GAS LAWS

Boyle?s law.

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


State Boyle?s law.
Explain Boyle?s law using kinetic theory of matter.

Teacher demonstration ? Use syringes / pumps to show variation of volume with pressure.
Teacher asks probing questions leading to statement of the law.
Discuss the cause of build-up-in pressure.

Chart
Volume-pressure relationship.

Syringes.

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

Longhorn Book III
PP 1 -2

GAS LAWS

Boyle?s law: - Equation and graphical representation.

By the end of the lesson, the learner should be able to:
Represent Boyle?s law mathematically and graphically.

Q/A: relation between volume and pressure mathematically and graphically.
Derive the relation P1V1=P2V2, and sketch graphs to illustrate Boyle?s law.
Worked examples.
Assignment.

chart

K.L.B. BK III
PP. 3-4

Longhorn Book III
PP 3-5

GAS LAWS

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

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

Supervised exercise: Volume in cm?, m?, litres, and pressure in Pa, mmHg, cmHg, atmospheres.
Assignment.
Completing tables and plotting graphs.
Interpret the plotted graphs.
Make deductions from the graphs.

Calculators.
Graph papers.

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

GAS LAWS

Charles? law.
Temperature in Degree Celsius and Kelvin. Equation and graphs from Charles? law.

By the end of the lesson, the learner should be able to:
State Charles? law.
Explain Charles? law using kinetic theory of matter.
Convert temperature in degree Celsius to Kelvin and vice-versa.

Teacher demonstration:- To show expansion of air when heated and contraction when pressure is constant.
Explain increase in volume when temperature is raised.
Q/A: - relation between volume and temperature, leading to Charles? law.
Teacher explains inter-conversion of the units.
Students complete a table of temperature in the two units.

Coloured water,
Glass tube,
Warm water,
Cork and
Flask.
student book

.K.L.B.
BK III P. 6

Longhorn Book III PP 9-11

GAS LAWS

Charles? law- equation and graphical representation.
Numerical questions on Charles? Law.

By the end of the lesson, the learner should be able to:
Express Charles? law with equations.
Give a graphical representation of Charles? law.
Solve numerical problems based on Charles? Law.

Derive equations from volume and temperature relationship.
Exposition: - Teacher exposes a volume-temperature graph and extrapolates it to obtain the absolute temperature. The definition of absolute temperature is exposed.
Worked examples.
Supervised exercise.
Assignment.

student book
Calculators.

K.L.B. BK III
PP. 6-7

Longhorn Book III P 10

GAS LAWS

Combined Gas Law.
Standard conditions, S.T.P. conditions and R.T.P. conditions.

By the end of the lesson, the learner should be able to:
Derive the Gas Law.
Derive the combined gas law equation.
Solve numerical problems using the equation.
State standard conditions of temperature and pressure of an ideal gas.
State room temperature and pressure of a gas.
Use standard conditions in problem solving.

Q/A: - Combining Boyle?s and Charles? Laws.
Worked examples.
Exposition of s.t.p. and r.t.p.
Problem solving.

Calculators.
student book

K.L.B.
BK III P. 12

Longhorn Book III PP 14-16

GAS LAWS

Diffusion.
Rates of diffusion.

By the end of the lesson, the learner should be able to:
Define diffusion.
Describe experiments to show diffusion.
Compare rates of diffusion of ammonia gas and hydrogen chloride in air.

Group experiments.
Diffusion of KMnO4 crystals, concentrated ammonia solution.
Teacher demonstration: - To deduce rate of diffusion of ammonia gas and hydrogen chloride.
Q/A: - Students calculate ratio of rates of diffusion of the gases.

KMnO4 crystals,
Litmus papers.
student book

K.L.B. BK III
PP. 14-15

Longhorn Book III P 19

GAS LAWS
THE MOLE

Graham?s Law.
Mole, molar mass and R.A.M.

By the end of the lesson, the learner should be able to:
Carry out numerical tasks.
Define the term mole as a quantity of measurement.
Relate the mole to R.A.M and molar mass.

Solve problems involving RMM, equal volumes of the gases involved.
Supervised practice.
Assignment.
Discuss various analogies that lead to the definition of the mole.
Expose the meaning of R.A.M., Avogadro?s constant and molar mass.

Calculators
Chart- table of molar masses of elements.

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

Longhorn Book III PP 22-24

THE MOLE

Number of moles in a substance.
Relative molecular mass & Relative formula mass.

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

Worked examples.
Supervised practice.
Q/A: - Review formulae of compounds.
Complete a table of compounds and their molecular / formula mass.

student book
Calculators.

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

THE MOLE

Moles and Avogadro?s number.
Empirical Formula.

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

Review standard form of numbers.
Worked examples.
Supervised exercise.
Supervised practice.
Assignment.

Calculators.
student book

K.L.B.BK III
PP. 3132
Longhorn
Book III
PP 30-31

THE MOLE

Molecular formula.
Concentration of a solution.

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.

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.

Calculators.
chart

K.L.B.BK III
P. 45

Longhorn
Book III
PP 73-75

THE MOLE

Molarity of a solution.
Preparation of molar solutions.

By the end of the lesson, the learner should be able to:
Define molarity of a solution.
Find molarity of a solution in M/dm?
Define molar solutions.
Prepare molar 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.

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

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

Longhorn
Book III
PP 76-81

THE MOLE

Calculators on molar solutions.
Dilution of solutions.

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.

Worked examples.
Supervised exercise.
Assignment.
Group experiments.
Calculations.

student book

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

THE MOLE

Stoichiometry of a chemical reaction.
Stoichiometric equations.

By the end of the lesson, the learner should be able to:
To determine mole ratio of given reactions.
To define a stoichiometric equation.

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

CuSO4 solution and iron metal.
student book

K.L.B. BK III
P. 56
Longhorn Book III PP 87-92

THE MOLE
ORGANIC CHEMISTRY (I)

Stoichiometric equations of various reactions.
Hydrocarbons.

By the end of the lesson, the learner should be able to:
To investigate and determine Stoichiometric equations of various reactions.
To define organic Chemistry.
To define a hydrocarbon.
To identify groups of hydrocarbons.
To describe the carbon atom.

Class experiments.
Problem solving.
Discuss composition of the carbon atom; hence deduce number of valence electrons.
Exposition of new terms.

student book

K.L.B. BK III
P. 62

ORGANIC CHEMISTRY (I)

Alkanes.
Naming Alkanes.

By the end of the lesson, the learner should be able to:
To identify various alkanes.
To list sources of alkanes.
To state uses of different fractions of crude oil.
To define cracking of alkanes.
To define a homologous series.

Expose various alkanes.
Discuss the biomass digester, fractional distillation of crude oil and uses of the fractions.
Discuss the cracking process.
Discussion and exposition of new concepts.

Chart of biomass digester.
student book

K.L.B. BK III
PP. 93-94

Longhorn
Book III
PP 135-6

ORGANIC CHEMISTRY (I)

Members of Alkane series.
Isomerism in alkanes.

By the end of the lesson, the learner should be able to:
To name members of alkane series and identify their characteristics.
To draw the structures of alkane series.
To draw and name isomers of simple hydrocarbons.

Discussion and exposition of new concepts.

Chart- structure of alkanes.
Models.

K.L.B. BK III
PP. 97-99

Longhorn Book III
PP 137-9

ORGANIC CHEMISTRY (I)

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 describe laboratory preparation of a given alkane.
To state physical properties of the gases prepared.
To describe the trend in physical properties of alkanes.

Teacher demonstration.
Discussion.
Study a table of comparative properties of alkanes.
Make deductions from the table.

Sodium ethanoate, sodalime,
Pestle and mortar.
student book

K.L.B. BK III
P. 103

Longhorn
Book III
PP 146

ORGANIC CHEMISTRY (I)

Chemical properties of alkanes.
Substitution reactions involving alkanes. Uses of alkanes.

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.

Discussion
Examples of balanced equations.
Discussion
Teacher elucidates uses of alkanes.

student book

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

ORGANIC CHEMISTRY (I)

Alkenes. Molecular formulae of alkenes.
Naming alkenes.

By the end of the lesson, the learner should be able to:
To write molecular formulae of alkenes.
To name various alkenes.

Examine table of members of alkenes.
To identify members of alkene series.
Q/Q: Nomenclature in alkenes.
Compare alkenes; hence deduce names of various alkenes.

student book

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

ORGANIC CHEMISTRY (I)

Alkene isomerism.
Preparing ethene in the lab.

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

Discussion and drawing of molecular structures.
Teacher demonstration: - Carry out tests on ethene as students note down the observations in a table.

student book
chart

K.L.B. BK III
P. 113
Longhorn
Book III
PP 158-60

ORGANIC CHEMISTRY (I)

Physical properties of ethene.
Chemical properties of ethene.

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

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

student book
charts

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

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.

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.

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

charts

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

ORGANIC CHEMISTRY (I)
ELECTRO-CHEMISTRY.

Tests for alkynes. Uses of alkynes.
Redox reactions.

By the end of the lesson, the learner should be able to:
To describe tests for alkynes and state uses of alkynes.
Describe redox reactions in terms of gain / loss of electrons.
Identify oxidizing / reducing agents involved in redox reactions.

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

charts
student book

K.L.B. BK III
P.130

Longhorn Book III
PP 180-84

ELECTRO-CHEMISTRY.

Oxidizing Numbers.
Displacement reactions.

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.
Explain change of oxidation numbers during redox / displacement reactions. Arrange elements in order of their reducing power.

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.
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.

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

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

ELECTRO-CHEMISTRY.

The oxidizing power of an element.
Cell diagrams.

By the end of the lesson, the learner should be able to:
Arrange elements in order of their oxidizing power.
Define the terms electrode, potential and e.m.f. of an electrochemical cell.
Describe components of a cell diagram.
Draw cell diagrams using correct notations.

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.
Teacher demonstration: Zinc/ copper cell.
Q/A & discussion: changes in oxidation numbers.
Exposition: cell diagram and deducing the direction of electron flow.

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

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.
Emf of a cell.
Possibility of a reaction to take place.

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.
Calculate emf of a cell using standard electrodes potentials.
Predict whether a reaction will take place or not using standard electrode potentials.

Q/A: review reactivity series, oxidizing agent, reducing agent.
Exposition: the order of standard electrode potentials.
Discussion: oxidizing and reducing powers of substances.
Q/A: review half-cells.
Worked examples; supervised practice.
Assignment.
Worked examples.
Oral exercise.

student book

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

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

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.
Explain factors that affect electrolytic products discharged at electrodes.

Teacher demonstration/ group experiments.
Test for the products of electrolysis.
Write relevant equations.
Q/A: review the electrochemical series of elements.
Teacher writes down order of ease of discharge of ions at electrodes.
Discussion: other factors; giving suitable examples.

Sulphuric acid voltameter.
student book

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

ELECTRO-CHEMISTRY.
ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Application of electrolysis.
Faraday?s law of electrolysis.
Physical properties of alkanols.

By the end of the lesson, the learner should be able to:
Describe some applications of electrolysis.
State Faraday?s law of electrolysis.
Solve problems related to Faraday?s law of electrolysis.
Explain the physical properties of alkanols.

Probing questions and brief discussion on applications of electrolysis.
Practical assignment on electrolysis: electroplating an iron nail with a suitable metal.
Discuss above results, leading to Faraday?s law of electrolysis.
Worked examples.
Assignment.
Comparative evaluation of physical properties of alkanols.
Q/A & discussion on variation in physical properties of alkanols.

Suitable voltameter.
Weighing balance, stop watch, copper sulphate voltameter.
student book

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

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Chemical properties of alkanols.
Esters and esterification.

By the end of the lesson, the learner should be able to:
Describe some chemical reactions of alkanols.
Explain formation of esters.
Describe the esterification process.

Group experiments/ teacher demonstration to investigate combustion of ethanol and its reaction with metals.
Write corresponding chemical equations.
Teacher exposes and explains new concepts.
Assignment.

student book

K.L.B. BK IV
Pages 213-5

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Oxidation of ethanol. Uses of alkanols.

By the end of the lesson, the learner should be able to:
Explain oxidation of ethanol by an oxidizing agent.
State uses of alkanols.
Explain the effects of alcohol on human health

Q/A: review redox reactions, oxidizing and reducing agents.
Brief discussion: oxidation of ethanol using potassium (VII) manganate or potassium (VI) dichromate.
Write corresponding chemical equations.
Open discussion.

student book

K.L.B. BK IV
Pages 216-8

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Alkanoic (Carboxylic Acids).
Nomenclature of alkanoic 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.
Name and draw the structure of simple alkanoic acids.

Q/A: review functional group of alkanols.
Brief discussion.
Guided discovery of the naming system for alkanoic acids.

student book
Chart: homologous series of alkanoic acids.

K.L.B. BK IV
Page 219

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Lab preparation of ethanoic acid.

By the end of the lesson, the learner should be able to:
Describe laboratory preparation of ethanoic acid.

Teacher demonstration: prepare ethanoic acid in the lab.

Brief discussion on preparation of ethanoic acid.

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

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

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Physical properties of alkanoic acids.
Chemical properties of alkanoic acids.
Chemical properties & Uses of alkanoic acids.

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

Compare physical properties of some alkanoic acids.
Discuss the difference in physical properties among alkanoic acids.
Group experiment: investigate some chemical properties of ethanoic acid.
Carry out tests and record observations in a table.
Review and discuss the observations above.
Write corresponding chemical equations.
Teacher elucidates uses of alkanoic acids.

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

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

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Soap preparation in the lab.
Cleaning action of soap.

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

Group experiments,
Answer questions based on the experiments already carried out.
Expository and descriptive approaches.
Answer oral questions.

student book

K.L.B. BK IV
Pages 227-230

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

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.
Define radioactivity, a nuclide and radioactive decay.
Differentiate between natural and artificial radioactivity.

Teacher exposes and explains new concepts.
Detailed discussion.
Assignment.
Q/A: Review the atomic structure.
Exposition: symbolic representation of an atom / nucleus.
Exposition: meaning of radioactivity and radioactive decay.
Discussion: artificial and natural radioactivity.

student book

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

RADIOACTIVITY

Alpha particles.
Equations involving alpha particles.
Beta particles. Gamma rays.
Radioactive Half-Life.
Radioactive decay curve.
Nuclear fusion and nuclear fission. Applications of radioactivity.

By the end of the lesson, the learner should be able to:
State properties of alpha particles.
Describe methods of detecting alpha particles.
Write down and balance equations involving alpha particles.
State properties of beta particles.
Define isotopes and isobars.
Write down balanced equations involving both alpha and beta particles.
State properties of gamma rays.
Define the term radioactive half-life. Solve problems relating to half ?life
Plot a radioactive decay curve to deduce the
half ?life from the curve.
Differentiate between nuclear fusion and nuclear fission.
Describe applications of radioactivity.

Q/A: position of helium in the periodic table.
Expository approach:
Q/A: Review atomic and mass numbers.
Examples of balanced equations.
Supervised practice.
Q/A: Review isotopes.
Expository approach: teacher briefly exposes new concepts.
Examples of equations.
Supervised practice.
Assignment.
Teacher demonstration: Dice experiment.
Exposition of the term half-life.
Worked examples.
Written exercise
Drawing a radioactive decay curve inferring the half-life of the sample from the graph.
Exposition of new concepts accompanied by nuclear equations.
Brief discussion: Carbon dating, detecting leakage, medication, agriculture, industry; effect of static charges, etc.

student book
Dice.
Graph papers.

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