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

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Sp ec Ne i w ca tio n Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education 2009 Chemistry Assessment Unit AS 1 Module 1: Basic Concepts in Physical and Inorganic Chemistry AC111 assessing [AC111] WEDNESDAY 3 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 seventeen 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 seven questions in Section B. Write your answers in the spaces provided in this question paper. INFORMATION FOR CANDIDATES The total mark for this paper is 100. Quality of written communication will be assessed in question 16(a)(i). In Section A all questions carry equal marks, i.e. two marks for each question. In Section B the figures in the 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. For Examiner s use only Question Marks Number Section A 1 10 Section B 11 12 13 14 15 16 17 Total Marks 4669 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 How many electrons are present in a potassium ion, K+? A B C D 2 18 19 20 39 Which one of the following represents the first five ionisation energies in kJ mol 1 of an s-block element? 1st A B C D 3 4th 5th 580 740 1000 14 800 1800 1500 2300 11 600 2700 7700 3400 2700 11 600 10 500 4600 1800 14 800 13 600 7000 580 0.5 5 7 13 Which one of the following contains a coordinate bond? A B C D 4669 3rd A sample of 4.64 g of hydrated sodium carbonate, Na2CO3.xH2O, was dissolved in 1 dm3 of water. 25.0 cm3 of this solution required 20.0 cm3 of 0.05 mol dm 3 hydrochloric acid for neutralisation. Which one of the following is the value of x? A B C D 4 2nd Ammonium, NH4+ Boron trifluoride, BF3 Sulphur hexafluoride, SF6 Water, H2O 2 [Turn over 5 Which one of the following lists the colour of solid iodine and of iodine dissolved in the solvent stated? Solid Water Hexane A purple yellow/brown B dark purple yellow/brown purple C yellow/brown grey/black yellow/brown D 6 grey/black grey/black yellow/brown purple Which one of the following does not show the number of each bond present in the named molecules? Molecule Single bond Double bond Triple bond A 1 0 Nitrogen, N2 0 0 1 C Carbon dioxide, CO2 0 2 0 D Beryllium chloride, BeCl2 2 0 0 In which one of the following molecules does the named element have two lone pairs of electrons? A B C D 4669 2 B 7 Ethene, C2H4 Beryllium in BeCl2 Carbon in CH4 Nitrogen in NH3 Oxygen in H2O 3 [Turn over 8 Using the half-equations below, which one of the following is the balanced ionic equation for the reaction between acidified manganate(VII) ions and ethanedioate ions? Acidified manganate(VII) ions: MnO4 8H+ + 5e + Mn2+ + 4H2O Ethanedioate ions: C2O42 A B C D 9 2MnO4 MnO4 2MnO4 5MnO4 + + + + 16H+ 8H+ 16H+ 40H+ + + + + C2O42 5C2O42 5C2O42 2C2O42 2CO2 + 2e 2Mn2+ + Mn2+ + 2Mn2+ + 5Mn2+ + 8H2O + 2CO2 4H2O + 10CO2 8H2O + 10CO2 20H2O + 4CO2 Which one of the following molecules is non-polar? A B C D Ammonia, NH3 Carbon dioxide, CO2 Hydrogen fluoride, HF Water, H2O 10 The extraction and purification of uranium from its ore involves the following reaction between uranium(IV) fluoride and magnesium. 2Mg + UF4 U + 2MgF2 What mass of uranium can be extracted from 500 tonnes of uranium(IV) fluoride and 50 tonnes of magnesium? A B C D 4669 192 246 379 495 tonnes tonnes tonnes tonnes 4 [Turn over Section B Examiner Only Marks Remark Answer all seven questions in this section 11 (a) Complete the table naming the strongest intermolecular force between molecules in each of the following liquids. Liquid Intermolecular force Ammonia, NH3(l) Hydrogen chloride, HCl(l) Methane, CH4(l) [3] (b) Explain why ice has a lower density than water. _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [2] (c) Draw and explain the shape of an ammonia molecule. _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [3] 4669 5 [Turn over 12 Neon has several isotopes. Examiner Only Marks Remark (a) Complete the table below. Number of protons Number of electrons Number of neutrons Neon-20 Neon-21 Neon-22 [2] (b) The table below gives the abundance of each isotope of neon. Calculate the relative atomic mass of neon to two decimal places. Isotope % abundance Neon-20 90.92 Neon-21 0.26 Neon-22 8.82 _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [2] (c) Name the isotope used as the standard to compare the relative atomic mass of atoms. ___________________________________________________________ [1] (d) Label the sub-shells below and draw the electronic structure of neon in the ground state. [2] 4669 6 [Turn over (e) Draw the shape of an s and of a p orbital. Examiner Only Marks s orbital 4669 p orbital 7 Remark [2] [Turn over 13 The percentage of calcium carbonate present in egg shells can be found by back titration using excess hydrochloric acid and standard sodium hydroxide solution. Examiner Only Marks Remark (a) Write an equation for the reaction between calcium carbonate and hydrochloric acid. ___________________________________________________________ [2] (b) Explain what is meant by a standard solution. _____________________________________________________________ ___________________________________________________________ [1] (c) 1.12 g of an egg shell was reacted with 20.0 cm3 of 2M hydrochloric acid and the solution formed made up to 250 cm3 in a volumetric flask. 25.0 cm3 of this solution completely reacted with 18.6 cm3 of 0.1 M sodium hydroxide. Calculate the percentage of calcium carbonate in the egg shell using the headings below. Moles of hydrochloric acid added to the egg shell _____________________________________________________________ Moles of sodium hydroxide used _____________________________________________________________ Moles of hydrochloric acid in 250 cm3 _____________________________________________________________ Moles of hydrochloric acid which reacted with the egg shell _____________________________________________________________ Mass of calcium carbonate in the egg shell _____________________________________________________________ Percentage of calcium carbonate in the egg shell ___________________________________________________________ [6] 4669 8 [Turn over (d) Name a suitable indicator for the titration of hydrochloric acid with sodium hydroxide solution. Give the colour change observed at the end point. Examiner Only Marks Remark Indicator: __________________________ Colour change: from __________________________ to __________________________ [3] 4669 9 [Turn over 14 The Periodic Table identifies various relationships between elements. Examiner Only Marks Remark (a) (i) What property is used to order the elements in the Periodic Table? _______________________________________________________ [1] (ii) Explain why transition metals are classified as d-block elements. _______________________________________________________ [1] (b) A number of distinct trends can be seen in the 3rd period from sodium to argon. (i) Describe the change in melting point across this period. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] (ii) Describe and explain the change in atomic radius across this period. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] (iii) On the axes below sketch the change in the 1st ionisation energy across the 3rd period. 1st ionisation energy (kJ mol 1) 11 4669 12 13 16 14 15 atomic number 10 17 18 [3] [Turn over BLANK PAGE (Questions continue overleaf) 4669 11 [Turn over 15 (a) Diamond and graphite have giant covalent structures. Examiner Only Marks Remark (i) Explain what is meant by the term covalent. _______________________________________________________ [1] (ii) Describe the structures of diamond and graphite. Diamond: ________________________________________________ _________________________________________________________ _______________________________________________________ [2] Graphite: ________________________________________________ _________________________________________________________ _______________________________________________________ [2] (iii) Explain why graphite conducts electricity. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] (iv) Explain why diamond is exceptionally hard. _________________________________________________________ _______________________________________________________ [1] 4669 12 [Turn over (b) Carbon dioxide, CO2, and beryllium chloride, BeCl2, are both covalent compounds. Examiner Only Marks Remark (i) Draw dot and cross diagrams for carbon dioxide and for beryllium chloride. carbon dioxide beryllium chloride [2] (ii) State the octet rule and explain why beryllium chloride does not obey it. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] 4669 13 [Turn over 16 Rock salt, impure sodium chloride, is found in large underground deposits at Kilroot. Examiner Only Marks Remark (a) (i) Describe how you would carry out chemical tests used to show that solid rock salt contains sodium chloride. _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [5] Quality of written communication [2] (ii) Draw dot and cross diagrams to show how sodium chloride is formed from sodium and chlorine atoms. [4] (b) Chlorine is manufactured by the electrolysis of concentrated sodium chloride solution. (i) Explain why sodium chloride solution conducts electricity but solid sodium chloride does not. _________________________________________________________ _______________________________________________________ [1] 4669 14 [Turn over (ii) Household bleach is manufactured by reacting chlorine with sodium hydroxide solution. Cl2 + 2NaOH NaCl + NaOCl + Examiner Only Marks Remark H2O Using oxidation numbers, explain why this reaction is described as disproportionation. _________________________________________________________ _________________________________________________________ _______________________________________________________ [3] (iii) Describe what you would observe when chlorine is bubbled through a solution of potassium bromide. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] (iv) Write an ionic equation for the reaction of chlorine with potassium bromide. _______________________________________________________ [1] (c) Concentrated sulphuric acid reacts with sodium halides to form the corresponding hydrogen halide. (i) Write an equation for the reaction of concentrated sulphuric acid with sodium chloride. _______________________________________________________ [2] (ii) Give two observations when concentrated sulphuric acid is added to sodium iodide. _________________________________________________________ _______________________________________________________ [2] 4669 15 [Turn over 17 The electronic structure of atoms has been interpreted from analysis of emission spectra. Examiner Only Marks Remark The diagram below shows the emission spectrum of hydrogen in the ultraviolet region. Convergence limit 91.1 nm 90 95 122 nm 100 105 110 115 120 125 Wavelength (nm) (a) Draw the electron transition responsible for the line at 122 nm. n = 4 _____________________________ n = 3 _____________________________ n = 2 _____________________________ n = 1 _____________________________ [2] (b) Explain what is meant by the convergence limit. ___________________________________________________________ [1] 4669 16 [Turn over (c) The convergence limit can be used to calculate the ionisation energy for hydrogen. Examiner Only Marks Remark (i) Write an equation, including state symbols, for the ionisation of atomic hydrogen. _______________________________________________________ [2] (ii) Use the information below to calculate the frequency of the line at the convergence limit. (speed of light = 3 108 m s 1, 1 nm = 1 10 9 m) speed of light = frequency wavelength _________________________________________________________ _______________________________________________________ [1] (iii) Use this frequency value to calculate the energy required to ionise one mole of hydrogen atoms. Energy required to ionise one hydrogen atom _________________________________________________________ Energy required to ionise one mole of hydrogen atoms in kJ mol 1 ________________________________________________ kJ mol 1 [2] THIS IS THE END OF THE QUESTION PAPER 4669 17 [Turn over 936-021-1

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