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.
Electronic configuration in diagrams.

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

Represent isotopes symbolically.
Define an energy level.
Describe electronic configuration in an atom.

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

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

Periodic table.

Periodic table.
text book

K.L.B.
BOOK II
P. 4





PP. 5-8
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.

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 represent formation of positive ions symbolically.

Supervised practice involving calculation of RMM from isotopic composition.

Diagrammatic representation of cations.

text book
Chart  ion model.

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

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

Chart  ion model.
Periodic table.

K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Valencie of non-metals.

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.

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

Valencies of radicals.
Oxidation number.
Electronic configuration, ion formed, valency and oxidation number

By the end of the lesson, the learner should be able to:
Define a radical.
Recall the valencies of common radicals.
Relate electronic configuration, ion formed, valency and oxidation number of different elements.

Exposition ? teacher defines a radical, gives examples of radicals and exposes their valencies.
Students draw a table of radicals and their valencies.

Written exercise;
Exercise review.

text book
The periodic table.

K.L.B. BOOK IIP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

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

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

Discuss formation of compounds such as
-Copper (I) Oxide.
-Copper (II) Oxide.
-Iron (II) Sulphate.
-Iron (III) Sulphate.

text book

K.L.B. BOOK IIP 20

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Chemical equations.
Balanced chemical equations.
Balanced chemical equations.(contd)

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

To balance chemical equations correctly.

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

text book

K.L.B. BOOK IIPP 21-23
K.L.B. BOOK IIPP 24-25

CHEMICAL FAMILIES

Chemical properties of alkaline earth metals. Reaction of alkaline earth metals with oxygen.

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

K.L.B. BOOK IIP. 38

CHEMICAL FAMILIES

Chemical properties of alkaline earth metals. Reaction of alkaline earth metals with water.
Reaction of alkaline earth metals with chlorine gas.

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

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.

Some alkaline earth metals.
Sodium, chlorine.

K.L.B. BOOK IIP. 39

CHEMICAL FAMILIES

Reaction of alkaline earth metals with dilute acids.
Chemical formulae of alkaline earth metals.
Uses of some alkaline earth metals and their compounds.

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

Changing word to chemical equations.
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.

revision book
text book

K.L.B. BOOK II PP. 43
K.L.B. BOOK II PP. 45-47

CHEMICAL FAMILIES

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:
Identify halogens in the periodic table.
Give examples of halogens.
Identify physical states of halogens.

Teacher demonstration: - To examine electrical properties of iodine, solubility in water of chlorine.

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

KLB BK II
P. 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

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.

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

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

Make A comparative analysis of tabulated physical properties of noble gases.

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

K.L.B. BOOK II P. 51
  K.L.B. BOOK IIPP. 52-53

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.
Trend in physical properties of molecular structures.
Giant atomic structure in diamond.

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

K.L.B. BOOK II P 65

STRUCTURE & BONDING
PROPERTIES AND TRENDS ACROSS PERIOD THREE

Giant atomic structure in graphite.
Metallic bond. Uses of some metals.
Physical properties of elements in periods.
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 describe giant atomic structure in graphite.
To state uses of graphite.




To compare electrical conductivity of elements in period 3

Diagrammatic representation of graphite.

Discuss uses of graphite.
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.

Diagrams in textbooks.
text book
The periodic table.

K.L.B. BOOK II pp 69
K.L.B. BOOK IIP. 76

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.

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.

K.L.B. BOOK II P. 91

SALTS

Solubility of bases in water.
Methods of preparing various salts.
Direct synthesis of a salts.
Ionic equations.
Effects of heat on carbonates.

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.
To describe direct synthesis of a salt.
To write balanced equations for the reactions.

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


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.

Oxides, hydroxides, of various metals, litmus papers.
CuO, H2SO4, HCl, NaOH, PbCO3, dil HNO3.
Iron,
Sulphur
PbNO3, MgSO4 solutions.
Various carbonates.

K.L.B. BOOK IIPP. 94-95
K.L.B. BOOK II P. 104

SALTS

Effects of heat on nitrates.
Effects of heat on sulphates.
Hygroscopy, Deliquescence and Efflorescence.

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
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Uses of salts.
Electrical conductivity.

By the end of the lesson, the learner should be able to:
To state uses of salts

Teacher elucidates uses of salts.

Various solids, bulb, battery, & wires.

K.L.B. BOOK II P. 114