THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

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

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

Electronic configuration.

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.

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

Periodic table.

K.L.B.
BOOK II
P. 4





PP. 5-9

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Electronic configuration in diagrams.

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

Supervised practice;
Written exercise.

text book

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

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Periods of the periodic table.
Groups of the periodic table.
R.M.M. and isotopes.

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

Exposition ? Definition of a period.
Q/A: Examples of elements of the same period.
Supervised practice involving calculation of RMM from isotopic composition.

Periodic table.
text book

K.L.B. BOOK IIP. 9
K.L.B. BOOK IIPP. 11-13

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Positive ions and ion formation.

By the end of the lesson, the learner should be able to:
To define an ion and a cation.

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 14-15

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Positive ions representation.
Negative ions and ion formation.

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

Valencies of metals.
Valencie of non-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.
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.

By the end of the lesson, the learner should be able to:
Define a radical.
Recall the valencies of common radicals.

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

text book

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.
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
Ionisation energy 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
text book

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

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.

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.

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.

Sodium, chlorine.
text book

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

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.

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

Some alkaline earth metals.

K.L.B. BOOK II P. 35

CHEMICAL FAMILIES
STRUCTURE & BONDING
STRUCTURE & BONDING
STRUCTURE & BONDING

Electrical properties of alkaline earth metals.
Chemical bonds. Ionic bond.
Ionic bond representation.
Grant ionic structures.
Physical properties of ionic compounds.
Covalent bond.
Co-ordinate bond.

By the end of the lesson, the learner should be able to:
To describe electrical properties of alkaline earth metals.
Describe physical properties of ionic compounds.
Explain the differences in the physical properties of ionic compounds.

Teacher demonstration: -
To show alkaline metals are good conductors of electric charge.
Analyse tabulated comparative physical properties of ionic compounds.

Teacher asks probing questions.

Alkaline earth metals.
text book
Chart- dot and cross diagrams.
Models for bonding.
Giant sodium chloride model.

K.L.B. BOOK IIP. 37
K.L.B. BOOK IIPP 58-59

STRUCTURE & BONDING

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 molecular structure.
To give examples of substance exhibiting molecular structure

Discussion ? To explain formation of the giant structure and give examples of substance exhibiting molecular structure.

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

K.L.B. BOOK IIP 65

STRUCTURE & BONDING

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 graphite.
To state uses of graphite.

Diagrammatic representation of graphite.

Discuss uses of graphite.

Diagrams in textbooks.
text book

K.L.B. BOOK II pp 69

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.

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 oxygen.

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: 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.

The periodic table.

K.L.B. BOOK IIP. 76
K.L.B. BOOK II PP. 79-80

PROPERTIES AND TRENDS ACROSS PERIOD THREE
SALTS
SALTS

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 explain chemical behavior of their chlorides.
To describe hydrolysis reaction.

Comparative analysis, discussion and explanation.

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

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.
Effects of heat on carbonates.
Effects of heat on nitrates.

By the end of the lesson, the learner should be able to:
To describe various methods of preparing some salts.
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.


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.
Various carbonates.
Common metal nitrates.

K.L.B. BOOK II pp96

SALTS

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 sulphates.
To predict products results from heating metal sulphates.

Group experiments- To investigate effects of heat on various sulphates.
Observe various colour changes before, during and after heating.
Write equations for the reactions.

Common sulphates.

K.L.B. BOOK II P. 113

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Electrical conductivity.
Molten electrolytes.
Electrolysis.

By the end of the lesson, the learner should be able to:
To test for electrical conductivities of substances.

Group experiments- to identify conductors and non-conductors.
Explain the difference in (non) conductivities.

Various solids, bulb, battery, & wires.
Molten candle wax
Sugar
Sulphur
Lead oxide.

K.L.B. BOOK II PP. 118-119

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Aqueous electrolytes. Electrodes.
Reaction on electrodes.
Binary electrolyte.
Application of electrolysis.
Electroplating.

By the end of the lesson, the learner should be able to:
To define an electrolyte
To test for electrical conductivities of electrodes.
To define a binary electrolyte.
To state the products of a binary electrolyte.

To investigate chemical effect of an electric current.
Classify the solutions as electrolyte or non -electrolytes.
Discuss the electrical properties of the solutions.
Completing a table of electrolysis of binary electrolytes.

Graphite electrodes
Battery
Various aqueous solutions switch bulb.
Various aqueous solutions switch.
text book
Silver nitrate
Iron nail
Complete circuit battery.

K.L.B. BOOK II PP.122-123
K.L.B. BOOK II P.127

CARBON AND SOME OF ITS COMPOUNDS.

Allotropy.
Physical and chemical properties of diamond, graphite and amorphous carbon
Burning carbon and oxygen.

By the end of the lesson, the learner should be able to:
Define allotropes and allotropy.
Identify allotropes of carbon.
Represent diamond and graphite diagrammatically.

Teacher exposes new terms.
Review covalent bond.
Discuss boding in diamond and graphite.

text book
Charcoal, graphite.
Carbon, limewater, tube, limewater stand& Bunsen burner.

K.L.B. BOOK II PP. 131-133

CARBON AND SOME OF ITS COMPOUNDS.

Reduction properties of carbon.
Reaction of carbon with acids. Preparation of CO2.

By the end of the lesson, the learner should be able to:
Describe reduction properties of carbon.
Show reduction properties of carbon.

Teacher demonstration ? Burn strongly a mixture of carbon and CuO on a bottle top.
Observe colour changes and give underlying explanation

CuO, pounded charcoal, Bunsen burner& bottle top
Conc. HNO3, limewater.

K.L.B. BOOK II P.126

CARBON AND SOME OF ITS COMPOUNDS.

Properties of CO2.
Chemical equations for reactions involving CO2.
Uses of CO2.
Carbon monoxide lab preparation.
Chemical properties of carbon monoxide.
Carbonates and hydrogen carbonates.

By the end of the lesson, the learner should be able to:
Describe properties of CO2
State uses of CO2

Simple experiments to determine properties of CO2.

Discuss the observations.

Discuss briefly the uses of CO2.

Lime water,
Magnesium ribbon,
Universal indicator,
lit candle.
text book

K.L.B. BOOK II PP.138-139
K.L.B. BOOK II PP.140-1

CARBON AND SOME OF ITS COMPOUNDS.

Heating carbonates and hydrogen carbonates.
Extraction of sodium carbonate from trona.
Solvay process of preparing sodium carbonate.

By the end of the lesson, the learner should be able to:
To write equations for reaction of carbonates and hydrogen carbonates on heating.

Discuss the above observations.
Write corresponding balanced equations.

text book
text book, chart

K.L.B. BOOK II PP.150-151

CARBON AND SOME OF ITS COMPOUNDS.

Importance of carbon in nature. & its effects on the environment.

By the end of the lesson, the learner should be able to:
To discuss: - Importance of carbon in nature.
&
Effects of carbon on the environment.

Discuss the carbon cycle and processes that increase/ reduce amount of CO2 in the air.
Uses of CO2 in soft drinks and fire extinguishers.

text book

K.L.B. BOOK II PP.157-158