2011 Module Score A

8/6/2019 2011 Module Score A

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Checklist for Scoring A In Chemistry 2011

1

CHECKLIST

FOR

SCORING

GRADE A

IN

CHEMISTRY

SPM 2011


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Chapter 2: The Structure of the Atom

A. Knowledge (Definition,

meaning and facts)

Check

1) State the kinetic theory ofmatter.State one example to supportthe kinetic theory of matter

2) What are atom, molecule andion?

3) What is melting point?

4) Define proton number andnucleon number.

5) State the meaning of isotopes.

6) State the uses of isotopes suchas carbon-14 and cobalt-60.

1. The kinetic theory of matter states that matter is made up of tinyand discrete particle which can collide among the particle.For anexample,the diffusion of gas particle is faster than the diffusion ofliquid particles.2.- An atom is the smallest particle of an element that can

participate in a chemical reaction.-A molecule is a group of two or more atoms which are chemically

bonded together.-An ion is positively-charge or negatively-charge particle.

3. Melting point is the temperature at which a solid changes into aliquid at a particular pressure.4. Proton number defined as the number of proton in its atom,whilenucleon number defined as the total number of proton and neutronin its atom.5. The meaning of isotopes are atoms of the same element withsame proton number but different number of neutrons.6. The uses of carbon-14 is to estimate the age of fossil,whilecobalt-60 is used in radiotherapy for the treatment of cancer.

B. Understanding /

Application / Analysis7) Explain why the temperature

remains unchanged during themelting process.

8) Explain why the temperatureremains unchanged during thefreezing process.

9) A solid compound is heateduntil it converts into gas.

Explain the changes in energycontent, forces of attractionbetween the particles, andarrangement of particles.

10) State the main subatomicparticles of an atom.Compare and contrast therelative atomic mass and therelative charge of thesubatomic particles of theatom.

11) Al27

13is the symbol of

aluminium.(a) Determine the number ofneutron of aluminium.(b) Draw the electronarrangement of aluminium.

7. The temperature remain unchanged during the melting processbecause the heat energy absorbed by the particles is used toovercome the forces between particles so that the solid can turninto liquid.8. The temperature remain unchanged during the freezing processbecause the heat loss to the surrounding is exactly balanced by theheat energy liberated as the particles attract to one anotherto formsolid.9. When solid is heated,the more heat energy absorbed by theparticles to overcome the force of attraction between the

particle.Then,the arrangement of particle become random andmove freely.10.- The main subatomic particle are proton,neutron and electron.

- Relative atomic mass of the subatomic particles most areconcentrated in the nucleus,while the relative charge of thesubatomic particles are overall positive charge due to the positive-chargedof protons in the nucleus.11. (a) The number of neutron = 27-13

= 14(b)

C. Synthesis (Experiment)12) Solid Z has a melting point of

65oC. Describe a laboratoryexperiment to determine the

Al

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melting point of Z. Your answershould show how the meltingpoint of Z is determined.

13) Compound W has a freezingpoint of 82oC. Describe alaboratory experiment todetermine the freezing point of

W.

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Chapter 3: Chemical Formulae and Equations

A. Knowledge (Definition, meaning and

facts)

Check

1) State the meaning of relative atomic massbased on carbon-12 scale.

2) Define a mole.

3) State the meaning of molar mass

4) State the meaning of molar volume of gas.

5) State the meaning of empirical formula.

6) State the meaning of molecular formula.

1. The relative atomic mass based on carbon-12 scale isthe average mass of one atom of the element per of themass of carbon-12 atom.2. Mole defined as the amount of substance that containsas many particles as the number of atom is exactly 12 g of

carbon-12.3. Molar mass means the mass of a substance thatcontains one mole of the substance.4. Molar volume of gas defined as the volume of one moleof gas.5. Empirical formula is the simplest ratio of atoms of eachelement that present in the compound.6. Molecular formula is the actual number of atoms of eachelement that are present in one molecule of thecompound.

B. Understanding / Application /

Analysis

7) Explain why we couldnt determine theempirical formula of copper(II) oxide byheating copper powder in a crucible.

8) Compare and contrast empirical formulawith molecular formula using ethane as anexample.

9) Vinegar is a dilute ethanoic acid with amolecular formula of CH3COOH.(a) Find the empirical formula of ethanoicacid.(b) Find the percentage composition by

mass of carbon in ethanoic acid.

10) 3.6 g of carbon reacted with 0.8 g ofhydrogen to form a compound.(a) Determine the empirical formula of thecompound formed.(b) Given that the relative molecular massof the compound is 88 g, find its molecularformula.

[Relative atomic mass: C ,12; H, 1]

11) Hydrogen Gas is reacted with 20 g of hotcopper(II) oxide powders to produce solid

copper and water.(a) Write the chemical equation for thereaction.(b) Calculate the maximum mass of solidcopper formed.

[Relative atomic mass: Cu, 64; O,16;H,1]

7. This is because the reactivity of copper(ll) oxide is toolow.The method of heating a metal in a crucible is only forother high reactivity metal.8.

Empirical Formula Molecular Formula

Ethane,C2H6 - Ethaneconsists ofcarbon andhydrogenatom at theratio of 1:3.

- Therefore,one

mole ofcarbon atomscombine with3 moles ofhydrogenatoms.

- Each moleof ethanecontains 2moles ofcarbonatoms and6 moles of

hydrogenatoms.

9.(a) CH2O(b) 40.68%

10.

11.(a) H2 + Cu2O Cu2 + H2O

(b) Maximum mass of solid copper form = 64(2)= 128 g

C. Synthesis (Experiment)12) Describe a laboratory experiment to

determine the empirical formula ofmagnesium oxide.Your answer should include all theprecautions and calculations involved.[Relative atomic mass: Mg, 24; O,16]

Aim : To determine the empirical formula of magnesiumoxide

Material : 10 cm of magnesium ribbon and sandpaper.

Apparatus : Crucible with lid,tongs,Bunsen burner,tripodstand, pipe-clay triangle and

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balance.

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Chapter 4: Periodic Table of Elements

A. Knowledge (Definition, meaning and

facts)

Check

1) State the basic principle of arranging theelements in the Periodic Table from itsproton number.

2) State the physical properties of Group 1.

3) State the physical properties of Group 17.

4) State the changes in the atomic size andelectronegativity of elements acrossPeriod 3.

5) State three special properties of transitionelements?

1. Elements are arranged horizontally ascending order oftheir proton number,from 1 to 113,in the periodic table.2. The physical properties of Group 1 elements are theelement have dull surface and have low melting and boilingpoint.

3. The physical properties of Group 17 elements are theelement do not conduct electricity and have low densities.4. The atomic size decrease across period 3 from left toright.Therefore,the electronegativity of element increase.5. The three special properties of transition elements aretransition element can form coloured ion,can form complexions and act as catalyst.

B. Understanding / Application /Analysis

6) State the position of element X39

20in

Periodic Table. Explain your answer.

7) When across Period 3 from sodium toargon, the atomic size decreases. Explainwhy.

8) When across Period 3 from sodium toargon, the electronegativity increases.Explain why.

9) The reactivity of Group 1 increases whengoing down the group. Explain why.

10) The reactivity of Group 17 decreaseswhen going down the group. Explain why.

11) Why helium gas is not reactive?

12) X is an element from Group 1. X in burntin oxygen and the product is dissolved inwater. What is the property of the solutionformed? Explain Why.

13) Chlorine gas is dissolved in water.What can you observe if a piece of bluelitmus paper is immersed into the solution

formed? Explain why.

14) W is an element from Group 1. Predict thechemical reaction of W with:a) water,b) Oxygen,

State the observation and write thechemical equation involve.

6. Group 2,Period 4.

C. Synthesis (Experiment)

15) Describe a laboratory experiment tocompare the reactivity of elements in

Group 1: lithium, sodium and potassium.

16) Describe a laboratory experiment tocompare the reactivity of chlorine,

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bromine and iodine in the reaction withiron wool. State the observation and writethe chemical equations involve inreactions.

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Chapter 5: Chemical Bonds


meaning and facts)

Check

1) What is anion?

2) What is cation?

3) State two physical

properties of ioniccompounds.

4) State two physicalproperties of covalentcompounds.

1. Anion is negatively-charge ion.2. Cation is positively-charge ion.3. The physical properties are ionic compound are non-volatile and canconduct electricity in molten state or aqueous solution.4. The physical properties are covalent compound are volatile and do not

conduct electricity in the solid or liquid states.

B. Understanding /Application / Analysis

5) Explain why sodium chloridecan conduct electricity inaqueous state but cannotconduct electricity in solidstate.

6) Magnesium chloride andhydrogen chloride are twocompounds of chlorine. Atroom condition, magnesiumchloride exists as a solid buthydrogen chloride exists asa gas. Explain why.

7) Describe the formation ofionic bond in sodiumchloride, NaCl.

8) By using example, describethe formation of covalentbond between element fromGroup 14 and element fromGroup 17.

5. Because the aqueous state have the present of water.6.

C. Synthesis

9) Draw electron arrangementof the compound formedfrom the following elements.a) Nitrogen and hydrogen,

b) Carbon and oxygen,c) Magnesium andchlorine,

d) Carbon and hydrogen,e) Hydrogen and chlorine,f) Sodium and oxygen.

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Chapter 6: Electrochemistry

A. Knowledge (Definition, meaning

and facts)

Check

1) State the meaning of electrolyte.

2) State the meaning of electrolysis.

3) State three factors affecting

electrolysis of an aqueous solution.

1. Electrolyte are substance that can conduct electricity eitherin molten state or in aqeuous solution and undergo chemicalchanges.2. Electrolysis is the process whereby compound isdecomposed into constiuent elements when an electric current

passes through an electrolyte.3. The position of the ion in he electrochemical series.

- The types of electrodes used in the electrolysis.- The concentrationof ions in the electrolysis.

B. Understanding / Application /

Analysis

4) Explain why solution of hydrogenchloride in water can conductelectricity but solution of hydrogenchloride in methylbenzene cannotconduct electricity?

5) By using example, explain how thefollowing factors can determine theselective discharge of ions at theelectrodes.a) Types of electrodes,b) Concentration of the ions.

6) Describe the electrolysis of moltenlead(II) bromide.

7) Describe the extraction of aluminiumby electrolysis.

8) Draw the structure of Daniell cell andexplain how it can produce electricity.

9) Draw the structure of a dry cell andexplain how it can produce electricity.

C. Synthesis

10) Describe a laboratory experiment toextract lead from lead(II) oxide byusing electrolysis.

11) Describe a laboratory experiment to

show that types of electrodesaffecting the selective discharge ofions in electrolysis of copper(II)sulphate solution.

12) You are given magnesium ribbon,copper plate, magnesium nitratesolution, copper(II) sulphate solution,connecting wires with crocodile clips,250 cm3 beaker, voltmeter and porouspot.Construct a voltaic cell by using theabove materials.

Explain how the voltaic cell canproduce electricity. Your answer mustinclude observation and halfequations for reaction at anode and

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cathode.

13) Describe a laboratory experiment toconstruct the electrochemical seriesof magnesium, copper, zinc and lead.

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Chapter 7: Acids and Bases and Chapter 8: Salts


meaning and facts)

Check

1) State the meaning of acid andalkali.

2) What is the meaning of strongacid and weak alkali?

3) What is neutralisation?

4) What is salt?

5) What is precipitate reaction?

1. - An acid is a substance which dissociates in water to producehydrogen ions.

- A base is a sustance which ionises in water to produce hydroxide ions.2. Strong acid is an acid which dissociates completely to produce highconcentration of hydrogen ions,while weak alkali is a base which

ionises partially to produce low concentration of hydroxide ions.3. Neutralisation is the reaction of an acid and a base.4. Salt is a compound form when the hydrogen ion is replaced by ametal ion or ammonium ion.5. Precipitate reaction is a reaction which cause the colour of ion canchange into other colour of ion.

B. Understanding /

Application / Analysis6) The pH value of solution

ammonia in water is 9 but the

pH value of solution ofammonia in trichlomethane is7. Explain why the pH valuesof the two solutions aredifferent.

7) 80 cm3 of distilled water isadded to 20 cm3 of 2.0moldm-3 solution of HCl. Findthe molarity of the dilutesolution.

8) In a titration, 40 cm3 of 0.25

moldm-3

potassium hydroxide,KOH solution is needed toneutralise 20 cm3 of nitricacid, HNO3. Calculate themolarity of the nitric acid,HNO3.

9) Given dilute nitric acid anddilute sulphuric acid have thesame concentration of 0.5moldm-3. In a neutralisationexperiment, 20 cm3 of nitricacid is required to neutralise

20 cm3 of sodium hydroxidesolution but only 10 cm3 ofsulphuric acid is required toneutralise 20 cm3 of sodiumhydroxide solution. Explainwhy.

C. Synthesis10) Describe a chemical test to

determine a given solution isan acid solution.

11) Describe a laboratoryexperiment to determine theconcentration of sodiumhydroxide by using titrationprocess. You are given 0.2

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moldm-3 of dilute sulphuricacid, phenolphthalein,burette, pipette and conicalflask.

12) You are given solid sodiumchloride. Describe how toprepare sodium chloride

solution of 0.2 moldm

-3

inlaboratory by using 250 cm3

volumetric flask.

13) Describe the preparation ofzinc sulphate .

14) Describe the preparation oflead(II) chloride.

15) Describe the preparation ofpotassium nitrate.

16) Solid W is a salt. Describe thetests you would carry out toconfirm the presence of zincions and nitrate ions in thesalt?

17) Solid X is a metal carbonate.Describe the tests you wouldcarry out to confirm that Xconsists of carbonate ionsbesides heating..

18) You are given four test tubes

filled with solution consist ofzinc ions, lead(II) ions,aluminium ions andmagnesium ions respectively.Describe the tests you wouldcarry out to confirm the ionthat present in each test tube.

19) You are given potassiumchloride solution, lead(II)oxide powder and dilute nitricacid.Describe how you would

prepare lead(II) chloride saltfrom the given materials.

20) You are given dilute sulphuricacid, copper(II) nitratesolution and sodiumcarbonate solution. Describehow you would preparecopper(II) sulphate salt fromthe given materials.

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Chapter 9: Manufactured Substance in Industry


meaning and facts)

Check

1) What is the meaning of alloy?State the aims of makingalloys.

2) What is the meaning of

composite materials?State the components of thefollowing compositematerials:a) Reinforced concrete,b) Superconductor,c) Fibre optic,d) Fibre glass,e) Photochromic glass.

3) State the catalyst,temperature and pressure ofthe following process:

a) (a) Contact processb) (b) Haber process

4) What is the meaning ofpolymers?Name the monomer ofpolythene and polyvinylchloride.

5) State four types of glass andtheir compositions. List theuses of each glass.

6) What is ceramics? State theproperties and list the uses ofceramics.

1. - An alloy is a mixture of two or more element at fixed composition inwhich the major component is a metal.

- The aims are to increase the strength and hardnessof a puremetal,to increase the resistanceto corrosion of a pure metal and toimprove the appearance of a pure metal.

2. Composite materials are strutural material that is formed bycombining two or more different substance likemetals,alloy,ceramics,glass and polymers.(a) Concrete and steel.(b) Yitrium oxide,barium carbonate,copper(ll) oxide.(c) Glass and plastic.(d) Plastic and glass.(e) Glass,silver chloride and silver bromide.

3. (a) The catalyst used is vanadium(V) oxide at a temperature of 480C and a pressure of 1 atmosphere.

(b) The catalyst used is iron powder at temperature of 450C to 500C and at a pressure of 200 to 300 atm in the presence of molybdenum asa promoter.

4. - Polymers are long chained formed by joining up many identicalrepeating sub-units called monomers.

- Monomer of polythene is ethene,while the monomer of polyvinyl chloride ischloroethene.

5. Soda-lime glass is used in mirror and light bulbs.- Fused glass is used in lenses and telescope mirrors.- Lead crystal glass is used in tableware and crystal.- Borosilicate glass is used in cookware and glass pipelines.

6. Ceramics are made up from clay and composed of aluminium silicatemixed with sand.- Hard and strong ceramic is used in building material.- Attractive and easily moulded ceramic is used in decorative piecesand household items.- Chemically inert and non-corrosive ceramic is used in kitchenware.- Good insulator of heat ceramic is used in insulation.- Electrical insulator ceramic is used in insulating parts in electricalappliances.- Inert and non-compressible ceramic is used in medical and dentalapparatus.

B. Understanding /

Application / Analysis7) Bronze is an alloy consists of

copper and tin. Explain whybronze is harder than copper.

8) Explain how acid rain isformed.Describe how acid raincauses environmentalpollution.

9) Explain the industrial processinvolved in the manufactureof sulphuric acid.Write all the chemicalequations involve.

10) Explain the industrial processinvolved in the manufactureof ammonia gas.Write all the chemical

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equations involve.

C. Synthesis11) Describe a laboratory

experiment to prepareammonium sulphate(ammonium fertiliser)

12) Describe a laboratoryexperiment to compare thehardness of brass andcopper.

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Chapter 10: Rate of Reaction


meaning and facts)

Check

1) What is rate of reaction?

2) What is stated in the collisiontheory?

3) What is activation energy?

4) What is effective collision?

1. Rate of reaction measured the speed of reactant are converted intoproduct in a chemical reaction.2. The collision theory states that only those collisions which achieve aminimum amount of energy,called activation energy and with thecorrect orientation,will result in reaction.

3. Activation energy is a barrier that must be overcome by the collidingparticle of reactant so that the reaction can occur.4.Effective collision is the collisions which achieve a minimum amountof energy and with the correct orientation.

B. Understanding /

Application / Analysis5) Explain how surface area

(size of reactant) canincrease the rate of reactionbased on collision theory.

6) Explain how temperature canincrease the rate of reactionbased on collision theory.

7) Explain how catalyst canincrease the rate of reactionbased on collision theory.

8) Explain why hydrochloric acidof 2.0 moldm-3 is reactedfaster with zinc compare tohydrochloric acid of 0.5moldm-3 .

C. Synthesis9) Hypothesis: The smaller the

size of reactant, the higherthe rate of reaction.Describe a laboratoryexperiment to confirm thehypothesis by using thereaction between calciumcarbonate and hydrochloricacid.

10) Describe a laboratory

experiment to show that thepresence of catalyst willincrease the rate ofdecomposition of hydrogenperoxide.

11) Describe a laboratoryexperiment to show that anincrease in temperature willincrease the rate of reactionbetween sodium thiosulphatesolution and sulphuric acid.

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Chapter 11: Carbon compounds


meaning and facts)

Check

1) What is homologous series?

2) What is saturated hydrocarbonand unsaturated hydrocarbon?State an example of each of

them.

3) Explain what is isomers andisomerism by using butane asan example.

4) What is polimer? State anexample of polymer and itsmonomer.

5) What are saturated andunsaturated fats?

1. Homologous series is a group or family of organic compound thathas certain characteristics.2. - Saturated hydrocarbon is compound that has single carbon-carbonbond,while unsaturated hydrocarbon is compound that has at leastcarbon-carbon double or triple bond.

- Example for saturated hydrocarbon is propane,while example forunsaturated hydrocarbon is propene.3. - Isomers are the molecules with the same molecular formula,butdfifferent strutural formula.

- Isomerism in butane starts with four carbon atoms.4. - Polymers are long chained formed by joining up many identicalrepeating sub-units called monomers.

- The example of polymer is polythene and its monomer is ethene.5. Saturated fats are the fatty acid that has all carbon atoms joinedtogether by carbon-carbon single bond,while unsaturated fats are thecarbon chain has one or more carbon-carbon double bonds.

B. Understanding /

Application / Analysis6) Explain what is isomers and

isomerism by using butane.

7) Explain why ethene gas candecolourises the acidifiedpotassium mangante(II)solution but ethane can notdecolourises acidifiedpotassium mangante(II)solution.

8) Explain why both hexane andhexane have six carbon atomsbut hexene burns with a moresooty flame.

9) Pentane and propane aremembers from alkane family.Explain why the melting pointof pentane is higher thanpropane.

10) Propanol and propanoic acid

are dissolved in water. It isfound that propanol solution isa neutral but propanoic acid isan acid solution.

11) Explain the coagulationprocess of latex.

12) Explain how to preventcoagulation of latex.

6. - Isomers are the molecules with the same molecular formula,butdfifferent strutural formula.

- Isomerism in butane starts with four carbon atoms.7.

C. Synthesis13) Describe a test to differential

hexene and hexane.

14) Describe a laboratoryexperiment to prepare ethane

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gas from ethanol.

15) Describe a laboratoryexperiment to prepare ethanoicacid gas from ethanol.

16) Ethylpropanoat is a productfrom reaction between alcohol

and carboxylic acid.(a) State two physicalproperties of ethylpropanoat.(b) Describe a laboratoryexperiment to prepareEthylpropanoat. Your answermust include the

drawing of the setup-apparatus and the chemicalequation involve.

17) Explain how to preparepropanoic acid from propene.

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Chapter 12: Oxidation and Reduction


meaning and facts)

Check

1) What is oxidation anddeduction based on loss orgain of oxygen?

2) What is oxidation and

deduction based on transferof electrons?

3) What is oxidation anddeduction based on changesin oxidation number?

4) What are redox reactions?State an example of redoxreactions.

5) What is oxidising agent andreducing agent? State an

example of oxidising agentand reducing agent.

B. Understanding /

Application / Analysis6) Determine whether the

reaction between hydrochloricacid and sodium hydroxide isa redox reaction. Explain youranswer based on changes inoxidation number.

7) Determine whether thereaction between lead(II)nitrate and copper(II) is aredox reaction. Explain youranswer based on changes inoxidation number.

8) The reaction between zincand copper(II) sulphatesolution is a redox reaction.Explain why.

9) When bromine water is added

to the potassium iodidesolution, the solution changescolour from colourless tobrown. Explain theobservation.

10) Describe the rusting of iron.

11) A mixture of copper(II) oxideand aluminium powder isheated strongly. The mixtureburns brightly. Explain thisobservation based on

oxidation and reduction.

12) Chlorine water is added topotassium iodide solution in a

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test tube. 2 cm3 of 1,1,1-trichloroethene is added tothe test tube and the mixtureis shaken thoroughly. Thecolour of 1,1,1-trichloroethenechanges from colourless topurple. Explain theobservation.

C. Synthesis13) Describe a laboratory

experiment to change theoxidation number of iron from+2 to +3.How would you confirm thatiron(III) is formed?

14) Describe a laboratoryexperiment to change theoxidation number of iron from+3 to +2 by using zinc.

15) Describe the extraction ofiron.

16) You are given lead, zinc,copper and their oxides.Describe a laboratoryexperiment to compare thereactivity of these metalstoward oxygen.

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Chapter 12: Thermochemistry

A. Knowledge (Definition, meaning and facts) Check 1) What is exothermic reaction and endothermic reaction?

State an example for each reaction.

2) What is heat of precipitation?

3) What is heat of displacement?

4) What is heat of neutralisation?

5) What is heat of combustion?

B. Understanding / Application / Analysis6) Explain how exothermic reaction and endothermic are formed based on energy change during

formation and breaking of chemical bonds.

7) Explain why the heat of combustion of butanol is higher than ethanol.

8) Explain why the heat of neutralisation between strong acids and strong alkalis is a constant,that is -57kJmol-1?

9) Explain why the heat of neutralisation between ethanoic acid and sodium hydroxide is lessthan-57kJmol-1?

10) 50 cm3 of 2 moldm-3 sodium hydroxide solution is added to 50 cm3 of 2 moldm-3 hydrochloricacid. The temperature increases t oC.a) If 100 cm3 of 2 moldm-3 sodium hydroxide solution is added to 100 cm3 of 2 moldm-3

hydrochloric acid, predict the increase in temperature.

b) If 50 cm3 of 1 moldm-3 sodium hydroxide solution is added to 50 cm3 of 1 moldm-3


c) If 50 cm3 of 4 moldm-3 sodium hydroxide solution is added to 50 cm3 of 4 moldm-3


C. Synthesis11) Describe a laboratory experiment to determine the heat of displacement of copper by zinc.

12) Describe a laboratory experiment to determine the heat of neutralisation between strong acidsand strong alkalis.

13) Describe a laboratory experiment to determine the heat of combustion of methanol.

14) The higher the number of carbon atoms per molecule, the higher is the heat of combustion

Describe a laboratory experiment to prove that the above statement is true by using methanol,ethanol, propan-1-ol, butan-1-ol and pentan-1-ol.

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Chapter 13: Chemicals for Consumers

A. Knowledge (Definition, meaning and facts) Check 1) What is soap?

2) What is saponification process?

3) What is detergent?

4) State the functions of each of the following additives in detergent.a) Whitening agent(example: sodium perborate)b) Optical whitener(fluorescent dyes)c) Biological enzyme (Example: amylases, lipases, proteases and cellulases)d) Fragrance

5) What is hard water?

6) State the function of each of the following food additives:a) Preservatives ( Sodium nitrite, sodium benzoate)b) Antioxidants (Ascorbic acid)c) Flavourings (Monosodium glutamate (MSG), Aspartame)d) Stabilisers

e) Thickeners

7) State the functions of the following modern medicines.a) Analgesics ( Aspirin, Paracetamol, Codeine)b) Antibiotics ( Penicilin, Streptomycin)c) Psychotherapeutic medicine ( Stimulant, Antidepressant, Antipsychotic)

8) State the side effects of paracetamol and aspirin.

B. Understanding / Application / Analysis9) Describe the cleansing action of soap.

10) Explain why the cleansing action of a detergent is more effective than a soap in hard water.

C. Synthesis11) Describe a laboratory experiment to prepare soap from palm oil using the saponification

process.

12) Describe a laboratory experiment to investigate the cleansing action of a soap and a detergentin hard water.

2011 Module Score A

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Transcript of 2011 Module Score A