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GCE JAN 2009 : (AS 1) Basic Concepts in Physical and Inorganic Chemistry - Revised

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Sp ec Ne ifi w ca tio n 1 2 Centre Number 3 71 4 Candidate Number 5 6 ADVANCED SUBSIDIARy (AS) General Certificate of Education January 2009 7 8 9 Chemistry 10 assessing 12 Basic Concepts in Physical and Inorganic Chemistry 13 14 [AC111] 15 FRIDAy 16 JANUARy, MORNING 16 17 AC111 Assessment Unit AS 1 11 TIME 18 1 hour 30 minutes. 19 INSTRUCTIONS TO CANDIDATES 20 Write your Centre Number and Candidate Number in the spaces 21 provided at the top of this page. Answer all sixteen questions. 22 Answer all ten questions in Section A. Record your answers by 23 marking the appropriate letter on the answer sheet provided. Use only the spaces numbered 1 to 10. Keep in sequence when answering. 24 Answer all six questions in Section B. Write your answers in the 25 spaces provided in this question paper. 26 27 28 29 30 31 32 35 Question Marks Number Section A 1 10 INFORMATION FOR CANDIDATES The total mark for this paper is 100. Quality of written communication will be assessed in question 16(a)(iii). 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. 33 34 For Examiner s use only Section B 11 12 13 14 15 16 Total Marks 4270 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 p electrons in an oxide, O2 ion? A B C D 2 Which one of the following represents the electronic configuration for a chromium atom in its ground state? A B C D 3 1s2 1s2 1s2 1s2 2s2 2s2 2s2 2s2 2p6 2p6 2p6 2p6 3s2 3s2 3s2 3s2 3p6 3p6 3p6 3p6 3d3 3d6 3d5 4s1 3d4 4s2 Which one of the following represents the line emission spectrum of atomic hydrogen? A B frequency wavelength C D frequency 4270 frequency 2 [Turn over 4 The intermolecular forces of attraction in solid iodine are A B C D 5 Which one of the following molecules contains the most polar bond? A B C D 6 covalent bonds. hydrogen bonds. permanent dipole attractions. van der Waals forces. CH4 NH3 H2O HF The graph below represents the variation in the first ionisation energy with atomic number. First ionisation energy (kJ mol 1) P Q R S atomic number The elements indicated by the letters P Q, R and S are , A B C D 4270 alkali metals. halogens. noble gases. transition metals. 3 [Turn over 7 The melting point of the elements going across the Periodic Table from sodium to argon A B C D 8 How many moles of hydrogen ions are present in 40 cm3 of 0.2 M sulphuric acid? A B C D 9 increases steadily. decreases steadily. increases to silicon and then decreases. decreases to silicon and then increases. 8 x 10 3 1.6 x 10 2 0.2 0.4 In which one of the following do both molecules obey the octet rule? A B C D BeCl2 and NH3 BF3 and CH4 CH4 and NH3 BF3 and BeCl2 10 Phosphoric acid is manufactured by the reaction of sulphuric acid with calcium phosphate according to the equation: 3H2SO4 + Ca3(PO4)2 2H3PO4 + 3CaSO4 What mass of phosphoric acid would be obtained from reacting 60 kg of sulphuric acid with 60 kg of calcium phosphate? A B C D 4270 19 kg 38 kg 40 kg 60 kg 4 [Turn over Section B Examiner Only Marks Remark Answer all six questions in this section 11 Complete the table stating the shape of each of the molecules. Molecule Shape Ammonia Carbon dioxide Methane 4270 [3] 5 [Turn over 12 (a) Metal ions can be identified by the characteristic flame colour observed when their solutions are sprayed into a blue Bunsen flame. Examiner Only Marks Remark Complete the table by stating the flame colour for each of the ions listed. Metal ion Flame colour Ba2+ Ca2+ Cu2+ [3] (b) Explain, with the help of an energy level diagram, how flame colours arise. _______________________________________________________________ _______________________________________________________________ ____________________________________________________________ [3] (c) Flame colours are a consequence of the emission spectrum of an element. Explain how the emission spectrum can be used to calculate the first ionisation energy of an element. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ ____________________________________________________________ [2] 4270 6 [Turn over 13 Washing soda is hydrated sodium carbonate and can be represented by the formula Na2CO3.xH2O. The value of x can be found by titrating a solution of washing soda against standard hydrochloric acid solution. Examiner Only Marks Remark (a) (i) What is meant by the term standard solution? ________________________________________________________ [1] (ii) Write the equation for the reaction between sodium carbonate, Na2CO3, and excess hydrochloric acid. ________________________________________________________ [2] (b) In one experiment a 2.80 g sample of washing soda was made up to 250 cm3 of solution in a volumetric flask. 25 cm3 of this solution required 22.4 cm3 of 0.1 M hydrochloric acid for neutralisation. Find the value of x using the following headings. Moles of hydrochloric acid used _______________________________________________________________ Moles of sodium carbonate in 25 cm3 _______________________________________________________________ Moles of sodium carbonate in the sample _______________________________________________________________ Mass of sodium carbonate in the sample _______________________________________________________________ Mass of water in the sample _______________________________________________________________ Moles of water in the sample _______________________________________________________________ Value of x ____________________________________________________________ [5] (c) Suggest a suitable indicator for the titration, stating the colour change expected. Indicator: ________________________ Colour change: from _________________ to _________________ 4270 7 [3] [Turn over BLANK PAGE 4270 8 [Turn over 14 (a) Magnesium is extracted from dolomite, MgCO3.CaCO3. Dolomite is heated to form the metal oxides and carbon dioxide. After purification the magnesium oxide is heated with coke (carbon) in a stream of chlorine to form magnesium chloride and carbon monoxide. Magnesium is formed by the electrolysis of molten magnesium chloride. Examiner Only Marks Remark (i) Write the equation for the effect of heat on dolomite. ________________________________________________________ [2] (ii) Write the equation for the formation of magnesium chloride from magnesium oxide. ________________________________________________________ [2] (iii) Magnesium chloride is ionic. Explain why it must be molten for the electrolysis to take place. ___________________________________________________________ ________________________________________________________ [1] (iv) Draw dot and cross diagrams to show the formation of magnesium and chlorine atoms from their ions. [4] 4270 9 [Turn over (b) Magnesium is a typical metal. Examiner Only Marks Remark (i) Draw a labelled diagram to show the bonding in magnesium metal. [2] (ii) Explain why magnesium conducts electricity. ___________________________________________________________ ________________________________________________________ [2] (c) (i) Write the equation, including state symbols, for the first ionisation energy of magnesium. ________________________________________________________ [2] log ionisation energy (kJ mol 1) (ii) Using the axes below, sketch a graph to show the twelve successive ionisation energies of magnesium. 1 2 3 4 5 6 7 8 9 10 number of electrons 11 12 [2] 4270 10 [Turn over (iii) State two reasons why the first ionisation energy of calcium is less than that of magnesium. Examiner Only Marks Remark ___________________________________________________________ ___________________________________________________________ ________________________________________________________ [2] 4270 11 [Turn over 15 Xenon was first isolated by Ramsey and Travers in 1898. Examiner Only Marks Remark (a) Xenon makes up 1 part in 20 000 000 by volume of air. Calculate the number of atoms of xenon in 1 dm3 of air at room temperature and pressure using the following headings. Molar gas volume = 24 dm3 at room temperature and pressure. Number of moles in 1 dm3 of air. _______________________________________________________________ Number of particles (atoms and molecules) in 1 dm3 of air. _______________________________________________________________ Number of atoms of xenon in 1 dm3 of air. ____________________________________________________________ [3] (b) Xenon has a number of naturally occurring isotopes. The table lists the principal isotopes of xenon. Relative isotopic mass 129 % abundance 131 23 132 28 134 12 136 10 27 (i) Explain what is meant by the term isotope. ___________________________________________________________ ________________________________________________________ [2] (ii) Use the information in the table to calculate the relative atomic mass of xenon. ___________________________________________________________ ___________________________________________________________ ________________________________________________________ [2] 4270 12 [Turn over (c) The first compounds of xenon were isolated by Bartlett in 1962. Examiner Only Marks Remark The reaction between the hydrogenxenate and hydroxide ions can be represented as follows: 2OH + 2HXeO4 Xe + 2H2O + XeO64 + O2 (i) Deduce the oxidation number of xenon in each of the following. HXeO4 __________ Xe __________ XeO64 __________ [3] (ii) Explain why this is considered to be a disproportionation reaction. ___________________________________________________________ ___________________________________________________________ ________________________________________________________ [2] 4270 13 [Turn over 16 The halogens are found in Group VII of the Periodic Table. Examiner Only Marks Remark (a) (i) Complete the table. Fluorine Chlorine Bromine Iodine 9 17 35 53 Appearance at 20 C Yellow gas Green-yellow gas Boiling point ( C) 188 35 59 183 4.1 2.9 2.8 2.2 Atomic number Electronegativity [2] (ii) Explain the change in boiling point of the halogens. ___________________________________________________________ ___________________________________________________________ ________________________________________________________ [2] (iii) State what is meant by the term electronegativity and explain the trend for the halogens. ___________________________________________________________ ___________________________________________________________ ___________________________________________________________ ___________________________________________________________ ___________________________________________________________ ________________________________________________________ [3] Quality of written communication 4270 [2] 14 [Turn over (b) Chlorine reacts with cold dilute sodium hydroxide to form sodium chlorate(I) and with hot concentrated sodium hydroxide to form sodium chlorate(V). Examiner Only Marks Remark (i) Write the equation for the reaction of chlorine with cold dilute sodium hydroxide. ________________________________________________________ [2] (ii) What is the formula of sodium chlorate(V)? ________________________________________________________ [1] (c) Iodine is more soluble in hexane than in water. (i) Explain why iodine is more soluble in hexane. ___________________________________________________________ ________________________________________________________ [2] (ii) What colour is a solution of iodine in hexane? ________________________________________________________ [1] (d) The hydrogen halides can be formed by the reaction of concentrated sulphuric acid with the corresponding solid sodium halide. (i) Write the equation for the reaction of concentrated sulphuric acid with solid sodium chloride at room temperature. ________________________________________________________ [2] (ii) Name two products, other than hydrogen iodide, which are formed when sodium iodide reacts with concentrated sulphuric acid. ________________________________________________________ [2] (iii) State and explain the trend in thermal stability of the hydrogen halides. ___________________________________________________________ ___________________________________________________________ ________________________________________________________ [2] 4270 15 [Turn over (e) The presence of halide ions can be detected using silver ions and aqueous ammonia. Examiner Only Marks Remark (i) Write the ionic equation for the reaction between silver ions and chloride ions. ________________________________________________________ [1] (ii) Complete the table below. Effect of adding aqueous ammonia Halide ion Colour of silver salt dilute concentrated Chloride Bromide Iodide [3] (f) Explain why the public water supply may be fluoridated and why some people are opposed to this. _______________________________________________________________ _______________________________________________________________ ____________________________________________________________ [2] THIS IS THE END OF THE QUESTION PAPER 4270 16 [Turn over 0000 17 [Turn over 0000 18 [Turn over 0000 19 [Turn over 935-060-1

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Additional Info : Gce Chemistry January 2009 Assessment Unit AS 1 Basic Concepts in Physical and Inorganic Chemistry - Revised
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