SULPHUR AND ITS COMPOUNDS

Extraction of sulphur.
Allotropes of sulphur.

By the end of the lesson, the learner should be able to:
To describe extraction of sulphur by Frasch process.
To identify allotropes of sulphur.
To describe preparation of allotropes of sulphur.

Illustrate and discuss extraction of sulphur.
Discussion and exposition of new concepts.

Chart-the Frasch process.
video

K.L.B. BK III
PP.180-181
Longhorn
Book III
PP 126-129

SULPHUR AND ITS COMPOUNDS

Physical properties of sulphur. Heating of sulphur.

By the end of the lesson, the learner should be able to:
To list physical properties of sulphur.

To describe effects of heat on sulphur.

Class experiment:
Solubility of sulphur in water, benzene, e.t.c,.
Class experiments:
Heating sulphur gently then strongly.
Discuss the observations.

charts

K.L.B. BK III
P.184
Longhorn I
Book III
PP 253-255

SULPHUR AND ITS COMPOUNDS

Chemical properties of sulphur.
Uses of sulphur. Sulphur dioxide.

By the end of the lesson, the learner should be able to:
To investigate and describe chemical properties of sulphur.
State uses of sulphur.
Describe lab. preparation of sulphur dioxide.

Group experiments.
Discuss observations.
Write corresponding equations.
Teacher elucidates uses of sulphur.
Teacher demonstration:-
Preparation of sulphur dioxide in a fume chamber/in the open.
Carrying out tests on the gas.

charts

K.L.B.BK III
PP.188-190
Longhorn
Book III
PP 256-8

SULPHUR AND ITS COMPOUNDS

Physical properties of sulphur dioxide.
Acidic properties of SO2.
Reducing action of SO2.

By the end of the lesson, the learner should be able to:
To list down physical properties of sulphur dioxide.
To carry out experiments to determine acidic properties of SO2.
To verify reducing action of SO2.

Discuss the above tests.
Teacher demonstration to verify acidic properties of sulphur dioxide.
Write equations.
Class experiments: make observations and draw conclusions.
Write balanced corresponding equations.

text book
textbook
Experimental worksheets.

K.L.B.BK III
PP 193
Longhorn
Book III
PP 262-3

K.L.B.BK III
P. 195

SULPHUR AND ITS COMPOUNDS

Bleaching properties of SO2.
Oxidizing action of SO2.

By the end of the lesson, the learner should be able to:
To carry out experiments to determine bleaching properties of SO2.
To explain Oxidizing action of SO2.

Discuss the observations made above.
Write corresponding equations.
Q/A: review redox reactions.
Teacher demonstration: - Lowering magnesium into a jar of SO2; effect of SO2 on hydrogen sulphide.
Discuss observations.
Write equations for the reactions.

Burning magnesium.
Hydrogen sulphide.

K.L.B .BK III
P. 194
Longhorn
Book III
PP 263-4

SULPHUR AND ITS COMPOUNDS

Sulphate and sulphite ions. Uses of SO2.

By the end of the lesson, the learner should be able to:
To carry out tests for Sulphate and sulphite ions.

State uses of SO2.

Class experiments.
Make deductions from the observations made.
Write (ionic) equations for the reactions.
Teacher elucidates uses of SO2.

Sodium sulphate
Barium chloride
Barium nitrate.

K.L.B.
BK III P. 200
Longhorn
Book III
PP 268-9

SULPHUR AND ITS COMPOUNDS

Sulphuric acid. Contact process of manufacture.
Properties of conc. H2SO4.

By the end of the lesson, the learner should be able to:
To identify raw materials for manufacture of sulphuric acid.
To describe the contact process.
Describe properties of conc. H2SO4.

Discussion using schematic
flow charts.
Writing equations.
Discuss above observations.
Write relevant equations.

Chart-schematic
Flow charts.
charts

K.L.B. BK III
PP.201-203
Longhorn
Book III
PP 275-6

SULPHUR AND ITS COMPOUNDS

Physical properties of sulphuric acid.
Chemical properties of Sulphuric acid.
Dilute H2SO4, carbonates and hydrogen carbonates.

By the end of the lesson, the learner should be able to:
To dilute conc. sulphuric acid.
State physical properties of sulphuric acid.

To write equations to show that conc. sulphuric acid is a drying and dehydrating agent.
To describe reactions of dilute H2SO4 with metals.
To describe reaction of dilute H2SO4 with carbonates and hydrogen carbonates.

Teacher demonstration ? diluting conc. sulphuric acid.
Discuss use of conc. sulphuric acid as a drying and dehydrating agent.

Discussion and explanations.
Group expts. ? reaction of metals with dilute H2SO4, make observations and relevant deductions; writing corresponding equations.
Discussion, writing relevant equations.

Conc. sulphuric acid.

Magnesium, zinc, copper metals.
charts

K.L.B.
BK III P. 205
Longhorn
Book III
PP 274-5

K.L.B.
BK III P. 206
Longhorn
Book III
PP 276-8

SULPHUR AND ITS COMPOUNDS

Dilute H2SO4, and metal oxides and hydroxides.

By the end of the lesson, the learner should be able to:
To investigate reaction of dilute H2SO4 with metal oxides and hydroxides.

Class expts.
Observing colour changes.

Oxides of magnesium, zinc, copper.
NaOH Solution.

K.L.B.
BK III P. 210
Longhorn
Book III
PP 287-8

SULPHUR AND ITS COMPOUNDS

Dilute H2SO4 and metal oxides & hydroxides.

By the end of the lesson, the learner should be able to:
To explain reactions of dilute H2SO4 with metal oxides and hydroxides.

Discussion, writing relevant chemical equations.

charts

K.L.B.
BK III P. 211

SULPHUR AND ITS COMPOUNDS

Hydrogen sulphide. Preparation of the gas. Reaction of the gas with oxygen.

By the end of the lesson, the learner should be able to:
To describe preparation of hydrogen sulphide.
To state properties of the gas.

Theoretical / descriptive approach.
Writing corresponding equations.
Discuss physical properties of the gas and reaction of the gas with oxygen.

charts

K.L.B.
BK III P. 210
Longhorn
Book III
PP 289-90

SULPHUR AND ITS COMPOUNDS
CHLORINE & ITS COMPOUNDS

Reaction of the gas with water. Reducing properties of the gas.
Sulphur and its effects on the environment.
Lab. preparation of chlorine gas.
Physical properties of chlorine.

By the end of the lesson, the learner should be able to:
To write equations for reaction of the gas with water.
To demonstrate reducing properties of the gas.
To explain environmental pollution caused by sulphur and its compounds.
Describe laboratory preparation of chlorine gas.
State physical properties of chlorine.

Writing chemical equations for the reactions.
Discussion and explanation.
Teacher demonstration ? gas prep. tests on the gas.
Q/A: Relate the properties to the method of collection of the gas.
Write equations for the reaction leading to formation of chlorine.

charts
Conc. HCl, Manganese (IV) oxide.
charts

K.L.B.
BK III P. 212.
Longhorn
Book III
PP 291-2


K.L.B.BK III
P. 219
Longhorn
Book III
PP 298-9

CHLORINE & ITS COMPOUNDS

Chemical properties of chlorine ? reaction with water.

By the end of the lesson, the learner should be able to:
To investigate and explain reaction of chlorine with water.

Teacher demonstration:
Writing chemical equations.

Moist blue litmus papers.

K.L.B.BK III
P. 222
Longhorn
Book III
PP 301-2

CHLORINE & ITS COMPOUNDS

Chemical properties of chlorine - Reaction with metals - Reaction with non-metals.

By the end of the lesson, the learner should be able to:
To investigate and explain reaction of chlorine with metals / non-metals.

Teacher demonstration:
Discussion.
Writing chemical equations.

textbook

K.L.B.BK III
PP.
224 -225
Longhorn
Book III
PP 303-5

CHLORINE & ITS COMPOUNDS

- Oxidizing properties of chlorine.
Chlorine and alkalis.

By the end of the lesson, the learner should be able to:
To investigate and explain reaction of chlorine with reducing a gents.
To investigate and explain reaction of chlorine with alkalis.

Group experiments.
Discuss and explain observations made.
Write corresponding chemical equations.
Teacher demonstration: Bubbling chlorine with dilute cold / hot NaOH solution.
Make observations and account for them.

Expt. Worksheets.
Cold / hot NaOH solutions.

K.L.B. BK III
PP. 226 -227
Longhorn Book
PP 307-8

CHLORINE & ITS COMPOUNDS

Test for chlorides.
Uses of chlorine gas.

By the end of the lesson, the learner should be able to:
To carry out tests for chlorides.
To state uses of chlorine.

Class expts.
Discuss observations, results.
Write chemical equations for the reactions.

Teacher elucidates uses of chlorine.

Expt. Worksheets.
Zinc chloride, litmus paper, conc. Sulphuric acid.

K.L.B.BK III
P. 230
Longhorn Book III
PP 318-319

K.L.B.BK III
P. 231
Longhorn Book III
PP 320

CHLORINE & ITS COMPOUNDS

Hydrogen chloride gas. Lab. prep. Physical properties.
Aqueous hydrogen chloride.

By the end of the lesson, the learner should be able to:
To describe Lab. prep of hydrogen chloride gas.
To investigate and state physical properties of hydrogen chloride gas.
To prepare aqueous hydrogen chloride.

Teacher demonstration.
Carry out tests on the gas and deduce the properties of the gas.
Class experiment leading to deduction of chemical properties of hydrogen chloride gas.

Sodium chloride crystals, conc H2SO4
Distilled water.

K.L.B.BK III
P. 232
Longhorn
Book III
PP 323-4

CHLORINE & ITS COMPOUNDS

Further chemical properties of hydrogen chloride gas.

By the end of the lesson, the learner should be able to:
To determine chemical properties of hydrogen chloride gas.
To carry out confirmatory test for hydrogen chloride gas.

Class experiment leading to deduction of further chemical properties of hydrogen chloride gas / confirmatory test for hydrogen chloride gas.

Ammonia solution.

K.L.B. BK III
PP.
235 -223
Longhorn
Book III
PP 327-331

CHLORINE & ITS COMPOUNDS

Large-scale production of hydrochloric acid.
Uses of hydrochloric acid.

By the end of the lesson, the learner should be able to:
Identify raw materials for manufacture of hydrochloric acid in large scale.
Describe the manufacturing process.
To state uses of hydrochloric acid.

Discussion and giving relevant equations.
Brief discussion.

charts

K.L.B.BK III
P. 237
Longhorn Book III
P 330

CHLORINE & ITS COMPOUNDS
ACIDS, BASES AND SALTS.

Effects of hydrochloric acid on the environment.
Strength of acids. Acids in aqueous form.

By the end of the lesson, the learner should be able to:
To explain effects of hydrochloric acid on the environment.


Define an acid in terms of hydrogen ions.

Explain strength of acids in aqueous form in terms of number of hydrogen ions present.

Discussion and explanation.
Assignment.





Class experiments: investigate reactions of magnesium and zinc carbonate with different acids.
Make and record observations in tabular form.
Make deductions from the observations.
Write relevant chemical equations and ionic equations.
Detailed discussion leading to the definition of an acid and explanation of strength of an acid.

charts




Magnesium strip, zinc carbonate,
2M HCl,
2M H2SO4,
2M ethanoic acid.

K.L.B. BK III
P 238.
Longhorn Book III
PP 334-8





K.L.B. BK IV
Pages 1-4

ACIDS, BASES AND SALTS.

pH values of acids. Electrical conductivities of aqueous acids.
Definition of a base in terms of hydroxide ions.

By the end of the lesson, the learner should be able to:
Determine strength of acids using pH values.
Determine strengths of acids by comparing their electrical conductivities.
Classify acids as either strong or weak in terms of partial dissociations in aqueous solutions.
Define a base in terms of hydroxide ions.

Q/A: review determination of strength of acids using a litmus paper and pH scale.
Class / group experiments: record colour of universal indicator in
2M HCl and 2M ethanoic acid.
Set up voltameters of 2M HCl and 2M ethanoic acid in turns.
Record amounts of current .
Discuss the observations.
Write corresponding ionic equations.
Teacher demonstration:
Dissolve calcium hydroxide in water.
Carry out litmus test on the resulting solution.
Discuss the results; hence define a base in terms of hydroxide ions.

Universal
indicator,
2M HCl,
2M ethanoic acid,
dry cells,
carbon electrodes,
milli-ammeters,
wires, switches etc.
Red litmus paper, calcium hydroxide solid.

K.L.B. BK IV
Pages 4-6

ACIDS, BASES AND SALTS.

Neutralization reaction.

By the end of the lesson, the learner should be able to:
Determine the results of reaction of an acid and a base.

Add 1M HCl to an aqueous solution of Calcium hydroxide drop wise until colour, change of the universal indicator is noted.
Write ionic equation for the reaction.

1M HCl,
Calcium hydroxide,
universal indicator.

K.L.B. BK IV
Page 7

ACIDS, BASES AND SALTS.

Strength of bases.
Dissolving hydrogen chloride gas in water / methylbenzene.

By the end of the lesson, the learner should be able to:
Compare strengths of bases using pH values and electrical conductivity.
Classify bases/ alkali as either strong or weak in terms of complete / partial ionization.
Define a polar and a non-polar solvent.

Carry out pH tests of 2M NaOH and 2M ammonia solution using universal indicator solutions; and observe colour changes.
Carry out electrical conductivity tests of voltameters of the above solutions.
Discussion: relate number of hydroxide ions to pH values and electrical conductivity of bases.
Teacher demonstration:
Dissolving HCl gas in different solvents.
Discuss the observations.
Write down related balanced chemical equations.

2M NaOH,
2M ammonia solution, universal indicator solutions, dry cells,
carbon electrodes,
milliammeters,
wires, switches etc
Ammonia gas,
Methylbenzene, hydrogen chloride gas.

K.L.B. BK IV
Pages 7-9

ACIDS, BASES AND SALTS.

Dissolving ammonia gas in water/ methylbenzene.

By the end of the lesson, the learner should be able to:
Investigate effect of a polar / non-polar solvent on ammonia gas.

Carry out litmus tests on the resulting solution.
Make observations and deductions thereof.
Write down related balanced chemical equations.

Ammonia gas,
Methylbenzene.

K.L.B. BK IV
Pages 11-12

ACIDS, BASES AND SALTS.

Amphoteric oxides.

By the end of the lesson, the learner should be able to:
Define an amphoteric oxide.
Identify some amphoteric oxides.

Class experiment:
Carry out acid / base reactions with metal oxides.
Q/A: make deductions from the results.
Writing and balancing relevant equations.

2M Nitric acid
2M NaOH,
HNO3.
Amphoteric oxides.

K.L.B. BK IV
Pages 12-14

ACIDS, BASES AND SALTS.

Precipitation Reactions.
Solubility of chlorides sulphites and sulphates.

By the end of the lesson, the learner should be able to:
Define a precipitate.
Write ionic equations showing formation of precipitates.
Find out cations that form (in)soluble chlorides, sulphates and sulphites.

Q/A: review definition of a salt.
Class experiment;
Add sodium carbonate or a suitable carbonate to various salt solutions containing Mg2+, Al3+, Ca2+, etc.
Make observations and discuss the results.
Class experiments: measure 2cc of 0.1M solution containing Pb2+ into a test tube.
Add drops of 2M NaCl solution.
(Later 2M Sodium Sulphate and 2M Sodium Sulphate).
Warm the mixture and make observations.
Repeat the procedure using other salt solutions containing other ions.
Tabulate the results.

Soluble carbonates e.g. Na2CO3, K2CO3, (NH4)2CO3
Salt solutions containing Mg2+, Al3+, Ca2+, etc.
0.1M solution containing Pb2+, 2M NaCl solution, 2M sodium sulphate, source of heating.

K.L.B. BK IV
Pages 14-16

ACIDS, BASES AND SALTS.

Equations for formation of insoluble chlorides, sulphites and sulphates.

By the end of the lesson, the learner should be able to:
Write down equations for formation of insoluble chlorides, sulphites and sulphates.

Q/A: review observations made in the above experiments.
Discuss the solubility of the cations.
Write relevant ionic equations.

student book

K.L.B. BK IV
Pages 17-18

ACIDS, BASES AND SALTS.

Complex ions.
Solubility of a salt at a given temperature.
Problems solving on solubility.

By the end of the lesson, the learner should be able to:
Explain formation of complex ions.
Define the term solubility.
Determine solubility of a given salt at room temperature.
Solve problems involving solubility of a solute in a solvent at a given temperature.

Add drops of 2M sodium hydroxide / 2M ammonia solution to a solution containing Mg2+, Zn2+, etc.

Make observations and discuss the results.
Q/A: review the terms saturated, unsaturated solutions & crystallization.
Class experiment: determine mass of a solute that dissolves in 100cc of water at room temperature.
Worked examples.
Supervised practice.
Written assignment.

2M Sodium hydroxide (2M ammonia solution),
solution containing Mg2+, Zn2+, etc.

Suitable solutes.
Evaporating dish, watch glass, heating source, thermometer.

K.L.B. BK IV
Pages 18-20
K.L.B. BK IV
Pages 20-21

ACIDS, BASES AND SALTS.

Effect of temperature on solubility of a solute in a solvent.

By the end of the lesson, the learner should be able to:
Investigate the effect of temperature on solubility of a solute in a solvent.

Experiments involving solubility of KClO3 at different temperatures.
Note temperatures at which crystallization occurs.
Oral questions and discussion.

KClO3 thermometers, source of heat.

K.L.B. BK IV
Pages 22-25

ACIDS, BASES AND SALTS.

Effects of various salts on soap.
Removal of hardness of water.

By the end of the lesson, the learner should be able to:
Determine the effects of various salts on soap.
Identify ions for hardness of water.
Identify methods of removing hardness of water.
State merits & demerits of hard water.

Group experiments: form soap lather in distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+.
Note volume of soap that forms lather readily.
Review results of above experiments.
Probing questions & brief discussion.
Assignment.

distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+.
student book

K.L.B. BK IV
Pages 25-27

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Endothermic and Exothermic Reactions.
Energy level diagrams.

By the end of the lesson, the learner should be able to:
To differentiate between endothermic & exothermic reactions.
Represent endothermic reactions with exothermic reactions with energy level diagrams.

Investigate temperature changes in solution formation.
Obtain changes in temperature when ammonium nitrate and sodium hydroxide are dissolved in water, one at a time.
Probing questions on relative energies of reactants and products in endothermic and exothermic and endothermic reactions.

Ammonium nitrate,
Sodium hydroxide, thermometers.
student book

K.L.B. BK IV
Pages 32-33

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy Notation. Change of state.
CAT

By the end of the lesson, the learner should be able to:
Define the term enthalpy.
Distinguish positive enthalpy change from negative enthalpy change.

Determine the M.P/ B.P of a pure substance.

Q/A and brief discussion.
Class experiments: determine B.P of pure water/ M.P of naphthalene / ice.
Use experimental results to plot temperature-time graphs.
Explain the shape of the graphs.
Q/A: review kinetic theory of matter.
Apply the theory to explain the shape of the graph, and nature of bonding in substances.

Ice, naphthalene, thermometers, graph papers.

K.L.B. BK IV
Pages 35-39

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of solution.

By the end of the lesson, the learner should be able to:
Determine molar heat of solution of given substances.

Dissolve known masses of ammonia nitrate / sodium hydroxide in known volumes of water.
Determine temperature changes.
Calculate molar heat of solution. Supervised practice.

Ammonia nitrate / sodium hydroxide, thermometers.

K.L.B. BK IV
Pages 40-41

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of solution of H2SO4.

By the end of the lesson, the learner should be able to:
Determine molar heat of solution of H2SO4.

Dissolve some known volume of conc. H2SO4 in a given volume of water.
Note the change in temperature.
Work out the molar heat of solution of H2SO4.

Conc. H2SO4, thermometers.

K.L.B. BK IV
Pages 42-45

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy of combustion. Enthalpy of combustion.

By the end of the lesson, the learner should be able to:
Define the term enthalpy of combustion.
Determine the enthalpy of combustion of ethanol.
Explain why actual heats of combustion are usually lower than the theoretical values.

Group experiments / teacher demonstration.

Obtain and record results.


Work out calculations.

Ethanol, distilled water, thermometer, clear wick, tripod stand and wire gauze.

K.L.B. BK IV
Pages 45-48

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of displacement of ions.
Molar heat of solution of neutralization.
Standard enthalpy changes.

By the end of the lesson, the learner should be able to:
Define the term molar heat of solution of displacement of ions.
Determine the molar heat of solution of displacement of ions.
Define the term neutralization.
Determine the molar heat of neutralization of HCl with NaOH.
Define the term standard enthalpy change.
Denote standard enthalpy change with the correct notation.

Group experiments/ teacher demonstration.
Note steady temperature of solutions formed when zinc/ iron / magnesium reacts with copper sulphate solution.
Work out the molar heat of displacement of a substance from a solution of its ions.

Class experiments:
Neutralize 2M HCl of known volume with a determined volume of 1M / 2M sodium hydroxide.
Note highest temperature of the solution.
Work out the molar heat of neutralization.
Solve other related problems.
Assignment.
Exposition & brief discussion.

Zinc, iron, magnesium, copper sulphate solution.

2M HCl of known volume, 1M / 2M sodium hydroxide.
student book

K.L.B. BK IV
Pages 48-50
K.L.B. BK IV
Pages 50-53

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Hess?s Law.

By the end of the lesson, the learner should be able to:
State Hess?s law.

Solve problems related to Hess?s law.

Detailed discussion & guided discovery of the law.
Illustrations of energy cycles and energy levels leading to Hess?s law.
Worked examples.
Supervised practice
Written assignment.

student book

K.L.B. BK IV
Pages 56-57

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Heat of solution hydration energy and lattice energy.

By the end of the lesson, the learner should be able to:
Define the terms lattice energy and hydration energy.
Explain the relationship between heat of solution, hydration energy.
Solve related problems.

Exposition of new concepts.
Guided discovery of the relationship between heat solution hydration energy and lattice energy.
Worked examples.
Assignment.

student book

K.L.B. BK IV
Pages 60-64

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Heat values of fuels.
Environmental effects of fuels.

By the end of the lesson, the learner should be able to:
Define the term fuel.
Describe energy changes when a fuel undergoes combustion.
Outline factors considered when choosing a suitable fuel.
Outline some environmental effects of fuels.
Identify measures taken to reduce environmental
pollution.

Probing questions and brief discussion.
Q/A & open discussion.

student book

K.L.B. BK IV
Pages 64-66

RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of concentration on rate of a reaction
Effect of time of reaction on the rate of reaction.

By the end of the lesson, the learner should be able to:





Explain the effects of change of concentration of reactants on a reaction.

Explain how the rate or reaction changes as the reaction proceed

Group experiments to investigate effect of concentration on rate of reaction using dil. HCl and magnesium ribbons.
Determine the time taken for reactions to be complete.
Calculation of concentration of HCl in moles per litre.
Discuss the observations and sketch illustrative graphs.

Group experiments: investigate volume of gas evolved when magnesium reacts with dilute HCl.
Collect evolved gas and sketch and illustrative graphs.
Discuss the results.

Portions of 2M HCl diluted with different volumes of water,
Stopwatches.
Magnesium ribbons, stopwatches, conical flask.
100cm3 0.5M HCl, syringes, stoppers, tubes and connectors.

K.L.B. BK IV
Pages 73-74
K.L.B. BK IV
Pages 75-79