Chemistry 2024 May/June | Past Paper

Q1(a)

Short Answer 2 marks

Complete Table 1.1 using relevant information from the Periodic Table. Table 1.1 nucleon number proton number number of electrons

Q1(b)

Short Answer 1 mark

State and explain the difference in the ionic radius of Al compared to Mg

Q1(c)

Short Answer 1 mark

Draw a labelled diagram to show the structure and bonding in sodium.

Q1(d)

Short Answer 1 mark

Fig. 1.1 shows the variation in melting point of some Period 3 elements in their standard states at room temperature and pressure. 2000 2500 1500 1000 NaMgAlSi element melting point / K PSCl Fig. 1.1 * 0019655306502 *

Q1(i)

Short Answer 1 mark

Explain why Si has a high melting point.

Q1(ii)

Short Answer 2 marks

Complete Fig. 1.1 to show the variation in the melting points of the elements P , S and Cl.

Q1(e)

Short Answer 1 mark

Two Period 3 elements react with an excess of ox ygen at room pressure.

Q1(i)

Short Answer 2 marks

Complete T able 1.2. Table 1.2 1 2 3 Period 3 element state of oxide at room temperature and pressure approximate pH of solution made when oxide is added to water

Q1(ii)

Short Answer 1 mark

The solutions made in column 3 of Table 1.2 are mixed together. Name the type of reaction that occurs.

Q1(iii)

Short Answer 1 mark

Write an equation to describe the reaction between P and an excess of water.

Q1(f)

Short Answer 1 mark

Aluminium hydroxide is amphoteric.

Q1(i)

Short Answer 1 mark

Explain what is meant by amphoteric.

Q1(ii)

Short Answer 1 mark

Write an equation to describe the reaction that occurs when aluminium hydroxide, Al (OH) , reacts with NaOH(aq). [Total: 15] * 0019655306503 *

Q2

Short Answer 1 mark

Separate samples of Na and NaHCO react with HCl (aq) to produce the same products, as shown in Table 2.1. Table 2.1 1 Na + 2HCl 2NaCl + H O + CO 2 NaHCO + HCl NaCl + H O + CO = +27.2

Q2(a)

Short Answer 1 mark

Complete the reaction pathway diagram in Fig. 2.1 for reaction 2. , and the activation energy, E NaHCO + HCl energy / kJ mol progress of reaction [2] is determined by experiment using the following method. · 50.0 cm of 2.00 mol dm HCl (aq) is added to a polystyrene cup. · The initial temperature of the acid is recorded as 19.6 °C. · 0.0400 mol of Na is added and the mixture is stirred. · All the solid Na disappears and a colourless solution is produced. The maximum temperature recorded during the reaction is 26.2 °C.

Q2(i)

Short Answer 3 marks

Describe one other observation that shows the reaction is complete. in kJ mol Assume the specific heat capacity of the reaction mixture is the same as for water and no heat is lost to the surroundings. Show your working. = kJ mol

Q2(iii)

Short Answer 1 mark

Thermal decomposition occurs when NaHCO is heated. reaction 3 2NaHCO + H O + CO , using the data in Table 2.1 and the calculated in

Q2(iii)(ii)

Short Answer 1 mark

, assume the enthalpy change is ±38.4 kJ mol . This is not the correct value.) = kJ mol

Q2(c)

Short Answer 1 mark

Z is a salt that contains a Period 4 element from Group 2. When Z is heated brown gas forms. Identify the formula of Z and use it to write an equation for the reaction. [Total: 10] * 0019655306505 *

Q3(a)

Short Answer 1 mark

Describe what is meant by dynamic equilibrium.

Q3(b)

Short Answer 1 mark

Reaction 4 describes the reversible reaction between yellow Fe

Q3(aq)

Short Answer 1 mark

and colourlessSCN

Q3(aq)

Short Answer 1 mark

to produce red FeSCN

Q3(aq)

Short Answer 1 mark

reaction 4 Fe

Q3(aq)

Short Answer 1 mark

FeSCN

Q3(aq)

Short Answer 1 mark

yellow colourless red An equilibrium mixture contains Fe

Q3(aq)

Short Answer 1 mark

, SCN

Q3(aq)

Short Answer 1 mark

and FeSCN

Q3(aq)

Short Answer 1 mark

A few colourless crystals of soluble KSCN

Q3(aq)(s)

Short Answer 1 mark

are added. The mixture is then left until it reaches equilibrium again. The temperature of both equilibrium mixtures is the same.

Q3(i)

Short Answer 1 mark

Deduce the changes that occur , if any, in the equilibrium mixture after KSCN

Q3(i)(s)

Short Answer 1 mark

is added compared to the original equilibrium mixture. · change in appearance · change in relative concentration of Fe

Q3(aq)

Short Answer 1 mark

· change in value of the equilibrium constant, K [3] * 0019655306506 *

Q3(ii)

Short Answer 1 mark

The expression for the equilibrium constant, K , for reaction 4 is shown. [FeSCN

Q3(aq)

Short Answer 1 mark

] [Fe

Q3(aq)

Short Answer 1 mark

] × [SCN

Q3(aq)

Short Answer 1 mark

] 5.00 × 10 mol of Fe

Q3(aq)

Short Answer 1 mark

and 5.00 × 10 mol of SCN

Q3(aq)

Short Answer 1 mark

are added together and allowed to reach equilibrium. The total volume of the mixture is 25.0 cm At equilibrium the concentration of FeSCN

Q3(aq)

Short Answer 1 mark

is 4.23 × 10 mol dm Calculate the equilibrium constant, K , for reaction 4. Include the units in your answer. = units [4] * 0019655306507 *

Q3(c)

Short Answer 1 mark

Determine the full electronic configuration of Fe

Q3(aq)

Short Answer 1 mark

is colourless. Complete the dot-and-cross diagram in Fig. 3.1 to show the arrangement of outer electrons in an SCN ion. S C N [2] [Total: 12] * 0019655306508 *, , BLANK PAGE * 0019655306609 * 4 CH (CH CHBrCH exists as a pair of stereoisomers.

Q3(a)

Short Answer 2 marks

Draw the three-dimensional structures of the two stereoisomers of CH (CH CHBrCH R can be used to represent CH (CH

Q3(b)

Short Answer 3 marks

A sample of CH (CH CHBrCH reacts with NaOH to make CH (CH CH(OH)CH in an 1 mechanism. Complete Fig. 4.1 to show the mechanism for the reaction of CH (CH CHBrCH and NaOH. Include charges, dipoles, lone pairs of electrons and curly arrows, as appropriate. (CHBrC (CHOHC

Q3(c)

Short Answer 1 mark

Separate samples of CH (CH CHBrCH , CH (CH CH(OH)CH and CH (CH CHCH are tested with different reagents. Complete Table 4.1. If no reaction occurs, write × in the relevant box. Table 4.1 reagent added observation with (CH CHBrCH observation with (CH CH(OH)CH observation with (CH CHCH

Q3(l)

Short Answer 1 mark

in the darkPCl

Q3(aq)

Short Answer 1 mark

[3] * 0019655306610 *

Q3(d)

Short Answer 1 mark

CH (CH CHBrCH is heated with D to produce three dif ferent molecules, E, F and G. FE G

Q3(i)

Short Answer 1 mark

Name the type of reaction.

Q3(ii)

Short Answer 1 mark

Identify D and the conditions used.

Q3(e)

Short Answer 2 marks

(i) Both σ and π bonds are present in a molecule of E as a result of dif ferent types of hybridisation in the carbon atoms. Complete Table 4.2 to show the number of carbon atoms with each type of hybridisation in a molecule of E. Table 4.2 number of carbon atoms sp hybridised sp hybridised sp hybridised FE G

Q3(ii)

Short Answer 1 mark

Describe the essential feature of an unbranched hydrocarbon that causes its molecules to show stereoisomerism. Explain how this feature leads to stereoisomerism. [Total: 15] * 0019655306611 *

Q5

Short Answer 1 mark

Compound W has molecular formula C O. It contains only one functional group.

Q5(a)

Short Answer 1 mark

Table 5.1 shows the two peaks with the greatest m / e values in the mass spectrum of W. Table 5.1 m / e relative abundance 74 50 75 x

Q5(i)

Short Answer 1 mark

Calculate the relative abundance, x, of the peak at m / e = 75 using the information from Table 5.1. x =

Q5(ii)

Short Answer 2 marks

The mass spectrum of W also shows peaks at m / e = 29 and m / e = 59. Suggest the molecular formulae of these fragments. m / e = 29 m / e = 59

Q5(b)

Short Answer 1 mark

A sample of W, C O, is heated under reflux with an ex cess of acidified K until there is no further reaction. Only one organic product, X, is present in the mixture at the end of the reaction. Fig. 5.1 shows the infrared spectrum of W. 35004000 3000 2500 2000 wavenumber / cm transmittance / % 1500 1000 500 Fig. 5.1 * 0019655306612 * Fig. 5.2 shows the infrared spectrum of X. wavenumber / cm transmittance / % 35004000 3000 2500 2000 1500 1000 500 Table 5.2 bondfunctional groups containing the bond characteristic infrared absorption range (in wavenumbers) / cm C±O hydroxy, ester 1040±1300 C=C aromatic compound, alkene 1500±1680 C=O amide carbonyl, carboxyl ester 1640±1690 1670±1740 1710±1750 C±H alkane 2850±2950 N±H amine, amide 3300±3500 O±H carboxyl hydroxy 2500±3000 3200±3650

Q5(i)

Short Answer 1 mark

Absorption A is shown in Fig. 5.1. Absorption B is shown in Fig. 5.2. Complete Table 5.3 using the information given in Fig. 5.1, Fig. 5.2 and Table 5.2. Table 5.3 absorption bond functional group containing the bond [1] * 0019655306613 *

Q5(ii)

Short Answer 1 mark

Use the information in (a) and (b)(i) to draw the structure of X in the box in Fig. 5.3. acidified

Q5(c)

Short Answer 1 mark

Y is a structural isomer of W. Both W and Y produce colourless bubbles when sodium is added to them. Y does not react when heated with acidified K Y does not react when warmed with alkaline I

Q5(i)

Short Answer 1 mark

Name the functional group present in Y.

Q5(ii)

Short Answer 1 mark

Complete the equation to describe the reaction of W or Y with sodium. O + Na

Q5(iii)

Short Answer 1 mark

Draw the structure of Y. [1] [Total: 8] * 0019655306614 * Important values, constants and standards molar gas constant R = 8.31 J Kmol Faraday constant F = 9.65 × 10 C mol Avogadro constant L = 6.022 × 10mol electronic charge e = ±1.60 × 10±19 molar volume of gas V = 22.4 dmmol at s.t.p. (101 kPa and 273 K) = 24.0 dmmol at room conditions ionic product of water K = 1.00 × 10±14mol (at 298 K (25 °C)) speci®c heat capacity of waterc = 4.18 kJ kg (4.18 J g ) * 0019655306615 * To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge Assessment International Education Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cambridgeinternational.org after the live examination series. Group The Periodic Ta ble of Elements hydrogen 1.0 helium 4.0 12 13 14 15 16 17 18 3456789 10 11 12 lithium 6.9 beryllium 9.0 atomic number atomic symbolKey name relative atomic mass sodium 23.0 magnesium 24.3 potassium 39.1 calcium 40.1 rubidium 85.5 strontium 87.6 caesium 132.9 barium 137.3 francium radium boron 10.8 aluminium 27.0 gallium 69.7 indium 114.8 thallium 204.4 carbon 12.0 silicon 28.1 germanium 72.6tin 118.7 lead 207.2 titanium 47.9 zirconium 91.2 hafnium 178.5 rutherfordium vanadium 50.9 niobium 92.9 tantalum 180.9 dubnium chromium 52.0 molybdenum 95.9 tungsten 183.8 seaborgium manganese 54.9 technetium rhenium 186.2 bohrium iron 55.8 ruthenium 101.1 osmium 190.2 hassium cobalt 58.9 rhodium 102.9 iridium 192.2 meitnerium nickel 58.7 palladium 106.4 platinum 195.1 darmstadtium copper 63.5 silver 107.9 gold 197.0 roentgenium zinc 65.4 cadmium 112.4 mercury 200.6 copernicium flerovium livermorium nitrogen 14.0 phosphorus 31.0 arsenic 74.9 antimony 121.8 bismuth 209.0 oxygen 16.0 sulfur 32.1 selenium 79.0 tellurium 127.6 polonium fluorine 19.0 chlorine 35.5 bromine 79.9 iodine 126.9 neon 20.2 argon 39.9 krypton 83.8 xenon 131.3 radon nihonium moscovium tennessine oganesson scandium 45.0 yttrium 88.9 57±71 lanthanoids 89±103 actinoids lanthanum 138.9 lanthanoids actinoids actinium cerium 140.1 thorium 232.0 praseodymium 140.9 protactinium 231.0 neodymium 144.2 uranium 238.0 promethium neptunium samarium 150.4 plutonium europium 152.0 americium gadolinium 157.3 curium terbium 158.9 berkelium dysprosium 162.5 californium holmium 164.9 einsteinium erbium 167.3 fermium thulium 168.9 mendelevium ytterbium 173.1 nobelium lutetium 175.0 lawrencium ± * 0019655306616 *

Board	CAIE
Level	A Level
Subject	Chemistry
Code	`9701`
Year	2024
Session	May/June
Q&A	63 questions

Chemistry 2024 · May/June

Questions & Model Answers 63 Qs

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