1. Reactivity Series of Metals
Reactions of Metals
Effect of Heat on Metal Carbonates

2. Reactivity Series of Metals
Chemical Properties of Metals
Metal reaction with cold water & steam
Metal reaction with hydrochloric acid
Reaction of Metals: Displacement Reactions
With aqueous ions of another metal
With the oxide of another metal
Reaction of Metal Oxides
With carbon
With hydrogen
Effect of Heat on Metal Carbonates
Thermal stability & reactivity
Reactivity Series of Metals

3. Recap: Chemical Properties of Metals
Reaction with Water (Cold Water)
Metal + Cold Water  Metal Hydroxide + Hydrogen Gas
Eg. 2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
Which are some metals that react with cold water?

4. Recap: Chemical Properties of Metals
Reaction with Water (Steam)
Metal + Steam  Metal Oxide + Hydrogen Gas
Eg. Mg(s) + H2O(g)  MgO(s) + H2(g)
Which metals only react with steam?

5. Recap: Chemical Properties of Metals
Reaction with Hydrochloric Acid
Metal + Hydrochloric Acid  Salt + Hydrogen Gas
Eg. 2K(s) + 2HCl(l)  2KCl(aq) + H2(g)
The more vigorous the reaction
The higher it is in the reactivity series
The more reactive is the metal

6. Reaction of Metals With the Aqueous Ions of Another Metal
Displacement of metals from solution
More reactive metals can displace less reactive metals from their salt solutions.
This can be used to find the position of metals in the reactivity series.

7. Iron Nail in Copper(II) Sulphate Solution
Observations:
Reddish-brown solid forms on the surface of the iron nail
Blue solution becomes pale green
Fe (s) CuSO4 (aq)  FeSO4 (aq) Cu (s)
Iron
Copper(II) Sulphate
Solution
Iron(II) Sulphate
Solution
Copper

8. Iron Nail in Copper(II) Sulphate Solution
Brown solid: Copper metal
Solution turns pale green
Copper has been removed from the solution.
Iron(II) sulphate solution is pale green in colour.
We say that…
Iron has displaced copper from the copper(II) sulphate solution.

9. What will happen when a piece of magnesium strip is immersed in a solution of copper(II) sulphate?
Think!

10. Some Possible Observations
Deposit of the more reactive metal (from its aqueous solution)
Colour of the solution may change
Heat may be given off
Grey: zinc, iron, lead
Reddish-brown: copper

11. Displacement Reactions are Redox Reactions
The more reactive metal is oxidized
The less reactive metal is reduced
For example,
Chemical Equation:
Fe (s) + CuSO4 (aq)  FeSO4 (aq) + Cu (s)
Ionic Equation:
Fe (s) + Cu2+ (aq)  Fe2+ (aq) + Cu (s)
REDOX reaction!
Copper(II) ions are reduced to become copper atoms
Iron atoms are oxidized to become iron(II) ions

12. Displacement Reactions are Redox Reactions
A more reactive metal:
readily gives up electrons in reactions
has greater tendency to form positive ions
As a result…
A more reactive metal can displace
a less reactive metal,
from its solution or metallic oxide.

13. Reaction of Metals With the Oxide of Another Metal
Displacement of metals from metallic oxides
A more reactive metal can reduce the oxide of a less reactive metal.
For example: Thermit reaction
2Al (s) + Fe2O3 (s)  Al2O3 (s) + 2Fe (l)
Magnesium acts as a fuse. It provides enough energy to start the reaction.

14. Reaction of Metals With the Oxide of Another Metal
Thermit Reaction
2Al (s) + Fe2O3 (s)  Al2O3 (s) + 2Fe (l)
The more reactive the metal is, the more readily it forms compounds.
Unreactive metals tend to stay umcombined.
Iron(III) ions are reduced to become iron atoms
Aluminium atoms are oxidized to become aluminium(III) ions

15. Reaction of Metal Oxides With Carbon
Carbon can remove oxygen from the oxides of metals that are not too high up in the Reactivity Series.
The lower the position of a metal in the Reactivity Series, the easier it is for carbon to remove oxygen from the metal oxide.

16. Reaction of Metal Oxides With Carbon
potassium oxide
sodium oxide
calcium oxide
magnesium oxide
oxides are not reduced by carbon
zinc oxide
iron(II) oxide
lead(II) oxide
copper(II) oxide
oxides are reduced by carbon
silver oxide
oxide is reduced by heating
silver oxide decomposed to give silver and oxygen

17. Reaction of Metal Oxides With Carbon
The Importance!
Reaction of Metal Oxides With Carbon
metals need to be extracted from their ores before we can use them
metals below magnesium are often extracted from their ores by reduction with carbon (WHY?)
metals above zinc cannot be extracted by reduction with carbon bc they are stable (THEN WHAT?)

18. metal oxide + hydrogen  metal + steam
Reaction of Metal Oxides With Hydrogen
Hydrogen can remove oxygen from metallic oxides, producing the metal and water(steam).
metal oxide + hydrogen  metal + steam
The lower the position of a metal in the Reactivity Series, the easier it is for hydrogen to remove oxygen from the metal oxide.

19. reaction with hydrogen
Reaction of Metal Oxides With Hydrogen
metal oxide
reaction with hydrogen
potassium oxide
sodium oxide
calcium oxide
magnesium oxide
zinc oxide
heated metal oxides are not reduced by hydrogen
iron(II) oxide
lead(II) oxide
copper(II) oxide
silver oxide
heated metal oxides are reduced by hydrogen

20. Effect of Heat on Metal Carbonates: Thermal Stability & Reactivity
Most carbonates decompose when heated strongly to produce a metal oxide and carbon dioxide gas.
The ease of decomposition depends on the position of the metal in the reactivity series.
Recall the reactivity series.

21. Thermal Stability of Metal Carbonates
Effect of Heat
Potassium Carbonate
Stable to heat
No visible reaction
Sodium Carbonate
Calcium Carbonate
Decomposes into metal oxide and carbon dioxide
Magnesium Carbonate
Zinc Carbonate
Iron (III) Carbonate
Lead Carbonate
Copper(II) Carbonate
Silver Carbonate
Decomposes into silver and carbon dioxide 
Metal Metal Oxide + Carbon Dioxide
Silver carbonate decomposes to form silver oxide, which further decomposes to silver bc it is thermally unstable.

22. Reactions with water & dilute acids:
More vigorous reaction
 Higher in the reactivity series
 The metal is more reactive
Reaction with metal carbonates:
The more stable the metal carbonate is to heat, the higher it is in the reactivity series.

23. Class Activity & Discussion
Check this out!
ctions/projectfolder/flashfiles/redox/home.html
Class Activity & Discussion

24. So, what have you learnt today?
Displacement Reaction
They are redox reactions.
A more reactive metal can displace a less reactive metal, from its solution or metallic oxide.
Carbonates: Thermal stability & reactivity
The more stable the metal carbonate is to heat, the higher it is in the reactivity series.