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cost less than the value of the metal produced."},{"text":"Any metal or compound for extraction to be economically worthwhile.","correct":false,"explanation":"A rock is not an ore merely because it contains a metal; the amount must be economically worthwhile to extract, rather than simply detectable."},{"text":"No metal or compound for extraction to be economically worthwhile.","correct":false,"explanation":"Economic extraction requires a sufficient concentration of metal or its compound, not a rock containing no useful metal at all."},{"text":"A small amount of metal or compound for extraction to be economically worthwhile.","correct":false,"explanation":"The rock must contain enough valuable material to justify extraction. A small amount of metal would usually make mining uneconomic, not worthwhile."}]},{"id":"ca2a4849-3bae-4622-9512-fb1a95457485","cardType":"basic","points":1,"front":"How does higher metal reactivity affect how it is found in the crust?","back":"More reactive metals are more likely found as compounds in ores.","mcqOptions":[{"text":"More reactive metals are more likely found as compounds in ores.","correct":true,"explanation":"Highly reactive metals readily react with other elements, so they are usually present as compounds in ores rather than as uncombined metals."},{"text":"More reactive metals are more likely found as elements in ores.","correct":false,"explanation":"High reactivity makes metals more likely to form compounds, not remain uncombined. Metals low in the reactivity series are more likely to occur naturally."},{"text":"More reactive metals are more likely found as gases in ores.","correct":false,"explanation":"Reactivity affects whether a metal forms compounds, not whether it is found as a gas. Metallic ores contain solid metals or their solid compounds."},{"text":"Less reactive metals are more likely found as compounds in ores.","correct":false,"explanation":"The relationship is reversed here: less reactive metals are more likely to occur uncombined, while reactive metals commonly occur as compounds."}]},{"id":"8df5ed92-8496-4ceb-9aa4-8aaa04b3ece3","cardType":"basic","points":1,"front":"Why can gold and silver sometimes occur uncombined?","back":"They are very unreactive, so they do not readily form compounds.","mcqOptions":[{"text":"They are very unreactive, so they do not readily form compounds.","correct":true,"explanation":"Gold and silver are very unreactive, so they do not readily react with oxygen or other elements to form compounds in the crust."},{"text":"They are very reactive, so they do not readily form compounds.","correct":false,"explanation":"Highly reactive metals readily form compounds, so high reactivity would make uncombined gold or silver less likely, not explain their occurrence."},{"text":"They have high melting points, so they do not readily form compounds.","correct":false,"explanation":"Gold and silver can occur uncombined because they resist chemical reaction. Their high melting points do not prevent compound formation or explain this behaviour."},{"text":"They are very dense, so they do not readily form compounds.","correct":false,"explanation":"Density does not determine whether a metal reacts to form compounds. Gold and silver occur uncombined because their chemical reactivity is very low."}]},{"id":"3f9b8949-b3ac-4257-98e8-20cd2b97cfc8","cardType":"cloze","points":null,"front":"Metals above carbon are usually extracted by [ ].","back":"Metals above carbon are usually extracted by electrolysis.","mcqOptions":[{"text":"electrolysis","correct":true,"explanation":"Metals above carbon are more reactive than carbon, so carbon cannot remove oxygen from their compounds. Electrolysis supplies the needed chemical change."},{"text":"reduction with carbon","correct":false,"explanation":"Carbon reduction works for metals below carbon, not above it. A metal above carbon is too reactive for carbon to remove its oxygen."},{"text":"heating alone","correct":false,"explanation":"Heating alone cannot usually separate a highly reactive metal from its oxide. Electrolysis is needed to decompose the compound using electrical energy."},{"text":"carbon monoxide","correct":false,"explanation":"Carbon monoxide is a reducing agent for suitable oxides below carbon, but it cannot generally extract metals more reactive than carbon."}]},{"id":"4297dac8-9ee5-4f8c-b2e7-d718aec19f7a","cardType":"cloze","points":null,"front":"Metal oxides below carbon can often be extracted by heating with [ ] or [ ].","back":"Metal oxides below carbon can often be extracted by heating with carbon or carbon monoxide.","mcqOptions":[{"text":"Metal oxides below carbon can often be extracted by heating with carbon or carbon monoxide.","correct":true,"explanation":"Carbon and carbon monoxide both remove oxygen from suitable metal oxides when heated, leaving the less reactive metal behind."},{"text":"Metal oxides below carbon can often be extracted by heating with hydrogen or carbon monoxide.","correct":false,"explanation":"Hydrogen is a possible reducing agent in some extraction processes, but it is not the paired GCSE method stated here for these metal oxides."},{"text":"Metal oxides below carbon can often be extracted by heating with oxygen or carbon monoxide.","correct":false,"explanation":"Oxygen would oxidise the metal or oxide rather than remove oxygen from the oxide. Carbon and carbon monoxide are the reducing agents described."},{"text":"Metal oxides below carbon can often be extracted by heating with carbon or electrolysis.","correct":false,"explanation":"Electrolysis is used for metals above carbon, while carbon and carbon monoxide chemically reduce suitable oxides below carbon when heated."}]},{"id":"c163a23b-6680-45dd-85eb-16a726408120","cardType":"cloze","points":null,"front":"In metal extraction, reduction often means [ ] from a metal oxide.","back":"In metal extraction, reduction often means removal of oxygen from a metal oxide.","mcqOptions":[{"text":"removal of oxygen","correct":true,"explanation":"In this extraction context, reduction describes the removal of oxygen from a metal oxide, leaving the metal or a less oxygen-rich compound."},{"text":"addition of oxygen","correct":false,"explanation":"Reduction is not the addition of oxygen; adding oxygen is oxidation. Extracting a metal from its oxide requires oxygen to be removed."},{"text":"addition of electrons","correct":false,"explanation":"The definition involving electron gain is valid in broader chemistry, but this extraction statement specifically describes removing oxygen from the oxide."},{"text":"removal of the metal","correct":false,"explanation":"Removing the metal would not produce the extracted metal. Reduction in this context removes oxygen from the metal oxide instead."}]},{"id":"56d909b9-9945-41d0-b924-207897ca7b3e","cardType":"basic","points":2,"front":"Why can carbon monoxide extract iron from iron(III) oxide?","back":"Iron is below carbon, so CO can remove oxygen.","mcqOptions":[{"text":"Iron is below carbon, so CO can remove oxygen.","correct":true,"explanation":"Iron is below carbon in the reactivity series, so carbon monoxide can remove oxygen from iron(III) oxide and leave iron behind."},{"text":"Iron is above carbon, so CO can remove oxygen.","correct":false,"explanation":"A metal above carbon cannot usually be extracted by carbon monoxide because it holds oxygen more strongly. Iron is below carbon, not above it."},{"text":"Iron is below carbon, so CO can add oxygen.","correct":false,"explanation":"Carbon monoxide removes oxygen from the oxide; it does not add oxygen. The reaction is possible because iron is below carbon."},{"text":"Iron is as reactive as carbon, so CO can remove oxygen.","correct":false,"explanation":"Iron is not extracted because it is as reactive as carbon. Its position below carbon allows CO to reduce its oxide by removing oxygen."}]},{"id":"326edc65-7a67-48fb-8099-1fa3c8046cea","cardType":"basic","points":2,"front":"Write the equation for reducing iron(III) oxide with carbon monoxide.","back":"$$\\mathrm{Fe_2O_3(s) + 3CO(g) \\to 2Fe(l) + 3CO_2(g)}$","mcqOptions":[{"text":"$$\\mathrm{Fe_2O_3(s) + 3CO(g) \\to 2Fe(l) + 3CO_2(g)}$","correct":true,"explanation":"The equation is balanced: it has two iron atoms, three oxygen atoms in the oxide, three carbon atoms, and equal total atoms on both sides."},{"text":"$$\\mathrm{Fe_2O_3(s) + 2CO(g) \\to 2Fe(l) + 2CO_2(g)}$","correct":false,"explanation":"This has only two CO molecules, so there are too few carbon and oxygen atoms to form three carbon dioxide molecules. Three CO molecules are required."},{"text":"$$\\mathrm{Fe_2O_3(s) + 3CO(g) \\to 3Fe(l) + 3CO_2(g)}$","correct":false,"explanation":"Three iron atoms appear on the product side although the reactant contains only two iron atoms. The coefficient of iron must therefore be 2."},{"text":"$$\\mathrm{Fe_2O_3(s) + 3CO(g) \\to 2Fe(l) + 3CO_3(g)}$","correct":false,"explanation":"The products are written with the wrong carbon oxide. Carbon monoxide gains oxygen from iron(III) oxide to form carbon dioxide, not carbon trioxide."}]},{"id":"413d68fe-e5fc-4e68-9270-e3341dcbddf6","cardType":"basic","points":2,"front":"In iron extraction, why is carbon monoxide oxidised?","back":"It gains oxygen to form carbon dioxide.","mcqOptions":[{"text":"It gains oxygen to form carbon dioxide.","correct":true,"explanation":"Carbon monoxide becomes carbon dioxide by gaining oxygen from iron oxide. Gaining oxygen is the definition of oxidation used in this extraction reaction."},{"text":"It loses oxygen to form carbon dioxide.","correct":false,"explanation":"Carbon monoxide does not lose oxygen during the reaction. It gains oxygen from iron oxide to form carbon dioxide, so it is oxidised."},{"text":"It gains hydrogen to form carbon dioxide.","correct":false,"explanation":"Carbon monoxide is not converted by gaining hydrogen. It gains oxygen from iron oxide, producing carbon dioxide and meeting the definition of oxidation."},{"text":"It loses carbon to form carbon dioxide.","correct":false,"explanation":"Losing carbon could not convert carbon monoxide into carbon dioxide, which still contains carbon. Carbon monoxide is oxidised because it gains oxygen."}]},{"id":"2b67e130-5759-4342-b550-af5abce3ec0c","cardType":"basic","points":2,"front":"Why is aluminium oxide not reduced by carbon?","back":"Aluminium is above carbon; its oxide is too stable.","mcqOptions":[{"text":"Aluminium is above carbon; its oxide is too stable.","correct":true,"explanation":"Aluminium is more reactive than carbon, so aluminium oxide is very stable. Carbon cannot remove oxygen from the oxide and therefore cannot reduce it."},{"text":"Aluminium is below carbon; its oxide is too stable.","correct":false,"explanation":"Placing aluminium below carbon reverses the reactivity series. Aluminium is above carbon, making its oxide too stable to be reduced by carbon."},{"text":"Aluminium is above carbon; its oxide is too unstable.","correct":false,"explanation":"The position of aluminium above carbon means its oxide is especially stable, not unstable. Consequently, carbon cannot remove oxygen from aluminium oxide."},{"text":"Aluminium is below carbon; carbon cannot form oxides.","correct":false,"explanation":"Carbon readily forms oxides such as carbon monoxide and carbon dioxide. The reduction fails because aluminium is above carbon and aluminium oxide is too stable."}]},{"id":"151cc6cb-ac79-413f-82eb-003f5ac862b5","cardType":"basic","points":2,"front":"Why must an electrolyte be molten or dissolved?","back":"Its ions can move and carry charge.","mcqOptions":[{"text":"Its ions can move and carry charge.","correct":true,"explanation":"Melting or dissolving an ionic substance frees its ions from fixed lattice positions. These mobile charged particles can travel through the electrolyte and carry current."},{"text":"Its electrons can move and carry charge.","correct":false,"explanation":"Conduction through an electrolyte depends on mobile ions, not freely moving electrons as in a metal. Melting or dissolving releases the ions to carry charge."},{"text":"Its atoms can move and carry charge.","correct":false,"explanation":"Although atoms may move in a liquid, neutral atoms do not transport electrical charge through an electrolyte. Mobile positive and negative ions carry the charge."},{"text":"Its molecules can move and carry charge.","correct":false,"explanation":"Neutral molecules cannot carry current merely by moving. An electrolyte must be molten or dissolved so that its charged ions are free to move."}]},{"id":"5fe6238a-5140-491f-a2ad-d414a7f3a529","cardType":"basic","points":2,"front":"Why is aluminium oxide dissolved in molten cryolite?","back":"Cryolite lowers operating temperature, reducing energy costs.","mcqOptions":[{"text":"Cryolite lowers operating temperature, reducing energy costs.","correct":true,"explanation":"Cryolite lowers the temperature at which the aluminium oxide mixture can operate as a molten electrolyte. Less heating is therefore required, lowering energy costs."},{"text":"Cryolite raises operating temperature, increasing aluminium yield.","correct":false,"explanation":"Raising the operating temperature would require more heating rather than solving the energy problem. Cryolite lowers the required temperature and therefore reduces energy costs."},{"text":"Cryolite reacts with aluminium oxide, producing aluminium directly.","correct":false,"explanation":"Cryolite does not chemically produce aluminium directly; electrolysis reduces aluminium ions at the cathode. Its purpose is to lower the operating temperature and energy cost."},{"text":"Cryolite prevents electrolyte conduction, protecting the electrodes.","correct":false,"explanation":"Preventing conduction would stop electrolysis rather than assist it. Cryolite allows operation at a lower temperature, reducing the energy needed to keep the electrolyte molten."}]},{"id":"939c74bf-8e9e-4bfa-aaa8-2b9cead669ca","cardType":"cloze","points":null,"front":"At the negative cathode, aluminium ions [ ] to form aluminium.","back":"At the negative cathode, aluminium ions gain electrons to form aluminium.","mcqOptions":[{"text":"gain electrons","correct":true,"explanation":"Positive aluminium ions are attracted to the negative cathode, where they gain electrons. This reduction converts each aluminium ion into a neutral aluminium atom."},{"text":"lose electrons","correct":false,"explanation":"Losing electrons would make aluminium ions more positively charged rather than forming neutral atoms. At the cathode, aluminium ions gain electrons and are reduced."},{"text":"gain protons","correct":false,"explanation":"Electrolysis involves electron transfer at the electrodes, not aluminium ions gaining protons. Aluminium ions form aluminium atoms by gaining electrons at the cathode."},{"text":"lose protons","correct":false,"explanation":"Removing protons would change the identity of the atomic nucleus and is not an electrolysis process. Aluminium ions instead gain electrons at the cathode."}]},{"id":"0148a7d5-6ecb-49ff-b1cd-a62cddf145b7","cardType":"cloze","points":null,"front":"At the positive anode, oxide ions [ ] to form oxygen.","back":"At the positive anode, oxide ions lose electrons to form oxygen.","mcqOptions":[{"text":"lose electrons","correct":true,"explanation":"Negative oxide ions are attracted to the positive anode and release electrons there. Losing electrons is oxidation and leads to the formation of oxygen molecules."},{"text":"gain electrons","correct":false,"explanation":"Gaining electrons occurs during reduction at the cathode, not oxidation at the anode. Oxide ions lose electrons at the positive anode to form oxygen."},{"text":"lose protons","correct":false,"explanation":"Oxide ions do not contain protons that are transferred during electrolysis. They form oxygen at the anode by losing electrons in an oxidation reaction."},{"text":"gain protons","correct":false,"explanation":"Adding protons would be an acid-base process and would not explain oxygen formation at the anode. Oxide ions instead lose electrons and are oxidised."}]},{"id":"adc6a4f1-31c2-4629-98a2-17b6ace818ee","cardType":"basic","points":2,"front":"Why do carbon anodes in aluminium extraction wear away?","back":"Oxygen reacts with carbon to make carbon dioxide.","mcqOptions":[{"text":"Oxygen reacts with carbon to make carbon dioxide.","correct":true,"explanation":"Oxide ions discharge at the anode and form oxygen, which reacts with the hot carbon electrode. Producing carbon dioxide consumes the carbon, so the anode wears away."},{"text":"Aluminium reacts with carbon to make carbon dioxide.","correct":false,"explanation":"Aluminium cannot supply the oxygen needed to form carbon dioxide, and it is produced at the cathode. Anodes wear away because oxygen reacts with their carbon."},{"text":"Carbon melts at the cell temperature to form carbon dioxide.","correct":false,"explanation":"Carbon has a very high melting point and does not melt under the cell’s operating conditions. It is consumed when oxygen reacts with it to form carbon dioxide."},{"text":"Oxide ions plate onto carbon as solid oxygen.","correct":false,"explanation":"Oxygen is formed as a gas rather than deposited as a solid. This oxygen reacts with the carbon anode to produce carbon dioxide, consuming the electrode."}]},{"id":"0352d84c-c4e4-4c90-93bb-2d0946a0e9a8","cardType":"basic","points":2,"front":"Why is aluminium suitable for aircraft bodies and bicycle frames?","back":"Its low density reduces mass.","mcqOptions":[{"text":"Its low density reduces mass.","correct":true,"explanation":"Aluminium has a low density, so a component of a given volume has relatively little mass. This makes aircraft and bicycles lighter and more efficient."},{"text":"Its high density reduces mass.","correct":false,"explanation":"High density means greater mass for a given volume, making a structure heavier. Aluminium is suitable because its low density helps minimise the vehicle’s mass."},{"text":"Its low melting point reduces mass.","correct":false,"explanation":"A low melting point can make shaping a metal easier, but it does not directly reduce a finished component’s mass. Aluminium’s low density provides that advantage."},{"text":"Its high conductivity reduces mass.","correct":false,"explanation":"Electrical conductivity is useful for wires but does not make aircraft bodies or bicycle frames lighter. Their reduced mass results from aluminium’s low density."}]},{"id":"8ee4424b-acf1-4ff9-8665-fd02dfe5ad8e","cardType":"basic","points":3,"front":"Why is aluminium often used instead of copper for overhead power cables?","back":"

Conducts electricity well enough for cables.
Lower density means less sag/support.

","mcqOptions":[{"text":"

Conducts electricity well enough for cables.
Lower density means less sag/support.

","correct":true,"explanation":"Aluminium conducts electricity sufficiently well, while its lower density makes cables lighter than copper equivalents. This reduces sag and the amount of structural support required."},{"text":"

Conducts electricity better than copper.
Higher density means less sag/support.

","correct":false,"explanation":"Aluminium is less electrically conductive than copper and has a lower, not higher, density. It is chosen because it conducts well enough while its low density reduces sag and support requirements."},{"text":"

Insulates electricity well enough for cables.
Lower density prevents energy loss.

","correct":false,"explanation":"Confusing a conductor with an insulator overlooks the cable’s purpose, while density does not directly prevent energy loss. Aluminium conducts electricity adequately and its low density reduces cable sag."},{"text":"

Conducts electricity without resistance.
Greater strength means no support is needed.

","correct":false,"explanation":"All conductors have some electrical resistance, and overhead cables still require supports. Aluminium is used because it conducts sufficiently well and has a lower density than copper."}]},{"id":"f42d504b-ac79-4d8f-8d58-6252d26c1753","cardType":"basic","points":1,"front":"Which copper property makes it suitable for electrical wiring?","back":"It is an excellent electrical conductor.","mcqOptions":[{"text":"It is an excellent electrical conductor.","correct":true,"explanation":"Copper has very low electrical resistance, so current passes through it easily with relatively little energy transferred as heat. This makes it highly suitable for wiring."},{"text":"It is an excellent thermal conductor.","correct":false,"explanation":"Thermal conductivity concerns the transfer of heat, not the flow of electric current. Copper is suitable for wiring because it is an excellent electrical conductor."},{"text":"It is an excellent electrical insulator.","correct":false,"explanation":"An electrical insulator prevents charge from flowing, so it would be unsuitable for the conducting core of a wire. Copper is instead an excellent electrical conductor."},{"text":"It is a high-resistance electrical conductor.","correct":false,"explanation":"High resistance would cause substantial electrical energy to be transferred as heat. Copper is used because its excellent electrical conductivity gives it low resistance."}]},{"id":"60b9393b-d390-40cb-b33e-a3eb41ccdfe9","cardType":"basic","points":1,"front":"Why is copper used for heat exchangers and cooking bases?","back":"It is an excellent thermal conductor.","mcqOptions":[{"text":"It is an excellent thermal conductor.","correct":true,"explanation":"Copper transfers thermal energy rapidly because it has high thermal conductivity. This spreads heat effectively through heat exchangers and across the bases of cooking containers."},{"text":"It is an excellent electrical conductor.","correct":false,"explanation":"Electrical conductivity is important for wiring, but it does not directly explain the efficient transfer of heat. Copper is used here because it is an excellent thermal conductor."},{"text":"It is an excellent thermal insulator.","correct":false,"explanation":"A thermal insulator would slow heat transfer and make heat exchangers or cooking bases ineffective. Copper is suitable because it conducts thermal energy very well."},{"text":"It has a very low melting point.","correct":false,"explanation":"A low melting point would make a material unsafe for hot cooking equipment. Copper is suitable because its high thermal conductivity transfers and distributes heat efficiently."}]},{"id":"1d58abb4-4229-426a-8f04-32c7d7f3f8c9","cardType":"cloze","points":null,"front":"[ ], also called mild steel, is tough, malleable and easy to shape.","back":"Low-carbon steel, also called mild steel, is tough, malleable and easy to shape.","mcqOptions":[{"text":"Low-carbon steel","correct":true,"explanation":"Low-carbon steel contains a relatively small proportion of carbon, making it tough, malleable and easier to shape than steel with a higher carbon content."},{"text":"High-carbon steel","correct":false,"explanation":"High-carbon steel contains more carbon and is harder but also more brittle and less malleable. Low-carbon steel, also called mild steel, is tough and easy to shape."},{"text":"Stainless steel","correct":false,"explanation":"Stainless steel contains chromium to provide corrosion resistance and is not another name for mild steel. Mild steel is specifically low-carbon steel."},{"text":"Cast iron","correct":false,"explanation":"Cast iron has a high carbon content and is relatively brittle, so it is not malleable or easily shaped. Mild steel is another name for low-carbon steel."}]},{"id":"2ab4eb37-cfa9-4585-97b4-211289be4513","cardType":"basic","points":1,"front":"Why is high-carbon steel used for cutting tools and blades?","back":"It is harder than mild steel.","mcqOptions":[{"text":"It is harder than mild steel.","correct":true,"explanation":"A higher carbon content disrupts the iron lattice and makes high-carbon steel harder than mild steel. This hardness helps cutting edges resist deformation and remain sharp."},{"text":"It is softer than mild steel.","correct":false,"explanation":"Cutting tools require hardness so their edges do not deform during use. High-carbon steel is harder, not softer, than mild steel because it contains more carbon."},{"text":"It is more malleable than mild steel.","correct":false,"explanation":"Greater malleability would allow a blade to bend or deform more easily and is not the required property. High-carbon steel is used because it is harder than mild steel."},{"text":"It is more corrosion-resistant than stainless steel.","correct":false,"explanation":"Corrosion resistance is associated especially with chromium-containing stainless steel, not ordinary high-carbon steel. High-carbon steel is selected for blades because it is harder than mild steel."}]},{"id":"a4708c71-6ba3-4540-883d-8b7cfc186708","cardType":"basic","points":1,"front":"Why is stainless steel suitable for cutlery, sinks and surgical instruments?","back":"It resists corrosion.","mcqOptions":[{"text":"It resists corrosion.","correct":true,"explanation":"Stainless steel contains chromium, which forms a protective oxide layer on its surface. This resistance to corrosion makes it durable and hygienic in wet conditions."},{"text":"It reacts readily with water.","correct":false,"explanation":"Rapid reaction with water would cause damage and contamination, making a material unsuitable for these uses. Stainless steel is chosen because it resists corrosion."},{"text":"It has a very low melting point.","correct":false,"explanation":"A very low melting point would make the material unsuitable for hot cookware or sterilised surgical equipment. Stainless steel is suitable because it resists corrosion."},{"text":"It is softer than pure iron.","correct":false,"explanation":"Alloying iron generally increases hardness rather than making it softer, but hardness alone does not explain all these uses. Stainless steel is especially suitable because it resists corrosion."}]},{"id":"6b78f93d-7d73-4e19-9f3d-d0cc2c29c6e6","cardType":"cloze","points":null,"front":"An alloy is a [ ] of a metal with one or more other elements.","back":"An alloy is a mixture of a metal with one or more other elements.","mcqOptions":[{"text":"mixture","correct":true,"explanation":"An alloy consists of a metal combined physically with one or more other elements. Its composition can vary, so it is classified as a mixture rather than a pure substance."},{"text":"compound","correct":false,"explanation":"A compound contains elements chemically bonded in fixed proportions, whereas an alloy can have variable proportions. An alloy is therefore a mixture of a metal with other elements."},{"text":"element","correct":false,"explanation":"An element contains only one type of atom, but an alloy contains a metal and at least one other element. It is therefore a mixture."},{"text":"molecule","correct":false,"explanation":"A molecule is a discrete group of covalently bonded atoms, which does not describe the metallic structure of an alloy. An alloy is classified as a mixture."}]},{"id":"2b4e6b96-9baa-4cd8-942e-b7585ba819eb","cardType":"basic","points":2,"front":"Why are alloys harder than pure metals?","back":"Different-sized atoms distort regular layers, making sliding harder.","mcqOptions":[{"text":"Different-sized atoms distort regular layers, making sliding harder.","correct":true,"explanation":"Atoms of different sizes disrupt the regular arrangement of metal atoms. This prevents layers from sliding over one another as easily, making the alloy harder."},{"text":"Identical-sized atoms form regular layers, making sliding easier.","correct":false,"explanation":"Identical atoms can form regular layers that slide relatively easily, explaining why pure metals are often softer. Alloys are harder because different-sized atoms distort these layers."},{"text":"Different-sized atoms create regular layers, making sliding easier.","correct":false,"explanation":"Different-sized atoms do not create more regular layers or make sliding easier. They distort the regular arrangement and hinder layer movement, which increases hardness."},{"text":"Free-moving electrons lock regular layers, preventing all sliding.","correct":false,"explanation":"Delocalised electrons provide metallic bonding but do not lock atomic layers or prevent all movement. Alloy hardness arises because different-sized atoms distort layers and hinder sliding."}]}]}],"examCountdown":{"examDate":"2027-05-19","paperLabel":"Paper 1"},"heading":"Extraction and uses of metals","title":"Extraction and uses of metals Flashcards","topbar":{"backHref":"/igcse/chemistry/edexcel/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"54a25ddf-5c9e-55a9-bd9f-8e97cb403642","walled":"$L38"}],"$L39","$L3a"]