1. Starter:

2. Unit 3 Chemistry in Society Key Area 3 Fertilisers
National 5 Chemistry
Unit 3 Chemistry in Society
Key Area 3
Fertilisers

3. Date Fertilisers Learning Intentions
I know that fertilisers provide the essential elements, nitrogen, phosphorus and potassium, that are needed for healthy plant growth
I can name the catalyst used in the Haber Process
I can write the balanced equation for the Haber Process
I can name the reactants in the Ostwald process
I can work out the percentage composition of a fertiliser

4. Fertilisers
Growing plants require nutrients, including compounds containing nitrogen, phosphorous or potassium. (NPK)
These can be found in fertilisers

5. Fertilisers are………
Fertilisers are substances which restore elements, essential for healthy plant growth, to the soil.

6. Photosynthesis Plants produce their own glucose during photosynthesis.
To be able to photosynthesise efficiently, plants need nutrients from the soil
Nutrients are taken in through the roots so, Nutrients must be soluble in water

7. A Lack of Nutrients affects a plant’s ability to photosynthesise………………………

8. Lack of Nitrogen 1) Reduced root mass 2) Smaller leaf size
3) Lower leaves turn yellow
and die from the tip back

9. Lack of Potassium
Yellowing of the leaf edges

10. Lack of Phosphorus Purple coloration on the underside of the leaves.
In severe deficiencies the plant will be stunted, leaves will turn upward and show purpling of the leaves.

11. Types of Fertilisers Growing plants use up nutrients from the soil
Fertilisers can be natural or Synthetic

12. Natural Fertilisers Plant compost Animal manure Lightning
Nitrogen Fixing Bacteria in the nodules of some plants

13. Nitrogen in Air Lightning Ooo aaar Fertilizer !!
Decaying Plant and Animal Waste
Nitrogen Fixing Bacteria

14. Adding Nitrogen to the Soil
Manure and dead plants and animals decay to release nitrates
Legumes – peas, beans, clover contain bacteria that “fix” nitrogen into nitrates
Lightning flash combines N2 and O2 to produce NO2 which dissolves in rainwater

15. Nitrogen Fixing Bacteria

16. Problem
Increasing human population needs more food than natural fertilisers can provide

17. Artificial Fertilisers
These are man-made compounds which contain water soluble compounds
These compounds are taken up by the roots of plants
The farmer can chose specific fertilisers to replace nutrients that are missing from his soil

18. Starter: Calculate the percentage of:
Oxygen in Al(OH)3
Nitrogen in Mg3N2

19. Ammonia and Nitric Acid
Ammonia and nitric acid are important compounds used to produce soluble, nitrogen-containing salts that can be used as fertilisers.
Ammonia is a pungent, clear, colourless gas which dissolves in water to produce an alkaline solution.

20. Ammonia solutions react with acids to form soluble salts.
ammonia solution + an acid → an ammonium salt + water

21. Activity 10.5 Ammonia Fountain

22. The Haber Process
Ammonia (NH3) is an essential starting point for the production of synthetic fertilisers.
Diatomic nitrogen in the air has a triple covalent bond holding the atoms together.
This requires a large amount of energy to break, so the direct reaction of nitrogen to hydrogen is not usually possible.
The Haber Process overcomes these difficulties.

23. Nitrogen + Hydrogen ⇋ Ammonia
The Haber Process
Nitrogen Hydrogen ⇋ Ammonia
N2(g) H2(g) ⇋ NH3(l)
The double arrow tells us that the reaction is reversible.
This is a problem because, as the ammonia is made, it easily breaks down into the reactants nitrogen and hydrogen again.

24. The Haber Process
To make this process economic and efficient, the following conditions apply…………
Temperature –
A Moderate temperature is used
At low temperatures the forward reaction is too slow to be economical.
If the temperature is increased, the rate of reaction increases but, as the temperature increases, the backward reaction becomes more dominant.

25. The Haber Process Pressure
A High pressure is used. This increases the yield of ammonia.

26. The Haber Process Catalyst
An Iron (Fe) catalyst speeds up the production of ammonia, saving energy costs.
LEARN THIS

27. The Haber Process Condenser
This cools the reaction down, turning ammonia into a liquid which is easier to extract.

28. The Haber Process Recycled reactants
Unreacted nitrogen and hydrogen are returned to the reaction, saving money.

29. Starter

30. Starter - Answer

31. Learning Intentions and Success Criteria
To learn about the Ostwald process
To learn about percentage composition of fertilisers
Success Criteria
I can state the reactants and products of the Ostwald process
I can calculate the percentage composition of fertilisers

32. Ostwald Process
Ammonia is the starting material for the commercial production of nitric acid. (Ostwald process)
The Ostwald process uses ammonia, oxygen and water to produce nitric acid. A platinum catalyst is used in this process.

33. Steps in the Production of Nitric Acid (Ostwald Process)
Ammonia Oxygen → nitrogen monoxide
Nitrogen monoxide Oxygen → Nitrogen dioxide
Nitrogen dioxide Oxygen + water → Nitric acid

34. Percentage Composition of fertilisers
It is useful to be able to calculate exactly what proportion of essential nutrients are present in in a fertiliser. The process is exactly the same as calculating the percentage composition of a metal ore……..

35. Learn This Formula……….
% = total mass of element X total mass of the compound

36. Example 1 What is the percentage of Nitrogen in the fertiliser ammonium nitrate? (NH4NO3)  
Elements in Compound
N x 2
H x 4
O x3
Mass
14 x 2
= 28
1 x 4
= 4
16 x 3
= 48
Total mass = 80g

37. Example 1 What is the percentage of Nitrogen in the fertiliser ammonium nitrate? (NH4NO3)  
Elements in Compound
N x 2
H x 4
O x3
Mass
14 x 2
= 28
1 x 4
= 4
16 x 3
= 48
% of Nitrogen = total mass of element X
total mass of the compound

38. Example 1 What is the percentage of Nitrogen in the fertiliser ammonium nitrate? (NH4NO3)  
Elements in Compound
N x 2
H x 4
O x3
Mass
14 x 2
= 28
1 x 4
= 4
16 x 3
= 48
% of Nitrogen = X 80

39. Example What is the percentage of Nitrogen in the fertiliser ammonium nitrate? (NH4NO3)  
Elements in Compound
N x 2
H x 4
O x3
Mass
14 x 2
= 28
1 x 4
= 4
16 x 3
= 48
% of Nitrogen = %

40. Plenary

41. Unit 3 Key Area: Chemical Analysis

42. Date Chemical Analysis
Learning Intentions
To know about some of the ways chemists can monitor our environment and ensure it remains healthy and safe

43. What would you use the following for?
conical flask
beaker
measuring cylinder
delivery tube
dropper
test tubes/boiling tubes
funnel
filter paper
evaporating basin
pipette with safety filler
burette
thermometer

44. Could you do the following?
Simple filtration using filter paper and a funnel to separate the residue from the filtrate
Use a balance
Methods for the collection of gases including:
collection over water (for relatively insoluble gases)
downward displacement of air (for soluble gases that are less dense than air)
upward displacement of air (for soluble gases that are more dense than air)

45. Methods of heating using Bunsen burners and electric hotplates
Preparation of soluble salts by the reaction of acids with metals, metal oxides, metal hydroxides and metal carbonates
Preparation of insoluble salts by precipitation
Testing the electrical conductivity of solids and solutions

46. Setting up an electrochemical cell using a salt bridge and either metal or carbon electrodes
Electrolysis of solutions using a d.c. supply
Determination of Eh

47. Analytical Methods

48. Testing Gases
Simple tests can be used to identify oxygen, hydrogen and carbon dioxide gases.

49. Titration
A titration can be used to determine accurately, the volumes of solution required to reach the end-point of a chemical reaction.
An indicator is normally used to show when the end-point is reached.
Titre volumes within 0·2 cm3 are considered concordant.
Solutions of accurately known concentration are known as standard solutions.

50. Activity 10.b Titrations
In a titration a pipette is used to transfer a known volume of acid or base into a conical flask. An indicator is then added to the conical flask. The indicator allows the end point of the titration to be easily observed.
A burette is filled with acid or base of a known concentration.
The burette is then used to accurately add known volumes of acid or base into the conical flask. When a colour change is observed, the reaction has reached its end point.

51. Activity 10.9d Flame Testing
When metal compounds are placed in a flame, characteristic colours are produced.
Different metals give different colours, therefore the presence of a metal in a compound can be detected using flame colour.
Flame colours can be found in the data booklet on page 6.

52. Activity 10.9c Precipitation
Precipitation is the reaction of two solutions to form an insoluble salt called a precipitate.
Information on the solubility of compounds can be used to predict when a precipitate will form. The formation of a precipitate can be used to identify the presence of a particular ion.

53. Metal ions can also be detected using precipitation reactions.
The colour of the precipitate formed (insoluble solid) allows us to determine which metal ion was present.
Non-metal ions can also be detected using precipitation.

54. E.g.
Sodium Hydroxide reacting with cobalt(II)
2NaOH(aq) + Co2+(aq) → Co(OH)2(s) + 2Na+(aq)
Lead Nitrate +Potassium Iodide → Lead Iodide + Potassium Nitrate
Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

55. Reporting experimental work
Labelled, sectional diagrams can be drawn for common chemical apparatus.
Data can be presented in tabular form with appropriate headings and units of measurement.
Data can be presented as a bar, line or scatter graph with suitable scale(s) and labels.
A line of best fit (straight or curved) can be used to represent the trend observed in experimental data.

56. Average (mean) values can be calculated from data.
Given a description of an experimental procedure and/or experimental results, an improvement to the experimental method can be suggested and justified.