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.
List the first twenty elements of the periodic table.
Write chemical symbols of the first twenty elements of the periodic table.

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.

text book
Periodic table.

K.L.B.
BOOK II

PP. 1-3

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Isotopes.

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

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.
Identify elements of the same period.

Exposition ? teacher exposes new concepts about electronic configuration.
Written exercise.
Supervised practice;
Exposition ? Definition of a period.
Q/A: Examples of elements of the same period.

Periodic table.
text book

K.L.B.
BOOK II
P. 4





PP. 5-9
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.

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

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

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Positive ions representation.
Negative ions and ion formation.
Valencies of metals.

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

Diagrammatic representation of cations.
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.
Chart  ion model.
Periodic table.

K.L.B. BOOK IIP 16
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.

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

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.

text book
The periodic table.

K.L.B. BOOK IIP 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.
Chemical formulae of compounds. -Elements of unequal 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.
To derive the formulae of some compounds involving elements of equal valencies.
To derive the formulae of some compounds involving elements of unequal valencies.

Written exercise;
Exercise review.
Discuss formation of compounds such as NaCl, MgO.
Discuss formation of compounds such as MgCl2
Al (NO3)3

text book

K.L.B. BOOK IIP 18
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.

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
CHEMICAL FAMILIES

Balanced chemical equations.
Balanced chemical equations.(contd)
Alkali metals. Atomic and ionic radii of alkali metals

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





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

Exposition;
Supervised practice.
Supervised practice;
Written exercise.

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.

text book
The periodic

K.L.B. BOOK IIPP 24-25
K.L.B. BOOK IIPP 28-29

CHEMICAL FAMILIES

Ionisation energy of alkali metals.
Physical 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.

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.

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

K.L.B. BOOK II

CHEMICAL FAMILIES

Chemical properties of alkali metals.

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

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

K.L.B. BOOK IIP. 32

CHEMICAL FAMILIES

Reaction of alkali metals with chlorine gas.
Compounds of alkali metals.
Uses of alkali metals.

By the end of the lesson, the learner should be able to:
To write balanced equations for reaction of alkali metals with chlorine gas.
Write chemical formulae for compounds of alkali metals.
Explain formation of hydroxides, oxides and chlorides of alkali metals.
State uses of alkali 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.
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.

Sodium, chlorine.
text book

K.L.B. BOOK IIP. 33
K.L.B. BOOK II pp 34

CHEMICAL FAMILIES

Alkaline Earth metals Atomic and ionic radii 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.

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.

Some alkaline earth metals.

K.L.B. BOOK II pp 34

CHEMICAL FAMILIES
STRUCTURE & BONDING

Physical properties of alkaline earth metals.
Electrical properties of alkaline earth metals.
Chemical bonds. Ionic bond.

By the end of the lesson, the learner should be able to:
State and explain trends in physical properties of alkaline earth metals.
To describe electrical properties of alkaline earth metals.
Describe role of valence electrons in determining chemical bonding.
Explain formation of ionic bonding.

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.
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.

Some alkaline earth metals.
Alkaline earth metals.
text book

K.L.B. BOOK II P. 35

STRUCTURE & BONDING

Ionic bond representation.
Grant ionic structures.
Physical properties of ionic compounds.
Covalent bond.
Co-ordinate bond.
Molecular structure.
Trend in physical properties of molecular structures.

By the end of the lesson, the learner should be able to:
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.
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
To describe van- der -waals forces.
To explain the trend in physical properties of molecular structures.

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

Chart- dot and cross diagrams.
Models for bonding.
Giant sodium chloride model.
text book
text book
Sugar, naphthalene, iodine rhombic sulphur.

K.L.B. BOOK II P. 58
K.L.B. BOOK II PP 60-63

STRUCTURE & BONDING

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 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.

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.

Diagrams in textbooks.
text book

K.L.B. BOOK II P 69

PROPERTIES AND TRENDS ACROSS PERIOD THREE

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

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

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.
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 IIP. 76

PROPERTIES AND TRENDS ACROSS PERIOD THREE
PROPERTIES AND TRENDS ACROSS PERIOD THREE
SALTS
SALTS

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.
Types of salts.
Solubility of salts in water.

By the end of the lesson, the learner should be able to:
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.
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.
To test solubility of various salts in cold water/warm water.

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.
Comparative analysis, discussion and explanation.
Descriptive approach. Teacher exposes new concepts.
Class experiments- Dissolve salts in 5 cc of water.
Record the solubility in a table,
Analyse the results.

The periodic table.
The periodic table.
text book
Sulphates, chlorides, nitrates, carbonates of various metals.

K.L.B. BOOK II PP. 79-80
K.L.B. BOOK II PP. 77-78

SALTS

Solubility of bases in water.

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.

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

Oxides, hydroxides, of various metals, litmus papers.

K.L.B. BOOK IIPP. 94-95

SALTS

Methods of preparing various salts.
Direct synthesis of a salts.
Ionic equations.

By the end of the lesson, the learner should be able to:
To describe various methods of preparing some salts.
To describe direct synthesis of a salt.
To write balanced equations for the reactions.
To identify spectator ions in double decomposition reactions.
To write ionic equations correctly.

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

CuO, H2SO4, HCl, NaOH, PbCO3, dil HNO3.
Iron,
Sulphur
PbNO3, MgSO4 solutions.

K.L.B. BOOK II pp96

SALTS

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 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.
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 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.
Group experiments- To investigate effects of heat on various sulphates.
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.

Various carbonates.
Common metal nitrates.
Common sulphates.

K.L.B. BOOK II PP. 108-109
K.L.B. BOOK II P. 114