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| WK | LSN | TOPIC | SUB-TOPIC | OBJECTIVES | T/L ACTIVITIES | T/L AIDS | REFERENCE | REMARKS |
|---|---|---|---|---|---|---|---|---|
| 1 | 1-2 |
GAS LAWS
|
Boyle's Law - Introduction and Experimental Investigation
Boyle's Law - Mathematical Expression and Graphical Representation Boyle's Law - Numerical Problems and Applications Charles's Law - Introduction and Temperature Scales |
By the end of the
lesson, the learner
should be able to:
State Boyle's law Explain Boyle's law using kinetic theory of matter Investigate the relationship between pressure and volume of a fixed mass of gas Plot graphs to illustrate Boyle's law Express Boyle's law mathematically Apply the equation PV = constant Plot and interpret pressure vs volume graphs Plot pressure vs 1/volume graphs |
Teacher demonstration: Use bicycle pump to show volume-pressure relationship. Students observe force needed to compress gas. Q/A: Review kinetic theory. Class experiment: Investigate pressure-volume relationship using syringes. Record observations in table format. Discuss observations using kinetic theory.
Q/A: Recall previous lesson observations. Teacher exposition: Derive P₁V₁ = P₂V₂ equation from experimental data. Students plot graphs of pressure vs volume and pressure vs 1/volume. Analyze graph shapes and interpret mathematical relationship. |
Bicycle pump, Syringes, Gas jars, Chart showing volume-pressure relationship
Graph papers, Scientific calculators, Chart showing mathematical expressions Scientific calculators, Worked example charts, Unit conversion tables Round-bottomed flask, Narrow glass tube, Colored water, Rubber bung, Hot and cold water baths |
KLB Secondary Chemistry Form 3, Pages 1-3
KLB Secondary Chemistry Form 3, Pages 3-4 |
|
| 1 | 3 |
GAS LAWS
|
Charles's Law - Experimental Investigation and Mathematical Expression
Charles's Law - Numerical Problems and Applications Combined Gas Law and Standard Conditions Introduction to Diffusion - Experimental Investigation |
By the end of the
lesson, the learner
should be able to:
Investigate relationship between volume and temperature Express Charles's law mathematically Plot volume vs temperature graphs Extrapolate graphs to find absolute zero |
Class experiment: Volume-temperature relationship using flask and capillary tube. Record data at different temperatures. Plot graphs: volume vs temperature (°C) and volume vs absolute temperature (K). Extrapolate graph to find absolute zero. Derive V₁/T₁ = V₂/T₂ equation.
|
Glass apparatus, Thermometers, Graph papers, Water baths at different temperatures
Scientific calculators, Temperature conversion charts, Application examples Scientific calculators, Combined law derivation charts, Standard conditions reference table KMnO₄ crystals, Bromine liquid, Gas jars, Combustion tube, Litmus papers, Stopwatch |
KLB Secondary Chemistry Form 3, Pages 8-10
|
|
| 1 | 4 |
GAS LAWS
|
Rates of Diffusion - Comparative Study
Graham's Law of Diffusion - Theory and Mathematical Expression |
By the end of the
lesson, the learner
should be able to:
Compare diffusion rates of different gases Investigate factors affecting diffusion rates Measure relative distances covered by diffusing gases Calculate rates of diffusion using distance and time data |
Class experiment: Ammonia and HCl diffusion in glass tube. Insert cotton wool soaked in concentrated NH₃ and HCl at opposite ends. Time the formation of white NH₄Cl ring. Measure distances covered by each gas. Calculate rates: distance/time. Compare molecular masses of NH₃ and HCl.
|
Glass tube (25cm), Cotton wool, Concentrated NH₃ and HCl, Stopwatch, Ruler, Safety equipment
Graham's law charts, Molecular mass tables, Mathematical derivation displays |
KLB Secondary Chemistry Form 3, Pages 16-18
|
|
| 1 | 5 |
GAS LAWS
|
Graham's Law - Numerical Applications and Problem Solving
|
By the end of the
lesson, the learner
should be able to:
Solve numerical problems using Graham's law Calculate relative rates of diffusion Determine molecular masses from diffusion data Compare diffusion times for equal volumes of gases |
Worked examples: Calculate relative diffusion rates using √(M₂/M₁). Problems involving time comparisons for equal volumes. Calculate unknown molecular masses from rate data. Supervised practice: Various Graham's law calculations. Real-life applications: gas separation, gas masks.
|
Scientific calculators, Worked example charts, Molecular mass reference tables
|
KLB Secondary Chemistry Form 3, Pages 20-22
|
|
| 2 | 1-2 |
THE MOLE
|
Relative Mass - Introduction and Experimental Investigation
Avogadro's Constant and the Mole Concept Interconversion of Mass and Moles for Elements Molecules and Moles - Diatomic Elements |
By the end of the
lesson, the learner
should be able to:
Define relative mass using practical examples Compare masses of different objects using a reference standard Explain the concept of relative atomic mass Identify carbon-12 as the reference standard Apply the formula: moles = mass/molar mass Calculate mass from given moles of elements Convert between moles and number of atoms Solve numerical problems involving moles and mass |
Experiment: Weighing different sized nails using beam balance. Use smallest nail as reference standard. Q/A: Discuss everyday examples of relative measurements. Teacher exposition: Introduction of carbon-12 scale and IUPAC recommendations. Calculate relative masses from experimental data.
Worked examples: Mass-mole conversions using triangle method. Supervised practice: Calculate moles in given masses of common elements. Problem solving: Convert moles to atoms using Avogadro's number. Assignment: Practice problems on interconversion. |
Different sized nails ( 5-15cm), Beam balance, Fruits of different masses, Reference charts
Beam balance, Various sized nails, Scientific calculators, Avogadro's constant charts Scientific calculators, Periodic table, Worked example charts, Formula triangles Molecular models, Charts showing diatomic elements, Scientific calculators |
KLB Secondary Chemistry Form 3, Pages 25-27
KLB Secondary Chemistry Form 3, Pages 30-32 |
|
| 2 | 3 |
THE MOLE
|
Empirical Formula - Experimental Determination
|
By the end of the
lesson, the learner
should be able to:
Define empirical formula Determine empirical formula from experimental data Calculate mole ratios from mass data Express results as simplest whole number ratios |
Experiment: Burning magnesium in air to form magnesium oxide. Measure masses before and after reaction. Calculate moles of Mg and O from mass data. Determine mole ratio and empirical formula. Safety precautions during heating.
|
Crucible and lid, Magnesium ribbon, Bunsen burner, Beam balance, Tongs, Safety equipment
|
KLB Secondary Chemistry Form 3, Pages 32-35
|
|
| 2 | 4 |
THE MOLE
|
Empirical Formula - Reduction Method
Empirical Formula - Percentage Composition Method |
By the end of the
lesson, the learner
should be able to:
Determine empirical formula using reduction reactions Calculate empirical formula from reduction data Apply reduction method to copper oxides Analyze experimental errors and sources |
Experiment: Reduction of copper(II) oxide using laboratory gas. Measure masses before and after reduction. Calculate moles of copper and oxygen. Determine empirical formula from mole ratios. Discuss experimental precautions.
|
Combustion tube, Porcelain boat, Copper(II) oxide, Laboratory gas, Beam balance, Bunsen burner
Scientific calculators, Percentage composition charts, Worked example displays |
KLB Secondary Chemistry Form 3, Pages 35-37
|
|
| 2 | 5 |
THE MOLE
|
Molecular Formula - Determination from Empirical Formula
Molecular Formula - Combustion Analysis |
By the end of the
lesson, the learner
should be able to:
Define molecular formula Relate molecular formula to empirical formula Calculate molecular formula using molecular mass Apply the relationship (empirical formula)ₙ = molecular formula |
Teacher exposition: Difference between empirical and molecular formulas. Worked examples: Calculate molecular formula from empirical formula and molecular mass. Formula: n = molecular mass/empirical formula mass. Practice problems with various organic compounds.
|
Scientific calculators, Molecular mass charts, Worked example displays
Scientific calculators, Combustion analysis charts, Molecular models of hydrocarbons |
KLB Secondary Chemistry Form 3, Pages 38-40
|
|
| 3 | 1-2 |
THE MOLE
|
Concentration and Molarity of Solutions
Preparation of Molar Solutions Dilution 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 Describe procedure for preparing molar solutions Use volumetric flasks correctly Calculate masses needed for specific molarities Prepare standard solutions accurately |
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.
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. |
Scientific calculators, Molarity charts, Various salt samples for demonstration
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 41-43
KLB Secondary Chemistry Form 3, Pages 43-46 |
|
| 3 | 3 |
THE MOLE
|
Stoichiometry - Experimental Determination of Equations
Stoichiometry - Precipitation Reactions |
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
Test tubes, Lead(II) nitrate solution, Potassium iodide solution, Burettes, Ethanol, Rulers |
KLB Secondary Chemistry Form 3, Pages 50-53
|
|
| 3 | 4 |
THE MOLE
|
Stoichiometry - Gas Evolution Reactions
|
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 |
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.
|
Conical flask, Thistle funnel, Plastic bags, Rubber bands, Sodium carbonate, HCl solution
|
KLB Secondary Chemistry Form 3, Pages 56-58
|
|
| 3 | 5 |
THE MOLE
|
Volumetric Analysis - Introduction and Apparatus
Titration - Acid-Base Neutralization |
By the end of the
lesson, the learner
should be able to:
Define volumetric analysis and titration Identify and use titration apparatus correctly Explain functions of pipettes and burettes Demonstrate proper reading techniques |
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.
|
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 58-59
|
|
| 4 | 1-2 |
THE MOLE
|
Titration - Diprotic Acids
Standardization of Solutions Back Titration Method |
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 Understand principle of back titration Apply back titration to determine composition Calculate concentrations using back titration data Determine atomic masses from back titration |
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.
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. |
Burettes, Pipettes, 0.1M H₂SO₄, 0.1M NaOH, Phenolphthalein, Basicity reference chart
Anhydrous Na₂CO₃, Approximately 0.1M HCl, Methyl orange, Volumetric flasks, Analytical balance Metal carbonate sample, 0.5M HCl, 0M NaOH, Phenolphthalein, Conical flasks |
KLB Secondary Chemistry Form 3, Pages 62-65
KLB Secondary Chemistry Form 3, Pages 67-70 |
|
| 4 | 3 |
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 | 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 |
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.
|
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
|
|
| 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
|
|
| 5 | 1-2 |
THE MOLE
ORGANIC CHEMISTRY I |
Gas Laws and Chemical Equations
Introduction to Organic Chemistry and Hydrocarbons Sources of Alkanes - Natural Gas, Biogas, and Crude Oil Fractional Distillation of Crude Oil |
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 Identify natural sources of alkanes Describe composition of natural gas and biogas Explain crude oil as major source of alkanes Describe biogas digester and its operation |
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.
Discussion: Natural gas composition (80% methane). Explanation: Biogas formation from organic waste decomposition. Teacher demonstration: Biogas digester model/diagram. Q/A: Environmental benefits of biogas production. |
Scientific calculators, Gas law charts, Volume ratio examples
Carbon models, Hydrocarbon structure charts, Molecular model kits Biogas digester model/diagram, Natural gas composition charts, Organic waste samples Crude oil sample, Boiling tubes, High-temperature thermometer, Sand/porcelain chips, Bunsen burner, Test tubes |
KLB Secondary Chemistry Form 3, Pages 77-79
KLB Secondary Chemistry Form 3, Pages 86-87 |
|
| 5 | 3 |
ORGANIC CHEMISTRY I
|
Cracking of Alkanes - Thermal and Catalytic Methods
|
By the end of the
lesson, the learner
should be able to:
Define cracking of alkanes Distinguish between thermal and catalytic cracking Write equations for cracking reactions Explain industrial importance of cracking |
Teacher exposition: Definition and purpose of cracking. Discussion: Thermal vs catalytic cracking conditions. Worked examples: Cracking equations producing smaller alkanes, alkenes, and hydrogen. Q/A: Industrial applications and hydrogen production.
|
Cracking process diagrams, Chemical equation charts, Catalyst samples for demonstration
|
KLB Secondary Chemistry Form 3, Pages 89-90
|
|
| 5 | 4 |
ORGANIC CHEMISTRY I
|
Alkane Series and Homologous Series Concept
Nomenclature of Alkanes - Straight Chain and Branched |
By the end of the
lesson, the learner
should be able to:
Define homologous series using alkanes Write molecular formulas for first 10 alkanes Identify characteristics of homologous series Apply general formula CₙH₂ₙ₊₂ for alkanes |
Teacher exposition: Homologous series definition and characteristics. Table completion: Names, molecular formulas, and structures of first 10 alkanes. Discussion: General formula application. Pattern recognition: Gradual change in physical properties.
|
Alkane series chart, Molecular formula worksheets, Periodic table
Structural formula charts, IUPAC naming rules poster, Molecular model kits |
KLB Secondary Chemistry Form 3, Pages 90-92
|
|
| 5 | 5 |
ORGANIC CHEMISTRY I
|
Isomerism in Alkanes - Structural Isomers
Laboratory Preparation of Methane |
By the end of the
lesson, the learner
should be able to:
Define isomerism in alkanes Draw structural isomers of butane and pentane Distinguish between chain and positional isomerism Predict number of isomers for given alkanes |
Teacher exposition: Isomerism definition and types. Practical exercise: Draw all isomers of butane and pentane. Discussion: Physical property differences between isomers. Model building: Use molecular models to show isomeric structures.
|
Molecular model kits, Isomerism charts, Structural formula worksheets
Sodium ethanoate, Soda lime, Round-bottomed flask, Gas collection apparatus, Bromine water, Wooden splints |
KLB Secondary Chemistry Form 3, Pages 92-94
|
|
| 6 | 1-2 |
ORGANIC CHEMISTRY I
|
Laboratory Preparation of Ethane
Physical Properties of Alkanes Chemical Properties of Alkanes - Combustion and Substitution |
By the end of the
lesson, the learner
should be able to:
Prepare ethane using sodium propanoate and soda lime Compare preparation methods of methane and ethane Test properties of ethane gas Write general equation for alkane preparation Describe physical properties of alkanes Explain trends in melting and boiling points Relate molecular size to physical properties Compare solubility in different solvents |
Experiment: Prepare ethane from sodium propanoate and soda lime. Compare with methane preparation method. Carry out similar tests as for methane. Discussion: General pattern for alkane preparation from sodium alkanoates.
Data analysis: Study table of physical properties of first 10 alkanes. Graph plotting: Boiling points vs number of carbon atoms. Discussion: Intermolecular forces and property trends. Q/A: Solubility patterns in polar and non-polar solvents. |
Sodium propanoate, Soda lime, Gas collection apparatus, Testing materials
Physical properties data tables, Graph paper, Calculators, Solubility demonstration materials Molecular models, Halogenation reaction charts, Chemical equation worksheets |
KLB Secondary Chemistry Form 3, Pages 94-96
KLB Secondary Chemistry Form 3, Pages 96-97 |
|
| 6 | 3 |
ORGANIC CHEMISTRY I
|
Uses of Alkanes in Industry and Daily Life
Introduction to Alkenes and Functional Groups |
By the end of the
lesson, the learner
should be able to:
List major uses of different alkanes Explain industrial applications of alkanes Describe environmental considerations Evaluate economic importance of alkanes |
Discussion: Uses of gaseous alkanes as fuels. Teacher exposition: Industrial applications - carbon black, methanol production, hydrogen source. Q/A: Environmental impact and cleaner fuel initiatives. Assignment: Research local uses of alkane products.
|
Industrial application charts, Product samples, Environmental impact materials
Alkene series charts, Molecular models showing double bonds, Functional group posters |
KLB Secondary Chemistry Form 3, Pages 98-100
|
|
| 6 | 4 |
ORGANIC CHEMISTRY I
|
Nomenclature of Alkenes
|
By the end of the
lesson, the learner
should be able to:
Apply IUPAC rules for naming alkenes Number carbon chains to give lowest numbers to double bonds Name branched alkenes with substituents Distinguish position isomers of alkenes |
Teacher demonstration: Step-by-step naming of alkenes. Rules application: Longest chain with double bond, numbering from end nearest double bond. Practice exercises: Name various alkene structures. Group work: Complex branched alkenes with substituents.
|
IUPAC naming charts for alkenes, Structural formula worksheets, Molecular model kits
|
KLB Secondary Chemistry Form 3, Pages 101-102
|
|
| 6 | 5 |
ORGANIC CHEMISTRY I
|
Isomerism in Alkenes - Branching and Positional
Laboratory Preparation of Ethene |
By the end of the
lesson, the learner
should be able to:
Draw structural isomers of alkenes Distinguish between branching and positional isomerism Identify geometric isomers in alkenes Predict isomer numbers for given molecular formulas |
Practical exercise: Draw all isomers of butene and pentene. Teacher exposition: Branching vs positional isomerism in alkenes. Model building: Use molecular models for isomer visualization. Discussion: Geometric isomerism introduction (basic level).
|
Molecular model kits, Isomerism worksheets, Geometric isomer models
Ethanol, Concentrated H₂SO₄, Round-bottomed flask, Sand bath, Gas collection apparatus, Testing solutions |
KLB Secondary Chemistry Form 3, Pages 102
|
|
| 7 | 1-2 |
ORGANIC CHEMISTRY I
|
Alternative Preparation of Ethene and Physical Properties
Chemical Properties of Alkenes - Addition Reactions Oxidation Reactions of Alkenes and Polymerization |
By the end of the
lesson, the learner
should be able to:
Describe catalytic dehydration using aluminum oxide Compare different preparation methods List physical properties of ethene Explain trends in alkene physical properties Describe oxidation by KMnO₄ and K₂Cr₂O₇ Explain polymerization of ethene Define monomers and polymers Write equations for polymer formation |
Demonstration: Alternative method using Al₂O₃ catalyst. Comparison: Acid vs catalytic dehydration methods. Data analysis: Physical properties of alkenes table. Discussion: Property trends with increasing molecular size.
Demonstration: Decolorization of KMnO₄ by alkenes. Teacher exposition: Polymerization process and polymer formation. Examples: Ethene → polyethene formation. Discussion: Industrial importance of polymerization. Practice: Write polymerization equations. |
Aluminum oxide catalyst, Glass wool, Alternative apparatus setup, Physical properties charts
Addition reaction charts, Mechanism diagrams, Chemical equation worksheets Oxidizing agents for demonstration, Polymer samples, Polymerization charts, Monomer-polymer models |
KLB Secondary Chemistry Form 3, Pages 102-104
KLB Secondary Chemistry Form 3, Pages 107-108 |
|
| 7 | 3 |
ORGANIC CHEMISTRY I
|
Tests for Alkenes and Uses
Introduction to Alkynes and Triple Bond |
By the end of the
lesson, the learner
should be able to:
Perform chemical tests to identify alkenes Use bromine water and KMnO₄ as test reagents List industrial and domestic uses of alkenes Explain importance in plastic manufacture |
Practical session: Test known alkenes with bromine water and acidified KMnO₄. Observe rapid decolorization compared to alkanes. Discussion: Uses in plastics, ethanol production, fruit ripening, detergents. Assignment: Research alkene applications.
|
Test alkenes, Bromine water, Acidified KMnO₄, Plastic samples, Uses reference charts
Alkyne series charts, Triple bond molecular models, Unsaturation comparison charts |
KLB Secondary Chemistry Form 3, Pages 108-109
|
|
| 7 | 4 |
ORGANIC CHEMISTRY I
|
Nomenclature and Isomerism in Alkynes
Laboratory Preparation of Ethyne |
By the end of the
lesson, the learner
should be able to:
Apply IUPAC naming rules for alkynes Name branched alkynes with substituents Draw structural isomers of alkynes Identify branching and positional isomerism |
Teacher demonstration: Systematic naming of alkynes using -yne suffix. Practice exercises: Name various alkyne structures. Drawing exercise: Isomers of pentyne and hexyne. Group work: Complex branched alkynes with multiple substituents.
|
IUPAC naming rules for alkynes, Structural formula worksheets, Molecular model kits
Calcium carbide, Sand, Flat-bottomed flask, Dropping funnel, Gas collection apparatus, Testing solutions |
KLB Secondary Chemistry Form 3, Pages 110-111
|
|
| 7 | 5 |
ORGANIC CHEMISTRY I
|
Physical and Chemical Properties of Alkynes
|
By the end of the
lesson, the learner
should be able to:
Describe physical properties of alkynes Compare alkyne properties with alkenes and alkanes Write combustion equations for alkynes Explain addition reactions of alkynes |
Data analysis: Physical properties of alkynes table. Comparison: Alkynes vs alkenes vs alkanes properties. Worked examples: Combustion reactions of ethyne. Teacher exposition: Two-step addition reactions due to triple bond.
|
Physical properties charts, Comparison tables, Combustion equation examples
|
KLB Secondary Chemistry Form 3, Pages 112-113
|
|
| 8 | 1-2 |
ORGANIC CHEMISTRY I
NITROGEN AND ITS COMPOUNDS |
Addition Reactions of Alkynes and Chemical Tests
Uses of Alkynes and Industrial Applications Introduction to Nitrogen - Properties and Occurrence Isolation of Nitrogen from Air - Industrial and Laboratory Methods |
By the end of the
lesson, the learner
should be able to:
Write equations for halogenation of alkynes Describe hydrogenation and hydrohalogenation Compare reaction rates: alkynes vs alkenes Perform chemical tests for alkynes Describe position of nitrogen in the periodic table State electron configuration of nitrogen Identify natural occurrence of nitrogen Explain why nitrogen exists as diatomic molecules |
Worked examples: Two-step addition reactions of ethyne with Br₂, Cl₂, H₂. Discussion: Faster reaction rates in alkynes compared to alkenes. Practical session: Test alkynes with oxidizing agents. Comparison: Rate of decolorization vs alkenes.
Teacher exposition: Nitrogen as Group V element, atomic number 7, electron arrangement Discussion: 78% of atmosphere is nitrogen. Q/A: Combined nitrogen in compounds - nitrates, proteins. Explanation: N≡N triple bond strength. |
Addition reaction charts, Chemical equation worksheets, Test solutions, Stopwatch for rate comparison
Industrial application charts, Welding equipment demonstration/video, Synthetic fiber samples Periodic table charts, Atmospheric composition diagrams, Molecular models showing N≡N triple bond Aspirator, KOH solution, Copper turnings, Heating apparatus, Fractional distillation flow chart |
KLB Secondary Chemistry Form 3, Pages 113-115
KLB Secondary Chemistry Form 3, Pages 119 |
|
| 8 | 3 |
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
|
|
| 8 | 4 |
NITROGEN AND ITS COMPOUNDS
|
Properties and Uses of Nitrogen Gas
Nitrogen(I) 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 |
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.
|
Property summary charts, Uses of nitrogen displays, Industrial application diagrams
Ammonium nitrate, Test tubes, Gas collection apparatus, Copper turnings, Sulfur, Glowing splints |
KLB Secondary Chemistry Form 3, Pages 121-123
|
|
| 8 | 5 |
NITROGEN AND ITS COMPOUNDS
|
Nitrogen(II) Oxide - Preparation and Properties
Nitrogen(IV) Oxide - Preparation and Properties |
By the end of the
lesson, the learner
should be able to:
Prepare nitrogen(II) oxide from copper and dilute nitric acid Observe colorless gas and brown fumes formation Test reactions with air and iron(II) sulfate Explain oxidation in air to NO₂ |
Experiment: Add dilute HNO₃ to copper turnings. Observe brown fumes formation then disappearance. Tests: Effect on litmus, burning splint, FeSO₄ complex formation. Discussion: NO oxidation to NO₂ in air.
|
Copper turnings, Dilute nitric acid, Gas collection apparatus, Iron(II) sulfate solution, Test reagents
Copper turnings, Concentrated nitric acid, Lead(II) nitrate, Gas collection apparatus, U-tube with ice, Testing materials |
KLB Secondary Chemistry Form 3, Pages 125-127
|
|
| 9 | 1-2 |
NITROGEN AND ITS COMPOUNDS
|
Comparison of Nitrogen Oxides and Environmental Effects
Laboratory Preparation of Ammonia Preparation of Aqueous Ammonia and Solubility |
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 Prepare ammonia from ammonium salts and alkalis Set up apparatus with proper gas collection Test characteristic properties of ammonia Explain displacement reaction principle |
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.
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. |
Comparison charts, Environmental impact diagrams, Vehicle emission illustrations
Calcium hydroxide, Ammonium chloride, Round-bottomed flask, Calcium oxide, HCl solution, Glass rod, Litmus paper Ammonia generation apparatus, Funnel, Universal indicator, Fountain apparatus, pH meter/paper |
KLB Secondary Chemistry Form 3, Pages 123-131
KLB Secondary Chemistry Form 3, Pages 131-134 |
|
| 9 | 3 |
NITROGEN AND ITS COMPOUNDS
|
Reactions of Aqueous Ammonia with Metal Ions
Chemical Properties of Ammonia - Reactions with Acids and Combustion |
By the end of the
lesson, the learner
should be able to:
Test reactions of aqueous ammonia with various metal ions Observe precipitate formation and dissolution Explain complex ion formation Use reactions for metal ion identification |
Experiment: Add aqueous ammonia dropwise to solutions of Ca²⁺, Mg²⁺, Al³⁺, Zn²⁺, Fe²⁺, Fe³⁺, Pb²⁺, Cu²⁺. Record observations with few drops vs excess ammonia. Identify complex ion formation with Zn²⁺ and Cu²⁺.
|
Various metal salt solutions, Aqueous ammonia, Test tubes, Droppers, Observation recording tables
Various dilute acids, Methyl orange, Oxygen supply, Platinum wire, Copper(II) oxide, Combustion apparatus, U-tube for collection |
KLB Secondary Chemistry Form 3, Pages 136-138
|
|
| 9 | 4 |
NITROGEN AND ITS COMPOUNDS
|
Industrial Manufacture of Ammonia - The Haber Process
|
By the end of the
lesson, the learner
should be able to:
Describe raw materials and their sources Explain optimum conditions for ammonia synthesis Draw flow diagram of Haber process Explain economic considerations and catalyst use |
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.
|
Haber process flow charts, Industrial diagrams, Catalyst samples, Economic analysis sheets
|
KLB Secondary Chemistry Form 3, Pages 140-141
|
|
| 9 | 5 |
NITROGEN AND ITS COMPOUNDS
|
Uses of Ammonia and Introduction to Nitrogenous Fertilizers
Nitrogenous Fertilizers - Types and Calculations |
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
Various fertilizer formulas, Scientific calculators, Laboratory preparation materials, Environmental impact data |
KLB Secondary Chemistry Form 3, Pages 141-144
|
|
| 10 | 1-2 |
NITROGEN AND ITS COMPOUNDS
|
Laboratory Preparation of Nitric(V) Acid
Industrial Manufacture of Nitric(V) Acid Reactions of Dilute Nitric(V) Acid with Metals |
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 Test reactions with various metals Explain absence of hydrogen gas production Observe formation of nitrogen oxides Write equations for metal-acid reactions |
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.
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. |
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 Various metals (Mg, Zn, Cu), Dilute nitric acid, Test tubes, Gas testing apparatus, Burning splints |
KLB Secondary Chemistry Form 3, Pages 144-145
KLB Secondary Chemistry Form 3, Pages 147-150 |
|
| 10 | 3 |
NITROGEN AND ITS COMPOUNDS
|
Reactions of Dilute Nitric(V) Acid with Carbonates and Hydroxides
Reactions of Concentrated Nitric(V) Acid - Oxidizing Properties |
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 |
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.
|
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 |
KLB Secondary Chemistry Form 3, Pages 147-150
|
|
| 10 | 4 |
NITROGEN AND ITS COMPOUNDS
|
Uses of Nitric(V) Acid and Introduction to Nitrates
Action of Heat on Nitrates - Decomposition Patterns |
By the end of the
lesson, the learner
should be able to:
List major industrial uses of nitric acid Explain importance in fertilizer manufacture Describe use in explosives and dyes Introduce nitrate salts and their preparation |
Discussion: Uses - fertilizer production (NH₄NO₃), explosives (TNT), dyes, drugs, metal purification, etching. Introduction to nitrates as salts of nitric acid. Methods of preparation: acid + base, acid + carbonate, acid + metal. Examples of common nitrates.
|
Industrial use charts, Nitrate salt samples, Preparation method diagrams, Safety data sheets
Various nitrate salts, Test tubes, Bunsen burner, Gas collection apparatus, Glowing splints, Observation recording sheets |
KLB Secondary Chemistry Form 3, Pages 151
|
|
| 10 | 5 |
NITROGEN AND ITS COMPOUNDS
|
Test for Nitrates - Brown Ring Test
|
By the end of the
lesson, the learner
should be able to:
Perform brown ring test for nitrates Explain mechanism of complex formation Use alternative copper test method Apply tests to unknown samples |
Experiments: (a) Brown ring test - add FeSO₄ solution to nitrate, then carefully add concentrated H₂SO₄. Observe brown ring formation. (b) Alternative test - warm nitrate with H₂SO₄ and copper turnings. Observe brown fumes. Test unknown samples.
|
Sodium nitrate, Fresh FeSO₄ solution, Concentrated H₂SO₄, Copper turnings, Test tubes, Unknown nitrate samples
|
KLB Secondary Chemistry Form 3, Pages 153-154
|
|
| 11 | 1-2 |
NITROGEN AND ITS COMPOUNDS
|
Environmental Pollution by Nitrogen Compounds
Pollution Control and Environmental Solutions Comprehensive Problem Solving - Nitrogen Chemistry Laboratory Practical Assessment - Nitrogen Compounds |
By the end of the
lesson, the learner
should be able to:
Explain sources of nitrogen pollution Describe formation of acid rain Discuss effects on environment and health Evaluate pollution control measures Solve complex problems involving nitrogen compounds Apply knowledge to industrial processes Calculate yields and percentages in reactions Analyze experimental data and results |
Teacher exposition: NOₓ from vehicles, HNO₃ formation in atmosphere, acid rain effects. Discussion: Chlorosis in plants, building corrosion, soil leaching, smog formation, health effects. Control measures: Catalytic converters, emission controls, proper fertilizer use.
Problem-solving session: Mixed calculations involving nitrogen preparation, ammonia synthesis, nitric acid concentration, fertilizer analysis. Industrial application problems. Data analysis from experiments. Integration of all nitrogen chemistry concepts. |
Environmental pollution charts, Acid rain effect photos, Vehicle emission diagrams, Control measure illustrations
Case studies, Pollution control technology information, Group activity worksheets, Local environmental data Scientific calculators, Comprehensive problem sets, Industrial data sheets, Experimental result tables Unknown nitrogen compounds, All laboratory chemicals and apparatus used in chapter, Safety equipment, Assessment rubrics |
KLB Secondary Chemistry Form 3, Pages 154-157
KLB Secondary Chemistry Form 3, Pages 119-157 |
|
| 11 | 3 |
NITROGEN AND ITS COMPOUNDS
|
Industrial Applications and Economic Importance
|
By the end of the
lesson, the learner
should be able to:
Evaluate economic importance of nitrogen industry Analyze industrial production costs and benefits Compare different manufacturing processes Assess impact on agricultural productivity |
Case study analysis: Haber process economics, fertilizer industry impact, nitric acid production costs. Agricultural benefits: Crop yield improvements, food security. Economic calculations: Production costs, profit margins, environmental costs. Global nitrogen cycle importance.
|
Economic data sheets, Industry case studies, Agricultural statistics, Cost-benefit analysis templates
|
KLB Secondary Chemistry Form 3, Pages 119-157
|
|
| 11 | 4 |
NITROGEN AND ITS COMPOUNDS
SULPHUR AND ITS COMPOUNDS SULPHUR AND ITS COMPOUNDS SULPHUR AND ITS COMPOUNDS |
Chapter Review and Integration
Extraction of Sulphur Allotropes of Sulphur Physical Properties of Sulphur - Solubility |
By the end of the
lesson, the learner
should be able to:
Synthesize all nitrogen chemistry concepts Compare preparation methods for nitrogen compounds Relate structure to properties and reactivity Connect laboratory and industrial processes |
Comprehensive review: Concept mapping of all nitrogen compounds and their relationships. Comparison tables: Preparation methods, properties, uses. Flow chart: Nitrogen cycle in industry and environment. Integration exercises connecting all topics.
|
Concept mapping materials, Comparison charts, Flow diagram templates, Integration worksheets
Charts showing periodic table, Diagram of Frasch process, Samples of sulphur compounds (pyrites, gypsum) 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 |
KLB Secondary Chemistry Form 3, Pages 119-157
|
|
| 11 | 5 |
SULPHUR AND ITS COMPOUNDS
|
Physical Properties of Sulphur - Effect of Heat
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 effect of heat on sulphur. Describe changes in color and viscosity of molten sulphur. Explain the molecular changes occurring during heating. Identify "flowers of sulphur". |
Practical work: Experiment 2(b) - Heating sulphur and observing changes. Observation: Color changes from yellow to amber to reddish-brown to black. Testing viscosity by inverting test tube. Demonstration: Sublimation of sulphur vapour. Discussion: Breaking of S8 rings to form long chains.
|
Powdered sulphur, Test tubes, Bunsen burner, Cold surface for condensation, Thermometer, Safety equipment
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 164-165
|
|
| 12 | 1-2 |
SULPHUR AND ITS COMPOUNDS
|
Uses of Sulphur and Introduction to Oxides
Preparation of Sulphur(IV) Oxide Physical and Chemical Properties of Sulphur(IV) Oxide Bleaching Action of Sulphur(IV) Oxide Reducing Action 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. Investigate the bleaching properties of SO Compare SO2 bleaching with chlorine bleaching. Explain the mechanism of SO2 bleaching. Relate bleaching to paper manufacturing. |
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
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. |
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 Colored flower petals (red/blue), SO2 gas jars, Hand lens for observation, Charts comparing bleaching agents SO2 gas, Acidified K2Cr2O7, Acidified KMnO4, Bromine water, Iron(III) chloride solution, Concentrated HNO3, Test tubes |
KLB Secondary Chemistry Form 4, Pages 168-170
KLB Secondary Chemistry Form 4, Pages 173 |
|
| 12 | 3 |
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
|
|
| 12 | 4 |
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
|
|
| 12 | 5 |
SULPHUR AND ITS COMPOUNDS
|
Properties of Concentrated Sulphuric(VI) Acid - Dehydrating Properties
Properties of Concentrated Sulphuric(VI) Acid - Oxidizing 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
Copper foil, Zinc granules, Charcoal powder, Concentrated H2SO4, Acidified K2Cr2O7 paper, Lime water, Test tubes, Bunsen burner |
KLB Secondary Chemistry Form 4, Pages 181-183
|
|
| 13 | 1-2 |
SULPHUR AND ITS COMPOUNDS
|
Properties of Concentrated Sulphuric(VI) Acid - Displacement Reactions
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 acid displacement reactions. Demonstrate formation of volatile acids. Test the evolved gases for identification. Write equations for displacement reactions. 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 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.
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. |
Potassium nitrate crystals, Sodium chloride crystals, Concentrated H2SO4, Moist blue litmus paper, Concentrated ammonia, Test tubes, Bunsen burner
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
KLB Secondary Chemistry Form 4, Pages 184-185 |
|
| 13 | 3 |
SULPHUR AND ITS COMPOUNDS
|
Reactions of Dilute Sulphuric(VI) Acid - With Oxides and Hydroxides
Hydrogen Sulphide - Preparation and Physical Properties |
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
Iron(II) sulphide, Dilute HCl, Apparatus for gas generation, Anhydrous CaCl2, Gas jars, Safety equipment, Fume cupboard |
KLB Secondary Chemistry Form 4, Pages 186-187
|
|
| 13 | 4 |
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
|
|
| 13 | 5 |
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 |
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. |
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.
|
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 |
KLB Secondary Chemistry Form 4, Pages 190-194
|
|
| 14 | 1-2 |
CHLORINE AND ITS COMPOUNDS
|
Chemical Properties of Chlorine - Reaction with Water
Chemical Properties of Chlorine - Reaction with Metals Chemical Properties of Chlorine - Reaction with Non-metals Oxidising Properties of Chlorine Reaction of Chlorine with Alkali Solutions Oxidising Properties - Displacement Reactions Test for Chloride Ions |
By the end of the
lesson, the learner
should be able to:
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. Investigate reactions of chlorine with alkalis. Compare reactions with cold dilute and hot concentrated alkalis. Write equations for formation of chlorates and hypochlorites. Explain formation of bleaching powder. |
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.
Practical work: Experiment 6.7 - Bubbling chlorine through cold dilute NaOH and hot concentrated NaOH. Recording observations in Table 6. Formation of pale-yellow solution (cold) vs colorless solution (hot). Equations: 3Cl2 + 6NaOH → 5NaCl + NaClO3 + 3H2O (hot), Cl2 + 2NaOH → NaCl + NaClO + H2O (cold). Discussion: Industrial production of bleaching powder. |
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 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 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 197-199
KLB Secondary Chemistry Form 4, Pages 202-203 |
|
| 14 | 3 |
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 | 4 |
CHLORINE AND ITS COMPOUNDS
|
Hydrogen Chloride - Laboratory Preparation
Chemical Properties of Hydrogen Chloride |
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
Distilled water, Filter funnel, Metals (Zn, Fe, Mg, Cu), NaOH solution, Carbonates, Lead nitrate, Methylbenzene, Indicators |
KLB Secondary Chemistry Form 4, Pages 207-208
|
|
| 14 | 5 |
CHLORINE AND ITS COMPOUNDS
|
Large-scale Manufacture of Hydrochloric Acid
Uses of Hydrochloric Acid Environmental Pollution by Chlorine Compounds and Summary |
By the end of the
lesson, the learner
should be able to:
Describe industrial production of hydrochloric acid. Identify raw materials and conditions used. Explain the controlled combustion process. Draw flow diagrams of the industrial process. |
Study of Figure 6.4 - Large-scale manufacture setup. Discussion: Raw materials (H2 from electrolysis/cracking, Cl2 from electrolysis). Controlled combustion: H2 + Cl2 → 2HCl in jet burner. Dissolving HCl gas in water over glass beads. Safety: Explosive nature of H2/Cl2 mixture, use of excess chlorine. Industrial considerations: 35% concentration, transport in rubber-lined steel tanks.
|
Flow diagrams, Industrial photographs, Glass beads samples, Charts showing electrolysis processes, Safety equipment models
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 211-212
|
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