1. Metals Electrons in the outer shell are very unstable. Atoms are packed together in a regular pattern. Packed so tightly that some of the electrons become detached from their atoms. Free electrons move around between the spaces of the atoms.

2. - - - - - - - - - - - - - - - METAL IONS ELECTRONS

3. ‘SEA’ of electrons

4. Good Conductors Electrons carry a negative charge. Metal atoms carry a positive charge. Now have more protons than electrons; HENCE Strong attraction between the positive and negative charges  arrangement held closely together.

5. Metals conduct electricity When a current is passed through a metal the electrons move towards the positive charge. - - - - - -

6. Metals conduct heat - - - - - -

7. Properties Malleable – Can be hammered into shapes. Due to the closely packed arrangements; layers of atoms slide over each other. Ductile – Drawn into wires

8. Uses of Metals Group I Metals – Low melting points. – Very soft. – Low density. – Can be used to strengthen other metals. – Used in batteries

9. Group 2 Metals – Less reactive – Magnesium can be used in fireworks. – Also can be used in engines in combination with other metals. – Less dense than steel or aluminium. – Does not burn easily in large chunks. Uses of Metals

10. Transition Metals – Most widely used in industry and everyday life. – Hard, shiny and dense. – Good conductors of heat and electricity. – Malleable and ductile Iron, cobalt and nickel → Magnetic Uses of Metals

11. Copper – Water pipes, water tanks, wiring. Zinc – Zinc coated tanks. Tungston – Filaments in lightbulbs. Stainless Steel – Radiators Cobolt – in the form of an alloy found in razor blades. Cast iron – gates, old pots. Platinum – catalytic converters. Uses of Metals

12. ALUMINIUM

13. COPPER

14. Gold, Silver and Platinum

15. Uses of Ionic and Covalent Compounds