THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Atomic and mass numbers.

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.

Exposition on new concepts;
Probing questions;
Brief discussion.

text book

K.L.B.
BOOK II

PP. 1-3

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

First twenty elements of the periodic table.

By the end of the lesson, the learner should be able to:
List the first twenty elements of the periodic table.
Write chemical symbols of the first twenty elements of the periodic table.

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.

Periodic table.

K.L.B.
BOOK II

PP. 1-3

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Isotopes.
Electronic configuration.
Electronic configuration in diagrams.

By the end of the lesson, the learner should be able to:
Define isotopes.
Give examples of isotopes.

Represent electronic configuration diagrammatically.

Exposition of definition and examples of isotopes.
Giving examples of isotopes.

Supervised practice;
Written exercise.

Periodic table.
text book

K.L.B.
BOOK II
P. 4





PP. 5-8
K.L.B.
BOOK II
PP. 5-8

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.

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

Exposition ? definition of a group.
Q/A: examples of elements of the same group.

Periodic table.

K.L.B. BOOK IIP. 9

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

R.M.M. and isotopes.
Positive ions and ion formation.
Positive ions representation.

By the end of the lesson, the learner should be able to:
Calculate R.M.M. from isotopic composition.

To define an ion and a cation.

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.

text book
text book
Chart  ion model.

K.L.B. BOOK IIPP. 11-13
K.L.B. BOOK IIPP 14-15

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Negative ions and ion formation.

By the end of the lesson, the learner should be able to:
To define an anion.
To describe formation of negative ions symbolically.

Teacher gives examples of stable atoms.
Guided discovery of formation of negative ions.
Diagrammatic representation of anions.

Chart  ion model.

K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Valencies of metals.

By the end of the lesson, the learner should be able to:
Recall valencies of metals among the first twenty elements in the periodic table.

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

Periodic table.

K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Valencie of non-metals.
Valencies of radicals.

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.

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.

Periodic table.
text book

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

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Oxidation number.
Electronic configuration, ion formed, valency and oxidation number

By the end of the lesson, the learner should be able to:
Define oxidation number.
Predict oxidation numbers from position of elements in the periodic table.

Q/A: Valencies.
Expose oxidation numbers of common ions.
Students complete a table of ions and their oxidation numbers.

The periodic table.
text book

K.L.B. BOOK IIvP 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.

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.

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.

text book

K.L.B. BOOK IIPP 19-20
K.L.B. BOOK IIP 20

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Chemical equations.

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

Review word equations;
Exposition of new concepts with probing questions;
Brief discussion.

text book

K.L.B. BOOK IIPP 21-23

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Balanced chemical equations.

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

Exposition;
Supervised practice.

text book

K.L.B. BOOK IIPP 24-25

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
CHEMICAL FAMILIES

Balanced chemical equations.(contd)
Chemical properties of alkaline earth metals. Reaction of alkaline earth metals with oxygen.
Chemical properties of alkaline earth metals. Reaction of alkaline earth metals with water.

By the end of the lesson, the learner should be able to:
To balance chemical equations correctly.
To describe reaction of alkaline earth metals with water.

Supervised practice;
Written exercise.
Q/A: Review reaction of metals with water.
Writing down word and balanced chemical equations for the reactions.
Deduce and discuss the order of reactivity down the group.

text book
Some alkaline earth metals.

K.L.B. BOOK IIPP 25-8
K.L.B. BOOK IIP. 39

CHEMICAL FAMILIES

Reaction of alkaline earth metals with chlorine gas.

By the end of the lesson, the learner should be able to:
To write balanced equations for reaction of alkaline earth 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.
Supervised practice.

Sodium, chlorine.

K.L.B. BOOK II P. 41

CHEMICAL FAMILIES

Reaction of alkaline earth metals with dilute acids.

By the end of the lesson, the learner should be able to:
To write balanced equations for reactions of alkaline earth metals with dilute acids.

Changing word to chemical equations.
Supervised practice.

revision book

K.L.B. BOOK II PP. 43

CHEMICAL FAMILIES

Chemical formulae of alkaline earth metals.
Uses of some alkaline earth metals and their compounds.
Halogens. Physical properties of halogens.
Comparative physical properties of halogens.

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

Exercise: Completing a table of hydroxides, oxides and chlorides of alkaline earth metals.
Discuss combination of ions of alkaline earth metals with anions.

Descriptive approach: Teacher elucidates uses of alkaline earth metals.

text book
text book
Iodine crystals, electrical wire, a bulb.

K.L.B. BOOK II PP. 45-47
K.L.B. BOOK II PP. 45-47

CHEMICAL FAMILIES

Chemical properties of halogens.

By the end of the lesson, the learner should be able to:
To describe laboratory preparation of chlorine gas.

To describe reaction of halogens with metals.

Teacher demonstration: - preparation of chlorine gas.
Reaction of chlorine and iron wool.
Reaction of bromine and iron wool.
Reaction of iodine and iron wool.
Observe the rate of these reactions; hence deduce order of their reactivity of halogens.

Chlorine, iron wool, bromine.

K.L.B. BOOK IIPP. 48-50

CHEMICAL FAMILIES

Equations of reaction of halogens with metals.
Reaction of halogens with water.

By the end of the lesson, the learner should be able to:
To write balanced chemical equations of reactions involving halogens.

Re-write word equations as chemical equations then balance them.
Supervised practice.

text book
Chlorine gas, litmus papers.

K.L.B. BOOK II P. 50

CHEMICAL FAMILIES
CHEMICAL FAMILIES
STRUCTURE & BONDING
STRUCTURE & BONDING

Some uses of halogens and their compounds.
Noble Gases. Comparative physical properties of noble gases.
Uses of noble gases.
Chemical bonds. Ionic bond.
Ionic bond representation.

By the end of the lesson, the learner should be able to:
To state uses of halogens and their compounds.
State uses of noble gases.

Teacher elucidates uses of halogens and their compounds.
Teacher elucidates uses of noble gases.

text book
text book
Chart- dot and cross diagrams.
Models for bonding.

K.L.B. BOOK II pp 52
K.L.B. BOOK IIP. 54

STRUCTURE & BONDING

Grant ionic structures.
Physical properties of ionic compounds.
Covalent bond.

By the end of the lesson, the learner should be able to:
Describe the crystalline ionic compound.
Give examples of ionic substances.

Discuss the group ionic structures of NaCl.
Teacher gives examples of other ionic substances: KNO3, potassium bromide, Ca (NO3)2, sodium iodide.

Giant sodium chloride model.
text book

K.L.B. BOOK II PP 56-58

STRUCTURE & BONDING

Co-ordinate bond.
Molecular structure.

By the end of the lesson, the learner should be able to:
To describe the co-ordinate bond
To represent co-ordinate bond diagrammatically.

Exposition- teacher explains the nature of co-ordinate bond.
Students represent co-ordinate bond diagrammatically.

text book

K.L.B. BOOK II P 65

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 mutual electronic forces between electrons and nuclei.
To describe metallic bond.
To compare physical properties of metals.
To state uses of some metals.

Discuss comparative physical properties of substances. exhibiting molecular structure.
Explain variation in the physical properties.
Discussion:
Detailed analysis of comparative physical properties of metals and their uses.



Probing questions & brief explanations.

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.

By the end of the lesson, the learner should be able to:
To compare other physical properties of elements across period 3.

Analyse comparative physical properties presented in form of a table.
Explain the trend in the physical properties given.

The periodic table.

K.L.B. BOOK II P. 77

PROPERTIES AND TRENDS ACROSS PERIOD THREE

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

SALTS

Types of salts.
Solubility of salts in water.
Solubility of bases in water.

By the end of the lesson, the learner should be able to:
Define a salt.
Describe various types of salts and give several examples in each case.
To test solubility of various bases in water.
To carry out litmus test on the resulting solutions.

Descriptive approach. Teacher exposes new concepts.
Class experiments- Dissolve salts in 5cc of water.
Record the solubility in a table,
Carry out litmus tests.
Discuss the results.

text book
Sulphates, chlorides, nitrates, carbonates of various metals.
Oxides, hydroxides, of various metals, litmus papers.

K.L.B. BOOK II P. 91
K.L.B. BOOK IIPP. 94-95

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.

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

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

K.L.B. BOOK II pp96

SALTS

Ionic equations.
Effects of heat on carbonates.

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.
Various carbonates.

K.L.B. BOOK II

SALTS
SALTS
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

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

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.
To state uses of salts

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.

Teacher elucidates uses of salts.

Common metal nitrates.
Common sulphates.
Various solids, bulb, battery, & wires.

K.L.B. BOOK II PP. 110-111
K.L.B. BOOK II P. 114