Chemistry SL paper 1 TZ1 2009 - Examibrelics.weebly.com/.../chemistry_sl_paper_1_.pdf · 2209-6110 – 3 – Turn over M09/4/CHEMI/SPM/ENG/TZ1/XX+ 1. The molar mass of a compound

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M09/4/CHEMI/SPM/ENG/TZ1/XX+

1. Themolarmassofacompound isapproximately56gmol–1. Which formula ispossible for thiscompound?

A. NaNO3

B. AgOH

C. MgO

D. KOH

2. Whichcompoundhastheempiricalformulawiththelargestmass?

A. C2H6

B. C2H4

C. C2H2

D. C3H6

3. What is the coefficient forO2(g)when the equation for the combustion of 1mole of pentane isbalanced?

C H (g) _O (g) _CO (g) _H O(g)5 12 2 2 2

A. 5

B. 6

C. 8

D. 16

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4. What is themaximummass, ing,ofmagnesiumoxide thatcanbeobtained from the reactionofoxygenwith2.4gofmagnesium?

A. 2.4

B. 3.0

C. 4.0

D. 5.6

5. 5dm3ofcarbonmonoxide,CO(g),and2dm3ofoxygen,O2(g),atthesametemperatureandpressurearemixedtogether.Assumingcompletereactionaccordingtotheequationgiven,whatisthemaximumvolumeofcarbondioxide,CO2(g),indm

3,thatcanbeformed?

2 2CO g O g CO g2 2( ) ( ) ( )

A. 3

B. 4

C. 5

D. 7

6. Whichstatementaboutsolutionsiscorrect?

A. WhenvitaminDdissolvesinfat,vitaminDisthesolventandfatisthesolute.

B. InasolutionofNaClinwater,NaClisthesoluteandwateristhesolvent.

C. Anaqueoussolutionconsistsofwaterdissolvedinasolute.

D. Theconcentrationofasolutionistheamountofsolventdissolvedin1dm3ofsolution.

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7. Howmanyprotons,neutronsandelectronsarepresentineachatomof31P?

Protons Neutrons Electrons

A. 16 15 16

B. 15 16 15

C. 15 31 15

D. 16 31 16

8. Whichiscorrectforthefollowingregionsoftheelectromagneticspectrum?

Ultraviolet (UV) Infrared (IR)

A. highenergy shortwavelength lowenergy lowfrequency

B. highenergy lowfrequency lowenergy longwavelength

C. highfrequency shortwavelength highenergy longwavelength

D. highfrequency longwavelength lowfrequency lowenergy

9. Anelementisingroup4andperiod3oftheperiodictable.Howmanyelectronsareinthehighestoccupiedenergylevelofanatomofthiselement?

A. 3

B. 4

C. 12

D. 14

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10. Whichisthebestdefinitionofelectronegativity?

A. Electronegativityistheenergyrequiredforagaseousatomtogainanelectron.

B. Electronegativityistheattractionofanatomforabondingpairofelectrons.

C. Electronegativityistheattractionbetweenthenucleusandthevalenceelectronsofanatom.

D. Electronegativityistheabilityofanatomtoattractelectronsfromanotheratom.

11. Whatarethecorrectformulasofthefollowingions?

Ammonium Hydrogencarbonate Phosphate

A. NH4 HCO32 PO4

B. NH3 HCO3 PO43

C. NH4 HCO32 PO4

2

D. NH4 HCO3 PO43

12. Whathappenswhenmagnesiummetalreactswithchlorinegas?

A. Eachmagnesiumatomlosestwoelectronsandeachchlorineatomgainstwoelectrons.

B. Eachmagnesiumatomgainsoneelectronandeachchlorineatomlosesoneelectron.

C. Eachmagnesiumatomlosestwoelectronsandeachchlorineatomgainsoneelectron.

D. Eachmagnesiumatomgainsoneelectronandeachchlorineatomlosestwoelectrons.

13. Whichisthebestdescriptionofionicbonding?

A. Theelectrostaticattractionbetweenpositivelychargednucleiandanelectronpair

B. Theelectrostaticattractionbetweenpositiveionsanddelocalizednegativeions

C. Theelectrostaticattractionbetweenpositiveionsanddelocalizedelectrons

D. Theelectrostaticattractionbetweenoppositelychargedions

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14. Whichisthebestdescriptionofthebondingpresentinsilicondioxide,SiO2?

A. Eachsiliconatomformsfoursinglecovalentbondstooxygenatoms.

B. Eachsiliconatomformstwodoublecovalentbondstooxygenatoms.

C. Eachsiliconatomformstwosinglecovalentbondstooxygenatoms.

D. Eachsiliconatomformsfourdoublecovalentbondstooxygenatoms.

15. When some solid barium hydroxide and solid ammonium thiosulfate were reacted together,the temperatureof thesurroundingswasobserved todecrease from15ºC to–4ºC. Whatcanbededucedfromthisobservation?

A. ThereactionisexothermicandëH isnegative.

B. ThereactionisexothermicandëH ispositive.

C. ThereactionisendothermicandëH isnegative.

D. ThereactionisendothermicandëH ispositive.

16. WhichprocessrepresentstheC–Clbondenthalpyintetrachloromethane?

A. CCl g C g Cl g4 4( ) ( ) ( )+

B. CCl g CCl g Cl g4 3( ) ( ) ( )+

C. CCl l C g Cl g4 4( ) ( ) ( )+

D. CCl l C s Cl g4 22( ) ( ) ( )+

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17. Somewaterisheatedusingtheheatproducedbythecombustionofmagnesiummetal.Whichvaluesareneededtocalculatetheenthalpychangeofreaction?

I. Themassofmagnesium

II. Themassofthewater

III. Thechangeintemperatureofthewater

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

18. Whatisthebestdefinitionofrate of reaction?

A. Thetimeittakestouseupallthereactants

B. Therateatwhichallthereactantsareusedup

C. Thetimeittakesforoneofthereactantstobeusedup

D. Theincreaseinconcentrationofaproductperunittime

19. Whichfactorscanaffectreactionrate?

I. Thestateofthereactants

II. Thefrequencyofthecollisionsbetweenparticles

III. Theaveragekineticenergyoftheparticles

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

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20. Equalmassesofpowderedcalciumcarbonatewereaddedtoseparatesolutionsofhydrochloricacid.Thecalciumcarbonatewas inexcess. Thevolumeofcarbondioxideproducedwasmeasuredatregularintervals.Whichcurvesbestrepresenttheevolutionofcarbondioxideagainsttimefortheacidsolutionsshowninthetablebelow.

Volumeof CO2(g)/cm

3 I

II

III

IV

Time/s

25 cm3 of 2 mol dm–3 HCl 50 cm3 of 1 mol dm–3 HCl 25 cm3 of 1 mol dm–3 HCl

A. I III IV

B. I IV III

C. I II III

D. II I III

21. Considerthefollowingequilibriumreaction.

2SO (g) O (g) 2SO (g) = 197kJ2 2 3U ë ÖH

Which change in conditions will increase the amount of SO3 present when equilibrium isre-established?

A. DecreasingtheconcentrationofSO2

B. Increasingthevolume

C. Decreasingthetemperature

D. Addingacatalyst

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22. For equal volumes of 1.0moldm–3 solutions of hydrochloric acid,HCl(aq), andmethanoic acid,HCOOH(aq),whichstatementsarecorrect?

I. HCldissociatesmorethanHCOOH

II. HClisabetterelectricalconductorthanHCOOH

III. HClwillneutralizemoreNaOHthanHCOOH

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

23. When equal volumes of four 0.1moldm–3 solutions are arranged in order of increasing pH(lowestpHfirst),whatisthecorrectorder?

A. CH3COOH<HNO3<CH3CH2NH2<KOH

B. HNO3<CH3COOH<CH3CH2NH2<KOH

C. CH3CH2NH2<HNO3<CH3COOH<KOH

D. KOH<CH3CH2NH2<CH3COOH<HNO3

24. Whathappensatthenegativeelectrodeinavoltaiccellandinanelectrolyticcell?

Voltaic cell Electrolytic cell

A. oxidation reduction

B. reduction oxidation

C. oxidation oxidation

D. reduction reduction

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25. Considerhowcurrentisconductedinanelectrolyticcell.Whichstatementiscorrect?

A. Electronsmovethroughtheelectrolyteandtheexternalcircuit.

B. Ionsmovethroughtheelectrolyteandtheexternalcircuit.

C. Electronsmovethroughtheexternalcircuitandionsmovethroughtheelectrolyte.

D. Electronsmovethroughtheelectrolyteandionsmovethroughtheexternalcircuit.

26. Whichthreecompoundscanbeconsideredtobeahomologousseries?

A. CH3OH,CH3CH2OH,CH3CH2CH2OH

B. CH3CH2OH,CH3CHO,CH3COOH

C. CH3CH2CH(OH)CH3,CH3CH2CH2CH2OH,(CH3)3COH

D. CH3CH2CH2CH2OH,CH3CH2OCH2CH3,(CH3)2CH2CHO

27. WhatistheIUPACnameforCH3CH2CH(CH3)CH3?

A. 1,1-dimethylpropane

B. 2-ethylpropane

C. 2-methylbutane

D. 3-methylbutane

28. Whenbrominewaterisshakenwithaliquidorganiccompound,itisrapidlydecolourized.Whatcanbedeterminedfromthistest?

A. Thecompoundisanalcohol.

B. Thecompoundisanalkane.

C. Thecompoundisanalkene.

D. Thecompoundisaniodoalkane.

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29. Whichconditionsarerequiredtoobtainagoodyieldofacarboxylicacidwhenethanolisoxidizedusingpotassiumdichromate(VI),K2Cr2O7(aq)?

I. Addsulfuricacid

II. Heatthereactionmixtureunderreflux

III. Distiltheproductastheoxidizingagentisadded

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

30. Astudentrecordedthevolumeofagasas0.01450dm3.Howmanysignificantfiguresarethereinthisvalue?

A. 3

B. 4

C. 5

D. 6

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1. Whichamountofthefollowingcompoundscontainstheleastnumberofions?

A. 2molofNaOH

B. 1molofNH4Cl

C. 2molofCaCl2

D. 1molofAl2O3

2. Whatistheapproximatemolarmass,ingmol–1,ofMgSO H O4 2i7 ?

A. 120

B. 130

C. 138

D. 246

3. Whichisbothanempiricalandamolecularformula?

A. C5H12

B. C5H10

C. C4H8

D. C4H10

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4. 12moleculesofhydrogengas,H2(g),and5moleculesofoxygengas,O2(g),weremixedtogetherunderconditionswhichallowedthereactiontogotocompletion,accordingtothefollowingequation.

2H (g) O (g) 2H O(g)2 2 2

Thefollowingdiagramrepresentsthemixtureofreactants.

Key:

Oxygenatom

Hydrogenatom

Whichdiagramrepresentsthereactionmixturewhenthereactionwascomplete?

A.

B.

C.

D.

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5. Whichofthefollowingisanisotopeof 1224Mg ?

A. 1224Mg2+

B. 1226Mg

C. 1342Mg

D. 1326Mg

6. Whichdescribesthevisibleemissionspectrumofhydrogen?

A. Aseriesoflinesconvergingatlongerwavelength

B. Aseriesofregularlyspacedlines

C. Aseriesoflinesconvergingatlowerenergy

D. Aseriesoflinesconvergingathigherfrequency

7. Whichstatementsabouttheperiodictablearecorrect?

I. Elementsinperiod3havesimilarchemicalproperties.

II. Elementsingroup7showagradualchangeinphysicalproperties.

III. Thepositionofanelementinperiod3isrelatedtothenumberofelectronsinthehighestoccupiedenergylevel.

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

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8. Whichstatementsaboutperiod3arecorrect?

I. Theelectronegativityoftheelementsincreasesacrossperiod3.

II. Theatomicradiioftheelementsdecreasesacrossperiod3.

III. Theoxidesoftheelementschangefromacidictobasicacrossperiod3.

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

9. Whichisthebestdescriptionofthebondingpresentintheammoniumion,NH4+?

A. Sharingofelectronsbetweenatoms

B. Electrostaticattractionbetweenions

C. Electrostaticattractionbetweenpositiveionsanddelocalizedelectrons

D. Sharingofelectronsbetweenatomsandelectrostaticattractionbetweenions

10. Theformulaofcerium(III)sulfateisCe2(SO4)3.Whatisthecorrectformulaofcerium(III)phosphate?

A. CeP

B. Ce2(PO4)3

C. Ce3(PO4)2

D. CePO4

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11. Whichmoleculehastheshortestcarbon-oxygenbondlength?

A. CH3COOH

B. CH3CH2OH

C. CO2

D. CO

12. Whichpairofcompoundsisarrangedincorrectorderofrelativeboilingpoints?

Lower Boiling Point Higher Boiling Point

A. H2S H2O

B. NH3 PH3

C. HF HCl

D. CH3COOH CH3CH2OH

13. Whichstatementaboutthebondingbetweencarbonatomsiscorrect?

A. InC60fullereneeachcarbonatomiscovalentlybondedtothreeothercarbonatoms.

B. InC60fullereneeachcarbonatomiscovalentlybondedtofourothercarbonatoms.

C. Ingraphiteeachcarbonatomiscovalentlybondedtofourothercarbonatoms.

D. Ingraphiteeachcarbonatomformsadoublecovalentbondwiththreeothercarbonatoms.

14. Whichintermolecularforcesexistbetweenmoleculesofcarbonmonoxide,CO?

A. HydrogenbondsandvanderWaals’forces

B. Dipole-dipoleattractionsandvanderWaals’forces

C. VanderWaals’forcesonly

D. Dipole-dipoleattractionsonly

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15. Whichtypesofreactionarealwaysexothermic?

I. Neutralization

II. Decomposition

III. Combustion

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

16. Apurealuminiumblockwithamassof10gisheatedsothatitstemperatureincreasesfrom20 C to50 C .Thespecificheatcapacityofaluminiumis8.99 10 J g K1 1 1 .WhichexpressiongivestheheatenergychangeinkJ?

A. 10 8.99 10 3031

B. 10 8.99 10 301

C. 10 8.99 10 3031

1000

D. 10 8.99 10 301

1000

17. Underwhichconditionswillthereactionbetween1.0gcalciumcarbonateandexcesshydrochloricacidbethefastest?Assumethatallreactionsarecarriedoutatthesametemperature.

A. Onelargepieceofcalciumcarbonateand2moldm–3hydrochloricacid

B. Onelargepieceofcalciumcarbonateand1moldm–3hydrochloricacid

C. Powderedcalciumcarbonateand2moldm–3hydrochloricacid

D. Powderedcalciumcarbonateand1moldm–3hydrochloricacid

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18. Powdered manganese(IV) oxide, MnO2(s), increases the rate of the decomposition reaction ofhydrogenperoxide,H2O2(aq).WhichstatementsaboutMnO2arecorrect?

I. TherateisindependentoftheparticlesizeofMnO2.

II. MnO2 provides an alternative reaction pathway for the decomposition with a loweractivationenergy.

III. AlltheMnO2ispresentafterthedecompositionofthehydrogenperoxideiscomplete.

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

19. Whichstatementiscorrectforacrystalofiron(II)sulfateinastateofequilibriumwithasaturatedsolutionofiron(II)sulfate?

stopper

flask

iron(II)sulfatesolutioniron(II)sulfatecrystal

A. Thecolourofthesolutiondarkensasthecrystalcontinuestodissolve.

B. Theconcentrationoftheiron(II)sulfatesolutionincreasesasthewaterevaporates.

C. Theshapeoftheiron(II)sulfatecrystaldoesnotchange.

D. Thecolourofthesolutiondoesnotchangebuttheshapeofthecrystalmaychange.

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20. TheHaberprocessusesan ironcatalyst toconverthydrogengas,H2(g),andnitrogengas,N2(g),toammoniagas,NH3(g).

3H (g) N (g) 2NH (g)2 2 3

Whichstatementsarecorrectforthisequilibriumsystem?

I. Theironcatalystincreasestheratesoftheforwardandreversereactionsequally.

II. Theironcatalystdoesnotaffectthevalueoftheequilibriumconstant,Kc.

III. Theironcatalystincreasestheyieldofammoniagas,NH3(g).

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

21. Whichpropertyischaracteristicofacidsinaqueoussolution?

A. Acidsreactwithammoniasolutiontoproducehydrogengasandasalt.

B. Acidsreactwithmetaloxidestoproduceoxygengas,asaltandwater.

C. Acidsreactwithreactivemetalstoproducehydrogengasandasalt.

D. Acidsreactwithmetalcarbonatestoproducehydrogengas,asaltandwater.

22. A student has equal volumes of 1.0moldm–3 sodium hydroxide and ammonia solutions.Whichstatementaboutthesolutionsiscorrect?

A. Sodiumhydroxidehasalowerelectricalconductivitythanammonia.

B. Sodiumhydroxidehasahigherhydrogenionconcentrationthanammonia.

C. SodiumhydroxidehasahigherpHthanammonia.

D. Sodiumhydroxidehasahigherhydroxideionconcentrationthanammonia.

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23. Whichdefinitionofoxidationiscorrect?

A. Lossofelectronsandadecreaseinoxidationnumber

B. Lossofelectronsandanincreaseinoxidationnumber

C. Gainofelectronsandadecreaseinoxidationnumber

D. Gainofelectronsandanincreaseinoxidationnumber

24. WhatistheIUPACnameofFe2O3?

A. Ironoxide

B. Iron(II)oxide

C. Iron(III)oxide

D. Di-irontrioxide

25. Whichlabelsoftheelectrolyticcellarecorrect?

4

2 1

Pt Pt

KBr(l) 3

1 2 3 4

A. siteofreduction siteofoxidation conductor electrolyte

B. siteofoxidation siteofreduction electrolyte conductor

C. siteofreduction siteofoxidation electrolyte conductor

D. siteofoxidation siteofreduction conductor electrolyte

+–

crucible

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26. Whichisthebestdefinitionofstructuralisomers?

A. Compoundswhichhaveatomswiththesameatomicnumbersbutdifferentmassnumbers

B. CompoundswhichhavethesamegeneralformulabutdifferbyaCH2group

C. Compoundswhichhavethesameempiricalformulabutdifferentmolecularformulas

D. Compoundswhichhavethesamemolecularformulabutdifferentarrangementsofatoms

27. Whichisthecorrectclassificationofthesealcohols?

H C

H

H

C

H

H

C

OH

C

C

H

H

H

H

HH H C

H

H

C

H

H

C

C

H

C

H

H

H

HH

OH

H C

H

H

C

H

OH

C

C

H

C

H

H

H

HH

H

1 2 3

1 2 3

A. tertiary secondary primary

B. tertiary primary secondary

C. tertiary tertiary secondary

D. secondary primary secondary

28. Whichsubstancesarepossibleproductsoftheincompletecombustionofoctane?

A. Carbondioxideandhydrogengas

B. Carbonmonoxideandwatervapour

C. Carbonmonoxideandhydrogengas

D. Methaneandhydrogengas

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29. Whichstructurecouldrepresentarepeatingunitofapolymerformedfrompropene?

A. ( CH2–CH(CH3) (

B. ( CH2–CH2–CH2 (

C. ( CH(CH3)–CH(CH3) (

D. ( CH2–CH2 (

30. Whichexperimentalprocedureismostlikelytoleadtoalargesystematicerror?

A. Determiningtheconcentrationofanalkalibytitrationwithaburette

B. Measuringthevolumeofasolutionusingavolumetricpipette

C. Determiningtheenthalpychangeofneutralizationinabeaker

D. Measuringthevolumeofagasproducedwithagassyringe

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1. What is the coefficient of Fe3O4 when the following equation is balanced using the lowestwholenumbers?

__ __ __ __Al(s Fe O s Al O s Fe(s3 2) ( ) ( ) )4 3

A. 2

B. 3

C. 4

D. 5

2. Whatisthemass,ing,ofonemoleculeofethane,C2H6?

A. 3 0 10 23.

B. 5 0 10 23.

C. 30

D. 1 8 1025.

3. Whichmolecularformulaisalsoanempiricalformula?

A. PCl3

B. C2H4

C. H2O2

D. C6H12O6

4. WhichofthefollowingisconsistentwithAvogadro’slaw?

A. PT

constant(V,nconstant)

B. VT

constant(P,nconstant)

C. V n constant(P,Tconstant)

D. Vn

constant(P,Tconstant)

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5. AsampleofelementXcontains69%of63Xand31%of65X.WhatistherelativeatomicmassofXinthissample?

A. 63.0

B. 63.6

C. 65.0

D. 69.0

6. Howmanyelectronsdoestheion1531 3P contain?

A. 12

B. 15

C. 16

D. 18

7. WhatistheelectronarrangementoftheMg2+ion?

A. 2,2

B. 2,8

C. 2,8,2

D. 2,8,8

8. Whichpropertydecreasesdowngroup7intheperiodictable?

A. Meltingpoint

B. Electronegativity

C. Atomicradius

D. Ionicradius

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9. Whichoxidesproduceanacidicsolutionwhenaddedtowater?

I. P4O10II. MgO

III. SO3

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

10. Whatistheformulaofmagnesiumfluoride?

A. Mg2F3

B. Mg2F

C. Mg3F2

D. MgF2

11. Whatistheshapeoftheammoniamolecule,NH3?

A. Trigonalplanar

B. Trigonalpyramidal

C. Linear

D. V-shaped(bent)

12. Whichmoleculeispolar?

A. CH2Cl2

B. BCl3

C. Cl2

D. CCl4

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13. Whichsubstancecanformintermolecularhydrogenbondsintheliquidstate?

A. CH3OCH3

B. CH3CH2OH

C. CH3CHO

D. CH3CH2CH3

14. Whichcompoundhasacovalentmacromolecular(giantcovalent)structure?

A. MgO(s)

B. Al2O3(s)

C. P4O10(s)

D. SiO2(s)

15. Thestandardenthalpychangesforthecombustionofcarbonandcarbonmonoxideareshownbelow.

C(s O (g CO (g2 2) ) ) HcÖ 1394 kJmol

CO (g O (g CO (g2 2) ) )12 Hc kJmolÖ 283 1

Whatisthestandardenthalpychange,inkJ,forthefollowingreaction?

C(s O (g CO (g2) ) )12

A. –677

B. –111

C. +111

D. +677

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16. Whichiscorrectaboutenergychangesduringbondbreakingandbondformation?

Bond breaking Bond formation

A. exothermicand H positive endothermicand H negative

B. exothermicand H negative endothermicand H positive

C. endothermicand H positive exothermicand H negative

D. endothermicand H negative exothermicand H positive

17. Whichprocessesareexothermic?

I. Icemelting

II. Neutralization

III. Combustion

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

18. Whichunitcouldbeusedfortherateofachemicalreaction?

A. mol

B. moldm–3

C. moldm–3s–1

D. dm3

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19. Whichofthefollowingcanincreasetherateofachemicalreaction?

I. Increasingthetemperature

II. Addingacatalyst

III. Increasingtheconcentrationofreactants

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

20. Whatistheequilibriumconstantexpression,Kc,forthefollowingreaction?

N O (g NO (g2 4 2) )U 2

A. Kc2

2 4

NON O[ ][ ]

B. Kc2

NON O[ ][ ]

22

4

C. Kc2

NON O[ ][ ]

2

42

D. Kc 2NO N O[ ][ ]2 42

21. Considertheendothermicreactionbelow.

5 5CO (g I O (g CO (g I (g2 5 2 2) ) ) )U

AccordingtoLeChatelier’sprinciple,whichchangewouldresultinanincreaseintheamountofCO2?

A. Increasingthetemperature

B. Decreasingthetemperature

C. Increasingthepressure

D. Decreasingthepressure

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22. WhichspeciesbehaveasBrønsted-Lowryacidsinthefollowingreversiblereaction?

H PO aq CN aq HCN (aq HPO aq2 4 42( ) ( ) ) ( )U

A. HCNandCN–

B. HCNandHPO42–

C. H2PO4–andHPO4

2–

D. HCNandH2PO4–

23. Whichofthefollowingareweakacidsinaqueoussolution?

I. CH3COOH

II. H2CO3

III. HCl

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

24. Inwhichspeciesdoessulfurhaveanoxidationnumberof0?

A. SO3

B. S8

C. Na2SO4

D. H2S

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25. Whatisthereducingagentinthereactionbelow?

2 2 24 3MnO aq Br aq H O(l MnO (s BrO aq OH aq2 2( ) ( ) ) ) ( ) ( )

A. Br–

B. BrO3–

C. MnO4–

D. MnO2

26. Whichchangescouldtakeplaceatthepositiveelectrode(cathode)inavoltaiccell?

I. Zn2+(aq)toZn(s)

II. Cl2(g)toCl–(aq)

III. Mg(s)toMg2+(aq)

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

27. Whatisthestructuralformulaof2,3-dibromo-3-methylhexane?

A. CH3CHBrCHBrCH(CH3)CH2CH3

B. CH3CHBrCBr(CH3)CH2CH2CH3

C. CH3CH2CHBrCBr(CH2CH3)2

D. CH3CHBrCHBrCH(CH2CH3)2

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28. Whathappenswhenafewdropsofbrominewaterareaddedtoexcesshex-1-eneandthemixtureisshaken?

I. Thecolourofthebrominewaterdisappears.

II. Theorganicproductformeddoesnotcontainanycarbon-carbondoublebonds.

III. 2-bromohexaneisformed.

A. IandIIonly

B. IandIIIonly

C. IIandIIIonly

D. I,IIandIII

29. Whatistheproductofthefollowingreaction?

CH CH(OH)CH3 3Cr O H2 7

2 /

A. CH3COOH

B. CH3COCH3

C. CH3CH2COOH

D. CH3CH2CH3

30. Howmanysignificantfiguresaretherein0.00370?

A. 2

B. 3

C. 5

D. 6

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N08/4/CHEMI/SPM/ENG/TZ0/XX

1. Analytical chemists can detect amounts of amino acids as small as 2.0 10–21 mol of molecules. How many molecules does this represent?

A. 2.0 10–21

B. 1.2 103

C. 6.0 1023

D. 3.0 1044

2. One stage in the manufacture of nitric acid is the oxidation of ammonia:

__ NH (g) __ O (g) __ NO(g) __ H O(l)3 2 2

When the equation is balanced using the smallest possible whole numbers, what is the coefficient for NH3?

A. 2

B. 4

C. 5

D. 6

3. What amount of solute ions, in moles, is present in 50 cm3 of 0.10 mol dm–3 sodium hydroxide solution?

A. 2.5 10–3

B. 5.0 10–3

C. 1.0 10–2

D. 5.0 10–2

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4. Complete combustion of a hydrocarbon produces 0.44 g of CO2 and 0.18 g of H2O. What is the empirical formula of the hydrocarbon?

A. CH

B. CH2

C. CH3

D. CH4

5. Which species contains the same number of electrons and neutrons?

A. 11H

B. 12 H

C. 37 Li

D. 1735 Cl

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6. The mass spectrum of a sample of an element is shown below.

% a

bund

ance

40

20

064 65 66 67 68

mass / charge

Which value is closest to the relative atomic mass of the element?

A. 64.5

B. 65.0

C. 65.5

D. 66.0

7. In what order are the elements listed in the periodic table?

A. In order of relative atomic mass

B. In order of reactivity

C. In order of nuclear charge

D. In order of electronegativity

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8. The graph shows the trend in a physical property down group 7 in the periodic table.

Physical property

F Cl Br I

What is the physical property?

A. Atomic radius

B. Electronegativity

C. Density

D. Melting point

9. The table shows the boiling points of the hydrogen halides.

Compound Boiling point / °CHF 20HCl – 85HBr – 67HI – 35

Which statement explains the higher boiling point of hydrogen fluoride?

A. The covalent bond in hydrogen fluoride is stronger than those in the other hydrogen halides.

B. There is strong hydrogen bonding between the hydrogen fluoride molecules.

C. Fluorine is the most reactive element in group 7.

D. Fluorine has the highest first ionization energy in group 7.

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10. What happens when lithium and oxygen react together?

A. Each lithium atom gains one electron.

B. Each lithium atom loses one electron.

C. Each oxygen atom gains one electron.

D. Each oxygen atom loses one electron.

11. Which substance has the lowest electrical conductivity?

A. Al (s)

B. Al2O3(l)

C. KCl (aq)

D. HCl (g)

12. What is the C– C– C bond angle in CH3COCH3?

A. 180

B. 120

C. 109

D. 90

13. Which sample contains molecules with the greatest average kinetic energy?

A. H2 at 100 K

B. C3H8 at 273 K

C. N2 at 273 K

D. Br2 at 373 K

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14. Which graph shows the variation in volume of a fixed mass of an ideal gas with temperature in C at constant pressure?

A.

Volu

me

/ cm

3

0

B.

Volu

me

/ cm

3

00 0

Temp / C Temp / C

C.

Volu

me

/ cm

3

0

D.

Volu

me

/ cm

3

00 0

Temp / C Temp / C

15. Which statement about covalent bonds is correct?

A. Breaking covalent bonds is exothermic and releases energy.

B. Breaking covalent bonds is endothermic and absorbs energy.

C. Making covalent bonds is exothermic and absorbs energy.

D. Making covalent bonds is endothermic and releases energy.

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16. The average bond enthalpy for the C–H bond is 412 kJ mol–1 . Which process has an enthalpy change closest to this value?

A. CH (g) C(s) 2H (g)4 2

B. CH (g) C(g) 2H (g)4 2

C. CH (g) C(g) H (g)4 4

D. CH (g) CH (g) H (g)4 3

17. A reaction has a positive H Ö and a negative SÖ value. Which statement about this reaction is correct?

A. It is not spontaneous at any temperature.

B. It is spontaneous at all temperatures.

C. It is spontaneous only at low temperatures.

D. It is spontaneous only at high temperatures.

18. When 50 cm3 of 1.0 mol dm–3 nitric acid solution, HNO3(aq), is added to 50 cm3 of 1.0 mol dm–3

potassium hydroxide solution, KOH (aq), the temperature of the mixture increases by 6.4 C. What will be the temperature change when 25 cm3 of each of these solutions are mixed together?

A. 1.6 C

B. 3.2 C

C. 6.4 C

D. 12.8 C

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19. The graph below shows how the concentration of X changes with time during the following reaction:

X Y

[X] /

mol

dm

–3

0 50 100 150Time / s

Which graph shows the change in concentration of Y during the same time period?

A.

[Y] /

mol

dm

–3

B.

[Y] /

mol

dm

–3

0 50 100 150 0 50 100 150Time / s Time / s

C.

[Y] /

mol

dm

–3

D.

[Y] /

mol

dm

–3

0 50 100 150 0 50 100 150Time / s Time / s

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20. Which statement about the activation energy of a reaction is correct?

A. The activation energy is changed by the presence of a catalyst but not by an increase in temperature.

B. The activation energy is changed by an increase in temperature but not by the presence of a catalyst.

C. The activation energy is changed by both an increase in temperature and the presence of a catalyst.

D. The activation energy is not changed by either an increase in temperature or the presence of a catalyst.

21. The manufacture of ammonia is based on the equilibrium:

N (g) 3H (g) 2NH (g) kJ mol2 2 3U H Ö 92 1

Which changes will increase the equilibrium concentration of ammonia?

I. Increasing the pressure

II. Decreasing the temperature

III. Adding an iron catalyst

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

22. What alters the value of the equilibrium constant, Kc , for a reversible reaction?

A. Changing the temperature

B. Changing a reactant concentration

C. Changing a product concentration

D. Adding a catalyst

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23. Which statement describes a difference between strong acids and weak acids?

A. Solutions of weak acids cannot conduct an electric current but solutions of strong acids can conduct an electric current.

B. Strong acids can form concentrated solutions but weak acids cannot form concentrated solutions.

C. Weak acids are less soluble in water than strong acids.

D. Strong acids are more dissociated in aqueous solution than weak acids.

24. Which combinations form buffer solutions?

I. 50 cm3 of 0.1 mol dm–3 CH3COOH (aq) + 25 cm3 of 0.1 mol dm–3 NaOH (aq)

II. 50 cm3 of 0.1 mol dm–3 CH3COOH (aq) + 50 cm3 of 0.1 mol dm–3 NaOH (aq)

III. 50 cm3 of 0.1 mol dm–3 CH3COOH (aq) + 50 cm3 of 0.1 mol dm–3 CH3COONa (aq)

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

25. Which statement about the electrolysis of molten sodium bromide is correct?

A. Bromide ions lose electrons at the negative electrode.

B. Bromide ions gain electrons at the positive electrode.

C. Bromide ions gain electrons at the negative electrode.

D. Bromide ions move even if there is no current.

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26. In which compound does manganese have the highest oxidation number?

A. MnCl2

B. MnO2

C. Mn2O3

D. MnSO4

27. Palladium chloride changes colour in the presence of carbon monoxide as shown below.

PdCl (s) CO(g) H O(l) Pd (s) CO (g) 2HCl(aq)2 2 2

orange black

In terms of oxidation numbers, which changes occur during the reaction?

I. Palladium is reduced.

II. Carbon is oxidized.

III. Hydrogen is reduced.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

28. Which of the following can form an addition polymer?

A. Alanine (2-aminopropanoic acid)

B. Butane

C. But-2-ene

D. 1,2-dichlorobutane

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29. How many different compounds have the molecular formula C3H8O ?

A. 2

B. 3

C. 4

D. 5

30. Which compound, when hydrogenated, gives a product with a chiral centre?

A. CH2 = CH2

B. CH3CBr = CH2

C. CH3CH2CBr = CH2

D. CH3CH2C(CH3) = CH2

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1. What is the amount of atoms, in moles, in 88 g of carbon dioxide?

A. 6 02 1023.

B. 1 204 1024.

C. 6

D. 1

2. The isotopic abundances for an element, X, are 1428 X = 20 % and 14

29 X = 80 %. What is the relative atomic mass of element X?

A. 14

B. 28.2

C. 28.5

D. 28.8

3. Which statement is correct about the molecular formula of a compound?

A. It is an integer multiple of the empirical formula.It is an integer multiple of the empirical formula.

B. It shows how the atoms are bonded together in the molecule.It shows how the atoms are bonded together in the molecule.

C. It is the smallest ratio between the atoms present in a molecule.It is the smallest ratio between the atoms present in a molecule.

D. It is the percentage composition of a molecule.It is the percentage composition of a molecule.

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4. A sample of a hydrocarbon contains 84 g of carbon and 14 g of hydrogen. Which of the following statements are correct?

I. The empirical formula of the compound isThe empirical formula of the compound is CH2. II. The molecular formula of the compound isThe molecular formula of the compound is C H2 4. III. ��

is C H2 4.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

5. An isotope of uranium has a mass number of 235. What is the number of neutrons in the nucleus and the atomic number for this isotope?

Number of neutrons Atomic numberA. 143 235B. 92 235C. 143 92D. 238 92

6. Which process is responsible for the lines in the visible emission spectrum of hydrogen?

A. The release of energy by the electronThe release of energy by the electron

B. The release of energy by the excited nucleusThe release of energy by the excited nucleus

C. The excitation of the electronThe excitation of the electron

D. The absorption of energy by the electronThe absorption of energy by the electron

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7. Which reactions are spontaneous?

I. Cl (aq) KBr (aq) Br (aq) KCl(aq)2 22 2 II. I (aq) KBr (aq) Br (aq) KI (aq)2 22 2 III. Cl (aq) NaI (aq) I (aq) NaCl(aq)2 22 2

A. I and II onlyI and II only

B. I and III onlyI and III only

C. II and III onlyII and III only

D. I, II and IIII, II and III

8. Which statements support the description of aluminium oxide as amphoteric?

I. It can show acidic behaviour in the presence of strong alkalis. II. It can show alkaline behaviour in the presence of strong acids. III. It dissolves in water to form a neutral solution.

A. I and II onlyI and II only

B. I and III onlyI and III only

C. II and III onlyII and III only

D. I, II and IIII, II and III

9. Which species has the same electron arrangement as a Ca2 ion?

A. Al3 ion

B. Br ion

C. Ar atom

D. K atom

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10. W��?

A. Mg N2 3 and Al S2 3

B. Mg N3 2 and Al S2 3

C. Mg N2 3 and Al S3 2

D. Mg N3 2 and Al S3 2

11. Which molecule is the most polar?

A. CH4

B. CCl4 C. CF4 D. CHCl3

12. What is the shape of PCl3?

A. Trigonal planar

B. Trigonal pyramidal

C. Tetrahedral

D. V-shaped (bent)

13. Which changes occur when a liquid boils?

I. The spacing between the particles increases. II. The average energy of the particles increases. III. The attractive forces between the particles become weaker.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

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14. A gas sample occupies a volume V1 at a pressure P1 and a Kelvin temperature T1. What would be the temperature, T2, of the gas if both its pressure and volume are doubled?

A. T T212 1=

B. T T2 1

C. T T2 12

D. T T2 14

15. Which of the following is correct about the energy changes during bond breaking and bond formation?

Bond breaking Bond formationA. exothermic endothermicB. exothermic exothermicC. endothermic endothermicD. endothermic exothermic

16. A possible method of preparing hydrogen peroxide is:

H O (g) H O(l)2 2212( )g H xÖ

H O(l) O (g) H O (l)2 2 2212 H yÖ

Which expression can be used to calculate the enthalpy change for the decomposition of hydrogen peroxide using this data?

H O (l) H (g) O (g)2 2 2 2 H Ö

A. x y

B. x y

C. x y

D. x y

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17. What should be the signs of G, H and S for a chemical reaction to be spontaneous at any temperature?

∆∆G ∆∆H ∆∆SA. positive negative positiveB. negative negative negativeC. negative negative positiveD. negative positive negative

18. Which of the following reactions is likely to have the largest negative entropy change, S?

A. C(s) O (g) CO (g)22

B. N O (g) 2NO (g)2 4 2

C. 2 22 2 3SO (g) O (g) SO (g)

D. N (g) H (g) NH (g)2 23 2 3

19. Which statement explains why increasing the temperature increases the rate of a chemical reaction?

A. More molecules have energy equal to or greater than the activation energy.More molecules have energy equal to or greater than the activation energy.

B. At a higher temperature the activation energy for the reaction is lower.At a higher temperature the activation energy for the reaction is lower.

C. More molecules have the correct collision geometry.More molecules have the correct collision geometry.

D. The reaction proceeds according to Le Chatelier’s principle.The reaction proceeds according to Le Chatelier’s principle.

20. What is the best way to describe the rate-determining step in a reaction mechanism?

A. The fastest step of a chemical reactionThe fastest step of a chemical reaction

B. The slowest step of a chemical reactionThe slowest step of a chemical reaction

C. The step where the fewest molecules interactThe step where the fewest molecules interact

D. The step where most molecules have the highest energyThe step where most molecules have the highest energy

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21. Consider the reaction:

2A (g) B(g) C(g) D(g)3 2U

What is the expression for the equilibrium constant, Kc ?

A. Kc[C] 2[D]2[A] 3[B]

B. Kc2[A] [B][C] [D]

= 32

C. Kc

2

2 3

[C][D][A] [B]

D. Kc

2 3

2

[A] [B][C][D]

22. Consider the following reaction:

N (g) H (g) NH (g)2 2 33 2 92U H Ö kJ

Which of the following affects the value of Kc ?

A. Adding a catalystAdding a catalyst

B. Increasing the pressureIncreasing the pressurepressure

C. Increasing the concentrations of nitrogen and hydrogenIncreasing the concentrations of nitrogen and hydrogen

D. Increasing the temperatureIncreasing the temperature

23. Which compound will produce a solution with a pH greater than 7 when added to water?

A. NaHCO (s)3

B. SiO (s)2

C. SO (g)3

D. CH CO H (aq)3 2

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24. Which pair of solutions can be used to prepare a buffer solution?

A. CH COONa (aq) NaOH (aq)3 /

B. NH (aq) NH NO (aq)3 4 3/

C. NH Cl(aq) HCl(aq)4 /

D. HNO (aq) NaNO (aq)3 3/

25. What is the oxidation number of vanadium in the compound NaVO3?

A. –1 B. 0 C. +2 D. +5

26. Which statement about electrochemical cells is correct?

A. The reaction in a voltaic cell is spontaneous. B. The reaction in an electrolytic cell is spontaneous. C. The reaction in a voltaic cell uses electrical energy. D. The reaction in an electrolytic cell produces electrical energy.

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27. Consider the following reaction:

Sn (aq) Fe (aq) Sn (aq) Fe (aq)4 2 3 3

What is the correct combination of statements?

Species Undergoes Acts as

A. Sn4+ oxidation oxidizing agent

B. Fe2+ reduction reducing agent

C. Sn4+ reduction oxidizing agent

D. Fe2+ reduction oxidizing agent

28. Which molecule has a chiral carbon atom?

A. CH CClCH CH2 2 3

B. CH CHOHCH CH3 2 3

C. (CH ) CHCH CH3 2 2 3

D. H NCH COOH2 2

29. The polymerization of ethene H C CH2 2 produces polythene as shown below.

n = nH C CH CH CH2 2 2 2[ ]

What type of reaction has ethene undergone?

A. Hydrogenation

B. Addition

C. Isomerisation

D. Condensation

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30. What type of linkage forms between two amino acids, when they react with each other?

A. Ketone B. Amine C. Amide D. Ester

Documents

Chemistry SL paper 1 TZ1 2009 - Examibrelics.weebly.com/.../chemistry_sl_paper_1_.pdf · 2209-6110 – 3 – Turn over M09/4/CHEMI/SPM/ENG/TZ1/XX+ 1. The molar mass of a compound