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electric current to decompose an ionic compound into simpler substances, because its ions move towards oppositely charged electrodes."},{"text":"Distillation decomposes an ionic compound using an electric current.","correct":false,"explanation":"Distillation separates substances using differences in boiling point; it does not use electricity to decompose ionic compounds. The correct process is electrolysis."},{"text":"Neutralisation decomposes an ionic compound using an electric current.","correct":false,"explanation":"Neutralisation is the reaction between an acid and a base, not decomposition by electricity. The process that decomposes an ionic compound using current is electrolysis."},{"text":"Filtration decomposes an ionic compound using an electric current.","correct":false,"explanation":"Filtration separates an insoluble solid from a liquid and does not involve an electric current. Electrolysis is the process that decomposes an ionic compound electrically."}]},{"id":"997307b8-cb2d-480f-b5c9-f049edebefd8","cardType":"basic","points":1,"front":"How does carbon reduction extract a metal?","back":"Carbon reduction removes oxygen from a metal compound using carbon.","mcqOptions":[{"text":"Carbon reduction removes oxygen from a metal compound using carbon.","correct":true,"explanation":"Carbon reduction extracts a metal by reacting carbon with its compound. Carbon removes the oxygen, leaving the metal behind."},{"text":"Carbon oxidation adds oxygen to a metal compound using carbon.","correct":false,"explanation":"Carbon is oxidised while removing oxygen from a metal compound; it does not add oxygen to the compound. The correct process is carbon reduction."},{"text":"Electrolysis removes oxygen from a metal compound using carbon.","correct":false,"explanation":"Electrolysis uses an electric current rather than carbon to extract metals. Removing oxygen from a metal compound with carbon is called carbon reduction."},{"text":"Carbon reduction removes carbon from a metal compound using oxygen.","correct":false,"explanation":"The extraction reaction removes oxygen from the metal compound using carbon, rather than removing carbon with oxygen. This process is carbon reduction."}]},{"id":"1530badb-b546-4aab-9a2f-57471886371d","cardType":"basic","points":2,"front":"Why cannot metals more reactive than carbon be extracted using carbon?","back":"Metals above carbon in the reactivity series cannot be extracted by carbon reduction.","mcqOptions":[{"text":"Metals above carbon in the reactivity series cannot be extracted by carbon reduction.","correct":true,"explanation":"Metals above carbon are more reactive than carbon, so their compounds are too stable for carbon to remove the oxygen. They require electrolysis instead."},{"text":"Metals below carbon in the reactivity series cannot be extracted by carbon reduction.","correct":false,"explanation":"Metals below carbon are less reactive and can usually be extracted by carbon reduction. It is metals above carbon that cannot be extracted this way."},{"text":"Metals next to carbon in the reactivity series cannot be extracted by carbon reduction.","correct":false,"explanation":"Position next to carbon is not the deciding factor; relative reactivity is. Metals above carbon cannot be reduced by carbon, whereas metals below it can."},{"text":"All metals in the reactivity series cannot be extracted by carbon reduction.","correct":false,"explanation":"Carbon reduction can extract metals below carbon in the reactivity series. Only metals more reactive than carbon cannot be extracted by this method."}]},{"id":"465bccec-f773-4513-b10a-d8008eec3cc9","cardType":"basic","points":1,"front":"How are metals more reactive than carbon extracted?","back":"They require electrolysis of a molten compound.","mcqOptions":[{"text":"They require electrolysis of a molten compound.","correct":true,"explanation":"Metals more reactive than carbon cannot be reduced by carbon, so their molten ionic compounds must be electrolysed to release the metal."},{"text":"They require carbon reduction of a molten compound.","correct":false,"explanation":"Carbon cannot remove oxygen from compounds of metals more reactive than itself. These metals are extracted by electrolysis of a molten compound."},{"text":"They require electrolysis of an aqueous compound.","correct":false,"explanation":"An aqueous solution can contain water that is preferentially discharged instead of the very reactive metal. The compound is therefore electrolysed when molten."},{"text":"They require heating of a solid compound.","correct":false,"explanation":"Heating alone does not provide the charged particles and electrode reactions needed for these extractions. Electrolysis of the molten compound is required."}]},{"id":"fb22b137-f938-4744-8e28-6d3d4c2e8304","cardType":"basic","points":2,"front":"Why must the ionic compound be molten during electrolysis?","back":"The compound must be molten so its ions can move to the electrodes.","mcqOptions":[{"text":"The compound must be molten so its ions can move to the electrodes.","correct":true,"explanation":"When molten, the ionic lattice is broken and the ions are free to move. This allows them to reach the electrodes and be discharged."},{"text":"The compound must be solid so its ions can move to the electrodes.","correct":false,"explanation":"Ions are fixed in position in a solid ionic lattice and cannot reach the electrodes. Melting frees the ions so electrolysis can occur."},{"text":"The compound must be aqueous so its atoms can move to the electrodes.","correct":false,"explanation":"Electrolysis involves ions, not neutral atoms, moving to electrodes. For highly reactive metals, the ionic compound must be molten rather than aqueous."},{"text":"The compound must be gaseous so its molecules can move to the electrodes.","correct":false,"explanation":"The compound must provide mobile ions, not simply moving molecules. Melting the ionic compound allows its ions to travel to the electrodes."}]},{"id":"24daeed4-46f8-487c-aa38-844fbe877772","cardType":"basic","points":1,"front":"Which metals can be extracted by carbon reduction?","back":"Carbon reduction works only for metals below carbon in the reactivity series.","mcqOptions":[{"text":"Carbon reduction works only for metals below carbon in the reactivity series.","correct":true,"explanation":"Metals below carbon are less reactive than carbon, so carbon can remove oxygen from their compounds and leave the metal."},{"text":"Carbon reduction works only for metals above carbon in the reactivity series.","correct":false,"explanation":"Metals above carbon hold oxygen more strongly and cannot be reduced by carbon. Carbon reduction works for metals below carbon."},{"text":"Electrolysis works only for metals below carbon in the reactivity series.","correct":false,"explanation":"Electrolysis is used especially for metals above carbon, while less reactive metals can be extracted by carbon reduction. The question asks about carbon reduction."},{"text":"Carbon reduction works only for non-metals below carbon in the reactivity series.","correct":false,"explanation":"The reactivity series compares metals, and carbon reduction extracts metals below carbon. Non-metals are not the relevant class in this extraction rule."}]},{"id":"961b6fa3-5b5f-45ff-b538-a26752b91820","cardType":"basic","points":2,"front":"Why is electrolysis more expensive than carbon reduction?","back":"Electrolysis is more expensive because it requires large amounts of energy.","mcqOptions":[{"text":"Electrolysis is more expensive because it requires large amounts of energy.","correct":true,"explanation":"Electrolysis requires a continuous supply of electrical energy to drive the extraction reactions. Carbon reduction generally uses less costly heating and chemical reactions."},{"text":"Electrolysis is more expensive because it requires large amounts of carbon.","correct":false,"explanation":"Carbon consumption is associated with carbon reduction, not the main reason electrolysis is expensive. Electrolysis costs more because it requires large amounts of electrical energy."},{"text":"Electrolysis is more expensive because it produces large amounts of oxygen.","correct":false,"explanation":"Oxygen production is a reaction product, not the main cost. The greater expense comes from supplying the large amount of electrical energy needed."},{"text":"Electrolysis is more expensive because it requires large amounts of water.","correct":false,"explanation":"Water is not the essential reactant in extracting these metals by electrolysis. The process is expensive because it consumes substantial electrical energy."}]},{"id":"ebb03cd5-6d4f-4c9d-8fbf-8bd8c87f7108","cardType":"basic","points":1,"front":"Which compound is electrolysed to extract aluminium?","back":"Aluminium is extracted from aluminium oxide, $\\text{Al}_2\\text{O}_3$.","mcqOptions":[{"text":"Aluminium is extracted from aluminium oxide, $\\text{Al}_2\\text{O}_3$.","correct":true,"explanation":"Aluminium oxide contains aluminium ions and oxide ions, so electrolysis of molten $\\text{Al}_2\\text{O}_3$ produces aluminium at the cathode."},{"text":"Aluminium is extracted from aluminium chloride, $\\text{AlCl}_3$.","correct":false,"explanation":"Aluminium is extracted industrially from aluminium oxide, not aluminium chloride. The compound used is $\\text{Al}_2\\text{O}_3$, electrolysed when molten."},{"text":"Aluminium is extracted from aluminium carbonate, $\\text{Al}_2(\\text{CO}_3)_3$.","correct":false,"explanation":"Aluminium extraction uses aluminium oxide, $\\text{Al}_2\\text{O}_3$. Aluminium carbonate is not the compound named for the industrial electrolysis process."},{"text":"Aluminium is extracted from aluminium hydroxide, $\\text{Al(OH)}_3$.","correct":false,"explanation":"Aluminium hydroxide is not the compound electrolysed in the extraction process. Aluminium is extracted from aluminium oxide, $\\text{Al}_2\\text{O}_3$."}]},{"id":"ce019765-6964-4744-bc0d-3eef1e38e9c0","cardType":"basic","points":1,"front":"Why would melting aluminium oxide alone use a great deal of energy?","back":"Aluminium oxide has a very high melting point.","mcqOptions":[{"text":"Aluminium oxide has a very high melting point.","correct":true,"explanation":"Aluminium oxide has a very high melting point, so melting it alone would require a large energy input before electrolysis could begin."},{"text":"Aluminium oxide has a very low melting point.","correct":false,"explanation":"A low melting point would make melting relatively easy and would not explain the high energy requirement. Aluminium oxide has a very high melting point."},{"text":"Aluminium oxide has a very high boiling point.","correct":false,"explanation":"The process requires melting, so the relevant property is melting point rather than boiling point. Aluminium oxide has a very high melting point."},{"text":"Aluminium oxide has a very low electrical conductivity.","correct":false,"explanation":"The major energy issue described here is the energy needed to melt aluminium oxide, because its melting point is very high."}]},{"id":"e60c4783-420b-412a-9f38-f1d36ffeeb83","cardType":"basic","points":2,"front":"Why is aluminium oxide dissolved in molten cryolite?","back":"Cryolite lowers the operating temperature, reducing the energy cost.","mcqOptions":[{"text":"Cryolite lowers the operating temperature, reducing the energy cost.","correct":true,"explanation":"Dissolving aluminium oxide in molten cryolite lowers the mixture’s operating temperature, so less energy is needed to keep the electrolyte molten."},{"text":"Cryolite raises the operating temperature, increasing the energy cost.","correct":false,"explanation":"Cryolite is added to lower, not raise, the operating temperature. This reduces the energy needed to maintain the molten electrolyte."},{"text":"Cryolite changes the electrolysis products, reducing the energy cost.","correct":false,"explanation":"Cryolite lowers the operating temperature but does not change the products formed. Aluminium and oxygen are still produced during electrolysis."},{"text":"Cryolite removes the aluminium ions, reducing the energy cost.","correct":false,"explanation":"Cryolite acts as a solvent that lowers the operating temperature; it does not remove aluminium ions. Aluminium ions remain available for reduction at the cathode."}]},{"id":"6b91b42a-2199-4559-9291-0a969a5e6c79","cardType":"basic","points":2,"front":"What is cryolite's purpose in aluminium extraction?","back":"Cryolite saves energy; it does not change the electrolysis products.","mcqOptions":[{"text":"Cryolite saves energy; it does not change the electrolysis products.","correct":true,"explanation":"Cryolite lowers the operating temperature of the electrolyte, saving energy, while the electrolysis products remain aluminium and oxygen."},{"text":"Cryolite saves carbon; it does not change the electrolysis products.","correct":false,"explanation":"Cryolite’s key benefit is reducing the energy needed for the process, not saving carbon. It lowers the operating temperature without changing the products."},{"text":"Cryolite produces energy; it does not change the electrolysis products.","correct":false,"explanation":"Cryolite does not generate energy. It reduces energy consumption by lowering the operating temperature of the molten electrolyte."},{"text":"Cryolite saves energy; it changes the electrolysis products.","correct":false,"explanation":"Cryolite saves energy by lowering the operating temperature, but it does not alter the products formed at the electrodes."}]},{"id":"059c968d-cf2f-45b8-9fc1-6915a1c66c63","cardType":"basic","points":2,"front":"What happens to aluminium ions at the cathode?","back":"Aluminium ions gain electrons to form molten aluminium: $\\text{Al}^{3+} + 3\\text{e}^{-} \\rightarrow \\text{Al}$.","mcqOptions":[{"text":"Aluminium ions gain electrons to form molten aluminium: $\\text{Al}^{3+} + 3\\text{e}^{-} \\rightarrow \\text{Al}$.","correct":true,"explanation":"At the cathode, positive aluminium ions are attracted to the negative electrode and gain three electrons. This reduction forms molten aluminium."},{"text":"Aluminium ions lose electrons to form molten aluminium: $\\text{Al}^{3+} \\rightarrow \\text{Al} + 3\\text{e}^{-}$.","correct":false,"explanation":"Positive aluminium ions gain electrons at the cathode; losing electrons would oxidise them and cannot produce neutral aluminium. The correct equation includes three electrons on the left."},{"text":"Aluminium ions gain electrons to form molten aluminium: $\\text{Al}^{3+} + 3\\text{e}^{-} \\rightarrow \\text{Al}^{3-}$.","correct":false,"explanation":"Gaining three electrons neutralises $\\text{Al}^{3+}$ to form aluminium atoms, not $\\text{Al}^{3-}$. The product is neutral molten aluminium."},{"text":"Aluminium atoms gain electrons to form molten aluminium: $\\text{Al} + 3\\text{e}^{-} \\rightarrow \\text{Al}^{3+}$.","correct":false,"explanation":"The species present before discharge is the aluminium ion, not a neutral aluminium atom. It gains electrons to become neutral aluminium: $\\text{Al}^{3+} + 3\\text{e}^{-} \\rightarrow \\text{Al}$."}]},{"id":"515859e8-895e-44be-9ce1-de8380fc6d5f","cardType":"basic","points":2,"front":"What happens to oxide ions at the anode?","back":"Oxide ions lose electrons to form oxygen gas: $2\\text{O}^{2-} \\rightarrow \\text{O}_2 + 4\\text{e}^{-}$.","mcqOptions":[{"text":"Oxide ions lose electrons to form oxygen gas: $2\\text{O}^{2-} \\rightarrow \\text{O}_2 + 4\\text{e}^{-}$.","correct":true,"explanation":"At the anode, negative oxide ions lose electrons in oxidation. Two oxide ions combine to form one oxygen molecule and release four electrons."},{"text":"Oxide ions gain electrons to form oxygen gas: $2\\text{O}^{2-} + 4\\text{e}^{-} \\rightarrow \\text{O}_2$.","correct":false,"explanation":"Oxide ions are oxidised at the anode, so they lose rather than gain electrons. The correct equation releases four electrons: $2\\text{O}^{2-} \\rightarrow \\text{O}_2 + 4\\text{e}^{-}$."},{"text":"Oxide ions lose electrons to form oxygen gas: $\\text{O}^{2-} \\rightarrow \\text{O} + 2\\text{e}^{-}$.","correct":false,"explanation":"The extraction produces oxygen molecules, $\\text{O}_2$, so two oxide ions are needed. The balanced equation releases four electrons overall."},{"text":"Oxide ions lose electrons to form hydrogen gas: $2\\text{O}^{2-} \\rightarrow \\text{H}_2 + 4\\text{e}^{-}$.","correct":false,"explanation":"Oxide ions contain oxygen and form oxygen gas at the anode, not hydrogen. Hydrogen would require hydrogen-containing ions, which are not the reacting anions here."}]},{"id":"e1e59e2f-297d-4726-b411-af325497d5aa","cardType":"basic","points":2,"front":"Why do carbon anodes burn away during aluminium extraction?","back":"The oxygen reacts with the hot carbon anodes to form carbon dioxide.","mcqOptions":[{"text":"The oxygen reacts with the hot carbon anodes to form carbon dioxide.","correct":true,"explanation":"Oxygen produced at the anode reacts with the hot carbon electrode. This forms carbon dioxide, gradually consuming the carbon anode."},{"text":"The oxygen reacts with the hot carbon anodes to form carbon monoxide.","correct":false,"explanation":"Carbon monoxide can form in some incomplete combustion conditions, but the stated product in aluminium extraction is carbon dioxide. The carbon anodes therefore burn away."},{"text":"The oxygen reacts with the hot carbon anodes to form aluminium oxide.","correct":false,"explanation":"Aluminium oxide is the electrolyte being decomposed, not the product formed when oxygen attacks carbon. The carbon anodes react with oxygen to form carbon dioxide."},{"text":"The oxygen reacts with the hot carbon anodes to form methane.","correct":false,"explanation":"Methane requires hydrogen as well as carbon, and no suitable hydrogen source is involved at the carbon anode. Oxygen oxidises the carbon to carbon dioxide."}]},{"id":"6a826e94-8b30-4c26-9af4-2e55efebe012","cardType":"cloze","points":null,"front":"Metals [ ] require electrolysis for extraction.","back":"Metals more reactive than carbon require electrolysis for extraction.","mcqOptions":[{"text":"more reactive than carbon","correct":true,"explanation":"Metals more reactive than carbon form compounds from which carbon cannot remove oxygen. Their molten compounds therefore require electrolysis for extraction."},{"text":"less reactive than carbon","correct":false,"explanation":"Metals less reactive than carbon can generally be extracted by carbon reduction because carbon can remove oxygen from their compounds. The blank requires “more reactive than carbon”."},{"text":"at the same reactivity as carbon","correct":false,"explanation":"The extraction rule concerns metals positioned above carbon, meaning more reactive than carbon. Metals at the same level are not the intended category."},{"text":"with a lower melting point than carbon","correct":false,"explanation":"Melting point does not determine whether electrolysis is required. The relevant factor is reactivity: metals more reactive than carbon need electrolysis."}]},{"id":"fe6fb855-187e-463e-8cba-584c1826eb2a","cardType":"cloze","points":null,"front":"Carbon reduction works for metals [ ].","back":"Carbon reduction works for metals below carbon in the reactivity series.","mcqOptions":[{"text":"below carbon in the reactivity series","correct":true,"explanation":"Carbon reduction works for metals below carbon because they are less reactive, allowing carbon to remove oxygen from their compounds during extraction."},{"text":"above carbon in the reactivity series","correct":false,"explanation":"Metals above carbon are more reactive and cannot usually be reduced by carbon. They require electrolysis instead, so the correct term is “below carbon in the reactivity series”."},{"text":"beside carbon in the reactivity series","correct":false,"explanation":"The rule depends on whether a metal is above or below carbon, not simply beside it. Metals below carbon are the ones suitable for carbon reduction."},{"text":"below hydrogen in the reactivity series","correct":false,"explanation":"Hydrogen’s position is not the criterion for carbon reduction in this rule. Carbon reduction works for metals below carbon in the reactivity series."}]},{"id":"841dc133-76b8-470b-956a-297a1779f5f7","cardType":"cloze","points":null,"front":"The compound is molten because its [ ] to the electrodes.","back":"The compound is molten because its ions are free to move to the electrodes.","mcqOptions":[{"text":"ions are free to move","correct":true,"explanation":"Molten ionic compounds contain charged ions that can move through the liquid towards the electrodes, allowing the ions to carry charge and undergo electrolysis."},{"text":"ions are unable to move","correct":false,"explanation":"Solid ionic compounds have fixed ions, but molten compounds have mobile ions. The correct answer is that ions are free to move to the electrodes."},{"text":"electrons are free to move","correct":false,"explanation":"Electrons are not the mobile charged particles in the molten ionic compound. The correct answer is that ions are free to move to the electrodes."},{"text":"atoms are free to move","correct":false,"explanation":"The particles moving to the electrodes are charged ions, not neutral atoms. The correct answer is that ions are free to move through the molten compound."}]},{"id":"bbebaa76-276f-4e78-a468-5a4e66197e6a","cardType":"cloze","points":null,"front":"Molten cryolite [ ] of aluminium extraction.","back":"Molten cryolite lowers the operating temperature of aluminium extraction.","mcqOptions":[{"text":"lowers the operating temperature","correct":true,"explanation":"Cryolite dissolves aluminium oxide and lowers the temperature needed for electrolysis, reducing the energy required to keep the electrolyte molten during aluminium extraction."},{"text":"raises the operating temperature","correct":false,"explanation":"Raising the temperature would increase energy use rather than make extraction more efficient. The correct answer is that molten cryolite lowers the operating temperature."},{"text":"increases the electrical resistance","correct":false,"explanation":"Increasing resistance would make electrolysis less efficient by causing more energy loss. The correct answer is that molten cryolite lowers the operating temperature."},{"text":"removes the need for electrolysis","correct":false,"explanation":"Cryolite helps aluminium oxide melt at a lower temperature but does not replace the electrolysis process. The correct answer is that it lowers the operating temperature."}]},{"id":"230238d9-73ac-465b-9ac5-76ff208bf351","cardType":"cloze","points":null,"front":"At the cathode, aluminium ions are [ ] to aluminium.","back":"At the cathode, aluminium ions are reduced to aluminium.","mcqOptions":[{"text":"reduced","correct":true,"explanation":"At the cathode, aluminium ions gain electrons to form aluminium atoms. Gaining electrons is reduction, so aluminium ions are reduced to aluminium."},{"text":"oxidised","correct":false,"explanation":"Oxidation involves losing electrons, which happens at the anode. At the cathode, aluminium ions gain electrons, so the correct answer is reduced."},{"text":"neutralised","correct":false,"explanation":"Neutralisation is a reaction between an acid and a base, not the electron gain occurring at the cathode. Aluminium ions are reduced by gaining electrons."},{"text":"decomposed","correct":false,"explanation":"Decomposition describes breaking a compound into simpler substances, but it does not identify the electron transfer at the cathode. Aluminium ions are reduced there."}]},{"id":"01978e84-2d69-4269-b369-bd0e4a67c8e2","cardType":"cloze","points":null,"front":"Carbon anodes must be [ ] because they gradually burn away.","back":"Carbon anodes must be replaced regularly because they gradually burn away.","mcqOptions":[{"text":"replaced regularly","correct":true,"explanation":"Carbon anodes react with oxygen produced at the anode, forming carbon dioxide and gradually being consumed. They must therefore be replaced regularly during extraction."},{"text":"heated continuously","correct":false,"explanation":"The electrolyte is kept molten by heating, but heating does not prevent carbon anodes reacting with oxygen. The correct answer is that they are replaced regularly."},{"text":"coated with copper","correct":false,"explanation":"A copper coating would not stop carbon reacting with oxygen and is not the method used in extraction. Carbon anodes must be replaced regularly as they are consumed."},{"text":"removed before electrolysis","correct":false,"explanation":"Removing the anodes would stop them providing the electrode surface needed for electrolysis. They remain in use and are replaced regularly because they gradually burn away."}]}]}],"examCountdown":{"examDate":"2027-05-17","paperLabel":"Paper 1"},"heading":"4.3.3 Using electrolysis to extract metals","title":"4.3.3 Using electrolysis to extract metals Flashcards","topbar":{"backHref":"/gcse/chemistry/aqa/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"976b36ba-92ea-5561-bb16-ba15bd420a07","walled":"$L38"}],"$L39","$L3a"]