0620_s18_qp_41
A paper of Chemistry, 0620
Questions:
6
Year:
2018
Paper:
4
Variant:
1
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1
Substances can be classified as elements, compounds or mixtures. What is meant by the term compound ? Mixtures can be separated by physical processes. A sequence of physical processes can be used to separate common salt (sodiumchloride) from a mixture containing sand and common salt only. Give the order and the correct scientific term for the physical processes used to separate the common salt from the mixture.  The boiling points of four different alcohols, A, B, C and D, are shown. alcohol A B C D boiling point / °C A student suggested that the apparatus shown could be used to separate the mixture of alcohols. mixture of alcohols A, B, C and D X fractionating column hot water electric heater Apparatus X needs to have cold water flowing through it. ● Draw an arrow on the diagram to show where the cold water enters apparatus X. ● Name apparatus X.  Part of the fractionating column is missing. This means that the experiment will not work. ● Draw on the diagram the part of the fractionating column which is missing. ● Explain why the experiment will not work with this part of the fractionating column missing.  Suggest why a Bunsen burner is not used to heat the flask. A hot water bath cannot be used to separate alcohols C and D. Explain why. 
12. Experimental techniques and chemical analysis  →  12.4. Separation and purification
11. Organic chemistry  →  11.3. Fuels
12. Experimental techniques and chemical analysis  →  12.1. Experimental design
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Flerovium, Fl, atomic number 114, was first made in research laboratories in 1998. Flerovium was made by bombarding atoms of plutonium, Pu, atomic number 94, with atoms of elementZ. ● ● The nucleus of one atom of plutonium combined with the nucleus of one atom of elementZ. ● ● This formed the nucleus of one atom of flerovium. Suggest the identity of elementZ. In which period of the Periodic Table is flerovium? Predict the number of outer shell electrons in an atom of flerovium. Two isotopes of flerovium are 286Fl and 289Fl. The nuclei of both of these isotopes are unstable and emit energy when they split up. State the term used to describe isotopes with unstable nuclei. Complete the table to show the number of protons, neutrons and electrons in the atoms of the isotopes shown. isotope number of protons number of neutrons number of electrons 286Fl 289Fl  Only a relatively small number of atoms of flerovium have been made in the laboratory and the properties of flerovium have not yet been investigated. It has been suggested that flerovium is a typical metal. Suggest two physical properties of flerovium.  Suggest one chemical property of flerovium oxide. 
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
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This question is about iron. Three of the raw materials added to a blast furnace used to extract iron from hematite are coke, hematite and limestone. Name one other raw material added to the blast furnace. A series of reactions occurs in a blast furnace during the extraction of iron from hematite. Describe these reactions. Include: ● ● one chemical equation for the reduction of hematite ● ● one chemical equation for the formation of slag. The iron extracted from hematite using a blast furnace is impure. Identify the main impurity in this iron and explain how it is removed in the steel‑making process. main impurity how it is removed  
9. Metals  →  9.6. Extraction of metals
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This question is about masses, volumes and moles. Which term is defined by the following statement? The average mass of naturally occurring atoms of an element on a scale where the 12C atom has a mass of exactly 12 units. Butane, C4H10, has a relative molecular mass of 58. Potassium fluoride, KF, has a relative formula mass of 58. Explain why the term relative molecular mass can be used for butane but cannot be used for potassiumfluoride. A 0.095 g sample of gaseous element Y occupies 60.0 cm3 at room temperature and pressure. ● ● Determine the number of moles of elementY in 60.0 cm3.  moles of element Y = mol ● ● Calculate the relative molecular mass of elementY and hence suggest the identity of elementY.  relative molecular mass =  identity of element Y =  A 1.68 g sample of phosphorus was burned and formed 3.87 g of an oxide of phosphorus. Calculate the empirical formula of this oxide of phosphorus.  empirical formula = Another oxide of phosphorus has the empirical formula P2O3. One molecule of this oxide of phosphorus contains four atoms of phosphorus. Calculate the mass of one mole of this oxide of phosphorus.  mass = g 
3. Stoichiometry  →  3.2. Relative masses of atoms and molecules
3. Stoichiometry  →  3.3. The mole and the Avogadro constant
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The table gives some chemical properties of transition elements and their compounds, and of GroupI elements and their compounds. chemical property transition elements GroupI elements ability to act as catalysts yes no exist as coloured compounds yes no What is meant by the term catalyst? Give one other chemical property shown by transition elements which is not shown by GroupI elements. Give two physical properties shown by transition elements which are not shown by GroupI elements.  The energy level diagram shows the energy profile for the reaction between zinc and dilute sulfuricacid. energy progress of reaction Zn+ H2SO4Complete the diagram by adding the formulae of the products. Include state symbols. Draw an arrow on the diagram to represent the activation energy. Is the reaction endothermic or exothermic? Explain your answer. The reaction between zinc and dilute sulfuricacid can be catalysed by the addition of aqueous copper(sulfate. On the diagram, add the energy profile for the catalysed reaction. energy progress of reaction Zn+ H2SO4 A student electrolyses aqueous copper(sulfate using the apparatus shown. + – carbon electrodes aqueous copper(sulfate power supply Oxygen gas forms at the positive electrode . Write an ionic half‑equation for the reaction at the negative electrode . Include state symbols. Describe what the student observes at the negative electrode. Give two other observations which the student makes during the electrolysis.  What difference would the student observe at the positive electrode if the aqueous copper(sulfate were replaced by concentrated aqueous copper(chloride? 
4. Electrochemistry  →  4.1. Electrolysis
9. Metals  →  9.4. Reactivity series
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The table shows the structures of four hydrocarbons. P Q R S CH3–CH3 CH2=CH2 CH2=CH–CH3 CH2=CH–CH2–CH3 Why are compounds P, Q, R and S known as hydrocarbons? CompoundP is saturated. What is meant by the term saturated ? CompoundP undergoes a substitution reaction with chlorine. What is meant by the term substitution reaction? State a condition required for this reaction to occur. Write a chemical equation for this reaction. CompoundR undergoes an addition reaction with bromine. Why is this reaction an addition reaction? A compound containing bromine is formed in this reaction. Draw the structure of this compound. Show all of the atoms and all of the bonds.  To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after the live examination series. Draw the structure of an unbranched isomer of compoundS. Show all of the atoms and all of the bonds. Name this unbranched isomer of compoundS. structure name  CompoundQ undergoes polymerisation. Name the polymer formed. Complete the chemical equation to show the polymerisation of compoundQ. n CH2=CH2  Amino acids undergo polymerisation to form proteins. Part of a protein molecule with the linkages missing is shown. Draw the linkages on the diagram. Show all of the atoms and all of the bonds. N H C O  The structure shows an ester. CH2 C O O CH2 CH3 CH2 CH3 Write the word equation for a reaction which could be used to make this ester. 
11. Organic chemistry  →  11.5. Alkenes
11. Organic chemistry  →  11.2. Naming organic compounds
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