GAS LAWS

Boyle?s law.
Boyle?s law: - Equation and graphical representation.

By the end of the lesson, the learner should be able to:
State Boyle?s law.
Explain Boyle?s law using kinetic theory of matter.
Represent Boyle?s law mathematically and graphically.

Teacher demonstration ? Use syringes / pumps to show variation of volume with pressure.
Teacher asks probing questions leading to statement of the law.
Discuss the cause of build-up-in pressure.
Q/A: relation between volume and pressure mathematically and graphically.
Derive the relation P1V1=P2V2, and sketch graphs to illustrate Boyle?s law.
Worked examples.
Assignment.

Chart
Volume-pressure relationship.
Syringes.
chart

K.L.B. BK III
PP. 1-2

Longhorn Book III
PP 1 -2

GAS LAWS

Boyle?s law: Numerical questions.
Boyle?s law: Interpretation of graphs.
Charles? law.

By the end of the lesson, the learner should be able to:
Solve further problems involving Boyle?s law.
Plot and intepret graphs involving pressure and volume of gases.
State Charles? law.
Explain Charles? law using kinetic theory of matter.

Supervised exercise: Volume in cm?, m?, litres, and pressure in Pa, mmHg, cmHg, atmospheres.
Assignment.
Completing tables and plotting graphs.
Interpret the plotted graphs.
Make deductions from the graphs.
Teacher demonstration:- To show expansion of air when heated and contraction when pressure is constant.
Explain increase in volume when temperature is raised.
Q/A: - relation between volume and temperature, leading to Charles? law.

Calculators.
Graph papers.
Coloured water,
Glass tube,
Warm water,
Cork and
Flask.

K.L.B. BK III
PP. 4-5
Longhorn Book III PP 6-8

GAS LAWS

Temperature in Degree Celsius and Kelvin. Equation and graphs from Charles? law.
Charles? law- equation and graphical representation.
Numerical questions on Charles? Law.

By the end of the lesson, the learner should be able to:
Convert temperature in degree Celsius to Kelvin and vice-versa.
Express Charles? law with equations.
Give a graphical representation of Charles? law.
Solve numerical problems based on Charles? Law.

Teacher explains inter-conversion of the units.
Students complete a table of temperature in the two units.
Derive equations from volume and temperature relationship.
Exposition: - Teacher exposes a volume-temperature graph and extrapolates it to obtain the absolute temperature. The definition of absolute temperature is exposed.
Worked examples.
Supervised exercise.
Assignment.

student book
Calculators.

K.L.B.
BK III P. 10

Longhorn Book III P 11

GAS LAWS
GAS LAWS
THE MOLE
THE MOLE

Combined Gas Law.
Standard conditions, S.T.P. conditions and R.T.P. conditions.
Diffusion.
Rates of diffusion.
Graham?s Law.
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:
Derive the Gas Law.
Derive the combined gas law equation.
Solve numerical problems using the equation.
State standard conditions of temperature and pressure of an ideal gas.
State room temperature and pressure of a gas.
Use standard conditions in problem solving.
Define diffusion.
Describe experiments to show diffusion.
Compare rates of diffusion of ammonia gas and hydrogen chloride in air.
Carry out numerical tasks.
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.

Q/A: - Combining Boyle?s and Charles? Laws.
Worked examples.
Exposition of s.t.p. and r.t.p.
Problem solving.
Group experiments.
Diffusion of KMnO4 crystals, concentrated ammonia solution.
Teacher demonstration: - To deduce rate of diffusion of ammonia gas and hydrogen chloride.
Q/A: - Students calculate ratio of rates of diffusion of the gases.
Solve problems involving RMM, equal volumes of the gases involved.
Supervised practice.
Assignment.
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.

Calculators.
student book
KMnO4 crystals,
Litmus papers.
Calculators
Chart- table of molar masses of elements.
student book

K.L.B.
BK III P. 12

Longhorn Book III PP 14-16

K.L.B. BK III
PP. 24-26

Longhorn Book III PP 22-24

THE MOLE

Relative molecular mass & Relative formula mass.
Moles and Avogadro?s number.
Empirical Formula.

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.

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.

Calculators.
student book

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

Longhorn Book III PP 44-60

THE MOLE

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 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.

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

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.

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.

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

student book
CuSO4 solution and iron metal.

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

THE MOLE
Volumetric Analysis.
Volumetric Analysis.

Stoichiometric equations of various reactions.
Apparatus used in titration experiments.
Titration process.
Titration experiment (Neutralization reaction)
Titration experiment (Neutralization reaction)
Basicity of an acid.
Standardization of HCl.

By the end of the lesson, the learner should be able to:
To investigate and determine Stoichiometric equations of various reactions.
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.
To define basicity of an acid.
To define standardization of HCl.

Class experiments.
Problem solving.
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.
Complete a table of number of replaceable hydrogen ions of an acid; hence define basicity of an acid.
Write corresponding ionic equations.
Class experiments.

student book
Pipettes
Burettes.
Indicators
Suitable acid and base.
student book
Calculators.
Dilute HCl, Na2CO3 solutions.

K.L.B. BK III
P. 62
K.L.B. BK III
P. 66

Longhorn Book III PP 108-114

Volumetric Analysis.

Concentration of HCl.
Redox Titration Reactions.
Water of crystallization.

By the end of the lesson, the learner should be able to:
To calculate concentration of HCl from experimental results.
To standardize a solution with an iron (II) salt.
To determine amount of water of crystallization in ammonium iron sulphate crystals.

Calculations & supervised practice.
Experiment and calculations.
Teacher exposes the formula of water of crystallization.
Class experiment.
Filling in a table of results.

Potassium Magnate
(VII)
Ammonium
Iron (II)
Sulphate crystals.
Dilute sulphuric (VI) acid.

K.L.B. BK III
PP. 74-75

Volumetric Analysis.

Formula mass of ammonium iron (II) sulphate.
Formula mass of a given salt.
Atomicity of gases.
Mass and volume of gases.

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

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.

student book
Lubricated syringes
Oxygen/
CO2.

K.L.B. BK III
PP. 76 -77

Volumetric Analysis.

Molar gas volume.
Combining volumes of gases.
Gay Lussac?s Law.

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

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.

student book

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

ORGANIC CHEMISTRY (I)

Hydrocarbons.
Alkanes.
Naming Alkanes.
Members of Alkane series.
Isomerism in alkanes.
Laboratory preparation of a given alkane.
Trend in physical properties of alkanes.
Chemical properties of alkanes.
Substitution reactions involving alkanes. Uses of alkanes.

By the end of the lesson, the learner should be able to:
To define organic Chemistry.
To define a hydrocarbon.
To identify groups of hydrocarbons.
To describe the carbon atom.
To identify various alkanes.
To list sources of alkanes.
To state uses of different fractions of crude oil.
To define cracking of alkanes.
To define a homologous series.
To name members of alkane series and identify their characteristics.
To draw the structures of alkane series.
To draw and name isomers of simple hydrocarbons.
To describe laboratory preparation of a given alkane.
To state physical properties of the gases prepared.
To describe the trend in physical properties of alkanes.
Describe chemical properties of alkanes.
To describe substitution reactions involving alkanes.
To list down uses of alkanes.

Discuss composition of the carbon atom; hence deduce number of valence electrons.
Exposition of new terms.
Expose various alkanes.
Discuss the biomass digester, fractional distillation of crude oil and uses of the fractions.
Discuss the cracking process.
Discussion and exposition of new concepts.
Teacher demonstration.
Discussion.
Study a table of comparative properties of alkanes.
Make deductions from the table.
Discussion
Examples of balanced equations.
Discussion
Teacher elucidates uses of alkanes.

student book
Chart of biomass digester.
Chart- structure of alkanes.
Models.
Sodium ethanoate, sodalime,
Pestle and mortar.
student book

K.L.B. BK III
P. 92
Longhorn
Book III
P 135

K.L.B. BK III
P. 103

Longhorn
Book III
PP 146

ORGANIC CHEMISTRY (I)

Alkenes. Molecular formulae of alkenes.
Naming alkenes.
Alkene isomerism.
Preparing ethene in the lab.

By the end of the lesson, the learner should be able to:
To write molecular formulae of alkenes.
To name various alkenes.
Differentiate between branching and positional isomerism.
To describe lab preparation of ethene.

Examine table of members of alkenes.
To identify members of alkene series.
Q/Q: Nomenclature in alkenes.
Compare alkenes; hence deduce names of various alkenes.
Discussion and drawing of molecular structures.
Teacher demonstration: - Carry out tests on ethene as students note down the observations in a table.

student book
chart

K.L.B. BK III
PP 153-4

ORGANIC CHEMISTRY (I)

Physical properties of ethene.
Chemical properties of ethene.
Alkenes and oxidizing agents.
Uses of alkenes & Topic review.

By the end of the lesson, the learner should be able to:
To describe physical properties of ethene and other alkenes.
To explain halogenation and hydrogenation reactions.
To describe reactions of alkenes with oxidizing agents.
To list down uses of alkenes.

To discuss physical properties of ethene and other alkenes.
Discussion and drawing structures.
Review the double bonds in alkenes.
Review reduction process, oxidizing agent.
Discuss reactions of alkenes with conc. H2SO4, acidified potassium chromate.
Expose hydrolysis process.
Teacher elucidates uses of alkenes.
Assignment.

student book
charts

K.L.B. BK III
PP. 116-117
Longhorn Book III
PP 126-129
165-6

ORGANIC CHEMISTRY (I)

Alkynes. Nomenclature.
Isomerism in alkynes.
Physical properties of ethyne.

By the end of the lesson, the learner should be able to:
To identify various alkynes.
To name and draw structures of alkynes.
To draw structure showing positional and branching isomerism.
To list down physical properties of ethyne.

Discuss a table of members of alkynes.
Review naming of alkanes and alkene and compare this with naming of alkynes.
Discussion and drawing structures.
Teacher demonstration: Preparation of ethyne.
Deduce properties of other alkynes.

charts

K.L.B. BK III
P. 122-123
Longhorn
Book III
PP 126-129 171-5

ORGANIC CHEMISTRY (I)
NITROGEN & ITS COMPOUNDS.
NITROGEN & ITS COMPOUNDS.

Chemical properties of ethyne.
Tests for alkynes. Uses of alkynes.
Isolation of nitrogen from air.
Industrial production of nitrogen.
Lab. preparation of nitrogen.
Physical and chemical properties of nitrogen. Uses of nitrogen.
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 combustion, halogenation and hydrogenation processes.
To describe tests for alkynes and state uses of alkynes.
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.
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.

Discussion and writing of equations.
Discussion and explanations.
Assignment.
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.
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.

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

K.L.B. BK III
PP. 127-129
Longhorn Book III
PP 180-184

K.L.B. BK III
P. 137

Longhorn
Book III
P 190-1

NITROGEN & ITS COMPOUNDS.

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 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.

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.
Deduce physical properties from the table of observations.
To describe chemical properties from the table of observations.
Discuss uses of nitrogen (1V) oxide.

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.

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.

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.

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.

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.

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

NITROGEN & ITS COMPOUNDS.

Haber process.
Uses of ammonia.
Nitric acid. Lab preparation.
Nitric acid Industrial manufacture.
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:
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.
To describe action of nitric acid on carbonates and hydrogen carbonates.
Write equations for reaction of dil. nitric acid with hydrogen carbonates.

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.
Group experiments: - Action of Nitric acid on hydrogen carbonates.
Discussion and corresponding equations.

Chart- schematic diagram.
charts
Retort stand
Conc. H2SO4
KNO3
Chart
Schematic diagram.
Magnesium
Zinc
Copper
Solutions of
Na2CO3
NaHCO3
ZnCO3
CuCO3

K.L.B. BK III
PP. 159-160
225-226
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

NITROGEN & ITS COMPOUNDS.
SULPHUR AND ITS COMPOUNDS

Test for nitrates.
Nitrogen compounds and the environment.
Extraction of sulphur.

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.
To describe extraction of sulphur by Frasch process.

Class experiments.
Make observations and deductions.
Discuss the brown ring test for nitrates.
Brief guided discussion.
Illustrate and discuss extraction of sulphur.

charts
Chart-the Frasch process.

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

Longhorn
Book III
PP 243

SULPHUR AND ITS COMPOUNDS

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 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.

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.

video
charts

K.L.B. BK III
PP. 182-183
Longhorn Book
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.

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.

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.

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

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

K.L.B.BK III
P. 195

SULPHUR AND ITS COMPOUNDS

Sulphuric acid. Contact process of manufacture.
Properties of conc. H2SO4.
Physical properties of sulphuric acid.
Chemical properties of Sulphuric acid.
Dilute H2SO4, carbonates and hydrogen carbonates.
Dilute H2SO4, and metal oxides and hydroxides.

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.
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.
To investigate reaction of dilute H2SO4 with metal oxides and hydroxides.

Discussion using schematic
flow charts.
Writing equations.
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.
Class expts.
Observing colour changes.

Chart-schematic
Flow charts.
charts
Conc. sulphuric acid.
Magnesium, zinc, copper metals.
charts
Oxides of magnesium, zinc, copper.
NaOH Solution.

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

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

SULPHUR AND ITS COMPOUNDS

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

Discussion, writing relevant chemical equations.
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. 211

SULPHUR AND ITS COMPOUNDS
CHLORINE & 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.

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

CHLORINE & ITS COMPOUNDS

Chemical properties of chlorine ? reaction with water.
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 water.
To investigate and explain reaction of chlorine with metals / non-metals.

Teacher demonstration:
Writing chemical equations.
Discussion.

Moist blue litmus papers.
textbook

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

CHLORINE & ITS COMPOUNDS

- Oxidizing properties of chlorine.
Chlorine and alkalis.
Test for chlorides.
Uses of chlorine gas.
Hydrogen chloride gas. Lab. prep. Physical properties.
Aqueous hydrogen chloride.

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.
To carry out tests for chlorides.
To state uses of chlorine.
To describe Lab. prep of hydrogen chloride gas.
To investigate and state physical properties of hydrogen chloride gas.
To prepare aqueous hydrogen chloride.

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.
Class expts.
Discuss observations, results.
Write chemical equations for the reactions.
Teacher elucidates uses of chlorine.
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.

Expt. Worksheets.
Cold / hot NaOH solutions.
Zinc chloride, litmus paper, conc. Sulphuric acid.
Sodium chloride crystals, conc H2SO4
Distilled water.

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

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

CHLORINE & ITS COMPOUNDS

Further chemical properties of hydrogen chloride gas.
Large-scale production of hydrochloric acid.
Uses of hydrochloric acid.

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.
Identify raw materials for manufacture of hydrochloric acid in large scale.
Describe the manufacturing process.
To state uses of hydrochloric acid.

Class experiment leading to deduction of further chemical properties of hydrogen chloride gas / confirmatory test for hydrogen chloride gas.
Discussion and giving relevant equations.
Brief discussion.

Ammonia solution.
charts

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

CHLORINE & ITS COMPOUNDS
ACIDS, BASES AND SALTS.
ACIDS, BASES AND SALTS.

Effects of hydrochloric acid on the environment.
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:
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.
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.

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.
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.

charts
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 III
P 238.
Longhorn Book III
PP 334-8

ACIDS, BASES AND SALTS.

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

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.
Compare strengths of bases using pH values and electrical conductivity.
Classify bases/ alkali as either strong or weak in terms of complete / partial ionization.

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.

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

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

ACIDS, BASES AND SALTS.

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

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.
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.

Ammonia gas,
Methylbenzene, hydrogen chloride gas.
Methylbenzene.
2M Nitric acid
2M NaOH,
HNO3.
Amphoteric oxides.
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 9-11
K.L.B. BK IV
Pages 14-16

ACIDS, BASES AND SALTS.

Complex ions.
Solubility of a salt at a given temperature.

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.

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.

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

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

ACIDS, BASES AND SALTS.

Problems solving on solubility.
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:
Solve problems involving solubility of a solute in a solvent at a given temperature.
Investigate the effect of temperature on solubility of a solute in a solvent.
Determine the effects of various salts on soap.

Worked examples.
Supervised practice.
Written assignment.
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.

Evaporating dish, watch glass, heating source, thermometer.
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 21-22

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

Removal of hardness of water.
Endothermic and Exothermic Reactions.
Energy level diagrams.
Enthalpy Notation. Change of state.

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.
Define the term enthalpy.
Distinguish positive enthalpy change from negative enthalpy change.
Determine the M.P/ B.P of a pure substance.

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.
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.

student book
Ammonium nitrate,
Sodium hydroxide, thermometers.
Ice, naphthalene, thermometers, graph papers.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

CAT
Molar heat of solution.
Molar heat of solution of H2SO4.
Enthalpy of combustion. Enthalpy of combustion.

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.
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.

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

Ammonia nitrate / sodium hydroxide, thermometers.
Conc. H2SO4, thermometers.
Ethanol, distilled water, thermometer, clear wick, tripod stand and wire gauze.

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

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Hess?s Law.
Heat of solution hydration energy and lattice energy.

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

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

student book

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
RATES OF REACTION & REVERSIBLE REACTIONS.
RATES OF REACTION & REVERSIBLE REACTIONS.
RATES OF REACTION & REVERSIBLE REACTIONS.
RATES OF REACTION & REVERSIBLE REACTIONS.

Heat values of fuels.
Environmental effects of fuels.
Effect of concentration on rate of a reaction
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:
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.
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.

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.
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.

student book
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.
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 64-66