1. Oxygen and oxides
2.16 recall the gases present in air and their approximate percentage by volume

2. Air is a mixture of gases which contains 4/5 nitrogen 1/5 oxygen

3. Experiment with copper
2.17 describe how experiments involving the reactions of elements such as copper, iron and phosphorus with air can be used to determine the percentage by volume of oxygen in air
Experiment with copper
This can be demonstrated by the reaction of a fixed amount of air with heated copper. Copper will react with oxygen in the air to form copper(II) oxide.
copper   +   oxygen         copper(II) oxide. 2Cu(s)    +    O2(g)              2CuO(s)

4. A known amount of air is passed backward and forward over the heated copper. As copper(II) oxide is formed, oxygen is removed from the air and the volume of air in the syringes is seen to decrease.
When the reaction is complete, only 80% of the original volume of air remains. This shows that the proportion of oxygen in the air is about 20%.

5. Experiment using iron
If the original volume was 15cm3 and the final volume is 12cm3
then the oxygen used up measured is 3 cm3. % of oxygen
= 3/15 *100
= 20%

6. Experiment with phosphorous

7. 2.18 describe the laboratory preparation of oxygen from hydrogen peroxide

8. EQUATION:. Catalyst. Hydrogen peroxide = Water + Oxygen. 2H2O2
EQUATION: Catalyst Hydrogen peroxide = Water    Oxygen H2O2 = H2O O2   
DESCRIPTION:    The apparatus is set up as shown above.                                     10 volume hydrogen peroxide is added slowly to the flask.                                     [CARE: If O2 is released too quickly the cork will explode out.] Oxygen is collected by downward displacement of water.
  PROPERTIES:     Colourless, odourless gas.                                     Slightly soluble in water (hence fish can breathe in it).                                     Many substances, both elements and compounds,                                     burn in oxygen (and in air which is one fifth oxygen).
TEST:   Oxygen relights a glowing splint.

9. Reaction with magnesium. What precaution you need to take? Why?
2.19 describe the reactions with oxygen in air of magnesium, carbon and sulphur, and the acid base character of the oxides produced
Reaction with magnesium.
What precaution you need to take? Why?
Write a balanced chemical reaction for the same .

10. Reaction with carbon and sulphur

11. Reaction of these oxides with water
MgO
CO2
SO2
Which are acidic and which are basic

12. 2.20 describe the laboratory preparation of carbon dioxide from calcium carbonate and dilute hydrochloric acid
Adding dilute hydrochloric acid to calcium carbonate powder or chips. The carbon dioxide gas is collected by downward delivery.

13. 2.21 describe the formation of carbon dioxide from the thermal decomposition of metal carbonates such as copper(II) carbonate  

14. Observations What is the change in colour of the solid?
What do you think are the new products?
Write a balanced chemical reaction for the reaction that has taken place.

15. 2.22 recall the properties of carbon dioxide, limited to its solubility and density