· 2020. 7. 11. · BOOKII PP.1-3 2 Firsttwenty elementsofthe periodictable. Listthefirsttwenty elementsoftheperiodic table. Writechemicalsymbols ofthefirsttwenty elementsoftheperiodic

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SCHEME OF WORK FORM TWO CHEMISTRY TERM ONE 2020

WKNO.

L/NO

TOPIC/SUBTOPIC

LESSON / SPECIFICOBJECTIVES

TEACHING / LEARNINGACTIVITIES

MATERIALS/

RESOURCESREFERE-NCES REMARKS

1 1 THE STRUCTUREOF THE ATOM &THE PERIODICTABLE

Atomic and massnumbers.

By the end of thelesson, the learnershould be able to:

Name the subatomicparticles in an atom.Define atomic numberand mass number of anatom.Represent atomic andmass numberssymbolically.

Exposition on newconcepts;Probing questions;Brief discussion.

K.L.B.BOOK II

PP. 1-3

2 First twentyelements of theperiodic table.

List the first twentyelements of the periodictable.Write chemical symbolsof the first twentyelements of the periodictable.

Expository approach:referring to the periodictable, teacher exposes thefirst twenty elements.Writing down a list of firsttwenty elements of theperiodic table.

Periodic table. K.L.B.BOOK II

PP. 1-3

3

&

Isotopes. Define isotopes.Give examples ofisotopes.

Exposition of definition andexamples of isotopes.Giving examples ofisotopes.

Periodic table. K.L.B.BOOK IIP. 4

http://www.teachersupdates.co.ke


4 Electronicconfiguration.

Represent isotopessymbolically.Define an energy level.Describe electronicconfiguration in anatom.

Exposition – teacherexposes new conceptsabout electronicconfiguration.Written exercise.

PP. 5-8

2 1 Electronicconfiguration indiagrams.

Represent electronicconfigurationdiagrammatically.

Supervised practice;Written exercise.

K.L.B.BOOK IIPP. 5-8

2 Periods of theperiodic table.

Identify elements of thesame period.

Exposition – Definition of aperiod.Q/A: Examples of elementsof the same period.

Periodic table. P. 9

3 Groups of theperiodic table.

Identify elements of thesame period.

Exposition – definition of agroup.Q/A: examples of elementsof the same group.

Periodic table. P. 9

4 R.M.M. andisotopes.

Calculate RMM fromisotopic composition.To describe relativeabundance of isotopesof an element.

Teacher exposes definitionof R.M.M.

Worked examples.

PP. 11-13

3 1 R.M.M. andisotopes.

Calculate R.M.M. fromisotopic composition.

Supervised practiceinvolving calculation ofRMM from isotopiccomposition.

PP. 11-13



2 Positive ions and ionformation.

To define an ion and acation.

Teacher gives examples ofstable atoms.Guided discovery thatmetals need to lose one,two or three electrons toattain stability.Examples of positive ions.

PP 14-15

3 3 Positive ionsrepresentation.

To represent formationof positive ionssymbolically.

Diagrammaticrepresentation of cations.

Chart – ionmodel.

P 16

4 Negative ions andion formation.

To define an anion.To describe formation ofnegative ionssymbolically.

Teacher gives examples ofstable atoms.Guided discovery offormation of negative ions.Diagrammaticrepresentation of anions.

Chart – ionmodel.

P 17

4 1 Valencies of metals. Recall valencies ofmetals among the firsttwenty elements in theperiodic table.

Q/A to review previouslesson;Exposition;Guided discovery.

Periodic table. P 17

2 Valencie of non-metals.

Recall valencies of non-metals among the firsttwenty elements in theperiodic table.

Q/A to review previouslesson;Exposition;Guided discovery.

Periodic table. P 17



3 Valencies ofradicals.

Define a radical.Recall the valencies ofcommon radicals.

Exposition – teacher definesa radical, gives examples ofradicals and exposes theirvalencies.Students draw a table ofradicals and their valencies.

P 18

4 Oxidation number. Define oxidationnumber.Predict oxidationnumbers from positionof elements in theperiodic table.

Q/A: Valencies.Expose oxidation numbersof common ions.Students complete a tableof ions and their oxidationnumbers.

The periodictable.

P 18

5 1 Electronicconfiguration, ionformed, valency andoxidation number

Relate electronicconfiguration, ionformed, valency andoxidation number ofdifferent elements.

Written exercise;Exercise review.

P 18

2 Chemical formulaeof compounds.- Elements of equalvalencies.

To derive the formulaeof some compoundsinvolving elements ofequal valencies.

Discuss formation ofcompounds such as NaCl,MgO.

PP 19-20

3 Chemical formulaeof compounds.-Elements ofunequal valencies.

To derive the formulaeof some compoundsinvolving elements ofunequal valencies.

Discuss formation ofcompounds such as MgCl2Al (NO3)3

PP 19-20



4 Chemical formulaeof compounds.-Elements ofvariable valencies.

To derive the formulaeof some compoundsinvolving elements ofvariable valencies.

Discuss formation ofcompounds such as-Copper (I) Oxide.-Copper (II) Oxide.-Iron (II) Sulphate.-Iron (III) Sulphate.

P 20

6 1 Chemical equations. To identify componentsof chemical equations.

Review word equations;Exposition of new conceptswith probing questions;Brief discussion.

PP 21-23

2 Balanced chemicalequations.

To balance chemicalequations correctly.

Exposition;Supervised practice.

PP 24-25

3 Balanced chemicalequations.(contd)

To balance chemicalequations correctly.

Supervised practice;Written exercise.

PP 25-8

4 TEST

7 1 CHEMICALFAMILIES

Alkali metals.

Atomic and ionicradii of alkali metals

Identify alkali metals.State changes in atomicand ionic radii of alkalimetals.

Q/A to reviews elements ofgroup I and their electronicconfiguration.Examine a table ofelements, their symbolsand atomic & ionic radii.Discussion & makingdeductions from the table.

The periodicPP 28-29



2 Ionisation energy ofalkali metals.

State changes innumber of energy levelsand ionisation energy ofalkali metals.

Examine a table ofelements, number of energylevels and their ionizationenergy.Discuss the trend deducedfrom the table.

3,4 Physical propertiesof alkali metals.

State and explain trendsin physical properties ofalkali metals.

Examine a table showingcomparative physicalproperties of Li, Na, and K.Q/A: Teacher asks probingquestions as students referto the table for answers.Detailed discussion onphysical properties of alkalimetals.

Chart –comparativeproperties of Li,Na, K.

PP 30-31

8 1 Chemical propertiesof alkali metals.

To describe reaction ofalkali metals withoxygen.

Q/A: review reactions ofNa, K, etc. with oxygen.The corresponding wordand then chemicalequations are then written.

P 31

8 2 Chemical propertiesof alkali metals.

To describe reaction ofalkali metals with water.

Q/A: Review reaction ofmetals with water.Writing down chemicalequations for the reactions.Deduce and discuss theorder of reactivity down thegroup.

P. 32



3,4 Reaction of alkalimetals with chlorinegas.

To write balancedequations for reaction ofalkali metals withchlorine gas.

Teacher demonstration-reaction of sodium withchlorine in a fumechamber.Q/A: Students to predict asimilar reaction betweenpotassium and chlorine.Word and balancedchemical equations forvarious reactions.

Sodium,chlorine.

P. 33

9 1 Compounds of alkalimetals.

Write chemical formulaefor compounds of alkalimetals.Explain formation ofhydroxides, oxides andchlorides of alkalimetals.

Exercise: Completing atable of hydroxides, oxidesand chlorides of alkalimetals.Discuss combination ofions of alkali metals withanions.

2 Uses of alkalimetals.

State uses of alkalimetals.

Descriptive approach:Teacher elucidates uses ofalkali metals.

9 3 Alkaline Earthmetals

Atomic and ionicradii of alkalineearth metals.

Identify alkaline earthmetals.

State changes in atomicand ionic radii ofalkaline earth metals.

Q/A: Elements of group Iand their electronconfiguration.Examine a table ofelements, their symbolsand atomic & ionic radii.Make deductions from thetable.

Some alkalineearth metals.



4 Physical propertiesof alkaline earthmetals.

State and explain trendsin physical properties ofalkaline earth metals.

Examine a table showingcomparative physicalproperties of Be, Mg, Ca.Q/A: Teacher asks probingquestions as students referto the table for answers.Detailed discussion ofphysical properties ofalkaline earth metals.


P. 35

10 1 Electrical propertiesof alkaline earthmetals.

To describe electricalproperties of alkalineearth metals.

Teacher demonstration: -To show alkaline metals aregood conductors of electriccharge.

Alkaline earthmetals.

P. 37

2 Chemical propertiesof alkaline earthmetals.Reaction of alkalineearth metals withoxygen.

To describe reaction ofalkaline earth metalswith oxygen

Q/A: Review reactions ofMg, Ca, with oxygen.The corresponding wordand then chemicalequations are then writtenand their correctnessverified by the teacher.

P. 38

10 3 Chemical propertiesof alkaline earthmetals.Reaction of alkalineearth metals withwater.

To describe reaction ofalkaline earth metalswith water.

Q/A: Review reaction ofmetals with water.Writing down word andbalanced chemicalequations for the reactions.Deduce and discuss theorder of reactivity down thegroup.


P. 39



4 Reaction of alkalineearth metals withchlorine gas.

To write balancedequations for reaction ofalkaline earth metalswith chlorine gas.

Teacher demonstration-Reaction of sodium withchlorine in a fumechamber.Q/A: Students to predict asimilar reaction betweenpotassium and chlorine.Word and balancedchemical equations forvarious reactions.Supervised practice.

Sodium,chlorine.

P. 41

11 1 Reaction of alkalineearth metals withdilute acids.

To describe reaction ofalkaline earth metalswith acids.

Group experiments-Drop a ribbon of Mg indilute HCl, H2SO4.Test for evolved gas with aburning splint.

Magnesiumribbon, diluteHCl, diluteH2SO4.

P. 42

2 Reaction of alkalineearth metals withdilute acids.

To write balancedequations for reactionsof alkaline earth metalswith dilute acids.

Changing word to chemicalequations.Supervised practice.

PP. 43

11 3 Chemical formulaeof alkaline earthmetals.

Write chemical formulaefor compounds ofalkaline earth metals.Explain formation ofhydroxides, oxides andchlorides of alkalineearth metals.

Exercise: Completing atable of hydroxides, oxidesand chlorides of alkalineearth metals.Discuss combination ofions of alkaline earthmetals with anions.

PP. 45-47



4 Uses of somealkaline earthmetals and theircompounds.

State uses of alkalineearth metals.

Descriptive approach:Teacher elucidates uses ofalkaline earth metals.

PP. 45-47

12-13 END OF FIRST TERM EXAMS

SCHEME OF WORK FORM TWO CHEMISTRY TERM TWO 2020WKNO. L/

NOTOPIC/SUBTOPIC



MATERIALS/




1 1 Halogens.

Physical propertiesof halogens.

Identify halogens in theperiodic table.Give examples ofhalogens.Identify physical statesof halogens.

Teacher demonstration: -To examine electricalproperties of iodine,solubility in water ofchlorine.

Iodine crystals,electrical wire, abulb.

KLB BK IIP. 47

2 Comparativephysical propertiesof halogens.

To state and explain thetrends in physicalproperties of halogens.

Examine a comparativetable of physical propertiesof halogens.Discuss the deductionsmade from the table.

P. 47

3,4 Chemical propertiesof halogens.

To describe laboratorypreparation of chlorinegas.

To describe reaction ofhalogens with metals.

Teacher demonstration: -preparation of chlorine gas.Reaction of chlorine andiron wool.Reaction of bromine andiron wool.Reaction of iodine and ironwool.Observe the rate of thesereactions; hence deduceorder of their reactivity ofhalogens.

Chlorine, ironwool, bromine.

PP. 48-50

2 1 Equations ofreaction of halogenswith metals.

To write balancedchemical equations ofreactions involvinghalogens.

Re-write word equations aschemical equations thenbalance them.Supervised practice.

P. 50



2 2 Reaction of halogenswith water.

To describe reaction ofhalogens with water andthe results obtained.

Bubbling chlorine gasthrough water.Carry out litmus test forthe water.Explain the observations.

Chlorine gas,litmus papers.

P. 51

3,4 Some uses ofhalogens and theircompounds.

To state uses ofhalogens and theircompounds.

Teacher elucidates uses ofhalogens and theircompounds.

3 1 Noble Gases.

Comparativephysical propertiesof noble gases.

To describe physicalproperties of noblegases.To explain physicalproperties of noblegases.

Make A comparative analysis oftabulated physicalproperties of noble gases.

PP. 52-53

2 Uses of noble gases. State uses of noblegases.

Teacher elucidates uses ofnoble gases.

P. 54

3 STRUCTURE &BONDING

Chemical bonds.

Ionic bond.

Describe role of valenceelectrons in determiningchemical bonding.

Explain formation ofionic bonding.

Q/A: Review valenceelectrons of atoms ofelements in groups I, II, III,VII and VIII.Q/A: Review group I andgroup VII elements.Discuss formation of ionicbond.

P54

PP 57-58



4 Ionic bondrepresentation.

Use dot and crossdiagrams to representionic bonding.

Drawing diagrams of ionicbonds.

Chart- dot andcross diagrams.Models forbonding.

P. 58

41

Grant ionicstructures.

Describe the crystallineionic compound.Give examples of ionicsubstances.

Discuss the group ionicstructures of NaCl.Teacher gives examples ofother ionic substances:KNO3, potassium bromide,Ca (NO3)2, sodium iodide.

Giant sodiumchloride model.

PP 56-58

2 Physical propertiesof ionic compounds.

Describe physicalproperties of ioniccompounds.Explain the differencesin the physicalproperties of ioniccompounds.

Analyse tabulatedcomparative physicalproperties of ioniccompounds.

Teacher asks probingquestions.

PP 58-59

3,4 Covalent bond. Explain the formation ofcovalent bondUse dot and crossdiagrams to representcovalent bond.

Exposition: Shared pair ofelectrons in a hydrogenmolecule, H2O, NH3, Cl2,and CO2.Drawing of dot-and-crossdiagrams of covalent bonds.

PP 60-63

5 1 Co-ordinate bond. To describe the co-ordinate bondTo represent co-ordinatebond diagrammatically.

Exposition- teacherexplains the nature of co-ordinate bond.Students represent co-ordinate bonddiagrammatically.

P 65



2 Molecular structure. To describe themolecular structure.To give examples ofsubstance exhibitingmolecular structure

Discussion – To explainformation of the giantstructure and giveexamples of substanceexhibiting molecularstructure.

P 65

3 &4

Trend in physicalproperties ofmolecularstructures.

To describe van- der -waals forces.To explain the trend inphysical properties ofmolecular structures.

Discuss comparativephysical properties ofsubstances. exhibitingmolecular structure.Explain variation in thephysical properties.

Sugar,naphthalene,iodine rhombicsulphur.

P 65

6 1 Giant atomicstructure indiamond.

To describe giant atomicstructure in diamond.To state uses ofdiamond.

Diagrammaticrepresentation of diamond.Discuss uses of diamond.

Diagrams intextbooks.

P 69

2 Giant atomicstructure ingraphite.

To describe giant atomicstructure in graphite.To state uses ofgraphite.

Diagrammaticrepresentation of graphite.

Discuss uses of graphite.

Diagrams intextbooks.

3 Metallic bond.

Uses of somemetals.

To describe mutualelectronic forcesbetween electrons andnuclei.To describe metallicbond.To compare physicalproperties of metals.To state uses of somemetals.

Discussion:Detailed analysis ofcomparative physicalproperties of metals andtheir uses.

Probing questions & briefexplanations.

P 70



4TEST

7 1 PROPERTIES ANDTRENDS ACROSSPERIOD THREE

Physical propertiesof elements inperiods.

To compare electricalconductivity of elementsin period 3

Group experiments-Construct electrical circuitsincorporating a magnesiumribbon, then aluminum foil,then sulphur in turns.The brightness of the bulbis noted in each case.Discuss the observations interms of delocalisedelectrons.

The periodictable.

P. 76

2 Physical propertiesof elements inperiod 3.

To compare otherphysical properties ofelements across period3.

Analyse comparativephysical propertiespresented in form of atable.Explain the trend in thephysical properties given.

The periodictable.

P. 77

3 Chemical propertiesof elements inperiod 3.

To compare reactions ofelements in period 3with oxygen.

Q/A: Products of reactionsof Na, Mg, Al, P, & S withoxygen.Discuss the trend in theirreactivity; identify basicand acidic oxides.Exercise – balancedchemical equations for theabove reactions.

The periodictable.

PP. 79-80



4 Chemical propertiesof elements in thethird period.

To compare reactions ofelements in period 3with water

Q/A: Review reaction ofsodium, Mg, chlorine, withwater.Infer that sodium is mostreactive metal; non-metalsdo not react with water.

The periodictable.

PP. 80-81

8 1 Oxides of period 3elements.

To identify bonds acrosselements in period 3.To explain chemicalbehavior of their oxide.

Comparative analysis,discussion and explanation.

The periodictable.

P. 84

2 Chlorides of period 3elements.

To explain chemicalbehavior of theirchlorides.To describe hydrolysisreaction.

Comparative analysis,discussion and explanation.

The periodictable.

PP. 77-78

3,4 SALTS

Types of salts.

Define a salt.Describe various typesof salts and give severalexamples in each case.

Descriptive approach.Teacher exposes newconcepts.

P. 91

9 1,2 Solubility of salts inwater.

To test solubility ofvarious salts in coldwater/warm water.

Class experiments- Dissolvesalts in 5 cc of water.Record the solubility in atable,Analyse the results.

Sulphates,chlorides,nitrates,carbonates ofvarious metals.

PP. 92-93



3,4 Solubility of bases inwater.

To test solubility ofvarious bases in water.To carry out litmus teston the resultingsolutions.

Class experiments- Dissolvesalts in 5cc of water.Record the solubility in atable,Carry out litmus tests.Discuss the results.

Oxides,hydroxides, ofvarious metals,litmus papers.

PP. 94-95

10 1-4 Methods ofpreparing varioussalts.

To describe variousmethods of preparingsome salts.

Experimental anddescriptive treatments ofpreparation of salts e.g.ZnSO4, CuSO4, NaCl andPb(NO3)2.

CuO, H2SO4, HCl,NaOH, PbCO3, dilHNO3.

11 1,2 Direct synthesis of asalts.

To describe directsynthesis of a salt.To write balancedequations for thereactions.

Group experiments-preparation of iron (II)sulphide by directsynthesis.Give other examples of saltsprepared by directsynthesis.Students write downcorresponding balancedequations.

Iron,Sulphur

P. 104

3,4 Ionic equations. To identify spectatorions in doubledecompositionreactions.To write ionic equationscorrectly.

Q/A: Ions present in givenreactants.Deduce the products ofdouble decompositionreactions.Give examples of equations.Supervised practice.

PbNO3, MgSO4solutions.



1213 END OF SECOND TERM TEST

SCHEME OF WORK FORM TWO CHEMISTRY TERM THREE 2020WKNO. L/

NOTOPIC/SUBTOPIC



MATERIALS/


1 1 Effects of heat oncarbonates.

To state effects of heaton carbonates.To predict productsresulting from heatingmetal carbonates.

Group experiments- Toinvestigate effects of heaton Na2CO3, K2CO3, CaCO3,ZnCO3, PbCO3, e.t.c.Observe various colourchanges before, during andafter heating.Write equations for thereactions.

Variouscarbonates.

PP. 108-109

2 Effects of heat onnitrates.

To state effects of heaton nitrates.To predict productsresulting from heatingmetal nitrates.

Group experiments- Toinvestigate effects of heaton various metal nitrates.Observe various colourchanges before, during andafter heating.Write equations for thereactions.

Common metalnitrates.

PP. 110-111



3,4 Effects of heat onsulphates.

To state effects of heaton sulphates.To predict productsresults from heatingmetal sulphates.

Group experiments- Toinvestigate effects of heaton various sulphates.Observe various colourchanges before, during andafter heating.Write equations for thereactions.

Commonsulphates.

P. 113

2 1 Hygroscopy,Deliquescence andEfflorescence.

To define hygroscopicdeliquescent andefflorescent salts.To give examples ofhygroscopicdeliquescent andefflorescent salts.

Prepare a sample of varioussalts.Expose them to theatmosphere overnight.Students classify the saltsas hygroscopic,deliquescent and / orefflorescent.

P. 114

2 Uses of salts. To state uses of salts Teacher elucidates uses ofsalts.

P. 114

3,4 EFFECTS OF ANELECTRICCURRENT ONSUBSTANCES.

Electricalconductivity.

To test for electricalconductivities ofsubstances.

Group experiments- toidentify conductors andnon-conductors.Explain the difference in(non) conductivities.

Various solids,bulb, battery, &wires.

PP. 118-119

3 1,2 Molten electrolytes. To test for electricalconductivities moltenelectrolytes.

Group experiments- toidentify electrolytes inmolten form.Explain the difference inmolten electrolytes.

Molten candlewaxSugarSulphurLead oxide.

PP. 120-121



3,4 Electrolysis. To define electrolysisTo describe the processof electrolysis in termsof charge movement.

Descriptive approachpunctuated with Q/A.

4 1,2 Aqueouselectrolytes.Electrodes.

To define an electrolyteTo test for electricalconductivities ofelectrodes.

To investigate chemicaleffect of an electric current.Classify the solutions aselectrolyte or non -electrolytes.Discuss the electricalproperties of the solutions.

GraphiteelectrodesBatteryVarious aqueoussolutions switchbulb.

PP.122-123

3,4 Reaction onelectrodes.

To describe half-equation reactions atthe cathode and anode

To demonstrate –Electrolysis of molten lead(II) bromideObserve colour changesExplanation of half-equations and reactions atthe electrodes.

GraphiteelectrodesBatteryVarious aqueoussolutions switch.

PP.126-127

5 1,2 Binary electrolyte. To define a binaryelectrolyte.To state the products ofa binary electrolyte.

Completing a table ofelectrolysis of binaryelectrolytes.

P.127

3 Application ofelectrolysis.

To state application ofelectrolysis.

Discussion andexplanations.

P. 128



4 Electroplating. To describeelectroplating process.

Experiment- Left overnight.Electroplating an iron nailwith silver nitrate/ coppersulphate.Brief discussion.

Silver nitrateIron nailComplete circuitbattery.

PP. 129-30

6 1 Topic assessment.

2 CARBON ANDSOME OF ITSCOMPOUNDS.

Allotropy.

Define allotropes andallotropy.Identify allotropes ofcarbon.Represent diamond andgraphitediagrammatically.

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

PP. 131-133

3,4 Physical andchemical propertiesof diamond, graphiteand amorphouscarbon

Describe physical andchemical properties ofdiamond, graphite andamorphous carbon.State uses of carbonallotropes.

Discuss physical andchemical properties ofdiamond, graphite andamorphous carbon.Explain the Physical andchemical properties ofdiamond, graphite andamorphous carbon.Discuss uses of carbonallotropes.

Charcoal,graphite.

7 1 Burning carbon andoxygen.

Describe reaction ofcarbon with oxygen.

Teacher demonstration-Prepare oxygen and passdry oxygen into a tubecontaining carbon. Heat thecarbon. Observe effects onlimewater.

Carbon,limewater, tube,limewater stand&Bunsen burner.

PP. 134-135



2 Reduction propertiesof carbon.

Describe reductionproperties of carbon.Show reductionproperties of carbon.

Teacher demonstration –Burn strongly a mixture ofcarbon and CuO on a bottletop.Observe colour changesand give underlyingexplanation

CuO, poundedcharcoal, Bunsenburner& bottletop

P.126

3&4 Reaction of carbonwith acids.

Preparation of CO2.

Describe reaction ofcarbon with acids.

Prepare CO2 in the lab.

Teacher demonstration-reaction of carbon with hotconc HNO3.Write balanced equationsfor the reaction.

Review effects of heat oncarbonates.Group experiments/teacherdemonstration- preparationof CO2.

Conc. HNO3,limewater.

P.126

8 1,2 Properties of CO2. Describe properties ofCO2

Simple experiments todetermine properties ofCO2.

Discuss the observations.

Lime water,Magnesiumribbon,Universalindicator,lit candle.

PP.138-139

3,4 Chemical equationsfor reactionsinvolving CO2.

Write balanced CO2. Give examples of reactions.Write correspondingbalanced chemicalequations.

PP.139-140

9 1 Uses of CO2. State uses of CO2 Discuss briefly the uses ofCO2.

PP.140-1



2 Carbon monoxidelab preparation.

To describe preparationof carbon monoxide inthe lab

Teacher demonstration:preparation of carbonmonoxide in the lab.Make observations.

PP. 142-143

3 Chemical propertiesof carbon monoxide.

To describe chemicalproperties of carbonmonoxide.

Description of properties ofcarbon monoxide.Discussion and writing ofchemical equations.

PP. 44-145

4 Carbonates andhydrogencarbonates.

To state the differencebetween carbonates andhydrogen carbonates.To describe chemicalreactions of carbonatesand hydrogencarbonates with acids.

Observe reactions ofcarbonates of Ca, Cu, Zn,NaHCO3 with HCl, HNO3,and H2SO4.

Record observations in atable.

Carbonates of Ca,Cu, Zn, NaHCO3with HCl, HNO3,and H2SO4.

PP.148-149

10 1 Carbonates andhydrogencarbonates.

To write chemicalequations for reactionsof carbonates andhydrogen carbonateswith acids.

Discuss the observationsabove.Write chemical equationsfor the reactions.

2 Heating carbonatesand hydrogencarbonates.

To investigate reactionsof carbonates andhydrogen carbonates onheating.

Heat the above carbonatesand record observations ina table.

Variouscarbonates andhydrogencarbonates.

3,4 Heating carbonatesand hydrogencarbonates.

To write equations forreaction of carbonatesand hydrogencarbonates on heating.

Discuss the aboveobservations.Write correspondingbalanced equations.

PP.150-151



11 1 Extraction ofsodium carbonatefrom trona.

To draw schematicdiagram for extraction ofsodium carbonates.

Discuss each step of theprocess.Write relevant equations.

PP. 153-157

2 Solvay process ofpreparing sodiumcarbonate.

To draw schematicdiagram for extraction ofsodium carbonates.

Discuss each step of theprocess.

Write relevant equations.

3,4 Importance ofcarbon in nature.& itseffects on theenvironment.

To discuss: - Importanceof carbon in nature.&Effects of carbon on theenvironment.

Discuss the carbon cycleand processes thatincrease/ reduce amount ofCO2 in the air.Uses of CO2 in soft drinksand fire extinguishers.

PP.157-158

1213 END OF YEAR EXAMS


SALTS

Documents

· 2020. 7. 11. · BOOKII PP.1-3 2 Firsttwenty elementsofthe periodictable. Listthefirsttwenty elementsoftheperiodic table. Writechemicalsymbols ofthefirsttwenty elementsoftheperiodic