SULPHUR AND ITS COMPOUNDS

Extraction of sulphur.
Allotropes 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.
video

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

SULPHUR AND ITS COMPOUNDS

Physical properties of sulphur. Heating of sulphur.
Chemical properties of sulphur.

By the end of the lesson, the learner should be able to:
To list physical properties of sulphur.

To describe effects of heat on sulphur.
To investigate and describe chemical properties of sulphur.

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.

charts

K.L.B. BK III
P.184
Longhorn I
Book III
PP 253-255

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

SULPHUR AND ITS COMPOUNDS

Uses of sulphur. Sulphur dioxide.

By the end of the lesson, the learner should be able to:
State uses of sulphur.
Describe lab. preparation 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.

charts

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

SULPHUR AND ITS COMPOUNDS

Physical properties of sulphur dioxide.

By the end of the lesson, the learner should be able to:
To list down physical properties of sulphur dioxide.

Discuss the above tests.

text book

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

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.

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

SULPHUR AND ITS COMPOUNDS

Oxidizing action of SO2.

By the end of the lesson, the learner should be able to:
To explain Oxidizing action 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.

Burning magnesium.
Hydrogen sulphide.

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

SULPHUR AND ITS COMPOUNDS

Sulphate and sulphite ions. Uses of SO2.

By the end of the lesson, the learner should be able to:
To carry out tests for Sulphate and sulphite ions.

State uses of SO2.

Class experiments.
Make deductions from the observations made.
Write (ionic) equations for the reactions.
Teacher elucidates uses of SO2.

Sodium sulphate
Barium chloride
Barium nitrate.

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

SULPHUR AND ITS COMPOUNDS

Sulphuric acid. Contact process of manufacture.

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.

Discussion using schematic
flow charts.
Writing equations.

Chart-schematic
Flow charts.

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

SULPHUR AND ITS COMPOUNDS

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

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

Discuss above observations.
Write relevant equations.

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

charts
Conc. sulphuric acid.

K.L.B.
BK III
P. 204
K.L.B.
BK III P. 205
Longhorn
Book III
PP 274-5

SULPHUR AND ITS COMPOUNDS

Chemical properties of Sulphuric acid.

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.

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

Magnesium, zinc, copper metals.

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

SULPHUR AND ITS COMPOUNDS

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 describe reaction of dilute H2SO4 with carbonates and hydrogen carbonates.

Discussion, writing relevant equations.

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

K.L.B.
BK III P. 208

SULPHUR AND ITS COMPOUNDS

Dilute H2SO4 and metal oxides & hydroxides.

By the end of the lesson, the learner should be able to:
To explain reactions of dilute H2SO4 with metal oxides and hydroxides.

Discussion, writing relevant chemical equations.

charts

K.L.B.
BK III P. 211

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

SULPHUR AND ITS COMPOUNDS

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

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

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

Sulphur and its effects on the environment.

By the end of the lesson, the learner should be able to:
To explain environmental pollution caused by sulphur and its compounds.

Discussion and explanation.

charts

K.L.B.
BK III P. 214
Longhorn Book
PP 293-5

ACIDS, BASES AND SALTS.

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

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


Define an acid in terms of hydrogen ions.

Explain strength of acids in aqueous form in terms of number of hydrogen ions present.
Determine strength of acids using pH values.

Determine strengths of acids by comparing their electrical conductivities.

Classify acids as either strong or weak in terms of partial dissociations in aqueous solutions.

Class experiments: investigate reactions of magnesium and zinc carbonate with different acids.
Make and record observations in tabular form.
Make deductions from the observations.
Write relevant chemical equations and ionic equations.
Detailed discussion leading to the definition of an acid and explanation of strength of an acid.

Q/A: review determination of strength of acids using a litmus paper and pH scale.
Class / group experiments: record colour of universal indicator in
2M HCl and 2M ethanoic acid.
Set up voltameters of 2M HCl and 2M ethanoic acid in turns.
Record amounts of current .
Discuss the observations.
Write corresponding ionic equations.

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

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

ACIDS, BASES AND SALTS.

Definition of a base in terms of hydroxide ions.

By the end of the lesson, the learner should be able to:
Define a base in terms of hydroxide ions.

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.

Red litmus paper, calcium hydroxide solid.

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

ACIDS, BASES AND SALTS.

Neutralization reaction.

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

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.

1M HCl,
Calcium hydroxide,
universal indicator.

K.L.B. BK IV
Page 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.

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.
Write down related balanced chemical equations.

Ammonia gas,
Methylbenzene, hydrogen chloride gas.
Ammonia gas,
Methylbenzene.

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

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.

By the end of the lesson, the learner should be able to:
Define a precipitate.
Write ionic equations showing formation of precipitates.

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.

Soluble carbonates e.g. Na2CO3, K2CO3, (NH4)2CO3
Salt solutions containing Mg2+, Al3+, Ca2+, etc.

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

ACIDS, BASES AND SALTS.

Solubility of chlorides sulphites and sulphates.

By the end of the lesson, the learner should be able to:
Find out cations that form (in)soluble chlorides, sulphates and sulphites.

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.

0.1M solution containing Pb2+, 2M NaCl solution, 2M sodium sulphate, source of heating.

K.L.B. BK IV
Pages 16-17

ACIDS, BASES AND SALTS.

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

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

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.

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

K.L.B. BK IV
Pages 17-18
K.L.B. BK IV
Pages 18-20

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.

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.

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.

Suitable solutes.

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

ACIDS, BASES AND SALTS.

Problems solving on solubility.

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.

Worked examples.
Supervised practice.
Written assignment.

Evaporating dish, watch glass, heating source, thermometer.

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

ACIDS, BASES AND SALTS.

Effect of temperature on solubility of a solute in a solvent.

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.

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

KClO3 thermometers, source of heat.

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

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
K.L.B. BK IV
Pages 25-27

ACIDS, BASES AND SALTS.

Removal of hardness of water.

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.

Review results of above experiments.

Probing questions & brief discussion.

Assignment.

student book

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Endothermic and Exothermic Reactions.
Energy level diagrams.

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






To differentiate between endothermic & exothermic reactions.

Investigate temperature changes in solution formation.

Obtain changes in temperature when ammonium nitrate and sodium hydroxide are dissolved in water, one at a time.

Ammonium nitrate,
Sodium hydroxide, thermometers.
student book

K.L.B. BK IV
Pages 32-33

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy Notation. Change of state.

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

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

Q/A and brief discussion.
Class experiments: determine B.P of pure water/ M.P of naphthalene / ice.
Use experimental results to plot temperature-time graphs.
Explain the shape of the graphs.
Q/A: review kinetic theory of matter.
Apply the theory to explain the shape of the graph, and nature of bonding in substances.

Ice, naphthalene, thermometers, graph papers.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy Notation. Change of state.
CAT

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

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

Q/A and brief discussion.
Class experiments: determine B.P of pure water/ M.P of naphthalene / ice.
Use experimental results to plot temperature-time graphs.
Explain the shape of the graphs.
Q/A: review kinetic theory of matter.
Apply the theory to explain the shape of the graph, and nature of bonding in substances.

Ice, naphthalene, thermometers, graph papers.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of solution.

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

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

Ammonia nitrate / sodium hydroxide, thermometers.

K.L.B. BK IV
Pages 40-41

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.

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

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

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

Group experiments / teacher demonstration.

Obtain and record results.


Work out calculations.
Group experiments/ teacher demonstration.
Note steady temperature of solutions formed when zinc/ iron / magnesium reacts with copper sulphate solution.
Work out the molar heat of displacement of a substance from a solution of its ions.

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

K.L.B. BK IV
Pages 45-48
K.L.B. BK IV
Pages 48-50

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of displacement of ions.

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.

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.

Zinc, iron, magnesium, copper sulphate solution.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of solution of neutralization.

By the end of the lesson, the learner should be able to:
Define the term neutralization.
Determine the molar heat of neutralization of HCl with NaOH.

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.

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

K.L.B. BK IV
Pages 50-53