1. Fertilisers

2. Population and Food Needs
The ever increasing world population means more food is needed and fertilisers are used to grow plants efficiently.

3. Organic fertilisers such as animal manure can be used but additional chemical fertilisers are also needed.
Growing plants need nutrients - soluble compounds containing nitrogen, phosphorus and potassium which are absorbed by roots.
This is why ammonium salts (such as NH4Cl), potassium salts and nitrates (such as KNO3) and phosphates (such as Na3PO4) are important fertilisers as they contain the essential elements that plants need and they are soluble in water.

4. Fertilisers containing Nitrogen (N), Phosphorus (P) and Potassium (K) are known as NPK fertilisers.
When crops are harvested, these nutrients are removed from the soil in the plant and need to be replaced.

5. Effects of Shortages of Nutrients on Plants
Role in Plant growth
Effect of Shortage
Nitrogen
Needed to make protein and chlorophyll
Stunted growth, pale leaves, weak roots
Phosphorus
Needed for strong roots, stem and seeds and for energy transfer
Slow growth of plants, poor fruit
Potassium
Needed to make protein and sugars
Plants stunted with poor resistance to frost, drought and disease

6. Percentage Composition
You have learned to calculate the % of elements in a compound. Ammonium nitrate, NH4NO3 has a formula mass of 80.
Mass of Nitrogen present in the formula mass = 14 x 2 = 28
Percentage of Nitrogen = (28/80) x 100 = 35%

7. The Nitrogen Cycle

8. A drag and drop activity

9. The Nitrogen Cycle

10. Clover, pea and bean plants change atmospheric nitrogen into soluble nitrogen compounds by 'fixing' nitrogen. They are called leguminous plants.
This happens because swellings (or nodules) on the roots contain nitrifying bacteria which add nitrogen to the soil, increasing fertility.
It is cheaper than chemical fertilisers and without pollution problems.
Some nitrifying bacteria are free-living.

11. Problems Caused by the Use of Fertilisers
Fertilisers need to be soluble to get into plants.
Rain can wash fertilisers into rivers and lochs and cause harmful algae and bacteria to grow rapidly.
These remove oxygen from the water and kill fish and plants.

12. Converting Unreactive Nitrogen into Ammonia - the Haber Process
Nitrogen (from the fractional distillation of liquid air) and Hydrogen (from natural gas) are mixed together at a moderately high temperature (400oC) and high pressure with an iron catalyst and nitrogen hydride (ammonia, NH3) is made.
N2(g) + H2(g)  NH3(g) (Unbalanced)

13. The previous reaction is reversible i.e. it can go in both directions.
If too high a temperature is used, the ammonia changes back to nitrogen.
This is why a moderately high, but not too high a temperature is used.
It also explains why not all of the nitrogen and hydrogen are changed into ammonia.

14. /use this animation if you wish to show the process step by step.

15. Use this animation if you wish to show the process as a whole

16. Activity

17. Making Ammonia in the Laboratory
Heating any ammonium compound with alkali produces ammonia
NH4Cl + NaOH  NH3 + NaCl + H2O
This reaction can be used to prove that a compound is an ammonium compound

18. NH3(g) + H2O(l)  NH4OH(aq)
Properties of Ammonia
Ammonia is a colourless gas which turns moist pH paper blue/purple i.e. it is an alkali.
NH3(g) + H2O(l)  NH4OH(aq)
Ammonia has a characteristic smell.
Ammonia is very soluble in water as shown by the fountain experiment.
Ammonia reacts with acids to make salts. These salts can be used as fertilisers as they contain nitrogen.
NH3 + HNO3  NH4NO3

19. /use this animation if you wish to show the process step by step.

20. /use this animation if you wish to show the process step by step.

21. Activity

22. Making Nitric Acid Nitric acid is needed to make some fertilisers.
It can be made as follows:
Nitrogen dioxide, a brown gas, can be made when air (21% oxygen and 78% nitrogen) is sparked for about 20 minutes
N2 + O2  NO2 (Unbalanced)
N2 + 2O2  2NO2 (Balanced)

23. Nitric acid is made if the brown gas formed shaken with water and oxygen.
2H2O + 4NO2 + O2  4HNO3
The spark plug causes the same reaction in a petrol engine, as does lightning.
Time and cost make this method unsuitable to make large quantities of nitric acid

24. Nitrogen is Unreactive
Many elements burn in air to form element oxides, but nitrogen is very unreactive.
In Topic 4 you discovered that there is a triple covalent bond holding nitrogen atoms tightly in the diatomic nitrogen molecule.
It is hard to break this bond and nitrogen does not burn in oxygen.
The spark plug and lightning provide more than enough Activation energy to cause this reaction to happen.

25. The Catalytic Oxidation of Ammonia (Ostwald Process)

26. This is an economic route to making nitrogen dioxide and then nitric acid. It can be done in the laboratory.
The reaction is an example of oxidation as ammonia reacts with oxygen on the platinum catalyst.