Metallic Bonding

• In metals, the outermost electron shell is not full, so it can be easily lost or shared with other atoms.
• Metals have high melting points due to strong interatomic forces, while non-metals have low melting points because they are held together by weak van der Waals forces.
• The metallic bond is the electrostatic attraction between positive metal ions (cations) and delocalized electrons.
• Metal atoms have strong metallic bonds due to the sharing of electrons between metal atoms.
• Delocalization refers to the movement of electrons throughout the lattice structure rather than being bound to specific atoms.
• The strength of metallic bonding depends on the number of valence electrons per atom and their ability to move freely through the lattice structure.
• The metallic bond involves the sharing of electrons between metal atoms, resulting in a sea of delocalized electrons that move freely throughout the lattice structure.