1. Wednesday 27th July
Reactions of metals

2. Metals and Non-metals metal Non-metal Hard to say! H Li Na K Rb Cs FrBe Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? Ac Al P N O S Cl F Ne Ar Rn I Si Xe He B C As Mg Mg P P S S Fe Fe Cu Cu Sb Sb I I

3. Metals and Non-metals
Metals and non-metals have very different physical properties. Because of this the position of metals and non-metals show a pattern in the Periodic Table:
Metals are on the left and centre.
Non-metals are mostly on the right
In between are metalloids – these are like metals in some ways and like non-metals in others.

4. Properties of metals:

5. Properties of non-metals
Except graphite

6. Reactions of metal with oxygen

7. Reactions with oxygen
Most metals react with oxygen (tarnish) – but they may do so in very different ways. Some react faster than others and some may not react at all.
Some metals burn better than others
When a metal reacts with oxygen it forms a metal oxide.

8. Demo: reactions with oxygen
Below are some observations.
Magnesium
The ribbon burned with a dazzling white flame giving grey-white smoke and ash.
Copper
The copper turnings went through reds and oranges and then slowly got a permanent coating of black.
Iron
The iron filings glowed red and sparkled leaving a brown-black looking solid.

9. Reaction with oxygen - equations
Metal + oxygen  metal oxide 
oxygen +
magnesium
magnesium oxide
2Mg + O2 
2MgO 
oxygen +
copper
2Cu + O2 
2CuO  +
iron
4Fe +
3O2 
2Fe2O3

10. Put these three metals in order of reactivity with oxygen - magnesium, copper, iron.2. 3.

11. Reactions of metal with water

12. Observing reactions with water
Some metals (like lead and copper) react only slowly with water – they used to be used for pipes.
Other metals react quickly with water and can be dangerous.
Modern pipes – not lead but copper or plastic
Metal + water  Metal hydroxide + hydrogen
( less reactive metal + steam  Metal oxide + hydrogen)

13. Reactivity series Potassium Sodium Calcium Magnesium Aluminium Zinc
Iron
Lead
Copper
Silver
Gold

14. What will happen? K + Cu
SO4

15. Copy and complete Potassium + iron sulphate 
Aluminium + silver nitrate 
Copper + Zinc chloride 
Iron + Sodium chloride 
Magnesium + iron Sulphate 
Potassium + aluminium chloride 
Calcium + lead nitrate 
Sodium + calcium chloride 
Iron + lead sulphate 
Aluminium + iron oxide 

16. The Thermit reaction
magnesium fuse
The thermit reaction takes place between aluminium and iron oxide. It is so exothermic that molten iron is produced and the reaction is used to repair broken railway tracks.
iron oxide + aluminium
powder K Na Ca Mg Al Zn Fe Cu Ag Au + 
Aluminium Oxide
Aluminium
Iron Oxide +
Iron
more
reactive
less
reactive
Aluminium wins the competition. Iron is displaced and melts at the high temperatures produced.

17. Here is a photo of the thermit reaction being carried out in a laboratory.
magnesium fuse
iron oxide + aluminium
powder

18. Extension
How many words can you make out of the word:
DISPLACEMENT