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If atoms of any other element are present, the substance is not a hydrocarbon."},{"text":"A hydrocarbon contains carbon and oxygen atoms only.","correct":false,"explanation":"Confusing hydrocarbons with oxygen-containing organic compounds introduces oxygen incorrectly. A hydrocarbon contains only carbon and hydrogen atoms."},{"text":"A hydrocarbon contains hydrogen and oxygen atoms only.","correct":false,"explanation":"Hydrogen and oxygen alone form substances such as water, not hydrocarbons. Hydrocarbons must contain carbon and hydrogen atoms only."},{"text":"A hydrocarbon contains carbon and nitrogen atoms only.","correct":false,"explanation":"Nitrogen may occur in some organic compounds, but its presence means the compound is not a hydrocarbon. Hydrocarbons contain only carbon and hydrogen."}]},{"id":"565a9cdf-7302-41a7-a096-24feab72d92f","cardType":"basic","points":1,"front":"Why is crude oil a finite resource?","back":"It is used faster than it naturally forms, so it will run out.","mcqOptions":[{"text":"It is used faster than it naturally forms, so it will run out.","correct":true,"explanation":"Crude oil takes millions of years to form but is consumed rapidly. Its reserves are therefore depleted much faster than natural processes can replace them."},{"text":"It is formed faster than it is currently used, so it will run out.","correct":false,"explanation":"Formation faster than use would allow supplies to be replenished rather than depleted. Crude oil is finite because it is used faster than it naturally forms."},{"text":"It is too difficult to extract from rocks, so it will run out.","correct":false,"explanation":"Difficulty extracting a resource does not make it finite. Crude oil is finite because consumption occurs much faster than its extremely slow natural formation."},{"text":"It is found only beneath the Earth’s surface, so it will run out.","correct":false,"explanation":"Crude oil is stored underground, but its location is not why it is finite. It will run out because it is used faster than it forms."}]},{"id":"5df4e6b1-487f-409a-b6e8-db12b63d9840","cardType":"basic","points":1,"front":"Why must crude oil be separated before use?","back":"It is a complex mixture of hydrocarbons, not useful on its own.","mcqOptions":[{"text":"It is a complex mixture of hydrocarbons, not useful on its own.","correct":true,"explanation":"Crude oil contains many hydrocarbons with different properties. Separating this complex mixture produces fractions that are suitable for particular fuels and chemical feedstocks."},{"text":"It is a single compound of hydrocarbons, not useful on its own.","correct":false,"explanation":"Crude oil is not a single pure compound with uniform properties. It is a complex mixture of hydrocarbons, so it must be separated into useful fractions."},{"text":"It is a concentrated solution of hydrocarbons, not useful on its own.","correct":false,"explanation":"Crude oil does not mainly consist of dissolved ionic substances. It is a complex mixture of hydrocarbons whose different boiling points allow them to be separated."},{"text":"It is a pure element of hydrocarbons, not useful on its own.","correct":false,"explanation":"Crude oil is not an element because it contains numerous different compounds. It is a complex mixture of hydrocarbons that must be divided into useful fractions."}]},{"id":"8e1c6995-a11a-4fae-bf84-13e29bc50583","cardType":"cloze","points":null,"front":"Alkanes are saturated hydrocarbons with general formula [ ].","back":"Alkanes are saturated hydrocarbons with general formula C_nH_2n+2.","mcqOptions":[{"text":"C_nH_2n+2","correct":true,"explanation":"Acyclic alkanes contain only single carbon-carbon bonds, giving each molecule twice as many hydrogen atoms as carbon atoms, plus two additional hydrogen atoms."},{"text":"C_nH_2n","correct":false,"explanation":"The formula C_nH_2n belongs to alkenes with one carbon-carbon double bond. Saturated alkanes have the general formula C_nH_2n+2."},{"text":"C_nH_2n-2","correct":false,"explanation":"The formula C_nH_2n-2 is associated with alkynes containing a triple bond. Saturated alkanes instead have the formula C_nH_2n+2."},{"text":"C_nH_n+2","correct":false,"explanation":"Using n+2 hydrogen atoms overlooks carbon’s valency of four and does not describe the alkane homologous series. The correct general formula is C_nH_2n+2."}]},{"id":"4bcbc8c2-681c-44c3-b48d-bbb3c088daa2","cardType":"basic","points":1,"front":"What bonding feature makes alkanes saturated?","back":"They contain only single C-C covalent bonds.","mcqOptions":[{"text":"They contain only single C-C covalent bonds.","correct":true,"explanation":"Alkanes are saturated because every carbon-carbon bond is single. This leaves each carbon bonded to the maximum possible number of hydrogen atoms."},{"text":"They contain only double C=C covalent bonds.","correct":false,"explanation":"A carbon-carbon double bond makes a hydrocarbon unsaturated and identifies the alkene functional group. Alkanes contain only single C-C covalent bonds."},{"text":"They contain only triple C≡C covalent bonds.","correct":false,"explanation":"Triple carbon-carbon bonds occur in alkynes and make them unsaturated. Alkanes are saturated because they contain only single C-C covalent bonds."},{"text":"They contain only single C-C ionic bonds.","correct":false,"explanation":"Carbon and hydrogen are joined by covalent bonds, not ionic bonds. Saturation specifically means that all carbon-carbon covalent bonds in an alkane are single."}]},{"id":"39292cc2-e851-4f48-9bf8-a197d8ada6c6","cardType":"cloze","points":null,"front":"Fractional distillation separates hydrocarbons by their different [ ].","back":"Fractional distillation separates hydrocarbons by their different boiling points.","mcqOptions":[{"text":"boiling points","correct":true,"explanation":"Hydrocarbons vaporise and condense at different temperatures, allowing them to be collected at different heights in the fractionating column according to their boiling points."},{"text":"relative densities","correct":false,"explanation":"Density differences are not the basis of fractional distillation. The process separates hydrocarbons because they have different boiling points and therefore condense at different temperatures."},{"text":"molecular masses","correct":false,"explanation":"Hydrocarbons may have different molecular masses, but the column separates them directly according to their different boiling points, not by weighing their molecules."},{"text":"combustion temperatures","correct":false,"explanation":"Combustion temperatures concern how substances burn, whereas fractional distillation involves vaporisation and condensation. Hydrocarbons are separated by their different boiling points."}]},{"id":"f6b476af-41c4-4568-ab93-40e86ee7959b","cardType":"basic","points":2,"front":"Why do longer-chain hydrocarbons have higher boiling points?","back":"

Larger molecules have stronger intermolecular forces.
More thermal energy is needed to separate them.

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

Larger molecules have stronger intermolecular forces.
More thermal energy is needed to separate them.

","correct":true,"explanation":"Longer hydrocarbon molecules have larger electron clouds and greater contact areas, producing stronger intermolecular attractions. More thermal energy is consequently required to overcome these forces."},{"text":"

Larger molecules have stronger covalent bonds.
More thermal energy is needed to break them.

","correct":false,"explanation":"Boiling does not break the covalent bonds within hydrocarbon molecules. Longer chains have stronger intermolecular forces, so more thermal energy is needed to separate the molecules."},{"text":"

Larger molecules have weaker intermolecular forces.
Less thermal energy is needed to separate them.

","correct":false,"explanation":"This reverses the chain-length trend. Larger molecules experience stronger, not weaker, intermolecular forces, so more thermal energy is needed to separate them during boiling."},{"text":"

Larger molecules have stronger intermolecular forces.
More thermal energy is needed to break their bonds.

","correct":false,"explanation":"Stronger intermolecular forces are correctly identified, but boiling overcomes these forces rather than breaking covalent bonds. More thermal energy is needed to separate whole molecules."}]},{"id":"d82a1fbc-cc35-4fc2-b7e7-3895a31aec98","cardType":"basic","points":1,"front":"What happens when hydrocarbon vapour reaches a tray cooler than its boiling point?","back":"It condenses into a liquid.","mcqOptions":[{"text":"It condenses into a liquid.","correct":true,"explanation":"Below its boiling point, a hydrocarbon vapour changes state from gas to liquid. This condensation allows the liquid fraction to be collected from the tray."},{"text":"It evaporates into a liquid.","correct":false,"explanation":"Evaporation is the change from liquid to gas and requires heating. Vapour reaching a tray below its boiling point instead condenses into a liquid."},{"text":"It freezes into a liquid.","correct":false,"explanation":"Freezing changes a liquid into a solid and occurs at the freezing point. Hydrocarbon vapour cooled below its boiling point condenses into a liquid."},{"text":"It sublimes into a liquid.","correct":false,"explanation":"Sublimation is a direct change between solid and gas, so it does not describe this stage. Cooled hydrocarbon vapour condenses into a liquid."}]},{"id":"06fd22a2-2e31-4b56-9902-bfe193c5b1d6","cardType":"basic","points":2,"front":"Why is cracking used in the oil industry?","back":"To convert surplus long-chain hydrocarbons into in-demand short-chain ones.","mcqOptions":[{"text":"To convert surplus long-chain hydrocarbons into in-demand short-chain ones.","correct":true,"explanation":"Cracking increases the supply of useful short-chain hydrocarbons by breaking down less-demanded surplus long-chain molecules, helping refineries match the market demand for fuels and chemical feedstocks."},{"text":"To convert surplus short-chain hydrocarbons into in-demand long-chain ones.","correct":false,"explanation":"Cracking breaks hydrocarbons into smaller molecules rather than joining short chains together. It is used to convert surplus long-chain hydrocarbons into more valuable, in-demand short-chain ones."},{"text":"To remove unwanted impurities from crude oil before fractional distillation.","correct":false,"explanation":"Removing impurities is part of refining but is not the purpose of cracking. Cracking converts surplus long-chain hydrocarbons into smaller hydrocarbons for which demand is greater."},{"text":"To separate useful hydrocarbon fractions by their boiling points.","correct":false,"explanation":"Fractional distillation separates existing hydrocarbons without converting their molecules. Cracking is a chemical process used to turn surplus long-chain hydrocarbons into in-demand short-chain ones."}]},{"id":"e65201e8-48a8-4203-aa9f-fc4e34fa23ec","cardType":"basic","points":2,"front":"What products are formed when a long-chain alkane is cracked?","back":"

A short-chain alkane.
At least one alkene.

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

A short-chain alkane.
At least one alkene.

","correct":true,"explanation":"Cracking breaks a long-chain alkane into smaller hydrocarbons. The products include a short-chain alkane and at least one alkene containing a carbon-carbon double bond."},{"text":"

A short-chain alkane.
At least one long-chain alkane.

","correct":false,"explanation":"Cracking does not normally produce only saturated molecules; breaking the original chain leaves at least one unsaturated product. It forms a short-chain alkane and at least one alkene."},{"text":"

A hydrogen molecule.
At least one carbon dioxide molecule.

","correct":false,"explanation":"Hydrogen and carbon dioxide are not the characteristic products of cracking an alkane. Cracking instead forms a short-chain alkane and at least one alkene."},{"text":"

A short-chain alcohol.
At least one carboxylic acid.

","correct":false,"explanation":"Alcohols and carboxylic acids contain oxygen, which is absent from the alkane being cracked. The products are a short-chain alkane and at least one alkene."}]},{"id":"3a33a3e4-148e-4061-a754-fc5eff091e63","cardType":"cloze","points":null,"front":"Catalytic cracking heats hydrocarbon vapour to about [ ] and passes it over a hot [ ].","back":"Catalytic cracking heats hydrocarbon vapour to about 550 °C and passes it over a hot catalyst.","mcqOptions":[{"text":"Catalytic cracking heats hydrocarbon vapour to about 550 °C and passes it over a hot catalyst.","correct":true,"explanation":"In catalytic cracking, hydrocarbon vapour is heated to approximately 550 °C and passed over a hot catalyst, which speeds up the breaking of long hydrocarbon chains."},{"text":"Catalytic cracking heats hydrocarbon vapour to about 100 °C and passes it over a hot catalyst.","correct":false,"explanation":"A temperature near 550 °C is needed to provide enough energy for catalytic cracking. At 100 °C, the vapour is instead insufficiently heated before passing over the catalyst."},{"text":"Catalytic cracking heats hydrocarbon vapour to about 550 °C and passes it over a hot oxygen supply.","correct":false,"explanation":"Oxygen would encourage combustion rather than catalyse cracking. The hydrocarbon vapour is heated to about 550 °C and passed over a hot catalyst, which speeds up the reaction."},{"text":"Catalytic cracking heats hydrocarbon vapour to about 1000 °C and passes it over a hot oxygen supply.","correct":false,"explanation":"This confuses catalytic cracking with combustion conditions. Catalytic cracking uses about 550 °C and a hot catalyst, rather than the much higher stated temperature and an oxygen supply."}]},{"id":"36f2b4c9-cac7-411f-a7f4-8926bae77cbe","cardType":"cloze","points":null,"front":"Alkenes contain a reactive [ ] and have general formula [ ].","back":"Alkenes contain a reactive C=C double bond and have general formula C_nH_2n.","mcqOptions":[{"text":"Alkenes contain a reactive C=C double bond and have general formula C_nH_2n.","correct":true,"explanation":"Alkenes are unsaturated because they contain a reactive carbon-carbon double bond. A non-cyclic alkene with one double bond has the general formula C_nH_2n."},{"text":"Alkenes contain a reactive C-C single bond and have general formula C_nH_2n.","correct":false,"explanation":"A carbon-carbon single bond is characteristic of saturated hydrocarbons and does not define an alkene. Alkenes contain a C=C double bond and have the general formula C_nH_2n."},{"text":"Alkenes contain a reactive C=C double bond and have general formula C_nH_2n+2.","correct":false,"explanation":"C_nH_2n+2 is the general formula for alkanes, not alkenes. Alkenes contain a C=C double bond and have two fewer hydrogen atoms, giving C_nH_2n."},{"text":"Alkenes contain a reactive C≡C triple bond and have general formula C_nH_2n-2.","correct":false,"explanation":"A carbon-carbon triple bond and the formula C_nH_2n-2 describe alkynes. Alkenes instead contain a C=C double bond and have the formula C_nH_2n."}]},{"id":"d5d840e7-c9e7-40f0-a8e4-45577abb5241","cardType":"basic","points":1,"front":"Why is there no compound called methene?","back":"A C=C double bond needs at least two carbon atoms.","mcqOptions":[{"text":"A C=C double bond needs at least two carbon atoms.","correct":true,"explanation":"A carbon-carbon double bond must connect two carbon atoms. Methene would contain only one carbon atom, so it cannot possess the defining C=C bond of an alkene."},{"text":"A C=C double bond needs at least four hydrogen atoms.","correct":false,"explanation":"Although alkenes contain hydrogen, the number of hydrogen atoms is not what prevents methene from existing. A C=C double bond requires at least two carbon atoms."},{"text":"A C=C double bond needs at least two oxygen atoms.","correct":false,"explanation":"A C=C bond specifically joins carbon atoms, not oxygen atoms. Methene cannot exist because forming the defining double bond requires at least two carbon atoms."},{"text":"A C=C double bond needs at least three carbon atoms.","correct":false,"explanation":"Two carbon atoms are sufficient to form the C=C bond, as demonstrated by ethene. Methene is impossible because its single carbon atom cannot form a carbon-carbon double bond."}]},{"id":"bda23de3-bcf5-4537-ae5d-45854332c297","cardType":"basic","points":1,"front":"What is the positive bromine water test for an alkene?","back":"Orange bromine water turns colourless.","mcqOptions":[{"text":"Orange bromine water turns colourless.","correct":true,"explanation":"An alkene reacts with bromine by addition across its C=C double bond, consuming the orange bromine and making the bromine water turn colourless."},{"text":"Orange bromine water turns blue-black.","correct":false,"explanation":"A blue-black colour is associated with the iodine test for starch, not the alkene test. An alkene decolourises orange bromine water because bromine adds across its C=C bond."},{"text":"Orange bromine water turns brick-red.","correct":false,"explanation":"A brick-red precipitate is associated with a positive Benedict’s test for reducing sugars. An alkene instead reacts with bromine, causing orange bromine water to turn colourless."},{"text":"Orange bromine water turns purple.","correct":false,"explanation":"Bromine water does not turn purple when an alkene is present. The alkene consumes bromine in an addition reaction, so the original orange solution becomes colourless."}]},{"id":"8aa7101d-adf2-4d80-af85-cfc217e28f09","cardType":"basic","points":1,"front":"Why are alkenes more reactive than alkanes?","back":"Alkenes contain an unstable, reactive C=C double bond.","mcqOptions":[{"text":"Alkenes contain an unstable, reactive C=C double bond.","correct":true,"explanation":"The carbon-carbon double bond in an alkene includes a relatively weak, reactive component that can open during addition reactions, making alkenes more reactive than alkanes."},{"text":"Alkenes contain an unstable, reactive C-C single bond.","correct":false,"explanation":"Carbon-carbon single bonds are present in both alkanes and alkenes and do not explain their different reactivities. Alkenes are more reactive because they contain a reactive C=C double bond."},{"text":"Alkenes contain an unstable, reactive C≡C triple bond.","correct":false,"explanation":"A carbon-carbon triple bond defines an alkyne rather than an alkene. The greater reactivity of alkenes compared with alkanes comes from their reactive C=C double bond."},{"text":"Alkenes contain an unstable, reactive O-H single bond.","correct":false,"explanation":"Alkenes are hydrocarbons and therefore do not contain an O-H bond. Their greater reactivity arises from the unstable, reactive C=C double bond that undergoes addition reactions."}]},{"id":"a02b32c8-f22e-460d-aabd-fb6abddbb320","cardType":"basic","points":1,"front":"What does hydrogenation of an alkene produce?","back":"The corresponding saturated alkane.","mcqOptions":[{"text":"The corresponding saturated alkane.","correct":true,"explanation":"Hydrogenation adds hydrogen across an alkene’s C=C double bond, converting it into a C-C single bond and producing the corresponding saturated alkane."},{"text":"The corresponding saturated alcohol.","correct":false,"explanation":"Hydration, not hydrogenation, produces an alcohol by adding water across the double bond. Hydrogenation adds hydrogen and forms the corresponding saturated alkane."},{"text":"The corresponding saturated alkyne.","correct":false,"explanation":"An alkyne contains a carbon-carbon triple bond and is more unsaturated than an alkene. Hydrogenation removes unsaturation by producing the corresponding saturated alkane."},{"text":"The corresponding saturated carboxylic acid.","correct":false,"explanation":"Hydrogenation does not introduce the carboxyl functional group or oxygen atoms. It adds hydrogen across the C=C bond to produce the corresponding saturated alkane."}]},{"id":"be6efba8-cad5-4807-9748-a9f51b9dec59","cardType":"cloze","points":null,"front":"Alkenes react with steam using a [ ] to produce [ ].","back":"Alkenes react with steam using a phosphoric acid catalyst to produce alcohols.","mcqOptions":[{"text":"Alkenes react with steam using a phosphoric acid catalyst to produce alcohols.","correct":true,"explanation":"Steam hydrates the alkene across its C=C bond. A phosphoric acid catalyst speeds this reaction, and the addition of H and OH forms an alcohol."},{"text":"Alkenes react with steam using a nickel catalyst to produce alcohols.","correct":false,"explanation":"Nickel catalyses hydrogenation rather than hydration. Steam reacts with alkenes using a phosphoric acid catalyst, adding H and OH across the double bond to produce alcohols."},{"text":"Alkenes react with steam using a phosphoric acid catalyst to produce carboxylic acids.","correct":false,"explanation":"Carboxylic acids can be produced by oxidising suitable alcohols, not by directly hydrating alkenes. Reaction with steam adds H and OH to produce alcohols."},{"text":"Alkenes react with steam using a concentrated sulfuric acid catalyst to produce aldehydes.","correct":false,"explanation":"Concentrated sulfuric acid is associated with other organic reactions, while aldehydes form through controlled oxidation. Alkene hydration uses phosphoric acid and steam to produce alcohols."}]},{"id":"19762dbd-63a9-4720-a4e0-993c9f2c7f30","cardType":"basic","points":1,"front":"What product forms when alcohols are oxidised?","back":"Carboxylic acids.","mcqOptions":[{"text":"Carboxylic acids.","correct":true,"explanation":"Oxidising an alcohol adds oxygen or removes hydrogen. Under the expected GCSE conditions, oxidation proceeds to form a compound containing the carboxyl functional group."},{"text":"Alkenes.","correct":false,"explanation":"Alkenes are normally formed by dehydrating alcohols, which removes water rather than oxidising them. Oxidation of alcohols produces carboxylic acids in this context."},{"text":"Esters.","correct":false,"explanation":"Esters form when alcohols react with carboxylic acids in esterification, not when alcohols are oxidised. The expected oxidation products here are carboxylic acids."},{"text":"Alkanes.","correct":false,"explanation":"Alkanes contain fewer oxygen atoms than alcohols, so producing them would involve reduction rather than oxidation. Oxidising alcohols gives carboxylic acids in this reaction."}]},{"id":"056ec0a1-a466-450b-98db-deef3735d3bd","cardType":"cloze","points":null,"front":"Carboxylic acids contain the [ ] functional group and their names end in [ ].","back":"Carboxylic acids contain the -COOH functional group and their names end in -anoic acid.","mcqOptions":[{"text":"Carboxylic acids contain the -COOH functional group and their names end in -anoic acid.","correct":true,"explanation":"The carboxyl functional group is -COOH. Carboxylic acid names retain the alkane stem for the carbon count and use the ending -anoic acid."},{"text":"Carboxylic acids contain the -OH functional group and their names end in -anoic acid.","correct":false,"explanation":"The -OH group alone identifies an alcohol, even though it is part of the larger carboxyl group. Carboxylic acids contain -COOH and end in -anoic acid."},{"text":"Carboxylic acids contain the -COOH functional group and their names end in -anol.","correct":false,"explanation":"The ending -anol belongs to alcohols and reflects their hydroxyl group. Compounds containing the -COOH carboxyl group instead have names ending in -anoic acid."},{"text":"Carboxylic acids contain the -CHO functional group and their names end in -anal.","correct":false,"explanation":"The -CHO group and -anal ending identify aldehydes, not carboxylic acids. Carboxylic acids contain the -COOH group and use the ending -anoic acid."}]},{"id":"81e78fd4-7655-4e84-a97a-8f76a2adb033","cardType":"basic","points":2,"front":"Why does ethanoic acid have two carbon atoms in total?","back":"The -COOH carbon counts as one of the eth- carbons.","mcqOptions":[{"text":"The -COOH carbon counts as one of the eth- carbons.","correct":true,"explanation":"Ethanoic acid is CH3COOH: the methyl group contributes one carbon and the -COOH group contributes another. Both are included in the two-carbon eth- chain."},{"text":"The methyl-group carbon counts as both of the eth- carbons.","correct":false,"explanation":"The CH3 group contains only one carbon atom, not two. Ethanoic acid has two carbons because the carbon in its -COOH group is also counted."},{"text":"The two oxygen atoms count as the two eth- carbons.","correct":false,"explanation":"Oxygen atoms do not count towards the carbon-chain prefix. In CH3COOH, one carbon comes from CH3 and the other is the carbon within -COOH."},{"text":"The -COOH carbon is excluded from the eth- carbon count.","correct":false,"explanation":"Excluding the carboxyl carbon is a common naming mistake. The -COOH carbon must be counted, giving two total carbon atoms and therefore the prefix eth-."}]},{"id":"bb07f286-d37f-4c88-8749-6b31b68ee45d","cardType":"basic","points":2,"front":"What happens to C=C bonds during addition polymerisation?","back":"They open into single bonds, linking monomers into chains.","mcqOptions":[{"text":"They open into single bonds, linking monomers into chains.","correct":true,"explanation":"The alkene C=C double bond opens so each monomer can form new single bonds to neighbouring monomers. Repetition of this process builds the polymer chain."},{"text":"They remain as double bonds, linking monomers into chains.","correct":false,"explanation":"If the double bonds remained unchanged, the monomers could not make the new bonds needed for chain formation. They open into single bonds that link adjacent monomers."},{"text":"They break completely, releasing carbon atoms from the chains.","correct":false,"explanation":"Addition polymerisation rearranges the bonding electrons but does not release carbon atoms. The C=C bonds open into single bonds, allowing all monomers to remain in the chain."},{"text":"They change into triple bonds, linking monomers into chains.","correct":false,"explanation":"A C=C bond does not gain another shared electron pair during addition polymerisation. It opens into single bonds, which connect each monomer to its neighbours."}]},{"id":"5a428c95-f81b-4ef7-8660-25334196ba9d","cardType":"basic","points":1,"front":"What by-product forms during addition polymerisation?","back":"None.","mcqOptions":[{"text":"None.","correct":true,"explanation":"In addition polymerisation, every atom from each alkene monomer is incorporated into the polymer chain. No small molecule is removed, so there is no by-product."},{"text":"Water.","correct":false,"explanation":"Water is commonly removed during condensation polymerisation, not addition polymerisation. Addition polymers form by opening C=C bonds, with all monomer atoms retained and no by-product."},{"text":"Hydrogen chloride.","correct":false,"explanation":"Hydrogen chloride may be eliminated in some condensation reactions involving acyl chlorides. Addition polymerisation simply opens C=C bonds and produces no separate by-product."},{"text":"Carbon dioxide.","correct":false,"explanation":"Carbon dioxide is not released when alkene monomers undergo addition polymerisation. The monomers join directly through opened double bonds, so no by-product forms."}]},{"id":"d71c1a50-289f-4d11-9e96-4f44a93bd3c4","cardType":"basic","points":1,"front":"What small molecule may be lost during condensation polymerisation?","back":"Water or hydrogen chloride.","mcqOptions":[{"text":"Water or hydrogen chloride.","correct":true,"explanation":"Condensation polymerisation joins functional groups while eliminating a small molecule. Depending on the monomers used, this eliminated molecule may be water or hydrogen chloride."},{"text":"Hydrogen or oxygen.","correct":false,"explanation":"Hydrogen and oxygen are not separately eliminated in standard condensation polymerisation. The reacting functional groups instead commonly release water or hydrogen chloride as a small molecule."},{"text":"Carbon dioxide or methane.","correct":false,"explanation":"Carbon dioxide and methane are not the characteristic eliminated molecules in condensation polymerisation. Reactions producing polyesters or polyamides commonly lose water or hydrogen chloride."},{"text":"Ethene or ethanol.","correct":false,"explanation":"Ethene and ethanol are organic starting materials or products in other reactions, not typical condensation by-products. Condensation polymerisation may instead eliminate water or hydrogen chloride."}]},{"id":"501deac5-e528-4cb2-873d-5621e5ec1344","cardType":"basic","points":2,"front":"Why do condensation polymer monomers need functional groups at both ends?","back":"So each monomer can link at both ends into a chain.","mcqOptions":[{"text":"So each monomer can link at both ends into a chain.","correct":true,"explanation":"A functional group at each end allows a monomer to react with two neighbours. Repeating these reactions extends the structure in both directions to form a chain."},{"text":"So each monomer can link at one end only into a chain.","correct":false,"explanation":"A monomer that can react at only one end terminates growth rather than extending the polymer. Two reactive ends allow linkage to neighbouring monomers on both sides."},{"text":"So each monomer can act as a catalyst at both ends during chain formation.","correct":false,"explanation":"Condensation monomers do not need terminal functional groups to act as catalysts. The groups react with neighbouring monomers, allowing each unit to link at both ends."},{"text":"So each monomer can open C=C bonds at both ends into a chain.","correct":false,"explanation":"Opening C=C bonds describes addition polymerisation and does not explain two terminal functional groups. Condensation monomers need reactive groups at both ends to build a continuous chain."}]},{"id":"a14a26cd-5be9-4cc4-b00c-3c5f10e4438c","cardType":"cloze","points":null,"front":"DNA monomers are [ ]; protein monomers are [ ].","back":"DNA monomers are nucleotides; protein monomers are amino acids.","mcqOptions":[{"text":"DNA monomers are nucleotides; protein monomers are amino acids.","correct":true,"explanation":"DNA is built from nucleotide monomers, while proteins are polypeptides assembled by joining amino acid monomers through peptide bonds."},{"text":"DNA monomers are monosaccharides; protein monomers are amino acids.","correct":false,"explanation":"Monosaccharides are the monomers of carbohydrates, not DNA. DNA monomers are nucleotides, while the monomers used to build proteins are amino acids."},{"text":"DNA monomers are nucleotides; protein monomers are fatty acids.","correct":false,"explanation":"Fatty acids contribute to lipid formation rather than acting as protein monomers. DNA consists of nucleotides, whereas proteins are assembled from amino acids."},{"text":"DNA monomers are amino acids; protein monomers are nucleotides.","correct":false,"explanation":"This reverses the two biological monomers. Nucleotides join to form DNA, while amino acids join through peptide bonds to form proteins."}]},{"id":"83eca592-66f0-4019-a58c-2233bf83583e","cardType":"basic","points":2,"front":"In a simple chemical cell, why do electrons flow between the electrodes?","back":"The more reactive metal loses electrons to the less reactive metal.","mcqOptions":[{"text":"The more reactive metal loses electrons to the less reactive metal.","correct":true,"explanation":"The greater tendency of the more reactive metal to oxidise means it releases electrons. These electrons travel through the external circuit towards the less reactive metal."},{"text":"The less reactive metal loses electrons to the more reactive metal.","correct":false,"explanation":"This reverses the direction of electron transfer. The more reactive metal is more easily oxidised, so it loses electrons to the less reactive metal."},{"text":"The more reactive metal gains electrons from the less reactive metal.","correct":false,"explanation":"Gaining electrons describes reduction, but the more reactive metal undergoes oxidation in a simple cell. It therefore loses electrons to the less reactive metal."},{"text":"The less reactive metal gains electrons from the more reactive metal.","correct":false,"explanation":"The less reactive metal does not send electrons to the more reactive one. Electrons are released by oxidation of the more reactive metal and flow towards the less reactive metal."}]},{"id":"049750fb-2c6b-47e7-a2da-b9e48671f3a5","cardType":"cloze","points":null,"front":"The overall hydrogen-oxygen fuel cell reaction is [ ].","back":"The overall hydrogen-oxygen fuel cell reaction is 2H₂ + O₂ → 2H₂O.","mcqOptions":[{"text":"2H₂ + O₂ → 2H₂O","correct":true,"explanation":"Hydrogen reacts with oxygen to produce water. The coefficients balance four hydrogen atoms and two oxygen atoms on each side of the overall equation."},{"text":"H₂ + O₂ → H₂O","correct":false,"explanation":"This represents the correct substances but is not balanced: there are two oxygen atoms on the left and only one on the right. The balanced equation uses 2H₂O."},{"text":"2H₂ + O₂ → 2H₂O₂","correct":false,"explanation":"Hydrogen-oxygen fuel cells produce water, not hydrogen peroxide. Combining two hydrogen molecules with one oxygen molecule gives two water molecules overall."},{"text":"2H₂O → 2H₂ + O₂","correct":false,"explanation":"This is the reverse process, corresponding to splitting water rather than operating a fuel cell. In the fuel cell, hydrogen and oxygen react to form water."}]}]}],"examCountdown":{"examDate":"2027-05-17","paperLabel":"Paper 1"},"heading":"Organic chemistry","title":"Organic chemistry Flashcards","topbar":{"backHref":"/gcse/chemistry/ocr/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"ecc7a1cb-e03b-56ee-9780-e756f3f6103c","walled":"$L38"}],"$L39","$L3a"]