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SMK RAJA PEREMPUAN, IPOHCHEMISTRY LESSON PLAN

UPPER SIX 2010

FIRST TERM [ 5 / 1 / 2010 29 / 5 / 2010 ]

Week Learning objective Learning outcome Material

8. THERMOCHEMISTRY AND CHEMICAL

ENERGETICS (7 periods)

8.1 Enthalphy changes, H, of reactions, formation,

combustion, neutralisation, hydration, fusion,

atomisation, solution

8.2 Hess law

8.3 Lattice energies for simple ionic crystals. A

qualitative appreciation of their effects of ioniccharge and ionic radius on the magnitude of

lattice energy

Candidates should be able to:

1. explain that most chemical reactions are accompanied by

energy changes, principally in the form of heat energy ;

the energy changes can be exothermic or endothermic.

2. calculate the heat energy change from experimental

measurements using the relationship : energy change =

mcT

3. define the term enthalphy change of formation, combustion,

hydration, solution, neutralisation, atomisation, ionisation

energy4. explain the terms enthalphy change of reaction and standard

conditions

5. calcualte enthalphy changes from experimental results

6. state Hess law and its use to find enthalphy changes that

cannot be determined directly, eg an enthalphy change of

formation from enthalphy changes of combustion.

7. construct energy level diagrams relating the enthalphy to

reaction path and activation energy

8. define lattice energy for simple ionic crystals in terms of the

change from gaseous ions to solid lattice.9. explain qualitatively the effects of ionic charge and ionic

radius on the numerical magnitude of lattice energy values.

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8.4 The Born-Haber cycle for the formation of

simple ionic crystals and their aqueous solution

8.5 The solubility of solids in liquids

10. construct energy cycles for the formation of simple ionic

crystals and their aqueous solutions.

11. calculate enthaphy changes from energy cycles

12. explain qualitatively the influence on solubility of therelationship between enthalphy change of solution, lattice

energy of solid, and enthalphy change of hydration, or other

solvent / solute interaction.

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15. THE CHEMISTRY OF CARBON (10 periods)

15.1 Bonding of the carbon atoms: the shapes of the

ethane, ethene, ethyne and benzene molecules.

15.2 General, empirical, molecular and structural

formulae for organic chemistry.

15.3 Isomerism structural, geometric and optical

Candidates should be able to :

1. explain the concept of hybridisation in the bonding of carbon

atoms with reference specially to carbon atoms which have avalency of four and the types of hybridization such as the

following : sp linear , sp2 triangular, sp3 tetrahedral

2. describe the formation of and bonds as exemplified bydiagrams of the overlapping of orbitals in CH4, C2H4, C2H2

and C6H6 molecules.3. explain the concept of delocalisation of electrons in

benzene rings (aromaticity)

4. explain the meaning of general, empirical, molecular and

structural formulae of organic compounds

5. calculate empirical formulae and derive molecular formulae

6. interpret structural isomerism with reference to the ability of

carbon atoms to link together with each other in a straightline and / or in branches

7. explain geometric / cis-trans isomerism in alkenes in terms of

restricted rotation due to bond / C = C bonds8. explain the meaning of a chiral center and how such a center

gives rise to optical isomerism

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15.4 Classification based on functional groups

(general formula)

15.5 Nomenclature and structural formulae for each

functional / radical group (refer to their trivialnames)

15.6 Nucleophile and electrophile.

15.7 Structure and its effect on

(a) physical properties : eg boiling point, meltingpoint and solubility in water

(b) acidity and basicity

The effect of the structure and delocalisation of

electrons on the relative acid or base strength, ie

proton donors or acceptors, in ethylamine,

phenylamine, ethanol, phenol, and chlorine-

substituted ethanoic acids

9. identify chiral centers and / orcis-trans isomerism in a

molecule of given structural formula

10. determine the possible isomers for an organic compound of

known molecular formula

11. describe the classification of organic compounds by

functional groups and the nomenclature of classes of

organic compounds according to the IUP AC system of the

following classes of compounds :

(a) alkanes, alkenes

(b) haloalkanes

(c) alcohols (including primary, secondary and tertiary) and

phenols

(d) aldehydes and ketones

(e) carboxylic acids and esters

(f) primary amines, amides, and amino acids

12. define the term nucleophile and electrophile

13. describe the relationship between the size of molecules in

the homologous series and the melting and boiling points

14. explain the attractive forces between molecules (van der

Waals forces and hydrogen bonding)

l5. explain the meaning of Lewis acids and bases in terms of

charge / electron density

16. explain why many organic compounds containing oxygen /nitrogen which have lone pair electrons (as Lewis bases)

form bonds with electron acceptors (as Lewis acids)17. explain how nucleophiles such as OH-, NH3 , H2O, Br

- , I-

and carbanion have Lewis base properties, whereas

electrophiles such as H+, NO2+, Br2 , AICI3 , ZnCl2 , FeBr3,

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BF3, and carbonium ions have Lewis acid properties

18. explain induction effect which can determine the properties

and reactions of functional groups

19. explain how most functional groups such as -NO2 ,-CN,

-COOH , -COOR, > C=O , SO3H ,-X (halogen) , -OH, -OR,-NH2 , C6H5 are electron acceptors whereas functional

groups such as CH3, R, (alkyl or aryl) are electron donors

20. explain how the concept of induction can account for the

differences in acidity between CH3COOH, CICH2COOH ,

Cl2CHCOOH and CI3CCOOH ; between

CH2CH2CH2COOH and CH3CH2CHCICOOH

21. use the concept of delocalisation of electrons to explain the

differences in acidity between ethanol and phenol, as well as

the differences in basicity between CH3NH2 and C6H5NH2

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CHINESE NEW YEAR HOLIDAY

16 HYDROCARBONS (14 periods)

16.1 Alkanes, exemplified by ethane

(a) Free radical substitution, eg the effect of

chlorination of hydrocarbons in water on theenvironment (refer to 13.5)

(b) Free radical reactions illustrated by thereaction of methane with chlorine


1. explain alkanes as saturated aliphatic hydrocarbons

2. explain the construction of the alkane series (straight and

branched) and IUPAC nomenclature of alkanes for C1 to C53. name alkyl groups derived from alkanes and identify primary,

secondary , tertiary and quartenary carbons.

4. explain the homolytic cleavage of bonds which produces free

radicals that determine the mechanism of a reaction

5. explain the halogenation of alkanes and its mechanism as wellas the oxidation of alkane with limited and excess oxygen,

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(c) Crude oil as a source of energy andchemicals: cracking reactions (d) The

unreactivity of alkanes towards polar

reagents

and the use of alkanes as fuels6. explain the mechanism of free radical substitution

7. explain the use of crude oil as source of aliphatic

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(e) the effect of hydrocarbons on the

environment

16.2 Alkenes, exemplified by ethene

(a) Electrophilic addition

(b) Addition by electrophilic reagents,

illustrated by the reactions of bromine /

ethene or hydrogen bromide / ethene

(c) Simple tests for alkenes

(d) The importance of ethene in industry

16.3 Arenes, exemplified by benzene and

hydrocarbons 8. explain how cracking reactions can be used

to obtain alkanes

and alkenes of lower Mrfrom larger hydrocarbon molecules

9. show awareness of the environmental consequences of CO,CO2 and unburnt hydrocarbons arising from the internal

combustion engine.

10. define alkenes as unsaturated aliphatic hydrocarbons with

one or more double bonds

11. name alkenes according to the IUPAC nomenclature and the

common names for C1 to C5.

12. explain the mechanism of electrophilic addition in alkenes

13. explain the chemistry of alkenes as exemplified by thefollowing reactions of ethene :

(a) addition of hydrogen, steam, hydrogen halides, halogens

(decolourisation) of bromine water and concentrated

sulphuric acid

(b) oxidation -decolourisation of the manganate (VII) ions

(c) polymerisation

14. explain the use of bromination reaction and decolourisation

of MnO4- ions as simple tests for alkenes and unsaturated

compounds

methylbenzene (toluene)

(a) Electrophilic substitution reactions

(b) Influence of substitution groups to the

15. explain briefly the preparation of chloroethane, epoxyethane,

ethane-l,2-diol and polyethene

16. explain the nomenclature of aromatic compounds derived

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benzene ring on further substitution. The

effect of induction as exemplified by OH,

-Cl, CH3 , -NO2 , -COCH3 , -NH2

(c) Oxidation of the side-chain to produce

RCOOH. Halogenation in the side-chain or

aromatic nucleus depending on the reaction

conditions.

(d) Effects of arene compounds on health

from benzene and the use of o (ortho), m (meta) and p (para)

or the numbering of substitution groups to the benzene ring

17. describe the mechanism of electrophilic substitution in

arenes illustrated by the nitration of benzene18. explain the chemistry of arenes as exemplified by

substitution reactions of benzene and methylbenzene

(toluene) with halogen, HNO3, CH3I / AlCI3, CH3COCI and

SO319. explain why the benzene ring is more stable against oxidants

like KMnO4 and K2Cr2O7compared with aliphatic alkenes

20. explain how a reaction between an alkylbenzene and an

oxidant such as acidified KMnO4 will cause the carbon

atoms which are joined directly to the benzene ring to

become a carboxyl group, and the remaining alkyl chainswill turn into water and CO2

21. determine the products of halogenation of methylbenzene

(toluene) with Lewis acid catalysts such as AlCl3and FeCl3

and in the presence of light only

22. predict the reaction products when the substitution group in

benzene is an electron accepting or donating group

23. explain the uses of arene compounds as solvents

24. explain that arene compounds are carcinogenic

17 HALOALKANES (6 periods)

17.1 (a) Nucleophilic substitution reactions

(b) Reactivity of chlorobenzene compared with

chloroalkanes

Candidates should be able to

1. explain the chemistry of haloalkanes as exemplified by

(a) nucleophilic substitution reactions represented by the

hydrolysis of bromoethane, the formation of nitriles, and

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17.2 Nucleophilic substitution at the carbon atom in

haloalkanes

the formation of primary amines by reaction with NH3(b) haloalkane elimination reactions which produce alkenes

17.3 Relative reactivity of primary, secondary and

tertiary alkyl halides

17.4 Elimination reactions

17.5 Haloalkanes as the starting material in the

preparation of organometals

17.6 Uses of haloalkanes

17.7 Effects of haloalkanes on the environment

2. explain the mechanism of nucleophilic substitution in

haloalkanes

3. explain the difference in the reactivity of chlorobenzenecompared with chloroalkanes, with particular reference to

hydrolysis reactions.

4. explain the relative reactivity of primary, secondary and

tertiary alkyl halides

5. explain the use of haloalkanes in the synthesis of organometal

compounds such as the following :

(a) Reactions with lithium and magnesium to give

organolithium and organomagnesium (Grignard reagents)

compounds, and their respective uses in reactions with

carbonyl compounds, silicon halides (SiCl4) and tinhalides (SnCl4)

(b) Reactions of chloroethane witll Na/Pb alloy to give

tetraethyllead (IV)

6. explain the uses of fluoroalkanes and chlorofluoroalkanes as

inert substances for aerosol propellants, detergents, coolants,

fire-extinguishers and insecticides (DDT)

7. explain the bad effects of DDT and chlorofluoroalkanes on

the environment, especially in the depletion of the ozone layer8. explain the formation of ozone in the atmosphere and in

factories9. explain the role of ozone in the atmosphere, ie the ozone layer

as an absorber of ultraviolet light.

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UJIAN SELARAS BERFOKUS

18 HYDROXY COMPOUNDS (10 periods)

18.1 Classification of hydroxy compounds into

primary, secondary and tertiary alcohols

18.2 Reactions of hydroxy compounds

(a) Reactions of alcohols as exemplified by

ethanol

(b) Use of triiodomethane test

(c) Comparison of the acidity of phenol, alcohol

and water (refer to 15.7)

(d) Reactions of phenol


1. describe the classification of hydroxy compounds into

primary, secondary, and tertiary alcohols and explain the

nomenclature of alcohols.

2. explain that most alcohol reactions can be divided into two

groups, ie

(a) the RO- H bond is broken and H is replaced by other

groups because alcohol and phenol, have the

characteristics of weak acid (formation of hydroxides and

phenoxides)(b) the R-OH bond is broken and OH is replaced by other

groups caused by nucleophilic substitution reactions

3. explain the chemistry of alcohol compounds as exemplified

by following reactions

(a) The formation of halogenoalkanes

(b) The formation of an alkoxide with sodium

(c) Oxidation to carbonyl compounds and carboxylic acids

(d) Dehydration to alkenes and ether

(e) Esterification

(f) Acylation

4. explain the difference in reactivity of primary, secondary and

tertiary alcohols as exemplified by(a) the reaction rate of such alcohols to give haloalkanes

(b) the reaction products of KMnO4 / K2Cr2O7 oxidation in

the presence of sulphuric acid

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MID-TERM HOLIDAY

5. explain the reactions of the alcohol with the structure computer, 8

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18.3 Preparation and manufacture of hydroxy

compounds

(a) Alcohol in the laboratory and industry(b) Phenol in industry

18.4 Use of hydroxy compounds in industry

(a) alcohol

(b) phenol

H

I

CH3 ---- C --- with alkaline aqueous iodine to give

I triiodomethane

OH6. discuss the relative acidities of water , phenol and ethanol

with particular reference to the inductive effect and the effect

of delocalised electrons

7. explain the reactions of phenol with sodium hydroxide,

sodium and acid chlorides8. explain the reactions of phenol with bromine water and

aqueous iron (III) chloride

9. describe the preparation and manufacture of alcohol from

(a) the hydration of ethane (in the laboratory and industry)

(b) natural gas and fermentation process (ethanol)10. describe the process of manufacturing phenol involving the

use of cumene

11. explain the uses of alcohol as antiseptic, solvent and fuel

12. explain the use of phenol in the manufacture of cyclohexanol

and hence nylon -6,6.

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19 CARBONYL COMPOUNDS (6 periods)

19.1 (a) Aldehydes, exemplified by ethanal

(acetaldehyde) and benzaldehyde(phenylmethanal)

(b) Ketones, exemplified by propanone and

phenylethanone

19.2 Preparation of carbonyl compounds


1. write the general formula for aldehydes and ketones, and

name their compounds according to the IUPAC nomenclatureand their common names.

2. write the reaction equations for the preparation of aldehydes

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19.3 Chemical reactions

(a) Aldehydes

-oxidation to carboxylic acids (with KMnO4)

-oxidation with Fehling's solution and Tollen'sreagent

(b) Ketones

-reaction with alkaline iodine as a

triiodomethane test for methylketone

(c) Aldehyde and Ketone

-reduction to alcohols

-condensation with 2,4-dinitrophenylhydrazine

-nucleophilic addition witll hydrogen cyanide

19.4 Reducing sugar and carbohydrates as examples of

natural compounds which have the functional

groups -OH and >C=O, eg glucose and cellulose,

with cellulose as a polymer for glucose

and ketones

3. determine the properties of an unknown carbonyl compound

- aldehyde or ketone -on the results of simple tests (eg

Fehling's solution, Tollen's reagent and ease of oxidation)

4. explain the reaction of ketone compounds with the

structure CH3 ---C = O with alkaline aqueous iodine to give

I triiodomethane.

5. explain the reduction reactions of aldehydes or ketones to

primary and secondary alcohols through catalytic

hydrogenation reaction and with LiAlH46. explain the use of 2,4-dinitrophenylhydrazine reagent as a

simple test to detect the presence of >C=O groups.7. explain the mechanism of the nucleophilic addition reactions

of hydrogen cyanide with aldehydes or ketones

8. explain that natural compounds such as glucose, sucrose and

other carbohydrates have the >C=O group

9. explain the characteristics of glucose as reducing sugar

20 CARBOXYLIC ACIDS (4 periods)

Carboxylic acids as exemplified by ethanoic acidand benzoic acid

(a) Preparation of carboxylic acids by the oxidation

of primary alcohols and hydrolysis of nitriles


1. name aliphatic and aromatic acids according to IUPACnomenclature, and their common names for C1 to C6

2. write the reaction equations for the formation of carboxylic

acids from alcohols, aldehydes and nitriles

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(b) Chemical reactions of carboxylic acids

(c) Uses of carboxylic acids in industry

3. explain the acidic characteristics of carboxylic acids

compared with HCI, HNO3 or H2SO4 and their reactions

with bases to form salts

4. explain the substitution of the -OH group by the nucleophiles

-OR and -Cl to form esters and acyl chlorides respectively5. explain the reduction of carboxylic acids to primary alcohols

6. explain the oxidation and dehydration of methanoic and

ethanoic acids

7. explain the various uses of carboxylic acids in foods,

perfumes, polymers and other industries

] 21 CARBOXYLIC ACID DERIVATIVES (6

periods)

21.1 Acyl chlorides

(a) Relative reactivity -hydrolysis of acylchlorides and alkyl chlorides

(b) Chemical reactions with alcohols, phenols,

and primary amines

21.2 Esters as exemplified by ethyl ethanoate and

phenyl benzoate

(a) Preparation of esters from carboxylic acids and

acyl chlorides(b) Chemical reactions of esters

(c) Fats and oils as natural esters: general structure

of glycerol ester derivatives of given long-

chain carboxylic acids

(d) Uses of esters


1. compare the ease hydrolysis of acyl chlorides with that of

alkyl chlorides

2. explain the formations of esters by the reactions of acylchlorides with alcohols and phenols

3. explain the formations of amides by the reaction of acyl

chlorides with primary amines

4. explain the acid and base hydrolysis of esters: saponification

5. explain the reduction of esters to primary alcohols

6. explain tile importance of esters as fats and oils

7. explain the use of esters as taste enhancers, flavourings,

preservatives, solvents and in the production of polyesters

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21.3 Amides as exemplified by ethanamide

(a) Preparation of amides

(b) Hydrolysis of amides

8. explain the nomenclature of amides according to the IUPAC

system

9. explain the preparation of primary and secondary amides from

reactions of acid chlorides with amines

10. explain the hydrolysis of amides in acidic or basicconditions.

22 AMINES (4 periods)

Primary amines as exemplified by ethylamine and

phenylamine

(a) Preparation of amines (refer to 17.1)

(b) Chemical reactions of amines with mineral

acids, nitrous acid and with aqueous bromine

(refer to practical chemistry)


1. name amines according to the IUPAC nomenclature and their

common names

2. explain the preparation of ethylamine by the reduction ofnitriles, phenylamine by the reduction of nitrobenzene and

amine by the nucleophilic substitution reaction between

ammonia and alkyl halides .

3. explain the formation of salts when amines react with mineral

acids

4. differenciate between primary aliphatic amines and primary

aryl (aromatic) amines by their respective reactions with

nitrous acid and aqueous bromine

5. explain the structures of diazonium ion and diazonium salt6. explain the formation of dyes by the coupling reaction of the

diazonium salt (benzenediazonium chloride) and phenol

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23 AMINO ACIDS AND PROTEINS (4 periods)

23.1 Amino acid as exemplified by aminoethanoic

acid (glycine) and 2-aminopropanoic acid

(alanine)


1. explain the structure and general formula of amino acid with

one amino group.

2. identify the chiral center in the amino acid molecules.

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(a) General formula and structure of amino acids

(b) Acid / base properties

(c) Formation of zwitterions

(d) Formation of the peptide linkage

23.2 Protein-structure and hydrolysis of proteins

23.3 Importance of amino acids and proteins

3. explain the acid/ base properties of amino acids.

4. explain the formation of zwitterions

5. explain the peptide linkage as amide linkage formed by the

condensation between amino acids as exemplified by

glycylanine and ananilglycine

6. explain that the protein structure is based on the peptide

linkage

7. explain the hydrolysis of proteins

8. explain the roles of amino acids and proteins in the biological

system.

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24 POLYMERS (9 periods)

24.1 Introduction artificial/ synthetic polymers,

natural polymers and copolymers.

24.2 Preparation

(a) Condensation polymerisation

(b) Addition polymerisation, including free

radicals and ionic (cationic and anionic)

reactions use of Ziegler Natta catalyst

24.3 Classifications of polymers

24.4 Use of polymers in daily life


1. explain the meaning of monomer, polymer, repeating unit

and copolymer.2. identify monomers in a polymer

3. explain polymerisation

4. explain condensation polymerisation and addition

polymerisation

5. explain addition polymerisation which involves free radicals

and ionic reactions mechanism

6. explain the use and role of the Ziegler Natta catalyst in theaddition polymerisation process

7. suggest polymers which can be prepared from a monomer or apair of monomer

8. identify the manufacturing process for the preparation of

polyethene / polyethylene / PE, polypropene / propylene / PP,

polyphenylethene / polystyrene / PS and SBR synthetic

rubber, ie phenylethene-buta-1,3-diene / styrene-butadiene

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24.5 Natural rubber (2-methybuta-1,3-diene) polymer

or polyisoprene

(a) Microstructure : cis and trans forms

(b) Production of bulk rubber from latex(c) Vulcanisation

(d) Uses of latex and bulk rubber

copolymer

9. explain the classification of polymers as thermosetting,

thermoplastic and elastomer depending on their thermal

properties

10. explain the uses of polyethylene, polypropylene,

polystyrene and synthetic rubber (styrene-butadiene

copolymer) in the making of domestic products

11. explain the isoprene monomer in natural rubber

12. explain the existence of two isomers in poly(2-methylbuta-

1,3-diene)

(a) the elastic cis form (from the Hevea brasiliensis trees)

(b) the inelastic trans form (from the gutta percha trees)

13. explain the process of producing bulk rubber from latex14. explain the formation of cross-linkages via sulphur to change

the physical properties of natural rubber

15. explain the use of latex in the making of gloves, threads, etc,

and the use of bulk rubber in the making of tyres, belts, etc.

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MID-YEAR EXAM

MID-YEAR HOLIDAY

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SECOND TERM [ 15 / 6 / 08 20 / 11 / 08 ]

Week Learning Objective Learning outcome Material9. PERIOD 3 AND GROUP 2: SELECTED

PROPERTIES (4 periods)

9.1 Reaction of Period 3 elements, sodium to argon,

with oxygen and water

9.2 Acid / base properties of oxides and hydrolysis of

oxides (reaction with water)

9.3 Trends in trhe properties of nitrates, carbonates,

hydroxides and sulphates of Group 2 elements


1. describe the reactions of Period 3 elements with oxygen and

water

2. intrepret the ability of elements to act as oxidising and

reducing agents

3. describe and explain the acid / base properties of the oxides

of Period 3 elements

4. describe the properties and the reactions with water of the

oxides of Period 3 elements

5. describe the clasification of the oxides of Period 3 elements as

basic, amphoteric or acidic based on their reactions with

water, acid and alkali6. describe the thermal decomposition of the nitrates, carbonates

and hydroxides of Group 2 elements

7. interpret qualitatively and explain the thermal decomposition

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Week Learning Objective Learning outcome Material

of the nitrates, carbonates and hydroxides in terms of the

charge density and polarity of large anions.

8. interpret qualitatively and explain the variation in solubility of

sulphate, in terms of the relative magnitudes of the enthalphy

change of hydration for the relevant ions and thecorresponding lattice energy.

9. interpret, and make.predictions from, the trends in physical

and chemical properties of Group 2 compounds.

10 GROUP 13: ALUMINIUM (4 periods)

10.1 Extraction (refer to 7.10)


1. explain the electrolytic method of extraction of aluminium

from pure bauxite

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] 10.2 Bonding and properties of the oxides and

chlorides related to charge density of the Al3+ions

10.3 Acidic character of aqueous aluminium salts and

their reactions with concentrated aqueous alkalis

10.4 Resistance of aluminium to corrosion

10.5 Uses of aluminium and its compounds in industry

2. explain the relationship between charge density of the Al3+

ions and their bonding properties, and the oxides andchlorides

3. explain aluminium's affinity for oxygen in the Thermite

process

4. explain the acidic character of aqueous aluminium salts and

their reactions with concentrated aqueous alkalis

5. explain why the aluminium metal resist corrosion

6. describe some important uses of the aluminium metal inrelation to its resistance to corrosion, good electrical and

thermal conductivity and low density

7. describe the uses of the compounds containing aluminium in

modern industry, and examples of such compounds like

alloys, alums, zeolites and ceramics

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11 GROUP 14: C, Si, Ge, Sn, Pb (9 periods)

11.1 General study of the chemical trends for Group

14 elements and their oxides and chlorides

11.2 Bonding, molecular form, sublimation, thermal

stability, and hydrolysis of tetrachlorides,

including mixed chlorides of carbon (freon) (refer

to 17.7)

11.3 Bonding, acid /base nature, and thermal stabilityof the oxides of oxidation states II and IV


1. explain the changing trends in chemical properties of Group

14 elements and their oxides and chlorides

2. describe and describe the bonding in and molecular shape of

the tetrachloride

3. explain the formation of freon and the ill-effects of its use

4. explain the volatility, thermal stability and hydrolysis of the

chloride in terms of structure and bonding

5. describe and explain the bonding, acid-base nature and thestability of the oxides of oxidation states II and IV

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11.4 Relative stability for higher and lower states of

oxidation for e1ements from carbon to lead intheir oxides, chlorides and aqueous cations

11.5 (a) Structure of the covalent crystal of carbon,

eg, diamond and graphite

(b) Use of carbon in industry

11.6 (a) Use of silicon and silicate in industry

(b) Structure of silicate

6. describe and explain the relative stability of higher and lower

oxidation states of the elements in their oxides and aqueouscations

7. explain the existence of different coordination numbers

8. explain the descending property of catenation in the group

9. explain the relationship between the structure of covalent

crystal for graphite and diamond and their uses

10. explain the uses of carbon as a component in composite

material (such as bullet-proof jackets, fibre and amorphous

carbon)

11. explain the use of silicon as a semiconductor and silicone as

a fluid, elastomer and resin

12. explain the importance of silicate as a basic material for

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(c) Quartz glass and the effect of adding metallic

and non- metallic oxides

11.7 Use of tin alloys

cement, glass and ceramics

13. explain silicate, SiO44- , as a primary structural unit and

connect these units to form chains (pyroxenes and

amphiboles), sheets (mica) and framework structure (quartz)

14. outline the structure of kaolinite and montmorillonite15. explain the composition of soda glass, borosilicate glass,

quartz glass and lead glass

16. explain the effects of adding metallic and non-metallic

oxides to glass

17. describe the use of tin alloys in the production of solder and

pewter

12 GROUP 15: NITROGEN AND ITS

COMPOUNDS (9 periods)

12.1 Nitrogen

(a) The inert nature of nitrogen

(b) Principle of nitrogen extraction from air

12.2 Ammonia

(a) Its formation from ammonium salts (refer to

practical chemistry)

(b) Its properties as a base

(c) Its uses particularly in the manufacture of

nitric acid and fertilisers

12.3 Oxides of nitrogen (NO, NO2, N204)


1. explain the bonding in the nitrogen molecules2. explain the inertness of nitrogen in terms of high bonding

energy as well as the non-polar nature of nitrogen molecules

3. show knowledge of the principles of extraction of nitrogen

from air

4. explain the formation of ammonia from ammonium salts

5. explain the properties of ammonia as a base

6. exp1ain the importance of ammonia particularly in the

manufacture of nitric acid and fertilisers.

7. explain the structure of the oxides of nitrogen (NO, NO2,

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(a) Formation of the oxides of nitrogen in internal

combustion engines and from lightning

(b) Use of catalytic converters to reduce airpollution

N204)

8. explain how the oxides of nitrogen are produced in internal

combustion engines and from lightning

9. explain the function of catalytic converters to reduce airpollution by oxidising CO to CO2 and reducing NOx to N2

10. explain the effects of the oxides of nitrogen and sulphur on

air pollution

13. GROUP 17: CI, Br, I (6 periods)

13.1 Variations in the volatility and colour intensity ofthe elements


1. state that the colour intensity of the halogens increase on

going down the group in the Periodic Table.2. explain how the volatility of the halogens decrease on going

down the group in the Periodic Table.

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13.2 Relative reactivity of the elements as oxidizing

agents

13.3 Reactions of the elements with hydrogen, and the

relative stability of the hydrides (with reference

to the reactivity of fluorine comparatively)

13.4 Reactions of halide ions

13.5 Reactions of chlorine with aqueous sodium

hydroxide

13.6 Important uses of the halogens and halogen

compounds

3. explain the relative reactivity of these elements as oxidizing

agents

4. explain the order of reactivity between the halogens and

hydrogen as well as relative stability of the halides

5. explain and write equations of reactions between halide ions

with aqueous silver ions followed by aqueous ammonia (refer

to practical chemistry) and with concentrated sulphuric acid

6. explain the reactions of chlorine with cold and hot aqueous

sodium hydroxide

7. describe the important uses of the halogens and halogen

compounds as antiseptic, bleaching agent, in purifying water,

and in black-and-white photography (explained as an example

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of redox equation)

14 AN INTRODUCTION TO THE CHEMISTRY

OF d-BLOCK ELEMENTS (12 periods)

14.1 Chemical properties of d-block elements (Ti, Mn,Cr, and Fe)

(a) Variable oxidation states and colour changes

(refer to 7)

Note: No discussion of the zero and negative

oxidation states is required.


1. explain variable oxidation states in terms of the energies of 3d

and 4s orbitals2. explain the colour changes of transition metals ions in terms

of a half-filled 3d orbitals and state the colours of the

complex aqueous ions of elements

3. state the principle oxidation numbers of these elements in

their common cations, oxides and oxo ions

4. explain qualitatively the relative stabilities of these oxidation

states5. explain the use of standard redox potentials in predicting the

relative stabilities of aqueous ions

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(b) Formation of complex ions by exchange of

ligands

(c) Catalytic properties

(i) Heterogenous catalysis

(ii) Homogenous catalysis

6. explain the terms complex ion and ligand

7. explain the formation of complex ions by exchange ofligands, eg water, ammonia, cyanide ions, thiocyanide ions,

ethanadiote ions, ethylenediaminetetraethanoate and halide

ions; examples: [Fe(CN)6]4- , [Fe(CN)6]

3- ,

[Fe (H2O)5(SCN)]2+

8. explain the catalytic activity of transition elements in terms of

variable oxidation states (homogenous catalysis) or adsorption

by coordinate bond information (heterogenous catalysis)

9. explain heterogenous catalysis, eg Ni and Pt in the

hydrogenation of alkenes and Fe/Fe203 in the Haber process

10. explain the availability of the d-orbitals resulting in a

different mechanism of lower activation energy

11. explain homogenous catalysis in terms of the reduction of

Fe3+ by iodide ions and the subsequent reoxidation by S2082-

Ions

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14.2 Nomenclature of complex compounds

14.3 Bonding in complex ions

14.4 Stereoisomerism of complex ions and compounds

(refer to 15.3)

14.5 Use of d-block elements and their compounds, eg

chromium, manganese, cobalt and titanium (IV)

oxide

12. show understanding of the naming of complex compounds .

13. discuss coordinate bond formation between ligands and the

central metal ions, and state the type of ligands, iemonodentate, bidentate and hexadentate

14. explain the phenomenon of stereoisomerism :

(a) geometric isomers. eg cis and trans - [Cr(NH3)4Cl2]+ ,

merand fac [Cr(NH3)CI3] ;

(b) optical isomers. eg dand 1 -[Cr(C204)33-

15. explain the use of chromium in the hardening process of

steel and in stainless steel, cobalt and manganese in alloys,

and Ti02 as a pigment, eg in plastics and paint

SECOND MID-TERM BREAK

STPM TRIALHARI RAYA HOLIDAY

STRATEGIC REVISION

STPM EXAM

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