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GCE JUN 2010 : (AS 1) Basic Concepts in Physical and Inorganic Chemistry - Revised

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Sp N ec e i w ca tio n Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education 2010 Chemistry assessing Basic Concepts in Physical and Inorganic Chemistry AC111 Assessment Unit AS 1 [AC111] MONDAY 7 JUNE, MORNING TIME 1 hour 30 minutes. INSTRUCTIONS TO CANDIDATES Write your Centre Number and Candidate Number in the spaces provided at the top of this page. Answer all fifteen questions. Answer all ten questions in Section A. Record your answers by marking the appropriate letter on the answer sheet provided. Use only the spaces numbered 1 to 10. Keep in sequence when answering. Answer all five questions in Section B. Write your answers in the spaces provided in this question paper. For Examiner s use only Question Number Marks Section A 1 10 INFORMATION FOR CANDIDATES The total mark for this paper is 100. Quality of written communication will be assessed in question 13(d). In Section A all questions carry equal marks, i.e. two marks for each question. In Section B the figures in brackets printed down the right-hand side of pages indicate the marks awarded to each question or part question. A Periodic Table of Elements (including some data) is provided. 5631.02 R Section B 11 12 13 14 15 Total Marks Section A For each of the following questions only one of the lettered responses (A D) is correct. Select the correct response in each case and mark its code letter by connecting the dots as illustrated on the answer sheet. 1 Which one of the following represents the ground state electronic configuration of a nitrogen atom? A B C D 2p 2s 1s 2 When burned in a plentiful supply of oxygen, methane produces carbon dioxide and water. CH4 + 2O2 CO2 + 2H2O What is the number of molecules of oxygen required for the complete combustion of 1.6 g of methane? A 6.0 1022 B 1.2 1023 C 6.0 1023 D 1.2 1024 3 In which one of the following molecules are the bond angles closest to 107 ? A BF3 B CH4 C H2O D NH3 5631.02 R 2 [Turn over 4 Which one of the following gives the correct flame colour for the named compound? A B C D 5 barium chloride copper(II) chloride potassium chloride sodium chloride red blue-green yellow/orange lilac An element was analysed using a mass spectrometer. The spectrum showed that there were four isotopes. The relative isotopic masses and relative abundances are given below. Relative isotopic mass Relative abundance 50 2 52 35 53 4 54 1 The relative atomic mass of this element is A B C D 6 52.00. 52.05. 52.25. 52.50. Which one of the following is produced when concentrated sulphuric acid reacts with solid sodium chloride? A B C D 5631.02 R chlorine hydrogen chloride hydrogen sulphide sulphur dioxide 3 [Turn over 7 Titanium is extracted in a two-stage process. The first stage involves the conversion of titanium(IV) oxide to titanium(IV) chloride. In the second stage, the titanium(IV) chloride is reduced using magnesium. TiO2 + C + 2Cl2 TiCl4 + CO2 TiCl4 + 2Mg Ti + 2MgCl2 What is the maximum mass of titanium which can be obtained when 8.0 kg of titanium(IV) oxide is converted to titanium(IV) chloride and then reduced using 7.2 kg of magnesium? A B C D 8 2.4 kg 4.8 kg 9.6 kg 14.4 kg Which one of the following electron transitions is responsible for the lowest frequency line in the visible region of the emission spectrum of atomic hydrogen? n=4 C n=3 B D n=2 A n=1 5631.02 R 4 [Turn over 9 Which one of the letters represents the first ionisation energy of an alkali metal? C B first ionisation energy /kJ mol 1 A D atomic number 10 The ionisation energy of hydrogen is 1312 kJ mol 1. Use this value to calculate the frequency at convergence in the hydrogen emission spectrum. A 2.179 10 21 Hz B 1.312 106 Hz C 3.287 1015 Hz D 1.979 1036 Hz 5631.02 R 5 [Turn over Section B Examiner Only Marks Remark Answer all five questions in this section. 11 Aluminium is the most abundant metal in the Earth s crust. It is used in electrical cables and is present in high strength alloys. (a) All atoms of aluminium have a mass number of 27. How many neutrons are present in the nucleus of these atoms? _____________________________________________________ [1] (b) (i) Write the equation, including state symbols, which represents the first ionisation energy of aluminium. _________________________________________________ [2] (ii) Explain why the first ionisation energy of boron has a larger value than the first ionisation energy of aluminium. ___________________________________________________ ___________________________________________________ _________________________________________________ [2] (iii) Explain why the first ionisation energy of magnesium has a larger value than the first ionisation energy of aluminium. ___________________________________________________ ___________________________________________________ _________________________________________________ [2] (iv) Give the ground state electronic configuration of the Al4+ ion. _________________________________________________ [1] 5631.02 R 6 [Turn over (v) Sketch a graph to show the successive ionisation energies of aluminium. Examiner Only Remark log (ionisation energy) Marks 1 2 3 4 5 6 7 8 9 10 11 12 13 number of electrons removed 5631.02 R 7 [2] [Turn over 12 Fluorine is the most reactive non-metallic element. It combines with both metals and non-metals. Examiner Only Marks Remark (a) (i) Using dot and cross diagrams, explain how strontium atoms combine with fluorine atoms to form strontium fluoride. Show the outer electrons only. [4] (ii) Compare the electrical conductivity of solid strontium metal with that of solid strontium fluoride. Explain your answer. ____________________________________________________ ___________________________________________________ ___________________________________________________ _________________________________________________ [3] 5631.02 R 8 [Turn over (b) Sulphur and fluorine combine to form a non-polar molecule sulphur hexafluoride, SF6. Examiner Only Marks Remark (i) Define the term electronegativity. ___________________________________________________ _________________________________________________ [2] (ii) Label the diagram below to show the polarity of the S F bond. S F [1] (iii) Draw a dot and cross diagram to show the bonding in SF6 using outer shell electrons only. [2] (iv) Explain whether the SF6 molecule obeys the octet rule. ___________________________________________________ ___________________________________________________ _________________________________________________ [2] 5631 5631.02 R 9 [Turn over (v) Draw, name and explain the shape of the SF6 molecule. Examiner Only Marks Remark ___________________________________________________ ___________________________________________________ _________________________________________________ [4] (vi) Suggest why SF6 is a non-polar molecule, even though it contains polar bonds. ___________________________________________________ _________________________________________________ [2] (c) Boron trifluoride can combine with ammonia to form the following molecule. F H B F F N H H (i) Name the type of bond formed between the boron and nitrogen atoms. _________________________________________________ [1] (ii) Explain how this bond is formed. ___________________________________________________ _________________________________________________ [1] 5631.02 R 10 [Turn over 13 Concentrated nitric acid (HNO3) oxidises iodide ions to form iodine. In the reaction the nitric acid is reduced to form nitrogen monoxide (NO). Examiner Only Marks Remark (a) Reduction and oxidation can be defined in different ways. (i) Define oxidation in terms of electron transfer. _________________________________________________ [1] (ii) Define reduction in terms of changes in oxidation state. _________________________________________________ [1] (b) Deduce the oxidation number of nitrogen in (i) HNO3 _________________________________________ [1] (ii) NO _________________________________________ [1] (c) The half-equation for the reduction of concentrated nitric acid is shown below. HNO3 + 3H+ + 3e NO + 2H2O (i) Write a half-equation for the oxidation of iodide ions to form an iodine molecule. _________________________________________________ [1] (ii) Combine the reduction and oxidation half-equations to give the overall ionic equation. _________________________________________________ [2] 5631.02 R 11 [Turn over (d) At room temperature and pressure, iodine exists as a grey-black shiny solid. Describe the bonding in, and explain the structure of iodine crystals. Explain the relative solubilities of iodine in water and hexane. Examiner Only Marks Remark _______________________________________________________ _______________________________________________________ _______________________________________________________ _______________________________________________________ _______________________________________________________ _______________________________________________________ _____________________________________________________ [5] Quality of written communication 5631.02 R [2] 12 [Turn over 14 Chlorine is produced by the electrolysis of concentrated sodium chloride solution (brine). It is then used by other industries to produce a variety of useful products. Examiner Only Marks Remark (a) The reaction between chlorine and cold dilute sodium hydroxide is used in the manufacture of bleach. (i) Write the equation for this reaction. _________________________________________________ [2] (ii) This reaction is described as disproportionation. Explain the meaning of this term. ___________________________________________________ ___________________________________________________ _________________________________________________ [2] (b) Chlorine reacts with hydrogen to produce hydrogen chloride. (i) Write the equation for this reaction. _________________________________________________ [2] (ii) Suggest why hydrogen chloride has a much lower boiling point than hydrogen fluoride. ___________________________________________________ ___________________________________________________ _________________________________________________ [3] (iii) Explain why hydrogen chloride is more thermally stable than hydrogen iodide. ___________________________________________________ ___________________________________________________ _________________________________________________ [2] 5631.02 R 13 [Turn over (c) The presence of chloride ions in brine can be established by adding an aqueous solution of silver nitrate. Examiner Only Marks Remark (i) What would be observed in this reaction? _________________________________________________ [2] (ii) Write an ionic equation, including state symbols, for the reaction. _________________________________________________ [2] (iii) State what is observed when an excess of dilute aqueous ammonia is then added. _________________________________________________ [1] 5631.02 R 14 [Turn over 15 The degree of hydration in samples of hydrated sodium carbonate (Na2CO3.xH2O) can be determined by different methods. Examiner Only Marks Remark (a) When 10.04 g of a sample was heated to constant mass, 3.97 g of anhydrous sodium carbonate was obtained. (i) Explain the term anhydrous. ___________________________________________________ _________________________________________________ [1] (ii) Calculate the number of moles of anhydrous sodium carbonate obtained. _________________________________________________ [1] (iii) Calculate the mass of water present in the sample. _________________________________________________ [1] (iv) Calculate the number of moles of water present. _________________________________________________ [1] (v) Calculate the value of x in the sample. _________________________________________________ [1] 5631.02 R 15 [Turn over (b) The degree of hydration can also be determined by dissolving the sample in water and titrating with a standard solution of hydrochloric acid. Examiner Only Marks Remark (i) What is a standard solution? _________________________________________________ [1] (ii) Give the equation for the reaction between sodium carbonate and hydrochloric acid. _________________________________________________ [2] (iii) Name a suitable indicator for this titration. _________________________________________________ [1] 5631.02 R 16 [Turn over (c) 3.57 g of a second sample of sodium carbonate was dissolved in water and the resulting solution was made up to 250 cm3 in a volumetric flask. A 25.0 cm3 sample of this solution required 28.5 cm3 of 0.1 mol dm 3 hydrochloric acid to reach the end point. (i) Give the colour change which would be obtained at the end point, using the indicator given in (b)(iii). From _____________________ to _____________________ [2] (ii) Calculate the number of moles of hydrochloric acid used in the titration. _________________________________________________ [1] (iii) Calculate the number of moles of sodium carbonate present in 25.0 cm3 of solution. _________________________________________________ [1] (iv) Calculate the number of moles of sodium carbonate present in 250 cm3 of solution. _________________________________________________ [1] (v) Calculate the mass of sodium carbonate present in the second sample. _________________________________________________ [1] (vi) Calculate the mass of water present in the second sample. _________________________________________________ [1] (vii) Calculate the number of moles of water present in the second sample. _________________________________________________ [1] (viii) Calculate the value of x in the second sample. _________________________________________________ [1] 5631.02 R 17 Examiner Only Marks Remark THIS IS THE END OF THE QUESTION PAPER 1847-076-1

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Additional Info : : Gce Chemistry June 2010 Assessment Unit AS 1 Basic Concepts in Physical and Inorganic Chemistry - Revised
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