
	Trending ▼ ICSE CBSE 10th ISC CBSE 12th CTET GATE UGC NET Vestibulares ResFinder

GCE JAN 2011 : (AS 1) Basic Concepts in Physical and Inorganic Chemistry - Revised (Irish Medium)

20 pages, 51 questions, 0 questions with responses, 0 total responses,

	gce	+Fave Message
	Profile Timeline Uploads Q & A

Home > gce >

Instantly get Model Answers to questions on this ResPaper. Try now!
NEW ResPaper Exclusive!

Formatting page ...

Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2011 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC111] THURSDAY 13 JANUARY, 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 sixteen 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 six questions in Section B. Write your answers in the spaces provided in this question paper. INFORMATION FOR CANDIDATES 111554 The total mark for this paper is 100. Quality of written communication will be assessed in question 14(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. For Examiner s use only Question Marks Number Section A 1 10 Section B 11 12 13 14 15 16 Total Marks 6781 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 An atom in which the number of protons is greater than the number of neutrons is A B C D 2 2H. 3He. 10B. 39K. Which one of the following is a correct description of electronic transitions in a given series in the atomic emission spectrum of hydrogen? A They all start from the ground state. B They all end at the ground state. C They all start from one particular energy level. D They all end at one particular energy level. 3 Which one of the following lists the first ionisation energies (in kJ mol 1) of the elements magnesium, aluminium, silicon, phosphorus and sulfur in this order? A 496 B 577 C 736 D 786 6781 736 786 577 1060 577 1060 786 1000 786 1000 1060 1260 1060 1260 1000 1520 2 [Turn over 4 The mass spectrum of molecular chlorine, Cl2, is shown below. An additional peak is in the spectrum which should not be present. Which one of the following peaks should not be present? 35 70 71 72 74 37 m/e A 35 B 71 C 72 D 74 5 A solid melts sharply at 100 101 C. It does not conduct electricity even when molten. It dissolves in hydrocarbon solvents. The solid has A an atomic structure. B a giant covalent structure. C an ionic structure. D a molecular covalent structure. 6 Which one of the following gaseous hydrides most readily decomposes into its elements on contact with a hot glass rod? A ammonia B hydrogen fluoride C hydrogen iodide D steam 6781 3 [Turn over 7 Arsine, AsH3, is a molecular hydride of arsenic which is found in Group V of the Periodic Table. Which one of the following is the structure of arsine in the vapour state? A B H As As H H H Bond angles 120 C D H As H H Bond angles less than 109.5 8 H Bond angles greater than 109.5 As H H H H Bond angles 109.5 50 cm3 of 0.20 mol dm 3 sulphuric acid is exactly neutralised by A 100 cm3 of 0.40 mol dm 3 potassium hydroxide solution. B 25 cm3 of 0.20 mol dm 3 potassium hydroxide solution. C 50 cm3 of 0.20 mol dm 3 potassium hydroxide solution. D 100 cm3 of 0.20 mol dm 3 potassium hydroxide solution. 9 Which one of the following is the number of electrons which have approximately the same mass as that of a proton? A 20 B 200 C 2000 D 20000 10 Which one of the following oxides is not polar? A B C D 6781 CO CO2 H2O NO 4 [Turn over Section B Examiner Only Marks Remark Answer all six questions in this section. 11 Nitrogen dioxide, NO2, is one of the components of photochemical smog. The energy required to dissociate this molecule into NO molecules and O atoms is 305 kJ mol 1. Use the following headings to calculate the frequency of radiation required to cause the dissociation. (a) Convert 305 kJ into Joules (b) Calculate the number of Joules required to dissociate one molecule of nitrogen dioxide. (c) Use the equation E = hf to convert the value in Joules into a frequency and state the units. _____________________________________________________________ ___________________________________________________________ [1] 6781 ___________________________________________________________ [1] ___________________________________________________________ [1] 5 [Turn over 12 The mineral beryl, Be3Al2Si6O18, is the principal source of beryllium. Although there are minerals richer in beryllium they are scarce and costly. Examiner Only Marks Remark (a) Calculate the percentage, by mass, of beryllium in beryl. _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [3] (b) The metal beryllium is obtained either by the electrolysis of a fused mixture of beryllium and potassium chlorides at 350 C or by the reduction of beryllium fluoride with magnesium. (i) Write an equation for the formation of beryllium from beryllium ions. _______________________________________________________ [1] (ii) Write an equation for the formation of beryllium from the reduction of beryllium fluoride with magnesium. _______________________________________________________ [1] (c) The first element in a Group often has more distinctive properties than the elements in the rest of the Group. This is often as a result of the difference in electronegativities. The electronegativity values of the Group II elements are shown below. Be electronegativity value Mg Ca Sr Ba atomic number (i) Explain the meaning of the term electronegativity. _________________________________________________________ _______________________________________________________ [2] 6781 6 [Turn over (ii) Using electronegativity suggest why beryllium chloride is a covalent molecule and barium chloride is ionic. Examiner Only Marks Remark _________________________________________________________ _______________________________________________________ [2] (iii) State two physical properties which could be used to distinguish these two chlorides. _________________________________________________________ _______________________________________________________ [2] (d) Beryllium chloride may be prepared by the action of chlorine or hydrogen chloride on the metal. (i) Write the equation for the reaction of beryllium with hydrogen chloride. _______________________________________________________ [1] (ii) Draw a dot and cross diagram to show the formation of beryllium chloride from beryllium and chlorine atoms. Use only the outer electrons of each atom. [3] (iii) State the octet rule. _________________________________________________________ _______________________________________________________ [2] (iv) Beryllium chloride can be said to obey the octet rule and also not to obey the octet rule. Explain this contradiction. _________________________________________________________ _______________________________________________________ [2] 6781 7 [Turn over (v) Draw the shape of a beryllium chloride molecule. Examiner Only Marks Remark [1] (vi) State the shape of the beryllium chloride molecule. _______________________________________________________ [1] (vii) Explain the shape of the beryllium chloride molecule. _________________________________________________________ _______________________________________________________ [2] 6781 8 [Turn over 13 Chlorine forms a series of oxides some of which are listed below. Examiner Only Marks chlorine monoxide Cl2O chlorine dioxide ClO2 chlorine hexoxide Cl2O6 chlorine heptoxide Cl2O7 (a) Deduce the systematic name for chlorine heptoxide using the oxidation number of chlorine. Remark (b) Chlorine dioxide dissolves in water to form a solution which eventually forms a mixture of chloric and hydrochloric acids. ___________________________________________________________ [1] 6ClO2 + 3H2O 5HClO3 + HCl The chlorine atoms in chlorine dioxide undergo disproportionation in this reaction. (i) Explain the meaning of the term disproportionation. _________________________________________________________ _______________________________________________________ [1] (ii) Calculate the oxidation number of chlorine in the reactant and in the products of this reaction and use them to confirm that the reaction is a disproportionation reaction. _________________________________________________________ _________________________________________________________ _______________________________________________________ [3] 6781 9 [Turn over (c) Chlorine gas dissolves in water to the extent of 0.8 g in 100 cm3 at atmospheric pressure and 20 C. Examiner Only Marks Remark (i) Calculate the molarity of the chlorine water, Cl2 (aq), produced. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] (ii) Name another solvent in which chlorine will readily dissolve. _______________________________________________________ [1] 6781 10 [Turn over 14 An experiment was set up to investigate the displacement reactions of the halogens. Examiner Only Marks Remark Solutions of sodium halides were prepared and reacted with other halogens. The results table is shown below. sodium iodide (aq) sodium bromide (aq) iodine solution bromine solution X sodium chloride (aq) X chlorine solution means that a reaction took place X means that no reaction took place (a) Complete the three remaining places in the table. [2] (b) (i) Both bromine and iodine solutions are coloured. Describe the observations which would indicate that a reaction took place when aqueous sodium iodide is added to a bromine solution. _________________________________________________________ _______________________________________________________ [2] (ii) Write the ionic equation for the reaction between bromine solution and aqueous sodium iodide. _______________________________________________________ [1] (c) (i) Describe what is observed when chlorine solution is added to aqueous sodium bromide. _________________________________________________________ _______________________________________________________ [2] (ii) Write the equation for the reaction between chlorine solution and aqueous sodium bromide. _______________________________________________________ [1] 6781 11 [Turn over (d) If you had poured solutions of sodium iodide, bromide and chloride into beakers A, B and C and forgotten to label them, describe how, using aqueous silver nitrate and both dilute and concentrated ammonia solutions, you would determine which sodium salt was in which beaker. Each beaker must be tested. Examiner Only Marks Remark _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [6] Quality of written communication 6781 [2] 12 [Turn over 15 The structure of ice is shown below. The water molecules are held together by hydrogen bonds which are a type of intermolecular force. Examiner Only Marks Remark (a) Name two other types of intermolecular force. ___________________________________________________________ [2] (b) (i) Explain how hydrogen bonding takes place between the water molecules in ice. _________________________________________________________ _______________________________________________________ [2] (ii) Explain, using the structure above, why ice is less dense than water. _________________________________________________________ _________________________________________________________ _______________________________________________________ [2] (c) Although water is capable of forming hydrogen bonds it does not form long chains of polywater at room temperature. However, in the liquid state, molecules such as hydrogen fluoride do form very short chains. Suggest why water does not form chains and liquid hydrogen fluoride does. _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [2] 6781 13 [Turn over (d) Ammonia is another substance that can form hydrogen bonds. However, ammonia has a pyramidal structure. Examiner Only Marks Remark (i) Draw two molecules of ammonia and show the hydrogen bond between the two molecules. [2] (ii) Explain why when ammonia reacts with a hydrogen ion it loses the ability to form hydrogen bonds. _________________________________________________________ _______________________________________________________ [1] (e) Explain why ammonia is extremely soluble in water. _____________________________________________________________ ___________________________________________________________ [2] 6781 14 [Turn over 16 Lithium exists in nature as two isotopes, 6Li and 7Li. The composition of a sample of lithium in nature is shown in the table below. isotope 7.42 lithium 7 Remark % abundance lithium 6 Examiner Only Marks 92.58 (a) Draw the structure of a 7Li atom, labelling all the sub-atomic particles. [3] (b) State and explain to which of the s, p or d blocks lithium belongs. _____________________________________________________________ ___________________________________________________________ [2] (c) Calculate the relative atomic mass of lithium to two decimal places. _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [3] 6781 15 [Turn over (d) Lithium sulphate is readily soluble in water and crystallises from solution as the hydrate. Examiner Only Marks Remark (i) Explain what is meant by the term water of crystallisation. _________________________________________________________ _______________________________________________________ [1] (ii) Write the formula of anhydrous lithium sulphate. _______________________________________________________ [1] (iii) Calculate the formula of hydrated lithium sulphate if 3.76 g of the hydrated lithium salt produces 3.23 g of anhydrous lithium sulphate on heating. _________________________________________________________ _________________________________________________________ _________________________________________________________ _________________________________________________________ _______________________________________________________ [3] (e) Lithium sulphate can be used in a flame test. Explain how a flame test could be carried out and state the expected colour of the flame. _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ _____________________________________________________________ ___________________________________________________________ [4] THIS IS THE END OF THE QUESTION PAPER 6781 16 [Turn over Permission to reproduce all copyright material has been applied for. In some cases, efforts to contact copyright holders may have been unsuccessful and CCEA will be happy to rectify any omissions of acknowledgement in future if notified. 111554

Formatting page ...

Additional Info : Gce Chemistry January 2011 Assessment Unit AS 1 Basic Concepts in Physical and Inorganic Chemistry - Revised (Irish Medium)
Tags : General Certificate of Education, A Level and AS Level, uk, council for the curriculum examinations and assessment, gce exam papers, gce a level and as level exam papers , gce past questions and answer, gce past question papers, ccea gce past papers, gce ccea past papers

gce chat

Horizontal lines at:
Guest Horizontal lines at:
AutoRM Data:
Box geometries: