Metallic Bonding

Valence electrons are not confined to individual atoms (free electrons). Metal atoms form positive ions, and free electrons move throughout the metal structure.

Electron Sea Model

Sea of delocalized electrons creates a strong electrostatic attraction between metal cations and the electron sea.

Properties of Metals

• Malleability
• Ductility
• High melting and boiling points
• High electrical and thermal conductivity
• Metallic lustre

Structure and Industrial Applications

• Giant structures with strong metallic bonds.
• Thermally stable due to high melting/boiling points.
• Malleable and ductile, allowing them to be drawn into wires and sheets.
• Good conductors of electricity and thermal energy.

Key Concepts

• Octet Rule: Atoms tend to acquire eight-electron configurations in the valence shell, aiming for noble gas electron configuration.
• Ionic Bonds: Formed by electron transfer between atoms, with high melting points and conductivity in molten state.
• Covalent Bonds: Formed by electron sharing; can be single, double, or triple bonds.
• Hydrogen Bonding: Occurs between electron-deficient hydrogen and a lone pair on an electronegative atom; important for adhesive properties of paints and dyes.