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| WK | LSN | TOPIC | SUB-TOPIC | OBJECTIVES | T/L ACTIVITIES | T/L AIDS | REFERENCE | REMARKS |
|---|---|---|---|---|---|---|---|---|
| 2 | 1 |
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
|
Atomic and mass numbers.
|
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
|
K.L.B.
BOOK II PP. 1-3 |
|
| 2 | 2-3 |
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
|
First twenty elements of the periodic table.
Isotopes. |
By the end of the
lesson, the learner
should be able to:
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. |
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. |
Periodic table.
Periodic table. |
K.L.B.
BOOK II PP. 1-3 K.L.B. BOOK II P. 4 PP. 5-8 |
|
| 2 | 4 |
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 |
|
| 2 | 5 |
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 |
|
| 3 | 1 |
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
|
|
| 3 | 2-3 |
THE STRUCTURE OF THE ATOM & 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 group.
Q/A: examples of elements of the same group. 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 |
|
| 3 | 4 |
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
|
|
| 3 | 5 |
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
|
|
| 4 | 1 |
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
|
Negative ions and ion formation.
|
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.
|
K.L.B. BOOK IIP 17
|
|
| 4 | 2-3 |
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. Recall valencies of metals among the first twenty elements in the periodic table. |
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.
Periodic table. |
K.L.B. BOOK IIP 17
|
|
| 4 | 4 |
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
|
|
| 4 | 5 |
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
|
|
| 5 | 1 |
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
|
|
| 5 | 2-3 |
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
|
Electronic configuration, ion formed, valency and oxidation number
Chemical formulae of compounds. - Elements of equal 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. |
Written exercise;
Exercise review. Discuss formation of compounds such as NaCl, MgO. |
text book
|
K.L.B. BOOK IIP 18
K.L.B. BOOK IIPP 19-20 |
|
| 5 | 4 |
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
|
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 unequal valencies. |
Discuss formation of compounds such as MgCl2
Al (NO3)3 |
text book
|
K.L.B. BOOK IIPP 19-20
|
|
| 5 | 5 |
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
|
|
| 6 | 1 |
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
|
|
| 6 | 2-3 |
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
|
Balanced chemical equations.
Balanced chemical equations.(contd) |
By the end of the
lesson, the learner
should be able to:
To balance chemical equations correctly. |
Exposition;
Supervised practice. Supervised practice; Written exercise. |
text book
|
K.L.B. BOOK IIPP 24-25
K.L.B. BOOK IIPP 25-8 |
|
| 6 | 4 |
CHEMICAL FAMILIES
|
Alkali metals.
Atomic and ionic radii of alkali metals
|
By the end of the
lesson, the learner
should be able to:
Identify alkali metals. State changes in atomic and ionic radii of alkali metals. |
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. |
The periodic
|
K.L.B. BOOK IIPP 28-29
|
|
| 6 | 5 |
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
|
|
| 7 |
Midterm |
|||||||
| 8 | 1 |
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
|
|
| 8 | 2-3 |
CHEMICAL FAMILIES
|
Chemical properties of alkali metals.
Reaction of alkali metals with chlorine gas. |
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. |
K.L.B. BOOK IIP. 32
K.L.B. BOOK IIP. 33 |
|
| 8 | 4 |
CHEMICAL FAMILIES
|
Compounds of alkali metals.
|
By the end of the
lesson, the learner
should be able to:
Write chemical formulae for compounds of alkali metals. Explain formation of hydroxides, oxides and chlorides of alkali metals. |
Exercise: Completing a table of hydroxides, oxides and chlorides of alkali metals.
Discuss combination of ions of alkali metals with anions. |
text book
|
K.L.B. BOOK II pp 33
|
|
| 8 | 5 |
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
|
|
| 9 | 1 |
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
|
|
| 9 | 2-3 |
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 |
|
| 9 | 4 |
STRUCTURE & BONDING
|
Chemical bonds.
Ionic bond.
Ionic bond representation. |
By the end of the
lesson, the learner
should be able to:
Describe role of valence electrons in determining chemical bonding. Explain formation of ionic bonding. |
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. |
text book
Chart- dot and cross diagrams. Models for bonding. |
K.L.B. BOOK IIP54
PP 57-58 |
|
| 9 | 5 |
STRUCTURE & BONDING
|
Grant ionic structures.
Physical properties of ionic compounds. |
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
|
|
| 10 | 1 |
STRUCTURE & BONDING
|
Covalent bond.
Co-ordinate bond. |
By the end of the
lesson, the learner
should be able to:
Explain the formation of covalent bond Use dot and cross diagrams to represent covalent bond. |
Exposition: Shared pair of electrons in a hydrogen molecule, H2O, NH3, Cl2, and CO2.
Drawing of dot-and-cross diagrams of covalent bonds. |
text book
|
K.L.B. BOOK II PP 60-63
|
|
| 10 | 2-3 |
STRUCTURE & BONDING
|
Molecular structure.
Trend in physical properties of molecular structures. 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 the molecular structure. To give examples of substance exhibiting molecular structure To describe giant atomic structure in graphite. To state uses of graphite. |
Discussion ? To explain formation of the giant structure and give examples of substance exhibiting molecular structure.
Diagrammatic representation of graphite. Discuss uses of graphite. |
text book
Sugar, naphthalene, iodine rhombic sulphur. Diagrams in textbooks. Diagrams in textbooks. text book |
K.L.B. BOOK IIP 65
K.L.B. BOOK II pp 69 |
|
| 10 | 4 |
PROPERTIES AND TRENDS ACROSS PERIOD THREE
|
Physical properties of elements in periods.
|
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
|
|
| 10 | 5 |
PROPERTIES AND TRENDS ACROSS PERIOD THREE
|
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 other physical properties of elements across period 3. |
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 II P. 77
|
|
| 11 | 1 |
PROPERTIES AND TRENDS ACROSS PERIOD THREE
|
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 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
|
|
| 11 | 2-3 |
PROPERTIES AND TRENDS ACROSS PERIOD THREE
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. To test solubility of various salts in cold water/warm water. |
Comparative analysis, discussion and explanation.
Class experiments- Dissolve salts in 5 cc of water. Record the solubility in a table, Analyse the results. |
The periodic table.
text book Sulphates, chlorides, nitrates, carbonates of various metals. |
K.L.B. BOOK II PP. 77-78
K.L.B. BOOK II PP. 92-93 |
|
| 11 | 4 |
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
|
|
| 11 | 5 |
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
|
|
| 12 | 1 |
SALTS
|
Ionic equations.
Effects of heat on carbonates. |
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. |
Q/A: Ions present in given reactants.
Deduce the products of double decomposition reactions. Give examples of equations. Supervised practice. |
PbNO3, MgSO4 solutions.
Various carbonates. |
K.L.B. BOOK II
|
|
| 12 | 2-3 |
SALTS
|
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 nitrates. To predict products resulting from heating metal nitrates. To define hygroscopic deliquescent and efflorescent salts. To give examples of hygroscopic deliquescent and efflorescent salts. |
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. Prepare a sample of various salts. Expose them to the atmosphere overnight. Students classify the salts as hygroscopic, deliquescent and / or efflorescent. |
Common metal nitrates.
Common sulphates. |
K.L.B. BOOK II PP. 110-111
K.L.B. BOOK II P. 114 |
|
| 12 | 4 |
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
|
Electrical conductivity.
Molten electrolytes. |
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
|
|
| 12 | 5 |
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
|
Electrolysis.
Aqueous electrolytes. Electrodes. |
By the end of the
lesson, the learner
should be able to:
To define electrolysis To describe the process of electrolysis in terms of charge movement. |
Descriptive approach punctuated with Q/A.
|
Graphite electrodes
Battery Various aqueous solutions switch bulb. |
K.L.B. BOOK II
|
|
| 13 | 1 |
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
|
Reaction on electrodes.
|
By the end of the
lesson, the learner
should be able to:
To describe half- equation reactions at the cathode and anode |
To demonstrate ?Electrolysis of molten lead (II) bromide
Observe colour changes Explanation of half-equations and reactions at the electrodes. |
Graphite electrodes
Battery Various aqueous solutions switch. |
K.L.B. BOOK II PP.126-127
|
|
| 13 | 2-3 |
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
CARBON AND SOME OF ITS COMPOUNDS. |
Binary electrolyte.
Application of electrolysis. Electroplating. Allotropy. Physical and chemical properties of diamond, graphite and amorphous carbon |
By the end of the
lesson, the learner
should be able to:
To define a binary electrolyte. To state the products of a binary electrolyte. Define allotropes and allotropy. Identify allotropes of carbon. Represent diamond and graphite diagrammatically. |
Completing a table of electrolysis of binary electrolytes.
Teacher exposes new terms. Review covalent bond. Discuss boding in diamond and graphite. |
text book
Silver nitrate Iron nail Complete circuit battery. text book Charcoal, graphite. |
K.L.B. BOOK II P.127
K.L.B. BOOK II PP. 131-133 |
|
| 13 | 4 |
CARBON AND SOME OF ITS COMPOUNDS.
|
Burning carbon and oxygen.
Reduction properties of carbon. |
By the end of the
lesson, the learner
should be able to:
Describe reaction of carbon with oxygen. |
Teacher demonstration- Prepare oxygen and pass dry oxygen into a tube containing carbon. Heat the carbon. Observe effects on limewater.
|
Carbon, limewater, tube, limewater stand& Bunsen burner.
CuO, pounded charcoal, Bunsen burner& bottle top |
K.L.B. BOOK II PP. 134-135
|
|
| 13 | 5 |
CARBON AND SOME OF ITS COMPOUNDS.
|
Reaction of carbon with acids.
Preparation of CO2.
Properties of CO2. |
By the end of the
lesson, the learner
should be able to:
Describe reaction of carbon with acids. Prepare CO2 in the lab. |
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. |
Conc. HNO3, limewater.
Lime water, Magnesium ribbon, Universal indicator, lit candle. |
K.L.B. BOOK II P.126
|
|
| 14 | 1 |
CARBON AND SOME OF ITS COMPOUNDS.
|
Chemical equations for reactions involving CO2.
|
By the end of the
lesson, the learner
should be able to:
Write balanced CO2. |
Give examples of reactions. Write corresponding balanced chemical equations.
|
text book
|
K.L.B. BOOK II PP.139-140
|
|
| 14 | 2-3 |
CARBON AND SOME OF ITS COMPOUNDS.
|
Uses of CO2.
Carbon monoxide lab preparation. Chemical properties of carbon monoxide. Carbonates and hydrogen carbonates. Heating carbonates and hydrogen carbonates. |
By the end of the
lesson, the learner
should be able to:
State uses of CO2 To write chemical equations for reactions of carbonates and hydrogen carbonates with acids. |
Discuss briefly the uses of CO2.
Discuss the observations above. Write chemical equations for the reactions. |
text book
|
K.L.B. BOOK II PP.140-1
|
|
| 14 | 4 |
CARBON AND SOME OF ITS COMPOUNDS.
|
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 draw schematic diagram for extraction of sodium carbonates. |
Discuss each step of the process.
Write relevant equations. |
text book
text book, chart |
K.L.B. BOOK II PP. 153-157
|
|
| 14 | 5 |
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
|
|
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