THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

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

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
Periodic table.

K.L.B.
BOOK II

PP. 1-3

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Isotopes.
Electronic configuration.

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

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

Periodic table.

K.L.B.
BOOK II
P. 4





PP. 5-8

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Electronic configuration in diagrams.
Periods of the periodic table.
Groups of the periodic table.

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

Supervised practice;
Written exercise.
Exposition ? Definition of a period.
Q/A: Examples of elements of the same period.

text book
Periodic table.

K.L.B.
BOOK II
PP. 5-8
K.L.B. BOOK IIP. 9

THE STRUCTURE OF THE ATOM & 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:
Calculate R.M.M. from isotopic composition.

Supervised practice involving calculation of RMM from isotopic composition.

text book

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.
Valencie of non-metals.
Valencies of radicals.

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 non-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.
Periodic table.
text book

K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

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.

K.L.B. BOOK IIvP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Electronic configuration, ion formed, valency and oxidation number
Chemical formulae of compounds. - Elements of equal valencies.

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 unequal valencies.
Chemical formulae of compounds. -Elements of variable valencies.
Chemical equations.
Balanced 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 identify components of chemical equations.

Discuss formation of compounds such as MgCl2
Al (NO3)3
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.(contd)

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

Supervised practice;
Written exercise.

text book

K.L.B. BOOK IIPP 25-8

CHEMICAL FAMILIES

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 describe reaction of alkaline earth metals with oxygen

Q/A: Review reactions of Mg, Ca, with oxygen.
The corresponding word and then chemical equations are then written and their correctness verified by the teacher.

text book
Some alkaline earth metals.

K.L.B. BOOK IIP. 38

CHEMICAL FAMILIES

Reaction of alkaline earth metals with chlorine gas.
Reaction of alkaline earth metals with dilute acids.
Chemical formulae of alkaline earth metals.

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.
Write chemical formulae for compounds of alkaline earth metals.
Explain formation of hydroxides, oxides and chlorides of alkaline earth metals.

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.

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

Sodium, chlorine.
revision book
text book

K.L.B. BOOK II P. 41
K.L.B. BOOK II PP. 45-47

CHEMICAL FAMILIES

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

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

Descriptive approach: Teacher elucidates uses of alkaline earth metals.

text book
Iodine crystals, electrical wire, a bulb.
Chlorine, iron wool, bromine.

K.L.B. BOOK II PP. 45-47

CHEMICAL FAMILIES

Equations of reaction of halogens with metals.

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

K.L.B. BOOK II P. 50

CHEMICAL FAMILIES
CHEMICAL FAMILIES
STRUCTURE & BONDING
STRUCTURE & BONDING
STRUCTURE & BONDING

Reaction of halogens with water.
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.
Grant ionic structures.

By the end of the lesson, the learner should be able to:
To describe reaction of halogens with water and the results obtained.
State uses of noble gases.

Bubbling chlorine gas through water.
Carry out litmus test for the water.
Explain the observations.

Teacher elucidates uses of noble gases.

Chlorine gas, litmus papers.
text book
text book
Chart- dot and cross diagrams.
Models for bonding.
Giant sodium chloride model.

K.L.B. BOOK II P. 51
K.L.B. BOOK IIP. 54

STRUCTURE & BONDING

Physical properties of ionic compounds.
Covalent bond.
Co-ordinate bond.
Molecular structure.

By the end of the lesson, the learner should be able to:
Describe physical properties of ionic compounds.
Explain the differences in the physical properties of ionic compounds.

Analyse tabulated comparative physical properties of ionic compounds.

Teacher asks probing questions.

text book

K.L.B. BOOK IIPP 58-59

STRUCTURE & BONDING

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

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.

Discuss comparative physical properties of substances. exhibiting molecular structure.
Explain variation in the physical properties.

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

K.L.B. BOOK IIP 65

PROPERTIES AND TRENDS ACROSS PERIOD THREE

Physical properties of elements in periods.
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.
Chlorides of period 3 elements.

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




To compare electrical conductivity of elements in period 3
To compare reactions of elements in period 3 with water

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.

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 IIP. 76
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.

Descriptive approach. Teacher exposes new concepts.

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

K.L.B. BOOK II P. 91

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.
Effects of heat on nitrates.
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 identify spectator ions in double decomposition reactions.
To write ionic equations correctly.

To define hygroscopic deliquescent and efflorescent salts.
To give examples of hygroscopic deliquescent and efflorescent salts.

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

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

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

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