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| WK | LSN | TOPIC | SUB-TOPIC | OBJECTIVES | T/L ACTIVITIES | T/L AIDS | REFERENCE | REMARKS |
|---|---|---|---|---|---|---|---|---|
| 1 |
REPORTING TO SCHOOL FOR TERM II |
|||||||
| 2 | 1 |
THE MOLE
|
Concentration and Molarity of Solutions
|
By the end of the
lesson, the learner
should be able to:
Define concentration and molarity of solutions Calculate molarity from mass and volume data Convert between different concentration units Apply molarity calculations to various solutions |
Teacher exposition: Definition of molarity (moles/dm³). Worked examples: Calculate molarity from mass of solute and volume. Convert between g/dm³ and mol/dm³. Practice problems: Various salt solutions and their molarities.
|
Scientific calculators, Molarity charts, Various salt samples for demonstration
|
KLB Secondary Chemistry Form 3, Pages 41-43
|
|
| 2 | 2 |
THE MOLE
|
Preparation of Molar Solutions
Dilution of Solutions |
By the end of the
lesson, the learner
should be able to:
Describe procedure for preparing molar solutions Use volumetric flasks correctly Calculate masses needed for specific molarities Prepare standard solutions accurately |
Experiment: Prepare 1M, 0.5M, and 0.25M NaOH solutions in different volumes. Use volumetric flasks of 1000cm³, 500cm³, and 250cm³. Calculate required masses. Demonstrate proper dissolution and dilution techniques.
|
Volumetric flasks (250, 500, 1000cm³), Sodium hydroxide pellets, Beam balance, Wash bottles, Beakers
Volumetric flasks, Hydrochloric acid (2M), Measuring cylinders, Pipettes, Safety equipment |
KLB Secondary Chemistry Form 3, Pages 43-46
|
|
| 2 |
OPENER EXAM |
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| 3 | 1 |
THE MOLE
|
Stoichiometry - Experimental Determination of Equations
|
By the end of the
lesson, the learner
should be able to:
Determine chemical equations from experimental data Calculate mole ratios from mass measurements Write balanced chemical equations Apply stoichiometry to displacement reactions |
Experiment: Iron displacement of copper from CuSO₄ solution. Measure masses of iron used and copper displaced. Calculate mole ratios. Derive balanced chemical equation. Discuss spectator ions.
|
Iron filings, Copper(II) sulphate solution, Beam balance, Beakers, Filter equipment
|
KLB Secondary Chemistry Form 3, Pages 50-53
|
|
| 3 | 2 |
THE MOLE
|
Stoichiometry - Precipitation Reactions
|
By the end of the
lesson, the learner
should be able to:
Investigate stoichiometry of precipitation reactions Determine mole ratios from volume measurements Write ionic equations for precipitation Analyze limiting and excess reagents |
Experiment: Pb(NO₃)₂ + KI precipitation reaction. Use different volumes to determine stoichiometry. Measure precipitate heights. Plot graphs to find reaction ratios. Identify limiting reagents.
|
Test tubes, Lead(II) nitrate solution, Potassium iodide solution, Burettes, Ethanol, Rulers
|
KLB Secondary Chemistry Form 3, Pages 53-56
|
|
| 3 | 3-4 |
THE MOLE
|
Stoichiometry - Gas Evolution Reactions
Volumetric Analysis - Introduction and Apparatus Titration - Acid-Base Neutralization |
By the end of the
lesson, the learner
should be able to:
Determine stoichiometry of gas-producing reactions Collect and measure gas volumes Calculate mole ratios involving gases Write equations for acid-carbonate reactions Define volumetric analysis and titration Identify and use titration apparatus correctly Explain functions of pipettes and burettes Demonstrate proper reading techniques |
Experiment: HCl + Na₂CO₃ reaction. Collect CO₂ gas in plastic bag. Measure gas mass and calculate moles. Determine mole ratios of reactants and products. Write balanced equation.
Practical session: Familiarization with pipettes and burettes. Practice filling and reading burettes accurately. Learn proper meniscus reading. Use pipette fillers safely. Rinse apparatus with appropriate solutions. |
Conical flask, Thistle funnel, Plastic bags, Rubber bands, Sodium carbonate, HCl solution
Pipettes (10, 20, 25cm³), Burettes (50cm³), Pipette fillers, Conical flasks, Various solutions Burettes, Pipettes, 0.1M NaOH, 0.1M HCl, Phenolphthalein indicator, Conical flasks |
KLB Secondary Chemistry Form 3, Pages 56-58
KLB Secondary Chemistry Form 3, Pages 58-59 |
|
| 3 | 5 |
THE MOLE
|
Titration - Diprotic Acids
|
By the end of the
lesson, the learner
should be able to:
Investigate titrations involving diprotic acids Determine basicity of acids from titration data Compare volumes needed for mono- and diprotic acids Write equations for diprotic acid reactions |
Experiment: Titrate 25cm³ of 0.1M NaOH with 0.1M H₂SO₄. Compare volume used with previous HCl titration. Calculate mole ratios. Explain concept of basicity. Introduce dibasic and tribasic acids.
|
Burettes, Pipettes, 0.1M H₂SO₄, 0.1M NaOH, Phenolphthalein, Basicity reference chart
|
KLB Secondary Chemistry Form 3, Pages 62-65
|
|
| 3 | 6 |
THE MOLE
|
Standardization of Solutions
|
By the end of the
lesson, the learner
should be able to:
Define standardization process Standardize HCl using Na₂CO₃ as primary standard Calculate accurate concentrations from titration data Understand importance of primary standards |
Experiment: Prepare approximately 0.1M HCl and standardize using accurately weighed Na₂CO₃. Use methyl orange indicator. Calculate exact molarity from titration results. Discuss primary standard requirements.
|
Anhydrous Na₂CO₃, Approximately 0.1M HCl, Methyl orange, Volumetric flasks, Analytical balance
|
KLB Secondary Chemistry Form 3, Pages 65-67
|
|
| 4 | 1 |
THE MOLE
|
Back Titration Method
|
By the end of the
lesson, the learner
should be able to:
Understand principle of back titration Apply back titration to determine composition Calculate concentrations using back titration data Determine atomic masses from back titration |
Experiment: Determine atomic mass of divalent metal in MCO₃. Add excess HCl to carbonate, then titrate excess with NaOH. Calculate moles of acid that reacted with carbonate. Determine metal's atomic mass.
|
Metal carbonate sample, 0.5M HCl, 0M NaOH, Phenolphthalein, Conical flasks
|
KLB Secondary Chemistry Form 3, Pages 67-70
|
|
| 4 | 2 |
THE MOLE
|
Redox Titrations - Principles
Redox Titrations - KMnO₄ Standardization |
By the end of the
lesson, the learner
should be able to:
Explain principles of redox titrations Identify color changes in redox reactions Understand self-indicating nature of some redox reactions Write ionic equations for redox processes |
Teacher exposition: Redox titration principles. Demonstrate color changes: MnO₄⁻ (purple) → Mn²⁺ (colorless), Cr₂O₇²⁻ (orange) → Cr³⁺ (green). Discussion: Self-indicating reactions. Write half-equations and overall ionic equations.
|
Potassium manganate(VII), Potassium dichromate(VI), Iron(II) solutions, Color change charts
Iron(II) ammonium sulfate, KMnO₄ solution, Dilute H₂SO₄, Pipettes, Burettes |
KLB Secondary Chemistry Form 3, Pages 68-70
|
|
| 4 | 3-4 |
THE MOLE
|
Water of Crystallization Determination
Atomicity and Molar Gas Volume |
By the end of the
lesson, the learner
should be able to:
Determine water of crystallization in hydrated salts Use redox titration to find formula of hydrated salt Calculate value of 'n' in crystallization formulas Apply analytical data to determine complete formulas Define atomicity of gaseous elements Classify gases as monoatomic, diatomic, or triatomic Determine molar gas volume experimentally Calculate gas densities and molar masses |
Experiment: Determine 'n' in FeSO₄(NH₄)₂SO₄·nH₂O. Dissolve known mass in acid, titrate with standardized KMnO₄. Calculate moles of iron(II), hence complete formula. Compare theoretical and experimental values.
Experiment: Measure volumes and masses of different gases (O₂, CO₂, Cl₂). Calculate densities and molar masses. Determine volume occupied by one mole. Compare values at different conditions. |
Hydrated iron(II) salt, Standardized KMnO₄, Dilute H₂SO₄, Analytical balance
Gas syringes (50cm³), Various gases, Analytical balance, Gas supply apparatus |
KLB Secondary Chemistry Form 3, Pages 72-73
KLB Secondary Chemistry Form 3, Pages 73-75 |
|
| 4 | 5 |
THE MOLE
|
Combining Volumes of Gases - Experimental Investigation
|
By the end of the
lesson, the learner
should be able to:
Investigate Gay-Lussac's law experimentally Measure combining volumes of reacting gases Determine simple whole number ratios Write equations from volume relationships |
Experiment: React NH₃ and HCl gases in measured volumes. Observe formation of NH₄Cl solid. Measure residual gas volumes. Determine combining ratios. Apply to other gas reactions.
|
Gas syringes, Dry NH₃ generator, Dry HCl generator, Glass connecting tubes, Clips
|
KLB Secondary Chemistry Form 3, Pages 75-77
|
|
| 4 | 6 |
THE MOLE
NITROGEN AND ITS COMPOUNDS |
Gas Laws and Chemical Equations
Introduction to Nitrogen - Properties and Occurrence |
By the end of the
lesson, the learner
should be able to:
Apply Avogadro's law to chemical reactions Use volume ratios to determine chemical equations Calculate product volumes from reactant volumes Solve problems involving gas stoichiometry |
Worked examples: Use Gay-Lussac's law to determine equations. Calculate volumes of products from given reactant volumes. Apply Avogadro's law to find number of molecules. Practice: Complex gas stoichiometry problems.
|
Scientific calculators, Gas law charts, Volume ratio examples
Periodic table charts, Atmospheric composition diagrams, Molecular models showing N≡N triple bond |
KLB Secondary Chemistry Form 3, Pages 77-79
|
|
| 5 | 1 |
NITROGEN AND ITS COMPOUNDS
|
Isolation of Nitrogen from Air - Industrial and Laboratory Methods
|
By the end of the
lesson, the learner
should be able to:
Describe isolation of nitrogen from air Explain fractional distillation of liquid air Set up apparatus for laboratory isolation Identify impurities removed during isolation |
Experiment: Laboratory isolation using aspirator. Pass air through KOH solution to remove CO₂, then over heated copper to remove oxygen. Teacher demonstration: Fractional distillation principles. Flow chart study: Industrial nitrogen production steps.
|
Aspirator, KOH solution, Copper turnings, Heating apparatus, Fractional distillation flow chart
|
KLB Secondary Chemistry Form 3, Pages 119-121
|
|
| 5 | 2 |
NITROGEN AND ITS COMPOUNDS
|
Laboratory Preparation of Nitrogen Gas
|
By the end of the
lesson, the learner
should be able to:
Prepare nitrogen gas from ammonium compounds Use sodium nitrite and ammonium chloride method Test physical and chemical properties of nitrogen Write equations for nitrogen preparation |
Experiment: Mix sodium nitrite (7g) and ammonium chloride ( 5g) with water. Heat gently and collect gas over water. Tests: Color, smell, burning splint, litmus paper, lime water, burning Mg and S. Safety precautions during heating.
|
Sodium nitrite, Ammonium chloride, Round-bottomed flask, Gas collection apparatus, Test reagents, Deflagrating spoon
|
KLB Secondary Chemistry Form 3, Pages 121-123
|
|
| 5 | 3-4 |
NITROGEN AND ITS COMPOUNDS
|
Properties and Uses of Nitrogen Gas
Nitrogen(I) Oxide - Preparation and Properties Nitrogen(II) Oxide - Preparation and Properties |
By the end of the
lesson, the learner
should be able to:
Describe physical properties of nitrogen Explain chemical inertness of nitrogen Describe reactions at high temperatures List industrial uses of nitrogen Prepare nitrogen(I) oxide from ammonium nitrate Test physical and chemical properties Explain decomposition and oxidizing properties Describe uses of nitrogen(I) oxide |
Analysis of test results: Colorless, odorless, does not burn or support combustion. Discussion: Triple bond strength and chemical inertness. High temperature reactions with metals forming nitrides. Uses: Haber process, light bulbs, refrigerant, inert atmosphere.
Experiment: Heat ammonium nitrate carefully in test tube. Collect gas over warm water. Tests: Color, smell, glowing splint test, reaction with heated copper and sulfur. Safety: Stop heating while some solid remains to avoid explosion. |
Property summary charts, Uses of nitrogen displays, Industrial application diagrams
Ammonium nitrate, Test tubes, Gas collection apparatus, Copper turnings, Sulfur, Glowing splints Copper turnings, Dilute nitric acid, Gas collection apparatus, Iron(II) sulfate solution, Test reagents |
KLB Secondary Chemistry Form 3, Pages 121-123
KLB Secondary Chemistry Form 3, Pages 123-125 |
|
| 5 | 5 |
NITROGEN AND ITS COMPOUNDS
|
Nitrogen(IV) Oxide - Preparation and Properties
|
By the end of the
lesson, the learner
should be able to:
Prepare nitrogen(IV) oxide from copper and concentrated nitric acid Prepare from thermal decomposition of nitrates Test properties including equilibrium with N₂O₄ Describe reactions and uses |
Experiment: Add concentrated HNO₃ to copper turnings. Collect red-brown gas by downward delivery. Alternative: Heat lead(II) nitrate with cooling U-tube. Tests: Solubility, effect on litmus, burning elements, cooling/heating effects.
|
Copper turnings, Concentrated nitric acid, Lead(II) nitrate, Gas collection apparatus, U-tube with ice, Testing materials
|
KLB Secondary Chemistry Form 3, Pages 127-131
|
|
| 5 | 6 |
NITROGEN AND ITS COMPOUNDS
|
Comparison of Nitrogen Oxides and Environmental Effects
|
By the end of the
lesson, the learner
should be able to:
Compare preparation methods of nitrogen oxides Distinguish between different nitrogen oxides Explain formation in vehicle engines Describe environmental pollution effects |
Comparative study: Properties table of N₂O, NO, NO₂. Discussion: Formation in internal combustion engines. Environmental effects: Acid rain formation, smog, health problems. Worked examples: Distinguishing tests for each oxide.
|
Comparison charts, Environmental impact diagrams, Vehicle emission illustrations
|
KLB Secondary Chemistry Form 3, Pages 123-131
|
|
| 6 | 1 |
NITROGEN AND ITS COMPOUNDS
|
Laboratory Preparation of Ammonia
|
By the end of the
lesson, the learner
should be able to:
Prepare ammonia from ammonium salts and alkalis Set up apparatus with proper gas collection Test characteristic properties of ammonia Explain displacement reaction principle |
Experiment: Heat mixture of calcium hydroxide and ammonium chloride. Collect gas by upward delivery using calcium oxide as drying agent. Tests: Color, smell, combustion, HCl fumes test, litmus paper. Safety: Slanted flask position.
|
Calcium hydroxide, Ammonium chloride, Round-bottomed flask, Calcium oxide, HCl solution, Glass rod, Litmus paper
|
KLB Secondary Chemistry Form 3, Pages 131-134
|
|
| 6 | 2 |
NITROGEN AND ITS COMPOUNDS
|
Preparation of Aqueous Ammonia and Solubility
Reactions of Aqueous Ammonia with Metal Ions |
By the end of the
lesson, the learner
should be able to:
Prepare aqueous ammonia solution Demonstrate high solubility using fountain experiment Explain alkaline properties of aqueous ammonia Write equations for ammonia in water |
Experiment: Dissolve ammonia in water using inverted funnel method. Fountain experiment: Show partial vacuum formation due to high solubility. Tests: Effect on universal indicator, pH measurement. Theory: NH₃ + H₂O equilibrium.
|
Ammonia generation apparatus, Funnel, Universal indicator, Fountain apparatus, pH meter/paper
Various metal salt solutions, Aqueous ammonia, Test tubes, Droppers, Observation recording tables |
KLB Secondary Chemistry Form 3, Pages 134-136
|
|
| 6 | 3-4 |
NITROGEN AND ITS COMPOUNDS
|
Chemical Properties of Ammonia - Reactions with Acids and Combustion
Industrial Manufacture of Ammonia - The Haber Process |
By the end of the
lesson, the learner
should be able to:
Test neutralization reactions with acids Investigate combustion of ammonia Examine catalytic oxidation with platinum Study reducing properties with metal oxides Describe raw materials and their sources Explain optimum conditions for ammonia synthesis Draw flow diagram of Haber process Explain economic considerations and catalyst use |
Experiments: (a) Neutralize H₂SO₄, HCl, HNO₃ with aqueous ammonia using indicators. (b) Attempt combustion in air and oxygen. (c) Catalytic oxidation with heated platinum wire. (d) Reduction of CuO by ammonia. Record all observations.
Teacher exposition: N₂ from air, H₂ from natural gas/cracking. Process conditions: 500°C, 200 atm, iron catalyst. Flow diagram study: Purification, compression, catalytic chamber, separation, recycling. Economic factors: Compromise between yield and rate. |
Various dilute acids, Methyl orange, Oxygen supply, Platinum wire, Copper(II) oxide, Combustion apparatus, U-tube for collection
Haber process flow charts, Industrial diagrams, Catalyst samples, Economic analysis sheets |
KLB Secondary Chemistry Form 3, Pages 138-140
KLB Secondary Chemistry Form 3, Pages 140-141 |
|
| 6 | 5 |
NITROGEN AND ITS COMPOUNDS
|
Uses of Ammonia and Introduction to Nitrogenous Fertilizers
|
By the end of the
lesson, the learner
should be able to:
List major uses of ammonia Explain importance as fertilizer Calculate nitrogen percentages in fertilizers Compare different nitrogenous fertilizers |
Discussion: Uses - fertilizer, refrigerant, cleaning agent, hydrazine production. Introduction to fertilizers: Ammonium sulfate, ammonium nitrate, ammonium phosphate, urea, CAN. Calculations: Percentage nitrogen content in each fertilizer type.
|
Fertilizer samples, Percentage calculation worksheets, Use application charts, Calculator
|
KLB Secondary Chemistry Form 3, Pages 141-144
|
|
| 6 | 6 |
NITROGEN AND ITS COMPOUNDS
|
Nitrogenous Fertilizers - Types and Calculations
|
By the end of the
lesson, the learner
should be able to:
Calculate percentage nitrogen in various fertilizers Compare fertilizer effectiveness Prepare simple nitrogenous fertilizers Discuss environmental considerations |
Worked examples: Calculate % N in (NH₄)₂SO₄, NH₄NO₃, (NH₄)₃PO₄, CO(NH₂)₂, CAN. Comparison: Urea has highest nitrogen content. Practical: Prepare ammonium sulfate from ammonia and sulfuric acid. Environmental impact discussion.
|
Various fertilizer formulas, Scientific calculators, Laboratory preparation materials, Environmental impact data
|
KLB Secondary Chemistry Form 3, Pages 141-144
|
|
| 7 | 1 |
NITROGEN AND ITS COMPOUNDS
|
Laboratory Preparation of Nitric(V) Acid
Industrial Manufacture of Nitric(V) Acid |
By the end of the
lesson, the learner
should be able to:
Prepare nitric acid from nitrate and concentrated sulfuric acid Set up all-glass apparatus safely Explain brown fumes and yellow color Purify nitric acid by air bubbling |
Experiment: Heat mixture of KNO₃ and concentrated H₂SO₄ in all-glass apparatus. Collect yellow nitric acid. Explain brown fumes (NO₂) and yellow color. Bubble air through to remove dissolved NO₂. Safety: Gentle heating, fume cupboard.
|
Potassium nitrate, Concentrated sulfuric acid, All-glass apparatus, Condenser, Retort stand, Safety equipment
Industrial process flow charts, Catalyst samples, Process condition charts, Efficiency calculation sheets |
KLB Secondary Chemistry Form 3, Pages 144-145
|
|
| 7 | 2 |
NITROGEN AND ITS COMPOUNDS
|
Reactions of Dilute Nitric(V) Acid with Metals
|
By the end of the
lesson, the learner
should be able to:
Test reactions with various metals Explain absence of hydrogen gas production Observe formation of nitrogen oxides Write equations for metal-acid reactions |
Experiment: Add dilute HNO₃ to Mg, Zn, Cu. Test gases produced with burning splint. Observe that no H₂ is produced (except with Mg in very dilute acid). Explain oxidation of any H₂ formed to water. Record observations and write equations.
|
Various metals (Mg, Zn, Cu), Dilute nitric acid, Test tubes, Gas testing apparatus, Burning splints
|
KLB Secondary Chemistry Form 3, Pages 147-150
|
|
| 7 | 3-4 |
NITROGEN AND ITS COMPOUNDS
NITROGEN AND ITS COMPOUNDS SULPHUR AND ITS COMPOUNDS |
Reactions of Dilute Nitric(V) Acid with Carbonates and Hydroxides
Reactions of Concentrated Nitric(V) Acid - Oxidizing Properties Extraction of Sulphur |
By the end of the
lesson, the learner
should be able to:
Test reactions with carbonates and hydrogen carbonates Test neutralization with metal hydroxides and oxides Identify products formed Write balanced chemical equations Demonstrate strong oxidizing properties Test reactions with FeSO₄, sulfur, and copper Observe formation of nitrogen dioxide Explain electron transfer in oxidation |
Experiments: (a) Add dilute HNO₃ to Na₂CO₃, CaCO₃, ZnCO₃, CuCO₃, NaHCO₃. Test gas evolved with lime water. (b) Neutralize NaOH, CaO, CuO, PbO with dilute HNO₃. Record color changes and write equations.
Experiments: (a) Add concentrated HNO₃ to acidified FeSO₄ - observe color change. (b) Add to sulfur - observe reaction. (c) Add to copper turnings - observe vigorous reaction and brown fumes. Explain oxidizing power and reduction to NO₂. |
Various carbonates and hydroxides, Dilute nitric acid, Lime water, Universal indicator, Test tubes
Concentrated nitric acid, Iron(II) sulfate, Sulfur powder, Copper turnings, Test tubes, Fume cupboard access Charts showing periodic table, Diagram of Frasch process, Samples of sulphur compounds (pyrites, gypsum) |
KLB Secondary Chemistry Form 3, Pages 147-150
KLB Secondary Chemistry Form 3, Pages 150-151 |
|
| 7 | 5 |
SULPHUR AND ITS COMPOUNDS
|
Allotropes of Sulphur
Physical Properties of Sulphur - Solubility Physical Properties of Sulphur - Effect of Heat |
By the end of the
lesson, the learner
should be able to:
Define allotropy and allotropes. Prepare rhombic sulphur in the laboratory. Prepare monoclinic sulphur in the laboratory. Compare the properties of rhombic and monoclinic sulphur. |
Practical work: Experiment 1(a) - Preparation of rhombic sulphur using carbon(IV) sulphide. Practical work: Experiment 1(b) - Preparation of monoclinic sulphur by heating and cooling. Observation: Using hand lens to examine crystal shapes. Discussion: Compare crystal structures and transition temperature.
|
Powdered sulphur, Carbon(IV) sulphide, Evaporating dish, Glass rod, Hand lens, Boiling tubes, Filter paper, Beakers
Powdered sulphur, Water, Benzene, Methylbenzene, Carbon(IV) sulphide, Test tubes, Charts showing molecular structure Powdered sulphur, Test tubes, Bunsen burner, Cold surface for condensation, Thermometer, Safety equipment |
KLB Secondary Chemistry Form 4, Pages 161-163
|
|
| 7 | 6 |
SULPHUR AND ITS COMPOUNDS
|
Chemical Properties of Sulphur - Reactions with Elements
Chemical Properties of Sulphur - Reactions with Acids |
By the end of the
lesson, the learner
should be able to:
Investigate the reaction of sulphur with oxygen. Investigate the reaction of sulphur with metals. Write balanced equations for reactions of sulphur. Explain the formation of sulphides. |
Practical work: Experiment 3(a) - Burning sulphur in oxygen using deflagrating spoon. Testing with moist litmus paper. Practical work: Heating mixtures of sulphur with iron powder and copper powder. Observation: Exothermic reactions and color changes. Writing equations: Fe + S → FeS, 2Cu + S → Cu2S.
|
Sulphur, Iron powder, Copper powder, Oxygen gas jar, Deflagrating spoon, Moist litmus papers, Test tubes, Bunsen burner
Sulphur powder, Concentrated HNO3, Concentrated H2SO4, Concentrated HCl, Barium chloride solution, Test tubes, Fume cupboard access |
KLB Secondary Chemistry Form 4, Pages 165-167
|
|
| 8 | 1 |
SULPHUR AND ITS COMPOUNDS
|
Uses of Sulphur and Introduction to Oxides
Preparation of Sulphur(IV) Oxide Physical and Chemical Properties of Sulphur(IV) Oxide |
By the end of the
lesson, the learner
should be able to:
List the uses of sulphur in industry and agriculture. Identify the two main oxides of sulphur. Compare sulphur(IV) oxide and sulphur(VI) oxide. Plan laboratory preparation methods for sulphur oxides. |
Discussion: Industrial uses - sulphuric acid manufacture, fungicide, vulcanization of rubber, bleaching agents, dyes and fireworks. Q/A: Review oxidation states of sulphur in compounds. Introduction: SO2 and SO3 as important compounds. Preparation planning: Methods for laboratory preparation of SO
|
Charts showing uses of sulphur, Samples of vulcanized rubber, Fungicides, Industrial photographs, Textbook diagrams
Sodium sulphite, Dilute HCl, Round-bottomed flask, Delivery tubes, Gas jars, Concentrated H2SO4 for drying, Acidified potassium chromate(VI) paper SO2 gas from previous preparation, Litmus papers, Universal indicator, 0.1M NaOH solution, Water, Test tubes, Safety equipment |
KLB Secondary Chemistry Form 4, Pages 168-170
|
|
| 8 | 2 |
SULPHUR AND ITS COMPOUNDS
|
Bleaching Action of Sulphur(IV) Oxide
|
By the end of the
lesson, the learner
should be able to:
Investigate the bleaching properties of SO Compare SO2 bleaching with chlorine bleaching. Explain the mechanism of SO2 bleaching. Relate bleaching to paper manufacturing. |
Practical work: Experiment 6 - Placing colored flower petals in SO2 gas. Observation: Temporary bleaching effect. Discussion: SO2 + H2O → H2SO3, reduction of organic dyes. Comparison: Permanent vs temporary bleaching. Application: Paper industry bleaching processes.
|
Colored flower petals (red/blue), SO2 gas jars, Hand lens for observation, Charts comparing bleaching agents
|
KLB Secondary Chemistry Form 4, Pages 173
|
|
| 8 |
CAT TWO EXAM |
|||||||
| 9 | 1 |
SULPHUR AND ITS COMPOUNDS
|
Reducing Action of Sulphur(IV) Oxide
|
By the end of the
lesson, the learner
should be able to:
Investigate SO2 as a reducing agent. Test reactions with various oxidizing agents. Write ionic equations for redox reactions. Identify color changes in redox reactions. |
Practical work: Experiment 7 - Testing SO2 with acidified potassium dichromate(VI), potassium manganate(VII), bromine water, iron(III) chloride. Recording observations in Table 6. Color changes: Orange to green, purple to colorless, brown to colorless, yellow to pale green. Writing half-equations and overall equations.
|
SO2 gas, Acidified K2Cr2O7, Acidified KMnO4, Bromine water, Iron(III) chloride solution, Concentrated HNO3, Test tubes
|
KLB Secondary Chemistry Form 4, Pages 173-176
|
|
| 9 | 2 |
SULPHUR AND ITS COMPOUNDS
|
Oxidising Action of Sulphur(IV) Oxide
|
By the end of the
lesson, the learner
should be able to:
Investigate SO2 as an oxidizing agent. Demonstrate reaction with stronger reducing agents. Explain the dual nature of SO Write equations for oxidation reactions by SO |
Practical work: Experiment 8 - Lowering burning magnesium into SO2 gas. Observation: Continued burning, white fumes of MgO, yellow specks of sulphur. Reaction with hydrogen sulphide gas (demonstration). Discussion: SO2 decomposition providing oxygen. Writing equations: 2Mg + SO2 → 2MgO + S.
|
SO2 gas jars, Magnesium ribbon, Deflagrating spoon, Hydrogen sulphide gas, Water droppers, Safety equipment
|
KLB Secondary Chemistry Form 4, Pages 176-177
|
|
| 9 | 3 |
SULPHUR AND ITS COMPOUNDS
|
Test for Sulphate and Sulphite Ions & Uses of SO2
Large-scale Manufacture of Sulphuric(VI) Acid - Contact Process |
By the end of the
lesson, the learner
should be able to:
Carry out confirmatory tests for sulphate and sulphite ions. Distinguish between sulphate and sulphite using chemical tests. List the uses of sulphur(IV) oxide. Explain the applications in industry. |
Practical work: Experiment 9 - Testing sodium sulphate and sodium sulphite with barium chloride. Adding dilute HCl to precipitates. Recording observations in Table 8. Discussion: BaSO4 insoluble in acid, BaSO3 dissolves. Uses: Raw material for H2SO4, bleaching wood pulp, fumigant, preservative.
|
Sodium sulphate solution, Sodium sulphite solution, Barium chloride solution, Dilute HCl, Test tubes, Charts showing industrial uses
Flow chart diagrams, Charts showing industrial plant, Samples of catalyst (V2O5), Photographs of Thika chemical plant, Calculator for percentage calculations |
KLB Secondary Chemistry Form 4, Pages 178-179
|
|
| 9-10 |
MID TERM BREAK |
|||||||
| 10 | 2 |
SULPHUR AND ITS COMPOUNDS
|
Properties of Concentrated Sulphuric(VI) Acid - Dehydrating Properties
|
By the end of the
lesson, the learner
should be able to:
Investigate the dehydrating properties of concentrated H2SO Demonstrate removal of water from hydrated salts. Show dehydration of organic compounds. Explain the hygroscopic nature of the acid. |
Practical work: Experiment 10 - Adding concentrated H2SO4 to copper(II) sulphate crystals, sucrose crystals, ethanol. Observations: Blue to white crystals, charring of sugar, formation of ethene. Safety: Proper dilution technique - acid to water. Testing evolved gases. Discussion: Chemical vs physical dehydration.
|
Concentrated H2SO4, Copper(II) sulphate crystals, Sucrose, Ethanol, KMnO4 solution, Test tubes, Beakers, Safety equipment, Fume cupboard
|
KLB Secondary Chemistry Form 4, Pages 181-183
|
|
| 10 | 3-4 |
SULPHUR AND ITS COMPOUNDS
|
Properties of Concentrated Sulphuric(VI) Acid - Oxidizing Properties
Properties of Concentrated Sulphuric(VI) Acid - Displacement Reactions |
By the end of the
lesson, the learner
should be able to:
Investigate the oxidizing properties of concentrated H2SO Test reactions with metals and non-metals. Identify the products of oxidation reactions. Write balanced equations for redox reactions. Investigate acid displacement reactions. Demonstrate formation of volatile acids. Test the evolved gases for identification. Write equations for displacement reactions. |
Practical work: Experiment 10 (continued) - Reactions with copper foil, zinc granules, charcoal. Testing evolved gases with acidified K2Cr2O7 paper, lime water. Observations: SO2 evolution, color changes. Discussion: H2SO4 → SO2 + H2O + [O]. Writing half-equations and overall equations.
Practical work: Experiment 10 (continued) - Reactions with potassium nitrate and sodium chloride. Testing evolved gases with moist blue litmus, concentrated ammonia. Observations: Brown fumes (NO2), white fumes (HCl). Discussion: Less volatile acid displacing more volatile acids. Industrial applications. |
Copper foil, Zinc granules, Charcoal powder, Concentrated H2SO4, Acidified K2Cr2O7 paper, Lime water, Test tubes, Bunsen burner
Potassium nitrate crystals, Sodium chloride crystals, Concentrated H2SO4, Moist blue litmus paper, Concentrated ammonia, Test tubes, Bunsen burner |
KLB Secondary Chemistry Form 4, Pages 183-184
KLB Secondary Chemistry Form 4, Pages 184 |
|
| 10 | 5 |
SULPHUR AND ITS COMPOUNDS
|
Reactions of Dilute Sulphuric(VI) Acid - With Metals
Reactions of Dilute Sulphuric(VI) Acid - With Carbonates |
By the end of the
lesson, the learner
should be able to:
Investigate reactions of dilute H2SO4 with metals. Compare reactivity of different metals. Test for hydrogen gas evolution. Relate reactions to reactivity series. |
Practical work: Experiment 11 - Reactions with magnesium, zinc, copper. Testing evolved gas with burning splint. Recording observations in Table 10. Discussion: More reactive metals above hydrogen displace it. Vigour of reaction decreases down reactivity series. Writing ionic equations.
|
Magnesium ribbon, Zinc granules, Copper turnings, Dilute H2SO4, Test tubes, Burning splints, Reactivity series chart
Sodium carbonate, Zinc carbonate, Calcium carbonate, Copper(II) carbonate, Dilute H2SO4, Lime water, Test tubes |
KLB Secondary Chemistry Form 4, Pages 184-185
|
|
| 10 | 6 |
SULPHUR AND ITS COMPOUNDS
|
Reactions of Dilute Sulphuric(VI) Acid - With Oxides and Hydroxides
|
By the end of the
lesson, the learner
should be able to:
Investigate reactions of dilute H2SO4 with metal oxides and hydroxides. Identify neutralization reactions. Explain formation of insoluble sulphates. Write equations for acid-base reactions. |
Practical work: Experiment 13 - Reactions with magnesium oxide, zinc oxide, copper(II) oxide, lead(II) oxide, sodium hydroxide. Recording observations in Table 1 Discussion: Salt and water formation, immediate stopping with lead(II) oxide due to insoluble PbSO Acid-base neutralization concept.
|
Metal oxides (MgO, ZnO, CuO, PbO), NaOH solution, 2M H2SO4, Test tubes, Bunsen burner for warming
|
KLB Secondary Chemistry Form 4, Pages 186-187
|
|
| 11 | 1 |
SULPHUR AND ITS COMPOUNDS
|
Hydrogen Sulphide - Preparation and Physical Properties
|
By the end of the
lesson, the learner
should be able to:
Describe laboratory preparation of hydrogen sulphide. Set up apparatus for H2S preparation. State the physical properties of H2S. Explain the toxicity and safety precautions. |
Demonstration: Figure 13 apparatus setup for H2S preparation. Reaction: FeS + 2HCl → FeCl2 + H2S. Collection over warm water due to solubility. Drying: Using anhydrous CaCl2 (not H2SO4). Properties: Colorless, rotten egg smell, poisonous, denser than air. Safety precautions in handling.
|
Iron(II) sulphide, Dilute HCl, Apparatus for gas generation, Anhydrous CaCl2, Gas jars, Safety equipment, Fume cupboard
|
KLB Secondary Chemistry Form 4, Pages 187-188
|
|
| 11 | 2 |
SULPHUR AND ITS COMPOUNDS
|
Chemical Properties of Hydrogen Sulphide
|
By the end of the
lesson, the learner
should be able to:
Investigate H2S as a reducing agent. Test reactions with oxidizing agents. Demonstrate precipitation of metal sulphides. Write ionic equations for redox reactions. |
Practical demonstrations: H2S with bromine water, iron(III) chloride, acidified KMnO4, K2Cr2O7. Precipitation tests: H2S with copper(II) sulphate, lead(II) nitrate, zinc sulphate. Color changes: Brown to colorless, yellow to green, purple to colorless. Formation of black, yellow, and white precipitates.
|
H2S gas, Bromine water, Iron(III) chloride, KMnO4, K2Cr2O7, Metal salt solutions, Test tubes, Droppers
|
KLB Secondary Chemistry Form 4, Pages 188-190
|
|
| 11 | 3-4 |
SULPHUR AND ITS COMPOUNDS
CHLORINE AND ITS COMPOUNDS CHLORINE AND ITS COMPOUNDS |
Pollution Effects and Summary
Introduction and Preparation of Chlorine Physical Properties of Chlorine Chemical Properties of Chlorine - Reaction with Water Chemical Properties of Chlorine - Reaction with Metals |
By the end of the
lesson, the learner
should be able to:
Explain environmental pollution by sulphur compounds. Describe formation and effects of acid rain. Suggest methods to reduce sulphur pollution. Summarize key concepts of sulphur chemistry. Investigate the reaction of chlorine with water. Explain the formation of chlorine water. Test the acidic nature of chlorine water. Demonstrate the bleaching action of chlorine. |
Discussion: Sources of SO2 pollution - burning fossil fuels, metal extraction, H2SO4 manufacture. Formation of acid rain: SO2 + H2O → H2SO3 → H2SO Effects: Plant damage, aquatic life destruction, building corrosion, soil acidification. Control measures: Scrubbing with Ca(OH)2, catalytic converters. Revision: Key reactions, properties, uses.
Practical work: Experiment 6.3 - Bubbling chlorine through water. Testing with litmus papers (dry vs moist). Testing with colored flower petals. Formation of green-yellow chlorine water. Writing equations: Cl2 + H2O → HCl + HOCl. Discussion: Formation of hypochlorous acid and hydrochloric acid. |
Charts showing pollution effects, Photographs of acid rain damage, Environmental data, Summary charts of reactions, Industrial pollution control diagrams
Manganese(IV) oxide, Concentrated HCl, Gas collection apparatus, Water, Concentrated H2SO4, Blue litmus paper, Gas jars Preserved chlorine gas, Water trough, Gas jars, Observation tables, Safety equipment Chlorine gas, Distilled water, Blue and red litmus papers, Colored flower petals, Gas jars, Boiling tubes Magnesium ribbon, Iron wire, Chlorine gas, Deflagrating spoon, Combustion tube, Anhydrous CaCl2, Gas jars |
KLB Secondary Chemistry Form 4, Pages 190-194
KLB Secondary Chemistry Form 4, Pages 197-199 |
|
| 11 | 5 |
CHLORINE AND ITS COMPOUNDS
|
Chemical Properties of Chlorine - Reaction with Non-metals
Oxidising Properties of Chlorine Reaction of Chlorine with Alkali Solutions |
By the end of the
lesson, the learner
should be able to:
Investigate reactions of chlorine with non-metals. Demonstrate reaction with phosphorus and hydrogen. Write equations for non-metal chloride formation. Explain the vigorous nature of these reactions. |
Practical work: Experiment 6.5 - Warming red phosphorus and lowering into chlorine. Demonstration: Burning hydrogen jet in chlorine. Observations: White fumes of phosphorus chlorides, hydrogen chloride formation. Writing equations: P4 + 6Cl2 → 4PCl3, H2 + Cl2 → 2HCl. Discussion: Formation of covalent chlorides.
|
Red phosphorus, Hydrogen gas, Chlorine gas, Deflagrating spoon, Gas jars, Bunsen burner, Safety equipment
Sodium sulphite solution, Barium nitrate, Lead nitrate, Hydrogen sulphide gas, Aqueous ammonia, Chlorine gas, Test tubes Sodium hydroxide solutions (dilute cold, concentrated hot), Chlorine gas, Beakers, Bunsen burner, Thermometer |
KLB Secondary Chemistry Form 4, Pages 201
|
|
| 11 | 6 |
CHLORINE AND ITS COMPOUNDS
|
Oxidising Properties - Displacement Reactions
Test for Chloride Ions |
By the end of the
lesson, the learner
should be able to:
Investigate displacement reactions of chlorine with halides. Test reactions with bromides and iodides. Write ionic equations for displacement reactions. Explain the order of reactivity of halogens. |
Practical work: Experiment 6.8 - Bubbling chlorine through potassium bromide and potassium iodide solutions. Observations: Colorless to orange (Br2), colorless to brown (I2). Writing ionic equations: Cl2 + 2Br⁻ → 2Cl⁻ + Br2, Cl2 + 2I⁻ → 2Cl⁻ + I Discussion: Displacement as evidence of relative reactivity.
|
Potassium bromide solution, Potassium iodide solution, Chlorine gas, Test tubes, Observation charts
Sodium chloride, Concentrated H2SO4, Lead(II) nitrate solution, Aqueous ammonia, Glass rod, Test tubes, Bunsen burner |
KLB Secondary Chemistry Form 4, Pages 203-204
|
|
| 12-13 |
END TERM EXAM |
|||||||
| 13 | 6 |
CHLORINE AND ITS COMPOUNDS
|
Uses of Chlorine and its Compounds
|
By the end of the
lesson, the learner
should be able to:
List the industrial uses of chlorine. Explain the use of chlorine in water treatment. Describe manufacture of chlorine compounds. Relate properties to uses of chlorine. |
Discussion: Industrial applications - HCl manufacture, bleaching agents for cotton and paper industries, water treatment and sewage plants. Study Figure 6.3(a) - bleaching chemicals. Applications: Chloroform (anaesthetic), solvents (trichloroethane), CFCs, PVC plastics, pesticides (DDT), germicides and fungicides. Q/A: Relating chemical properties to practical applications.
|
Charts showing industrial uses, Samples of bleaching agents, PVC materials, Photographs of water treatment plants, Industrial application diagrams
|
KLB Secondary Chemistry Form 4, Pages 205-207
|
|
| 14 | 1 |
CHLORINE AND ITS COMPOUNDS
|
Hydrogen Chloride - Laboratory Preparation
|
By the end of the
lesson, the learner
should be able to:
Describe laboratory preparation of hydrogen chloride gas. Set up apparatus for HCl preparation. Investigate physical properties of HCl gas. Explain the method of collection used. |
Practical work: Experiment 6.10 - Preparation using rock salt (NaCl) + concentrated H2SO Setup apparatus as in Figure 6.3(b). Testing physical properties and recording in Table 6.6. Tests: Solubility (fountain experiment), reaction with ammonia, effect on litmus. Collection by downward delivery due to density. Writing equation: NaCl + H2SO4 → NaHSO4 + HCl.
|
Rock salt (NaCl), Concentrated H2SO4, Gas collection apparatus, Ammonia solution, Litmus papers, Water trough, Gas jars
|
KLB Secondary Chemistry Form 4, Pages 207-208
|
|
| 14 | 2 |
CHLORINE AND ITS COMPOUNDS
|
Chemical Properties of Hydrogen Chloride
Large-scale Manufacture of Hydrochloric Acid |
By the end of the
lesson, the learner
should be able to:
Prepare aqueous hydrogen chloride (hydrochloric acid). Investigate acid properties of HCl solution. Test reactions with metals, bases, and carbonates. Compare HCl in water vs organic solvents. |
Practical work: Experiment 6.11 - Preparation of aqueous HCl using apparatus in Figure 6. Testing with metals (Zn, Fe, Mg, Cu), NaOH, carbonates, lead nitrate. Recording observations in Table 6.7. Testing HCl in methylbenzene - no acid properties. Discussion: Ionization in water vs molecular existence in organic solvents. Writing equations for acid reactions.
|
Distilled water, Filter funnel, Metals (Zn, Fe, Mg, Cu), NaOH solution, Carbonates, Lead nitrate, Methylbenzene, Indicators
Flow diagrams, Industrial photographs, Glass beads samples, Charts showing electrolysis processes, Safety equipment models |
KLB Secondary Chemistry Form 4, Pages 208-211
|
|
| 14 | 3-4 |
CHLORINE AND ITS COMPOUNDS
|
Uses of Hydrochloric Acid
Environmental Pollution by Chlorine Compounds and Summary |
By the end of the
lesson, the learner
should be able to:
List the industrial uses of hydrochloric acid. Explain applications in metal treatment. Describe use in water treatment and manufacturing. Relate acid properties to industrial applications. Explain environmental effects of chlorine compounds. Describe the impact of CFCs on ozone layer. Discuss pollution by chlorine-containing pesticides. Summarize key concepts of chlorine chemistry. |
Discussion: Applications - rust removal and descaling, galvanizing preparation, electroplating preparation, water treatment (chlorination), sewage treatment. Manufacturing uses: dyes, drugs, photographic materials (AgCl), pH control in industries. Q/A: How acid properties make HCl suitable for these uses. Case studies: Metal cleaning processes, water purification systems.
Discussion: Environmental impacts - chlorine gas forming acid rain, CFCs (life span CCl3F = 75 years, CCl2F2 = 110 years) breaking down ozone layer. DDT as persistent pesticide, PVC as non-biodegradable plastic. NEMA role in environmental protection, Stockholm Convention on DDT. Control measures and alternatives. Revision: Key reactions, properties, uses, and environmental considerations. Summary of halogen chemistry concepts. |
Samples of rusted and cleaned metals, Photographic materials, pH control charts, Industrial application videos, Water treatment diagrams
Environmental pollution charts, Ozone layer diagrams, DDT restriction documents, PVC waste samples, NEMA guidelines, Summary charts of reactions |
KLB Secondary Chemistry Form 4, Pages 212-213
KLB Secondary Chemistry Form 4, Pages 213-215 |
|
| 14 |
CLOSING OF SCHOOL FOR AUGUST HOLLY DAY |
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