9701_m18_qp_42
A paper of Chemistry, 9701
Questions:
9
Year:
2018
Paper:
4
Variant:
2
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1
State how the solubilities of the hydroxides of the Group2 elements vary down the group. Explain the factors that are responsible for this variation. The solubility of Sr(OH)2 is 3.37×10–2 mol dm–3 at 0 °C. Write an expression for the solubility product of Sr(OH)2. Ksp =  Calculate the value of Ksp at 0 °C. Include units in your answer.  Ksp = units =  Metal peroxides contain the –O–O– ion. The peroxides of the Group2 elements, MO2, decompose on heating to produce a single gas and the solid oxide, MO, only. Write an equation for the thermal decomposition of strontiumperoxide, SrO2. Suggest how the temperature at which thermal decomposition of MO2 occurs varies down Group2. Explain your answer. The ethanedioates of the Group2 elements, MC2O4, decompose on heating to produce a mixture of two different gases and the solid oxide, MO, only. Complete the equation for the thermal decomposition of bariumethanedioate. BaC2O4 + +  Describe two observations you would make during the reaction when ethanedioicacid, H2C2O4, is warmed with acidified manganate(ions. 
10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds
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Describe the trend in the reactivity of the halogens Cl 2, Br2 and I2 as oxidising agents. Explain this trend using values of E o (X2 / X–) from the Data Booklet. Write an equation for the reaction between chlorine and water. Use standard electrode potential, E o, data from the Data Booklet to calculate the for the following reaction. Cl 2 + 2OH– Cl – + Cl O– + H2O  = V The [OH–] was increased and the Ecell was measured. Indicate how the value of the Ecell measured would compare to the calculated in by placing one tick () in the table. Ecell becomes less positive than . Ecell stays the same as . Ecell becomes more positive than . Explain your answer.  A half-equation involving bromate(ions, BrO3 –, and bromide ions is shown. BrO3 –+ 3H2O+ 6e– Br –+ 6OH–E o = +0.58 V An alkaline solution of chlorate(, Cl O–, can be used to oxidise bromide ions to bromate(ions. Use the Data Booklet and the half-equation shown to write an equation for this reaction. Calculate the for the reaction in .  = V When a concentrated solution of bromic(acid, HBrO3, is warmed, it decomposes to form bromine, oxygen and water only. Write an equation for this reaction. The use of oxidation numbers may be helpful. 
11. Group 17  →  11.4. The reactions of chlorine
11. Group 17  →  11.2. The chemical properties of the halogen elements and the hydrogen halides
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Hydrogen cyanide, HCN, is a weak acid in aqueous solution. HCNH++ CN–Ka = 6.2 × 10–10 mol dm–3 Calculate the pH of 0.10 mol dm–3 HCN.  pH = Draw a ‘dot-and-cross’ diagram to represent the bonding in the hydrogencyanide molecule. Show the outer shell electrons only.  State the hybridisation of the carbon and nitrogen atoms in hydrogencyanide, and give the H–C–N bond angle. hybridisation of C hybridisation of N H–C–N bond angle  Suggest structures for the organic products A and B in the following reactions. Assume that HCN reacts in a similar way to RCN. HCN H2 + Ni heat with HCl A B  Adding a measured quantity of KCN to a solution of NiCl 2 produces the complex [Ni(CN)2Cl 2]x. Deduce the overall charge, x, on this complex.  x = The complex can exist as two separate isomers with the same geometry around the nickel ion. State the type of isomerism shown by these isomers. If bromide ions are present in the solution, the complex [Ni(CN)2Cl Br]x can form. Assuming that [Ni(CN)2Cl Br]x has the same geometry as [Ni(CN)2Cl 2]x, state the number of isomers of [Ni(CN)2Cl Br]x that could exist, and draw their structures in the box. ● number of isomers of [Ni(CN)2Cl Br]x structures of the isomers of [Ni(CN)2Cl Br]x  An aqueous solution of KCN is gradually added to a solution of NiSO4 until the KCN is in excess. The following series of reactions takes place. NiSO4 more KCN KCN C green precipitate D yellow solution E red solution KCN in excess ● ● The oxidation state of nickel does not change during these reactions. ● ● None of C, D or E contains sulfur. ● ● C contains no potassium. ● ● The K : Ni ratio in D is 2 : 1. ● ● The K : Ni ratio in E is 3 : 1. Use the information to suggest the formulae of C, D and E. C D E  
17. Carbonyl compounds  →  17.1. Aldehydes and ketones
14. Hydrocarbons  →  14.2. Alkenes
12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur
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State what is meant by the term partition coefficient. Ammonia is soluble in both water and organic solvents. An aqueous solution of ammonia is shaken with the immiscible organic solvent trichloromethane. The mixture is left to reach equilibrium. Samples are taken from each layer and titrated with dilute hydrochloric acid. ● ● A 25.0 cm3 sample from the trichloromethane layer requires 13.0 cm3 of 0.100 mol dm–3 HCl to reach the end-point. ● ● A 10.0 cm3 sample from the aqueous layer requires 12.5 cm3 of 0.100 mol dm–3 HCl to reach the end-point. Calculate the partition coefficient, Kpartition, of ammonia between trichloromethane and water.  Kpartition = Butylamine, C4H9NH2, is also soluble in both water and organic solvents. Suggest how the value of Kpartition of butylamine between trichloromethane and water would compare to the value of Kpartition calculated in . Explain your answer. Explain why butylamine is basic. Write an equation to show butylamine reacting as a base. State how the basicity of butanamide, C3H7CONH2, compares to that of butylamine. State a reagent for the conversion of butanamide into butylamine. 
11. Group 17  →  11.4. The reactions of chlorine
12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur
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Complete the electronic configuration of a chromium atom. 1s22s22p63s2 State the two highest oxidation states of chromium commonly seen in its compounds. Six different compounds or complexes, H, J, K, L, M and N, are formed when an excess of aqueous NH3, aqueous NaOH and concentrated aqueous HCl are separately added to separate solutions containing Cu2+or Co2+. solution reagent an excess of NH3an excess of NaOHan excess of concentrated HCl Cu2+H J K Co2+L M N State the colours of the following compounds or complexes. H K M  Write the formulae of the following compounds or complexes. L N  State the appearance of compound J. 
11. Group 17  →  11.1. Physical properties of the Group 17 elements
2. Atoms, molecules and stoichiometry  →  2.3. Formulas
1. Atomic structure  →  1.3. Electrons, energy levels and atomic orbitals
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The apparatus shows a cell which can be used to determine a value of the Avogadro constant, L. X power supply silver electrodes electrolyte Y variable resistor Name component X. Suggest a suitable electrolyte Y. In an experiment, a current of 0.200 A was passed through the cell for 40.0minutes. The mass of the silver cathode increased by 0.500 g. The charge on the electron is –1.60×10–19 C. Calculate the: ● ● number of moles of silver deposited on the cathode ● ● number of coulombs of charge passed ● ● number of electrons passed ● ● number of electrons needed to deposit 1 mol of silver at the cathode.  
2. Atoms, molecules and stoichiometry  →  2.2. The mole and the Avogadro constant
1. Atomic structure  →  1.3. Electrons, energy levels and atomic orbitals
1. Atomic structure  →  1.1. Particles in the atom and atomic radius
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Complete the equations to show the two types of polymerisation. Draw one repeat unit for each polymer. Include any other products. ● addition polymerisation n CH2=CHCH3● condensation polymerisation n HO2CCH2CO2H+ n HOCH2CH2OH Suggest the sign of the entropy changes, ΔS o, for each of the two types of polymerisation. Explain your answers. ● ΔS o for addition polymerisation ● ΔS o for condensation polymerisation  An amide bond forms when a carboxylic acid reacts with an amine. Complete the equation by writing the products in the box. R–CO2H + H2N–R' +  Use your answer to to work out the bonds that are broken and the bonds that are formed during the reaction between a carboxylic acid and an amine. ● ● bonds that are broken ● ● bonds that are formed  Use bond energy values from the Data Booklet to calculate the enthalpy change, ΔH o, when one mole of amide bonds is formed in the reaction in . ΔH o = kJ Amide bonds can also be formed by reacting acyl chlorides with amines. The enthalpy change for this process, ΔH o, is – 6.00 kJ mol–1. Calculate the minimum entropy change, ΔS o, for this reaction to be spontaneous at 298 K. ΔS o = J K–1 mol–1 The repeat unit of the polyamide Kevlar is shown. O O N H N H The monomers of Kevlar, benzene-1,4-dioic acid and 1,4-diaminobenzene, can be synthesised as follows. H3C CH3 HO2C CO2H benzene-1,4-dioic acid reaction 1 O2N NO2 H2N NH2 1,4-diaminobenzene reaction 2 State the reagents and conditions needed for: reaction 1 reaction 2 Kevlar is both strong and rigid. Complete the table to identify two intermolecular forces and the groups involved which are responsible for these properties of Kevlar. intermolecular force groupinvolved  
20. Polymerisation  →  20.1. Addition polymerisation
14. Hydrocarbons  →  14.2. Alkenes
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Cumin is a spice used to flavour food. Two compounds responsible for its flavour are cuminaldehyde and cuminyl alcohol. O cuminaldehyde OH cuminyl alcohol Deduce the number of peaks that would be present in the 13C NMR spectrum of cuminylalcohol. number of peaks Identify two bonds that are responsible for the differences in the infra-red spectra of cuminaldehyde and cuminyl alcohol, and state their absorption ranges. absorption range in the infra-red spectrum / cm–1 bond responsible for the difference cuminaldehyde cuminyl alcohol  Cuminyl alcohol can be synthesised from benzene by the following route. OH cuminyl alcohol benzene step 4 CO2H step 3 step 2 step 1 O Suggest reagents and conditions for steps 1– 4. step 1 step 2 step 3 step 4  Name the mechanism of step2 and state the type of reaction in step4. mechanism of step 2 type of reaction in step 4  
16. Hydroxy compounds  →  16.1. Alcohols
21. Organic synthesis  →  21.1. Organic synthesis
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Two molecules of compoundF react together under suitable conditions to form compoundG. Some information about compounds F and G is given. ● ● The mass spectrum of F has a peak due to the molecular ion at m / e=106, and a peak at m / e=107 with an abundance 8% of the 106 peak. ● ● The mass spectrum of G has a peak due to the molecular ion at m / e=212, and major peaks at m / e=91 and m / e=105. ● ● Both F and G contain oxygen and are neutral compounds which are insoluble in water. ● ● The 1H NMR spectrum of F includes a singlet peak at δ=10.0 due to one proton. ● ● The 1H NMR spectrum of G includes a singlet peak at δ=5.1 due to two protons. ● ● When G is heated with dilute sulfuric acid, benzoic acid, C6H5CO2H, and phenylmethanol, C6H5CH2OH, are produced. Use this information to answer – . Explain how the mass spectrum of F shows that a molecule of F contains seven carbon atoms. Show your working.  Suggest the molecular formula of the fragment of G at m / e=91. Suggest the molecular formulae of F and G. F G  Suggest structures for compounds F and G. F G  On the structures you have drawn in , circle the protons responsible for the 1HNMR peaks at δ=10.0 in F and δ=5.1 in G. State the type of reaction that G undergoes when heated with dilute sulfuricacid. Describe and explain the relative acidities of benzoicacid, phenylmethanol and 4-methylphenol. CO2H benzoic acid CH2OH H3C phenylmethanol OH 4-methylphenol The ester 4-methylphenyl benzoate is used in the manufacture of perfumes. O O 4-methylphenyl benzoate H3C Suggest a two-step route for the synthesis of 4-methylphenyl benzoate from 4-methylphenol and benzoicacid. Include reagents and conditions for each step, and the structure of the intermediate compound.  
22. Analytical techniques  →  22.2. Mass spectrometry
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