ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Endothermic and Exothermic Reactions.
Energy level diagrams.
Enthalpy Notation. Change of state.
CAT
Molar heat of solution.
Molar heat of solution of H2SO4.

By the end of the lesson, the learner should be able to:
To differentiate between endothermic & exothermic reactions.
Represent endothermic reactions with exothermic reactions with energy level diagrams.
Define the term enthalpy.
Distinguish positive enthalpy change from negative enthalpy change.
Determine the M.P/ B.P of a pure substance.

Determine molar heat of solution of given substances.
Determine molar heat of solution of H2SO4.

Investigate temperature changes in solution formation.
Obtain changes in temperature when ammonium nitrate and sodium hydroxide are dissolved in water, one at a time.
Probing questions on relative energies of reactants and products in endothermic and exothermic and endothermic reactions.
Q/A and brief discussion.
Class experiments: determine B.P of pure water/ M.P of naphthalene / ice.
Use experimental results to plot temperature-time graphs.
Explain the shape of the graphs.
Q/A: review kinetic theory of matter.
Apply the theory to explain the shape of the graph, and nature of bonding in substances.
Dissolve known masses of ammonia nitrate / sodium hydroxide in known volumes of water.
Determine temperature changes.
Calculate molar heat of solution. Supervised practice.
Dissolve some known volume of conc. H2SO4 in a given volume of water.
Note the change in temperature.
Work out the molar heat of solution of H2SO4.

Ammonium nitrate,
Sodium hydroxide, thermometers.
student book
Ice, naphthalene, thermometers, graph papers.
Ammonia nitrate / sodium hydroxide, thermometers.
Conc. H2SO4, thermometers.

K.L.B. BK IV
Pages 32-33
K.L.B. BK IV
Pages 35-39

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.

Enthalpy of combustion. Enthalpy of combustion.
Molar heat of displacement of ions.
Molar heat of solution of neutralization.
Standard enthalpy changes.

By the end of the lesson, the learner should be able to:
Define the term enthalpy of combustion.
Determine the enthalpy of combustion of ethanol.
Explain why actual heats of combustion are usually lower than the theoretical values.
Define the term molar heat of solution of displacement of ions.
Determine the molar heat of solution of displacement of ions.
Define the term neutralization.
Determine the molar heat of neutralization of HCl with NaOH.
Define the term standard enthalpy change.
Denote standard enthalpy change with the correct notation.

Group experiments / teacher demonstration.
Obtain and record results.
Work out calculations.
Group experiments/ teacher demonstration.
Note steady temperature of solutions formed when zinc/ iron / magnesium reacts with copper sulphate solution.
Work out the molar heat of displacement of a substance from a solution of its ions.
Class experiments:
Neutralize 2M HCl of known volume with a determined volume of 1M / 2M sodium hydroxide.
Note highest temperature of the solution.
Work out the molar heat of neutralization.
Solve other related problems.
Assignment.
Exposition & brief discussion.

Ethanol, distilled water, thermometer, clear wick, tripod stand and wire gauze.
Zinc, iron, magnesium, copper sulphate solution.
2M HCl of known volume, 1M / 2M sodium hydroxide.
student book

K.L.B. BK IV
Pages 45-48

ENERGY CHANGES IN PHYSICAL & CHEMICAL PROCESSES.
ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Hess?s Law.
Heat of solution hydration energy and lattice energy.
Heat values of fuels.
Environmental effects of fuels.
Physical properties of alkanols.

By the end of the lesson, the learner should be able to:
State Hess?s law.
Solve problems related to Hess?s law.
Define the terms lattice energy and hydration energy.
Explain the relationship between heat of solution, hydration energy.
Solve related problems.
Define the term fuel.
Describe energy changes when a fuel undergoes combustion.
Outline factors considered when choosing a suitable fuel.
Outline some environmental effects of fuels.
Identify measures taken to reduce environmental
pollution.
Explain the physical properties of alkanols.

Detailed discussion & guided discovery of the law.
Illustrations of energy cycles and energy levels leading to Hess?s law.
Worked examples.
Supervised practice
Written assignment.
Exposition of new concepts.
Guided discovery of the relationship between heat solution hydration energy and lattice energy.
Assignment.
Probing questions and brief discussion.
Q/A & open discussion.
Comparative evaluation of physical properties of alkanols.
Q/A & discussion on variation in physical properties of alkanols.

student book

K.L.B. BK IV
Pages 56-57

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)

Chemical properties of alkanols.
Esters and esterification.
Oxidation of ethanol. Uses of alkanols.
Alkanoic (Carboxylic Acids).
Nomenclature of alkanoic acids.

By the end of the lesson, the learner should be able to:
Describe some chemical reactions of alkanols.
Explain formation of esters.
Describe the esterification process.
Explain oxidation of ethanol by an oxidizing agent.
State uses of alkanols.
Explain the effects of alcohol on human health
Identify the functional group of alkanoic (carboxylic) acids.
Explain formation of alkanoic acid molecule.
Name and draw the structure of simple alkanoic acids.

Group experiments/ teacher demonstration to investigate combustion of ethanol and its reaction with metals.
Write corresponding chemical equations.
Teacher exposes and explains new concepts.
Assignment.
Q/A: review redox reactions, oxidizing and reducing agents.
Brief discussion: oxidation of ethanol using potassium (VII) manganate or potassium (VI) dichromate.
Write corresponding chemical equations.
Open discussion.
Q/A: review functional group of alkanols.
Brief discussion.
Guided discovery of the naming system for alkanoic acids.

student book
Chart: homologous series of alkanoic acids.

K.L.B. BK IV
Pages 213-5

ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)
ORGANIC CHEMISTRY II (ALKANES & ALKANOIC ACIDS)
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY

Lab preparation of ethanoic acid.
Physical properties of alkanoic acids.
Chemical properties of alkanoic acids.
Chemical properties & Uses of alkanoic acids.
Soap preparation in the lab.
Cleaning action of soap.
Effects of hard / soft water on soap.
Soapless detergents.
Polymers and polymerization.
Definition of radioactivity.
Alpha particles.
Equations involving alpha particles.
Beta particles. Gamma rays.
Radioactive Half-Life.
Radioactive decay curve.
Nuclear fusion and nuclear fission. Applications of radioactivity.

By the end of the lesson, the learner should be able to:
Describe laboratory preparation of ethanoic acid.
Explain some physical properties of alkanoic acids.
Explain some chemical properties of alkanoic acids.
Write equations for chemical reactions involving acids.
State uses of alkanoic acids.
Describe soap preparation in the lab.
Describe the nature of a soap molecule.
Explain the mode of action in cleaning.
Explain the effects of hard/ soft water on soap.
Prepare soapless detergents in the lab.
State merits of soapless detergents over soaps.
Explain the concepts additional and condensation polymerization as methods of making synthetic polymers.
Identify some products of polymerization.
State merits and demerits of synthetic polymers over natural materials.
Define radioactivity, a nuclide and radioactive decay.
Differentiate between natural and artificial radioactivity.
State properties of alpha particles.
Describe methods of detecting alpha particles.
Write down and balance equations involving alpha particles.
State properties of beta particles.
Define isotopes and isobars.
Write down balanced equations involving both alpha and beta particles.
State properties of gamma rays.
Define the term radioactive half-life. Solve problems relating to half ?life
Plot a radioactive decay curve to deduce the
half ?life from the curve.
Differentiate between nuclear fusion and nuclear fission.
Describe applications of radioactivity.

Teacher demonstration: prepare ethanoic acid in the lab.
Brief discussion on preparation of ethanoic acid.
Compare physical properties of some alkanoic acids.
Discuss the difference in physical properties among alkanoic acids.
Group experiment: investigate some chemical properties of ethanoic acid.
Carry out tests and record observations in a table.
Review and discuss the observations above.
Write corresponding chemical equations.
Teacher elucidates uses of alkanoic acids.
Group experiments,
Answer questions based on the experiments already carried out.
Expository and descriptive approaches.
Answer oral questions.
Group experiments: form soap lather in different solutions.
Deduce the effects of hard/ soft water on soap.
Teacher demonsration.
Brief discussion.
Teacher exposes and explains new concepts.
Detailed discussion.
Assignment.
Q/A: Review the atomic structure.
Exposition: symbolic representation of an atom / nucleus.
Exposition: meaning of radioactivity and radioactive decay.
Discussion: artificial and natural radioactivity.

Q/A: position of helium in the periodic table.
Expository approach:
Q/A: Review atomic and mass numbers.
Examples of balanced equations.
Supervised practice.
Q/A: Review isotopes.
Expository approach: teacher briefly exposes new concepts.
Examples of equations.
Supervised practice.
Teacher demonstration: Dice experiment.
Exposition of the term half-life.
Worked examples.
Written exercise
Drawing a radioactive decay curve inferring the half-life of the sample from the graph.
Exposition of new concepts accompanied by nuclear equations.
Brief discussion: Carbon dating, detecting leakage, medication, agriculture, industry; effect of static charges, etc.

Concentrated H2SO4, potassium manganate
(VII) Crystals, water bath.
student book
Ethanoic acid, universal indicator, sodium carbonate, magnesium strip, ethanol, conc. H2SO4 and sodium hydroxide.
student book
Distilled water, tap water, rainwater, sodium chloride solution.
Calcium nitrate, Zinc Sulphate, etc.
Dice.
Graph papers.

K.L.B. BK IV
Pages 221-223
K.L.B. BK IV
Pages 230-232