NITROGEN & ITS COMPOUNDS.

Isolation of nitrogen from air.
Industrial production of nitrogen.
Lab. preparation of nitrogen.
Physical and chemical properties of nitrogen. Uses of nitrogen.

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



Describe isolation of nitrogen from air.
Describe industrial production of nitrogen.
Describe lab preparation of nitrogen.
State physical and chemical properties of nitrogen.
List down uses of nitrogen.

Teacher demonstration, explanations and equations.

Discussion and description.
Drawing schematic diagram for the process.
Teacher demonstration:
Students? record observations made from tests on the gas.
Writing equations of reactions.
Discussion and writing equations.

Aspirator, copper turnings, gas jar, combustion tube, trogh.
charts
Ammonium chloride, sodium nitrate

K.L.B. BK III
PP. 134-135

Longhorn Book
P 186

K.L.B. BK III
PP.135-136

Longhorn Book
PP 188-9

NITROGEN & ITS COMPOUNDS.

Nitrogen (I) oxide. Lab preparation.
Properties and uses of Nitrogen (I) oxide.

By the end of the lesson, the learner should be able to:
To describe Nitrogen (I) oxide.
To list down physical properties of nitrogen (I) oxide.
To describe chemical properties of nitrogen (I) oxide.
To list down uses of nitrogen (I) oxide.

Teacher demonstration: -
Carry out tests on the gas.
Students record observations in a table.
Guided discussion.
Q/A: Deductions from tests carried out.
Discussion of chemical properties and writing of equations.
Teacher elucidates uses of nitrogen (1) oxide.

Ammonium nitrate.
charts

K.L.B. BK III
PP. 139-141

Longhorn
Book III
PP 195-6

NITROGEN & ITS COMPOUNDS.

Nitrogen (II) oxide. Lab preparation.
Properties of the gas.
Nitrogen (1V) oxide Lab preparation.

By the end of the lesson, the learner should be able to:
To describe lab preparation of nitrogen (II) oxide.
To list down physical properties of nitrogen (II) oxide
To describe chemical properties of nitrogen (11) oxide
To describe nitrogen (IV) oxide lab preparation.

Class experiment: Preparation and carrying out tests on the gas.
Observations recorded in a table.
Q/A: Deductions from tests carried out.
Discussion of chemical properties and writing of equations.
Carry out a confirmatory test for the presence of the gas.
Teacher demonstration: - Preparation of the gas and corresponding equation.
Tests on the gas and make observations.

Dil nitric acid, copper turnings.
charts
Conc. nitric acid, copper turnings.

K.L.B. BK III
P. 142
Longhorn
Book III
PP 200-1

NITROGEN & ITS COMPOUNDS.

Properties of Nitrogen (IV) oxide.
Ammonia. Lab preparation of ammonia.

By the end of the lesson, the learner should be able to:
To list down physical properties of nitrogen (IV) oxide
To describe chemical properties of nitrogen (IV) oxide
To state uses of nitrogen (1V) oxide.
To describe lab preparation of ammonia

Deduce physical properties from the table of observations.
To describe chemical properties from the table of observations.
Discuss uses of nitrogen (1V) oxide.
Q/A: Structure of ammonia.
Group experiments: Preparation of ammonia.
Tests on the gas.

charts
Ca(OH)2, NH4Cl Solutions, CaO, litmus papers..M THREE CHEMISTRY TERM TWO 20....

K.L.B. BK III
PP. 144-147

Longhorn
Book III
P 204

NITROGEN & ITS COMPOUNDS.

Properties of ammonia.
Solubility of ammonia.
Reaction of ammonia with metal ions.
Ionic equations of above reactions.
Burning ammonia in the air.

By the end of the lesson, the learner should be able to:
To list down physical properties of ammonia.
To describe an experiment to determine solubility of ammonia.
To prepare aqueous solution of ammonia.
To carry out tests of aqueous ammonia on metal ions.
To write iIonic equations of above reactions.
To describe burning ammonia in the air.

Deduce physical properties from the observations above.
Discuss chemical properties from the observations above.
Write down chemical equations.
Teacher demonstration.
Discussion.
Teacher demonstration: - Preparation of aqueous solution of ammonia.
Class experiments: -
Students record observations when drops of aqueous ammonia are added, then in excess.
Discuss precipitation of metal hydroxides by aqueous ammonia.
Confirmatory tests for various concentrations.
Teacher demonstration
Discussion
Chemical equations of reactions.

charts
2 cm Solutions containing various metal ions.
charts
Conc. Ammonium solution
Hot platinum rod
Oxygen.

K.L.B. BK III
P. 150

K.L.B.
BK III
PP. 152-153

NITROGEN & ITS COMPOUNDS.

Reaction of ammonia with copper (II) Oxide.
Haber process.
Uses of ammonia.

By the end of the lesson, the learner should be able to:
To name products formed when ammonia reacts with hot CuCl2 solid.
To explain reducing properties of ammonia.
Identify raw materials for Haber process and how they are obtained in large scale.
Discuss the Haber process.
Represent Haber process in a schematic diagram.
To list down uses of ammonia.
To list down nitrogenous fertilizers.

Teacher demonstration and discussion.
Write down equations for the reactions.
Discussion and explanations.
Teacher elucidates uses of ammonia and nitrogenous fertilizers.

Granular CuCl2
Combustion tube,
Dry ammonia
U-tube
Gas jar.
Chart- schematic diagram.
charts

K.L.B.
BK III
P. 158

NITROGEN & ITS COMPOUNDS.

Nitric acid. Lab preparation.
Nitric acid Industrial manufacture.

By the end of the lesson, the learner should be able to:
To describe lab preparation of nitric acid.
To describe industrial manufacture of nitric acid.

Teacher demonstration.
Write equations of reaction.
Discussion.
Discussion and writing equations.

Retort stand
Conc. H2SO4
KNO3
Chart
Schematic diagram.

K.L.B. BK III
P. 163

NITROGEN & ITS COMPOUNDS.

Reaction of dilute Nitric acid with metals.
Nitric acid and carbonates.
Reaction of dil. nitric acid with hydrogen carbonates.

By the end of the lesson, the learner should be able to:
To describe reaction of dilute nitric acid with metals.
To write equations of reactions of dilute nitric acid with metals.
To describe action of nitric acid on carbonates and hydrogen carbonates.
Write equations for reaction of dil. nitric acid with hydrogen carbonates.

Class experiment:- making observations and recording them in a table.
Discuss the observations.
Write down equations for the reactions.
Group experiments: - Action of Nitric acid on hydrogen carbonates.
Discussion and corresponding equations.

Magnesium
Zinc
Copper
Solutions of
Na2CO3
NaHCO3
ZnCO3
CuCO3

K.L.B. BK III
PP. 165-166

Longhorn
Book III
PP 166-8

NITROGEN & ITS COMPOUNDS.

Dilute nitric acid and metal hydroxides and oxides.
Reaction of nitric acid as an oxidizing agent.
Uses of nitric acid & nitrates.
Action of heat on nitrates.

By the end of the lesson, the learner should be able to:
Predict results of reacting dilute nitric acid with metal hydroxides and oxides.
Describe reactions of nitric acid as an oxidizing agent.
To state uses of nitrates.
To describe preparation of nitrates.
To write equations of decomposition of nitrates on heating.

Group experiments & writing equations for the reactions.
Class experiments: -
Explain observations made.
Discussion
Equations for the reactions for preparation of nitrates.
Discuss above observations.
Write relevant equations.

Metal hydroxides.
Nitric acid acidified iron sulphate, sulphur, and copper metal.
charts

K.L.B. BK III
P. 168

Longhorn
Book III
PP 238-240

K.L.B. BK III
P. 171

Longhorn Book III
PP 240

NITROGEN & ITS COMPOUNDS.

Test for nitrates.
Nitrogen compounds and the environment.

By the end of the lesson, the learner should be able to:
To carry out tests on nitrates.
To explain the pollution of nitrogen compounds in the environment.
To state ways of reducing environmental pollution by nitrogen compounds.

Class experiments.
Make observations and deductions.
Discuss the brown ring test for nitrates.
Brief guided discussion.

charts

K.L.B. BK III
PP 173-174

Longhorn
Book III
PP 243

SULPHUR AND ITS COMPOUNDS

Extraction of sulphur.
Allotropes of sulphur.
Physical properties of sulphur. Heating 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.
To list physical properties of sulphur.
To describe effects of heat on sulphur.

Illustrate and discuss extraction of sulphur.
Discussion and exposition of new concepts.
Class experiment:
Solubility of sulphur in water, benzene, e.t.c,.
Class experiments:
Heating sulphur gently then strongly.
Discuss the observations.

Chart-the Frasch process.
video
charts

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

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.
Bleaching properties of SO2.
Oxidizing 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.
To carry out experiments to determine bleaching properties of SO2.
To explain Oxidizing 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.
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.

text book
textbook
Experimental worksheets.
Burning magnesium.
Hydrogen sulphide.

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

K.L.B.BK III
P. 195

SULPHUR AND ITS COMPOUNDS

Sulphate and sulphite ions. Uses of SO2.
Sulphuric acid. Contact process of manufacture.

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.
To identify raw materials for manufacture of sulphuric acid.
To describe the contact process.

Class experiments.
Make deductions from the observations made.
Write (ionic) equations for the reactions.
Teacher elucidates uses of SO2.
Discussion using schematic
flow charts.
Writing equations.

Sodium sulphate
Barium chloride
Barium nitrate.
Chart-schematic
Flow charts.

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

SULPHUR AND ITS COMPOUNDS

Properties of conc. H2SO4.
Physical properties of sulphuric acid.

By the end of the lesson, the learner should be able to:
Describe properties of conc. H2SO4.
To dilute conc. sulphuric acid.
State physical properties of sulphuric acid.

Discuss above observations.
Write relevant equations.
Teacher demonstration ? diluting conc. sulphuric acid.
Discuss use of conc. sulphuric acid as a drying and dehydrating agent.

charts
Conc. sulphuric acid.

K.L.B.
BK III
P. 204

SULPHUR AND ITS COMPOUNDS

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

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

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

Magnesium, zinc, copper metals.
charts

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

SULPHUR AND ITS COMPOUNDS

Dilute H2SO4, and metal oxides and hydroxides.
Dilute H2SO4 and metal oxides & hydroxides.
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 investigate reaction of dilute H2SO4 with metal oxides and hydroxides.
To explain reactions of dilute H2SO4 with metal oxides and hydroxides.
To describe preparation of hydrogen sulphide.
To state properties of the gas.

Class expts.
Observing colour changes.
Discussion, writing relevant chemical equations.
Theoretical / descriptive approach.
Writing corresponding equations.
Discuss physical properties of the gas and reaction of the gas with oxygen.

Oxides of magnesium, zinc, copper.
NaOH Solution.
charts

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

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

SULPHUR AND ITS COMPOUNDS

Reaction of the gas with water. Reducing properties of the gas.
Sulphur and its effects on the environment.

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.

Writing chemical equations for the reactions.
Discussion and explanation.

charts

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

ACIDS, BASES AND SALTS.

Strength of acids. Acids in aqueous form.
pH values of acids. Electrical conductivities of aqueous acids.

By the end of the lesson, the learner should be able to:
Define an acid in terms of hydrogen ions.
Explain strength of acids in aqueous form in terms of number of hydrogen ions present.
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.

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.
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.

Magnesium strip, zinc carbonate,
2M HCl,
2M H2SO4,
2M ethanoic acid.
Universal
indicator,
2M ethanoic acid,
dry cells,
carbon electrodes,
milli-ammeters,
wires, switches etc.

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

ACIDS, BASES AND SALTS.

Definition of a base in terms of hydroxide ions.
Neutralization reaction.

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

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.
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.

Red litmus paper, calcium hydroxide solid.
1M HCl,
Calcium hydroxide,
universal indicator.

K.L.B. BK IV
Pages 6-7

ACIDS, BASES AND SALTS.

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

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.
Investigate effect of a polar / non-polar solvent on ammonia gas.
Define an amphoteric oxide.
Identify some amphoteric oxides.

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.
Carry out litmus tests on the resulting solution.
Make observations and deductions thereof.
Write down related balanced chemical equations.
Class experiment:
Carry out acid / base reactions with metal oxides.
Q/A: make deductions from the results.
Writing and balancing relevant equations.

2M NaOH,
2M ammonia solution, universal indicator solutions, dry cells,
carbon electrodes,
milliammeters,
wires, switches etc
Ammonia gas,
Methylbenzene, hydrogen chloride gas.
Ammonia gas,
Methylbenzene.
2M Nitric acid
2M NaOH,
HNO3.
Amphoteric oxides.

K.L.B. BK IV
Pages 7-9
K.L.B. BK IV
Pages 11-12

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.
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:
Write down equations for formation of insoluble chlorides, sulphites and sulphates.
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.

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

student book
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 17-18
K.L.B. BK IV
Pages 20-21

ACIDS, BASES AND SALTS.

Effect of temperature on solubility of a solute in a solvent.
Effects of various salts on soap.

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.
Determine the effects of various salts on soap.

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

KClO3 thermometers, source of heat.
distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+.

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

ACIDS, BASES AND SALTS.
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Removal of hardness of water.
Endothermic and Exothermic Reactions.
Energy level diagrams.

By the end of the lesson, the learner should be able to:
Identify ions for hardness of water.
Identify methods of removing hardness of water.
State merits & demerits of hard water.
To differentiate between endothermic & exothermic reactions.
Represent endothermic reactions with exothermic reactions with energy level diagrams.

Review results of above experiments.
Probing questions & brief discussion.
Assignment.
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.

student book
Ammonium nitrate,
Sodium hydroxide, thermometers.

K.L.B. BK IV
Pages 27-29

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy Notation. Change of state.

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.

CAT
Molar heat of solution.
Molar heat of solution of H2SO4.

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

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

Ammonia nitrate / sodium hydroxide, thermometers.
Conc. H2SO4, thermometers.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy of combustion. Enthalpy of combustion.
Molar heat of displacement of ions.

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.
Define the term molar heat of solution of displacement of ions.
Determine the molar heat of solution of displacement of ions.

Group experiments / teacher demonstration.
Obtain and record results.
Work out calculations.
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.

Ethanol, distilled water, thermometer, clear wick, tripod stand and wire gauze.
Zinc, iron, magnesium, copper sulphate solution.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of solution of neutralization.
Standard enthalpy changes.

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

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.

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

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.
RATES OF REACTION & REVERSIBLE REACTIONS.

Heat of solution hydration energy and lattice energy.
Heat values of fuels.
Environmental effects of fuels.
Effect of concentration on rate of a reaction

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.
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.





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

Exposition of new concepts.
Guided discovery of the relationship between heat solution hydration energy and lattice energy.
Worked examples.
Assignment.
Probing questions and brief discussion.
Q/A & open discussion.
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.

student book
Portions of 2M HCl diluted with different volumes of water,
Stopwatches.

K.L.B. BK IV
Pages 60-64
K.L.B. BK IV
Pages 73-74

RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of time of reaction on the rate of reaction.
Effect of temperature of reactants on rate of reaction.
Effect of change in surface area of reactants on the rate of a reaction.

By the end of the lesson, the learner should be able to:
Explain how the rate or reaction changes as the reaction proceed
Explain the effect of temperature on rate of reaction.
Explain the effect of change in surface area on the rate of a reaction.

Group experiments: investigate volume of gas evolved when magnesium reacts with dilute HCl.
Collect evolved gas and sketch and illustrative graphs.
Discuss the results.
Group experiments: investigate the effects of temperature on the rate of reaction of sodium thiosulphate with dilute HCl.
Sketch and interpret relevant graphs.
Discuss the collision theory and effects of activation energy.
Group experiment/ teacher demonstration.
Compare reactions of marble chips with dilute HCl and that of marble chips powder with equally diluted HCl.
Collect evolved gas in each case.
Teacher asks probing questions related to the observations made.

Magnesium ribbons, stopwatches, conical flask.
100cm3 0.5M HCl, syringes, stoppers, tubes and connectors.
Sodium thiosulphate heated at different temperatures, dilute HCl, stopwatches.
Graph papers.
Marble chips, marble chips powder, syringes, conical flasks with stoppers, 1M HCl.

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

RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of a suitable catalyst on the rate of a reaction
Effect of light on rate of specific reactions.
Reversible reactions.

By the end of the lesson, the learner should be able to:
Explain effects of a suitable catalyst on the rate of a reaction.
Identify reactions that are affected by light.
Write down equations for reversible reactions.

Teacher demonstration: preparation and collection of oxygen gas without using a catalyst, then using manganese (IV) oxide as a catalyst.
Explain the results in terms of activation energy.
Teacher demonstration: decomposition of silver bromide in the presence of light.
Mention other examples of reactions affected by light.
Q/A: review temporary and permanent changes.
Teacher demonstration: heating crystals of hydrated copper (II) sulphate, then ?hydrating? them.
Write the corresponding chemical equations.
Give further examples of reversible reactions.

Hydrogen peroxide, manganese (IV) oxide.
Silver bromide.
Crystals of hydrated copper (II) sulphate.

K.L.B. BK IV
Pages 85-88

RATES OF REACTION & REVERSIBLE REACTIONS.

State of equilibrium in chemical reactions.
Le Chatelier?s Principle.
Effect of change of pressure and temperature on equilibrium shift.
The Haber Process.
The Contact Process.

By the end of the lesson, the learner should be able to:
Define the term equilibrium as used in reversible reactions.
Write down equations of reversible reactions in a state of equilibrium.
State Le Chatelier?s Principle.
Explain the effect of change of pressure & te,perature on equilibrium shift.
Explain the concept optimum conditions of a chemical equilibrium.
Explain factors that change the position of equilibrium of the Harber process.
Explain how change of temperature and pressure affect rate of manufacture of sulphur (VI) acid.

Brief discussion, giving examples of chemical equations for reversible reactions.
Investigate the effect of change of concentration of reactants on equilibrium.
Add 2M sodium hydroxide in steps to bromine water.
Make and record observations.
Discuss the results leading to
Le Chatelier?s Principle.
Q/A: review kinetic theory of matter.
Q/A & discussion on effect of change of pressure / temperature on shifting of equilibrium; giving specific examples of chemical equations.
Written assignment.
Q/A and detailed discussion on change of pressure, temperature, concentration of ammonia and effect of presence of a suitable catalyst on the Haber process.
Probing questions and brief discussion.
Assignment.

student book
Add 2M sodium hydroxide,

K.L.B. BK IV
Pages 94-95