1. Patterns of Reactivity

2. Properties of metals and non-metals
Metals have very high melting points (which means that they are usually _____) whereas non-metals will melt at lower ___________
All metals conduct heat and __________ very well, whereas non-metals don’t (usually)
Metals are strong and ______ but bendable. Non-metals are usually _____ or they will snap.
Metals will _____ when freshly cut or scratched, whereas non-metals are usually dull
Metals have higher _______ than non-metals (i.e. they weigh more)
Metals can be used to make ______ (a mixture of different metals)
Words - alloys, electricity, solids, weak, densities, temperatures, tough, shine

3. Reactions of metals with oxygen
When a metal reacts with oxygen it will form a METAL OXIDE. This is what happens when a metal rusts or burns.
METAL + OXYGEN METAL OXIDE Mg O
Copy and complete the following reactions:
Magnesium + oxygen
Copper + oxygen
Calcium + oxygen
Iron + oxygen

4. Reactions of metals with water
When a metal reacts with water hydrogen is always given off. The other product will be either a metal hydroxide or a metal oxide.
METAL + WATER METAL OXIDE + HYDROGEN
METAL + WATER METAL HYDROXIDE + HYDROGEN
Copy and complete the following reactions:
Sodium + water
Potassium + water
Calcium + water
Iron + steam

5. Complete the following reactions:
Lithium + water
Lithium + hydrochloric acid
Silver + oxygen
Magnesium + sulphuric acid
Potassium + oxygen
Aluminium + oxygen
Manganese + water
Sodium + sulphuric acid
Lithium + oxygen
Nickel + hydrochloric acid
Lithium hydroxide + hydrogen
Lithium chloride + hydrogen
Silver oxide
Magnesium sulphate + hydrogen
Potassium oxide
Aluminium oxide
Manganese oxide + hydrogen
Sodium sulphate + hydrogen
Lithium oxide
Nickel chloride + hydrogen

6. Name the following compounds:
For example:
HS = Hydrogen sulphide
Na2CO3 = sodium carbonate
CO2
KBr HI
NaCl
CaCO3
MgCO3
MgSO4
KMnO4
Carbon dioxide
Potassium bromide
Hydrogen iodide
Sodium chloride
Calcium carbonate
Magnesium carbonate
Magnesium sulphate
Potassium permanganate

7. Increasing reactivity
The Reactivity Series
Increasing reactivity
Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Lead
Copper
Silver
Gold
The Reactivity Series lists metals in order of reactivity:

8. Some example reactions…
Prediction
Observations
Zinc + copper sulphate
Zinc + lead nitrate
Copper + lead nitrate
Copper + silver nitrate
Extension work – write down the equations for these reactions

9. Some example reactions…
Prediction
Observations
Zinc + copper sulphate
Reaction DID happen
Zinc + lead nitrate
Copper + lead nitrate
Reaction DID NOT happen
Copper + silver nitrate
Extension work – write down the equations for these reactions

10. Reactions of metals with acids
METAL + ACID SALT + HYDROGEN
e.g. magnesium + hydrochloric acid magnesium chloride + hydrogen Mg H Cl
Copy and complete the following reactions:
Calcium + hydrochloric acid
Zinc + hydrochloric acid
Iron + hydrochloric acid
Lithium + sulphuric acid

11. Reactions of metals carbonates with acid
A metal carbonate is a compound containing a metal, carbon and oxygen.
METAL CARBONATE + ACID SALT + CARBON DIOXIDE + WATER Mg H Cl C O
Copy and complete the following reactions:
Magnesium carbonate + hydrochloric acid
Calcium carbonate + hydrochloric acid
Sodium carbonate + sulphuric acid

12. Reactions of metal oxides with acid
A metal oxide is a compound containing a metal and oxide. They are sometimes called BASES. For example: Mg O Na Al
Magnesium oxide
Sodium oxide
Aluminium oxide
METAL OXIDE + ACID SALT + WATER Mg O H Cl
Copy and complete the following reactions:
Magnesium oxide + hydrochloric acid
Calcium oxide + hydrochloric acid
Sodium oxide + sulphuric acid

13. Neutralisation reactions
A neutralisation reaction occurs when an acid reacts with an alkali. An alkali is a metal oxide or metal hydroxide dissolved in water.
ACID + ALKALI SALT + WATER Na Cl H O
Copy and complete the following reactions:
Sodium hydroxide + hydrochloric acid
Calcium hydroxide + hydrochloric acid
Sodium hydroxide + sulphuric acid
Magnesium hydroxide + sulphuric acid

14. Burning Hydrogen Recall the test for hydrogen: The reaction:
“POP”
The reaction: O H
Notice that no carbon dioxide or carbon monoxide is produced! H O
Hydrogen
Oxygen +
Water

15. Displacement reactions
A displacement reaction is one where a MORE REACTIVE metal will DISPLACE a LESS REACTIVE metal from a compound. Mg
Magnesium
SO4 Cu
Copper sulphate
The magnesium DISPLACES the copper from copper sulphate
SO4 Mg
Magnesium sulphate Cu
Copper
Magnesium + copper sulphate magnesium sulphate + copper

16. Energy from Displacement Reactions
Increasing reactivity
Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Lead
Copper
Silver
Gold
In previous work we considered the reactivity series:
We also looked at displacement reactions, where a more reactive metal will displace a less reactive one from one of its compounds.

17. Energy from Displacement Reactions
Lots of energy
Example 1 – Magnesium and copper sulphate O Cu S
Copper sulphate + Mg O S
Magnesium sulphate + Cu
Copper Mg
Magnesium
Some energy
Example 2 – Zinc and copper sulphate Zn O Cu S
Zinc +
Copper sulphate
Copper
Zinc sulphate

18. Electrical energy from differences in reactivity
Zinc rod
Copper rod
Filter paper soaked in potassium nitrate V
Zinc sulphate
Copper sulphate
The bigger the difference in reactivity, the bigger the voltage

19. Conservation of mass in reactions
In any reaction the total mass of products is the same as the total mass of the reactants
Example 1 – Magnesium oxide and hydrochloric acid Mg O H Cl
1 x magnesium, 1 x oxygen, 2 x hydrogen and 2 x chlorine atoms
Also 1 x magnesium, 1 x oxygen, 2 x hydrogen and 2 x chlorine atoms
Example 2 – Burning methane C H O