NITROGEN & ITS COMPOUNDS.

Nitrogen (II) oxide. Lab preparation.
Properties of the gas.
Nitrogen (1V) oxide Lab preparation.

By the end of the lesson, the learner should be able to:
To describe lab preparation of nitrogen (II) oxide.
To list down physical properties of nitrogen (II) oxide
To describe chemical properties of nitrogen (11) oxide
To describe nitrogen (IV) oxide lab preparation.

Class experiment: Preparation and carrying out tests on the gas.
Observations recorded in a table.
Q/A: Deductions from tests carried out.
Discussion of chemical properties and writing of equations.
Carry out a confirmatory test for the presence of the gas.
Teacher demonstration: - Preparation of the gas and corresponding equation.
Tests on the gas and make observations.

Dil nitric acid, copper turnings.
charts
Conc. nitric acid, copper turnings.

K.L.B. BK III
P. 142
Longhorn
Book III
PP 200-1

K.L.B. BK III
PP. 144-145

NITROGEN & ITS COMPOUNDS.

Properties of Nitrogen (IV) oxide.
Ammonia. Lab preparation of ammonia.

By the end of the lesson, the learner should be able to:
To list down physical properties of nitrogen (IV) oxide
To describe chemical properties of nitrogen (IV) oxide
To state uses of nitrogen (1V) oxide.
To describe lab preparation of ammonia

Deduce physical properties from the table of observations.
To describe chemical properties from the table of observations.
Discuss uses of nitrogen (1V) oxide.
Q/A: Structure of ammonia.
Group experiments: Preparation of ammonia.
Tests on the gas.

charts
Ca(OH)2, NH4Cl Solutions, CaO, litmus papers..M THREE CHEMISTRY TERM TWO 20....

K.L.B. BK III
PP. 144-147

Longhorn
Book III
P 204

NITROGEN & ITS COMPOUNDS.

Properties of ammonia.

By the end of the lesson, the learner should be able to:
To list down physical properties of ammonia.

Deduce physical properties from the observations above.
Discuss chemical properties from the observations above.
Write down chemical equations.

charts

K.L.B. BK III
P. 150

NITROGEN & ITS COMPOUNDS.

Solubility of ammonia.

By the end of the lesson, the learner should be able to:
To describe an experiment to determine solubility of ammonia.

Teacher demonstration.

Discussion.

charts

K.L.B. BK III
P. 150

NITROGEN & ITS COMPOUNDS.

Reaction of ammonia with metal ions.
Ionic equations of above reactions.
Burning ammonia in the air.

By the end of the lesson, the learner should be able to:
To prepare aqueous solution of ammonia.


To carry out tests of aqueous ammonia on metal ions.
To write iIonic equations of above reactions.
To describe burning ammonia in the air.

Teacher demonstration: - Preparation of aqueous solution of ammonia.

Class experiments: -
Students record observations when drops of aqueous ammonia are added, then in excess.
Discuss precipitation of metal hydroxides by aqueous ammonia.
Confirmatory tests for various concentrations.
Teacher demonstration
Discussion
Chemical equations of reactions.

2 cm Solutions containing various metal ions.
charts
Conc. Ammonium solution
Hot platinum rod
Oxygen.

K.L.B.
BK III
PP. 152-153

K.L.B. BK III
P.154

Longhorn BK III
P 223

NITROGEN & ITS COMPOUNDS.

Reaction of ammonia with copper (II) Oxide.

By the end of the lesson, the learner should be able to:
To name products formed when ammonia reacts with hot CuCl2 solid.
To explain reducing properties of ammonia.

Teacher demonstration and discussion.
Write down equations for the reactions.

Granular CuCl2
Combustion tube,
Dry ammonia
U-tube
Gas jar.

K.L.B.
BK III
P. 158

NITROGEN & ITS COMPOUNDS.

Haber process.

By the end of the lesson, the learner should be able to:
Identify raw materials for Haber process and how they are obtained in large scale.
Discuss the Haber process.
Represent Haber process in a schematic diagram.

Discussion and explanations.

Chart- schematic diagram.

K.L.B. BK III
PP. 159-160
225-226

NITROGEN & ITS COMPOUNDS.

Uses of ammonia.
Nitric acid. Lab preparation.

By the end of the lesson, the learner should be able to:
To list down uses of ammonia.
To list down nitrogenous fertilizers.
To describe lab preparation of nitric acid.

Teacher elucidates uses of ammonia and nitrogenous fertilizers.
Teacher demonstration.
Write equations of reaction.
Discussion.

charts
Retort stand
Conc. H2SO4
KNO3

K.L.B. BK III
P. 161

Longhorn
Book III
PP 126 -226

NITROGEN & ITS COMPOUNDS.

Nitric acid Industrial manufacture.
Reaction of dilute Nitric acid with metals.

By the end of the lesson, the learner should be able to:
To describe industrial manufacture of nitric acid.
To describe reaction of dilute nitric acid with metals.
To write equations of reactions of dilute nitric acid with metals.

Discussion and writing equations.
Class experiment:- making observations and recording them in a table.
Discuss the observations.
Write down equations for the reactions.

Chart
Schematic diagram.
Magnesium
Zinc
Copper

K.L.B. BK III
P. 164

K.L.B. BK III
PP. 165-166

Longhorn
Book III
PP 166-8

NITROGEN & ITS COMPOUNDS.

Nitric acid and carbonates.

By the end of the lesson, the learner should be able to:
To describe action of nitric acid on carbonates and hydrogen carbonates.

Group experiments: - Action of Nitric acid on hydrogen carbonates.

Solutions of
Na2CO3
NaHCO3
ZnCO3
CuCO3

K.L.B. BK III
P. 167

Longhorn
Book III
229-30

NITROGEN & ITS COMPOUNDS.

Reaction of dil. nitric acid with hydrogen carbonates.
Dilute nitric acid and metal hydroxides and oxides.

By the end of the lesson, the learner should be able to:
Write equations for reaction of dil. nitric acid with hydrogen carbonates.
Predict results of reacting dilute nitric acid with metal hydroxides and oxides.

Discussion and corresponding equations.
Group experiments & writing equations for the reactions.

Metal hydroxides.

K.L.B. BK III
P. 167

NITROGEN & ITS COMPOUNDS.

Reaction of nitric acid as an oxidizing agent.

By the end of the lesson, the learner should be able to:
Describe reactions of nitric acid as an oxidizing agent.

Class experiments: -
Explain observations made.

Nitric acid acidified iron sulphate, sulphur, and copper metal.

K.L.B. BK III
PP. 169-170

Longhorn Book III
PP 239 -240

NITROGEN & ITS COMPOUNDS.

Uses of nitric acid & nitrates.
Action of heat on nitrates.

By the end of the lesson, the learner should be able to:
To state uses of nitrates.
To describe preparation of nitrates.
To write equations of decomposition of nitrates on heating.

Discussion
Equations for the reactions for preparation of nitrates.
Discuss above observations.
Write relevant equations.

charts

K.L.B. BK III
P. 171

Longhorn Book III
PP 240
K.L.B. BK III
P 172

NITROGEN & ITS COMPOUNDS.

Test for nitrates.

By the end of the lesson, the learner should be able to:
To carry out tests on nitrates.

Class experiments.
Make observations and deductions.
Discuss the brown ring test for nitrates.

charts

K.L.B. BK III
PP 173-174

Longhorn
Book III
PP 243

NITROGEN & ITS COMPOUNDS.

Nitrogen compounds and the environment.

By the end of the lesson, the learner should be able to:
To explain the pollution of nitrogen compounds in the environment.
To state ways of reducing environmental pollution by nitrogen compounds.

Brief guided discussion.

charts

K.L.B.BK III
PP. 173-174

Longhorn
Book III
PP 244-6

ACIDS, BASES AND SALTS.

Strength of acids. Acids in aqueous form.

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


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

ACIDS, BASES AND SALTS.

pH values of acids. Electrical conductivities of aqueous acids.

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.

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.

Universal
indicator,
2M HCl,
2M ethanoic acid,
dry cells,
carbon electrodes,
milli-ammeters,
wires, switches etc.

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

ACIDS, BASES AND SALTS.

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

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.

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.

Universal
indicator,
2M HCl,
2M ethanoic acid,
dry cells,
carbon electrodes,
milli-ammeters,
wires, switches etc.

Red litmus paper, calcium hydroxide solid.

K.L.B. BK IV
Pages 4-6
K.L.B. BK IV
Pages 6-7

ACIDS, BASES AND SALTS.

Neutralization reaction.

By the end of the lesson, the learner should be able to:
Determine the results of reaction of an acid and a base.

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.

1M HCl,
Calcium hydroxide,
universal indicator.

K.L.B. BK IV
Page 7

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.

By the end of the lesson, the learner should be able to:
Define a polar and a non-polar solvent.

Teacher demonstration:
Dissolving HCl gas in different solvents.
Discuss the observations.
Write down related balanced chemical equations.

Ammonia gas,
Methylbenzene, hydrogen chloride gas.

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

ACIDS, BASES AND SALTS.

Dissolving ammonia gas in water/ methylbenzene.
Amphoteric oxides.

By the end of the lesson, the learner should be able to:
Investigate effect of a polar / non-polar solvent on ammonia gas.
Define an amphoteric oxide.
Identify some amphoteric oxides.

Carry out litmus tests on the resulting solution.
Make observations and deductions thereof.
Write down related balanced chemical equations.
Class experiment:
Carry out acid / base reactions with metal oxides.
Q/A: make deductions from the results.
Writing and balancing relevant equations.

Ammonia gas,
Methylbenzene.
2M Nitric acid
2M NaOH,
HNO3.
Amphoteric oxides.

K.L.B. BK IV
Pages 11-12
K.L.B. BK IV
Pages 12-14

ACIDS, BASES AND SALTS.

Precipitation Reactions.

By the end of the lesson, the learner should be able to:
Define a precipitate.
Write ionic equations showing formation of precipitates.

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.

Soluble carbonates e.g. Na2CO3, K2CO3, (NH4)2CO3
Salt solutions containing Mg2+, Al3+, Ca2+, etc.

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

ACIDS, BASES AND SALTS.

Solubility of chlorides sulphites and sulphates.

By the end of the lesson, the learner should be able to:
Find out cations that form (in)soluble chlorides, sulphates and sulphites.

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.

0.1M solution containing Pb2+, 2M NaCl solution, 2M sodium sulphate, source of heating.

K.L.B. BK IV
Pages 16-17

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
K.L.B. BK IV
Pages 20-21

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.

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

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.

Experiments involving solubility of KClO3 at different temperatures.
Note temperatures at which crystallization occurs.
Oral questions and discussion.

KClO3 thermometers, source of heat.

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

ACIDS, BASES AND SALTS.

Effect of temperature on solubility of a solute in a solvent.
Effects of various salts on soap.

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.

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.

KClO3 thermometers, source of heat.
distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+.

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

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

Removal of hardness of water.
Endothermic and Exothermic Reactions.
Energy level diagrams.

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

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.

student book
Ammonium nitrate,
Sodium hydroxide, thermometers.
student book

K.L.B. BK IV
Pages 27-29
K.L.B. BK IV
Pages 32-33

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

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

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.
Molar heat of solution of H2SO4.

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

Dissolve known masses of ammonia nitrate / sodium hydroxide in known volumes of water.
Determine temperature changes.
Calculate molar heat of solution. Supervised practice.


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.

Ammonia nitrate / sodium hydroxide, thermometers.
Conc. H2SO4, thermometers.

K.L.B. BK IV
Pages 40-41
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 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.

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.

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.

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 54-56

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Hess?s Law.

By the end of the lesson, the learner should be able to:
State Hess?s law.

Solve problems related to Hess?s law.

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.

student book

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

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Heat of solution hydration energy and lattice energy.

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.

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 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 concentration on rate of a 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.






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

Q/A & open discussion.
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.

student book
Portions of 2M HCl diluted with different volumes of water,
Stopwatches.

K.L.B. BK IV
Pages 67-68
K.L.B. BK IV
Pages 73-74

RATES OF REACTION & REVERSIBLE REACTIONS.

Effect of time of reaction on the rate of reaction.

By the end of the lesson, the learner should be able to:
Explain how the rate or reaction changes as the reaction proceed

Group experiments: investigate volume of gas evolved when magnesium reacts with dilute HCl.
Collect evolved gas and sketch and illustrative graphs.
Discuss the results.

Magnesium ribbons, stopwatches, conical flask.
100cm3 0.5M HCl, syringes, stoppers, tubes and connectors.

K.L.B. BK IV
Pages 75-79