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1 Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups Medium banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching from September Candidate Style Answers (Medium) 1
2 Contents Contents 2 Introduction 3 Candidate Style Answer 4 Question 1 (a) 4 4 Question 1 (b) 5 5 Question 1 (c) 5 6 Question 2 (a) 6 7 Question 2 (b) 7 7 Question 3 (a) 8 8 Question 3 (b) 8 9 Question 3 (c) 9 9 Question 4 (a) Question 4 (b) Question 4 (c) Question 5 (a) Question 5 (b) Overall 13 Candidate Style Answers (Medium) 2
3 Introduction OCR has produced these candidate style answers to support teachers in interpreting the assessment criteria for the new GCE specifications and to bridge the gap between new specification release and availability of exemplar candidate work. This content has been produced by senior OCR examiners, with the input of Chairs of Examiners, to illustrate how the sample assessment questions might be answered and provide some commentary on what factors contribute to an overall grading. The candidate style answers are not written in a way that is intended to replicate student work but to demonstrate what a good or excellent response might include, supported by examiner commentary and conclusions. As these responses have not been through full moderation and do not replicate student work, they have not been graded and are instead, banded medium or high to give an indication of the level of each response. Please note that this resource is provided for advice and guidance only and does not in any way constitute an indication of grade boundaries or endorsed answers. Candidate Style Answers (Medium) 3
4 Unit F321 Atoms, Bonds and Groups Medium banded response Question 1 (a) 1 The Group 7 element bromine was discovered by Balard in Bromine gets its name from the Greek bromos meaning stench. (a) Bromine consists of a mixture of two isotopes, 79 Br and 81 Br. (i) What is meant by the term isotopes? [1] Atoms with a different number of neutrons (ii) Complete the table below to show the atomic structures of the bromine isotopes. [2] protons neutrons electrons 79 Br Br (iii) Write the full electronic configuration of a bromine atom. [1] 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4p 6 5s 2 5p 6 6s 1 The definition of isotopes is insufficient; atoms of different elements have different numbers of neutrons. The particles are all correct in (ii). The electronic structure, a more difficult example, is missing any d-electrons. Candidate Style Answers (Medium) 4
5 Question 1 (b) (b) A student added an aqueous solution of sodium iodide to a solution of bromine. The colour turned from orange to a deep brown. The student then added an aqueous solution of sodium chloride to a solution of bromine. The orange colour was unchanged. (i) Explain these observations. In your answer, you should use appropriate technical terms, spelled correctly. [3] In the first experiment bromine displaced iodine. In the second experiment nothing happens. This proves that chlorine is most reactive, then bromine, then iodine. (ii) Write an ionic equation for the reaction that has taken place. [1] I Br - Br I - The response in part (i) makes no reference to iodide (ions). No conclusions are made from the individual experiments, but the overall order of reactivity is given. The equation is incorrect. Question 1 (c) (c) A student read about possible health problems arising from the use of common salt added to different foods. The student decided to compare the salt content of different foods using simple test-tube tests to test the chloride content. Plan a simple qualitative experiment to compare the quantity of chloride ions in different foods. Comment on the validity of claiming that the chloride content is the same as the salt content. [4] I would add silver nitrate solution to each food sample. A white precipitate of silver chloride would form if there were chloride ions in the food. Ag + + Cl - AgCl This would tell you how much chloride there was in the food, not how much salt there was. Candidate Style Answers (Medium) 5
6 The answer clearly covers the test for chloride ions and its result, despite the fact that the food has not been made into a solution. However there is no attempt to compare the results for different foods and the comment about chloride and salt is irrelevant. Question 2 (a) 2 This question refers to the elements in the first four periods of the Periodic Table. H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr (a) Identify an element from the first four periods that fits each of the following descriptions. (i) The element that forms a 2 ion with the same electronic configuration as Ar. [1] 0 (ii) The element that forms a 3+ ion with ten electrons. [1] Al (iii) An element that forms a compound with fluorine with trigonal planar molecules. B [1] (iv) The element that forms a chloride XCl 2 with a molar mass of g mol 1. [1] Ca (v) The element with the largest atomic radius. [1] Kr (vi) The element with the smallest first ionisation energy. [1] Kr Candidate Style Answers (Medium) 6
7 In (i) O has been incorrectly selected: although it does form an O 2- ion, it is not in Period 3. The candidate has made the common error that the heaviest atom must be the largest in (v) and gone on to assume that it will therefore have the lowest ionisation energy in (vi). The other three answers are correct. Question 2 (b) (b) Ionisation energies provide information about the model for the electron structure of elements. (i) Explain why first ionisation energies show a general increase across Period 3, Na Ar. [3] As you go across a period, protons are added to the nucleus, pulling the electrons in. (ii) Write an equation, including state symbols, to represent the third ionisation energy of sodium. [1] Na(g) -> Na 3+ (g) + 3e - (g) (iii) Element X is in Period 3 of the Periodic Table, Na Ar. The first six ionisation energies of an element X are shown below. ionisation number 1st 2nd 3rd 4th 5th 6th ionisation energy /kj mol 1 Predict, with reasons, the identity of element X. [2] The big jump in numbers between 4 th and 5 th means it is in Group 4 with 4 electrons in its outer shell, so it must be silicon. In (i), the increasing number of protons in the nucleus and for the pulling in, which is equivalent to a decrease in atomic radius, are both given. In (ii) there is the common error of combining the first three ionisation energies. The very basic answer to (iii) covers the marking points. Candidate Style Answers (Medium) 7
8 Question 3 (a) 3 Chemists have developed models for bonding and structure. These models are used to explain different properties of metals and non-metals. (a) (i) Draw a labelled diagram to show the currently accepted model for metallic bonding. [2] (ii) What feature of this model allows metals to conduct electricity? [1] The electrons can move. The drawing of a giant metallic structure is good but the nuclei label is incorrect. Part (ii) is correct. Question 3 (b) (b) The metal magnesium reacts with the non-metal chlorine to form a compound magnesium chloride, MgCl 2, which has ionic bonding. (i) State what is meant by an ionic bond. [1] Electrons are transferred from one atom to another. (ii) Dot-and-cross diagrams are used to model which electrons are present in the ion. Draw a dot-and-cross diagram, including outer electron shells only, to show the ions present in magnesium chloride, MgCl 2. [2] Candidate Style Answers (Medium) 8
9 (iii) A student finds that solid magnesium chloride and pure water do not conduct electricity. The student dissolved the magnesium chloride in the water and the resulting solution does conduct electricity. Explain these observations. [3] In solid magnesium chloride and pure water there are no ions. In magnesium chloride solution there are ions. The definition of ionic bonding shows a common misconception, this is not the definition. The dot and cross diagram shows another common error, with magnesium chloride being drawn as a covalent molecule. In part (iii), although the candidate gives an explanation of why water does not conduct electricity, the candidate clearly believes that the ions are only formed when the solid dissolves in water. Question 3 (c) (c) The non-metals chlorine and carbon have very different boiling points. Chlorine is a gas at room temperature but carbon does not boil until well over 4500 o C. Explain this difference, in terms of bonding and structure. In your answer, you should use appropriate technical terms, spelled correctly. [3] Chlorine is a gas because it s made of little molecules with weak forces between the molecules. Carbon is a giant structure with strong bonds. It s easier to break weak bonds. The answer is just too vague. There is no mention of van des Waals or intermolecular forces. Neither are covalent bonds mentioned. However, there is some idea of comparison of the bond strengths. Candidate Style Answers (Medium) 9
10 Question 4 (a) 4 Calcium and its compounds, have properties typical of Group 2 in the Periodic Table. (a) Calcium carbonate, CaCO 3, reacts with acids such as nitric acid. A student neutralised 2.68 g of CaCO 3 with 2.50 mol dm 3 nitric acid, HNO 3. The equation for this reaction is shown below. CaCO 3 (s) + 2HNO 3 (aq) Ca(NO 3 ) 2 (aq) + CO 2 (g) + H 2 O(l) (i) Determine the amount, in mol, of CaCO 3 reacted. [2] Mol CaCO 3 = 2.68/100 = (ii) Calculate the volume, in cm 3, of CO 2 produced at room temperature and pressure. [1] Volume CO 2 = x = 643 cm 3 (iii) Calculate the volume of 2.50 mol dm 3 HNO 3 needed to neutralise 2.68 g of CaCO 3. [2] Mol HNO 3 = 2 x = Volume of HNO 3 = x 2.5 = cm 3 The candidate did not use their data sheet and therefore got the relative formula mass as 100 rather than They lost the first mark but carried their error forward to pick up the second mark. Part (ii) is correct. In (iii) they calculate the number of moles correctly but cannot then continue to a correct volume of nitric acid. Candidate Style Answers (Medium) 10
11 Question 4 (b) (b) The student left the solution of calcium nitrate formed in (a) to crystallise. Crystals of hydrated calcium nitrate formed containing 30.50% of H 2 O, by mass. Calculate the formula of the hydrated calcium nitrate. [3] Mol Ca(NO 3 ) 2 = 69.50/82 = Mol H 2 O = 30.50/18 = Ratio = : = 1:2 Formula is Ca(NO 3 ) 2.2H 2 O Despite the incorrect answer, the only error is the incorrect rfm for calcium nitrate, where the candidate appears to have used atomic numbers. Both other marks can be awarded consequentially, as the candidate has shown all their working. Question 4 (c) (c) A student prepared an aqueous solution of calcium chloride by reacting calcium with hydrochloric acid. Ca(s) + 2HCl(aq) CaCl 2 (aq) + H 2 (g) (i) Using oxidation numbers, show that this is a redox reaction. [2] Calcium s oxidation number has gone up from 0 to 2. Hydrogen s has gone down. (ii) The student had added the exact amount of calcium required to react with the hydrochloric acid used. After carrying out the experiment, the student accidentally added some more calcium. The student was surprised that the extra calcium still reacted. Explain this observation. Include an equation in your answer. [2] Ca +2H 2 O Ca(OH) 2 + H 2 Candidate Style Answers (Medium) 11
12 In the first part hydrogen s oxidation numbers are not given. In the second part there is no written answer, but the mark scheme accepts the correct equation. Question 5 (a) 5 Water, ammonia and sulfur dioxide are simple molecular compounds. (a) Pairs of electrons in molecules may be present as bonding pairs or as lone pairs. (i) Complete the table below for water, ammonia and sulfur dioxide. [2] molecule H 2 O NH 3 SO 2 number of bonding pairs of electrons number of lone pairs of electrons around central atom (two double bonds) (ii) Use your answers to a(i) to help you draw the shape of, and bond angle in, a molecule of NH 3 and of SO 2. molecule NH 3 SO 2 shape of molecule with bond angles [4] The numbers of bonding and lone pairs are correct in (i). The ammonia molecule is drawn as trigonal planar, ignoring the lone pair. Sulfur dioxide is one of the analogous molecules referred to in the specification and this candidate has assumed that it is like carbon dioxide, losing these marks. Candidate Style Answers (Medium) 12
13 Question 5 (b) (b) Water forms hydrogen bonds which influences its properties. Explain, with a diagram, what is meant by hydrogen bonding and explain two anomalous properties of water resulting from hydrogen bonding. [6] Oxygen is very electronegative polarising the bonds. Ice floats on top of water. Water a higher melting point than expected. Paper Total [60] The diagram is wrong, as the hydrogen bond is between two hydrogens. However the dipoles are correct. The density is described, without explanation. Similarly, the statement that water s melting point is higher than expected is correct, but again there is no explanation. Overall This candidate has scored about half of the available marks. Candidate Style Answers (Medium) 13
Candidate Style Answer
Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching
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