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.
Enthalpy of combustion. Enthalpy of combustion.

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

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.

Group experiments / teacher demonstration.

Obtain and record results.


Work out calculations.

Conc. H2SO4, thermometers.
Ethanol, distilled water, thermometer, clear wick, tripod stand and wire gauze.

K.L.B. BK IV
Pages 42-45
K.L.B. BK IV
Pages 45-48

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Standard enthalpy changes.

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.

Exposition & brief discussion.

student book

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

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

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

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 56-57
K.L.B. BK IV
Pages 60-64

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Heat values of fuels.

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.

Probing questions and brief discussion.

student book

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
RATES OF REACTION & REVERSIBLE REACTIONS.

Environmental effects of fuels.
Effect of temperature of reactants on rate of reaction.

By the end of the lesson, the learner should be able to:
Outline some environmental effects of fuels.
Identify measures taken to reduce environmental
pollution.

Q/A & open discussion.

student book
Sodium thiosulphate heated at different temperatures, dilute HCl, stopwatches.
Graph papers.

K.L.B. BK IV
Pages 67-68

RATES OF REACTION & REVERSIBLE REACTIONS.

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

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

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.

Marble chips, marble chips powder, syringes, conical flasks with stoppers, 1M HCl.

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

RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of a suitable catalyst on the rate of a reaction
Effect of light on rate of specific reactions.
Reversible reactions.

By the end of the lesson, the learner should be able to:
Explain effects of a suitable catalyst on the rate of a reaction.
Identify reactions that are affected by light.

Teacher demonstration: preparation and collection of oxygen gas without using a catalyst, then using manganese (IV) oxide as a catalyst.
Explain the results in terms of activation energy.

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

Hydrogen peroxide, manganese (IV) oxide.
Silver bromide.
Crystals of hydrated copper (II) sulphate.

K.L.B. BK IV
Pages 85-88
K.L.B. BK IV
Pages 89-91

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.

By the end of the lesson, the learner should be able to:
State Le Chatelier?s Principle.

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.

Add 2M sodium hydroxide,

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

RATES OF REACTION & REVERSIBLE REACTIONS.

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:
Explain the effect of change of pressure & te,perature on equilibrium shift.

Q/A: review kinetic theory of matter.
Q/A & discussion on effect of change of pressure / temperature on shifting of equilibrium; giving specific examples of chemical equations.
Written assignment.

student book

K.L.B. BK IV
Pages 97-101

RATES OF REACTION & REVERSIBLE REACTIONS.
ELECTRO-CHEMISTRY.

The Contact Process.
Redox reactions.
Oxidizing Numbers.

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.


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

Probing questions and brief discussion.

Assignment.


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 103-104
K.L.B. BK IV
Pages 108-9

ELECTRO-CHEMISTRY.

Displacement reactions.

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.

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.

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

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

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.

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.

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

Zinc/ copper cell.

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

ELECTRO-CHEMISTRY.

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

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.

Recall the order of standard electrode potentials.
Compare oxidizing and reducing powers of substances.

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.

student book

K.L.B. BK IV
Pages 129-131
K.L.B. BK IV
Pages 131-133

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.

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.
Factors affecting electrolysis.

By the end of the lesson, the learner should be able to:
Identify products of electrolysis of brine.
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.

Brine voltameter.
Sulphuric acid voltameter.
student book

K.L.B. BK IV
Pages 144-146
K.L.B. BK IV
Pages 153-5

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.
METALS

Faraday?s law of electrolysis.
Ores of some metals.

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

METALS

Occurrence and extraction of sodium.

By the end of the lesson, the learner should be able to:
Describe occurrence and extraction of sodium.

Oral questions on electrolysis and equations at electrodes.
Brief discussion on occurrence and extraction.

Chart: Down?s cell.

K.L.B. BK IV
Pages 170-171

METALS

Occurrence and extraction of aluminium.
Occurrence and extraction of iron.
Occurrence and extraction of zinc.

By the end of the lesson, the learner should be able to:
Describe occurrence and extraction of aluminium.
Describe occurrence and extraction of zinc by electrolysis and reduction methods.

Brief discussion.
Write relevant chemical equations.

student book
Chart: Blast furnace.
Flow chart: extraction of Zinc.

K.L.B. BK IV
Pages 171-3
K.L.B. BK IV
Pages 175-9

METALS

Extraction of lead.

By the end of the lesson, the learner should be able to:
Explain how lead is extracted.

Q/A & brief discussion.
Write balanced chemical equations leading to extraction of lead.

Flow chart: extraction of lead.

K.L.B. BK IV
Pages 179-80

METALS

Occurrence and extraction of copper.

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

Q/A & brief discussion.
Write balanced chemical equations leading to extraction of copper.

Flow chart: extraction of copper.

K.L.B. BK IV
Pages 181-183

METALS

Physical properties of some metals.

By the end of the lesson, the learner should be able to:
State general properties of metals.
Explain the difference in physical properties of metals.

Compare physical properties of some metals as summarized in a chart.
Q/A & discussion based on physical properties.

student book

K.L.B. BK IV
Pages 183-4

METALS

Reaction of metals with oxygen.
Reaction of metals with cold water and steam.

By the end of the lesson, the learner should be able to:
Explain effect of burning metals in air.
Describe reaction of metals with cold water and steam.

Arrange the metals in order of reactivity with cold water and steam.

Teacher demonstration / Group experiments.
Burning some metals in air.
Write relevant equations.
Brief discussion.

Class experiments:
Investigate reaction of some metals with cold water and steam.
Analyse the results.

Common lab. metals.
Metals: Al, Zn, Fe, Cu.

K.L.B. BK IV
Pages 184-6
K.L.B. BK IV
Pages 186-9

METALS

Reaction of metals with chlorine.

By the end of the lesson, the learner should be able to:
Describe the reaction of metals with chlorine.

Teacher demonstration in a fume cupboard / in the open.
Investigate reaction of metals with chorine
Write corresponding equations.

Metals: Al, Zn, Fe, Cu.

K.L.B. BK IV
Pages 189-191

METALS

Reaction of metals with acids.

By the end of the lesson, the learner should be able to:
Describe and explain reaction of metals with acids.

Group experiments: investigate reaction of metals with dilute acids.
Teacher demonstration: investigate reaction of metals with concentrated acids.
Discuss the observations made and write relevant chemical equations.

Metals: Al, Zn, Fe, Cu.

Acids; HCl, HNO3, H2SO4.

K.L.B. BK IV
Pages 191-4

METALS

Uses of metals.

By the end of the lesson, the learner should be able to:
State uses of some metals and alloys.

Q/A & brief discussion;
Uses of Sodium, Aluminium, Zinc, Iron and Copper & some alloys.

student book

K.L.B. BK IV
Pages 194-7

METALS
ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Environmental effects of extraction of metals.
Alkanols (Alcohols).
Nomenclature of alkanols.

By the end of the lesson, the learner should be able to:
Identify some environmental effects of extraction of metals.
Name and draw the structure of simple alkanols.

Oral questions and open discussion.

Assignment / Topic review.
Guided discovery of naming system for alkanols.
Draw and name structures of alkanols.

student book

K.L.B. BK IV
Pages 197-8
K.L.B. BK IV
Pages 206-8

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Isomerism in alkanols.

By the end of the lesson, the learner should be able to:
Describe positional and chain isomerism in alkanols.
Explain formation of primary and secondary alkanols.

Q/A: review the terms positional and chain isomerism.
Brief discussion on isomerism.
Oral exercise: naming given organic compounds.
Written exercise: writing structural formulae for isomers of organic compounds of a given molecular formula.

student book

K.L.B. BK IV
Pages 208-10

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)
RADIOACTIVITY

Preparation of ethanol in the lab.
Definition of radioactivity.

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

Group experiments / teacher demonstration.

Discuss the fermentation process.

Calcium hydroxide solution, sugar solution, yeast.
student book

K.L.B. BK IV
Pages 210-11

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

By the end of the lesson, the learner should be able to:
Write down and balance equations involving alpha particles.
Plot a radioactive decay curve to deduce the
half ?life from the curve.

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

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

student book
Dice.
Graph papers.
student book

K.L.B. BK IV
Page 257
K.L.B. BK IV
Pages 254-5