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WK | LSN | TOPIC | SUB-TOPIC | OBJECTIVES | T/L ACTIVITIES | T/L AIDS | REFERENCE | REMARKS |
---|---|---|---|---|---|---|---|---|
2 | 1-2 |
NITROGEN & ITS COMPOUNDS.
|
Isolation of nitrogen from air.
Industrial production of nitrogen. Lab. preparation of nitrogen. Physical and chemical properties of nitrogen. Uses of nitrogen. |
By the end of the
lesson, the learner
should be able to:
Describe isolation of nitrogen from air. Describe industrial production of nitrogen. Describe lab preparation of nitrogen. State physical and chemical properties of nitrogen. List down uses of nitrogen. |
Teacher demonstration, explanations and equations. Discussion and description. Drawing schematic diagram for the process. Teacher demonstration: Students? record observations made from tests on the gas. Writing equations of reactions. Discussion and writing equations. |
Aspirator, copper turnings, gas jar, combustion tube, trogh.
charts Ammonium chloride, sodium nitrate |
K.L.B. BK III
PP. 134-135 Longhorn Book P 186 K.L.B. BK III PP.135-136 Longhorn Book PP 188-9 |
|
2 | 3 |
NITROGEN & ITS COMPOUNDS.
|
Nitrogen (I) oxide.
Lab preparation.
Properties and uses of Nitrogen (I) oxide. Nitrogen (II) oxide. Lab preparation. |
By the end of the
lesson, the learner
should be able to:
To describe Nitrogen (I) oxide. To list down physical properties of nitrogen (I) oxide. To describe chemical properties of nitrogen (I) oxide. To list down uses of nitrogen (I) oxide. To describe lab preparation of nitrogen (II) oxide. |
Teacher demonstration: -
Carry out tests on the gas. Students record observations in a table. Guided discussion. Q/A: Deductions from tests carried out. Discussion of chemical properties and writing of equations. Teacher elucidates uses of nitrogen (1) oxide. Class experiment: Preparation and carrying out tests on the gas. Observations recorded in a table. |
Ammonium nitrate.
charts Dil nitric acid, copper turnings. |
K.L.B. BK III
PP. 139-141 Longhorn Book III PP 195-6 |
|
2 | 4 |
NITROGEN & ITS COMPOUNDS.
|
Properties of the gas.
Nitrogen (1V) oxide Lab preparation. Properties of Nitrogen (IV) oxide. |
By the end of the
lesson, the learner
should be able to:
To list down physical properties of nitrogen (II) oxide To describe chemical properties of nitrogen (11) oxide To describe nitrogen (IV) oxide lab preparation. To list down physical properties of nitrogen (IV) oxide To describe chemical properties of nitrogen (IV) oxide To state uses of nitrogen (1V) oxide. |
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. Deduce physical properties from the table of observations. To describe chemical properties from the table of observations. Discuss uses of nitrogen (1V) oxide. |
charts
Conc. nitric acid, copper turnings. |
K.L.B.
BK III P. 143 Longhorn Book III PP 192-200 |
|
2 | 5 |
NITROGEN & ITS COMPOUNDS.
|
Ammonia.
Lab preparation of ammonia.
Properties of ammonia. Solubility of ammonia. |
By the end of the
lesson, the learner
should be able to:
To describe lab preparation of ammonia To list down physical properties of ammonia. To describe an experiment to determine solubility of ammonia. |
Q/A: Structure of ammonia.
Group experiments: Preparation of ammonia. Tests on the gas. Deduce physical properties from the observations above. Discuss chemical properties from the observations above. Write down chemical equations. Teacher demonstration. Discussion. |
Ca(OH)2, NH4Cl Solutions, CaO, litmus papers..M THREE CHEMISTRY TERM TWO 20....
charts |
K.L.B. BK III
PP. 147-148 |
|
3 | 1-2 |
NITROGEN & ITS COMPOUNDS.
|
Reaction of ammonia with metal ions.
Ionic equations of above reactions. Burning ammonia in the air. Reaction of ammonia with copper (II) Oxide. Haber process. Uses of ammonia. |
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. To name products formed when ammonia reacts with hot CuCl2 solid. To explain reducing properties of ammonia. 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. To list down uses of ammonia. To list down nitrogenous fertilizers. |
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. Teacher demonstration and discussion. Write down equations for the reactions. Discussion and explanations. Teacher elucidates uses of ammonia and nitrogenous fertilizers. |
2 cm Solutions containing various metal ions.
charts Conc. Ammonium solution Hot platinum rod Oxygen. Granular CuCl2 Combustion tube, Dry ammonia U-tube Gas jar. Chart- schematic diagram. charts |
K.L.B. BK III PP. 152-153 K.L.B. BK III P. 158 |
|
3 | 3 |
NITROGEN & ITS COMPOUNDS.
|
Nitric acid.
Lab preparation.
Nitric acid Industrial manufacture. |
By the end of the
lesson, the learner
should be able to:
To describe lab preparation of nitric acid. To describe industrial manufacture of nitric acid. |
Teacher demonstration.
Write equations of reaction. Discussion. Discussion and writing equations. |
Retort stand
Conc. H2SO4 KNO3 Chart Schematic diagram. |
K.L.B. BK III
P. 163 |
|
3 | 4 |
NITROGEN & ITS COMPOUNDS.
|
Reaction of dilute Nitric acid with metals.
Nitric acid and carbonates. 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:
To describe reaction of dilute nitric acid with metals. To write equations of reactions of dilute nitric acid with metals. To describe action of nitric acid on carbonates and hydrogen carbonates. Write equations for reaction of dil. nitric acid with hydrogen carbonates. Predict results of reacting dilute nitric acid with metal hydroxides and oxides. |
Class experiment:- making observations and recording them in a table.
Discuss the observations. Write down equations for the reactions. Group experiments: - Action of Nitric acid on hydrogen carbonates. Discussion and corresponding equations. Group experiments & writing equations for the reactions. |
Magnesium
Zinc Copper Solutions of Na2CO3 NaHCO3 ZnCO3 CuCO3 Metal hydroxides. |
K.L.B. BK III
PP. 165-166 Longhorn Book III PP 166-8 |
|
3 | 5 |
NITROGEN & ITS COMPOUNDS.
|
Reaction of nitric acid as an oxidizing agent.
Uses of nitric acid & nitrates. |
By the end of the
lesson, the learner
should be able to:
Describe reactions of nitric acid as an oxidizing agent. To state uses of nitrates. To describe preparation of nitrates. |
Class experiments: -
Explain observations made. Discussion Equations for the reactions for preparation of nitrates. |
Nitric acid acidified iron sulphate, sulphur, and copper metal.
charts |
K.L.B. BK III
PP. 169-170 Longhorn Book III PP 239 -240 |
|
4 | 1-2 |
NITROGEN & ITS COMPOUNDS.
NITROGEN & ITS COMPOUNDS. SULPHUR AND ITS COMPOUNDS SULPHUR AND ITS COMPOUNDS |
Action of heat on nitrates.
Test for nitrates. Nitrogen compounds and the environment. Extraction of sulphur. Allotropes of sulphur. |
By the end of the
lesson, the learner
should be able to:
To write equations of decomposition of nitrates on heating. To carry out tests on nitrates. To explain the pollution of nitrogen compounds in the environment. To state ways of reducing environmental pollution by nitrogen compounds. To describe extraction of sulphur by Frasch process. To identify allotropes of sulphur. To describe preparation of allotropes of sulphur. |
Discuss above observations.
Write relevant equations. Class experiments. Make observations and deductions. Discuss the brown ring test for nitrates. Brief guided discussion. Illustrate and discuss extraction of sulphur. Discussion and exposition of new concepts. |
charts
charts Chart-the Frasch process. video |
K.L.B. BK III
P 172 K.L.B.BK III PP. 173-174 Longhorn Book III PP 244-6 |
|
4 | 3 |
SULPHUR AND ITS COMPOUNDS
|
Physical properties of sulphur.
Heating of sulphur.
Chemical properties of sulphur. Uses of sulphur. Sulphur dioxide. |
By the end of the
lesson, the learner
should be able to:
To list physical properties of sulphur. To describe effects of heat on sulphur. To investigate and describe chemical properties of sulphur. State uses of sulphur. Describe lab. preparation of sulphur dioxide. |
Class experiment:
Solubility of sulphur in water, benzene, e.t.c,. Class experiments: Heating sulphur gently then strongly. Discuss the observations. Group experiments. Discuss observations. Write corresponding equations. Teacher elucidates uses of sulphur. Teacher demonstration:- Preparation of sulphur dioxide in a fume chamber/in the open. Carrying out tests on the gas. |
charts
|
K.L.B. BK III
P.184 Longhorn I Book III PP 253-255 |
|
4 | 4 |
SULPHUR AND ITS COMPOUNDS
|
Physical properties of sulphur dioxide.
Acidic properties of SO2. |
By the end of the
lesson, the learner
should be able to:
To list down physical properties of sulphur dioxide. To carry out experiments to determine acidic properties of SO2. |
Discuss the above tests.
Teacher demonstration to verify acidic properties of sulphur dioxide. Write equations. |
text book
textbook |
K.L.B.BK III
PP 193 Longhorn Book III PP 262-3 |
|
4 | 5 |
SULPHUR AND ITS COMPOUNDS
|
Reducing action of SO2.
Bleaching properties of SO2. Oxidizing action of SO2. |
By the end of the
lesson, the learner
should be able to:
To verify reducing action of SO2. To carry out experiments to determine bleaching properties of SO2. To explain Oxidizing action of SO2. |
Class experiments: make observations and draw conclusions.
Write balanced corresponding equations. Discuss the observations made above. Write corresponding equations. Q/A: review redox reactions. Teacher demonstration: - Lowering magnesium into a jar of SO2; effect of SO2 on hydrogen sulphide. Discuss observations. Write equations for the reactions. |
Experimental worksheets.
Burning magnesium. Hydrogen sulphide. |
K.L.B.BK III
P. 195 |
|
5 | 1-2 |
SULPHUR AND ITS COMPOUNDS
|
Sulphate and sulphite ions.
Uses of SO2.
Sulphuric acid. Contact process of manufacture. Properties of conc. H2SO4. Physical properties of sulphuric acid. Chemical properties of Sulphuric acid. |
By the end of the
lesson, the learner
should be able to:
To carry out tests for Sulphate and sulphite ions. State uses of SO2. To identify raw materials for manufacture of sulphuric acid. To describe the contact process. Describe properties of conc. H2SO4. To dilute conc. sulphuric acid. State physical properties of sulphuric acid. To write equations to show that conc. sulphuric acid is a drying and dehydrating agent. To describe reactions of dilute H2SO4 with metals. |
Class experiments.
Make deductions from the observations made. Write (ionic) equations for the reactions. Teacher elucidates uses of SO2. Discussion using schematic flow charts. Writing equations. Discuss above observations. Write relevant equations. Teacher demonstration ? diluting conc. sulphuric acid. Discuss use of conc. sulphuric acid as a drying and dehydrating agent. Discussion and explanations. Group expts. ? reaction of metals with dilute H2SO4, make observations and relevant deductions; writing corresponding equations. |
Sodium sulphate
Barium chloride Barium nitrate. Chart-schematic Flow charts. charts Conc. sulphuric acid. Magnesium, zinc, copper metals. |
K.L.B.
BK III P. 200 Longhorn Book III PP 268-9 K.L.B. BK III P. 205 Longhorn Book III PP 274-5 |
|
5 | 3 |
SULPHUR AND ITS COMPOUNDS
|
Dilute H2SO4, carbonates and hydrogen carbonates.
Dilute H2SO4, and metal oxides and hydroxides. |
By the end of the
lesson, the learner
should be able to:
To describe reaction of dilute H2SO4 with carbonates and hydrogen carbonates. To investigate reaction of dilute H2SO4 with metal oxides and hydroxides. |
Discussion, writing relevant equations.
Class expts. Observing colour changes. |
charts
Oxides of magnesium, zinc, copper. NaOH Solution. |
K.L.B. BK III P. 208 |
|
5 | 4 |
SULPHUR AND ITS COMPOUNDS
|
Dilute H2SO4 and metal oxides & hydroxides.
Hydrogen sulphide. Preparation of the gas. Reaction of the gas with oxygen. |
By the end of the
lesson, the learner
should be able to:
To explain reactions of dilute H2SO4 with metal oxides and hydroxides. To describe preparation of hydrogen sulphide. To state properties of the gas. |
Discussion, writing relevant chemical equations.
Theoretical / descriptive approach. Writing corresponding equations. Discuss physical properties of the gas and reaction of the gas with oxygen. |
charts
|
K.L.B. BK III P. 211 |
|
5 | 5 |
SULPHUR AND ITS COMPOUNDS
CHLORINE & ITS COMPOUNDS |
Reaction of the gas with water.
Reducing properties of the gas.
Sulphur and its effects on the environment. Lab. preparation of chlorine gas. |
By the end of the
lesson, the learner
should be able to:
To write equations for reaction of the gas with water. To demonstrate reducing properties of the gas. To explain environmental pollution caused by sulphur and its compounds. Describe laboratory preparation of chlorine gas. |
Writing chemical equations for the reactions.
Discussion and explanation. Teacher demonstration ? gas prep. tests on the gas. |
charts
Conc. HCl, Manganese (IV) oxide. |
K.L.B.
BK III P. 212. Longhorn Book III PP 291-2 |
|
6 | 1-2 |
CHLORINE & ITS COMPOUNDS
|
Physical properties of chlorine.
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:
State physical properties of chlorine. 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. |
Q/A: Relate the properties to the method of collection of the gas.
Write equations for the reaction leading to formation of chlorine. Teacher demonstration: Writing chemical equations. Teacher demonstration: Discussion. Writing chemical equations. Group experiments. Discuss and explain observations made. Write corresponding chemical equations. |
charts
Moist blue litmus papers. textbook Expt. Worksheets. |
K.L.B.BK III
P. 220. Longhorn Book III P 301 K.L.B.BK III PP. 224 -225 Longhorn Book III PP 303-5 |
|
6 | 3 |
CHLORINE & ITS COMPOUNDS
|
Chlorine and alkalis.
Test for chlorides. Uses of chlorine gas. |
By the end of the
lesson, the learner
should be able to:
To investigate and explain reaction of chlorine with alkalis. To carry out tests for chlorides. To state uses of chlorine. |
Teacher demonstration: Bubbling chlorine with dilute cold / hot NaOH solution.
Make observations and account for them. Class expts. Discuss observations, results. Write chemical equations for the reactions. Teacher elucidates uses of chlorine. |
Cold / hot NaOH solutions.
Expt. Worksheets. Zinc chloride, litmus paper, conc. Sulphuric acid. |
K.L.B.BK III
P. 228 Longhorn Book III PP 313-4 |
|
6 | 4 |
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 |
|
6 | 5 |
CHLORINE & ITS COMPOUNDS
|
Further chemical properties of hydrogen chloride gas.
Large-scale production 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. |
Class experiment leading to deduction of further chemical properties of hydrogen chloride gas / confirmatory test for hydrogen chloride gas.
Discussion and giving relevant equations. |
Ammonia solution.
charts |
K.L.B. BK III
PP. 235 -223 Longhorn Book III PP 327-331 |
|
7 | 1-2 |
CHLORINE & ITS COMPOUNDS
ACIDS, BASES AND SALTS. |
Uses of hydrochloric acid.
Effects of hydrochloric acid on the environment. Strength of acids. Acids in aqueous form. 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:
To state uses of hydrochloric acid. To explain effects of hydrochloric acid on the environment. Define an acid in terms of hydrogen ions. Explain strength of acids in aqueous form in terms of number of hydrogen ions present. 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. |
Brief discussion.
Discussion and explanation. 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. 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. |
charts
Magnesium strip, zinc carbonate, 2M HCl, 2M H2SO4, 2M ethanoic acid. 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 III
P. 237 Longhorn Book III P 331-3 K.L.B. BK IV Pages 4-6 |
|
7 | 3 |
ACIDS, BASES AND SALTS.
|
Neutralization reaction.
Strength of bases. |
By the end of the
lesson, the learner
should be able to:
Determine the results of reaction of an acid and a base. Compare strengths of bases using pH values and electrical conductivity. Classify bases/ alkali as either strong or weak in terms of complete / partial ionization. |
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. 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. |
1M HCl,
Calcium hydroxide, universal indicator. 2M NaOH, 2M ammonia solution, universal indicator solutions, dry cells, carbon electrodes, milliammeters, wires, switches etc |
K.L.B. BK IV
Page 7 |
|
7 | 4 |
ACIDS, BASES AND SALTS.
|
Dissolving hydrogen chloride gas in water / methylbenzene.
Dissolving ammonia gas in water/ methylbenzene. Amphoteric oxides. |
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. Define an amphoteric oxide. Identify some amphoteric oxides. |
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. 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, hydrogen chloride gas. Methylbenzene. 2M Nitric acid 2M NaOH, HNO3. Amphoteric oxides. |
K.L.B. BK IV
Pages 9-11 |
|
7 | 5 |
ACIDS, BASES AND SALTS.
|
Precipitation Reactions.
Solubility of chlorides sulphites and sulphates. |
By the end of the
lesson, the learner
should be able to:
Define a precipitate. Write ionic equations showing formation of precipitates. Find out cations that form (in)soluble chlorides, sulphates and sulphites. |
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. |
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 14-16 |
|
8 |
Midterm |
|||||||
9 | 1-2 |
ACIDS, BASES AND SALTS.
|
Equations for formation of insoluble chlorides, sulphites and sulphates.
Complex ions. Solubility of a salt at a given temperature. Problems solving on solubility. |
By the end of the
lesson, the learner
should be able to:
Write down equations for formation of insoluble chlorides, sulphites and sulphates. Explain formation of complex ions. Define the term solubility. Determine solubility of a given salt at room temperature. Solve problems involving solubility of a solute in a solvent at a given temperature. |
Q/A: review observations made in the above experiments.
Discuss the solubility of the cations. Write relevant ionic equations. 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. Worked examples. Supervised practice. Written assignment. |
student book
2M Sodium hydroxide (2M ammonia solution), solution containing Mg2+, Zn2+, etc. Suitable solutes. Evaporating dish, watch glass, heating source, thermometer. |
K.L.B. BK IV
Pages 17-18 K.L.B. BK IV Pages 20-21 |
|
9 | 3 |
ACIDS, BASES AND SALTS.
|
Effect of temperature on solubility of a solute in a solvent.
Effects of various salts on soap. Removal of hardness of water. |
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. |
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. |
KClO3 thermometers, source of heat.
distilled water, tap water, rainwater, dilute solution of sodium chloride and solutions containing Ca2+ and Zn2+. student book |
K.L.B. BK IV
Pages 22-25 |
|
9 | 4 |
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
|
Endothermic and Exothermic Reactions.
Energy level diagrams. |
By the end of the
lesson, the learner
should be able to:
To differentiate between endothermic & exothermic reactions. Represent endothermic reactions with exothermic reactions with energy level diagrams. |
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. |
Ammonium nitrate,
Sodium hydroxide, thermometers. student book |
K.L.B. BK IV
Pages 32-33 |
|
9 | 5 |
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
|
Enthalpy Notation.
Change of state.
CAT |
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 |
|
10 | 1-2 |
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
|
Molar heat of solution.
Molar heat of solution of H2SO4. Enthalpy of combustion. Enthalpy of combustion. Molar heat of displacement of ions. |
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. 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. Define the term molar heat of solution of displacement of ions. Determine the molar heat of solution of displacement of ions. |
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. Group experiments / teacher demonstration. Obtain and record results. Work out calculations. 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. |
Ammonia nitrate / sodium hydroxide, thermometers.
Conc. H2SO4, thermometers. Ethanol, distilled water, thermometer, clear wick, tripod stand and wire gauze. Zinc, iron, magnesium, copper sulphate solution. |
K.L.B. BK IV
Pages 40-41 K.L.B. BK IV Pages 45-48 |
|
10 | 3 |
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 |
|
10 | 4 |
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. Assignment. |
student book
|
K.L.B. BK IV
Pages 56-57 |
|
10 | 5 |
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
RATES OF REACTION & REVERSIBLE REACTIONS. RATES OF REACTION & REVERSIBLE REACTIONS. |
Heat values of fuels.
Environmental effects of fuels. 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:
Define the term fuel. Describe energy changes when a fuel undergoes combustion. Outline factors considered when choosing a suitable fuel. 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. Explain how the rate or reaction changes as the reaction proceed |
Probing questions and brief discussion.
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. Group experiments: investigate volume of gas evolved when magnesium reacts with dilute HCl. Collect evolved gas and sketch and illustrative graphs. Discuss the results. |
student book
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 64-66 |
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