9701_w16_qp_43
A paper of Chemistry, 9701
Questions:
7
Year:
2016
Paper:
4
Variant:
3
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1
Copper is a transition element and has atomic number 29. Complete the electronic configuration for the copper atom and the copper ion in the +2 oxidation state. • copper atom [Ar] • copper ion in the +2 oxidation state [Ar] The following equilibrium exists between two complex ions of copper in the +2 oxidation state. [Cu(H2O)6]2+ + 4Cl – [CuCl 4]2– + 6H2O Name the type of reaction occurring here. State the colours of these two complex ions. [Cu(H2O)6]2+ [CuCl 4]2– State the shape of the [CuCl 4]2– ion. Write the expression for the stability constant, Kstab, for this equilibrium. Kstab = Copper also forms the complex ions [Cu(NH3)2(H2O)4]2+ and [Cu(H2O)4]2+ where en is the bidentate ligand ethane-1,2-diamine, H2NCH2CH2NH2. [Cu(H2O)6]2+ + 2NH3 [Cu(NH3)2(H2O)4]2+ + 2H2O equilibrium 1 [Cu(H2O)6]2+ + en [Cu(H2O)4]2+ + 2H2O equilibrium 2 What is meant by the term bidentate ligand? The table lists the values of stability constants for these two complexes. stability constant, Kstab [Cu(NH3)2(H2O)4]2+ 7.94 × 107 [Cu(H2O)4]2+ 3.98 × 1010 What do these Kstab values tell us about the relative positions of equilibria 1 and 2? Nickel forms the complex ion [Ni3]2+ in which it is surrounded octahedrally by six nitrogen atoms. Name the type of stereoisomerism displayed by [Ni3]2+. Draw three-dimensional diagrams to show the two stereoisomers of [Ni3]2+. Ethane-1,2-diamine is a useful reagent in organic chemistry. Explain how the amino groups in ethane-1,2-diamine allow the molecule to act as a Brønsted-Lowry base. Write an equation for the reaction of ethane-1,2-diamine with an excess of hydrochloricacid. Under certain conditions, ethane-1,2-diamine reacts with ethanedioic acid, HO2CCO2H, to form the polymer Z. Draw the structure of this polymer, Z, showing two repeat units. Name the type of reaction occurring during this polymerisation. Polymer Z is an example of a biodegradable polymer. Name a polymer that is non-biodegradable.
2. Atoms, molecules and stoichiometry  →  2.3. Formulas
7. Equilibria  →  7.1. Chemical equilibria: reversible reactions, dynamic equilibrium
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When copper(carbonate is heated strongly, it decomposes in a similar way to Group2 carbonates. Predict what would be observed when anhydrous copper(carbonate is heated. Describe and explain how the thermal stability of the Group 2 carbonates varies down the group. Calcium cyanamide, CaCN2, can be used as a fertiliser. Complete the ‘dot-and-cross’ diagram for the cyanamide ion, CN2 2–. Use the following key for the electrons. • electrons from carbon × electrons from nitrogen □ added electronresponsible for the overall negative charge N C N 2– CaCN2 decomposes readily on contact with water forming an insoluble white solid and ammonia only. Suggest an equation for this reaction.
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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The spontaneity of a chemical reaction depends on the standard Gibbs free energy change, ∆G o. This is related to the standard enthalpy and entropy changes by the equation shown. ∆G o = ∆H o – T∆S o State and explain whether the following processes will lead to an increase or decrease in entropy. the reaction of magnesium with hydrochloric acid entropy change explanation solid potassium chloride dissolving in water entropy change explanation steam condensing to water entropy change explanation Magnesium carbonate can be decomposed. MgCO3→ MgO+ CO2∆H o = +117 kJ mol–1 Standard entropies are shown in the table. substance MgCO3MgOCO2S o / J mol–1 K–1 +65.7 +26.9 +214 Calculate ∆G o for this reaction at 298 K. Include a relevant sign and give your answer to three significant figures. ∆G o = kJ mol–1 Explain, with reference to ∆G o, why this reaction becomes more feasible at higher temperatures. On heating, sodium hydrogencarbonate decomposes into sodium carbonate as shown. 2NaHCO3→ Na2CO3+ CO2+ H2O∆H o = +130 kJ mol–1 ∆S o = +316 J mol–1 K–1 Calculate the minimum temperature at which this reaction becomes spontaneous . Show your working. temperature = K The solubility of Group 2 sulfates decreases down the Group. Explain this trend.
8. Reaction kinetics  →  8.2. Effect of temperature on reaction rates and the concept of activation energy
5. Chemical energetics  →  5.1. Enthalpy change, \(\Delta H\)
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Cobalt is a transition element that forms complex ions with oxidation states +2 and +3. Explain what is meant by the term transition element. The following scheme shows some reactions of [Co(H2O)6]2+. precipitate A solution of C solution of B [Co(H2O)6]2+ OH–excess Cl –excess NH3State the formula of each of the following. A B C State the colour of the following solutions. [Co(H2O)6]2+ solution of B solution of C Define the term standard electrode potential. An electrochemical cell was set up to measure the standard electrode potential, , of a cell made of a Co2+ / Co half-cell and a Fe3+ / Fe2+ half-cell. Complete the table with the substance used to make the electrode in each of these half-cells. half-cell electrode Co2+ / Co Fe3+ / Fe2+ Write the equation for the overall cell reaction. Use the Data Booklet to calculate the . = V The electrochemical cell in was set up again but this time the concentration of Co2+was 0.050 mol dm–3. The Nernst equation can be used to calculate the value of an electrode potential at different concentrations. E = E o + (0.059 / z) log [Co2+] Nernst equation Use the Data Booklet and the Nernst equation to calculate the value of E for the Co2+ / Co half-cell in this experiment. E for Co2+ / Co = V Suggest how this change will affect the overall cell potential, Ecell, compared to in . Circle your answer. less positive no change more positive Iron(ions can oxidise vanadium metal. Construct an equation for the reaction of an excess of iron(ions with vanadium metal. Use of the Data Booklet will be helpful.
2. Atoms, molecules and stoichiometry  →  2.3. Formulas
11. Group 17  →  11.4. The reactions of chlorine
1. Atomic structure  →  1.3. Electrons, energy levels and atomic orbitals
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Compound F contains the elements carbon, hydrogen and oxygen only. All carbon-carbon bonds in F are single bonds. The structure of F was analysed by mass spectrometry and infra-red and NMRspectroscopy. The mass spectrum shows that the m / e value for the M peak is 90. The ratio of the heights of the M and M+1 peaks is 22.1 : 0.7. Use the ratio of the heights of the M and M+1 peaks to calculate the number of carbon atoms in a molecule of F. number of carbon atoms = Suggest the molecular formula of F. molecular formula = C H O The infra-red spectrum of F was obtained. Use the Data Booklet and your knowledge of infra-red spectroscopy to identify the type of bond and the functional group responsible for these three absorptions. absorption / cm–1 appearance of the peak type of bond functional group broad and strong very broad and strong strong F was dissolved in deuterated trichloromethane, CDCl 3, and the proton NMR spectrum of this solution obtained. δ / ppm Use the Data Booklet and your answer to to complete Table1 for the proton NMR spectrum of F. The actual chemical shifts for the four absorptions in F have been added for you. Table 1 δ / ppm type of proton relative peak area 1.4 3.9 4.7 12.9 Describe and explain the splitting pattern for the absorption at δ = 1.4. F was dissolved in D2O and the proton NMR spectrum of this new solution obtained. Two of the absorptions in Table1 were not present in this spectrum. Which absorptions were not present?  and Suggest the structure of F. Molecules of cycloheptadiene, C7H10, consist of a seven-membered ring with two carbon-carbon double bonds. Complete the skeletal formulae of two isomers of cycloheptadiene. P Q The isomers P and Q were analysed using carbon-13 NMR spectroscopy. Predict the number of peaks that will be seen in the carbon-13 NMR spectra of P and Q. isomer number of peaks P Q
22. Analytical techniques  →  22.2. Mass spectrometry
13. An introduction to AS Level organic chemistry  →  13.1. Formulas, functional groups and the naming of organic compounds
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Ibuprofen and paracetamol are pain-relief drugs. ibuprofen paracetamol O OH N H O OH Ibuprofen and paracetamol both contain the aryl functional group. Name the other functional groups present in each molecule. ibuprofen paracetamol Ibuprofen contains a chiral centre and shows stereoisomerism. State what is meant by the term chiral centre. Draw the two stereoisomers of ibuprofen. C C Draw the structures of the organic products when ibuprofen and paracetamol react separately with LiAl H4. product with ibuprofen product with paracetamol A student carried out some reactions with solutions of ibuprofen and paracetamol using reagents D and E and the following results were obtained. ( means a reaction took place.) reagent ibuprofen paracetamol D   E   Suggest a possible identity for each reagent D and E. D E Give the structure of the organic product formed when reagent D reacted with ibuprofen. product with ibuprofen Give the structure of the organic product formed when reagent E reacted with paracetamol. product with paracetamol One of the steps in the manufacture of ibuprofen is shown. X Y CH3COCl Al Cl 3 O Write an equation for the reaction between CH3COCl and Al Cl 3. Complete the mechanism for the conversion of X into Y. Include all necessary curly arrows, any relevant dipoles and charges. X Name the mechanism in .
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
13. An introduction to AS Level organic chemistry  →  13.2. Characteristic organic reactions
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Sodium chlorate(, NaCl O, is the active ingredient in commercial bleach. The concentration of chlorate(ions was determined by titration. • 10.0 cm3 of a bleach solution was diluted to 250 cm3 in a volumetric flask using distilled water. • Dilute sulfuric acid and an excess of potassium iodide solution were added to a 25.0 cm3 portion of this solution to liberate iodine. • The resulting solution required 20.80 cm3 of 0.100 mol dm–3 aqueous sodium thiosulfate solution to react with the iodine produced. The titration reactions are shown. Cl O– + 2I– + 2H+ → I2 + Cl – + H2O I2 + 2S2O3 2– → 2I– + S4O6 2– Calculate the concentration, in mol dm–3, of Cl O– ions in the bleach solution. concentration of Cl O– = mol dm–3 An indicator was used in the thiosulfate-iodine titration. Name a suitable indicator for this titration. State the expected colour change you would observe at the end-point in this titration. from to State when in the procedure you would add the indicator. The concentration of chlorate(ions can also be determined by adding an excess of hydrogenperoxide to the sample of bleach and measuring the volume of oxygen gas produced. H2O2 + NaCl O → NaCl + O2 + H2O water oxygen gas 100 cm3 measuring cylinder hydrogen peroxide 5.0 cm3 bleach When an excess of aqueous hydrogen peroxide was added to 5.0 cm3 of a different bleach solution, 82 cm3 of oxygen was produced at room temperature and pressure. Calculate the concentration of Cl O– ions in this bleach solution. concentration of Cl O– = mol dm–3 Trichlorocyanuric acid, C3Cl 3N3O3, acts as a chlorine buffer and disinfectant for swimming pools. It reacts with water to give chloric(acid, HCl O. C3Cl 3N3O3 + 3H2O C3H3N3O3 + 3HCl O Write the expression for Kc for this equilibrium. Kc = In outdoor swimming pools, the HCl O is decomposed by sunlight. The decomposition of HCl O is a redox reaction which forms a gas that relights a glowing splint. Describe and explain the effect of the decomposition of HCl O on the equilibrium in . State the effect on Kc. effect on Kc The decomposition of HCl O is a redox reaction. Suggest an equation for this reaction. The buffer solution in blood is a mixture of carbonic acid, H2CO3, and hydrogencarbonate ions, HCO3 –. Healthy blood has a pH of 7.40. H2CO3 + H2O HCO3 – + H3O+ Ka = 7.94 × 10–7 mol dm–3 Explain how this buffer system acts to control the blood pH. Include equations in your answer. A patient’s blood has a [HCO3 –] : [H2CO3] ratio of 9.5 : 1. Calculate the pH of the patient’s blood. pH =
11. Group 17  →  11.4. The reactions of chlorine
11. Group 17  →  11.1. Physical properties of the Group 17 elements
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