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The more readily their atoms lose electrons, the more reactive the metal is in chemical reactions."},{"text":"How easily metal atoms gain electrons to form negative ions.","correct":false,"explanation":"This reverses the electron behaviour of metals. Metals tend to lose electrons and form positive ions, so the correct definition describes how easily metal atoms lose electrons to form positive ions."},{"text":"How easily metal atoms share electrons to form covalent molecules.","correct":false,"explanation":"Sharing electrons is associated with covalent bonding, not the usual formation of metal ions. Reactivity is defined by how easily metal atoms lose electrons to form positive ions."},{"text":"How easily metal atoms lose neutrons to form isotopes.","correct":false,"explanation":"Neutron loss changes an isotope rather than forming an ion, and it does not define chemical reactivity. Metals react by losing electrons to form positive ions."}]},{"id":"e3a23a6a-e48d-4374-bde7-4dd38c1597e6","cardType":"basic","points":3,"front":"List the first five elements of the IGCSE reactivity series in order.","back":"

Potassium
Sodium
Calcium
Magnesium
Aluminium

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

Potassium
Sodium
Calcium
Magnesium
Aluminium

","correct":true,"explanation":"The first five elements are arranged from most reactive to less reactive as potassium, sodium, calcium, magnesium, and aluminium."},{"text":"

Sodium
Potassium
Calcium
Magnesium
Aluminium

","correct":false,"explanation":"This swaps potassium and sodium. Potassium is above sodium because it loses electrons more easily, so the correct order begins potassium, sodium, calcium, magnesium, aluminium."},{"text":"

Potassium
Calcium
Sodium
Magnesium
Aluminium

","correct":false,"explanation":"This places calcium above sodium, confusing their order in the series. Sodium is more reactive than calcium, giving the correct sequence potassium, sodium, calcium, magnesium, aluminium."},{"text":"

Potassium
Sodium
Magnesium
Calcium
Aluminium

","correct":false,"explanation":"This swaps calcium and magnesium. Calcium is higher in the reactivity series because it loses electrons more readily, so magnesium comes after calcium."}]},{"id":"623af88d-0918-484e-9398-6c17013f5a3e","cardType":"basic","points":1,"front":"Which three metals in the series react with cold water?","back":"Potassium, sodium, and calcium.","mcqOptions":[{"text":"Potassium, sodium, and calcium.","correct":true,"explanation":"Potassium, sodium, and calcium are sufficiently reactive to react with cold water. They form metal hydroxides and release hydrogen gas."},{"text":"Potassium, sodium, and magnesium.","correct":false,"explanation":"Magnesium reacts very slowly, if at all, with cold water and is not one of the three metals listed. Calcium reacts with cold water, so the correct set is potassium, sodium, and calcium."},{"text":"Potassium, calcium, and magnesium.","correct":false,"explanation":"Magnesium is below calcium and does not significantly react with cold water. Sodium is the missing metal, making the correct three potassium, sodium, and calcium."},{"text":"Sodium, calcium, and aluminium.","correct":false,"explanation":"Aluminium does not react with cold water because its oxide layer protects the metal. Potassium is also included among the three metals that react with cold water."}]},{"id":"364256d3-3448-47f5-aa03-3ea68ad5b2ac","cardType":"cloze","points":null,"front":"Metal + water → [ ] + hydrogen","back":"Metal + water → metal hydroxide + hydrogen","mcqOptions":[{"text":"metal hydroxide","correct":true,"explanation":"Reactive metals reacting with water produce a metal hydroxide and hydrogen. The hydroxide contains the metal ion combined with hydroxide ions from the water."},{"text":"metal oxide","correct":false,"explanation":"A metal oxide forms when a metal reacts with steam, not usually with cold water. With water, the products are metal hydroxide and hydrogen."},{"text":"metal carbonate","correct":false,"explanation":"Metal carbonates are not formed in the reaction between a metal and water because no carbonate ions are present. The product is metal hydroxide, alongside hydrogen."},{"text":"metal chloride","correct":false,"explanation":"Metal chlorides require a source of chloride ions, such as hydrochloric acid. Water provides hydroxide ions instead, so the product is metal hydroxide and hydrogen."}]},{"id":"fb43d150-cd0a-44ec-a65e-0e5627fa5bb0","cardType":"cloze","points":null,"front":"Metal + water → metal hydroxide + [ ]","back":"Metal + water → metal hydroxide + hydrogen","mcqOptions":[{"text":"hydrogen","correct":true,"explanation":"The metal displaces hydrogen from water. The metal combines with hydroxide ions to form metal hydroxide, while hydrogen gas is released."},{"text":"oxygen","correct":false,"explanation":"Water does not release oxygen in this reaction. A reactive metal displaces hydrogen from water, producing metal hydroxide and hydrogen gas."},{"text":"steam","correct":false,"explanation":"Steam is water in the gas state and is a reactant in some metal reactions, not the gaseous product of metal reacting with liquid water. The product is hydrogen."},{"text":"carbon dioxide","correct":false,"explanation":"Carbon dioxide is not produced because there is no carbon-containing reactant. The reaction forms metal hydroxide and releases hydrogen gas."}]},{"id":"4148e314-c984-4295-aa23-105749a65490","cardType":"cloze","points":null,"front":"The balanced symbol equation for sodium reacting with water is: [ ]","back":"The balanced symbol equation for sodium reacting with water is: $2Na + 2H_2O \\to 2NaOH + H_2$","mcqOptions":[{"text":"$$2Na + 2H_2O \\to 2NaOH + H_2$","correct":true,"explanation":"Two sodium atoms react with two water molecules to form two sodium hydroxide units and one hydrogen molecule. These coefficients balance every atom on both sides."},{"text":"$$Na + H_2O \\to NaOH + H_2$","correct":false,"explanation":"The hydrogen atoms are not balanced in this equation. Doubling all coefficients gives the balanced equation $2Na + 2H_2O \\to 2NaOH + H_2$."},{"text":"$$2Na + H_2O \\to 2NaOH + H_2$","correct":false,"explanation":"This uses too little water for the two sodium atoms and leaves oxygen unbalanced. The correct equation requires two water molecules: $2Na + 2H_2O \\to 2NaOH + H_2$."},{"text":"$$Na + 2H_2O \\to 2NaOH + H_2$","correct":false,"explanation":"Two sodium hydroxide units require two sodium atoms, so one sodium atom cannot balance this equation. The balanced coefficients are $2Na + 2H_2O \\to 2NaOH + H_2$."}]},{"id":"43c2a58f-44f9-4619-870b-a48cd5e703bb","cardType":"basic","points":1,"front":"What are the products when magnesium reacts with steam?","back":"Magnesium oxide and hydrogen gas.","mcqOptions":[{"text":"Magnesium oxide and hydrogen gas.","correct":true,"explanation":"Magnesium reacts with steam to form magnesium oxide while displacing hydrogen from the water. The hydrogen is released as a gas."},{"text":"Magnesium hydroxide and hydrogen gas.","correct":false,"explanation":"Magnesium hydroxide forms when magnesium reacts with liquid water, whereas steam produces the oxide. The products with steam are magnesium oxide and hydrogen gas."},{"text":"Magnesium oxide and oxygen gas.","correct":false,"explanation":"Steam provides hydrogen, which is displaced by magnesium. Oxygen is not released as a product, so the correct products are magnesium oxide and hydrogen gas."},{"text":"Magnesium chloride and hydrogen gas.","correct":false,"explanation":"Magnesium chloride would require chloride ions, which are absent from steam. Magnesium reacts with the oxygen and hydrogen in steam to form magnesium oxide and hydrogen gas."}]},{"id":"5f3615fd-b504-44c7-aaf0-429f3b04de52","cardType":"basic","points":1,"front":"Why does magnesium react with steam but not significantly with cold water?","back":"Magnesium is less reactive than the metals above it (K, Na, Ca).","mcqOptions":[{"text":"Magnesium is less reactive than the metals above it (K, Na, Ca).","correct":true,"explanation":"Magnesium is below potassium, sodium, and calcium in the reactivity series. It reacts sufficiently with hot steam but not significantly with cold water."},{"text":"Magnesium is more reactive than the metals above it (K, Na, Ca).","correct":false,"explanation":"This reverses the series: metals above magnesium are more reactive and react more readily with cold water. Magnesium is less reactive than K, Na, and Ca."},{"text":"Magnesium is less reactive than the metals below it (Al, Zn, Fe).","correct":false,"explanation":"Magnesium is above aluminium, zinc, and iron in the reactivity series, so it is more reactive than them. Its slow reaction with cold water is because it is less reactive than K, Na, and Ca."},{"text":"Magnesium is equally reactive as the metals above it (K, Na, Ca).","correct":false,"explanation":"The metals above magnesium are more reactive, which is why they react with cold water more readily. Magnesium is less reactive than K, Na, and Ca."}]},{"id":"7a6e8c39-7e49-45c4-b4a8-5bebdb27d8d5","cardType":"basic","points":1,"front":"What is the general word equation for a metal reacting with dilute hydrochloric acid?","back":"metal + hydrochloric acid → metal chloride + hydrogen","mcqOptions":[{"text":"metal + hydrochloric acid → metal chloride + hydrogen","correct":true,"explanation":"Hydrochloric acid provides chloride ions, forming a metal chloride, while the metal displaces hydrogen ions to produce hydrogen gas."},{"text":"metal + hydrochloric acid → metal hydroxide + hydrogen","correct":false,"explanation":"Metal hydroxides are not the products of this acid reaction. Hydrochloric acid reacts with a suitable metal to form metal chloride and hydrogen."},{"text":"metal + hydrochloric acid → metal oxide + water","correct":false,"explanation":"Water formation is associated with an acid reacting with a metal oxide, not usually with a metal itself. The correct products are metal chloride and hydrogen."},{"text":"metal + hydrochloric acid → metal sulfate + hydrogen","correct":false,"explanation":"Sulfates form when a metal reacts with sulfuric acid, not hydrochloric acid. Hydrochloric acid produces a metal chloride and hydrogen."}]},{"id":"e7b55225-6b6f-4cd9-b6a6-6d80c884cb21","cardType":"cloze","points":null,"front":"Metals [ ] hydrogen in the reactivity series react with dilute acid, while metals below hydrogen do not.","back":"Metals above hydrogen in the reactivity series react with dilute acid, while metals below hydrogen do not.","mcqOptions":[{"text":"above","correct":true,"explanation":"Metals above hydrogen are more reactive than hydrogen, so they displace hydrogen from dilute acids and release hydrogen gas."},{"text":"below","correct":false,"explanation":"Being below hydrogen means the metal is less reactive and cannot displace hydrogen from dilute acid. The correct term is above."},{"text":"beside","correct":false,"explanation":"The reactivity series ranks metals above or below one another; beside does not describe the required position. Metals above hydrogen react with dilute acid."},{"text":"near","correct":false,"explanation":"A metal’s position near hydrogen does not determine this rule. Metals must be above hydrogen in the reactivity series to react with dilute acid."}]},{"id":"58570005-974f-4da5-a4f5-0ee8b5dadd96","cardType":"cloze","points":null,"front":"Metals above hydrogen in the reactivity series react with dilute acid, while metals [ ] hydrogen do not.","back":"Metals above hydrogen in the reactivity series react with dilute acid, while metals below hydrogen do not.","mcqOptions":[{"text":"below","correct":true,"explanation":"Metals below hydrogen are less reactive than hydrogen, so they cannot displace hydrogen from dilute acids and do not react in this way."},{"text":"above","correct":false,"explanation":"Metals above hydrogen are more reactive and do react with dilute acid. The missing term must be below because those metals cannot displace hydrogen."},{"text":"beside","correct":false,"explanation":"Beside is not a meaningful ranking in the reactivity series. Metals below hydrogen are the metals that do not react with dilute acid."},{"text":"near","correct":false,"explanation":"Being near hydrogen is not the relevant condition. The rule depends on whether the metal is below hydrogen in the reactivity series."}]},{"id":"11cd55a2-6ea3-41ec-941f-1478eaeb1c1d","cardType":"basic","points":1,"front":"Which three metals in the syllabus do not react with dilute hydrochloric acid?","back":"

Copper
Silver
Gold

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

Copper
Silver
Gold

","correct":true,"explanation":"Copper, silver and gold are below hydrogen in the reactivity series, so they cannot displace hydrogen from dilute hydrochloric acid."},{"text":"

Iron
Tin
Aluminium

","correct":false,"explanation":"Iron, tin and aluminium are above hydrogen in the reactivity series and can react with dilute hydrochloric acid. The correct metals are copper, silver and gold."},{"text":"

Zinc
Iron
Lead

","correct":false,"explanation":"Zinc and iron readily react with dilute hydrochloric acid, while lead is also listed above hydrogen. The three metals that do not react are copper, silver and gold."},{"text":"

Magnesium
Zinc
Nickel

","correct":false,"explanation":"Magnesium and zinc are clearly above hydrogen and nickel is also more reactive than hydrogen. The correct non-reactive metals are copper, silver and gold."}]},{"id":"d733786e-8863-4ec1-bd09-da45f0ab0a86","cardType":"basic","points":3,"front":"List three variables that must be controlled to fairly compare metal reactivity in an experiment.","back":"

Acid concentration
Temperature
Metal surface area

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

Acid concentration
Temperature
Metal surface area

","correct":true,"explanation":"Keeping acid concentration, temperature and metal surface area constant ensures that differences in reaction rate are caused by the metals’ reactivities rather than other factors."},{"text":"

Acid colour
Temperature
Metal surface area

","correct":false,"explanation":"Acid colour does not normally affect reaction rate, so it is not a required control variable. The relevant controls are acid concentration, temperature and metal surface area."},{"text":"

Acid concentration
Reaction time
Metal surface area

","correct":false,"explanation":"Reaction time is usually measured as the outcome, not kept constant when comparing rates. The controls should be acid concentration, temperature and metal surface area."},{"text":"

Metal colour
Pressure
Hydrogen volume

","correct":false,"explanation":"Metal colour and hydrogen volume do not provide the standard controls for this comparison, while hydrogen volume is measured. Control acid concentration, temperature and metal surface area."}]},{"id":"0bd7064f-f61e-43ad-aff3-8b8b8e13b097","cardType":"cloze","points":null,"front":"Magnesium reacts [ ] than iron with dilute acid because it is higher in the reactivity series.","back":"Magnesium reacts more quickly than iron with dilute acid because it is higher in the reactivity series.","mcqOptions":[{"text":"more quickly","correct":true,"explanation":"Magnesium is higher in the reactivity series than iron, so it reacts more readily with dilute acid and produces hydrogen at a faster rate."},{"text":"more slowly","correct":false,"explanation":"This reverses the reactivity relationship: magnesium is more reactive than iron, so it reacts faster. The correct comparison is more quickly."},{"text":"less quickly","correct":false,"explanation":"Less quickly implies that magnesium is less reactive than iron, which is incorrect. Magnesium is higher in the reactivity series and reacts more quickly."},{"text":"at the same rate","correct":false,"explanation":"The two metals do not react at the same rate because they have different positions in the reactivity series. Magnesium reacts more quickly than iron."}]},{"id":"b38e2fb4-d073-4f84-a84f-a4a046a96909","cardType":"cloze","points":null,"front":"Magnesium reacts more quickly than iron with dilute acid because it is [ ] in the reactivity series.","back":"Magnesium reacts more quickly than iron with dilute acid because it is higher in the reactivity series.","mcqOptions":[{"text":"higher","correct":true,"explanation":"Magnesium is positioned higher than iron in the reactivity series, meaning it is more reactive and therefore reacts more quickly with dilute acid."},{"text":"lower","correct":false,"explanation":"A lower position would indicate lower reactivity, but magnesium is above iron in the reactivity series. The correct term is higher."},{"text":"equal","correct":false,"explanation":"Magnesium and iron do not have equal positions or equal reactivity. Magnesium is higher in the reactivity series, which explains its faster reaction."},{"text":"outside","correct":false,"explanation":"Outside is not used to describe a metal’s position in the reactivity series. Magnesium is higher in the series than iron and therefore more reactive."}]},{"id":"a237caa3-aaec-4238-a086-f3d0243da44e","cardType":"basic","points":1,"front":"In Extended theory, what is a displacement reaction?","back":"A reaction where a more reactive element takes the place of a less reactive element in a compound.","mcqOptions":[{"text":"A reaction where a more reactive element takes the place of a less reactive element in a compound.","correct":true,"explanation":"In a displacement reaction, the more reactive element replaces the less reactive element in its compound because it forms bonds more readily."},{"text":"A reaction where a less reactive element takes the place of a more reactive element in a compound.","correct":false,"explanation":"A less reactive element cannot normally displace a more reactive one. The correct rule is that a more reactive element replaces a less reactive element."},{"text":"A reaction where a more reactive element takes the place of a more reactive element in a compound.","correct":false,"explanation":"The element being displaced must be less reactive, not equally or more reactive. A more reactive element replaces a less reactive element in the compound."},{"text":"A reaction where a less reactive element takes the place of a less reactive element in a compound.","correct":false,"explanation":"Two less reactive elements do not define the displacement rule. The replacing element must be more reactive than the less reactive element in the compound."}]},{"id":"bae2ed37-4b43-4f87-ba69-4405e3715eb6","cardType":"cloze","points":null,"front":"In a displacement reaction, the more reactive metal atoms form [ ] by losing electrons.","back":"In a displacement reaction, the more reactive metal atoms form positive ions by losing electrons.","mcqOptions":[{"text":"positive ions","correct":true,"explanation":"A more reactive metal loses electrons during displacement, producing positively charged metal ions in solution."},{"text":"negative ions","correct":false,"explanation":"Negative ions gain electrons rather than result from metal atoms losing them. The correct product is positive ions because electron loss leaves the metal with a net positive charge."},{"text":"neutral atoms","correct":false,"explanation":"Neutral atoms have equal numbers of protons and electrons, so they have not lost electrons. The correct product is positive ions, formed when metal atoms lose electrons."},{"text":"molecules","correct":false,"explanation":"Molecules are groups of covalently bonded atoms, not the charged particles formed when reactive metal atoms lose electrons. The correct product is positive ions."}]},{"id":"e5799f55-6ddd-43d6-bfc3-d660ae5f8b84","cardType":"cloze","points":null,"front":"In a displacement reaction, the more reactive metal atoms form positive ions by [ ].","back":"In a displacement reaction, the more reactive metal atoms form positive ions by losing electrons.","mcqOptions":[{"text":"losing electrons","correct":true,"explanation":"Losing electrons gives metal atoms more positive charge than negative charge, so they become positive ions during the displacement reaction."},{"text":"gaining electrons","correct":false,"explanation":"Gaining electrons would make the metal atoms negative ions, which is the opposite of what occurs. The correct process is losing electrons to form positive ions."},{"text":"sharing electrons","correct":false,"explanation":"Sharing electrons forms covalent bonds rather than metal ions in this reaction. The correct process is losing electrons, leaving each metal atom positively charged."},{"text":"transferring protons","correct":false,"explanation":"Transferring protons would change the element itself and does not describe ordinary chemical reactions. The correct process is losing electrons, which forms positive ions."}]},{"id":"2cd10396-0f91-45e8-90a6-42ee25f4af5f","cardType":"basic","points":2,"front":"Why will zinc displace copper from copper(II) sulfate solution?","back":"Zinc is more reactive than copper and loses electrons more easily.","mcqOptions":[{"text":"Zinc is more reactive than copper and loses electrons more easily.","correct":true,"explanation":"Zinc is above copper in the reactivity series, so it loses electrons more readily and displaces copper ions from copper(II) sulfate solution."},{"text":"Copper is more reactive than zinc and loses electrons more easily.","correct":false,"explanation":"Copper is less reactive than zinc, so it cannot displace zinc or zinc ions. The correct explanation is that zinc is more reactive and loses electrons more easily."},{"text":"Zinc is less reactive than copper and gains electrons more easily.","correct":false,"explanation":"Zinc does not gain electrons more easily in this displacement. It loses electrons more readily because it is more reactive than copper, allowing it to displace copper ions."},{"text":"Zinc reacts because copper sulfate is more reactive than zinc and accepts electrons more easily.","correct":false,"explanation":"The sulfate ion is not the reason for displacement, and zinc does not react because it is less reactive. Zinc is more reactive than copper and loses electrons more easily."}]},{"id":"32b57c01-ae86-49ff-ab24-51ec44318e86","cardType":"basic","points":2,"front":"Metal X displaces silver but not zinc. Place X, silver, and zinc in order of decreasing reactivity.","back":"Zinc, X, silver.","mcqOptions":[{"text":"Zinc, X, silver.","correct":true,"explanation":"X displaces silver, so X is more reactive than silver. It does not displace zinc, so zinc is more reactive than X, giving zinc, X, silver."},{"text":"X, zinc, silver.","correct":false,"explanation":"This reverses the evidence from the reactions. X must be below zinc because it cannot displace zinc, but above silver because it displaces silver."},{"text":"Zinc, silver, X.","correct":false,"explanation":"Putting silver above X contradicts X displacing silver. A metal must be more reactive than the metal it displaces, so the correct order is zinc, X, silver."},{"text":"Silver, X, zinc.","correct":false,"explanation":"This places X above zinc even though X cannot displace it. The observations require zinc to be most reactive, followed by X, then silver."}]},{"id":"f849e175-ddee-4ec5-b4c2-193b94506943","cardType":"basic","points":2,"front":"Why does aluminium often appear unreactive in laboratory conditions?","back":"It has a tough, protective oxide layer ($Al_2O_3$) on its surface.","mcqOptions":[{"text":"It has a tough, protective oxide layer ($Al_2O_3$) on its surface.","correct":true,"explanation":"Aluminium reacts with oxygen to form a tough aluminium oxide coating, $Al_2O_3$. This protective layer prevents substances from reaching the aluminium underneath."},{"text":"It has a low, easily reached melting point ($Al_2O_3$) on its surface.","correct":false,"explanation":"Aluminium is not unreactive because it has a low melting point. Its apparent lack of reaction is caused by the tough, protective oxide layer, $Al_2O_3$."},{"text":"It has a tough, protective sulfate layer ($Al_2(SO_4)_3$) on its surface.","correct":false,"explanation":"The coating is not aluminium sulfate, and sulfate does not explain the surface protection. Aluminium is protected by a tough oxide layer, $Al_2O_3$."},{"text":"It has a tough, protective carbonate layer ($Al_2(CO_3)_3$) on its surface.","correct":false,"explanation":"Aluminium does not form a protective carbonate coating responsible for this behaviour. Its surface is covered by tough aluminium oxide, $Al_2O_3$, which limits further reaction."}]},{"id":"df024b30-1a3d-437b-8dff-fb754b9fe376","cardType":"cloze","points":null,"front":"Aluminium is actually [ ] in the reactivity series, located between magnesium and carbon.","back":"Aluminium is actually high in the reactivity series, located between magnesium and carbon.","mcqOptions":[{"text":"high","correct":true,"explanation":"Aluminium is high in the reactivity series because it readily loses electrons, although its oxide coating can hide this reactivity in ordinary laboratory conditions."},{"text":"low","correct":false,"explanation":"Aluminium is not low in the reactivity series; it is above carbon and below magnesium. Its surface oxide layer can make it appear less reactive."},{"text":"medium","correct":false,"explanation":"Aluminium is more reactive than metals in the middle and lower parts of the series. The correct description is high, between magnesium and carbon."},{"text":"absent","correct":false,"explanation":"Aluminium does not have no position in the reactivity series. It is high in the series, even though its oxide coating may mask its reactions."}]},{"id":"562fabea-7796-46e5-b7d8-008a900edcd7","cardType":"cloze","points":null,"front":"Aluminium is actually high in the reactivity series, located between [ ] and carbon.","back":"Aluminium is actually high in the reactivity series, located between magnesium and carbon.","mcqOptions":[{"text":"magnesium","correct":true,"explanation":"In the reactivity series, aluminium is positioned below magnesium and above carbon. Therefore, the two reference substances are magnesium and carbon."},{"text":"calcium","correct":false,"explanation":"Calcium is higher than magnesium and is not the stated reference immediately before aluminium. Aluminium is located between magnesium and carbon."},{"text":"copper","correct":false,"explanation":"Copper is much lower in the reactivity series and cannot replace magnesium as the substance before aluminium. The correct term is magnesium."},{"text":"hydrogen","correct":false,"explanation":"Hydrogen is a reference point for reactions with dilute acids, but it is not the substance listed before aluminium here. The correct term is magnesium."}]},{"id":"f8cc6c76-dd27-4555-887c-4d79ca444acf","cardType":"basic","points":1,"front":"Why is hydrogen included in the reactivity series?","back":"To predict which metals react with dilute acids.","mcqOptions":[{"text":"To predict which metals react with dilute acids.","correct":true,"explanation":"Hydrogen marks whether a metal is reactive enough to displace hydrogen from a dilute acid. Metals above hydrogen generally react with dilute acids to release hydrogen gas."},{"text":"To predict which metals react with concentrated alkalis.","correct":false,"explanation":"Hydrogen is not included to predict reactions with concentrated alkalis. Its position helps show which metals can displace hydrogen from dilute acids."},{"text":"To predict which metals react with water.","correct":false,"explanation":"Hydrogen's position does not predict which metals react with water specifically. It is included mainly to predict reactions between metals and dilute acids."},{"text":"To predict which metals are suitable for metal extraction.","correct":false,"explanation":"Hydrogen is not used as the reference for metal extraction. Carbon provides the important extraction reference, while hydrogen helps predict reactions with dilute acids."}]},{"id":"29d868dc-3d54-4132-ac0e-cd9cd804ae7b","cardType":"basic","points":1,"front":"Why is carbon included in the reactivity series?","back":"It is a useful reference point for metal extraction.","mcqOptions":[{"text":"It is a useful reference point for metal extraction.","correct":true,"explanation":"Carbon provides a useful reference for extraction: metals below carbon can often be extracted by reduction with carbon, while more reactive metals require electrolysis."},{"text":"It is a useful reference point for reactions with dilute acids.","correct":false,"explanation":"Hydrogen, not carbon, is the key reference for predicting metal reactions with dilute acids. Carbon is included mainly as a reference point for metal extraction."},{"text":"It is a useful reference point for melting points.","correct":false,"explanation":"Carbon is not included to compare melting points. Its position indicates whether a metal can commonly be extracted from its oxide using carbon."},{"text":"It is a useful reference point for solubility in water.","correct":false,"explanation":"Carbon does not primarily indicate solubility in water. Its position is valuable because it helps predict the method used for metal extraction."}]}]}],"examCountdown":null,"heading":"Reactivity series","title":"Reactivity series Flashcards","topbar":{"backHref":"/igcse/chemistry/cie/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"9e0785ab-3bd9-5463-adcd-aa3773a20a7b","walled":"$L38"}],"$L39","$L3a"]