9701_w14_qp_43
A paper of Chemistry, 9701
Questions:
9
Year:
2014
Paper:
4
Variant:
3
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1
Chlorine exists naturally as a mixture of two isotopes, 35Cl and 37Cl , in the abundance ratio of 3 : 1. The mass spectrum of chlorine consists of fi ve peaks. Suggest the mass numbers for these fi ve peaks and the identities of the species responsible. mass number formula of species Predict the ratios of the abundances of the three species with the highest mass numbers. ratio of abundances = Strontium chloride, SrCl 2, can be used to produce a red colour in fi reworks. Draw the ‘dot-and-cross’ diagram for strontium chloride. Show outer shell electrons only. Use the following data, together with relevant data from the Data Booklet, to calculate a value for the lattice energy of strontium chloride. You may fi nd it helpful to construct a Born-Haber cycle. electron affi nity per mole of chlorine atoms –349 kJ mol–1 standard enthalpy of atomisation of Sr+164 kJ mol–1 standard enthalpy of formation of SrCl 2–830 kJ mol–1 lattice energy = kJ mol–1 Strontium nitrate, Sr(NO3)2, can also be used to produce a red colour in fi reworks. Strontium nitrate can easily be prepared from strontium carbonate, SrCO3. Suggest an equation for this preparation of strontium nitrate. Write an equation for the reaction that occurs when strontium nitrate is heated. Describe and explain the trend in the thermal stabilities of the nitrates of the Group II elements.
9. The Periodic Table: chemical periodicity  →  9.2. Periodicity of chemical properties of the elements in Period 3
11. Group 17  →  11.2. The chemical properties of the halogen elements and the hydrogen halides
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Bromate(ions, BrO3 –, react with bromide ions in the presence of acid to produce bromine. Write an ionic equation for this reaction. The initial rate of this reaction was measured, starting with different concentrations of the three reactants. The following results were obtained. experiment number [BrO3 –] / mol dm–3 [Br –] / mol dm–3 [H+] / mol dm–3 initial rate / mol dm–3 s–1 0.040 0.020 0.50 2.64 × 10–4 0.040 0.020 1.00 1.06 × 10–3 0.040 0.080 0.50 1.06 × 10–3 0.080 0.020 0.50 5.21 × 10–4 Use the data in the table to determine the order with respect to each reactant. Show your reasoning. Write the rate equation for this reaction. Use the results of experiment 1 to calculate the rate constant, k, for this reaction. Include the units of k. rate constant, k = units
8. Reaction kinetics  →  8.1. Rate of reaction
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Transition elements have characteristic properties due to their partially-fi lled d orbitals. Which two elements in the fi rst row of the d-block have only one electron in the 4s orbital of their neutral atoms? The d orbitals in an isolated transition metal atom or ion are described as being degenerate. What is meant by the term degenerate? Sketches of the shapes of the atomic orbitals from the d subshell are shown. In an octahedral complex, the d orbitals are split into two groups at different energy levels. On the diagram below, write an ‘H’ in the box under each of the orbitals at the higher energy level. z y x z y x z y x y x z z y x The following scheme shows some reactions of Cu2+. Cu2+pale blue precipitate A solution of B solution of C [CuCl 2]–concentrated HCl excess NH3heat with Cua few drops of NH3Suggest the formula of each of the following. A B C State the colour of the following solutions. solution of B solution of C Name the type of reaction that occurs when C is heated with copper. Deduce the role of the copper metal in this reaction. When the solution containing the complex [CuCl 2]– is poured into water, a precipitate of CuCl is formed. CuCl is white because it does not absorb visible light. Explain why CuCl does not absorb visible light. The complex ion [Cr(H2O)6]3+ is coloured because it absorbs visible light. The absorption spectrum for [Cr(H2O)6]3+ is shown below. absorbance wavelength / nm violet red Suggest the colour of this complex ion. Explain your answer.
1. Atomic structure  →  1.3. Electrons, energy levels and atomic orbitals
11. Group 17  →  11.1. Physical properties of the Group 17 elements
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4
The following circuits were set up using aqueous hydrochloric and aqueous ethanoic acids as electrolytes. Assume that the two circuits were identical apart from the electrolyte. graphite electrodes 1 mol dm–3 HCl bulb switch graphite electrodes 1 mol dm–3 CH3CO2Hbulb switch When the switches were closed, bulb 1 was brighter than bulb 2. Explain why. State what is meant by a buffer solution. Outline how a buffer solution can be prepared from ethanoic acid and a named base. Amino acids such as alanine, CH3CH(NH2)CO2H, can act as a buffer solution. Construct two equations to illustrate this. equation 1 equation 2 Tartaric acid is present in many plants. O O OH OH OH HO tartaric acid Tartaric acid has two dissociation constants, K1 and K2, for which the pKa values are 2.99 and 4.40. Suggest equations showing the two dissociations that give rise to these pKa values. pKa 2.99 pKa 4.40 One stereoisomer of tartaric acid is shown. CO2H HO2C OH HO H H Complete the diagrams showing two other stereoisomers of tartaric acid. CO2H CO2H
7. Equilibria  →  7.2. Brønsted–Lowry theory of acids and bases
18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids
11. Group 17  →  11.4. The reactions of chlorine
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5
L-DOPA is used in the treatment of Parkinson's disease. It can be prepared from vanillin. HO NH2 CO2H HO HO H CH3O O L-DOPA vanillin L-DOPA and vanillin each contain an aromatic benzene ring. Describe, with the aid of a diagram, the bonding and shape of a molecule of benzene, C6H6. A student carried out some reactions with samples of L-DOPA and vanillin using reagents X, Y and Z. ● Reagent X reacted with L-DOPA and with vanillin. ● Reagent Y reacted with L-DOPA but not with vanillin. ● Reagent Z reacted with vanillin but not with L-DOPA. Assume that the CH3O– group in vanillin does not react. Suggest possible identities of reagents X, Y and Z and give the structures of the organic products that were formed. Reagent X product with L-DOPA product with vanillin Reagent Y product with L-DOPA Reagent Z product with vanillin
17. Carbonyl compounds  →  17.1. Aldehydes and ketones
14. Hydrocarbons  →  14.2. Alkenes
21. Organic synthesis  →  21.1. Organic synthesis
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Methoxetamine is a derivative of the pharmaceutical drug, ketamine. O OCH3 NHCH2CH3 methoxetamine What is the molecular formula of methoxetamine? On the diagram above, circle any chiral centres that are present in methoxetamine. Name two functional groups in methoxetamine, in addition to the aryl group. In the table, complete the structure of each of the compounds formed when methoxetamine is reacted with the following reagents. State the type of reaction in each case. reagent structure of product type of reaction LiAl H4 OCH3 HCl OCH3 CH3COCl OCH3
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  →  13.4. Isomerism: structural isomerism and stereoisomerism
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7
Explain what is meant by the term partition coeffi cient. When 20 cm3 of ethoxyethane were shaken with 75 cm3 of an aqueous solution containing 5.00 g of an organic compound, J, in 75 cm3 of water, it was found that 2.14 g of J were extracted into the ethoxyethane. Calculate the partition coeffi cient, Kpartition, of J between ethoxyethane and water. Kpartition = In a new experiment ● 10 cm3 of ethoxyethane were shaken with 75 cm3 of an aqueous solution containing 5.00 g of J and the layers were separated. ● The aqueous layer was shaken with a second 10 cm3 portion of ethoxyethane and the layers were separated. ● The two organic layers were combined. Use the value of Kpartition you calculated in to calculate the total mass of J extracted by this procedure. total mass of J = Paper chromatography and gas / liquid chromatography both rely on the partition of compounds between mobile and stationary phases. Identify the mobile phase in paper chromatography. Suggest what type of liquid is used for the stationary phase in gas / liquid chromatography. Both these techniques can be used to separate mixtures. State what you would measure in order to distinguish between the components in the mixture in 1. paper chromatography, 2. gas / liquid chromatography. A mixture of three compounds was analysed by paper chromatography using a non-polar solvent. The resulting chromatogram is shown. mixture solvent front Identify which compound is responsible for each spot. compound spot CO2H CH2OH CO2H CO2H
22. Analytical techniques  →  22.2. Mass spectrometry
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Analysis of a sample of DNA showed that 33% of the nitrogenous bases present was guanine. Calculate the percentages of the other bases in this sample of DNA. adenine % cytosine % thymine % Many drug molecules are chiral, but are often produced as a mixture of optical isomers. Suggest why a larger mass of the mixture is required than of a single optical isomer. Suggest a problem that might arise as a result of taking a mixture of optical isomers. There are four structural isomers with the molecular formula C5H10O that are aldehydes. Draw the structures of these aldehydes. P Q R S The NMR spectrum of one of these isomers contains four absorptions. Which isomer P, Q, R or S gives this spectrum? isomer Predict the number of absorptions that would be given by each of the other three isomers. isomer letter (P, Q, R or S) number of absorptions
13. An introduction to AS Level organic chemistry  →  13.4. Isomerism: structural isomerism and stereoisomerism
13. An introduction to AS Level organic chemistry  →  13.1. Formulas, functional groups and the naming of organic compounds
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9
Polymers can be formed by addition or condensation polymerisation. Complete the table. polymer method of polymerisation nylon PVC Terylene Nomex is a polymeric material with excellent fl ame-resistant properties. It contains a polymer made from the two monomers shown below. NH2 H2N CO2H HO2C Draw the structure of the polymer showing two repeat units. The linkages between monomer units should be shown fully displayed. Proteins are natural polymers. Explain what is meant by the primary structure of a protein. Use the diagram to show an example of how the α-helix secondary structure in proteins is stabilised. The tertiary structure of a protein is destroyed during the process of denaturation. Explain how this can occur by the addition of alkali, the addition of Hg2+ ions, heating to 70 °C.
20. Polymerisation  →  20.1. Addition polymerisation
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