- Electrostatic forces of attraction between cations of metal and a sea of delocalised electrons
- Metal atoms are packed together in a giant metallic lattice
- Outer electrons are delocalised
- All metals can conduct electricity/heat with varying results
- The sea of delocalised electrons can move freely
- Therefore, they can move and conduct charge, as they are negatively charged
- High boiling/melting point
- Increases with the electrostatic force of attraction between electrons and the nucleus
- More delocalised electrons
- Higher charge on cation
- Stronger metallic bond
- Ductile: Able to be drawn out/stretched into a wire
- Cations are in a sea of delocalised electrons
- Therefore, they will slide when a force is applied, without breaking
- Malleable: Can be beaten into sheets without being broken
- Cations are in a sea of delocalised electrons
- Therefore, they will slide when a force is applied, without breaking
- Giant metallic lattice structure (Na, Mg, Al)
- Always describe metals as “grey solids”, with a few exceptions
- Gold is “yellow”
- Copper is “salmon-pink”
- There is no metal that is white
Ionic Bonding
Covalent Bonding