THE MOLE

Mole, molar mass and R.A.M.
Number of moles in a substance.

By the end of the lesson, the learner should be able to:
Define the term mole as a quantity of measurement.
Relate the mole to R.A.M and molar mass.
Calculate number of moles in a given mass of a substance.

Discuss various analogies that lead to the definition of the mole.
Expose the meaning of R.A.M., Avogadro?s constant and molar mass.
Worked examples.
Supervised practice.

Chart- table of molar masses of elements.
student book

K.L.B. BK III
PP. 27-31
Longhorn
Book III
PP 34-35

THE MOLE

Relative molecular mass & Relative formula mass.
Moles and Avogadro?s number.
Empirical Formula.
Molecular formula.
Concentration of a solution.
Molarity of a solution.
Preparation of molar solutions.
Calculators on molar solutions.

By the end of the lesson, the learner should be able to:
Define relative molecular mass.
Calculate RMM of a compound.
Calculate number of particles in a given number of moles.
Determine empirical formula of a compound given percentage composition by mass.
Define molecular formula of a compound.
Find molecular formula given percentage composition of a compound by mass.
Define concentration of a solution.
Find concentration of a solution in grams/litre and moles/litre.
Define molarity of a solution.
Find molarity of a solution in M/dm?
Define molar solutions.
Prepare molar solutions.
Solve numerical calculations on molar solutions.
Problems on molar solutions.

Q/A: - Review formulae of compounds.
Complete a table of compounds and their molecular / formula mass.
Review standard form of numbers.
Worked examples.
Supervised exercise.
Supervised practice.
Assignment.
Worked examples.
Supervised practice.
Q/A: - Equivalent ratios, e.g. 4g dissolved in 500cm? and
8g in 1 litre.
Worked examples on concentration of solutions.
Teacher explains that molarity of a solution is given in moles of the solute per litre.
Supervised exercise.
Q/A: - Description of preparation of molar solutions.
Assignment.

Calculators.
student book
Calculators.
chart
student book
Volumetric flasks, teat droppers/wash bottle.
Sodium hydrogen pellets.
Weighing balance.

K.L.B.BK III
PP. 34-35

Longhorn Book III PP 44-60

K.L.B.BK III
P. 45

Longhorn
Book III
PP 73-75

THE MOLE

Dilution of solutions.
Stoichiometry of a chemical reaction.
Stoichiometric equations.
Stoichiometric equations of various reactions.

By the end of the lesson, the learner should be able to:
Calculate molarity of a solution after dilution.
To determine mole ratio of given reactions.
To define a stoichiometric equation.
To investigate and determine Stoichiometric equations of various reactions.

Group experiments.
Calculations.
Group experiments: - Determine masses, hence moles of reacting CuSO4 solution and iron metal.
To write stoichiometric equations of the above reactions.
Class experiments.
Problem solving.

student book
CuSO4 solution and iron metal.

K.L.B. BK III
PP. 76-81

Volumetric Analysis.

Apparatus used in titration experiments.
Titration process.
Titration experiment (Neutralization reaction)
Titration experiment (Neutralization reaction)

By the end of the lesson, the learner should be able to:
To use and read a pipette and a burette.
To define titration as a process.
Define a titration end-point.
To carry out a titration experiment and obtain accurate results.
To carry out calculations from experimental results.

Discussion and practical use of the apparatus.
Emphasis is laid on need to sterilize the apparatus after use.
Review by Q/A: -
-Indicators and colour changes.
-Choice of indicators.
-Balanced chemical equations.
Discuss characteristics of a good titre, when an an-end point is attained.
Class experiments: - To neutralize HCl with NaOH solution.
Fill in a table of results.
Find the average base used.
Step-by-step calculations.

Pipettes
Burettes.
Indicators
Suitable acid and base.
student book
Calculators.

K.L.B. BK III
PP. 63-64
Longhorn
Book III
PP 104-8

Volumetric Analysis.

Basicity of an acid.
Standardization of HCl.
Concentration of HCl.
Redox Titration Reactions.

By the end of the lesson, the learner should be able to:
To define basicity of an acid.
To define standardization of HCl.
To calculate concentration of HCl from experimental results.
To standardize a solution with an iron (II) salt.

Complete a table of number of replaceable hydrogen ions of an acid; hence define basicity of an acid.
Write corresponding ionic equations.
Class experiments.
Calculations & supervised practice.
Experiment and calculations.

student book
Dilute HCl, Na2CO3 solutions.
Potassium Magnate
(VII)

K.L.B. BK III
P. 73

Volumetric Analysis.
Volumetric Analysis.
NITROGEN & ITS COMPOUNDS.

Water of crystallization.
Formula mass of ammonium iron (II) sulphate.
Formula mass of a given salt.
Atomicity of gases.
Mass and volume of gases.
Molar gas volume.
Combining volumes of gases.
Gay Lussac?s Law.
Isolation of nitrogen from air.

By the end of the lesson, the learner should be able to:
To determine amount of water of crystallization in ammonium iron sulphate crystals.
To find formula mass of ammonium iron (II) sulphate.
To solve numerical problems involving water of crystallization.
To define atomicity of gases.
To determine mass and volume of gases.
To define molar gas volume.
To compare combining volumes of two reacting gases.
To state Gay Lussac?s Law.
To compare Gay Lussac?s Law with Avogadro?s Law.
To solve numericals using Gay Lussac?s Law.
Describe isolation of nitrogen from air.

Teacher exposes the formula of water of crystallization.
Class experiment.
Filling in a table of results.
Calculations from experimental results.
Problem solving from sample results.
Review by Q/A atoms and molecules; hence the definition.
Discuss a table of gases and their atomicity.
Teacher demonstration: - Determining mass of known volumes of oxygen / CO2.
Use the above results to describe volume of one mole of a gas.
Discuss molar gas volume at R.T.P and S.T.P conditions.
Teacher demonstration: - Determining volumes of reacting gases; hence deduce volume rations.
Teacher exposes the law; and compares it with Gay Lussac?s Law.
Worked examples.
Supervised practice.
Teacher demonstration, explanations and equations.

Ammonium
Iron (II)
Sulphate crystals.
Dilute sulphuric (VI) acid.
student book
Lubricated syringes
Oxygen/
CO2.
student book
Aspirator, copper turnings, gas jar, combustion tube, trogh.

K.L.B. BK III
P. 76
K.L.B. BK III
79 ? 80
Longhorn
Book III
PP 126-127

NITROGEN & ITS COMPOUNDS.

Industrial production of nitrogen.
Lab. preparation of nitrogen.
Physical and chemical properties of nitrogen. Uses of nitrogen.
Nitrogen (I) oxide. Lab preparation.

By the end of the lesson, the learner should be able to:
Describe industrial production of nitrogen.
Describe lab preparation of nitrogen.
State physical and chemical properties of nitrogen.
List down uses of nitrogen.
To describe Nitrogen (I) oxide.

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.
Teacher demonstration: -
Carry out tests on the gas.
Students record observations in a table.
Guided discussion.

charts
Ammonium chloride, sodium nitrate
Ammonium nitrate.

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

Longhorn Book
PP 188-9

NITROGEN & ITS COMPOUNDS.

Properties and uses of Nitrogen (I) oxide.
Nitrogen (II) oxide. Lab preparation.
Properties of the gas.
Nitrogen (1V) oxide Lab preparation.
Properties of Nitrogen (IV) oxide.

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

Q/A: Deductions from tests carried out.
Discussion of chemical properties and writing of equations.
Teacher elucidates uses of nitrogen (1) oxide.
Class experiment: Preparation and carrying out tests on the gas.
Observations recorded in a table.
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.
Deduce physical properties from the table of observations.
To describe chemical properties from the table of observations.
Discuss uses of nitrogen (1V) oxide.

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

K.L.B. BK III
P. 141
Longhorn
Book III
PP 191-2

NITROGEN & ITS COMPOUNDS.

Ammonia. Lab preparation of ammonia.
Properties of ammonia.
Solubility of ammonia.

By the end of the lesson, the learner should be able to:
To describe lab preparation of ammonia
To list down physical properties of ammonia.
To describe an experiment to determine solubility of ammonia.

Q/A: Structure of ammonia.
Group experiments: Preparation of ammonia.
Tests on the gas.
Deduce physical properties from the observations above.
Discuss chemical properties from the observations above.
Write down chemical equations.
Teacher demonstration.
Discussion.

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

K.L.B. BK III
PP. 147-148

NITROGEN & ITS COMPOUNDS.

Reaction of ammonia with metal ions.
Ionic equations of above reactions.
Burning ammonia in the air.
Reaction of ammonia with copper (II) Oxide.
Haber process.
Uses of ammonia.
Nitric acid. Lab preparation.
Nitric acid Industrial manufacture.
Reaction of dilute Nitric acid with metals.

By the end of the lesson, the learner should be able to:
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.
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.
To describe lab preparation of nitric acid.
To describe industrial manufacture of nitric acid.
To describe reaction of dilute nitric acid with metals.
To write equations of reactions of dilute nitric acid with metals.

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.
Teacher demonstration and discussion.
Write down equations for the reactions.
Discussion and explanations.
Teacher elucidates uses of ammonia and nitrogenous fertilizers.
Teacher demonstration.
Write equations of reaction.
Discussion.
Discussion and writing equations.
Class experiment:- making observations and recording them in a table.
Discuss the observations.
Write down equations for the reactions.

2 cm Solutions containing various metal ions.
charts
Conc. Ammonium solution
Hot platinum rod
Oxygen.
Granular CuCl2
Combustion tube,
Dry ammonia
U-tube
Gas jar.
Chart- schematic diagram.
charts
Retort stand
Conc. H2SO4
KNO3
Chart
Schematic diagram.
Magnesium
Zinc
Copper

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

K.L.B. BK III
P. 161

Longhorn
Book III
PP 126 -226

NITROGEN & ITS COMPOUNDS.

Nitric acid and carbonates.
Reaction of dil. nitric acid with hydrogen carbonates.
Dilute nitric acid and metal hydroxides and oxides.
Reaction of nitric acid as an oxidizing agent.

By the end of the lesson, the learner should be able to:
To describe action of nitric acid on carbonates and hydrogen carbonates.
Write equations for reaction of dil. nitric acid with hydrogen carbonates.
Predict results of reacting dilute nitric acid with metal hydroxides and oxides.
Describe reactions of nitric acid as an oxidizing agent.

Group experiments: - Action of Nitric acid on hydrogen carbonates.
Discussion and corresponding equations.
Group experiments & writing equations for the reactions.
Class experiments: -
Explain observations made.

Solutions of
Na2CO3
NaHCO3
ZnCO3
CuCO3
Metal hydroxides.
Nitric acid acidified iron sulphate, sulphur, and copper metal.

K.L.B. BK III
P. 167

Longhorn
Book III
229-30

NITROGEN & ITS COMPOUNDS.

Uses of nitric acid & nitrates.
Action of heat on nitrates.
Test for nitrates.
Nitrogen compounds and the environment.

By the end of the lesson, the learner should be able to:
To state uses of nitrates.
To describe preparation of nitrates.
To write equations of decomposition of nitrates on heating.
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.

Discussion
Equations for the reactions for preparation of nitrates.
Discuss above observations.
Write relevant equations.
Class experiments.
Make observations and deductions.
Discuss the brown ring test for nitrates.
Brief guided discussion.

charts

K.L.B. BK III
P. 171

Longhorn Book III
PP 240

SULPHUR AND ITS COMPOUNDS

Extraction of sulphur.
Allotropes of sulphur.
Physical properties of sulphur. Heating of sulphur.
Chemical properties 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.
To investigate and describe chemical properties of 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.
Group experiments.
Discuss observations.
Write corresponding equations.

Chart-the Frasch process.
video
charts

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

SULPHUR AND ITS COMPOUNDS

Uses of sulphur. Sulphur dioxide.
Physical properties of sulphur dioxide.
Acidic properties of SO2.
Reducing action of SO2.
Bleaching properties of SO2.
Oxidizing action of SO2.
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:
State uses of sulphur.
Describe lab. preparation of sulphur dioxide.
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.
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.

Teacher elucidates uses of sulphur.
Teacher demonstration:-
Preparation of sulphur dioxide in a fume chamber/in the open.
Carrying out tests on the gas.
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.
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.

charts
text book
textbook
Experimental worksheets.
Burning magnesium.
Hydrogen sulphide.
Sodium sulphate
Barium chloride
Barium nitrate.
Chart-schematic
Flow charts.

K.L.B.BK III
PP 191- 192
Longhorn Book
P 258

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

SULPHUR AND ITS COMPOUNDS

Properties of conc. H2SO4.
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:
Describe properties of conc. H2SO4.
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.

Discuss above observations.
Write relevant equations.
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.

charts
Conc. sulphuric acid.
Magnesium, zinc, copper metals.

K.L.B.
BK III
P. 204

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

SULPHUR AND ITS COMPOUNDS
ACIDS, BASES AND SALTS.

Reaction of the gas with water. Reducing properties of the gas.
Sulphur and its effects on the environment.
Strength of acids. Acids in aqueous form.

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

Writing chemical equations for the reactions.
Discussion and explanation.
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. 212.
Longhorn
Book III
PP 291-2

ACIDS, BASES AND SALTS.

pH values of acids. Electrical conductivities of aqueous acids.
Definition of a base in terms of hydroxide ions.
Neutralization reaction.
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:
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.
Determine the results of reaction of an acid and a base.
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.

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

Universal
indicator,
2M HCl,
2M ethanoic acid,
dry cells,
carbon electrodes,
milli-ammeters,
wires, switches etc.
Red litmus paper, calcium hydroxide solid.
1M HCl,
Calcium hydroxide,
universal indicator.
2M NaOH,
2M ammonia solution, universal indicator solutions, dry cells,
carbon electrodes,
milliammeters,
wires, switches etc
Ammonia gas,
Methylbenzene, hydrogen chloride gas.
Methylbenzene.
2M Nitric acid
HNO3.
Amphoteric oxides.

K.L.B. BK IV
Pages 4-6
K.L.B. BK IV
Pages 7-9

ACIDS, BASES AND SALTS.

Precipitation Reactions.
Solubility of chlorides sulphites and sulphates.
Equations for formation of insoluble 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.
Write down equations for formation of insoluble chlorides, sulphites and sulphates.

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

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.
student book

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

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

ACIDS, BASES AND SALTS.
RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of temperature on solubility of a solute in a solvent.
Effects of various salts on soap.
Removal of hardness of water.
Effect of concentration on rate of a reaction

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.
Identify ions for hardness of water.
Identify methods of removing hardness of water.
State merits & demerits of hard water.
Explain the effects of change of concentration of reactants on a reaction.

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

KClO3 thermometers, source of heat.
distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+.
student book
Portions of 2M HCl diluted with different volumes of water,
Stopwatches.

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

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

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.
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.
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.

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.
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.
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.

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.
Hydrogen peroxide, manganese (IV) oxide.
Silver bromide.
Crystals of hydrated copper (II) sulphate.
student book
Add 2M sodium hydroxide,

K.L.B. BK IV
Pages 75-79
K.L.B. BK IV
Pages 91-93

RATES OF REACTION & REVERSIBLE REACTIONS.
ELECTRO-CHEMISTRY.
ELECTRO-CHEMISTRY.
ELECTRO-CHEMISTRY.

The Contact Process.
Redox reactions.
Oxidizing Numbers.
Displacement reactions.

By the end of the lesson, the learner should be able to:
Explain how change of temperature and pressure affect rate of manufacture of sulphur (VI) acid.
Describe redox reactions in terms of gain / loss of electrons.
Identify oxidizing / reducing agents involved in redox reactions.
Outline rules of assigning oxidation numbers.
Determine the oxidation numbers of an element in a given compound.
Explain the use of oxidation numbers in naming compounds.
Explain change of oxidation numbers during redox / displacement reactions. Arrange elements in order of their reducing power.

Probing questions and brief discussion.
Assignment.
Q/A: review cations, anions and charges.
Write down ionic half equations and identify reducing / oxidizing agents.
Exposition and giving specific examples.
Work out oxidizing number of elements in given compounds.
Copy and complete a table of compounds containing elements that more than one oxidation number.
Class standard experiments: reacting metals with solutions containing metal ions.
Taking note of reactions and those that do not take place; and tabulating the results.

student book
Metals: Ca, Na, Zn, Fe, Pb, and Cu.
Solutions containing Ca2+, Mg2+, Zn2+, Fe2+.

K.L.B. BK IV
Pages 103-104

ELECTRO-CHEMISTRY.

The oxidizing power of an element.
Cell diagrams.
Standard Electrode Potentials.
Standard electrode potential series.

By the end of the lesson, the learner should be able to:
Arrange elements in order of their oxidizing power.
Define the terms electrode, potential and e.m.f. of an electrochemical cell.
Describe components of a cell diagram.
Draw cell diagrams using correct notations.
Identify standard conditions for measuring electrode potentials.
Define the term standard electrode potential of a cell.
Write half reactions of electrochemical cells.
Recall the order of standard electrode potentials.
Compare oxidizing and reducing powers of substances.

Teacher demonstration / group expts:
Adding halogens to solutions containing halide ions.
Tabulate the results.
Discuss the results and arrive at the oxidizing power series of halogens.
Teacher demonstration: Zinc/ copper cell.
Q/A & discussion: changes in oxidation numbers.
Exposition: cell diagram and deducing the direction of electron flow.
Descriptive and expository approaches: teacher exposes new concepts.
Q/A: review reactivity series, oxidizing agent, reducing agent.
Exposition: the order of standard electrode potentials.
Discussion: oxidizing and reducing powers of substances.

Halogens:
Cl2 (g),
Br2 (l),
I2 (s).
Halides:
KCl, KBr, KI.
Zinc/ copper cell.
student book

K.L.B. BK IV
Pages 120-122

ELECTRO-CHEMISTRY.

Emf of a cell.
Possibility of a reaction to take place.
Primary and secondary chemical cells.

By the end of the lesson, the learner should be able to:
Calculate emf of a cell using standard electrodes potentials.
Predict whether a reaction will take place or not using standard electrode potentials.
Describe the functioning of primary and secondary chemical cells.

Q/A: review half-cells.
Worked examples; supervised practice.
Assignment.
Worked examples.
Oral exercise.
Exposition of new concepts and brief discussion

student book

K.L.B. BK IV
Pages 133-136

ELECTRO-CHEMISTRY.
ELECTRO-CHEMISTRY.
METALS
METALS
METALS
METALS

Electrolysis of dilute NaCl.
Electrolysis of brine.
Electrolysis of dilute sulphuric (VI) acid.
Factors affecting electrolysis.
Application of electrolysis.
Faraday?s law of electrolysis.
Ores of some metals.
Occurrence and extraction of sodium.
Occurrence and extraction of aluminium.
Occurrence and extraction of iron.

By the end of the lesson, the learner should be able to:
Define the term electrolysis.
Explain the concept of preferential discharge of ions.
Identify products of electrolysis of brine.
Identify products of electrolysis of dilute sulphuric (VI) acid.
Explain factors that affect electrolytic products discharged at electrodes.
Describe some applications of electrolysis.
State Faraday?s law of electrolysis.
Solve problems related to Faraday?s law of electrolysis.
Name the chief ores of some metals.
Describe occurrence and extraction of sodium.
Describe occurrence and extraction of aluminium.
Describe occurrence and extraction of iron.

Teacher demonstration: electrolysis of dilute sodium chloride with carbon electrodes.
Test for gases collected.
Write down equations of reactions at each electrode.
Discussion: preferential discharge of ions at electrodes.
Teacher demonstration/ group experiments.
Test for the products of electrolysis.
Write relevant equations.
Q/A: review the electrochemical series of elements.
Teacher writes down order of ease of discharge of ions at electrodes.
Discussion: other factors; giving suitable examples.
Probing questions and brief discussion on applications of electrolysis.
Practical assignment on electrolysis: electroplating an iron nail with a suitable metal.
Discuss above results, leading to Faraday?s law of electrolysis.
Worked examples.
Assignment.
Exposition and brief discussion.
Oral questions on electrolysis and equations at electrodes.
Brief discussion on occurrence and extraction.
Brief discussion.
Write relevant chemical equations.

Dilute sodium chloride voltameter.
Brine voltameter.
Sulphuric acid voltameter.
student book
Suitable voltameter.
Weighing balance, stop watch, copper sulphate voltameter.
Chart: Down?s cell.
student book
Chart: Blast furnace.

K.L.B. BK IV
Pages 141-144
K.L.B. BK IV
Pages 161-4

METALS

Occurrence and extraction of zinc.
Extraction of lead.
Occurrence and extraction of copper.
Physical properties of some metals.

By the end of the lesson, the learner should be able to:
Describe occurrence and extraction of zinc by electrolysis and reduction methods.
Explain how lead is extracted.
Describe extraction of copper.
State general properties of metals.
Explain the difference in physical properties of metals.

Brief discussion.
Write relevant chemical equations.
Q/A & brief discussion.
Write balanced chemical equations leading to extraction of lead.
Write balanced chemical equations leading to extraction of copper.
Compare physical properties of some metals as summarized in a chart.
Q/A & discussion based on physical properties.

Flow chart: extraction of Zinc.
Flow chart: extraction of lead.
Flow chart: extraction of copper.
student book

K.L.B. BK IV
Pages 175-9

METALS

Reaction of metals with oxygen.
Reaction of metals with cold water and steam.

By the end of the lesson, the learner should be able to:
Explain effect of burning metals in air.
Describe reaction of metals with cold water and steam.
Arrange the metals in order of reactivity with cold water and steam.

Teacher demonstration / Group experiments.
Burning some metals in air.
Write relevant equations.
Brief discussion.
Class experiments:
Investigate reaction of some metals with cold water and steam.
Analyse the results.

Common lab. metals.
Metals: Al, Zn, Fe, Cu.

K.L.B. BK IV
Pages 184-6

METALS

Reaction of metals with chlorine.
Reaction of metals with acids.
Uses of metals.
Environmental effects of extraction of metals.

By the end of the lesson, the learner should be able to:
Describe the reaction of metals with chlorine.
Describe and explain reaction of metals with acids.
State uses of some metals and alloys.
Identify some environmental effects of extraction of metals.

Teacher demonstration in a fume cupboard / in the open.
Investigate reaction of metals with chorine
Write corresponding equations.
Group experiments: investigate reaction of metals with dilute acids.
Teacher demonstration: investigate reaction of metals with concentrated acids.
Discuss the observations made and write relevant chemical equations.
Q/A & brief discussion;
Uses of Sodium, Aluminium, Zinc, Iron and Copper & some alloys.
Oral questions and open discussion.
Assignment / Topic review.

Metals: Al, Zn, Fe, Cu.
Metals: Al, Zn, Fe, Cu.
Acids; HCl, HNO3, H2SO4.
student book

K.L.B. BK IV
Pages 189-191

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Alkanols (Alcohols).
Nomenclature of alkanols.
Isomerism in alkanols.
Preparation of ethanol in the lab.
Physical properties of alkanols.
Chemical properties of alkanols.
Esters and esterification.
Oxidation of ethanol. Uses of alkanols.

By the end of the lesson, the learner should be able to:
Identify the functional group of alkanols.
Explain formation of alkanol molecules.
Name and draw the structure of simple alkanols.
Describe positional and chain isomerism in alkanols.
Explain formation of primary and secondary alkanols.
Describe preparation of ethanol in the laboratory.
Explain the physical properties of alkanols.
Describe some chemical reactions of alkanols.
Explain formation of esters.
Describe the esterification process.
Explain oxidation of ethanol by an oxidizing agent.
State uses of alkanols.
Explain the effects of alcohol on human health

Q/A: review alkanes, alkenes and alkynes.
Teacher exposes new concepts and links them with already known concepts.
Guided discovery of naming system for alkanols.
Draw and name structures of alkanols.
Q/A: review the terms positional and chain isomerism.
Brief discussion on isomerism.
Oral exercise: naming given organic compounds.
Written exercise: writing structural formulae for isomers of organic compounds of a given molecular formula.
Group experiments / teacher demonstration.
Discuss the fermentation process.
Comparative evaluation of physical properties of alkanols.
Q/A & discussion on variation in physical properties of alkanols.
Group experiments/ teacher demonstration to investigate combustion of ethanol and its reaction with metals.
Write corresponding chemical equations.
Teacher exposes and explains new concepts.
Assignment.
Q/A: review redox reactions, oxidizing and reducing agents.
Brief discussion: oxidation of ethanol using potassium (VII) manganate or potassium (VI) dichromate.
Write corresponding chemical equations.
Open discussion.

student book
Calcium hydroxide solution, sugar solution, yeast.

K.L.B. BK IV
Page 205
K.L.B. BK IV
Page 212

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Alkanoic (Carboxylic Acids).
Nomenclature of alkanoic acids.
Lab preparation of ethanoic acid.

By the end of the lesson, the learner should be able to:
Identify the functional group of alkanoic (carboxylic) acids.
Explain formation of alkanoic acid molecule.
Name and draw the structure of simple alkanoic acids.
Describe laboratory preparation of ethanoic acid.

Q/A: review functional group of alkanols.
Brief discussion.
Guided discovery of the naming system for alkanoic acids.
Teacher demonstration: prepare ethanoic acid in the lab.
Brief discussion on preparation of ethanoic acid.

student book
Chart: homologous series of alkanoic acids.
Concentrated H2SO4, potassium manganate
(VII) Crystals, water bath.

K.L.B. BK IV
Page 219

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Physical properties of alkanoic acids.
Chemical properties of alkanoic acids.
Chemical properties & Uses of alkanoic acids.
Soap preparation in the lab.
Cleaning action of soap.
Effects of hard / soft water on soap.
Soapless detergents.
Polymers and polymerization.

By the end of the lesson, the learner should be able to:
Explain some physical properties of alkanoic acids.
Explain some chemical properties of alkanoic acids.
Write equations for chemical reactions involving acids.
State uses of alkanoic acids.
Describe soap preparation in the lab.
Describe the nature of a soap molecule.
Explain the mode of action in cleaning.
Explain the effects of hard/ soft water on soap.
Prepare soapless detergents in the lab.
State merits of soapless detergents over soaps.
Explain the concepts additional and condensation polymerization as methods of making synthetic polymers.
Identify some products of polymerization.
State merits and demerits of synthetic polymers over natural materials.

Compare physical properties of some alkanoic acids.
Discuss the difference in physical properties among alkanoic acids.
Group experiment: investigate some chemical properties of ethanoic acid.
Carry out tests and record observations in a table.
Review and discuss the observations above.
Write corresponding chemical equations.
Teacher elucidates uses of alkanoic acids.
Group experiments,
Answer questions based on the experiments already carried out.
Expository and descriptive approaches.
Answer oral questions.
Group experiments: form soap lather in different solutions.
Deduce the effects of hard/ soft water on soap.
Teacher demonsration.
Brief discussion.
Teacher exposes and explains new concepts.
Detailed discussion.
Assignment.

student book
Ethanoic acid, universal indicator, sodium carbonate, magnesium strip, ethanol, conc. H2SO4 and sodium hydroxide.
Distilled water, tap water, rainwater, sodium chloride solution.
Calcium nitrate, Zinc Sulphate, etc.

K.L.B. BK IV
Pages 223-4