SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

· Define rate of reaction.

· Describe some methods used to measure the rates of reactions.

· Explain the effect of different factors on reaction rates.

· Illustrate reaction rates graphically and explain the representation qualitatively using experimental data.

· Recall simple reversible reactions.

· Recognize the reversible sign and explain how reversible reactions reach a state of “balance”.

· Definition of reaction rates.

· Reaction rate.

The effect of: concentration, pressure, temperature, surface area, light and catalysts on rate of reaction. Only qualitative, descriptive, graphical representation required, quantitative data given to illustrate a qualitative effect.

- Marble chips/dilute acids.

- Decomposition of H₂O₂.

- Manganese (IV) oxide to catalyze H₂O₂ decomposition.

- Plantinised asbestos to catalyze SO₂/O₂ combination.

Note: Candidates will be expected to appreciate the applications of reaction rate to laboratory and industrial processes.

· Reversible reactions

Elementary treatment incorporating the idea that two - way reactions can reach a state of “balance”, equilibrium is avoided.

Examples: acids - alkalis plus indicator, chromate/dichromate, acid, hydrated and anhydrous copper (II) sulphate.

Note: The effect of changing concentration, pressure, temperature on position of equilibrium NOT required. The use in industrial processes should be regarded as optimum only (some section in applied chemistry can be used as illustration i.e. Haber process, manufacture of nitric acid, contact process).

SUB-TOPIC

CONTENT

Nitrogen

(4 periods)

· Laboratory preparation of nitrogen.

· Properties and tests of nitrogen.

· Reactions of nitrogen and oxygen with Na, Ca, P,S (Compare reactivity of nitrogen and oxygen)

· Industrial preparation of nitrogen

· Uses of nitrogen

SUB-TOPIC

SPECIFIC OBJECTIVE

CONTENT

Ammonia

(4 periods)

Learners should be able to:

· Explain how ammonia is prepared in the laboratory.

· Explain the differences in chemical reactions of ammonia gas and ammonia in aqueous solution.

· Explain how ammonia is manufactured.

· List the uses of ammonia

· Ammonia .

- The laboratory preparation of

ammonia.

- Properties and tests of ammonia.

- Solubility in water

· Reactions of ammonia gas

- With air / oxygen (catalysed and uncatalysed), with copper (II) oxide, chlorine.

· Reactions of aqueous ammonia.

- Reaction of ammonia solution with dilute acids and metal ions.

· The industrial manufacture of ammonia – the Haber process.

· Uses of ammonia

- Making fertilizers – fertilizers as artificial replacements e.g. NO₂^-, PO₄^3-, SO₄^2-

Industrial production of nitric acid.

Nitric acid

(3 periods)

Learners should be able to:

· Explain the preparation and manufacture of nitric acid

· Explain the reactions of dilute and concentrated nitric acid

· Outline the uses of nitric acid

· Laboratory preparation of nitric acid

· Reactions of nitric acid
- Dilute: reactions with metals, carbonates, hydroxides, oxides
- Concentrated: oxidising action, Iron (II) solution, Sulphur, Copper metal.
- Acidic nature of nitrogen (iv) oxide

Industrial manufacture of nitric acid and it’s uses.

SUB-TOPIC

SPECIFIC OBJECTIVE

CONTENT

Nitrates

(2 periods)

Learners should be able to:

· Name the products when different metal nitrates are heated.

· State the method of preparation of nitrates.

· Test for nitrates in the laboratory.

· Effect of heat on nitrates.
- Action of heat on nitrates of Na, K , Cu, Pb, Ag..

· Test for nitrates
- Brown ring test for nitrates.( Teacher demonstration only)

Nitrogen compounds in the natural and industrial environment

(2 periods)

Learners should be able to:

· Explain the importance of compounds of nitrogen in the natural and industrial environments.

· The nitrogen cycle.

- Converting nitrogen in the air to nitrates in the soil.

- Returning nitrogen to the soil from plants and animals.

- Returning nitrogen from the soil to the air.

· Elements necessary for plant growth

- N, P, K, Ca, Mg, S

SUB-TOPIC

SPECIFIC OBJECTIVE

CONTENT

Sulphur

(6 periods)

Learners should be able to:

· Explain the extraction of sulphur from its ore.

· State the properties of sulphur.

· State the allotropes of sulphur.

· Describe how monoclinic and rhombic sulphur are prepared in the laboratory.

· Outline how sulphur reacts with oxygen, carbon, conc. nitric and conc. Sulphuric acid.

· Extraction of sulphur (the frasch process).

· The allotropes of sulphur.

- Rhombic

- Monoclinic

· Laboratory preparations of monoclinic sulphur and Rhombic sulphur.

· Chemical reaction of sulphur.

- Reaction with non-metals: carbon,

- oxygen.

- Reactions with concentrated acids:

Conc. Nitric acid,

Conc. Sulphuric acid.

· Uses of sulphur

SUB-TOPIC

SPECIFIC OBJECTIVE

CONTENT

Sulphur dioxide

(3 Periods)

Learners should be able to:

· Explain the preparation of sulphur dioxide.

· State the properties of sulphur dioxide.

· Outline the uses of sulphur dioxide.

· Explain the pollution effects of sulphur dioxide on the environment.

· Laboratory preparation of sulphur dioxide (sulphite + acid).

Relate method of collection to properties of the gas.

· Properties of sulphurdioxide

- Acid character.

- Bleaching action

- Test with potassium dichromate (VI).

Note: reducing action not required.

Combination with oxygen (laboratory demonstration; Pt. catalyst.)

· Uses of sulphur dioxide.

· Sulphur dioxide as a pollutant from the combustion of coal and heating oils.

SUB-TOPIC

SPECIFIC OBJECTIVE

CONTENT

Sulphuric acid

(3 periods)

Learners should be able to:

· Describe the manufacture of sulphuric acid.

· State the uses of sulphuric acid.

· Explain the differences in chemical action between dilute and concentrated sulphuric acid.

· Test for sulphates in the laboratory.

· The industrial manufacture of sulphuric acid – the Contact process.

· Uses of sulphuric acid.

· Reactions of dilute sulphuric acid with metals, carbonates and bases.

· Reactions of concentrated sulphuric acid: dilution with water, copper (II) sulphate crystals, ethanol, sucrose.

· Test for sulphates in solution with barium nitrate or barium chloride solution.

Hydrogen sulphide

(3 periods)

Learners should be able to:

· Name the reagents used in the preparation of hydrogen sulphide gas in the laboratory.

· Identify the gas from it’s smell.

· Explain the pollution effects of hydrogen sulphide on the environment

· Preparation of hydrogen sulphide gas in the laboratory.(only test tube preparation)

· Properties of hydrogen sulphide gas (e.g. “bad eggs” smell).

· Pollution effects of hydrogen sulphide on the environment.

SUB-TOPIC

SPECIFIC OBJECTIVE

CONTENT

Chlorine

(6 periods)

Learners should be able to:

· Describe and explain the laboratory preparation and manufacture of chlorine.

· Outline the properties of chlorine.

· Outline the uses of chlorine.

· Preparation of chlorine: Conc. HCl + Potassium mangnate (VII).

· Electrolysis of chloride solutions.

· Properties of chlorine gas.

Reaction of chlorine with metals (Mg, Fe, Na, Zn).

Reaction of chlorine with non metal (P, S).

Reaction of chlorine with:

Water and dilute alkali.

Bromides and iodides Bleaching action of chlorine

Reaction with hydrocarbons (turpentine)

Uses of chlorine

SUB-TOPIC

SPECIFIC OBJECTIVE

CONTENT

Hydrogen chloride

(9 periods)

Learners should be able to:

· Explain the preparation of hydrogen chloride in the laboratory.

· Explain how the composition of hydrogen chloride can be deduced from a series of chemical reactions.

· Explain the properties of hydrogen chloride.

· Explain the effect of a solvent on the properties of hydrogen chloride

· State the uses of hydrogen chloride.

· Test for chloride ions in the laboratory

· State the uses of hydrochloric acid

Preparation of hydrogen chloride in laboratory.(Common salt + conc.H₂ SO₄ )

Deduction of composition of hydrogen chloride using potassium manganate (VII) and iron metal, direct H₂ and Cl₂ combination

Properties of hydrogen chloride.

Reaction of hydrogen chloride with ammonia gas.

Behaviour of hydrogen chloride in water and methylbenzene.

Test for chloride ions.
- Dry solid (action of Conc H₂SO₄₎

- Using barium nitrate and lead (II)

nitrate.

- Using silver (I) nitrate solution.

- Uses of hydrochloric acid

SUB-TOPIC

CONTENT

Water resource pollution

(7 periods)

Industrial and domestic uses of water.

Causes of water pollution

Pollution from fertilizers, insecticides and others.

Agricultural wastes. (only the pollution aspects)

Oil pollution of the sea and lakes; the dispersal of oil slicks.

Hard and soft water

Definition

Causes of hard water

Removal of hardness (temporary and permanent hardness, include ion exchange method).

Water treatment: filtration, fluoridation and desalination.

Sewage: methods of sewage treatment; production of biogas(methane) and fertilizers.

SUB-TOPIC

SPECIFIC OBJECTIVE

CONTENT

Mineral resources and industrial processes

Learners should be able to:

· Outline the application of electrolysis in sodium extraction

· Describe how iron is extracted by reduction.

· Outline how copper is refined by electrolysis.

· Define an alloy.

· State some common alloys and give their composition.

· Describe how sugar is manufactured in an industry.

The following processes should be used to illustrate: -
The chemical principles already covered in the course.

- The influence of the following factors (particular reference to East Africa) availability of raw materials, choice of site, social and economic factors, health and pollution problems, supply and demands.

· Extraction of metals

- Sodium

Occurrence, extraction (downs cell). Uses of

Sodium

- Iron

Occurrence, extraction, uses of iron

(manufacture of steel).

- Copper refining and uses of copper.

- Alloys of metals

Examples of alloys, brass, solder,

duralumin,

bronze and steel their composition.

· Large scale extraction of sugar from sugar cane :

Note: Use of very simple flow – charts of the processes should be encourages.

Some of the processes are covered in the previous topics from Senior one to Senior four.