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1 Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials General Certificate of Education Advanced Subsidiary Examination January 2010 Question 1 2 Mark Chemistry Unit 1 Foundation Chemistry Thursday 14 January am to am For this paper you must have: the Periodic Table/Data Sheet, provided as an insert (enclosed) a calculator. CHEM TOTAL Time allowed 1 hour 15 minutes Instructions Use black ink or black ball-point pen. Fill in the boxes at the top of this page. Answer all questions. You must answer the questions in the spaces provided. Answers written in margins or on blank pages will not be marked. All working must be shown. Do all rough work in this book. Cross through any work you do not want to be marked. Information The marks for questions are shown in brackets. The maximum mark for this paper is 70. The Periodic Table/Data Sheet is provided as an insert. Your answers to the questions in Section B should be written in continuous prose, where appropriate. You will be marked on your ability to: use good English organise information clearly use accurate scientific terminology. Advice You are advised to spend about 50 minutes on Section A and about 25 minutes on Section B. (JAN10CHEM101) CHEM1

2 2 SECTION A Answer all questions in the spaces provided. 1 Ionisation energies provide evidence for the arrangement of electrons in atoms. 1 (a) Complete the electron configuration of the Mg + ion. 1s (b) (i) State the meaning of the term first ionisation energy. 1 (b) (ii) Write an equation, including state symbols, to show the reaction that occurs when the second ionisation energy of magnesium is measured. 1 (b) (iii) Explain why the second ionisation energy of magnesium is greater than the first ionisation energy of magnesium. 1 (b) (iv) Use your understanding of electron arrangement to complete the table by suggesting a value for the third ionisation energy of magnesium. First Second Third Fourth Fifth Ionisation energies of magnesium / kj mol (02)

3 3 1 (c) State and explain the general trend in the first ionisation energies of the Period 3 elements sodium to chlorine. Trend... Explanation... (3 marks) 1 (d) State how the element sulfur deviates from the general trend in first ionisation energies across Period 3. Explain your answer. How sulfur deviates from the trend... Explanation... (3 marks) 1 (e) A general trend exists in the first ionisation energies of the Period 2 elements lithium to fluorine. Identify one element which deviates from this general trend. 13 Turn over (03)

5 2 (c) Ammonia is manufactured by the Haber Process. 5 N 2 + 3H 2 2NH 3 Calculate the percentage atom economy for the production of ammonia in this process. 2 (d) A sample of ammonia gas occupied a volume of m 3 at 37 C and a pressure of 100 kpa. (The gas constant R = 8.31 J K 1 mol 1 ) Calculate the amount, in moles, of ammonia in this sample. (3 marks) 2 (e) Glauber s salt is a form of hydrated sodium sulfate that contains 44.1% by mass of sodium sulfate. Hydrated sodium sulfate can be represented by the formula Na 2 SO 4. xh 2 O where x is an integer. Calculate the value of x. (3 marks) 13 Turn over (05)

6 6 3 The table below shows the boiling points of some hydrogen compounds formed by Group 6 elements. H 2 O H 2 S H 2 Se H 2 Te Boiling point / K (a) State the strongest type of intermolecular force in water and in hydrogen sulfide (H 2 S). Water... Hydrogen sulfide... 3 (b) Draw a diagram to show how two molecules of water are attracted to each other by the type of intermolecular force you stated in part (a). Include partial charges and all lone pairs of electrons in your diagram. 3 (c) Explain why the boiling point of water is much higher than the boiling point of hydrogen sulfide. (3 marks) 3 (d) Explain why the boiling points increase from H 2 S to H 2 Te (06)

7 7 3 (e) When H + ions react with H 2 O molecules, H 3 O + ions are formed. Name the type of bond formed when H + ions react with H 2 O molecules. Explain how this type of bond is formed in the H 3 O + ion. Type of bond... Explanation... 3 (f) Sodium sulfide (Na 2 S) has a melting point of 1223 K. Predict the type of bonding in sodium sulfide and explain why its melting point is high. Type of bonding... Explanation... (3 marks) 13 Turn over for the next question Turn over (07)

8 8 4 Alkanes are saturated hydrocarbons which can be obtained from crude oil. Pentane is an example of an alkane. A molecule of pentane contains five carbon atoms. 4 (a) (i) State the meaning of the term saturated and of the term hydrocarbon as applied to alkanes. Saturated... Hydrocarbon... 4 (a) (ii) Give the general formula for the alkanes. 4 (b) Pentane burns completely in oxygen. 4 (b) (i) Write an equation for this reaction. 4 (b) (ii) State how the products of this reaction may affect the environment. 4 (c) Give the name of a solid pollutant which may form when pentane burns incompletely in air. (08)

9 9 4 (d) One molecule of C 9 H 20 can be cracked to form one molecule of pentane and one other product. 4 (d) (i) Write an equation for this cracking reaction. 4 (d) (ii) Suggest a type of compound that can be manufactured from the other product of this cracking reaction. 4 (d) (iii) State why a high temperature is needed for cracking reactions to occur. Question 4 continues on the next page Turn over (09)

11 11 SECTION B Answer all questions in the spaces provided. 5 A mass spectrometer can be used to investigate the isotopes in an element. 5 (a) Define the term relative atomic mass of an element. 5 (b) Element X has a relative atomic mass of 47.9 Identify the block in the Periodic Table to which element X belongs and give the electron configuration of an atom of element X. Calculate the number of neutrons in the isotope of X which has a mass number 49 (3 marks) Question 5 continues on the next page Turn over (11)

13 13 5 (d) State how vaporised atoms of Z are converted into Z + ions in a mass spectrometer. State and explain which of the Z + ions formed from the isotopes of Z in part (c) will be deflected the most in a mass spectrometer. (4 marks) 5 (e) Explain briefly how the relative abundance of an ion is measured in a mass spectrometer. 15 Turn over (13)

14 14 6 A molecule of ClF 3 reacts with a molecule of AsF 5 as shown in the following equation. ClF 3 + AsF 5 ClF AsF 6 Use your understanding of electron pair repulsion to draw the shape of the AsF 5 molecule and the shape of the ClF 2 + ion. Include any lone pairs of electrons. Name the shape made by the atoms in the AsF 5 molecule and in the ClF 2 + ion. Predict the bond angle in the ClF 2 + ion (5 marks) END OF QUESTIONS (14)

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