PROPERTIES AND TRENDS ACROSS PERIOD THREE

Chemical properties of elements in the third period.
Oxides of period 3 elements.

By the end of the lesson, the learner should be able to:
To compare reactions of elements in period 3 with water

Q/A: Review reaction of sodium, Mg, chlorine, with water.
Infer that sodium is most reactive metal; non-metals do not react with water.

The periodic table.

K.L.B. BOOK II PP. 80-81

PROPERTIES AND TRENDS ACROSS PERIOD THREE
SALTS

Chlorides of period 3 elements.
Types of salts.

By the end of the lesson, the learner should be able to:
To explain chemical behavior of their chlorides.
To describe hydrolysis reaction.
Define a salt.
Describe various types of salts and give several examples in each case.

Comparative analysis, discussion and explanation.
Descriptive approach. Teacher exposes new concepts.

The periodic table.
text book

K.L.B. BOOK II PP. 77-78
K.L.B. BOOK II P. 91

SALTS

Solubility of salts in water.

By the end of the lesson, the learner should be able to:
To test solubility of various salts in cold water/warm water.

Class experiments- Dissolve salts in 5 cc of water.
Record the solubility in a table,
Analyse the results.

Sulphates, chlorides, nitrates, carbonates of various metals.

K.L.B. BOOK II PP. 92-93

SALTS

Solubility of bases in water.

By the end of the lesson, the learner should be able to:
To test solubility of various bases in water.
To carry out litmus test on the resulting solutions.

Class experiments- Dissolve salts in 5cc of water.
Record the solubility in a table,
Carry out litmus tests.
Discuss the results.

Oxides, hydroxides, of various metals, litmus papers.

K.L.B. BOOK IIPP. 94-95

SALTS

Methods of preparing various salts.

By the end of the lesson, the learner should be able to:
To describe various methods of preparing some salts.

Experimental and descriptive treatments of preparation of salts e.g. ZnSO4, CuSO4, NaCl and Pb(NO3)2.

CuO, H2SO4, HCl, NaOH, PbCO3, dil HNO3.

K.L.B. BOOK II pp96

SALTS

Methods of preparing various salts.
Direct synthesis of a salts.

By the end of the lesson, the learner should be able to:
To describe various methods of preparing some salts.
To describe direct synthesis of a salt.
To write balanced equations for the reactions.

Experimental and descriptive treatments of preparation of salts e.g. ZnSO4, CuSO4, NaCl and Pb(NO3)2.


Group experiments- preparation of iron (II) sulphide by direct synthesis.
Give other examples of salts prepared by direct synthesis.
Students write down corresponding balanced equations.

CuO, H2SO4, HCl, NaOH, PbCO3, dil HNO3.
Iron,
Sulphur

K.L.B. BOOK II pp96
K.L.B. BOOK II P. 104

SALTS

Ionic equations.

By the end of the lesson, the learner should be able to:
To identify spectator ions in double decomposition reactions.
To write ionic equations correctly.

Q/A: Ions present in given reactants.
Deduce the products of double decomposition reactions.
Give examples of equations.
Supervised practice.

PbNO3, MgSO4 solutions.

K.L.B. BOOK II

SALTS

Effects of heat on carbonates.

By the end of the lesson, the learner should be able to:
To state effects of heat on carbonates.
To predict products resulting from heating metal carbonates.

Group experiments- To investigate effects of heat on Na2CO3, K2CO3, CaCO3, ZnCO3, PbCO3, e.t.c.
Observe various colour changes before, during and after heating.
Write equations for the reactions.

Various carbonates.

K.L.B. BOOK II PP. 108-109

SALTS

Effects of heat on nitrates.
Effects of heat on sulphates.

By the end of the lesson, the learner should be able to:
To state effects of heat on nitrates.
To predict products resulting from heating metal nitrates.

Group experiments- To investigate effects of heat on various metal nitrates.
Observe various colour changes before, during and after heating.
Write equations for the reactions.

Common metal nitrates.
Common sulphates.

K.L.B. BOOK II PP. 110-111

SALTS

Hygroscopy, Deliquescence and Efflorescence.
Uses of salts.

By the end of the lesson, the learner should be able to:
To define hygroscopic deliquescent and efflorescent salts.
To give examples of hygroscopic deliquescent and efflorescent salts.

To state uses of salts

Prepare a sample of various salts.
Expose them to the atmosphere overnight.
Students classify the salts as hygroscopic, deliquescent and / or efflorescent.

Teacher elucidates uses of salts.

K.L.B. BOOK II P. 114
K.L.B. BOOK II P. 114

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Electrical conductivity.
Molten electrolytes.

By the end of the lesson, the learner should be able to:
To test for electrical conductivities of substances.

Group experiments- to identify conductors and non-conductors.
Explain the difference in (non) conductivities.

Various solids, bulb, battery, & wires.
Molten candle wax
Sugar
Sulphur
Lead oxide.

K.L.B. BOOK II PP. 118-119

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Electrolysis.

By the end of the lesson, the learner should be able to:
To define electrolysis
To describe the process of electrolysis in terms of charge movement.

Descriptive approach punctuated with Q/A.

K.L.B. BOOK II

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Aqueous electrolytes. Electrodes.

By the end of the lesson, the learner should be able to:
To define an electrolyte
To test for electrical conductivities of electrodes.

To investigate chemical effect of an electric current.
Classify the solutions as electrolyte or non -electrolytes.
Discuss the electrical properties of the solutions.

Graphite electrodes
Battery
Various aqueous solutions switch bulb.

K.L.B. BOOK II PP.122-123

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Reaction on electrodes.
Binary electrolyte.

By the end of the lesson, the learner should be able to:
To describe half- equation reactions at the cathode and anode
To define a binary electrolyte.
To state the products of a binary electrolyte.

To demonstrate ?Electrolysis of molten lead (II) bromide
Observe colour changes
Explanation of half-equations and reactions at the electrodes.
Completing a table of electrolysis of binary electrolytes.

Graphite electrodes
Battery
Various aqueous solutions switch.
text book

K.L.B. BOOK II PP.126-127
K.L.B. BOOK II P.127

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Application of electrolysis.
Electroplating.

By the end of the lesson, the learner should be able to:
To state application of electrolysis.

Discussion and explanations.

text book
Silver nitrate
Iron nail
Complete circuit battery.

K.L.B. BOOK II P. 128

CARBON AND SOME OF ITS COMPOUNDS.

Allotropy.

By the end of the lesson, the learner should be able to:
Define allotropes and allotropy.
Identify allotropes of carbon.
Represent diamond and graphite diagrammatically.

Teacher exposes new terms.
Review covalent bond.
Discuss boding in diamond and graphite.

text book

K.L.B. BOOK II PP. 131-133

CARBON AND SOME OF ITS COMPOUNDS.

Physical and chemical properties of diamond, graphite and amorphous carbon

By the end of the lesson, the learner should be able to:
Describe physical and chemical properties of diamond, graphite and amorphous carbon.
State uses of carbon allotropes.

Discuss physical and chemical properties of diamond, graphite and amorphous carbon.
Explain the Physical and chemical properties of diamond, graphite and amorphous carbon.
Discuss uses of carbon allotropes.

Charcoal, graphite.

K.L.B. BOOK II pp 134

CARBON AND SOME OF ITS COMPOUNDS.

Burning carbon and oxygen.
Reduction properties of carbon.
Reaction of carbon with acids. Preparation of CO2.

By the end of the lesson, the learner should be able to:
Describe reaction of carbon with oxygen.
Describe reaction of carbon with acids.




Prepare CO2 in the lab.

Teacher demonstration- Prepare oxygen and pass dry oxygen into a tube containing carbon. Heat the carbon. Observe effects on limewater.
Teacher demonstration- reaction of carbon with hot conc HNO3.
Write balanced equations for the reaction.

Review effects of heat on carbonates.
Group experiments/teacher demonstration- preparation of CO2.

Carbon, limewater, tube, limewater stand& Bunsen burner.
CuO, pounded charcoal, Bunsen burner& bottle top
Conc. HNO3, limewater.

K.L.B. BOOK II PP. 134-135
K.L.B. BOOK II P.126

CARBON AND SOME OF ITS COMPOUNDS.

Properties of CO2.

By the end of the lesson, the learner should be able to:
Describe properties of CO2

Simple experiments to determine properties of CO2.

Discuss the observations.

Lime water,
Magnesium ribbon,
Universal indicator,
lit candle.

K.L.B. BOOK II PP.138-139

CARBON AND SOME OF ITS COMPOUNDS.

Chemical equations for reactions involving CO2.

By the end of the lesson, the learner should be able to:
Write balanced CO2.

Give examples of reactions. Write corresponding balanced chemical equations.

text book

K.L.B. BOOK II PP.139-140

CARBON AND SOME OF ITS COMPOUNDS.

Uses of CO2.

By the end of the lesson, the learner should be able to:
State uses of CO2

Discuss briefly the uses of CO2.

text book

K.L.B. BOOK II PP.140-1

CARBON AND SOME OF ITS COMPOUNDS.

Carbon monoxide lab preparation.
Chemical properties of carbon monoxide.
Carbonates and hydrogen carbonates.

By the end of the lesson, the learner should be able to:
To describe preparation of carbon monoxide in the lab
To write chemical equations for reactions of carbonates and hydrogen carbonates with acids.

Teacher demonstration: preparation of carbon monoxide in the lab.
Make observations.
Discuss the observations above.
Write chemical equations for the reactions.

text book

K.L.B. BOOK II PP. 142-143

CARBON AND SOME OF ITS COMPOUNDS.

Heating carbonates and hydrogen carbonates.
Extraction of sodium carbonate from trona.

By the end of the lesson, the learner should be able to:
To write equations for reaction of carbonates and hydrogen carbonates on heating.

Discuss the above observations.
Write corresponding balanced equations.

text book

K.L.B. BOOK II PP.150-151

CARBON AND SOME OF ITS COMPOUNDS.

Solvay process of preparing sodium carbonate.

By the end of the lesson, the learner should be able to:
To draw schematic diagram for extraction of sodium carbonates.

Discuss each step of the process.

Write relevant equations.

text book, chart

K.L.B. BOOK II

CARBON AND SOME OF ITS COMPOUNDS.

Importance of carbon in nature. & its effects on the environment.

By the end of the lesson, the learner should be able to:
To discuss: - Importance of carbon in nature.
&
Effects of carbon on the environment.

Discuss the carbon cycle and processes that increase/ reduce amount of CO2 in the air.
Uses of CO2 in soft drinks and fire extinguishers.

text book

K.L.B. BOOK II PP.157-158

CARBON AND SOME OF ITS COMPOUNDS.
GAS LAWS

Importance of carbon in nature. & its effects on the environment.
Boyle's Law - Introduction and Experimental Investigation

By the end of the lesson, the learner should be able to:
To discuss: - Importance of carbon in nature.
&
Effects of carbon on the environment.
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

Discuss the carbon cycle and processes that increase/ reduce amount of CO2 in the air.
Uses of CO2 in soft drinks and fire extinguishers.
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.

text book
Bicycle pump, Syringes, Gas jars, Chart showing volume-pressure relationship

K.L.B. BOOK II PP.157-158
KLB Secondary Chemistry Form 3, Pages 1-3

GAS LAWS

Boyle's Law - Mathematical Expression and Graphical Representation

By the end of the lesson, the learner should be able to:
Express Boyle's law mathematically
Apply the equation PV = constant
Plot and interpret pressure vs volume graphs
Plot pressure vs 1/volume graphs

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.

Graph papers, Scientific calculators, Chart showing mathematical expressions

KLB Secondary Chemistry Form 3, Pages 3-4

GAS LAWS

Boyle's Law - Mathematical Expression and Graphical Representation

By the end of the lesson, the learner should be able to:
Express Boyle's law mathematically
Apply the equation PV = constant
Plot and interpret pressure vs volume graphs
Plot pressure vs 1/volume graphs

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.

Graph papers, Scientific calculators, Chart showing mathematical expressions

KLB Secondary Chemistry Form 3, Pages 3-4

GAS LAWS

Boyle's Law - Numerical Problems and Applications

By the end of the lesson, the learner should be able to:
Solve numerical problems involving Boyle's law
Convert between different pressure units
Apply Boyle's law to real-life situations
Calculate volumes and pressures using P₁V₁ = P₂V₂

Worked examples: Demonstrate step-by-step problem solving. Supervised practice: Students solve problems involving pressure and volume calculations. Convert units (mmHg, atm, Pa). Discuss applications in tire inflation, aerosol cans. Assignment: Additional practice problems.

Scientific calculators, Worked example charts, Unit conversion tables

KLB Secondary Chemistry Form 3, Pages 4-5

GAS LAWS

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:
Solve numerical problems involving Boyle's law
Convert between different pressure units
Apply Boyle's law to real-life situations
Calculate volumes and pressures using P₁V₁ = P₂V₂
State Charles's law
Convert temperatures between Celsius and Kelvin scales
Define absolute zero temperature
Explain the concept of absolute temperature

Worked examples: Demonstrate step-by-step problem solving. Supervised practice: Students solve problems involving pressure and volume calculations. Convert units (mmHg, atm, Pa). Discuss applications in tire inflation, aerosol cans. Assignment: Additional practice problems.
Teacher demonstration: Flask with colored water column experiment. Q/A: Observe volume changes with temperature. Exposition: Introduce Kelvin scale and absolute zero concept. Practice: Temperature conversions between °C and K. Discuss absolute zero and ideal gas concept.

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 4-5
KLB Secondary Chemistry Form 3, Pages 6-8

GAS LAWS

Charles's Law - Experimental Investigation and Mathematical Expression

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

KLB Secondary Chemistry Form 3, Pages 8-10

GAS LAWS

Charles's Law - Experimental Investigation and Mathematical Expression

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

KLB Secondary Chemistry Form 3, Pages 8-10

GAS LAWS

Charles's Law - Numerical Problems and Applications

By the end of the lesson, the learner should be able to:
Solve numerical problems using Charles's law
Apply V₁/T₁ = V₂/T₂ in calculations
Predict gas behavior with temperature changes
Relate Charles's law to everyday phenomena

Worked examples: Step-by-step problem solving with temperature conversions. Supervised practice: Calculate volumes at different temperatures. Discuss applications: hot air balloons, tire pressure changes, weather balloons. Assignment: Practice problems with real-life contexts.

Scientific calculators, Temperature conversion charts, Application examples

KLB Secondary Chemistry Form 3, Pages 10-12

GAS LAWS

Charles's Law - Numerical Problems and Applications
Combined Gas Law and Standard Conditions

By the end of the lesson, the learner should be able to:
Solve numerical problems using Charles's law
Apply V₁/T₁ = V₂/T₂ in calculations
Predict gas behavior with temperature changes
Relate Charles's law to everyday phenomena
Derive the combined gas law equation
Apply PV/T = constant in problem solving
Define standard temperature and pressure (s.t.p)
Define room temperature and pressure (r.t.p)

Worked examples: Step-by-step problem solving with temperature conversions. Supervised practice: Calculate volumes at different temperatures. Discuss applications: hot air balloons, tire pressure changes, weather balloons. Assignment: Practice problems with real-life contexts.
Q/A: Combine Boyle's and Charles's laws. Teacher exposition: Derive P₁V₁/T₁ = P₂V₂/T₂. Define s.t.p (273K, 760mmHg) and r.t.p (298K, 760mmHg). Worked examples: Problems involving changes in all three variables. Supervised practice: Complex gas law calculations.

Scientific calculators, Temperature conversion charts, Application examples
Scientific calculators, Combined law derivation charts, Standard conditions reference table

KLB Secondary Chemistry Form 3, Pages 10-12
KLB Secondary Chemistry Form 3, Pages 12-14

GAS LAWS

Introduction to Diffusion - Experimental Investigation

By the end of the lesson, the learner should be able to:
Define diffusion process
Investigate diffusion in liquids and gases
Compare rates of diffusion in different media
Explain diffusion using kinetic theory

Class experiments: (a) KMnO₄ crystal in water - observe spreading over time. (b) Bromine vapor in gas jars - observe color distribution. (c) Ammonia gas in combustion tube with litmus paper. Record observations over time. Discuss particle movement and kinetic energy.

KMnO₄ crystals, Bromine liquid, Gas jars, Combustion tube, Litmus papers, Stopwatch

KLB Secondary Chemistry Form 3, Pages 14-16

GAS LAWS

Introduction to Diffusion - Experimental Investigation

By the end of the lesson, the learner should be able to:
Define diffusion process
Investigate diffusion in liquids and gases
Compare rates of diffusion in different media
Explain diffusion using kinetic theory

Class experiments: (a) KMnO₄ crystal in water - observe spreading over time. (b) Bromine vapor in gas jars - observe color distribution. (c) Ammonia gas in combustion tube with litmus paper. Record observations over time. Discuss particle movement and kinetic energy.

KMnO₄ crystals, Bromine liquid, Gas jars, Combustion tube, Litmus papers, Stopwatch

KLB Secondary Chemistry Form 3, Pages 14-16

GAS LAWS

Rates of Diffusion - Comparative Study

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

KLB Secondary Chemistry Form 3, Pages 16-18

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
State Graham's law of diffusion
Express Graham's law mathematically
Relate diffusion rate to molecular mass and density
Explain the inverse relationship between rate and √molecular mass

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.
Teacher exposition: Graham's law statement and mathematical derivation. Discussion: Rate ∝ 1/√density and Rate ∝ 1/√molecular mass. Derive comparative expressions for two gases. Explain relationship between density and molecular mass. Practice: Identify faster diffusing gas from molecular masses.

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
KLB Secondary Chemistry Form 3, Pages 18-20

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

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