9701_w10_qp_42
A paper of Chemistry, 9701
Questions:
9
Year:
2010
Paper:
4
Variant:
2
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1
Write a balanced equation for the reaction of each of the following chlorides with water. phosphorus(chloride silicon(chloride When sulfur is heated under pressure with chlorine, the major product is SCl2 (Cl-S-Cl). S8+ 8Cl28SCl2Use data from the Data Booklet to calculate the enthalpy change, ∆H, for this reaction. The eight sulfur atoms in the S8 molecule are all joined in a single ring by single bonds. ∆H = kJ mol–1 Under suitable conditions, SCl2 reacts with water to produce a yellow precipitate of sulfur and a solution A. Solution A contains a mixture of SO2and compound B. What is the oxidation number of sulfur in SCl2? Work out how the oxidation number of sulfur changes during the reaction of SCl2 with water. Suggest the identity of compound B. Construct an equation for the reaction between SCl2 and water. What would you observe when each of the following reagents is added to separate samples of solution A? AgNO3K2Cr2O7
11. Group 17  →  11.4. The reactions of chlorine
9. The Periodic Table: chemical periodicity  →  9.2. Periodicity of chemical properties of the elements in Period 3
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For Examiner’s Use What is meant by the term ligand in the context of transition element chemistry? Decide which of the following species could be a ligand, and which could not be. Place a tick (✓) in the appropriate column. species can be a ligand cannot be a ligand OH– NH4 + CH3OH CH3NH2 Read the following description of some reactions of copper(sulfate, and answer the questions that follow. When 0.1 mol of white anhydrous CuSO4 is dissolved in liquid ammonia at –33 °C, a deep blue solution C results. When 0.2 mol of solid NaOH is added to solution C, and the ammonia solvent allowed to evaporate, a solid residue is obtained. Heating this residue to 200 °C produces a dark coloured mixture of two solids. When water is added to this mixture, a black solid D and a colourless solution E are formed. Neither D nor E contains nitrogen. Adding BaCl2to solution E produces a white precipitate F. Solid D dissolves in HNO3on warming, without evolution of gas, to give a pale blue solution containing Cu(NO3)2. Suggest the formula of the compound contained in each of the following. solution C solid D solution E white precipitate F Name the type of reaction that is occurring when D reacts with HNO3. For Examiner’s Use Describe what you would observe when a solid sample of anhydrous Cu(NO3)2 is strongly heated. Write an equation for this reaction.
11. Group 17  →  11.3. Some reactions of the halide ions
2. Atoms, molecules and stoichiometry  →  2.3. Formulas
12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur
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For Examiner’s Use The electrolytic purification of copper can be carried out in an apparatus similar to the one shown below. impure copper anode anode ‘sludge’ pure copper cathode CuSO4 The impure copper anode contains small quantities of metallic nickel, zinc and silver, together with inert oxides and carbon resulting from the initial reduction of the copper ore with coke. The copper goes into solution at the anode, but the silver remains as the metal and falls to the bottom as part of the anode ‘sludge’. The zinc also dissolves. Write a half equation including state symbols for the reaction of copper at the anode. Use data from the Data Booklet to explain why silver remains as the metal. Use data from the Data Booklet to predict what happens to the nickel at the anode. Write a half equation including state symbols for the main reaction at the cathode. Use data from the Data Booklet to explain why zinc is not deposited on the cathode. Suggest why the blue colour of the electrolyte slowly fades as the electrolysis proceeds. For Examiner’s Use Most of the current passed through the cell is used to dissolve the copper at the anode and precipitate pure copper onto the cathode. However, a small proportion of it is ‘wasted’ in dissolving the impurities at the anode which then remain in solution. When a current of 20.0 A was passed through the cell for 10.0 hours, it was found that 225 g of pure copper was deposited on the cathode. Calculate the following, using appropriate data from the Data Booklet. • number of moles of copper produced at the cathode • number of moles of electrons needed to produce this copper • number of moles of electrons that passed through the cell Hence calculate the percentage of the current through the cell that has been ‘wasted’ in dissolving the impurities at the anode. Nickel often occurs in ores along with iron. After the initial reduction of the ore with coke, a nickel-iron alloy is formed. Use data from the Data Booklet to explain why nickel can be purified by a similar electrolysis technique to that used for copper, using an impure nickel anode, a pure nickel cathode, and nickel sulfate as the electrolyte. Explain what would happen to the iron during this process.
11. Group 17  →  11.4. The reactions of chlorine
11. Group 17  →  11.3. Some reactions of the halide ions
6. Electrochemistry  →  6.1. Redox processes: electron transfer and changes in oxidation number (oxidation state)
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For Examiner’s Use The most typical oxides of tin and lead are SnO, SnO2, PbO and PbO2. The following two generalisations can be made about the oxides of the elements in Group IV. • As the metallic character of the elements increases down the Group, the oxides become more basic. • The oxides of the elements in their higher oxidation states are more acidic than the oxides of the elements in their lower oxidation states. Use these generalisations to suggest which of the above oxides of tin or lead is most likely to react with each of the following reagents. In each case write a balanced equation for the reaction. with NaOHformula of oxide equation with HClformula of oxide equation ‘Red lead’ is used as a pigment, and as a metal primer paint to prevent the corrosion of steel. It is an oxide of lead that contains 9.30% oxygen by mass. Calculate to 3 significant figures the number of moles of oxygen and lead contained in a 100.0 g sample of red lead. Hence calculate its empirical formula. empirical formula: For Examiner’s Use Lead(chloride is slightly soluble in water. PbCl2Pb2++ 2Cl–Ksp = 2.0 × 10–5 Write an expression for the solubility product, Ksp for lead(chloride and state its units. Ksp = units Calculate [Pb2+] in a saturated solution of PbCl2. An excess of PbCl2is stirred with 0.50 mol dm–3 NaCl until equilibrium has been established. The excess PbCl2is then filtered off. Assuming [Cl–] remains at 0.50 mol dm–3 throughout, calculate the [Pb2+] in the remaining solution. Suggest an explanation for the difference between this value and the value that you calculated in .
10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds
9. The Periodic Table: chemical periodicity  →  9.2. Periodicity of chemical properties of the elements in Period 3
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For Examiner’s Use Compound G can be synthesised from benzene by the route shown below. H J (C6H5N2Cl) G HNO3 + H2SO4 NH2 step 2 step 4 step 5 step 3 55 °C OH O O CH3 Name the functional group formed in step 5. Draw the structures of the intermediates H and J in the boxes above. Suggest reagents and conditions for the following. step 2 step 3 step 4 step 5 For Examiner’s Use In a reaction discovered just over 100 years ago by the German chemist Karl Fries, compound G is converted into compound K when it is heated with AlCl3. Compound K is a structural isomer of G. K (C8H8O2) G AlCl3 O O CH3 Compound K is a 1,4-disubstituted benzene derivative. It is insoluble in water, but dissolves in NaOH. It gives a white precipitate with Br2, and a yellow precipitate with alkaline aqueous iodine. What is meant by the term structural isomerism? Use the information given above to name two functional groups in compound K. Suggest the structural formula of K, and draw it in the box above. Suggest structures for the aromatic products of the following reactions. Br2 NaOH I2 + NaOH K
21. Organic synthesis  →  21.1. Organic synthesis
13. An introduction to AS Level organic chemistry  →  13.1. Formulas, functional groups and the naming of organic compounds
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For Examiner’s Use Menthone, C10H18O, is a cyclic ketone that occurs in oil of peppermint. O menthone Use asterisks (*) on the formula above to identify any chiral centres in the molecule of menthone. Menthone can be reduced to menthol, which can be dehydrated to a mixture of two alkenes, L and M. O menthone L M HO menthol + step 1 step 2 Suggest reagents for step 1, step 2. Suggest structures for L and M and draw them in the boxes above. For Examiner’s Use When heated with concentrated, acidified KMnO4, one of the two alkenes L or M produces the dicarboxylic acid N. CO2H CO2H N Give the letter of the alkene that produced N by this reaction. Suggest the structure of the product, P, of the reaction between the other alkene you have drawn and hot concentrated acidified KMnO4. P Suggest one chemical test that would enable you to distinguish between N and P. reagentobservation Chlorocyclohexane can be prepared by bubbling HClthrough a solution of cyclohexene. Cl + HCl Suggest the mechanism of this 2-stage reaction by means of a diagram. Include all whole or partial charges, and represent the movements of electron pairs by curly arrows.
16. Hydroxy compounds  →  16.1. Alcohols
14. Hydrocarbons  →  14.2. Alkenes
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Whilst small amounts of some metal ions are vital in the human body, others can be highly toxic. Hg2+ ions are toxic for a number of reasons. Hg2+ ions can react with the R–S–S–R group, which is found in proteins. R–S–S–R + 2Hg2+ + H2 2 R–S–Hg+ + 2H+ reaction 1 What is the name of the R–S–S–R group in proteins? Which level of protein structure will be affected by reaction 1? Why will this affect the activity of an enzyme? Ag+ ions can combine with free –COOH groups in the side chains of the amino acid residues in proteins to form partially covalent silver carboxylates. RCOOH + Ag+ RCOOAg + H+ reaction 2 What type of behaviour is the –COOH group showing in reaction 2? What types of R group interactions will be affected by reaction 2? Explain your answer. For Examiner’s Use By contrast, iron is an extremely important metal used in haemoglobin to transport oxygen molecules from the lungs to muscle cells and to carry carbon dioxide in the reverse direction. One haemoglobin molecule contains four haem groups, each of which contains one iron atom. In the haem group four nitrogen atoms are in the same plane as the iron atom. The oxygen molecule is attached above this plane, and the iron atom is joined to a protein chain below this plane. H C Fe C H haem CH2 CH3 CH2 CH3 H3C H3C HOOC COOH N N N HC CH N How many oxygen atoms could one haemoglobin molecule transport? By what type of bonding is the oxygen molecule likely to be held to the iron atom in haem? What is the geometry of bonding around the iron atom?
11. Group 17  →  11.3. Some reactions of the halide 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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For Examiner’s Use NMR spectroscopy and X-ray crystallography are two techniques that use electromagnetic radiation to look at the structures of large molecules. For each technique state the sub-atomic particle involved, and explain how this particle interacts with the radiation. NMR X-ray The two NMR spectra 1 and 2 were obtained before and after an alcohol, Y, was oxidised to give compound Z. The numbers of hydrogen atoms responsible for each peak have not been shown. All the peaks have been shown. δ / ppm δ / ppm For Examiner’s Use State which spectrum, 1 or 2, was produced by the alcohol, giving a reason for your answer. spectrum reason The mass spectrum of Y showed an M : M + 1 peak ratio of 17.6:0.6. Use this and other information in the question to suggest the identities of both Y and Z. Draw a displayed formula for Y in the box provided Y is Explain why the NMR spectrum of Z only shows one peak.
22. Analytical techniques  →  22.2. Mass spectrometry
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For Examiner’s Use A possible source of energy for the road vehicles of the future is hydrogen. One of the problems still to be solved is the storage of the hydrogen in the vehicle. A conventional tank holding liquid hydrogen would have to be pressurised and refrigerated. In a crash, this type of tank could break resulting in the rapid release of hydrogen and an explosion. One alternative is to use a fuel tank packed with carbon nanotubes. The hydrogen in the tank would be adsorbed onto the surface of the nanotubes at a pressure of no more than a few atmospheres. What is the approximate width of a carbon nanotube? In what structural form is the carbon in a nanotube? What forces could be responsible for holding the hydrogen on the surface of the nanotubes? Explain your answer. The hydrogen atoms in a fuel tank packed with nanotubes are closer together than in liquid hydrogen. Suggest one advantage of this. When a nanotube-packed fuel tank is full of hydrogen there is a steady pressure of hydrogen in the tank. While hydrogen gas is being removed from the fuel tank to power the car, the pressure in the fuel tank drops very little for some time. State Le Chatelier’s principle, and suggest how it explains this observation.
11. Group 17  →  11.2. The chemical properties of the halogen elements and the hydrogen halides
3. Chemical bonding  →  3.6. Intermolecular forces, electronegativity and bond properties
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