Chemistry 9701/11 May/June 2023: question paper and mark scheme

Question

Element X has six more protons than element Y. Which statement must be correct? A Atoms of element Y are smaller than atoms of element X. B Element X has a full shell of electrons. C Element X and element Y are in the same group. D Element X and element Y are in the same period.

Question

Which statement explains why calcium has a higher melting point than barium? A Calcium cations are smaller than barium cations and have a stronger attraction to the delocalisedelectrons. B The structure of calcium is partly giant molecular. C Therearemoredelocalisedelectronsincalciumthaninbariumasithasalowerionisation energy. D There is greater repulsion between barium atoms as they have more complete electron shellsthancalciumatoms.

Question

Three statements about potassium and chlorine and their ions are listed. 1 The atomic radius of a potassium atom is greater than the atomic radius of a chlorine atom. 2 The first ionisation energy of potassium is greater than the first ionisation energy of chlorine. 3 The ionic radius of a potassium ion is greater than the ionic radius of a chloride ion. Which statements are correct? A 1 only B 2 only C 1 and 3 D 2 and 3

Question

For which equilibrium do both of the equilibrium constants Kc and Kp have no units? A H2(g) + I2(g) 2HI(g) B N2(g) + 3H2(g) 2NH3(g) C N2O4(g) 2NO2(g) D SO2(g) + O2(g) SO3(g) ‹8&/(6 0- –1

Question

Calciumcarbide,CaC2,reactswithwater,asshown.Thedatabelowtheequationshow,inkJmol , thestandardenthalpiesofformationofthecompoundsinvolved. CaC2(s) + H2O(l) → CaO(s) + C2H2(g) –60 –286 –635 +228 What is the standard enthalpy change of the reaction shown? –1 A –753 kJ mol –1 B –61 kJ mol –1 C +61 kJ mol –1 D +753 kJ mol

Question

Inthesodiumchloridelatticethenumberofchlorideionsthatsurroundeachsodiumioniscalled thecoordinationnumberofthesodiumions. Whatarethecoordinationnumbersofthesodiumionsandthechlorideionsinthesodiumchloride lattice? coordination number coordination number of sodium ions of chloride ions A 4 6 B 6 4 C 6 6 D 8 6

Question

Histidine is an amino acid. histidine H H 2 H 1 H N O C H N C C C C 3 C N H H O H H What are the approximate bond angles 1, 2, and 3? 1 2 3 A 109.5° 107° 90° B 120° 107° 109.5° C 120° 120° 90° D 120° 120° 109.5°

Question

The Contact process takes place at a pressure between 100 000 Pa and 200 000 Pa. A catalyst is used. Which statement is correct? A A V2O5 catalyst is added to increase the equilibrium yield of the reaction. B Changes in pressure have no effect on the position of equilibrium. C The equilibrium yield of the reaction is very high under the conditions used. D An iron catalyst is added to increase the rate of reaction. ‹8&/(6 0-

Question

Bromine reacts with aqueous sodium hydroxide at 25 °C. reaction 1 Br2(aq) + 2NaOH(aq) → NaBr(aq) + NaOBr(aq) + H2O(l) The NaOBr formed is unstable at 25 °C and reacts further. reaction 2 3NaOBr(aq) → 2NaBr(aq) + NaBrO3(aq) Which reactions are disproportionations? A both reaction 1 and reaction 2 B neither reaction 1 nor reaction 2 C reaction 1 only D reaction 2 only

Question

Which statement is correct? 35 A The relative atomic mass of a Cl atom is 35.5. B The relative formula mass of CaCO3 is 100.1. 24 C The relative isotopic mass of a Mg atom is 24.3. D The relative molecular mass of O2 is 16.0.

Question

Iodine and propanone react according to the following equation. I2(aq) + CH3COCH3(aq) → CH3COCH2I(aq) + HI(aq) If the concentration of propanone is increased, keeping the total reaction volume constant, the initial rate of the reaction also increases. What could be the reason for this? A A greater proportion of collisions are successful at the higher concentration. B The particles are further apart at the higher concentration. C The particles have more energy at the higher concentration. D There are more collisions per second between particles at the higher concentration.

Question

Four successive ionisation energies (IE) of element E are shown. Element E is in Period 3 of the Periodic Table. fifth IE sixth IE seventh IE eighth IE –1 –1 –1 –1 / kJ mol / kJ mol / kJ mol / kJ mol 16 000 20 000 24 000 29 000 In which group of the Periodic Table is E? A 14 B 15 C 16 D 17

Question

In this question you should assume that the gas formed behaves as an ideal gas. 3 –3 A 1.7 g sample of Mg reacts with 50.0 cm of 2.2 mol dm HCl at 303 K and 110 400 Pa. Which volume of gas is produced, measured under these conditions? 3 3 3 3 A 1.3 dm B 1.6 dm C 2.5 dm D 5.0 dm

Question

Chlorine dioxide, Cl O2, reacts with aqueous sodium hydroxide to produce water and a mixture of two sodium salts, NaCl O2 and NaCl O3. What is the mole ratio of NaCl O2 to NaCl O3 in the product mixture? A 1:2 B 3:5 C 1:1 D 5:3

Question

The temperature of a sample of an inert gas is increased. What effect does this have on the number of molecules with the most probable energy and on the number of molecules with higher energy? number of molecules with the number of molecules with most probable energy higher energy A decreases decreases B decreases increases C increases decreases D increases increases ‹8&/(6 0-

Question

For which compound is there the greatest percentage loss of mass on strong heating? A anhydrous calcium carbonate B anhydrous calcium nitrate C anhydrous magnesium carbonate D anhydrous magnesium nitrate

Question

The solids sodium chloride and sodium iodide both react with concentrated sulfuric acid at room temperature. With NaCl , the products are NaHSO4 and HCl . With NaI, the products are NaHSO4, HI, I2, SO2, H2O, S and H2S. What is the explanation for this difference in products? A Chloride ions will displace iodine from the solution. B Hydrogen chloride is more volatile than hydrogen iodide. C Iodide ions are better reducing agents than chloride ions. D Sulfuric acid is able to act as a dehydrating agent with NaI.

Question

SiO2 has a melting point of 1713 °C. It reacts with hot NaOH(aq) to form sodium silicate, Na2SiO3, and water. No reaction occurs when SiO2 is added to hot H2SO4(aq). What can be deduced from this information? chemical structure behaviour of SiO2 of SiO2 A amphoteric giant B amphoteric simple C acidic giant D acidic simple

Question

Element X has the second largest atomic radius in its period. An atom of X has three occupied electron shells only. The oxide of X is shaken with water. What could be the pH of the resulting solution? A 5 B 7 C 9 D 14

Question

Which emission from an internal combustion engine contributes to the erosion of marble statues? A carbon monoxide B nitrogen C nitrogen dioxide D unburnt hydrocarbons

Question

The diagram shows the melting points of eight elements with consecutive atomic numbers. Which element could be sodium? D melting point / K C A B atomic number ‹8&/(6 0-

Question

The boiling points of Br2, ICl and IBr are given in the table. Br2 ICl IBr boiling point / °C 59 97 116 Which row explains: • whytheboilingpointofIClisgreaterthanBr2 • whytheboilingpointofIBrisgreaterthanICl ? boiling point of ICl is boiling point of IBr is greater than Br2 greater than ICl A ICl has stronger instantaneous IBr has stronger instantaneous dipole-induced dipoles dipole-induced dipoles B ICl has permanent dipoles IBr has stronger instantaneous dipole-induced dipoles C ICl has stronger instantaneous IBr has stronger dipole-induced dipoles permanent dipoles D ICl has permanent dipoles IBr has stronger permanent dipoles 2+ 2+

Question

A solution contains both Mg (aq) and Sr (aq) at the same concentration. The solution is divided into two equal portions. Aqueous sodium hydroxide is added dropwise to one portion. Dilute sulfuric acid is added dropwise to the other portion. Which row is correct? precipitate seen first precipitate seen first when NaOH(aq) is added when H2SO4(aq) is added A magnesium hydroxide magnesium sulfate B magnesium hydroxide strontium sulfate C strontium hydroxide magnesium sulfate D strontium hydroxide strontium sulfate

Question

Structural isomerism and stereoisomerism should be considered when answering this question. If a molecule contains two non-identical chiral carbon atoms, four optical isomers exist. How many isomers are there with: • molecular formula C7H14O and • a five-membered ring and • a tertiary alcohol group? A 4 B 5 C 9 D 13

Question

Which reagent will react with pentan-3-ol to give a mixture of stereoisomers? A acidified potassium dichromate B concentrated sulfuric acid C ethanoic acid in the presence of a little concentrated H2SO4 D hydrogen chloride

Question

An organic molecule W contains 3 carbon atoms. It requires 4.5 molecules of oxygen for complete combustion. What could W be? A propane B propanoic acid C propanone D propan-1-ol

Question

Which equation represents a reaction that proceeds through initiation, propagation and termination steps? A C4H10 + Cl 2 → C4H9Cl + HCl B C5H11Br + NaOH → C5H11OH + NaBr C C6H12 + H2O → C6H13OH D C6H13CHO + HCN → C6H13CH(OH)CN ‹8&/(6 0-

Question

Structuralisomerismandstereoisomerismshouldbeconsideredwhenansweringthisquestion. Asetofisomerichydrocarbons • allcontain14.3%bymassofhydrogen • allreactwithbrominebyaddition,0.280gofeachhydrocarbonreactingwith0.799gof bromine. What is the maximum number of isomeric compounds in the set? A 1 B 3 C 4 D 5

Question

Which row describes the solvent used and type of reaction occurring when bromoethane reacts with NaOH to form ethene? solvent type of reaction A ethanol elimination B ethanol substitution C water elimination D water substitution

Question

Whichrowdescribesthetypeofreactionthatoccurswhenpropan-1-olreactstoformthenamed carbon-containingproduct? carbon-containing product type of reaction A 1-chloropropane addition to propan-1-ol B carbon monoxide complete combustion of propan-1-ol C propene dehydration of propan-1-ol D propanal reduction of propan-1-ol

Question

Which statement describes what happens when 2-chloro-2-methylpropane is warmed with NaOH(aq)? A This secondary halogenoalkane reacts by a mixture of an SN1 and an SN2 mechanism. B This secondary halogenoalkane reacts only by an SN2 mechanism. C This tertiary halogenoalkane reacts mostly by an SN1 mechanism. D This tertiary halogenoalkane does not react with hydroxide ions under these conditions.

Question

How many structurally isomeric secondary alcohols are there with the molecular formula C5H12O? A 1 B 2 C 3 D 4

Question

Which reagent: • canconfirmthepresenceofacarbonylgroupinanorganiccompound • doesnotdistinguishbetweenaldehydesandketones? A acidified K2Cr2O7 B 2,4-DNPH reagent C Fehling’s reagent D LiAl H4

Question

Which compound gives a positive test with alkaline aqueous iodine and does not show optical isomerism? A CH3COCH2CH2OH B CH3CH2CH(OH)CHO C CH3COCH(OH)CH3 D (CH3)2C(OH)CHO ‹8&/(6 0-

Question

TwosamplesofcompoundXweretreatedseparatelywithdifferentreagentswhichwereaddedin excess. Theproductsofthesetworeactionsareshown. OH O OH reaction 1 OH O O O compound X OH OH reaction 2 OH Which reagents could be used for reaction 1 and reaction 2? reaction 1 reaction 2 A hot acidifiedsodiumdichromate VI Na B hot acidifiedsodiumdichromate VI NaBH4 C Tollens’reagentfollowedbyHCl (aq) Na D Tollens’reagentfollowedbyHCl (aq) NaBH4

Question

Which method could produce butanoic acid? A an acid–base reaction involving CH3CH2CH2CO2Na B the hydrolysis of CH3CH2CH2CH2CN C the acidic hydrolysis of CH3CH2COOCH2CH2CH3 D the oxidation of CH3CH2CH2OH

Question

Which ester may be hydrolysed to produce two products, one of which may be reduced to the other? A CH3CH2CO2CH3 B CH3CH(CH3)CO2CH2CH(CH3)2 C CH3CH2CO2CH(CH3)2 D (CH3)2CHCO2CH(CH3)2

Question

Two compounds, X and Y, are mixed and a little concentrated H2SO4 is added. Ester Z is found in the resulting mixture of products. ester Z O O O O O O Which two compounds could be X and Y? X Y A CH3CH2OH CH(CO2H)3 B CH3CH2OH CH3CO2CH2CH(OH)CH2OCOCH2CH3 C CH3CO2H CH3CH2CO2CH2CH(OH)CH2OH D CH3CO2H CH2(OH)CH(OH)CH2(OH)

Question

The diagram shows a section of a polymer molecule. –CH2–CH=CH–CH2–CH2–CH=CH–CH2– Which monomer will produce this polymer? A CH2=CH2 B CH3CH=CH2 C CH3CH=CHCH3 D CH2=CH–CH=CH2 ‹8&/(6 0-

Question

There are two naturally occuring isotopes of bromine. One isotope has 44 neutrons. The other isotopehas46neutrons. 12 1 Ignoringfragments,howmanypeaksarethereinthemassspectrumoftribromomethane, C HBr3? A 2 B 3 C 4 D 6 ‹8&/(6 0- ‹8&/(6 0- ‹8&/(6 0- ‹8&/(6 0- ,PSRUWDQWYDOXHVFRQVWDQWVDQGVWDQGDUGV PRODUJDVFRQVWDQW R -.±PRO± )DUDGD\FRQVWDQW F u&PRO± $YRJDGURFRQVWDQW L uPRO± HOHFWURQLFFKDUJH e ±u±& PRODUYROXPHRIJDV VP GPPRO±DWVWS N3DDQG. VP GPPRO±DWURRPFRQGLWLRQV LRQLFSURGXFWRIZDWHU KZ u±PROGP± DW. q& VSHFLILFKHDWFDSDFLW\RIZDWHU c N-NJ±.± -J±.±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‹8&/(6 0- ‹8&/(6 The Periodic Table of Elements Group 1 2 13 14 15 16 17 18 1 2 H He hydrogen helium Key 1.0 4.0 3 4 atomic number 5 6 7 8 9 10 Li Be atomic symbol B C N O F Ne lithium beryllium name boron carbon nitrogen oxygen fluorine neon 6.9 9.0 relative atomic mass 10.8 12.0 14.0 16.0 19.0 20.2 11 12 13 14 15 16 17 18 Na Mg Al Si P S Cl Ar sodium magnesium aluminium silicon phosphorus sulfur chlorine argon 23.0 24.3 3 4 5 6 7 8 9 10 11 12 27.0 28.1 31.0 32.1 35.5 39.9 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton 39.1 40.1 45.0 47.9 50.9 52.0 54.9 55.8 58.9 58.7 63.5 65.4 69.7 72.6 74.9 79.0 79.9 83.8 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon 85.5 87.6 88.9 91.2 92.9 95.9 – 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 0- 55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 lanthanoids Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon 132.9 137.3 178.5 180.9 183.8 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 – – – 87 88 89–103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 actinoids Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium nihonium flerovium moscovium livermorium tennessine oganesson – – – – – – – – – – – – – – – – – 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium 138.9 140.1 140.9 144.4 – 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.1 175.0 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium – 232.0 231.0 238.0 – – – – – – – – – – –