THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Atomic and mass numbers.
First twenty elements of the periodic table.
Isotopes.

By the end of the lesson, the learner should be able to:
Name the subatomic particles in an atom.
Define atomic number and mass number of an atom.
Represent atomic and mass numbers symbolically.
List the first twenty elements of the periodic table.
Write chemical symbols of the first twenty elements of the periodic table.
Define isotopes.
Give examples of isotopes.

Exposition on new concepts;
Probing questions;
Brief discussion.
Expository approach: referring to the periodic table, teacher exposes the first twenty elements.
Writing down a list of first twenty elements of the periodic table.
Exposition of definition and examples of isotopes.
Giving examples of isotopes.

text book
Periodic table.
Periodic table.

K.L.B.
BOOK II

PP. 1-3
K.L.B.
BOOK II
P. 4





PP. 5-8

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Electronic configuration.
Electronic configuration in diagrams.

By the end of the lesson, the learner should be able to:
Represent isotopes symbolically.
Define an energy level.
Describe electronic configuration in an atom.
Represent electronic configuration diagrammatically.

Exposition ? teacher exposes new concepts about electronic configuration.
Written exercise.
Supervised practice;

Periodic table.
text book

K.L.B.
BOOK II
P. 4





PP. 5-9

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Periods of the periodic table.

By the end of the lesson, the learner should be able to:
Identify elements of the same period.

Exposition ? Definition of a period.
Q/A: Examples of elements of the same period.

Periodic table.

K.L.B. BOOK IIP. 9

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Groups of the periodic table.
R.M.M. and isotopes.
Positive ions and ion formation.

By the end of the lesson, the learner should be able to:
Identify elements of the same period.
Calculate R.M.M. from isotopic composition.
To define an ion and a cation.

Exposition ? definition of a group.
Q/A: examples of elements of the same group.
Supervised practice involving calculation of RMM from isotopic composition.

Teacher gives examples of stable atoms.
Guided discovery that metals need to lose one, two or three electrons to attain stability.
Examples of positive ions.

Periodic table.
text book

K.L.B. BOOK IIP. 9
K.L.B. BOOK IIPP. 11-13

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Positive ions representation.

By the end of the lesson, the learner should be able to:
To represent formation of positive ions symbolically.

Diagrammatic representation of cations.

Chart  ion model.

K.L.B. BOOK IIP 16

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Negative ions and ion formation.
Valencies of metals.

By the end of the lesson, the learner should be able to:
To define an anion.
To describe formation of negative ions symbolically.
Recall valencies of metals among the first twenty elements in the periodic table.

Teacher gives examples of stable atoms.
Guided discovery of formation of negative ions.
Diagrammatic representation of anions.
Q/A to review previous lesson;
Exposition;
Guided discovery.

Chart  ion model.
Periodic table.

K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Valencie of non-metals.
Valencies of radicals.
Oxidation number.

By the end of the lesson, the learner should be able to:
Recall valencies of non-metals among the first twenty elements in the periodic table.
Define a radical.
Recall the valencies of common radicals.
Define oxidation number.
Predict oxidation numbers from position of elements in the periodic table.

Q/A to review previous lesson;
Exposition;
Guided discovery.

Exposition ? teacher defines a radical, gives examples of radicals and exposes their valencies.
Students draw a table of radicals and their valencies.
Q/A: Valencies.
Expose oxidation numbers of common ions.
Students complete a table of ions and their oxidation numbers.

Periodic table.
text book
The periodic table.

K.L.B. BOOK IIP 17
K.L.B. BOOK IIP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Electronic configuration, ion formed, valency and oxidation number

By the end of the lesson, the learner should be able to:
Relate electronic configuration, ion formed, valency and oxidation number of different elements.

Written exercise;
Exercise review.

text book

K.L.B. BOOK IIP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Chemical formulae of compounds. - Elements of equal valencies.

By the end of the lesson, the learner should be able to:
To derive the formulae of some compounds involving elements of equal valencies.

Discuss formation of compounds such as NaCl, MgO.

text book

K.L.B. BOOK IIPP 19-20

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Chemical formulae of compounds. -Elements of unequal valencies.
Chemical formulae of compounds. -Elements of variable valencies.
Chemical equations.

By the end of the lesson, the learner should be able to:
To derive the formulae of some compounds involving elements of unequal valencies.
To derive the formulae of some compounds involving elements of variable valencies.
To identify components of chemical equations.

Discuss formation of compounds such as MgCl2
Al (NO3)3
Discuss formation of compounds such as
-Copper (I) Oxide.
-Copper (II) Oxide.
-Iron (II) Sulphate.
-Iron (III) Sulphate.
Review word equations;
Exposition of new concepts with probing questions;
Brief discussion.

text book

K.L.B. BOOK IIPP 19-20
K.L.B. BOOK IIPP 21-23

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Balanced chemical equations.
Balanced chemical equations.(contd)

By the end of the lesson, the learner should be able to:
To balance chemical equations correctly.

Exposition;
Supervised practice.
Supervised practice;
Written exercise.

text book

K.L.B. BOOK IIPP 24-25

CHEMICAL FAMILIES

Alkali metals. Atomic and ionic radii of alkali metals

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





Identify alkali metals.
State changes in atomic and ionic radii of alkali metals.

Q/A to reviews elements of group I and their electronic configuration.
Examine a table of elements, their symbols and atomic & ionic radii.
Discussion & making deductions from the table.

The periodic

K.L.B. BOOK IIPP 28-29

CHEMICAL FAMILIES

Ionisation energy of alkali metals.
Physical properties of alkali metals.
Chemical properties of alkali metals.

By the end of the lesson, the learner should be able to:
State changes in number of energy levels and ionisation energy of alkali metals.
State and explain trends in physical properties of alkali metals.
To describe reaction of alkali metals with water.

Examine a table of elements, number of energy levels and their ionization energy.
Discuss the trend deduced from the table.
Examine a table showing comparative physical properties of Li, Na, and K.
Q/A: Teacher asks probing questions as students refer to the table for answers.
Detailed discussion on physical properties of alkali metals.

Q/A: Review reaction of metals with water.
Writing down chemical equations for the reactions.
Deduce and discuss the order of reactivity down the group.

text book
Chart ? comparative properties of Li, Na, K.

K.L.B. BOOK II
K.L.B. BOOK IIP. 32

CHEMICAL FAMILIES

Reaction of alkali metals with chlorine gas.

By the end of the lesson, the learner should be able to:
To write balanced equations for reaction of alkali metals with chlorine gas.

Teacher demonstration- reaction of sodium with chlorine in a fume chamber.
Q/A: Students to predict a similar reaction between potassium and chlorine.
Word and balanced chemical equations for various reactions.

Sodium, chlorine.

K.L.B. BOOK IIP. 33

CHEMICAL FAMILIES

Compounds of alkali metals.
Uses of alkali metals.

By the end of the lesson, the learner should be able to:
Write chemical formulae for compounds of alkali metals.
Explain formation of hydroxides, oxides and chlorides of alkali metals.
State uses of alkali metals.

Exercise: Completing a table of hydroxides, oxides and chlorides of alkali metals.
Discuss combination of ions of alkali metals with anions.
Descriptive approach: Teacher elucidates uses of alkali metals.

text book

K.L.B. BOOK II pp 33

CHEMICAL FAMILIES

Alkaline Earth metals Atomic and ionic radii of alkaline earth metals.
Physical properties of alkaline earth metals.
Electrical properties of alkaline earth metals.

By the end of the lesson, the learner should be able to:
Identify alkaline earth metals.

State changes in atomic and ionic radii of alkaline earth metals.
State and explain trends in physical properties of alkaline earth metals.
To describe electrical properties of alkaline earth metals.

Q/A: Elements of group I and their electron configuration.
Examine a table of elements, their symbols and atomic & ionic radii.
Make deductions from the table.

Examine a table showing comparative physical properties of Be, Mg, Ca.
Q/A: Teacher asks probing questions as students refer to the table for answers.
Detailed discussion of physical properties of alkaline earth metals.
Teacher demonstration: -
To show alkaline metals are good conductors of electric charge.

Some alkaline earth metals.
Some alkaline earth metals.
Alkaline earth metals.

K.L.B. BOOK II pp 34
K.L.B. BOOK II P. 35

STRUCTURE & BONDING

Chemical bonds. Ionic bond.
Ionic bond representation.
Grant ionic structures.
Physical properties of ionic compounds.

By the end of the lesson, the learner should be able to:
Describe role of valence electrons in determining chemical bonding.
Explain formation of ionic bonding.
Use dot and cross diagrams to represent ionic bonding.
Describe the crystalline ionic compound.
Give examples of ionic substances.
Describe physical properties of ionic compounds.
Explain the differences in the physical properties of ionic compounds.

Q/A: Review valence electrons of atoms of elements in groups I, II, III, VII and VIII.
Q/A: Review group I and group VII elements.
Discuss formation of ionic bond.
Drawing diagrams of ionic bonds.
Discuss the group ionic structures of NaCl.
Teacher gives examples of other ionic substances: KNO3, potassium bromide, Ca (NO3)2, sodium iodide.
Analyse tabulated comparative physical properties of ionic compounds.
Teacher asks probing questions.

text book
Chart- dot and cross diagrams.
Models for bonding.
Giant sodium chloride model.

K.L.B. BOOK IIP54




PP 57-58

STRUCTURE & BONDING

Covalent bond.
Co-ordinate bond.
Molecular structure.

By the end of the lesson, the learner should be able to:
Explain the formation of covalent bond
Use dot and cross diagrams to represent covalent bond.
To describe the co-ordinate bond
To represent co-ordinate bond diagrammatically.
To describe the molecular structure.
To give examples of substance exhibiting molecular structure

Exposition: Shared pair of electrons in a hydrogen molecule, H2O, NH3, Cl2, and CO2.
Drawing of dot-and-cross diagrams of covalent bonds.
Exposition- teacher explains the nature of co-ordinate bond.
Students represent co-ordinate bond diagrammatically.
Discussion ? To explain formation of the giant structure and give examples of substance exhibiting molecular structure.

text book

K.L.B. BOOK II PP 60-63

STRUCTURE & BONDING
STRUCTURE & BONDING
PROPERTIES AND TRENDS ACROSS PERIOD THREE

Trend in physical properties of molecular structures.
Giant atomic structure in diamond.
Giant atomic structure in graphite.
Metallic bond. Uses of some metals.
Physical properties of elements in periods.

By the end of the lesson, the learner should be able to:
To describe van- der -waals forces.
To explain the trend in physical properties of molecular structures.
To describe giant atomic structure in diamond.
To state uses of diamond.
To describe giant atomic structure in graphite.
To state uses of graphite.
To describe mutual electronic forces between electrons and nuclei.
To describe metallic bond.
To compare physical properties of metals.
To state uses of some metals.
To compare electrical conductivity of elements in period 3

Discuss comparative physical properties of substances. exhibiting molecular structure.
Explain variation in the physical properties.
Diagrammatic representation of diamond.
Discuss uses of diamond.
Diagrammatic representation of graphite.
Discuss uses of graphite.
Discussion:
Detailed analysis of comparative physical properties of metals and their uses.
Probing questions & brief explanations.
Group experiments- Construct electrical circuits incorporating a magnesium ribbon, then aluminum foil, then sulphur in turns.
The brightness of the bulb is noted in each case.
Discuss the observations in terms of delocalised electrons.

Sugar, naphthalene, iodine rhombic sulphur.
Diagrams in textbooks.
text book
The periodic table.

K.L.B. BOOK IIP 65
K.L.B. BOOK IIP 70

PROPERTIES AND TRENDS ACROSS PERIOD THREE

Physical properties of elements in period 3.
Chemical properties of elements in period 3.
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 other physical properties of elements across period 3.
To compare reactions of elements in period 3 with oxygen.
To compare reactions of elements in period 3 with water
To identify bonds across elements in period 3.
To explain chemical behavior of their oxide.

Analyse comparative physical properties presented in form of a table.
Explain the trend in the physical properties given.
Q/A: Products of reactions of Na, Mg, Al, P, & S with oxygen.
Discuss the trend in their reactivity; identify basic and acidic oxides.
Exercise ? balanced chemical equations for the above reactions.
Q/A: Review reaction of sodium, Mg, chlorine, with water.
Infer that sodium is most reactive metal; non-metals do not react with water.
Comparative analysis, discussion and explanation.

The periodic table.

K.L.B. BOOK II P. 77

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

SALTS

Solubility of salts in water.
Solubility of bases in water.
Methods of preparing various salts.
Direct synthesis of a salts.

By the end of the lesson, the learner should be able to:
To test solubility of various salts in cold water/warm water.
To test solubility of various bases in water.
To carry out litmus test on the resulting solutions.
To describe various methods of preparing some salts.
To describe direct synthesis of a salt.
To write balanced equations for the reactions.

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

Sulphates, chlorides, nitrates, carbonates of various metals.
Oxides, hydroxides, of various metals, litmus papers.
CuO, H2SO4, HCl, NaOH, PbCO3, dil HNO3.
Iron,
Sulphur

K.L.B. BOOK II PP. 92-93
K.L.B. BOOK II pp96

SALTS

Ionic equations.
Effects of heat on carbonates.
Effects of heat on nitrates.

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.
To state effects of heat on carbonates.
To predict products resulting from heating metal carbonates.
To state effects of heat on nitrates.
To predict products resulting from heating metal nitrates.

Q/A: Ions present in given reactants.
Deduce the products of double decomposition reactions.
Give examples of equations.
Supervised practice.
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.
Group experiments- To investigate effects of heat on various metal nitrates.

PbNO3, MgSO4 solutions.
Various carbonates.
Common metal nitrates.

K.L.B. BOOK II

SALTS

Effects of heat on sulphates.
Hygroscopy, Deliquescence and Efflorescence.
Uses of salts.

By the end of the lesson, the learner should be able to:
To state effects of heat on sulphates.
To predict products results from heating metal sulphates.
To define hygroscopic deliquescent and efflorescent salts.
To give examples of hygroscopic deliquescent and efflorescent salts.
To state uses of salts

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

Common sulphates.

K.L.B. BOOK II P. 113

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Electrical conductivity.
Molten electrolytes.
Electrolysis.
Aqueous electrolytes. Electrodes.
Reaction on electrodes.
Binary electrolyte.

By the end of the lesson, the learner should be able to:
To test for electrical conductivities of substances.
To test for electrical conductivities molten electrolytes.
To define electrolysis
To describe the process of electrolysis in terms of charge movement.
To define an electrolyte
To test for electrical conductivities of electrodes.
To describe half- equation reactions at the cathode and anode
To define a binary electrolyte.
To state the products of a binary electrolyte.

Group experiments- to identify conductors and non-conductors.
Explain the difference in (non) conductivities.
Group experiments- to identify electrolytes in molten form.
Explain the difference in molten electrolytes.
Descriptive approach punctuated with Q/A.
To investigate chemical effect of an electric current.
Classify the solutions as electrolyte or non -electrolytes.
Discuss the electrical properties of the solutions.
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.

Various solids, bulb, battery, & wires.
Molten candle wax
Sugar
Sulphur
Lead oxide.
Graphite electrodes
Battery
Various aqueous solutions switch bulb.
Various aqueous solutions switch.
text book

K.L.B. BOOK II PP. 118-119
K.L.B. BOOK II PP.122-123

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
CARBON AND SOME OF ITS COMPOUNDS.

Application of electrolysis.
Electroplating.
Allotropy.

By the end of the lesson, the learner should be able to:
To state application of electrolysis.
To describe electroplating process.
Define allotropes and allotropy.
Identify allotropes of carbon.
Represent diamond and graphite diagrammatically.

Discussion and explanations.
Experiment- Left overnight.
Electroplating an iron nail with silver nitrate/ copper sulphate.
Brief discussion.
Teacher exposes new terms.
Review covalent bond.
Discuss boding in diamond and graphite.

text book
Silver nitrate
Iron nail
Complete circuit battery.

K.L.B. BOOK II P. 128

CARBON AND SOME OF ITS COMPOUNDS.

Physical and chemical properties of diamond, graphite and amorphous carbon
Burning carbon and oxygen.
Reduction properties of 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.
Describe reaction of carbon with oxygen.
Describe reduction properties of carbon.
Show reduction properties of carbon.

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.
Teacher demonstration- Prepare oxygen and pass dry oxygen into a tube containing carbon. Heat the carbon. Observe effects on limewater.
Teacher demonstration ? Burn strongly a mixture of carbon and CuO on a bottle top.
Observe colour changes and give underlying explanation

Charcoal, graphite.
Carbon, limewater, tube, limewater stand& Bunsen burner.
CuO, pounded charcoal, Bunsen burner& bottle top

K.L.B. BOOK II pp 134

CARBON AND SOME OF ITS COMPOUNDS.

Reaction of carbon with acids. Preparation of CO2.
Properties of CO2.
Chemical equations for reactions involving CO2.
Uses of CO2.
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:
Describe reaction of carbon with acids.
Prepare CO2 in the lab.
Describe properties of CO2
Write balanced CO2.
State uses of CO2
To describe preparation of carbon monoxide in the lab
To describe chemical properties of carbon monoxide.
To write chemical equations for reactions of carbonates and hydrogen carbonates with acids.

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.
Simple experiments to determine properties of CO2.
Discuss the observations.
Give examples of reactions. Write corresponding balanced chemical equations.
Discuss briefly the uses of CO2.
Teacher demonstration: preparation of carbon monoxide in the lab.
Make observations.
Description of properties of carbon monoxide.
Discussion and writing of chemical equations.
Discuss the observations above.
Write chemical equations for the reactions.

Conc. HNO3, limewater.
Lime water,
Magnesium ribbon,
Universal indicator,
lit candle.
text book

K.L.B. BOOK II P.126
K.L.B. BOOK II PP.140-1

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.
To draw schematic diagram for extraction of sodium carbonates.

Discuss the above observations.
Write corresponding balanced equations.
Discuss each step of the process.
Write relevant equations.

text book

K.L.B. BOOK II PP.150-151

CARBON AND SOME OF ITS COMPOUNDS.

Solvay process of preparing sodium carbonate.
Importance of carbon in nature. & its effects on the environment.

By the end of the lesson, the learner should be able to:
To draw schematic diagram for extraction of sodium carbonates.
To discuss: - Importance of carbon in nature.
&
Effects of carbon on the environment.

Discuss each step of the process.
Write relevant equations.
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, chart
text book

K.L.B. BOOK II