ORGANIC CHEMISTRY (I)

Hydrocarbons.
Alkanes.
Naming Alkanes.

By the end of the lesson, the learner should be able to:
To define organic Chemistry.
To define a hydrocarbon.
To identify groups of hydrocarbons.
To describe the carbon atom.
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.

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

student book
Chart of biomass digester.
student book

K.L.B. BK III
P. 92
Longhorn
Book III
P 135

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.
Chemical 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.
Describe chemical properties of alkanes.

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

Sodium ethanoate, sodalime,
Pestle and mortar.
student book

K.L.B. BK III
P. 103

Longhorn
Book III
PP 146

ORGANIC CHEMISTRY (I)

Substitution reactions involving alkanes. Uses of alkanes.
Alkenes. Molecular formulae of alkenes.

By the end of the lesson, the learner should be able to:
To describe substitution reactions involving alkanes.
To list down uses of alkanes.
To write molecular formulae of alkenes.

Discussion
Teacher elucidates uses of alkanes.
Examine table of members of alkenes.
To identify members of alkene series.

student book

K.L.B. BK III
P. 108

Longhorn
Book III
PP 149-50

ORGANIC CHEMISTRY (I)

Naming alkenes.
Alkene isomerism.
Preparing ethene in the lab.
Physical properties of ethene.
Chemical properties of ethene.

By the end of the lesson, the learner should be able to:
To name various alkenes.
Differentiate between branching and positional isomerism.
To describe lab preparation of ethene.
To describe physical properties of ethene and other alkenes.
To explain halogenation and hydrogenation reactions.

Q/Q: Nomenclature in alkenes.
Compare alkenes; hence deduce names of various alkenes.
Discussion and drawing of molecular structures.
Teacher demonstration: - Carry out tests on ethene as students note down the observations in a table.
To discuss physical properties of ethene and other alkenes.
Discussion and drawing structures.

student book
chart
student book
charts

K.L.B. BK III
PP. 110-113
Longhorn
Book III
PP 154-6


K.L.B. BK III
P 162

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.

By the end of the lesson, the learner should be able to:
To identify various alkynes.
To name and draw structures of alkynes.

Discuss a table of members of alkynes.
Review naming of alkanes and alkene and compare this with naming of alkynes.

charts

K.L.B. BK III
P. 122-123
Longhorn
Book III
PP 126-129 171-5

ORGANIC CHEMISTRY (I)

Isomerism in alkynes.
Physical properties of ethyne.
Chemical properties of ethyne.

By the end of the lesson, the learner should be able to:
To draw structure showing positional and branching isomerism.
To list down physical properties of ethyne.
To describe combustion, halogenation and hydrogenation processes.

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

charts

K.L.B. BK III
PP. 124-125
Longhorn
Book III
PP 176-8

ORGANIC CHEMISTRY (I)
ACIDS, BASES AND SALTS.

Tests for alkynes. Uses of alkynes.
Strength of acids. Acids in aqueous form.

By the end of the lesson, the learner should be able to:
To describe tests for alkynes and state uses of alkynes.


Define an acid in terms of hydrogen ions.

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

Discussion and explanations.

Assignment.




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.

charts




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

K.L.B. BK III
P.130

Longhorn Book III
PP 180-84





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

ACIDS, BASES AND SALTS.

pH values of acids. Electrical conductivities of aqueous acids.
Definition of a base in terms of hydroxide ions.
Neutralization reaction.

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.
Define a base in terms of hydroxide ions.
Determine the results of reaction of an acid and a base.

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.
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.
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.

Universal
indicator,
2M HCl,
2M ethanoic acid,
dry cells,
carbon electrodes,
milli-ammeters,
wires, switches etc.
Red litmus paper, calcium hydroxide solid.
1M HCl,
Calcium hydroxide,
universal indicator.

K.L.B. BK IV
Pages 4-6

ACIDS, BASES AND SALTS.

Strength of bases.

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.

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.

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

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

ACIDS, BASES AND SALTS.

Dissolving hydrogen chloride gas in water / methylbenzene.
Dissolving ammonia gas in water/ methylbenzene.

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

Teacher demonstration:
Dissolving HCl gas in different solvents.
Discuss the observations.
Write down related balanced chemical equations.
Carry out litmus tests on the resulting solution.
Make observations and deductions thereof.

Ammonia gas,
Methylbenzene, hydrogen chloride gas.
Methylbenzene.

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

ACIDS, BASES AND SALTS.

Amphoteric oxides.
Precipitation Reactions.
Solubility of chlorides sulphites and sulphates.

By the end of the lesson, the learner should be able to:
Define an amphoteric oxide.
Identify some amphoteric oxides.

Define a precipitate.
Write ionic equations showing formation of precipitates.
Find out cations that form (in)soluble chlorides, sulphates and sulphites.

Class experiment:
Carry out acid / base reactions with metal oxides.
Q/A: make deductions from the results.
Writing and balancing relevant equations.


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.
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.

2M Nitric acid
2M NaOH,
HNO3.
Amphoteric oxides.
Soluble carbonates e.g. Na2CO3, K2CO3, (NH4)2CO3
Salt solutions containing Mg2+, Al3+, Ca2+, etc.
0.1M solution containing Pb2+, 2M NaCl solution, 2M sodium sulphate, source of heating.

K.L.B. BK IV
Pages 12-14
K.L.B. BK IV
Pages 14-16

ACIDS, BASES AND SALTS.

Equations for formation of insoluble chlorides, sulphites and sulphates.

By the end of the lesson, the learner should be able to:
Write down equations for formation of insoluble chlorides, sulphites and sulphates.

Q/A: review observations made in the above experiments.
Discuss the solubility of the cations.
Write relevant ionic equations.

student book

K.L.B. BK IV
Pages 17-18

ACIDS, BASES AND SALTS.

Complex ions.
Solubility of a salt at a given temperature.

By the end of the lesson, the learner should be able to:
Explain formation of complex ions.
Define the term solubility.
Determine solubility of a given salt at room temperature.

Add drops of 2M sodium hydroxide / 2M ammonia solution to a solution containing Mg2+, Zn2+, etc.
Make observations and discuss the results.
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.

2M Sodium hydroxide (2M ammonia solution),
solution containing Mg2+, Zn2+, etc.
Suitable solutes.

K.L.B. BK IV
Pages 18-20

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.
ACIDS, BASES AND SALTS.
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Effect of temperature on solubility of a solute in a solvent.
Effects of various salts on soap.
Removal of hardness of water.
Endothermic and Exothermic Reactions.
Energy level diagrams.

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.
Identify ions for hardness of water.
Identify methods of removing hardness of water.
State merits & demerits of hard water.
To differentiate between endothermic & exothermic reactions.
Represent endothermic reactions with exothermic reactions with energy level diagrams.

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.
Review results of above experiments.
Probing questions & brief discussion.
Assignment.
Investigate temperature changes in solution formation.
Obtain changes in temperature when ammonium nitrate and sodium hydroxide are dissolved in water, one at a time.
Probing questions on relative energies of reactants and products in endothermic and exothermic and endothermic reactions.

KClO3 thermometers, source of heat.
distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+.
student book
Ammonium nitrate,
Sodium hydroxide, thermometers.

K.L.B. BK IV
Pages 22-25
K.L.B. BK IV
Pages 27-29

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy Notation. Change of state.

By the end of the lesson, the learner should be able to:
Define the term enthalpy.
Distinguish positive enthalpy change from negative enthalpy change.

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

Q/A and brief discussion.
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.

Ice, naphthalene, thermometers, graph papers.

K.L.B. BK IV
Pages 35-39

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

CAT
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.

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Molar heat of solution of H2SO4.

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

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.

Conc. H2SO4, thermometers.

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy of combustion. Enthalpy of combustion.

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

Group experiments / teacher demonstration.

Obtain and record results.


Work out calculations.

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

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.
Standard enthalpy changes.
Hess?s Law.

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.
Define the term standard enthalpy change.
Denote standard enthalpy change with the correct notation.
State Hess?s law.

Solve problems related to Hess?s law.

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.
Exposition & brief discussion.
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.

2M HCl of known volume, 1M / 2M sodium hydroxide.
student book

K.L.B. BK IV
Pages 50-53
K.L.B. BK IV
Pages 56-57

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Heat of solution hydration energy and lattice energy.
Heat values of fuels.

By the end of the lesson, the learner should be able to:
Define the terms lattice energy and hydration energy.
Explain the relationship between heat of solution, hydration energy.
Solve related problems.
Define the term fuel.
Describe energy changes when a fuel undergoes combustion.
Outline factors considered when choosing a suitable fuel.

Exposition of new concepts.
Guided discovery of the relationship between heat solution hydration energy and lattice energy.
Worked examples.
Assignment.
Probing questions and brief discussion.

student book

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Environmental effects of fuels.

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

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

RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of concentration on rate of a reaction
Effect of time of reaction on the rate of reaction.

By the end of the lesson, the learner should be able to:
Explain the effects of change of concentration of reactants on a reaction.
Explain how the rate or reaction changes as the reaction proceed

Group experiments to investigate effect of concentration on rate of reaction using dil. HCl and magnesium ribbons.
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.
Group experiments: investigate volume of gas evolved when magnesium reacts with dilute HCl.
Collect evolved gas and sketch and illustrative graphs.
Discuss the results.

Portions of 2M HCl diluted with different volumes of water,
Stopwatches.
Magnesium ribbons, stopwatches, conical flask.
100cm3 0.5M HCl, syringes, stoppers, tubes and connectors.

K.L.B. BK IV
Pages 73-74

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Alkanols (Alcohols).
Nomenclature of alkanols.
Isomerism in alkanols.
Preparation of ethanol in the lab.

By the end of the lesson, the learner should be able to:
Identify the functional group of alkanols.
Explain formation of alkanol molecules.
Name and draw the structure of simple alkanols.
Describe positional and chain isomerism in alkanols.
Explain formation of primary and secondary alkanols.
Describe preparation of ethanol in the laboratory.

Q/A: review alkanes, alkenes and alkynes.
Teacher exposes new concepts and links them with already known concepts.
Guided discovery of naming system for alkanols.
Draw and name structures of 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.
Group experiments / teacher demonstration.

Discuss the fermentation process.

student book
Calcium hydroxide solution, sugar solution, yeast.

K.L.B. BK IV
Page 205
K.L.B. BK IV
Pages 210-11

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Physical properties of alkanols.
Chemical properties of alkanols.

By the end of the lesson, the learner should be able to:
Explain the physical properties of alkanols.
Describe some chemical reactions of alkanols.

Comparative evaluation of physical properties of alkanols.
Q/A & discussion on variation in physical properties of alkanols.
Group experiments/ teacher demonstration to investigate combustion of ethanol and its reaction with metals.
Write corresponding chemical equations.

student book

K.L.B. BK IV
Page 212

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Esters and esterification.
Oxidation of ethanol. Uses of alkanols.

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

Teacher exposes and explains new concepts.
Assignment.
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 215-6

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

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


Describe laboratory preparation of ethanoic acid.
Explain some physical properties of alkanoic acids.
Explain some chemical properties of alkanoic acids.

Guided discovery of the naming system for 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.
Group experiment: investigate some chemical properties of ethanoic acid.
Carry out tests and record observations in a table.

Chart: homologous series of alkanoic acids.
Concentrated H2SO4, potassium manganate
(VII) Crystals, water bath.
student book
Ethanoic acid, universal indicator, sodium carbonate, magnesium strip, ethanol, conc. H2SO4 and sodium hydroxide.

K.L.B. BK IV
Pages 219-221
K.L.B. BK IV
Pages 221-223

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.
Describe soap preparation in the lab.

Review and discuss the observations above.
Write corresponding chemical equations.
Teacher elucidates uses of alkanoic acids.
Group experiments,
Answer questions based on the experiments already carried out.

student book

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

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Cleaning action of soap.
Effects of hard / soft water on soap.
Soapless detergents.
Polymers and polymerization.

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.
Explain the effects of hard/ soft water on soap.
Prepare soapless detergents in the lab.
State merits of soapless detergents over soaps.
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.

Expository and descriptive approaches.
Answer oral questions.
Group experiments: form soap lather in different solutions.
Deduce the effects of hard/ soft water on soap.
Teacher demonsration.
Brief discussion.
Teacher exposes and explains new concepts.
Detailed discussion.
Assignment.

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

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