Metallic Bonding

• Metals are good conductors of electricity because the electrons can move freely through the lattice.
• The three types of atomic bonds are... ionic,metallic and covalent bonding
• metal ions are arranged in a row/column called lattice
• metal atoms lose their outer electrons which drift apart and become free electrons
• free electrons have no fixed position so they can flow around the metal easily
• Electro-static attraction= charge repels and oppositely charged particles attract
• Delocalized electrons keep metallic structure/lattice together
• large number of electrons make metals good conductors of electricity and heat
• Metal atoms are held together which makes them have high melting and boiling point
• Metals are malleable because when pressure is applied, it causes the layers to slide over one another.
• A mixture of 2+ metals is called an alloy
• A metallic bonding is an attraction between positive ions and electrons
• In metals, the valence electrons form a shared sea of electrons
• When two different metals react with each other, they can exchange some of their delocalised electrons to form a compound that has a lower energy than either of its components
• The outer shell of metal atoms contain enough electrons to fill their orbitals so they don't need to lose or gain any electrons to become stable
• Metallic bonding forms between metal atoms