Checklist For Scoring Grade A In Chemistry Spm 2009

Chapter 2: The Structure ofthe Atom

II A.Knowledge (DefillitiOi1,-;'':;~~-T-'I-'i'-'£-'-a-il-d-4',-.a-c-t-s \-,--------------------C-,h-e-c-k-~ , ~,~, I

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I 1)

State the kinetic theory of matter, State one example to support the kinetic theory of matter

I 2)

What are

f 3)

What is melting point?

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Define proton number and nucleon number,

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State the meaning of isotopes,

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ate::!,

rrJolecule and ion?

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State the uses of isotopes such as carbon-14

and cobalt-60.

r'B--:-Understandin~ ; Application /Ana!y~.i~

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Explain why the temperature

remains uncha-ng-e-o~' -d-u-ri-ng-th-e-m-e-it-ir-,g-p-ro-c-e-s-s~. ------------.,

'8)

Explain why the temperature

remains unchanged

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, 10)

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diJi'ing the freezing process.

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A solid compound is heated until it converts into gas. Explain the changes forces of attraction between the particles, and arrangement of particles"

in energy content,

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State the main subatomic particles of an atom. Compare and contrast the relative atomic mass and the relative charge of the subatomic particles of the atom.

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11) ~; Al is the symbol of aluminium. (a) Determine the number of neutron of aluminium. (b) Draw the electron arrangement of aluminium.

C. Synthesis (Ex eriment) 12) Solid Z has a melting point o'f65°C. Describe a laboratory experiment to determine point of Z. Your answer should show how the melting point of Z is determined. 13) Compound \/V has a freezing point of 82°C. Describe a iaboratory freezing point of W.

experiment

the melting

to determine

the

· Chapter 3: Chemical Formulae and E~tions /A. Knowledge (j)efinition, meaning and facts)

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1) . State

the meaningof'relatlveatomlC

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-mass based -on carbon-12 scale.

2 ) sDteftinetha mole_ . f I a e e meaning 0 mo ar mass

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State the meaning of molar volume of gas_

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State the meaning of empirical formula

16)

State the meaning of molecular formula.

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Explain why we couldn't determine the empirical formula of copper(lI) oxide by heating copper powder in a crucible.

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Compare and contrast empirical formula with molecular formula using ethane as an example.

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IB.-cUnderstanding

/ Analysis

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/ Application

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Vinegar is a dilute ethanoic acid with a molecular formula of CH3COOH (a) Find the empirical formula of ethanoic acid. (b) Find the percentage composition by mass of carbon in ethanoic acid

10) 3.6 g of carbon reacted with 0.8 g of hydrogen to form a compound. (a) Determine the empirical formula of the compound formed. (b) Given that the relative molecular mass of the compound is 88 g, find its molecular formula. [Relative atomic mass: C ,12; H, 1] 11) Hydrogen Gas is reacted 'vvith20 g of hot copper(ll) oxide powders to produce solid copper and'vvater. (a) Write the chemical equation for the reaction. (b) Calculate the maximum mass of solid copper formed. [Relative atomic mass: Cu, 64; 0,16; H,1]

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sJ:~t~~~sa \;~~:~~~::~eriment to determine the empirical formula of magnesium oxide. Your answer should include all the precautions and calculations involved. [Relative atomic mass: Mg, 24; 0,16]

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Chapter 4: Periodic Table of Elements !

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State the basic principle of arranging the elements

Check in the Periodic Table from its proton

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number

I 2)

5)

State the physical properties

of Group 1.

State three special properties of transition elements?

B. Understanding! Application I Analysis /6) State the position of element ;~ X in Periodic

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8)

Table. Explain your answer.

When across Period 3 from sodIum to argon, the atomic size decreases When across Period 3 from sodium to argon, the eiectronegativity

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The reactivity of Group 1 increases

110)

The reactivity of Group 17 decreases

_111)

Explain why.

increases

Explain why

when going dovv'n the group. Explain why. when going down the group. Explain why.

Why helium gas is not reactive?

112) X is an element from Group

1. X in burnt in oxygen and the product is dissolved What is the properiy of the solution formed? Explain Why.

13) Chlorine gas is dissolved in water. What can you observe if a piece of blue litmus paper is immersed

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in water.

into the solut!on formed?

Explain why. I14) \/V is an element from Group 1. Predict the chemica! reaction of W with: a) water,

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b)

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observation

and wnte the chemical equation

~C. Synthesis (Experlment,---

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15) Describe a laboratory

experiment

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Involve

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to compare the reactivity of elements

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in Group 1. i1thium,

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sodium and potassium

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16) Describe a laboratory experiment to compare the reactivity of chlorine, bromine and iodine in the reaction with iron wool. State the observation and write the chemica! equations involve in

reactions.

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Chapter 5: Chemical Bonds

: A. Knowled e (Definition, mean!n and facts) 1) What is anion?

I Appli~C!.tionI Anal sis 5) Explain why sodium chloride ¢:f1 conduct electricity in aqueous state but cannot conduct electricity in solid state. ""

B. Understandin

6)

Magnesium chloride and hydrogen chloride are two compounds of chlorine. ,~.troom condition rnagnesiunl chloride exists as a solid but hydrogen chloride exists as a gas. Exp!ain t

8) By using example, describe the formation of covalent bond between element from Group 14 and element from Group 17. C. Synthesis

,9)

Draw electron arrangement of the compound formed from the following elements.

I ~! ~itr?gen an,dhydrogen, I oJ lvarDon ana oxygen, I c) Magnesium and chlorine, 'd) Carbon and hydrogen, II ~) iYdrOgen and chlorine, ~odium

and oxygen.

(:hapter 6: Electrochemistry !

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I A. ftno,\:v_h~a~ ipelliiit~~n~meaning and facts)

11)

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$tate the meaning of electrolyte.

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State the meaning of electrolysis. State three :.;:;~tors affecting

4)

Explain why solution of hydrogen chlonde In water can conduct electricity hydrogen chloride in methyl benzene cannot conduct electricity?

lB. Understanding

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electrolysis

cf

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an aqueous solution

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Application! Analysis ---------------------J---------J but solutIon of

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By using example, explain how the following factors can determine ions at the electrodes.

the selective discharge

of

a) Types of eiectrodes,

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b)

Concentration

of the ions.

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Describe the extraction

18)

Draw the structure

of aluminium

by electrolysis.

of Daniell ceil and explain how it can piOduce electricity.

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19)

Draw the structure of a dry cell and explain how it ca~~oduce

e!_e_c_t_ri_ci_ty_.

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! C. Synthesis ,~----_.~_ _------------_._----10) Describe a laboratory experiment to extract lead from lead(ll) oxide by using electrolysis. ..

11) Describe a laboratory experiment to show that types of electrodes discharge of ions in electrolysis of copper(il) sulphate solution

affecting the selective

12) You are given magnesium ribbon, copper plate, magnesium nitrate solution, copper(lI) sulphate solution, connecting wires with crocodile clips, 250 cm3 beaker, voltmeter and porous pot. Construct a.voltaic cel! by using the above materiais. Explain how the voltaiC cell can produce eiectricity. Your answer must inciude observation half equations for reaction at anode and cathode 13) Describe a laboratory

copper, zinc and lead.

experiment

to construct the electrochemical

series of magnesium,

and

Cha ter 7: Acids and Bases and Cha ter 8: Salts A. Knm'l1Jedge (Definition, meaning and facts) 1)

State the meaning of acid and alkali,

5)

What is precipitate

reaction?

I B. Understandin / An lication / Anal sis I 6) The pH value of solution ammonia in water is 9 but the pH value I

trichlomethane

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7)

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of solution of ammonia is 7. Explain why the pH values of the two solutions are different.

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80 cm3 of distiHed water is added to 20 crn3 of 2.0 fll01drn-3 so'ution of HeL Find the molarity of the dilute solution.

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In a titration, 40 cm3 of 0.25 moldm-3 potassium hydrOXide, KOH solution is needed to neutra!ise 20 cm3 of nitric acid, HN03. Calculate the molarity of the nitric acid, HN03 Given dilute nitric acid and dilute sulphuric acid have the same concentration of 0.5 moldm'3 In 3 a neutralisation experiment, 20 cm of nitric acid is required to neutralise 20 cm3 of sodium 3 hydroxide solution but only 10 cm of sulphuric acid is required to neutralise 20 cm 3 of sodium hydroxide solution. Explain why

Ie. Synthesis 110) Describe a chemical test to determine

a given

solution is an acid solution.

11) Describe a laboratory experiment to determine the concentration of sodium hydroxide by using titration process. You are given 0.2 moldm-3 of dilute sulphuric acid, phenolphthalein, burette, pipette and conical flask i 2) You are given soiid sodium chloride. Describe how to prepare sodium chloride solution of 0.2 moldm-3 in laboratory by using 250 cmJ volumetric flask.

16) Solid \N is a salt. Describe the tests you would carry out to confirmthe and nitiate ions in the salt?

presence

of zinc ions

17) Solid X is a metal carbonate. Describe the tests you would carry out to confirm that X consists of carbonate ions besides heating. "18) You are given four test tubes fined with soiution cons!st of zinc ions; lead(ii) ions} alurninium ions and magnesium ions respectiv€iy. Desc:rib~ the tests you \j\{o~Jd carry out to confirm the iun ti-~atpresent in each test tube. 19) You are given potassium chior!de sOlutIon ..lead(ll) oxide pO\AJder and dilute nitric acid. Describe ho~v you \/Vould prepare !ead(li) chioride sait Tiom the given rnaterials, 20) You are given dilute suiphuric acid, copper(ll) nitrate solution and sodium carbonate Describe how you would prepare copper(li) sulphate sait from the given materials.

solution.

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Chapter 9: Manufactured

Substance in Industry

i A. K~owiedge (Defini.tioll, meaning and facts) 1) What is the meaning of alloy? State the aims of making alloys. 2) What is the meaning of composite materials? State the components of the following composite materials: a) Reinforced concrete, b) Superconductor, c) Fibre optic, d) Fibre glass, e) P~otochromic glass. 3) State the catalyst, temperature and pressure of the following process: a) (a) Contact process b) (b) Haber process 4) Ifllhat is the meaning of polymers? Name the monomer of po!ythene and poiyviny! c.hloride

. B. Understanding

/ Application / Analysis

I 7)

Bronze is an alloy consists of copper and tin. Explain why bronze is harder than copper

I 8)

Explain how acid rain is formed. Describe how acid rain causes environmental pollution.

9)

Explain the industrial process involved in the manufacture of sulphuric acid. Write all the chemical equations involve.

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I 10) Explain the industrial process involved in the manufacture of ammonia gas. VVritea!! the chemical equations involve.

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I c. Svnthesis 11) Describe a laboratory experiment to prepare ammonium sulphate (ammonium fertiliser)

Cha ter 10: Rate of Reaction ¥.now!edge (Definition, meaning and facts)

I A. 1)

What is rate of reaction?

2)

What is stated in the collision theory?

B. Understandin

/A

Iication / Anal sis

Explain how surface area (size of reactant) theory. .

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can increase the rate of reaction based on collision

Ex!), lain how temo, erature can increase the rate of reaction based on coilision tileory.

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Explain how catalyst can increase the rate of reaction based on co!!ision theory

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Explain why hydrochloric acid of 2,0 moidm-3 is reacted faster with zinc compare to 3 hydrochloric acid of 0.5 moidrn-

I c. Synthesis 9)

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Hypothesis: The smaller the size of reactant, the higher the rate of reaction. Describe a laboratory experiment to confirm the hypothesis by using the reaction calcium carbonate and hydrochloric acid.

between

1\10) Describe

a laboratory experiment to show that the presence of catalyst will increase the rate of decomposition of hydrogen peroxide,

11) Describe a labor dlur'y o>~p"'fim~nt to, o;how that, <:>ninr-rp~se in temperature of reactlon between sodium thlosulphate solution and sulphurtc aoid.

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will increase the rate _

Ch~ ter 13: Chemicals for Consumers A. Knowled e 'Definition, meanin and facts) I 1)

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What is soap? .

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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 What is hard water? State the function of 6ach oUne following food additives: a) PreS8fvatives ( Sodium nitrite, sodium benzoate) b', f\ntioxidants (Ascorbic acid) c) Flavourings (rv1onosodiurn glutamate (rvlSG), Aspartame) 0)

Staf)!Hsef5

~;at~~~~g;~~~~~~s~~r~~~ ~~~~;~~~;'~~,d~~~~~~;;Cines. b)

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Antibiotics ( Peniciiin, Streptomycin) Psychotherap€utic medicine ( Stimuiant,

State the side effects of paracetamol o

Understandin

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A

Describe the cleansing

lication

10) Explain why the cleansing

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is more effective than a soap in hard water.

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~Ana)y,_,s_is_-_

action of a detergent

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111) Describe a iaboratory experiment I process.

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,"'.ntipsychotic)

and aspirin.

action of soap.

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Antidepressant,

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to prepare soap from palm oil using the saponification

+ +_

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Cha ter 11: Carbon com ounds A. Knowledge (Definition, meaning and facts)

11)

What is homologous

series?

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What is saturated them.

hydrocarbon

and unsaturated

hydrocarbon?

State an example of each of

B. Understanding I Application / Analysis 6)

Explain what is isomers and isomerism

by using butane.

7)

Explain \A/hy ethene gas can decolourises the acidified potassiurn iTlangante(ll) ethane can not decolourises acidified potassium mangante(ll) solution

solution but

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8)

Explain why both hexane and hexane have six carbon atoms but hexene burns with a more sooty flame.

9)

Pentane and propane are members from alkane family. pentane is higher than propane.

10) Propanol and propanoic acid are dissolved in water neutral but propanoic acid is an acid solution.

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Explain why the melting point of

It is found that propanol solution is a •

C. Synthesis 13) Describe a test to differential

hexene and hexane.

16) Ethy!propanoat is a product from reaction between alcohol and carboxylic acid. (a) State two physical properties of ethylpropanoat. (b) Describe a laboratory experiment to prepare Ethylpropanoat. Your answer must include the drawing of the setup-apparatus and the chemical equation involve. I

17) Exp!ain how to pr~rl;:)re propanoic

L.

aCid from propene.

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Chapter 12: Oxidation and Reduction A. Knowled e (Definition, meanin- and facts) 1)

What is oxidation

and deduction

5)

What is oxidising

agent and reducing agent? State an example of oxidising

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based on loss or gain of oxygen?

agent and reducing

agent.

i B. Understandin II

.

I A plication / Analysis

6)

Determine whether the reaction between hydrochloric

acid and sodium hydroxide

7'1

'Deaction. EX~!ai!"'h'YOLh,r answer baseh~ on c~a!"'d·g(el's) mto:idati:n

numbe(lrl') .

etermlne vmet er t .6 reaction belV'Jeen lea I nJ rale an" copper Explain your answer based on changes in oxidation number.

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is a redox

d

t'

IS a re ox reac Ion.

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9)

When bromine water is added to the potassium iodide solution, the solution changes from colourless to brown. Explain the observation

colour

1 i) A mixture of copper(I!) oxide and aluminium powder is heated strongly. The mixture burns brightly. Explain this observation based on oxidation and reduction. 12) Chlorine water is added to potassium

iodide solution in a test tube. 2 cm3 of i,1,1-

triCh~roethene_i_s_a_d_d_e_d_t_o_t_h_e_t_e_~_t_u_b_e_a_n_d_t_h_e_m~ix_tu_r_e_i_s_s_h_a_k_e_n_th_o_r_0_U_9_h_~_._T_h 1,1, l-trichloroethene changes from colourless to purple. Explain the observation. -

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I C. Synthesis 113) Describe a lci-b-o-ra-t-o-ry--e-Y-.p-e--r-im-e-nt-t-o-c-h-a-n-g-e-t-h-e-o-x-id-a-t-io-n-n--u-m-b-e-r-o-f ir-o-n-fr-o-m-+-2 to +3.

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How would you confirm that iron(II!) is formed? 14) Describe a laboratory

experiment

to change the oxidation

1,----1

, 1

number of iron from +3 to +2 by

us;ng z;nc.

1,5)

Desef;be the extract;on

\16) 1

You are given lead, zinc, copper and their oxides. Describe a iabof3tory compare the reactivity of these metals toward oxygen.

of ;ron experiment

to

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Chapter 12: Thermochemistry (Definition, meaning and facts)

I A. Knowledge 11)

What is exothermic reaction and endoih-e-r-m-i-c~re-a-c-t-io-r-,?---------------

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'3)

What is heat of displacement?

15)

\Nhat is heat of combustion?

B. Understandin I

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6)

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Hcatioii / Analysis

Explain how exothermic reaction and endothermic are formed based on energy change during formation and breaking of chemical bonds.

17)

Explain why the heat of combustion of butanol is higher than ethanol

18)

Explain why the heat of neutra!isation between strong acids and strong alkalis is a constant, that is -57kJmor1?

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Explain why the heat of neutralisation between ethanoic acid and sodium hydroxide is less than -57kJmor1? 3

10) 50 cm3 of 2 moldm-3 sodium hydroxide solution is added to 50 cm of 2 moldm-3 hydrochloric acid. The temperature increases tOe. a) If 100 em of 2 moldm-3 sodium hydrOXidesolution is added to 100 cm3 of 2 moidm-3 hydrochloric acid, predict the increase in temperature. 3

3

b)

If 50 cm3 of 1 moldm-3 sodium hydroxide solution is added to 50 cm of 1 moldm hydrochloric acid, predict the increase in temperature.

c)

If 50 cm3 of 4 moldm-3 sodium hydroxide solution is added to 50 cm3 of 4 moldm-3 hydrochloric acid, predict the inCiease in temperature.

C. Synthesis 11) Describe a laboratory experiment to determine the heat of displacement of copper by zinc. 12) Describe a laboratory experiment to determine the heat of neutra!isation between strong acids and strong alkalis.

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14) "The higher the nurl1ber of carbon atoms per molecule: the higher is the heat of cornbustion Describe a laboratory experiment to prove that the above statement is true by using methanol, ethanol, propan-1-ol, butan-1-o1 and pentan-1-ol. ll

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