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TOPIC  /

SUBTOPIC

OBJECTIVES

ACTIVITIES

/

RESOURCES

1

1,

2

ACIDS, BASES AND SALTS.

Strength of acids.

Acids in aqueous form.

Define an acid in terms of hydrogen ions.

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

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.

Magnesium strip, zinc carbonate,

2M HCl,

2M H₂SO₄,

2M ethanoic acid.

K.L.B.  BK  IV

Pages 1-4

3,

4

pH values of acids.

Electrical conductivities of aqueous acids.

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 / 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.

indicator,

2M HCl,

2M ethanoic acid,

dry cells,

carbon electrodes,

milli-ammeters,

wires, switches etc.

Pages 4-6

5

Definition of a base in terms of hydroxide ions.

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.

Pages6-7

2

1

Neutralization reaction.

Write ionic equation for the reaction.

Calcium hydroxide,

universal indicator.

Page 7

2,3

Strength of bases.

Classify bases/ alkali as either strong or weak in terms of complete /  partial ionization.

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 ammonia solution, universal indicator solutions, dry cells,

carbon electrodes,

milliammeters,

wires, switches etc

Pages7-9

4

Dissolving hydrogen chloride gas in water / methylbenzene.

Dissolving HCl gas in different solvents.

Discuss the observations.

Write down related balanced chemical equations.

Methylbenzene, hydrogen chloride gas.

Pages 9-11

5

Dissolving ammonia gas in water/ methylbenzene.

Make observations and deductions thereof.

Write down related balanced chemical equations.

Methylbenzene.

Pages 11-12

3

1,2

Amphoteric oxides.

Identify some amphoteric oxides.

Carry out acid / base reactions with metal oxides.

Q/A: make deductions from the results.

Writing and balancing relevant equations.

2M NaOH,

HNO₃.

Amphoteric oxides.

Pages 12-14

3,4

Precipitation Reactions.

Write ionic equations showing formation of precipitates.

Class experiment;

Add sodium carbonate or a suitable carbonate to various salt solutions containing Mg²⁺, Al³⁺, Ca²⁺, etc.

Make observations and discuss the results.

Salt solutions containing Mg²⁺, Al³⁺, Ca²⁺, etc.

Pages 14-16

5

Solubility of chlorides sulphites and sulphates.

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.

Pages 16-17

4

1

Equations for formation of insoluble chlorides, sulphites and sulphates.

Discuss the solubility of the cations.

Write relevant ionic equations.

Pages 17-18

2,3

Complex ions.

Make observations and discuss the results.

solution containing Mg²⁺, Zn²⁺, etc.

Pages 18-20

4,5

Solubility of a salt at a given temperature.

Determine solubility of a given salt at room temperature.

Class experiment: determine mass of a solute that dissolves in 100cc of water at room temperature.

Pages 20-21

5

1

Problems solving on solubility.

Supervised practice.

Written assignment.

Pages 21-22

2,3

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

Note temperatures at which crystallization occurs.

Oral questions and discussion.

Pages 22-25

4

Effects of various salts on soap.

Note volume of soap that forms lather readily.

Pages 25-27

5

Removal of hardness of water.

Identify methods of removing hardness of water.

State merits & demerits of hard water.

Probing questions & brief discussion.

Assignment.

Pages 27-29

6

1

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Endothermic and Exothermic Reactions.

Todifferentiate 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.

Pages32-33

2

Energy level diagrams.

Pages33-35

3,4

Enthalpy Notation.

Change of state.

Distinguish positive enthalpy change from negative enthalpy change.

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

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.

Pages 35-39

5

7

1,2

Molar heat of solution.

Determine temperature changes.

Calculate molar heat of solution. Supervised practice.

Pages 40-41

3,4

Molar heat of solution of H₂SO₄.

Note the change in temperature.

Work out the molar heat of solution of H₂SO₄.

Pages42-45

5,

1

Enthalpy of combustion.

Enthalpy of combustion.

Determine the enthalpy of combustion of ethanol.

Explain why actual heats of combustion are usually lower than the theoretical values.

Obtain and record results.

Work out calculations.

Pages45-48

8

2,3

Molar heat of displacement of ions.

Determine the molar heat of solution of displacement of ions.

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.

Pages 48-50

4,5

Molar heat of solution of neutralization.

Determine the molar heat of neutralization of HCl with NaOH.

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.

Pages 50-53

9

1

Standard enthalpy changes.

Denote standard enthalpy change with the correct notation.

Pages 54-56

2,3

Hess’s Law.

Solve problems related to Hess’s law.

Illustrations of energy cycles and energy levels leading to Hess’s law.

Worked examples.

Supervised practice

Written assignment.

Pages 56-57

4,5

Heat of solution hydration energy and lattice energy.

Explain the relationship between heat of solution, hydration energy.

Solve related problems.

Guided discovery of the relationship between heat solution hydration energy and lattice energy.

Worked examples.

Assignment.

Pages60-64

10

1

Heat values of fuels.

Describe energy changes when a fuel undergoes combustion.

Outline factors considered when choosing a suitable fuel.

Pages 64-66

2

Environmental effects of fuels.

Identify measures taken to reduce environmental

pollution.

Pages 67-68

3, 4

RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of concentration on rate of a reaction

Explain the effects of change of concentration of reactants on a reaction.

Determine the time taken for reactions to be complete.

Calculation of concentration of HCl in moles per litre.

Discuss the observations and sketch illustrative graphs.

Stopwatches.

Pages 73-74

5

Effect of time of reaction on the rate of reaction.

Collect evolved gas and sketch and illustrative graphs.

Discuss the results.

100cm³ 0.5M HCl, syringes, stoppers, tubes and connectors.

Pages 75-79

11

1

Sketch and interpret relevant graphs.

Discuss the collision theory and effects of activation energy.

Graph papers.

Pages 80-83

2

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

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.

Pages 83-85

3

Effect of a suitable catalyst on the rate of a reaction

Explain the results in terms of activation energy.

Pages 85-88

4

Effect of light on rate of specific reactions.

Mention other examples of reactions affected by light.

Pages 89-91

5

Reversible reactions.

Teacher demonstration: heating crystals of hydrated copper (II) sulphate, then “hydrating” them.

Write the corresponding chemical equations.

Give further examples of reversible reactions.

Pages 91-93

12

1

State of equilibrium in chemical reactions.

Write down equations of reversible reactions in a state of equilibrium.

Pages 94-95

2

Le Chatelier’s Principle.

Add 2M sodium hydroxide in steps to bromine water.

Make and record observations.

Discuss the results leading to

Le Chatelier’s Principle.

Pages 95-97

3

Effect of change of pressure and temperature on equilibrium shift.

Q/A & discussion on effect of change of pressure / temperature on shifting of equilibrium; giving specific examples of chemical equations.

Written assignment.

Pages 97-101

4

The Haber Process.

Explain factors that change the position of equilibrium of the Harber process.

Pages 102-103

5

The Contact Process.

Assignment.

Pages 103-104

13

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TOPIC  /

SUBTOPIC

OBJECTIVES

ACTIVITIES

RESOURCES

1

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ELECTRO-CHEMISTRY.

Redox reactions.

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.

Pages108-9

2

Oxidizing Numbers.

Determine the oxidation numbers of an element in a given compound.

Explain the use of oxidation numbers in naming compounds.

Work out oxidizing number of elements in given compounds.

Copy and complete a table of compounds containing elements that more than one oxidation number.

Pages109-116

3,4

Displacement reactions.

Taking note of reactions and those that do not take place; and tabulating the results.

Solutions containing Ca²⁺, Mg²⁺, Zn²⁺, Fe²⁺.

Pages116-120

5

The oxidizing power of an element.

Adding halogens to solutions containing halide ions.

Tabulate the results.

Discuss the results and arrive at the oxidizing power series of halogens.

Cl₂ (g),

Br₂ (l),

I₂ (s).

Halides:

KCl, KBr, KI.

Pages 120-122

2

1

Cell diagrams.

Describe components of a cell diagram.

Draw cell diagrams using correct notations.

Q/A & discussion: changes in oxidation numbers.

Exposition: cell diagram and deducing the direction of electron flow.

Pages 123-128

2

Standard Electrode Potentials.

Define the term standard electrode potential of a cell.

Write half reactions of electrochemical cells.

Pages 129-131

3,4

Standard electrode potential series.

Compare                oxidizing and reducing powers of substances.

Exposition:  the order of standard electrode potentials.

Discussion: oxidizing and reducing powers of substances.

Pages 131-133

5

Emf of a cell.

Worked examples; supervised practice.

Assignment.

Pages 133-136

3

1

Possibility of a reaction to take place.

Oral exercise.

Assignment.

Pages136-137

3

2

Primary and secondary chemical cells.

Assignment.

Pages 138-141

3,4

Electrolysis of dilute NaCl.

Explain the concept of preferential discharge of ions.

Test for gases collected.

Write down equations of reactions at each electrode.

Discussion: preferential discharge of ions at electrodes.

Pages 141-144

5

Electrolysis of brine.

Test for the products of electrolysis.

Write relevant equations.

Pages 144-146

4

1

Electrolysis of dilute sulphuric (VI) acid.

Test for the products of electrolysis.

Write relevant equations.

Pages 146-148

2

Factors affecting electrolysis.

Teacher writes down order of ease of discharge of ions at electrodes.

Discussion: other factors; giving suitable examples.

Pages 153-5

4

3

Application of electrolysis.

Practical assignment on electrolysis: electroplating an iron nail with a suitable metal.

Pages 155-7

4

Faraday’s law of electrolysis.

Calculate quantity of electricity using the equation Q = It.

Pages 160-161

5

Faraday’s law of electrolysis.

Solve problems related to Faraday’s law of electrolysis.

Worked examples.

Assignment.

Pages 161-4

5

1

2

METALS

Ores of some metals.

Name the chief ores of some metals.

Exposition and brief discussion.

Pages 168-9

3

Occurrence and extraction of sodium.

Brief discussion on occurrence and extraction.

Pages 170-171

4

Occurrence and extraction of aluminium.

Write relevant chemical equations.

Pages 171-3

5

Occurrence and extraction of iron.

Write relevant chemical equations.

Pages 173-5

6

1,2

Occurrence and extraction of zinc.

Write relevant chemical equations.

Pages175-9

3

Extraction of lead.

Write balanced chemical equations leading to extraction of lead.

Pages 179-80

4

Occurrence and extraction of copper.

Write balanced chemical equations leading to extraction of copper.

Pages 181-183

5

Physical properties of some metals.

Explain the difference in physical properties of metals.

Q/A & discussion based on physical properties.

Pages 183-4

7

1,2

Reaction of metals with oxygen.

Burning some metals in air.

Write relevant equations.

Brief discussion.

Pages 184-6

3,4

Reaction of metals with cold water and steam.

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

Investigate reaction of some metals with cold water and steam.

Analyse the results.

Pages 186-9

5,

1

Reaction of metals with chlorine.

Investigate reaction of metals with chorine

Write corresponding equations.

Pages 189-191

8

2,3

Reaction of metals with acids.

Teacher demonstration: investigate reaction of metals with concentrated acids.

Discuss the observations made and write relevant chemical equations.

Acids; HCl, HNO₃, H₂SO_4.

Pages 191-4

4

Uses of metals.

Uses of Sodium, Aluminium, Zinc, Iron and Copper & some alloys.

Pages 194-7

5

Environmental effects of extraction of metals.

Assignment / Topic review.

Pages 197-8

9

1

ORGANIC CHEMISTRY II

(ALKANES & ALKANOIC ACIDS)

Alkanols (Alcohols).

Identify the functional group of alkanols.

Explain formation of alkanol molecules.

Q/A: review alkanes, alkenes and alkynes.

Teacher exposes new concepts and links them with already known concepts.

Page 205

2

Nomenclature of alkanols.

Draw and name structures of alkanols.

Pages 206-8

3

Isomerism in alkanols.

Explain formation of primary and secondary alkanols.

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.

Pages 208-10

4-5

Preparation of ethanol in the lab.

Discuss the fermentation process.

Pages 210-11

10

1

Physical properties of alkanols.

Q/A & discussion on variation in physical properties of alkanols.

Page 212

2

Chemical properties of alkanols.

Write corresponding chemical equations.

Pages 213-5

3

Esters and esterification.

Describe the esterification process.

Assignment.

Pages 215-6

4,5

Oxidation of ethanol.

Uses of alkanols.

State uses of alkanols.

Explain the effects of alcohol on human health

Brief discussion: oxidation of ethanol using potassium (VII) manganate or potassium (VI) dichromate.

Write corresponding chemical equations.

Open discussion.

Pages 216-8

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RESOURCES

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Alkanoic (Carboxylic Acids).

Explain formation of alkanoic acid molecule.

Brief discussion.

Page 219

2,3

Nomenclature of alkanoic acids.

Pages219-221

4,5

Lab preparation of ethanoic acid.

Brief discussion on preparation of ethanoic acid.

(VII) Crystals, water bath.

Pages221-223

2

1

Physical properties of alkanoic acids.

Discuss the difference in physical properties among alkanoic acids.

Pages223-4

2

Chemical properties of alkanoic acids.

Carry out tests and record observations in a table.

Pages 224-5

2

3

Chemical properties &

Uses of alkanoic acids.

State uses of alkanoic acids.

Write corresponding chemical equations.

Teacher elucidates uses of alkanoic acids.

Pages 225-7

4

Answer questions based on the experiments already carried out.

Pages 227-230

5

Cleaning action of soap.

Explain the mode of action in cleaning.

Answer oral questions.

Pages 230-232

3

1

Effects of hard / soft water on soap.

Deduce the effects of hard/ soft water on soap.

Calcium nitrate, Zinc Sulphate, etc.

Pages 232-235

2

Soapless detergents.

State merits of soapless detergents over soaps.

Brief discussion.

Pages 235-238

3

Polymers and polymerization.

Identify some products of polymerization.

State merits and demerits of synthetic polymers over natural materials.

Teacher exposes and explains new concepts.

Detailed discussion.

Assignment.

Pages 238-242

RADIOACTIVITY

Definition of radioactivity.

Define radioactivity, a nuclide and radioactive decay.

Differentiate between natural and artificial radioactivity.

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.

Pages 249-251

Describe methods of detecting alpha particles.

Expository approach:

Pages 251-253

Examples of balanced equations.

Supervised practice.

Page 257

Gamma rays.

Define isotopes and isobars.

Write down balanced equations involving both alpha and beta particles.

State properties of gamma rays.

Expository approach: teacher briefly exposes new concepts.

Examples of equations.

Supervised practice.

Assignment.

Pages 251-253

Half-Life.

Exposition of the term half-life.

Worked examples.

Written exercise

Pages253-4

half –life from the curve.

Pages 254-5

Applications of radioactivity.

Describe applications of radioactivity.

Brief discussion: Carbon dating, detecting leakage, medication, agriculture, industry; effect of static charges, etc.

Pages 259-260