GAS LAWS

Boyle?s law.
Boyle?s law: - Equation and graphical representation.

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.
Represent Boyle?s law mathematically and graphically.

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.
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
Volume-pressure relationship.
Syringes.
chart

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

Longhorn Book III
PP 1 -2

GAS LAWS

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

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.

State Charles? law.
Explain Charles? law using kinetic theory of matter.

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.
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.

Calculators.
Graph papers.
Coloured water,
Glass tube,
Warm water,
Cork and
Flask.

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

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

Longhorn Book III PP 9-11

GAS LAWS

Temperature in Degree Celsius and Kelvin. Equation and graphs from Charles? law.
Charles? law- equation and graphical representation.

By the end of the lesson, the learner should be able to:
Convert temperature in degree Celsius to Kelvin and vice-versa.
Express Charles? law with equations.
Give a graphical representation of Charles? law.

Teacher explains inter-conversion of the units.
Students complete a table of temperature in the two units.
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.

student book

K.L.B.
BK III P. 10

Longhorn Book III P 11

GAS LAWS

Numerical questions on Charles? Law.
Combined Gas Law.

By the end of the lesson, the learner should be able to:
Solve numerical problems based on Charles? Law.
Derive the Gas Law.
Derive the combined gas law equation.
Solve numerical problems using the equation.

Worked examples.
Supervised exercise.
Assignment.
Q/A: - Combining Boyle?s and Charles? Laws.

Calculators.

K.L.B.
BK III P. 12

Longhorn Book III PP 12-14

GAS LAWS

Standard conditions, S.T.P. conditions and R.T.P. conditions.
Diffusion.

By the end of the lesson, the learner should be able to:
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.
Define diffusion.
Describe experiments to show diffusion.

Exposition of s.t.p. and r.t.p.
Problem solving.
Group experiments.
Diffusion of KMnO4 crystals, concentrated ammonia solution.

student book
KMnO4 crystals,
Litmus papers.

K.L.B.
BK III P. 14

GAS LAWS
THE MOLE

Rates of diffusion.
Graham?s Law.
Mole, molar mass and R.A.M.
Number of moles in a substance.

By the end of the lesson, the learner should be able to:
Compare rates of diffusion of ammonia gas and hydrogen chloride in air.
Carry out numerical tasks.
Define the term mole as a quantity of measurement.
Relate the mole to R.A.M and molar mass.
Calculate number of moles in a given mass of a substance.

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.
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.
Worked examples.
Supervised practice.

student book
Calculators
Chart- table of molar masses of elements.
student book

K.L.B.
BK III
PP. 18-19
Longhorn Book III 21

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

THE MOLE

Relative molecular mass & Relative formula mass.

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

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

Calculators.

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

Longhorn Book III PP 44-60

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.
Calculators on molar solutions.
Dilution of 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.
Solve numerical calculations on molar solutions.
Problems on molar solutions.
Calculate molarity of a solution after dilution.

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

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

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

Stoichiometric equations of various reactions.

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

Class experiments.

Problem solving.

student book

K.L.B. BK III
P. 62

CHLORINE & ITS COMPOUNDS

Lab. preparation of chlorine gas.
Physical properties of chlorine.

By the end of the lesson, the learner should be able to:
Describe laboratory preparation of chlorine gas.
State physical properties of chlorine.

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.

Conc. HCl, Manganese (IV) oxide.
charts

K.L.B.BK III
P. 219
Longhorn
Book III
PP 298-9

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.
Teacher demonstration:
Discussion.
Writing chemical equations.
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.
224 -225
Longhorn
Book III
PP 303-5

CHLORINE & ITS COMPOUNDS

Chlorine and alkalis.

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

Teacher demonstration: Bubbling chlorine with dilute cold / hot NaOH solution.
Make observations and account for them.

Cold / hot NaOH solutions.

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

CHLORINE & ITS COMPOUNDS

Test for chlorides.
Uses of chlorine gas.

By the end of the lesson, the learner should be able to:
To carry out tests for chlorides.
To state uses of chlorine.

Class expts.
Discuss observations, results.
Write chemical equations for the reactions.
Teacher elucidates uses of chlorine.

Expt. Worksheets.
Zinc chloride, litmus paper, conc. Sulphuric acid.

K.L.B.BK III
P. 230
Longhorn Book III
PP 318-319

CHLORINE & ITS COMPOUNDS

Hydrogen chloride gas. Lab. prep. Physical properties.
Aqueous hydrogen chloride.

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

Teacher demonstration.
Carry out tests on the gas and deduce the properties of the gas.
Class experiment leading to deduction of chemical properties of hydrogen chloride gas.

Sodium chloride crystals, conc H2SO4
Distilled water.

K.L.B.BK III
P. 232
Longhorn
Book III
PP 323-4

CHLORINE & ITS COMPOUNDS

Further chemical properties of hydrogen chloride gas.
Large-scale production of hydrochloric acid.
Uses of hydrochloric acid.

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.

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.

Ammonia solution.
charts

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

K.L.B.BK III
P. 237
Longhorn Book III
P 330

CHLORINE & ITS COMPOUNDS
ELECTRO-CHEMISTRY.

Effects of hydrochloric acid on the environment.
Redox reactions.

By the end of the lesson, the learner should be able to:
To explain effects of hydrochloric acid on the environment.
Describe redox reactions in terms of gain / loss of electrons.
Identify oxidizing / reducing agents involved in redox reactions.

Discussion and explanation.
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 238.
Longhorn Book III
PP 334-8

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.

By the end of the lesson, the learner should be able to:
Arrange elements in order of their oxidizing power.

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.

Halogens:
Cl2 (g),
Br2 (l),
I2 (s).

Halides:
KCl, KBr, KI.

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

ELECTRO-CHEMISTRY.

Cell diagrams.
Standard Electrode Potentials.
Standard electrode potential series.
Emf of a cell.

By the end of the lesson, the learner should be able to:
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.
Identify standard conditions for measuring electrode potentials.
Define the term standard electrode potential of a cell.
Write half reactions of electrochemical cells.
Recall the order of standard electrode potentials.
Compare oxidizing and reducing powers of substances.
Calculate emf of a cell using standard electrodes potentials.

Teacher demonstration: Zinc/ copper cell.
Q/A & discussion: changes in oxidation numbers.
Exposition: cell diagram and deducing the direction of electron flow.
Descriptive and expository approaches: teacher exposes new concepts.
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.

Zinc/ copper cell.
student book

K.L.B. BK IV
Pages 123-128
K.L.B. BK IV
Pages 131-133

ELECTRO-CHEMISTRY.

Possibility of a reaction to take place.
Primary and secondary chemical cells.

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.
Describe the functioning of primary and secondary chemical cells.

Worked examples.
Oral exercise.
Assignment.
Exposition of new concepts and brief discussion

student book

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

ELECTRO-CHEMISTRY.

Electrolysis of dilute NaCl.

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

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.

Dilute sodium chloride voltameter.

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

ELECTRO-CHEMISTRY.

Electrolysis of brine.
Electrolysis of dilute sulphuric (VI) acid.

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

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

Brine voltameter.
Sulphuric acid voltameter.

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

ELECTRO-CHEMISTRY.
ELECTRO-CHEMISTRY.
RADIOACTIVITY

Factors affecting electrolysis.
Application of electrolysis.
Faraday?s law of electrolysis.
Definition of radioactivity.

By the end of the lesson, the learner should be able to:
Explain factors that affect electrolytic products discharged at electrodes.
Describe some applications of electrolysis.
State Faraday?s law of electrolysis.
Solve problems related to Faraday?s law of electrolysis.
Define radioactivity, a nuclide and radioactive decay.
Differentiate between natural and artificial radioactivity.

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

K.L.B. BK IV
Pages 153-5
K.L.B. BK IV
Pages 161-4

RADIOACTIVITY

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

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

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

student book
Dice.

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

RADIOACTIVITY

Radioactive decay curve.
Nuclear fusion and nuclear fission. Applications of radioactivity.

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.
Differentiate between nuclear fusion and nuclear fission.
Describe applications of radioactivity.

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.

Graph papers.
student book

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