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| WK | LSN | TOPIC | SUB-TOPIC | OBJECTIVES | T/L ACTIVITIES | T/L AIDS | REFERENCE | REMARKS |
|---|---|---|---|---|---|---|---|---|
| 1 | 3-4 |
ACIDS, BASES AND SALTS
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Definition of Acids
Strength of Acids Definition of Bases Strength of Bases Acid-Base Reactions Effect of Solvent on Acids Effect of Solvent on Bases Amphoteric Oxides and Hydroxides Definition of Salts and Precipitation Solubility of Chlorides, Sulphates and Sulphites Complex Ions Formation Solubility and Saturated Solutions Effect of Temperature on Solubility Solubility Curves and Applications Fractional Crystallization Hardness of Water - Investigation Types and Causes of Water Hardness Effects of Hard Water Methods of Removing Hardness I Methods of Removing Hardness II |
By the end of the
lesson, the learner
should be able to:
- Define an acid in terms of hydrogen ions -Investigate reactions of magnesium and zinc carbonate with different acids -Write equations for reactions taking place -Explain why magnesium strip should be cleaned - Find out cations that form insoluble chlorides, sulphates and sulphites -Write ionic equations for formation of insoluble salts -Distinguish between sulphate and sulphite precipitates -Investigate effect of warming on precipitates |
Class experiment: React cleaned magnesium strips with 2M HCl, 2M ethanoic acid, 2M H₂SO₄, 2M ethanedioic acid. Record observations in table. Repeat using zinc carbonate. Write chemical equations. Discuss hydrogen ion displacement and gas evolution.
Class experiment: Add NaCl, Na₂SO₄, Na₂SO₃ to solutions of Pb²⁺, Ba²⁺, Mg²⁺, Ca²⁺, Zn²⁺, Cu²⁺, Fe²⁺, Fe³⁺, Al³⁺. Warm mixtures. Record observations in table. Test sulphite precipitates with dilute HCl. List soluble and insoluble salts. |
Magnesium strips, zinc carbonate, 2M HCl, 2M ethanoic acid, 2M H₂SO₄, 2M ethanedioic acid, test tubes, test tube rack
2M HCl, 2M ethanoic acid, universal indicator, pH chart, electrical conductivity apparatus, milliammeter, carbon electrodes, beakers, wires Calcium hydroxide, red litmus paper, phenolphthalein indicator, distilled water, test tubes, spatula, evaporating dish 2M NaOH, 2M ammonia solution, universal indicator, pH chart, electrical conductivity apparatus, milliammeter, carbon electrodes Various acids and bases from previous lessons, indicators, beakers, measuring cylinders, stirring rods HCl gas, distilled water, methylbenzene, magnesium ribbon, calcium carbonate, litmus paper, test tubes, gas absorption apparatus Dry ammonia gas, distilled water, methylbenzene, red litmus paper, test tubes, gas collection apparatus Al₂O₃, ZnO, PbO, Zn(OH)₂, Al(OH)₃, Pb(OH)₂, 2M HNO₃, 2M NaOH, boiling tubes, heating source Na₂CO₃ solution, salt solutions containing various metal ions, test tubes, droppers 2M NaCl, 2M Na₂SO₄, 2M Na₂SO₃, 0.1M salt solutions, dilute HCl, test tubes, heating source 2M NaOH, 2M NH₃ solution, 0.5M salt solutions, test tubes, droppers Saturated KNO₃ solution, evaporating dish, watch glass, measuring cylinder, thermometer, balance, heating source KClO₃, measuring cylinders, thermometer, burette, boiling tubes, heating source, graph paper Graph paper, ruler, pencil, calculator, data tables from textbook Calculator, graph paper, data tables, worked examples from textbook Soap solution, burette, various salt solutions, conical flasks, distilled water, tap water, rainwater, heating source Student books, examples from previous experiment, chalkboard for equations Samples of fur deposits, pictures of scaled pipes, calculator for cost analysis Hard water samples, heating source, soap solution, distillation apparatus diagram Na₂CO₃ solution, hard water samples, ion exchange resin diagram, Ca(OH)₂, NH₃ solution |
KLB Secondary Chemistry Form 4, Pages 1-3
KLB Secondary Chemistry Form 4, Pages 14-16 |
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| 1-9 |
Reporting and opener exam, Opener exam in progress, Week 9 End term exam and December Holiday |
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| 9 | 2 |
ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES
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Endothermic and Exothermic Reactions
Enthalpy Notation and Energy Content Bond Breaking and Bond Formation Latent Heat of Fusion and Vaporization Bond Energy Calculations Determination of Enthalpy of Solution I Thermochemical Equations Enthalpy of Solution of Concentrated Sulphuric Acid Enthalpy of Combustion Enthalpy of Displacement Enthalpy of Neutralization |
By the end of the
lesson, the learner
should be able to:
- Define endothermic and exothermic reactions using ΔH notation -Investigate temperature changes when ammonium nitrate and sodium hydroxide dissolve in water -Explain observations made during dissolution -Draw energy level diagrams for endothermic and exothermic reactions |
Class experiment: Wrap 250ml plastic beakers with tissue paper. Dissolve 2 spatulafuls of NH₄NO₃ in 100ml distilled water, record temperature changes. Repeat with NaOH pellets. Compare initial and final temperatures. Draw energy level diagrams showing relative energies of reactants and products.
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250ml plastic beakers, tissue paper, rubber bands, NH₄NO₃, NaOH pellets, distilled water, thermometers, spatulas, measuring cylinders
Student books, calculators, worked examples from textbook, chalkboard for calculations Crushed pure ice, 250ml glass beakers, thermometers, heating source, stopwatch, graph paper, stirring rods Data tables showing molar heats of fusion/vaporization, calculators, heating curves from previous lesson Bond energy data tables, calculators, worked examples, practice problems 250ml plastic beakers, 2.0g samples of NH₄NO₃ and NaOH, distilled water, thermometers, measuring cylinders, analytical balance, calculators Results from previous experiment, graph paper for energy level diagrams, practice examples Concentrated H₂SO₄, distilled water, 250ml plastic beaker, tissue paper, measuring cylinders, thermometer, safety equipment Ethanol, small bottles with wicks, 250ml glass beakers, tripod stands, wire gauze, thermometers, analytical balance, measuring cylinders Zinc powder, 0.5M CuSO₄ solution, 250ml plastic beakers, tissue paper, thermometers, analytical balance, stirring rods 2M HCl, 2M NaOH, 2M ethanoic acid, 2M ammonia solution, measuring cylinders, thermometers, 250ml plastic beakers, tissue paper |
KLB Secondary Chemistry Form 4, Pages 29-31
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| 9 | 3-4 |
ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES
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Standard Conditions and Standard Enthalpy Changes
Hess's Law - Introduction and Theory Energy Cycle Diagrams Hess's Law Calculations Lattice Energy and Hydration Energy Factors Affecting Lattice and Hydration Energies Definition and Types of Fuels Heating Values of Fuels Factors in Fuel Selection Environmental Effects of Fuels Fuel Safety and Precautions Endothermic and Exothermic Reactions Bond Breaking, Formation and Phase Changes Determination of Enthalpy of Solution Enthalpy of Solution of H₂SO₄ and Safety Enthalpy of Combustion Enthalpy of Displacement Enthalpy of Neutralization Standard Conditions and Standard Enthalpy Changes Hess's Law - Theory and Energy Cycles Hess's Law Calculations Lattice Energy and Hydration Energy |
By the end of the
lesson, the learner
should be able to:
- Identify standard conditions for measuring enthalpy changes -Define standard enthalpy changes using ΔH° notation -Explain importance of standard conditions -Use subscripts to denote different types of enthalpy changes - Define endothermic and exothermic reactions using the ΔH notation -Investigate what happens when ammonium nitrate and sodium hydroxide are separately dissolved in water -Define enthalpy and enthalpy change -Calculate enthalpy changes using ΔH = H(products) - H(reactants) |
Q/A: Review previous enthalpy measurements. Introduce standard conditions: 25°C (298K) and 1 atmosphere pressure (101.325 kPa). Explain ΔH° notation and subscripts (ΔH°c for combustion, ΔH°f for formation, etc.). Discuss why standard conditions are necessary for comparison. Practice using correct notation.
Class experiment: Dissolve NH₄NO₃ and NaOH separately in water, record temperature changes in Table 2.1. Explain heat absorption vs evolution. Introduce enthalpy (H) and enthalpy change (ΔH). Calculate enthalpy changes from experimental data. Draw energy level diagrams showing relative energies. |
Student books, examples of standard enthalpy data, notation practice exercises
Energy cycle diagrams for methane formation, chalkboard illustrations, worked examples from textbook Graph paper, energy cycle templates, combustion data tables, calculators Worked examples, combustion data, calculators, step-by-step calculation sheets Energy cycle diagrams, lattice energy and hydration energy data tables, calculators Data tables from textbook, calculators, trend analysis exercises Examples of different fuels, classification charts, pictures of fuel types Heating value data table, calculators, fuel comparison charts Fuel comparison tables, local fuel availability data, cost analysis sheets Pictures of environmental damage, pollution data, examples of clean technology Safety guideline charts, examples of fuel accidents, local safety case studies 250ml plastic beakers, tissue paper, NH₄NO₃, NaOH pellets, distilled water, thermometers, calculators Ice, glass beakers, thermometers, heating source, graph paper, bond energy data tables 2.0g samples of NH₄NO₃ and NaOH, plastic beakers, thermometers, analytical balance, calculators Concentrated H₂SO₄, distilled water, plastic beaker, tissue paper, thermometer, safety equipment Ethanol, bottles with wicks, glass beakers, tripod stands, thermometers, analytical balance Zinc powder, 0.5M CuSO₄ solution, plastic beakers, thermometers, analytical balance 2M HCl, 2M NaOH, 2M ethanoic acid, 2M ammonia solution, measuring cylinders, thermometers, plastic beakers Student books, standard enthalpy data examples, notation practice exercises Energy cycle diagrams for methane and CO formation, combustion data, calculators Worked examples, combustion data tables, graph paper for diagrams, calculators Energy cycle diagrams, hydration diagram (Fig 2.17), Tables 2.6 and 2.7 with lattice/hydration energies |
KLB Secondary Chemistry Form 4, Pages 49
KLB Secondary Chemistry Form 4, Pages 29-32 |
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| 9 | 5 |
ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES
ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II ORGANIC CHEMISTRY II |
Definition and Types of Fuels
Fuel Selection Factors Environmental Effects and Safety Introduction to Alkanols and Nomenclature Isomerism in Alkanols Laboratory Preparation of Ethanol Industrial Preparation and Physical Properties Chemical Properties of Alkanols I Chemical Properties of Alkanols II Uses of Alkanols and Health Effects Introduction to Alkanoic Acids Laboratory Preparation of Ethanoic Acid Physical and Chemical Properties of Alkanoic Acids Esterification and Uses of Alkanoic Acids Introduction to Detergents and Soap Preparation Mode of Action of Soap and Hard Water Effects Soapless Detergents and Environmental Effects Introduction to Polymers and Addition Polymerization Addition Polymers - Types and Properties Condensation Polymerization and Natural Polymers Polymer Properties and Applications Comprehensive Problem Solving and Integration |
By the end of the
lesson, the learner
should be able to:
- Define a fuel -Classify fuels into solid, liquid and gaseous types -Define heating value of a fuel -Calculate heating values from molar enthalpies of combustion |
Define fuel as "substance producing useful energy in chemical/nuclear reaction." Classify: solids (coal, charcoal, wood), liquids (petrol, kerosene, diesel), gases (natural gas, biogas, LPG). Define heating value as "heat energy per unit mass." Calculate for ethanol: -1360 kJ/mol ÷ 46 g/mol = 30 kJ/g. Compare values from Table 2.8.
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Examples of local fuels, Table 2.8 showing heating values, calculators
Fuel comparison tables, local fuel cost data, examples of specialized fuel applications Pictures of environmental damage, pollution reduction examples, safety guideline charts Molecular models, Table 6.1 and 6.2, alkanol structure charts, student books Isomer structure charts, molecular models, practice worksheets, student books Sugar, yeast, warm water, conical flask, delivery tube, lime water, thermometer Table 6.3, industrial process diagrams, ethene structure models, property comparison charts Ethanol, sodium metal, universal indicator, concentrated H₂SO₄, ethanoic acid, test tubes Acidified potassium chromate/manganate, ethanoic acid, concentrated H₂SO₄, heating apparatus Charts showing alkanol uses, health impact data, methylated spirit samples, discussion materials Alkanoic acid structure charts, Table 6.5 and 6.6, molecular models, student books Ethanol, KMnO₄, concentrated H₂SO₄, distillation apparatus, thermometer, round-bottom flask 2M ethanoic acid, universal indicator, Mg strip, Na₂CO₃, NaOH, phenolphthalein, test tubes Ethanoic acid, ethanol, concentrated H₂SO₄, test tubes, heating apparatus, cold water Castor oil, 4M NaOH, NaCl, evaporating dish, water bath, stirring rod, filter paper Soap samples, distilled water, hard water (CaCl₂/MgSO₄ solutions), test tubes, demonstration materials Flow charts of detergent manufacture, Table 6.9, environmental impact data, sample detergents Polymer samples, monomer structure charts, molecular models, calculators, polymer formation diagrams Various polymer samples, structure identification exercises, calculation worksheets, Table 6.10 Nylon samples, rubber samples, condensation reaction diagrams, natural polymer examples Table 6.10, polymer application samples, environmental impact studies, product examples Comprehensive problem sets, past examination papers, calculators, organic chemistry summary charts |
KLB Secondary Chemistry Form 4, Pages 56-57
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Your Name Comes Here