1. Metallic Bonding

3. Metals Look at the Periodic Table… 75% of elements are metals!

4. Metals O They can vary a lot…

5. General Properties of Metals Dense Malleable Ductile Good conductors of heat and electricity Shiny Lustre Silver in colour Any exceptions?

6. Structure of Metals Metal atoms tend to lose their valence electrons (outer electrons) to form positively charged ions. Metals consist of a lattice of these ions surrounded by a ‘sea’ of delocalised electrons.

8. Summary

9. Metallic Bonding

10. The structure of metal Physical PropertiesReasons High melting and boiling pointsStrong forces of attraction between the ‘sea’ of negatively charged electrons and the positively charged metal ions. Good conductor of heat and electricity (in solid or molten state) Presence of free electrons carries heat and electricity energy. Malleable (hammered into sheets) Ductile (drawn into wires) Layers of metal atoms can slide over each other without disrupting the metallic bonding. Hence, metallic bonds are strong and flexible. Lustrous surfacePresence of delocalised electrons at the surface

11. Metallic Bonding