together by weak van der Waals forces, which allow the layers to slide over each other, making graphite a good lubricant and giving it a slippery feel.3. Copper Cu : The bonding in copper is metallic. Metallic bonding occurs in metals, where the atoms are closely packed together in a lattice structure. In the case of copper, the positively charged copper ions Cu+ are surrounded by a "sea" of delocalized electrons. These electrons are free to move throughout the metal lattice, which gives copper its high electrical and thermal conductivity. The electrostatic attraction between the positively charged metal ions and the delocalized electrons results in the formation of a metallic bond. This type of bonding also gives copper its malleability and ductility, as the layers of metal ions can slide past each other without breaking the metallic bonds.