THE MOLE

Mole, molar mass and R.A.M.

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.

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

Chart- table of molar masses of elements.

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

THE MOLE

Number of moles in a substance.

By the end of the lesson, the learner should be able to:
Calculate number of moles in a given mass of a substance.

Worked examples.
Supervised practice.

student book

K.L.B .BK III
P. 34
Longhorn
BK III
PP 39-40

THE MOLE

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

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.

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.

Calculators.

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

Longhorn Book III PP 44-60

THE MOLE

Empirical Formula.

By the end of the lesson, the learner should be able to:
Determine empirical formula of a compound given percentage composition by mass.

Worked examples.
Supervised practice.

Assignment.

student book

K.L.B.
BK III P. 43

Longhorn Book III PP 66-71

THE MOLE

Molecular formula.
Concentration of a solution.
Molarity of a solution.
Preparation of 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.

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.
Worked examples.
Supervised exercise.
Q/A: - Description of preparation of molar solutions.

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

K.L.B. BK III
PP. 48-49

Longhorn
Book III
PP 76-81

THE MOLE

Calculators on molar solutions.
Dilution of solutions.
Stoichiometry of a chemical reaction.

By the end of the lesson, the learner should be able to:
Solve numerical calculations on molar solutions.
Problems on molar solutions.
Calculate molarity of a solution after dilution.
To determine mole ratio of given reactions.

Worked examples.
Supervised exercise.
Assignment.
Group experiments.
Calculations.
Group experiments: - Determine masses, hence moles of reacting CuSO4 solution and iron metal.

student book
CuSO4 solution and iron metal.

K.L.B. BK III
P 51
Longhorn Book III PP 76-81

THE MOLE

Stoichiometric equations.

By the end of the lesson, the learner should be able to:
To define a stoichiometric equation.

To write stoichiometric equations of the above reactions.

student book

K.L.B. BK III
Longhorn Book III PP 14-16
PP. 88-93

THE MOLE
NITROGEN & ITS COMPOUNDS.

Stoichiometric equations of various reactions.
Isolation of nitrogen from air.

By the end of the lesson, the learner should be able to:
To investigate and determine Stoichiometric equations of various reactions.
Describe isolation of nitrogen from air.

Class experiments.
Problem solving.
Teacher demonstration, explanations and equations.

student book
Aspirator, copper turnings, gas jar, combustion tube, trogh.

K.L.B. BK III
P. 62

NITROGEN & ITS COMPOUNDS.

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 industrial production of nitrogen.
Describe lab preparation of nitrogen.
State physical and chemical properties of nitrogen.


List down uses of nitrogen.

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.

charts
Ammonium chloride, sodium nitrate

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

Longhorn Book
PP 188-9

K.L.B. BK III
P. 138

Longhorn
Book III
PP 191-2

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.

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.

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.

charts
2 cm Solutions containing various metal ions.

K.L.B. BK III
P. 150

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

NITROGEN & ITS COMPOUNDS.

Ionic equations of above reactions.
Burning ammonia in the air.

By the end of the lesson, the learner should be able to:
To write iIonic equations of above reactions.
To describe burning ammonia in the air.

Discuss precipitation of metal hydroxides by aqueous ammonia.
Confirmatory tests for various concentrations.
Teacher demonstration
Discussion
Chemical equations of reactions.

charts
Conc. Ammonium solution
Hot platinum rod
Oxygen.

K.L.B. BK III
P.154

Longhorn BK III
P 223

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

K.L.B. BK III
P. 167

Longhorn
Book III
229-30

NITROGEN & ITS COMPOUNDS.

Dilute nitric acid and metal hydroxides and oxides.

By the end of the lesson, the learner should be able to:
Predict results of reacting dilute nitric acid with metal hydroxides and oxides.

Group experiments & writing equations for the reactions.

Metal hydroxides.

K.L.B. BK III
P. 168

Longhorn
Book III
PP 238-240

NITROGEN & ITS COMPOUNDS.

Reaction of nitric acid as an oxidizing agent.
Uses of nitric acid & nitrates.

By the end of the lesson, the learner should be able to:
Describe reactions of nitric acid as an oxidizing agent.
To state uses of nitrates.
To describe preparation of nitrates.

Class experiments: -
Explain observations made.
Discussion
Equations for the reactions for preparation of nitrates.

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

K.L.B. BK III
PP. 169-170

Longhorn Book III
PP 239 -240

NITROGEN & ITS COMPOUNDS.

Action of heat on nitrates.
Test for nitrates.

By the end of the lesson, the learner should be able to:
To write equations of decomposition of nitrates on heating.
To carry out tests on nitrates.

Discuss above observations.
Write relevant equations.
Class experiments.
Make observations and deductions.
Discuss the brown ring test for nitrates.

charts

K.L.B. BK III
P 172

NITROGEN & ITS COMPOUNDS.
SULPHUR AND ITS COMPOUNDS

Nitrogen compounds and the environment.
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 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.
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.

Brief guided discussion.
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.

charts
Chart-the Frasch process.
video
charts

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

Longhorn
Book III
PP 244-6

K.L.B. BK III
PP. 182-183
Longhorn Book
PP 126-129

SULPHUR AND ITS COMPOUNDS

Chemical properties of sulphur.

By the end of the lesson, the learner should be able to:
To investigate and describe chemical properties of sulphur.

Group experiments.
Discuss observations.
Write corresponding equations.

charts

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

SULPHUR AND ITS COMPOUNDS

Uses of sulphur. Sulphur dioxide.
Physical properties of sulphur dioxide.

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.

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.

charts
text book

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

SULPHUR AND ITS COMPOUNDS

Acidic properties of SO2.

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

Teacher demonstration to verify acidic properties of sulphur dioxide.
Write equations.

textbook

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

SULPHUR AND ITS COMPOUNDS

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:
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.

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.

Experimental worksheets.
Burning magnesium.
Hydrogen sulphide.
Sodium sulphate
Barium chloride
Barium nitrate.

K.L.B.BK III
P. 195
K.L.B.
BK III P. 200
Longhorn
Book III
PP 268-9

SULPHUR AND ITS COMPOUNDS

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

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

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

Chart-schematic
Flow charts.
charts

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

SULPHUR AND ITS COMPOUNDS

Physical properties of sulphuric acid.

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

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

Conc. sulphuric acid.

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

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
SULPHUR AND ITS COMPOUNDS
ACIDS, BASES AND SALTS.

Dilute H2SO4, and metal oxides and hydroxides.
Dilute H2SO4 and metal oxides & hydroxides.
Strength of acids. Acids in aqueous form.

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

Class expts.
Observing colour changes.
Discussion, writing relevant chemical equations.
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.

Oxides of magnesium, zinc, copper.
NaOH Solution.
charts
Magnesium strip, zinc carbonate,
2M HCl,
2M H2SO4,
2M ethanoic acid.

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


K.L.B.
BK III P. 211

ACIDS, BASES AND SALTS.

pH values of acids. Electrical conductivities of aqueous acids.

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.

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.

Universal
indicator,
2M HCl,
2M ethanoic acid,
dry cells,
carbon electrodes,
milli-ammeters,
wires, switches etc.

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

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.

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.

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.

2M NaOH,
2M ammonia solution, universal indicator solutions, dry cells,
carbon electrodes,
milliammeters,
wires, switches etc

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

ACIDS, BASES AND SALTS.

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:
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.

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.

Ammonia gas,
Methylbenzene, hydrogen chloride gas.
Methylbenzene.
2M Nitric acid
2M NaOH,
HNO3.
Amphoteric oxides.

K.L.B. BK IV
Pages 9-11
K.L.B. BK IV
Pages 12-14

ACIDS, BASES AND SALTS.

Precipitation Reactions.
Solubility of chlorides sulphites and sulphates.

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

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

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

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

ACIDS, BASES AND SALTS.

Equations for formation of insoluble chlorides, sulphites and sulphates.

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

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

student book

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

ACIDS, BASES AND SALTS.

Complex ions.

By the end of the lesson, the learner should be able to:
Explain formation of complex ions.

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

Make observations and discuss the results.

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

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

ACIDS, BASES AND SALTS.

Solubility of a salt at a given temperature.
Problems solving on solubility.
Effect of temperature on solubility of a solute in a solvent.
Effects of various salts on soap.
Removal of hardness of water.

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

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.
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.

Suitable solutes.
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+.
student book

K.L.B. BK IV
Pages 20-21
K.L.B. BK IV
Pages 22-25