WATER AND HYDROGEN
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
CHEMICAL FAMILIES
CHEMICAL FAMILIES
CHEMICAL FAMILIES
CHEMICAL FAMILIES
CHEMICAL FAMILIES
CHEMICAL FAMILIES
CHEMICAL FAMILIES
CHEMICAL FAMILIES
CHEMICAL FAMILIES
CHEMICAL FAMILIES
PROPERTIES AND TRENDS ACROSS PERIOD THREE
PROPERTIES AND TRENDS ACROSS PERIOD THREE
PROPERTIES AND TRENDS ACROSS PERIOD THREE
PROPERTIES AND TRENDS ACROSS PERIOD THREE
PROPERTIES AND TRENDS ACROSS PERIOD THREE
PROPERTIES AND TRENDS ACROSS PERIOD THREE
SALTS
SALTS
SALTS
SALTS
SALTS
SALTS
SALTS
SALTS
SALTS
SALTS
SALTS
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.

Burning candle wax in air.
Reaction of cold water with metals.
Reaction of steam with metals.
Hydrogen. - lab preparation.
Hydrogen. - physical properties.
Hydrogen as a reducing agent.
Burning hydrogen in air.
Uses of hydrogen.
Atomic and mass numbers.
First twenty elements of the periodic table.
Isotopes.
Electronic configuration.
Electronic configuration in diagrams.
Periods of the periodic table.
Groups of the periodic table.
R.M.M. and isotopes.
Positive ions and ion formation.
Positive ions representation.
Negative ions and ion formation.
Valencies of metals.
Valencie of non-metals.
Valencies of radicals.
Oxidation number.
Electronic configuration, ion formed, valency and oxidation number
Chemical formulae of compounds. - Elements of equal valencies.
Chemical formulae of compounds. -Elements of unequal valencies.
Chemical formulae of compounds. -Elements of variable valencies.
Chemical equations.
Balanced chemical equations.
Balanced chemical equations.(contd)
Alkali metals. Atomic and ionic radii of alkali metals
Ionisation energy of alkali metals.
Physical properties of alkali metals.
Chemical properties of alkali metals.
Reaction of alkali metals with chlorine gas.
Compounds of alkali metals.
Uses of alkali metals.
Alkaline Earth metals Atomic and ionic radii of alkaline earth metals.
Physical properties of alkaline earth metals.
Electrical properties of alkaline earth metals.
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.
Types of salts.
Solubility of salts in water.
Solubility of bases in water.
Methods of preparing various salts.
Direct synthesis of a 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.
Electrical conductivity.
Molten electrolytes.
Electrolysis.
Aqueous electrolytes. Electrodes.
Reaction on electrodes.
Binary electrolyte.
Application of electrolysis.
Electroplating.
Allotropy.
Physical and chemical properties of diamond, graphite and amorphous carbon
Burning carbon and oxygen.
Reduction properties of carbon.
Reaction of carbon with acids. Preparation of CO2.
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.
Heating carbonates and hydrogen carbonates.
Extraction of sodium carbonate from trona.
Solvay process of preparing sodium carbonate.
Importance of carbon in nature. & its effects on the environment.

By the end of the lesson, the learner should be able to:
Test for the products of burning candle wax in air.
Identify products of reaction of cold water with metals.
Identify products of reaction of steam with metals.
Recall the reactivity series of metals based on reaction with water.
Describe laboratory preparation of hydrogen.
State physical properties of hydrogen.
Describe an experiment to show reducing properties of hydrogen.
Identify products of burning hydrogen in air.
State uses of hydrogen.
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.
Define isotopes.
Give examples of isotopes.
Represent isotopes symbolically.
Define an energy level.
Describe electronic configuration in an atom.
Represent electronic configuration diagrammatically.
Identify elements of the same period.
Calculate R.M.M. from isotopic composition.
To define an ion and a cation.
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.
Recall valencies of non-metals among the first twenty elements in the periodic table.
Define a radical.
Recall the valencies of common radicals.
Define oxidation number.
Predict oxidation numbers from position of elements in the periodic table.
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.
To derive the formulae of some compounds involving elements of variable valencies.
To identify components of chemical equations.
To balance chemical equations correctly.
Identify alkali metals.
State changes in atomic and ionic radii of alkali metals.
State changes in number of energy levels and ionisation energy of alkali metals.
State and explain trends in physical properties of alkali metals.
To describe reaction of alkali metals with water.
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.
Identify alkaline earth metals.
State changes in atomic and ionic radii of alkaline earth metals.
State and explain trends in physical properties of alkaline earth metals.
To describe electrical properties of alkaline earth metals.
To compare electrical conductivity of elements in period 3
To compare other physical properties of elements across period 3.
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.
To test solubility of various bases in water.
To carry out litmus test on the resulting solutions.
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.
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
To test for electrical conductivities of substances.
To test for electrical conductivities molten electrolytes.
To define electrolysis
To describe the process of electrolysis in terms of charge movement.
To define an electrolyte
To test for electrical conductivities of electrodes.
To describe half- equation reactions at the cathode and anode
To define a binary electrolyte.
To state the products of a binary electrolyte.
To state application of electrolysis.
To describe electroplating process.
Define allotropes and allotropy.
Identify allotropes of carbon.
Represent diamond and graphite diagrammatically.
Describe physical and chemical properties of diamond, graphite and amorphous carbon.
State uses of carbon allotropes.
Describe reaction of carbon with oxygen.
Describe reduction properties of carbon.
Show reduction properties of carbon.
Describe reaction of carbon with acids.
Prepare CO2 in the lab.
Describe properties of CO2
Write balanced CO2.
State uses of CO2
To describe preparation of carbon monoxide in the lab
To describe chemical properties of carbon monoxide.
To write chemical equations for reactions of carbonates and hydrogen carbonates with acids.
To write equations for reaction of carbonates and hydrogen carbonates on heating.
To draw schematic diagram for extraction of sodium carbonates.
To discuss: - Importance of carbon in nature.
&
Effects of carbon on the environment.

Teacher demonstrations;
Discussion.
Discussion;
Write equations.
Test for evolved gas;
Review reactivity series.
Probing questions and discussion.
Teacher demonstration;
Probing questions;
Open discussion.
Exposition on new concepts;
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.
Exposition of definition and examples of isotopes.
Giving examples of isotopes.
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.
Exposition ? definition of a group.
Q/A: examples of elements of the same group.
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.
Diagrammatic representation of cations.
Guided discovery of formation of negative ions.
Diagrammatic representation of anions.
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.
Q/A: Valencies.
Expose oxidation numbers of common ions.
Students complete a table of ions and their oxidation numbers.
Written exercise;
Exercise review.
Discuss formation of compounds such as NaCl, MgO.
Discuss formation of compounds such as MgCl2
Al (NO3)3
Discuss formation of compounds such as
-Copper (I) Oxide.
-Copper (II) Oxide.
-Iron (II) Sulphate.
-Iron (III) Sulphate.
Review word equations;
Exposition of new concepts with probing questions;
Supervised practice.
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.
Examine a table of elements, number of energy levels and their ionization energy.
Discuss the trend deduced from the table.
ExamineatableshowingcomparativephysicalpropertiesofLi,Na,andK.
Q/A:Teacherasksprobingquestionsasstudentsrefertothetableforanswers.
Detaileddiscussiononphysicalpropertiesofalkalimetals.
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.
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.
Q/A: Elements of group I and their electron configuration.
Make deductions from the table.
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.
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.
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.
Descriptive approach. Teacher exposes new concepts.
Class experiments- Dissolve salts in 5 cc of water.
Record the solubility in a table,
Analyse the results.
Class experiments- Dissolve salts in 5cc of water.
Carry out litmus tests.
Discuss the results.
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.
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.
Group experiments- to identify conductors and non-conductors.
Explain the difference in (non) conductivities.
Group experiments- to identify electrolytes in molten form.
Explain the difference in molten electrolytes.
Descriptive approach punctuated with Q/A.
To investigate chemical effect of an electric current.
Classify the solutions as electrolyte or non -electrolytes.
Discuss the electrical properties of the solutions.
To demonstrate ?Electrolysis of molten lead (II) bromide
Observe colour changes
Explanation of half-equations and reactions at the electrodes.
Completing a table of electrolysis of binary electrolytes.
Discussion and explanations.
Experiment- Left overnight.
Electroplating an iron nail with silver nitrate/ copper sulphate.
Teacher exposes new terms.
Review covalent bond.
Discuss boding in diamond and graphite.
Discuss physical and chemical properties of diamond, graphite and amorphous carbon.
Explain the Physical and chemical properties of diamond, graphite and amorphous carbon.
Discuss uses of carbon allotropes.
Teacher demonstration- Prepare oxygen and pass dry oxygen into a tube containing carbon. Heat the carbon. Observe effects on limewater.
Teacher demonstration ? Burn strongly a mixture of carbon and CuO on a bottle top.
Observe colour changes and give underlying explanation
Teacher demonstration- reaction of carbon with hot conc HNO3.
Write balanced equations for the reaction.
Review effects of heat on carbonates.
Group experiments/teacher demonstration- preparation of CO2.
Simple experiments to determine properties of CO2.
Discuss the observations.
Give examples of reactions. Write corresponding balanced chemical equations.
Discuss briefly the uses of CO2.
Teacher demonstration: preparation of carbon monoxide in the lab.
Make observations.
Description of properties of carbon monoxide.
Discussion and writing of chemical equations.
Discuss the observations above.
Write chemical equations for the reactions.
Discuss the above observations.
Write corresponding balanced equations.
Discuss each step of the process.
Write relevant equations.
Discuss the carbon cycle and processes that increase/ reduce amount of CO2 in the air.
Uses of CO2 in soft drinks and fire extinguishers.

Candles, lime water.
Calcium, sodium grain.
Magnesium ribbon, sand, iron / steel wool.
Zinc granules,
dil HCl,
conc. sulphuric acid.
conc. sulphuric acid, litmus papers.
Copper (II) oxide, anhydrous Copper (II) sulphate., dry hydrogen.
Anhydrous calcium chloride,
hydrogen, U tube, ice cold water.
TEXT BOOK
Periodic table.
Chart  ion model.
The periodic table.
The periodic
Chart ? comparative properties of Li, Na, K.
Sodium, chlorine.
Some alkaline earth metals.
Alkaline earth metals.
Sulphates, chlorides, nitrates, carbonates of various metals.
Oxides, hydroxides, of various metals, litmus papers.
CuO, H2SO4, HCl, NaOH, PbCO3, dil HNO3.
Iron,
Sulphur
PbNO3, MgSO4 solutions.
Various carbonates.
Common metal nitrates.
Common sulphates.
Various solids, bulb, battery, & wires.
Molten candle wax
Sugar
Lead oxide.
Graphite electrodes
Battery
Various aqueous solutions switch bulb.
Various aqueous solutions switch.
Silver nitrate
Iron nail
Complete circuit battery.
Charcoal, graphite.
Carbon, limewater, tube, limewater stand& Bunsen burner.
CuO, pounded charcoal, Bunsen burner& bottle top
Conc. HNO3, limewater.
Lime water,
Magnesium ribbon,
Universal indicator,
lit candle.
text book, chart

K.L.B.
BOOK I
PP. 91-92