ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Alkanoic (Carboxylic Acids).

By the end of the lesson, the learner should be able to:
Identify the functional group of alkanoic (carboxylic) acids.
Explain formation of alkanoic acid molecule.

Q/A: review functional group of alkanols.

Brief discussion.

student book

K.L.B. BK IV
Page 219

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Nomenclature of alkanoic acids.

By the end of the lesson, the learner should be able to:
Name and draw the structure of simple alkanoic acids.

Guided discovery of the naming system for alkanoic acids.

Chart: homologous series of alkanoic acids.

K.L.B. BK IV
Pages 219-221

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Lab preparation of ethanoic acid.
Physical properties of alkanoic acids.

By the end of the lesson, the learner should be able to:
Describe laboratory preparation of ethanoic acid.
Explain some physical properties of alkanoic acids.

Teacher demonstration: prepare ethanoic acid in the lab.

Brief discussion on preparation of ethanoic acid.
Compare physical properties of some alkanoic acids.
Discuss the difference in physical properties among alkanoic acids.

Concentrated H2SO4, potassium manganate
(VII) Crystals, water bath.

student book

K.L.B. BK IV
Pages 221-223
K.L.B. BK IV
Pages 223-4

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Chemical properties of alkanoic acids.

By the end of the lesson, the learner should be able to:
Explain some chemical properties of alkanoic acids.

Group experiment: investigate some chemical properties of ethanoic acid.
Carry out tests and record observations in a table.

Ethanoic acid, universal indicator, sodium carbonate, magnesium strip, ethanol, conc. H2SO4 and sodium hydroxide.

K.L.B. BK IV
Pages 224-5

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Chemical properties & Uses of alkanoic acids.
Soap preparation in the lab.

By the end of the lesson, the learner should be able to:
Write equations for chemical reactions involving acids.
State uses of alkanoic acids.

Review and discuss the observations above.
Write corresponding chemical equations.
Teacher elucidates uses of alkanoic acids.

student book

K.L.B. BK IV
Pages 225-7

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Cleaning action of soap.

By the end of the lesson, the learner should be able to:
Describe the nature of a soap molecule.
Explain the mode of action in cleaning.

Expository and descriptive approaches.
Answer oral questions.

student book

K.L.B. BK IV
Pages 230-232

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Effects of hard / soft water on soap.
Soapless detergents.

By the end of the lesson, the learner should be able to:
Explain the effects of hard/ soft water on soap.
Prepare soapless detergents in the lab.

State merits of soapless detergents over soaps.

Group experiments: form soap lather in different solutions.

Deduce the effects of hard/ soft water on soap.
Teacher demonsration.

Brief discussion.

Distilled water, tap water, rainwater, sodium chloride solution.
Calcium nitrate, Zinc Sulphate, etc.

student book

K.L.B. BK IV
Pages 232-235
K.L.B. BK IV
Pages 235-238

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)
RADIOACTIVITY

Polymers and polymerization.
Definition of radioactivity.

By the end of the lesson, the learner should be able to:
Explain the concepts additional and condensation polymerization as methods of making synthetic polymers.
Identify some products of polymerization.
State merits and demerits of synthetic polymers over natural materials.

Teacher exposes and explains new concepts.

Detailed discussion.

Assignment.

student book

K.L.B. BK IV
Pages 238-242

RADIOACTIVITY

Alpha particles.

By the end of the lesson, the learner should be able to:
State properties of alpha particles.
Describe methods of detecting alpha particles.

Q/A: position of helium in the periodic table.

Expository approach:

student book

K.L.B. BK IV
Pages 251-253

RADIOACTIVITY

Equations involving alpha particles.
Beta particles. Gamma rays.
Radioactive Half-Life.

By the end of the lesson, the learner should be able to:
Write down and balance equations involving alpha particles.

Q/A: Review atomic and mass numbers.
Examples of balanced equations.
Supervised practice.

student book
Dice.

K.L.B. BK IV
Page 257

RADIOACTIVITY
ACIDS, BASES AND SALTS.

Radioactive decay curve.
Nuclear fusion and nuclear fission. Applications of radioactivity.
Strength of acids. Acids in aqueous form.

By the end of the lesson, the learner should be able to:
Plot a radioactive decay curve to deduce the
half ?life from the curve.


Define an acid in terms of hydrogen ions.

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

Drawing a radioactive decay curve inferring the half-life of the sample from the graph.





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.

Graph papers.
student book




Magnesium strip, zinc carbonate,
2M HCl,
2M H2SO4,
2M ethanoic acid.

K.L.B. BK IV
Pages 254-5




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

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.

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.
Dissolving hydrogen chloride gas in water / methylbenzene.

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.


Define a polar and a non-polar solvent.

Carry out pH tests of 2M NaOH and 2M ammonia solution using universal indicator solutions; and observe colour changes.

Carry out electrical conductivity tests of voltameters of the above solutions.

Discussion: relate number of hydroxide ions to pH values and electrical conductivity of bases.


Teacher demonstration:
Dissolving HCl gas in different solvents.
Discuss the observations.
Write down related balanced chemical equations.

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

Ammonia gas,
Methylbenzene, hydrogen chloride gas.

K.L.B. BK IV
Pages 7-9
K.L.B. BK IV
Pages 9-11

ACIDS, BASES AND SALTS.

Dissolving ammonia gas in water/ methylbenzene.

By the end of the lesson, the learner should be able to:
Investigate effect of a polar / non-polar solvent on ammonia gas.

Carry out litmus tests on the resulting solution.
Make observations and deductions thereof.
Write down related balanced chemical equations.

Ammonia gas,
Methylbenzene.

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

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.

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

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

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.
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

ELECTRO-CHEMISTRY.

Redox reactions.

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


Describe redox reactions in terms of gain / loss of electrons.
Identify oxidizing / reducing agents involved in redox reactions.

Q/A: review cations, anions and charges.
Write down ionic half equations and identify reducing / oxidizing agents.

student book

K.L.B. BK IV
Pages 108-9

ELECTRO-CHEMISTRY.

Oxidizing Numbers.

By the end of the lesson, the learner should be able to:
Outline rules of assigning oxidation numbers.
Determine the oxidation numbers of an element in a given compound.
Explain the use of oxidation numbers in naming compounds.

Exposition and giving specific examples.
Work out oxidizing number of elements in given compounds.
Copy and complete a table of compounds containing elements that more than one oxidation number.

student book

K.L.B. BK IV
Pages 109-116

ELECTRO-CHEMISTRY.

Displacement reactions.
The oxidizing power of an element.
Cell diagrams.

By the end of the lesson, the learner should be able to:
Explain change of oxidation numbers during redox / displacement reactions. Arrange elements in order of their reducing power.
Arrange elements in order of their oxidizing power.

Class standard experiments: reacting metals with solutions containing metal ions.
Taking note of reactions and those that do not take place; and tabulating the results.
Teacher demonstration / group expts:
Adding halogens to solutions containing halide ions.
Tabulate the results.
Discuss the results and arrive at the oxidizing power series of halogens.

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

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

K.L.B. BK IV
Pages 116-120
K.L.B. BK IV
Pages 120-122

ELECTRO-CHEMISTRY.

Standard Electrode Potentials.

By the end of the lesson, the learner should be able to:
Identify standard conditions for measuring electrode potentials.
Define the term standard electrode potential of a cell.
Write half reactions of electrochemical cells.

Descriptive and expository approaches: teacher exposes new concepts.

student book

K.L.B. BK IV
Pages 129-131

ELECTRO-CHEMISTRY.

Standard electrode potential series.

By the end of the lesson, the learner should be able to:
Recall the order of standard electrode potentials.
Compare oxidizing and reducing powers of substances.

Q/A: review reactivity series, oxidizing agent, reducing agent.
Exposition: the order of standard electrode potentials.
Discussion: oxidizing and reducing powers of substances.

student book

K.L.B. BK IV
Pages 131-133

ELECTRO-CHEMISTRY.

Emf of a cell.

By the end of the lesson, the learner should be able to:
Calculate emf of a cell using standard electrodes potentials.

Q/A: review half-cells.
Worked examples; supervised practice.
Assignment.

student book

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

ELECTRO-CHEMISTRY.

Possibility of a reaction to take place.

By the end of the lesson, the learner should be able to:
Predict whether a reaction will take place or not using standard electrode potentials.

Worked examples.
Oral exercise.
Assignment.

student book

K.L.B. BK IV
Pages 136-137

ELECTRO-CHEMISTRY.

Primary and secondary chemical cells.

By the end of the lesson, the learner should be able to:
Describe the functioning of primary and secondary chemical cells.

Exposition of new concepts and brief discussion
Assignment.

student book

K.L.B. BK IV
Pages 138-141

ELECTRO-CHEMISTRY.

Electrolysis of dilute NaCl.
Electrolysis of brine.

By the end of the lesson, the learner should be able to:
Define the term electrolysis.
Explain the concept of preferential discharge of ions.
Identify products of electrolysis of brine.

Teacher demonstration: electrolysis of dilute sodium chloride with carbon electrodes.
Test for gases collected.
Write down equations of reactions at each electrode.
Discussion: preferential discharge of ions at electrodes.

Teacher demonstration/ group experiments.
Test for the products of electrolysis.
Write relevant equations.

Dilute sodium chloride voltameter.
Brine voltameter.

K.L.B. BK IV
Pages 141-144
K.L.B. BK IV
Pages 144-146

ELECTRO-CHEMISTRY.

Electrolysis of dilute sulphuric (VI) acid.
Factors affecting electrolysis.

By the end of the lesson, the learner should be able to:
Identify products of electrolysis of dilute sulphuric (VI) acid.

Teacher demonstration/ group experiments.
Test for the products of electrolysis.
Write relevant equations.

Sulphuric acid voltameter.
student book

K.L.B. BK IV
Pages 146-148

ELECTRO-CHEMISTRY.

Application of electrolysis.

By the end of the lesson, the learner should be able to:
Describe some applications of electrolysis.

Probing questions and brief discussion on applications of electrolysis.
Practical assignment on electrolysis: electroplating an iron nail with a suitable metal.

Suitable voltameter.

K.L.B. BK IV
Pages 155-7

ELECTRO-CHEMISTRY.

Faraday?s law of electrolysis.

By the end of the lesson, the learner should be able to:
State Faraday?s law of electrolysis.
Solve problems related to Faraday?s law of electrolysis.

Discuss above results, leading to Faraday?s law of electrolysis.

Worked examples.

Assignment.

Weighing balance, stop watch, copper sulphate voltameter.

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

RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of temperature of reactants on rate of reaction.
Effect of change in surface area of reactants on the rate of a reaction.
Effect of a suitable catalyst on the rate of a reaction

By the end of the lesson, the learner should be able to:
Explain the effect of temperature on rate of reaction.
Explain the effect of change in surface area on the rate of a reaction.

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.

Sodium thiosulphate heated at different temperatures, dilute HCl, stopwatches.
Graph papers.
Marble chips, marble chips powder, syringes, conical flasks with stoppers, 1M HCl.
Hydrogen peroxide, manganese (IV) oxide.

K.L.B. BK IV
Pages 80-83
K.L.B. BK IV
Pages 83-85

RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of light on rate of specific reactions.

By the end of the lesson, the learner should be able to:
Identify reactions that are affected by light.

Teacher demonstration: decomposition of silver bromide in the presence of light.
Mention other examples of reactions affected by light.

Silver bromide.

K.L.B. BK IV
Pages 89-91

RATES OF REACTION & REVERSIBLE REACTIONS.

Reversible reactions.

By the end of the lesson, the learner should be able to:
Write down equations for reversible reactions.

Q/A: review temporary and permanent changes.
Teacher demonstration: heating crystals of hydrated copper (II) sulphate, then ?hydrating? them.
Write the corresponding chemical equations.
Give further examples of reversible reactions.

Crystals of hydrated copper (II) sulphate.

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

RATES OF REACTION & REVERSIBLE REACTIONS.

State of equilibrium in chemical reactions.

By the end of the lesson, the learner should be able to:
Define the term equilibrium as used in reversible reactions.
Write down equations of reversible reactions in a state of equilibrium.

Brief discussion, giving examples of chemical equations for reversible reactions.

student book

K.L.B. BK IV
Pages 94-95

RATES OF REACTION & REVERSIBLE REACTIONS.

Le Chatelier?s Principle.
Effect of change of pressure and temperature on equilibrium shift.
The Haber Process.

By the end of the lesson, the learner should be able to:
State Le Chatelier?s Principle.
Explain the concept optimum conditions of a chemical equilibrium.
Explain factors that change the position of equilibrium of the Harber process.

Investigate the effect of change of concentration of reactants on equilibrium.
Add 2M sodium hydroxide in steps to bromine water.
Make and record observations.
Discuss the results leading to
Le Chatelier?s Principle.

Q/A and detailed discussion on change of pressure, temperature, concentration of ammonia and effect of presence of a suitable catalyst on the Haber process.

Add 2M sodium hydroxide,
student book

K.L.B. BK IV
Pages 95-97
K.L.B. BK IV
Pages 102-103

RATES OF REACTION & REVERSIBLE REACTIONS.

The Contact Process.

By the end of the lesson, the learner should be able to:
Explain how change of temperature and pressure affect rate of manufacture of sulphur (VI) acid.

Probing questions and brief discussion.

Assignment.

student book

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