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
K.L.B. BOOK IIPP 14-15

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.

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.
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.

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

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.
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.
To derive the formulae of some compounds involving elements of unequal valencies.

Discuss formation of compounds such as NaCl, MgO.
Discuss formation of compounds such as MgCl2
Al (NO3)3

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.
Chemical equations.

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

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)
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.

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 25-8
K.L.B. BOOK IIPP 28-29

CHEMICAL FAMILIES

Ionisation energy 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.

Examine a table of elements, number of energy levels and their ionization energy.
Discuss the trend deduced from the table.

text book

K.L.B. BOOK II

CHEMICAL FAMILIES

Physical properties of alkali metals.

By the end of the lesson, the learner should be able to:
State and explain trends in physical properties of alkali metals.

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.

Chart ? comparative properties of Li, Na, K.

K.L.B. BOOK IIPP 30-31

CHEMICAL FAMILIES

Chemical properties of alkali metals.
Reaction of alkali metals with chlorine gas.
Compounds of alkali metals.

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

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.

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.

text book
Sodium, chlorine.
text book

K.L.B. BOOK IIP. 32
K.L.B. BOOK IIP. 33

CHEMICAL FAMILIES

Uses of alkali metals.

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

Descriptive approach: Teacher elucidates uses of alkali metals.

text book

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

Physical properties of alkaline earth metals.
Electrical properties of alkaline earth metals.

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.

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.

K.L.B. BOOK II P. 35
K.L.B. BOOK IIP. 37

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.

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.

K.L.B. BOOK IIP. 39

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.

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

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.
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.
To describe reaction of halogens with water and the results obtained.

Re-write word equations as chemical equations then balance them.
Supervised practice.
Bubbling chlorine gas through water.
Carry out litmus test for the water.
Explain the observations.

text book
Chlorine gas, litmus papers.

K.L.B. BOOK II P. 50
K.L.B. BOOK II P. 51

CHEMICAL FAMILIES

Some uses of halogens and their compounds.
Noble Gases. Comparative physical properties of noble gases.

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

Teacher elucidates uses of halogens and their compounds.

text book

K.L.B. BOOK II pp 52

CHEMICAL FAMILIES
STRUCTURE & BONDING
STRUCTURE & BONDING

Uses of noble gases.
Chemical bonds. Ionic bond.
Ionic bond representation.

By the end of the lesson, the learner should be able to:
State uses of noble gases.

Teacher elucidates uses of noble gases.

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

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

By the end of the lesson, the learner should be able to:
To describe the co-ordinate bond
To represent co-ordinate bond diagrammatically.
To describe giant atomic structure in diamond.
To state uses of diamond.

Exposition- teacher explains the nature of co-ordinate bond.
Students represent co-ordinate bond diagrammatically.
Diagrammatic representation of diamond.
Discuss uses of diamond.

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

K.L.B. BOOK II P 65
K.L.B. BOOK II P 69

STRUCTURE & BONDING

Metallic bond. Uses of some metals.

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

Discussion:
Detailed analysis of comparative physical properties of metals and their uses.



Probing questions & brief explanations.

text book

K.L.B. BOOK IIP 70

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.

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




To compare electrical conductivity of elements in 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.

The periodic table.

K.L.B. BOOK IIP. 76

PROPERTIES AND TRENDS ACROSS PERIOD THREE
SALTS

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 water
Define a salt.
Describe various types of salts and give several examples in each case.

Q/A: Review reaction of sodium, Mg, chlorine, with water.
Infer that sodium is most reactive metal; non-metals do not react with water.

Descriptive approach. Teacher exposes new concepts.

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

K.L.B. BOOK II PP. 80-81
K.L.B. BOOK II P. 91

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.

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.

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 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 various metal nitrates.
Observe various colour changes before, during and after heating.
Write equations for the reactions.

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

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

SALTS

Hygroscopy, Deliquescence and Efflorescence.
Uses of salts.

By the end of the lesson, the learner should be able to:
To define hygroscopic deliquescent and efflorescent salts.
To give examples of hygroscopic deliquescent and efflorescent salts.

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

K.L.B. BOOK II P. 114