SULPHUR AND ITS COMPOUNDS

Extraction of sulphur.

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

To describe extraction of sulphur by Frasch process.

Illustrate and discuss extraction of sulphur.

Chart-the Frasch process.

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

SULPHUR AND ITS COMPOUNDS

Allotropes of sulphur.
Physical properties of sulphur. Heating 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.

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.

video
charts

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

SULPHUR AND ITS COMPOUNDS

Chemical properties of sulphur.
Uses of sulphur. Sulphur dioxide.
Physical properties of sulphur dioxide.
Acidic properties of SO2.

By the end of the lesson, the learner should be able to:
To investigate and describe chemical properties of sulphur.
State uses of sulphur.
Describe lab. preparation of sulphur dioxide.
To list down physical properties of sulphur dioxide.
To carry out experiments to determine acidic properties of SO2.

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

charts
text book
textbook

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

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

SULPHUR AND ITS COMPOUNDS

Reducing action of SO2.
Bleaching properties 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.

Class experiments: make observations and draw conclusions.
Write balanced corresponding equations.
Discuss the observations made above.
Write corresponding equations.

Experimental worksheets.

K.L.B.BK III
P. 195

SULPHUR AND ITS COMPOUNDS

Oxidizing action of SO2.
Sulphate and sulphite ions. Uses of SO2.

By the end of the lesson, the learner should be able to:
To explain Oxidizing action of SO2.
To carry out tests for Sulphate and sulphite ions.
State uses of SO2.

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.

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

K.L.B.
BK III
PP. 198-199
Longhorn
Book III
PP 266-7

SULPHUR AND ITS COMPOUNDS

Sulphuric acid. Contact process of manufacture.
Properties of conc. H2SO4.
Physical properties of sulphuric acid.

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.

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.

Chart-schematic
Flow charts.
charts
Conc. sulphuric acid.

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

SULPHUR AND ITS COMPOUNDS

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 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 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.

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

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


K.L.B.
BK III P. 208

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

Reaction of the gas with water. Reducing properties of the gas.

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.

Writing chemical equations for the reactions.

charts

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

SULPHUR AND ITS COMPOUNDS
CHLORINE & ITS COMPOUNDS
CHLORINE & ITS COMPOUNDS

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 explain environmental pollution caused by sulphur and its compounds.
Describe laboratory preparation of chlorine gas.
State physical properties of chlorine.

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. 214
Longhorn Book
PP 293-5

CHLORINE & ITS COMPOUNDS

Chemical properties of chlorine ? reaction with water.
Chemical properties of chlorine - Reaction with metals - Reaction with non-metals.
- Oxidizing properties of chlorine.

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.
To investigate and explain reaction of chlorine with reducing a gents.

Teacher demonstration:
Writing chemical equations.
Discussion.
Group experiments.
Discuss and explain observations made.
Write corresponding chemical equations.

Moist blue litmus papers.
textbook
Expt. Worksheets.

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

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

CHLORINE & ITS COMPOUNDS

Chlorine and alkalis.
Test for chlorides.

By the end of the lesson, the learner should be able to:
To investigate and explain reaction of chlorine with alkalis.
To carry out tests for chlorides.

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.

Cold / hot NaOH solutions.
Expt. Worksheets.
Zinc chloride, litmus paper, conc. Sulphuric acid.

K.L.B.BK III
P. 228
Longhorn Book III
PP 313-4

CHLORINE & ITS COMPOUNDS

Uses of chlorine gas.
Hydrogen chloride gas. Lab. prep. Physical properties.

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

Teacher elucidates uses of chlorine.
Teacher demonstration.
Carry out tests on the gas and deduce the properties of the gas.

Sodium chloride crystals, conc H2SO4

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

CHLORINE & ITS COMPOUNDS

Aqueous hydrogen chloride.

By the end of the lesson, the learner should be able to:
To prepare aqueous hydrogen chloride.

Class experiment leading to deduction of chemical properties of hydrogen chloride gas.

Distilled water.

K.L.B.BK III
P. 234

CHLORINE & ITS COMPOUNDS
CHLORINE & ITS COMPOUNDS
ORGANIC CHEMISTRY (I)
ORGANIC CHEMISTRY (I)

Further chemical properties of hydrogen chloride gas.
Large-scale production of hydrochloric acid.
Uses of hydrochloric acid.
Effects of hydrochloric acid on the environment.
Hydrocarbons.
Alkanes.

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.
To explain effects of hydrochloric acid on the environment.
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.

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.
Discussion and explanation.
Assignment.
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.

Ammonia solution.
charts
charts
student book
Chart of biomass digester.

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

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

ORGANIC CHEMISTRY (I)

Naming Alkanes.
Members of Alkane series.

By the end of the lesson, the learner should be able to:
To identify various alkanes.
To define a homologous series.
To name members of alkane series and identify their characteristics.
To draw the structures of alkane series.

Discussion and exposition of new concepts.

student book
Chart- structure of alkanes.

K.L.B. BK III
PP. 94-98
Longhorn
Book III
PP 136-139

ORGANIC CHEMISTRY (I)

Isomerism in alkanes.
Laboratory preparation of a given alkane.
Trend in physical properties of alkanes.

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

Discussion and exposition of new concepts.
Teacher demonstration.
Discussion.
Study a table of comparative properties of alkanes.
Make deductions from the table.

Models.
Sodium ethanoate, sodalime,
Pestle and mortar.
student book

K.L.B. BK III
PP. 101-102 Longhorn Book III
PP 141-2

ORGANIC CHEMISTRY (I)

Chemical properties of alkanes.
Substitution reactions involving alkanes. Uses of alkanes.
Alkenes. Molecular formulae of alkenes.

By the end of the lesson, the learner should be able to:
Describe chemical properties of alkanes.
To describe substitution reactions involving alkanes.
To list down uses of alkanes.
To write molecular formulae of alkenes.

Discussion
Examples of balanced equations.
Discussion
Teacher elucidates uses of alkanes.
Examine table of members of alkenes.
To identify members of alkene series.

student book

K.L.B. BK III
P. 107
Longhorn
Book III
PP 148-9

ORGANIC CHEMISTRY (I)

Naming alkenes.
Alkene isomerism.
Preparing ethene in the lab.
Physical properties of ethene.
Chemical properties of ethene.

By the end of the lesson, the learner should be able to:
To name various alkenes.
Differentiate between branching and positional isomerism.
To describe lab preparation of ethene.
To describe physical properties of ethene and other alkenes.
To explain halogenation and hydrogenation reactions.

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.
To discuss physical properties of ethene and other alkenes.
Discussion and drawing structures.

student book
chart
student book
charts

K.L.B. BK III
PP. 110-113
Longhorn
Book III
PP 154-6


K.L.B. BK III
P 162

ORGANIC CHEMISTRY (I)

Alkenes and oxidizing agents.
Uses of alkenes & Topic review.

By the end of the lesson, the learner should be able to:
To describe reactions of alkenes with oxidizing agents.
To list down uses of alkenes.

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.

charts

K.L.B. BK III
PP. 120-121


Longhorn
Book III
PP 166-8

ORGANIC CHEMISTRY (I)

Alkynes. Nomenclature.
Isomerism in alkynes.

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.

Discuss a table of members of alkynes.
Review naming of alkanes and alkene and compare this with naming of alkynes.
Discussion and drawing structures.

charts

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

ORGANIC CHEMISTRY (I)

Physical properties of ethyne.
Chemical properties of ethyne.
Tests for alkynes. Uses of alkynes.

By the end of the lesson, the learner should be able to:
To list down physical properties of ethyne.
To describe combustion, halogenation and hydrogenation processes.
To describe tests for alkynes and state uses of alkynes.

Teacher demonstration: Preparation of ethyne.
Deduce properties of other alkynes.
Discussion and writing of equations.
Discussion and explanations.
Assignment.

charts

K.L.B. BK III
PP. 125-126
Longhorn
Book III
PP 197-80

ACIDS, BASES AND SALTS.

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

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


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.
Define a base in terms of hydroxide ions.

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.
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.

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

K.L.B. BK IV
Pages 1-4
K.L.B. BK IV
Pages 4-6

ACIDS, BASES AND SALTS.

Neutralization reaction.
Strength of bases.

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

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.

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
Page 7

ACIDS, BASES AND SALTS.

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

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.

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.

Ammonia gas,
Methylbenzene, hydrogen chloride gas.
Methylbenzene.

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

ACIDS, BASES AND SALTS.

Amphoteric oxides.

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

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

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

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

ACIDS, BASES AND SALTS.

Precipitation Reactions.
Solubility of chlorides sulphites and sulphates.
Equations for formation of insoluble chlorides, sulphites and sulphates.
Complex ions.

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.
Explain formation of complex ions.

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

Make observations and discuss 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.
student book
2M Sodium hydroxide (2M ammonia solution),
solution containing Mg2+, Zn2+, etc.

K.L.B. BK IV
Pages 14-16
K.L.B. BK IV
Pages 18-20

ACIDS, BASES AND SALTS.

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

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.

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.

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

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

ACIDS, BASES AND SALTS.

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

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

Experiments involving solubility of KClO3 at different temperatures.
Note temperatures at which crystallization occurs.
Oral questions and discussion.
Group experiments: form soap lather in distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+.
Note volume of soap that forms lather readily.

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

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

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

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

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

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

student book
Ammonium nitrate,
Sodium hydroxide, thermometers.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy Notation. Change of state.
CAT
Molar heat of solution.

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

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

Determine molar heat of solution of given substances.

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.


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

Ice, naphthalene, thermometers, graph papers.
Ammonia nitrate / sodium hydroxide, thermometers.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of solution of H2SO4.

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

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

Conc. H2SO4, thermometers.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy of combustion. Enthalpy of combustion.

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

Group experiments / teacher demonstration.

Obtain and record results.


Work out calculations.

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

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of displacement of ions.
Molar heat of solution of neutralization.

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.

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.

Zinc, iron, magnesium, copper sulphate solution.
2M HCl of known volume, 1M / 2M sodium hydroxide.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

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

By the end of the lesson, the learner should be able to:
Define the term standard enthalpy change.
Denote standard enthalpy change with the correct notation.
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.

Exposition & brief discussion.
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.
Worked examples.
Assignment.

student book

K.L.B. BK IV
Pages 54-56
K.L.B. BK IV
Pages 60-64

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
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.

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

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.

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.

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