9.6. Extraction of metals
A subsection of Chemistry, 0620, through 9. Metals
Listing 10 of 311 questions
The reactivity of different metal oxides was compared by heating them with metals in a crucible. heat mixture of metal oxide and metal The results are shown in the table below. mixture observations iron oxide + zinc reacts lead oxide + iron reacts magnesium oxide + zinc no reaction Use the results in the table to suggest the order of reactivity of the metals iron, lead, magnesium and zinc. most reactive least reactive Predict whether iron will react with zinc oxide. Explain your answer. Which two of the following statements about metals are correct? Tick two boxes. Metals conduct electricity and heat. All Group IV elements show metallic properties. Magnesium is extracted by heating its oxide with carbon. All metals have high densities. Iron is a transition element. Sand and salt (sodium chloride) are both solids. Describe the arrangement and movement of the particles in a solid. arrangement movement Describe how you could separate the sand from a mixture of sand and salt. Give full details of how this is carried out. The diagram below shows the apparatus used to separate ethanol and water from a mixture of ethanol and water. heat ethanol and water fractionating column water out water in Complete the following sentences about this separation using words from the list below. condenser crystallisation distillation fl ask heavy higher lower solid volatile vapour Fractional is used to separate a mixture of water and ethanol. The temperature at the top of the fractionating column is than the temperature at the bottom. The more liquid evaporates and moves further up the column. It eventually reaches the where the changes to a liquid.
0620_w12_qp_21
THEORY
2012
Paper 2, Variant 1
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Aluminium is obtained by the reduction of aluminium ions to aluminium atoms. Write an ionic equation for the reduction of an aluminium ion to an aluminium atom. The original method of extracting aluminium involved the reduction of aluminium chloride using the reactive metal sodium. Aluminium obtained by this method was very expensive due to the high cost of extracting sodium from sodium chloride. Complete the equation for this reduction. Al Cl 3 + Na → + How can sodium metal be obtained from sodium chloride? In the modern method, aluminium is obtained by the electrolysis of aluminium oxide dissolved in molten cryolite, Na3Al F6. carbon cathode (–) carbon anode (+) mixture of aluminium oxide and cryolite molten aluminium waste gases, O2, CO2, CO, F2 The major ore of aluminium is impure aluminium oxide. What is the name of this ore? This ore is a mixture of aluminium oxide, which is amphoteric, and iron(oxide which is basic. Explain how these two oxides can be separated by the addition of aqueous sodium hydroxide. Give two reasons why the electrolyte contains cryolite. The mixture of gases evolved at the positive electrode includes: carbon dioxide carbon monoxide fl uorine oxygen Explain the presence of these gases in the gaseous mixture formed at the positive electrode. Include at least one equation in your explanation. A major use of aluminium is the manufacture of pots and pans. One reason for this is its resistance to corrosion. Explain why aluminium, a reactive metal, is resistant to corrosion. Suggest two other reasons why aluminium is suitable for making pots and pans.
0620_w14_qp_32
THEORY
2014
Paper 3, Variant 2
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Iron is a metal. The equation for the reaction of iron with steam is shown. 3Fe + 4H2O → Fe3O4 + 4H2 Which substance is reduced in this reaction? Explain your answer. Iron is extracted by heating iron ore with carbon in a blast furnace. What is the meaning of the term ore? Air is blown into the blast furnace. What is the purpose of this air? The impurities in the iron ore are removed as slag. Which one of the following is slag? Tick one box. iron(oxide calcium silicate calcium carbonate coke Slag is less dense than iron. The diagram shows a blast furnace used to extract iron. On the diagram, write the letter S to show where the slag is removed. mixture including iron ore Iron from the blast furnace contains impurities. The diagram shows a converter used to make steel from iron. molten iron from blast furnace Describe how iron is converted into steel. In your answer • describe the impurities present, • describe how the impurities are removed, • include a relevant word equation.
0620_w16_qp_32
THEORY
2016
Paper 3, Variant 2
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Tin is a metallic element in Group IV. Its main ore is cassiterite which is an impure form of tin(oxide, SnO2. Tin also occurs in stannite, Cu2FeSnS4. Calculate the relative formula mass, Mr, of Cu2FeSnS4. Mr of Cu2FeSnS4 = The Mr of SnO2 is 151. Calculate the percentage of tin by mass in SnO2. percentage of tin by mass in SnO2 = The percentage of tin by mass in Cu2FeSnS4 is 27.6%. Use this information and your answer to to suggest whether it would be better to extract tin from SnO2 or Cu2FeSnS4. Explain your answer. Tin can be extracted by heating tin(oxide with carbon. Carbonmonoxide is the other product. Write a chemical equation for this reaction. The position of tin in the reactivity series is shown. iron most reactive tin copper least reactive A student added iron to a solution containing Sn2+ ions. The student then separately added tin to a solution containing Cu2+ ions. Complete the ionic equations. If there is no reaction write ‘no reaction’. Fe + Sn2+ Sn + Cu2+ Copper(nitrate, Cu(NO3)2, decomposes when it is heated. The only solid product is copper(oxide, CuO. There are two gaseous products. One of the gaseous products is oxygen. Describe a test for oxygen. test result  Name the other gaseous product. Describe its appearance. name appearance  Write a chemical equation for the thermal decomposition of copper(nitrate. Iron does not rust when it is completely coated with zinc. When the zinc is scratched, the iron still does not rust. Explain why the iron does not rust when it is completely coated with zinc. Explain why the iron still does not rust when the zinc is scratched.
0620_w18_qp_43
THEORY
2018
Paper 4, Variant 3
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Zinc is extracted from an ore containing zinc sulfide. State the name of this zinc ore. This ore is converted to zincoxide, ZnO. Zincoxide is then reacted with carbon. Write a chemical equation for the reaction of zincoxide with carbon. State what type of chemical change happens to the zinc in zincoxide in this reaction. Explain your answer. chemical change explanation  Explain why aluminium is not extracted from aluminiumoxide by heating with carbon. Suggest an alternative method for the extraction of zinc from zincoxide. Brass is an alloy of zinc. Explain, in terms of particles, why brass is harder than pure zinc. 
0620_w20_qp_41
THEORY
2020
Paper 4, Variant 1
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Questions Discovered
311