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| WK | LSN | TOPIC | SUB-TOPIC | OBJECTIVES | T/L ACTIVITIES | T/L AIDS | REFERENCE | REMARKS |
|---|---|---|---|---|---|---|---|---|
| 1 | 1 |
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
|
Endothermic and Exothermic Reactions.
|
By the end of the
lesson, the learner
should be able to:
To differentiate 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. |
K.L.B. BK IV
Pages 32-33 |
|
| 1 | 2 |
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
|
Energy level diagrams.
|
By the end of the
lesson, the learner
should be able to:
Represent endothermic reactions with exothermic reactions with energy level diagrams. |
Probing questions on relative energies of reactants and products in endothermic and exothermic and endothermic reactions.
|
student book
|
K.L.B. BK IV
Pages 33-35 |
|
| 1 | 3 |
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 |
|
| 1 | 4-5 |
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 |
|
| 2 | 1 |
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 |
|
| 2 | 2 |
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 |
|
| 2 | 3 |
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 |
|
| 2 | 4-5 |
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
|
Molar heat of solution of H2SO4.
Enthalpy of combustion. Enthalpy of combustion. |
By the end of the
lesson, the learner
should be able to:
Determine molar heat of solution of H2SO4. Define the term enthalpy of combustion. Determine the enthalpy of combustion of ethanol. Explain why actual heats of combustion are usually lower than the theoretical values. |
Dissolve some known volume of conc. H2SO4 in a given volume of water.
Note the change in temperature. Work out the molar heat of solution of H2SO4. Group experiments / teacher demonstration. Obtain and record results. Work out calculations. |
Conc. H2SO4, thermometers.
Ethanol, distilled water, thermometer, clear wick, tripod stand and wire gauze. |
K.L.B. BK IV
Pages 42-45 K.L.B. BK IV Pages 45-48 |
|
| 3 | 1 |
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 |
|
| 3 | 2 |
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 |
|
| 3 | 3 |
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 |
|
| 3 | 4-5 |
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
|
Molar heat of solution of neutralization.
|
By the end of the
lesson, the learner
should be able to:
Define the term neutralization. Determine the molar heat of neutralization of HCl with NaOH. |
Class experiments:
Neutralize 2M HCl of known volume with a determined volume of 1M / 2M sodium hydroxide. Note highest temperature of the solution. Work out the molar heat of neutralization. Solve other related problems. Assignment. |
2M HCl of known volume, 1M / 2M sodium hydroxide.
|
K.L.B. BK IV
Pages 50-53 |
|
| 4 | 1 |
ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
|
Standard enthalpy changes.
|
By the end of the
lesson, the learner
should be able to:
Define the term standard enthalpy change. Denote standard enthalpy change with the correct notation. |
Exposition & brief discussion.
|
student book
|
K.L.B. BK IV
Pages 54-56 |
|
| 4 | 2 |
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 |
|
| 4 | 3 |
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 |
|
| 4 | 4 |
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 |
|
| 4 | 4-5 |
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 |
|
| 5 |
Headstart exams |
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| 6 | 1 |
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 |
|
| 6 | 2 |
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 |
|
| 6 | 3 |
RATES OF REACTION & REVERSIBLE REACTIONS.
|
Effect of concentration on rate of a 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. |
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. |
Portions of 2M HCl diluted with different volumes of water,
Stopwatches. |
K.L.B. BK IV
Pages 73-74 |
|
| 6 | 4-5 |
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 K.L.B. BK IV Pages 75-79 |
|
| 7 |
Midterm exams |
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| 8 |
Midterm break |
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| 9 | 1 |
RATES OF REACTION & REVERSIBLE REACTIONS.
|
Effect of temperature of reactants on rate of reaction.
|
By the end of the
lesson, the learner
should be able to:
Explain the effect of temperature on rate of reaction. |
Group experiments: investigate the effects of temperature on the rate of reaction of sodium thiosulphate with dilute HCl.
Sketch and interpret relevant graphs. Discuss the collision theory and effects of activation energy. |
Sodium thiosulphate heated at different temperatures, dilute HCl, stopwatches.
Graph papers. |
K.L.B. BK IV
Pages 80-83 |
|
| 9 | 2 |
RATES OF REACTION & REVERSIBLE REACTIONS.
|
Effect of change in surface area of reactants on the rate of a reaction.
|
By the end of the
lesson, the learner
should be able to:
Explain the effect of change in surface area on the rate of a reaction. |
Group experiment/ teacher demonstration.
Compare reactions of marble chips with dilute HCl and that of marble chips powder with equally diluted HCl. Collect evolved gas in each case. Teacher asks probing questions related to the observations made. |
Marble chips, marble chips powder, syringes, conical flasks with stoppers, 1M HCl.
|
K.L.B. BK IV
Pages 83-85 |
|
| 9 | 3 |
RATES OF REACTION & REVERSIBLE REACTIONS.
|
Effect of a suitable catalyst on the rate of a reaction
|
By the end of the
lesson, the learner
should be able to:
Explain effects of a suitable catalyst on the rate of a reaction. |
Teacher demonstration: preparation and collection of oxygen gas without using a catalyst, then using manganese (IV) oxide as a catalyst.
Explain the results in terms of activation energy. |
Hydrogen peroxide, manganese (IV) oxide.
|
K.L.B. BK IV
Pages 85-88 |
|
| 9 | 4-5 |
RATES OF REACTION & REVERSIBLE REACTIONS.
|
Effect of light on rate of specific reactions.
Reversible reactions. |
By the end of the
lesson, the learner
should be able to:
Identify reactions that are affected by light. Write down equations for reversible reactions. |
Teacher demonstration: decomposition of silver bromide in the presence of light.
Mention other examples of reactions affected by light. Q/A: review temporary and permanent changes. Teacher demonstration: heating crystals of hydrated copper (II) sulphate, then ?hydrating? them. Write the corresponding chemical equations. Give further examples of reversible reactions. |
Silver bromide.
Crystals of hydrated copper (II) sulphate. |
K.L.B. BK IV
Pages 89-91 K.L.B. BK IV Pages 91-93 |
|
| 10 | 1 |
RATES OF REACTION & REVERSIBLE REACTIONS.
|
State of equilibrium in chemical reactions.
|
By the end of the
lesson, the learner
should be able to:
Define the term equilibrium as used in reversible reactions. Write down equations of reversible reactions in a state of equilibrium. |
Brief discussion, giving examples of chemical equations for reversible reactions.
|
student book
|
K.L.B. BK IV
Pages 94-95 |
|
| 10 | 2 |
RATES OF REACTION & REVERSIBLE REACTIONS.
|
Le Chatelier?s Principle.
|
By the end of the
lesson, the learner
should be able to:
State Le Chatelier?s Principle. |
Investigate the effect of change of concentration of reactants on equilibrium.
Add 2M sodium hydroxide in steps to bromine water. Make and record observations. Discuss the results leading to Le Chatelier?s Principle. |
Add 2M sodium hydroxide,
|
K.L.B. BK IV
Pages 95-97 |
|
| 10 | 3 |
RATES OF REACTION & REVERSIBLE REACTIONS.
|
Effect of change of pressure and temperature on equilibrium shift.
|
By the end of the
lesson, the learner
should be able to:
Explain the effect of change of pressure & te,perature on equilibrium shift. |
Q/A: review kinetic theory of matter.
Q/A & discussion on effect of change of pressure / temperature on shifting of equilibrium; giving specific examples of chemical equations. Written assignment. |
student book
|
K.L.B. BK IV
Pages 97-101 |
|
| 10 | 4-5 |
RATES OF REACTION & REVERSIBLE REACTIONS.
|
The Haber Process.
The Contact Process. |
By the end of the
lesson, the learner
should be able to:
Explain the concept optimum conditions of a chemical equilibrium. Explain factors that change the position of equilibrium of the Harber process. Explain how change of temperature and pressure affect rate of manufacture of sulphur (VI) acid. |
Q/A and detailed discussion on change of pressure, temperature, concentration of ammonia and effect of presence of a suitable catalyst on the Haber process.
Probing questions and brief discussion. Assignment. |
student book
|
K.L.B. BK IV
Pages 102-103 K.L.B. BK IV Pages 103-104 |
|
| 11 |
End term exams |
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