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22:[["$","$L31",null,{"feature":"flashcards"}],"$L32",["$","$L33",null,{"href":"/igcse/chemistry/edexcel/alcohols/flashcards","label":"Alcohols","subjectCode":"igcse_chemistry","surface":"flashcards"}],["$","$L34",null,{"runner":["$","div",null,{"className":"min-h-0 flex-1 overflow-hidden bg-background","children":["$","$L35",null,{"decks":[{"id":"ebc2fd56-70ca-4ba3-a963-e0739400c58d","title":"Alcohols Flashcards","topicId":"d5d6d4a2-692a-5721-9f83-2c07d0472001","topicSlug":"alcohols","cards":[{"id":"366bb496-4d28-47cf-a43c-06ad5e523cc1","cardType":"basic","points":1,"front":"What is the name and formula of the functional group in alcohols?","back":"The hydroxyl group, -OH.","mcqOptions":[{"text":"The hydroxyl group, -OH.","correct":true,"explanation":"Alcohols contain the hydroxyl functional group, written -OH. The oxygen and hydrogen are covalently bonded, and this group gives alcohols many of their characteristic reactions."},{"text":"The carbonyl group, C=O.","correct":false,"explanation":"The carbonyl group is found in aldehydes, ketones and some other compounds, not alcohols. Alcohols contain the hydroxyl group, written -OH."},{"text":"The carboxyl group, -COOH.","correct":false,"explanation":"The carboxyl group identifies carboxylic acids such as ethanoic acid. Alcohols instead contain the hydroxyl group, written -OH, attached to a carbon chain."},{"text":"The amino group, -NH_2.","correct":false,"explanation":"The amino group is characteristic of amines and contains nitrogen. Alcohols have no nitrogen in their functional group; their functional group is the hydroxyl group, -OH."}]},{"id":"b2da019d-fde0-48d4-a553-18b72d57992d","cardType":"basic","points":1,"front":"How does the –OH group in an alcohol differ from a hydroxide ion ($OH^-$)?","back":"It is neutral and covalently bonded to a carbon chain.","mcqOptions":[{"text":"It is neutral and covalently bonded to a carbon chain.","correct":true,"explanation":"In an alcohol, the -OH group is part of a neutral molecule and is covalently bonded to carbon. A hydroxide ion is a separate negatively charged ion, $OH^-$."},{"text":"It is negative and ionically bonded to a carbon chain.","correct":false,"explanation":"This confuses an alcohol with hydroxide. Alcohols contain a neutral -OH group joined to carbon by covalent bonding, whereas hydroxide is the negatively charged ion $OH^-$."},{"text":"It is neutral and ionically bonded to a carbon chain.","correct":false,"explanation":"The -OH group in an alcohol is neutral, but the bond to the carbon chain is covalent, not ionic. Ionic bonding would involve oppositely charged ions."},{"text":"It is negative and covalently bonded to a carbon chain.","correct":false,"explanation":"Although the atoms in the -OH group are covalently bonded to carbon, the group in an alcohol is neutral. The negative charge belongs to the hydroxide ion, $OH^-$."}]},{"id":"2e8aec29-225f-4d3b-8198-6fe5d28b5cce","cardType":"basic","points":2,"front":"What are the prefixes for carbon chains of length 1, 2, 3, and 4?","back":"

1: meth-
2: eth-
3: prop-
4: but-

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

1: meth-
2: eth-
3: prop-
4: but-

","correct":true,"explanation":"The prefixes count carbon atoms in the chain: meth- represents one, eth- two, prop- three and but- four. These prefixes form names such as methanol and butanol."},{"text":"

1: eth-
2: meth-
3: but-
4: prop-

","correct":false,"explanation":"The prefixes have been shifted between chain lengths. The correct order is meth- for one carbon, eth- for two, prop- for three and but- for four."},{"text":"

1: prop-
2: but-
3: meth-
4: eth-

","correct":false,"explanation":"These prefixes do not follow the carbon-count sequence. One, two, three and four carbon chains are named meth-, eth-, prop- and but-, respectively."},{"text":"

1: but-
2: prop-
3: eth-
4: meth-

","correct":false,"explanation":"This reverses the usual naming sequence. Carbon-chain prefixes increase as meth-, eth-, prop- and but- for one through four carbon atoms."}]},{"id":"93ce3709-7d07-44b8-bc0f-d582afecf0f0","cardType":"basic","points":1,"front":"What is the structural formula of propan-1-ol?","back":"$$CH_3CH_2CH_2OH$","mcqOptions":[{"text":"$$CH_3CH_2CH_2OH$","correct":true,"explanation":"Propan- means a three-carbon chain, and -1-ol places the hydroxyl group at carbon 1. The structural formula is therefore $CH_3CH_2CH_2OH$."},{"text":"$$CH_3CH_2OH$","correct":false,"explanation":"This formula contains only two carbon atoms, so it is ethanol. Propan-1-ol must have three carbons with the hydroxyl group at the end: $CH_3CH_2CH_2OH$."},{"text":"$$CH_3CH(OH)CH_3$","correct":false,"explanation":"This has three carbon atoms but the hydroxyl group is attached to carbon 2, making propan-2-ol. Propan-1-ol has the hydroxyl group at the end: $CH_3CH_2CH_2OH$."},{"text":"$$CH_3CH_2CH_2CH_2OH$","correct":false,"explanation":"This formula contains four carbon atoms, so it is butan-1-ol rather than propan-1-ol. The propan-1-ol formula has three carbons: $CH_3CH_2CH_2OH$."}]},{"id":"6e530574-5605-49c2-b129-12b2fedceec2","cardType":"basic","points":1,"front":"What are the products of the complete combustion of ethanol?","back":"Carbon dioxide ($CO_2$) and water ($H_2O$).","mcqOptions":[{"text":"Carbon dioxide ($CO_2$) and water ($H_2O$).","correct":true,"explanation":"Complete combustion supplies enough oxygen to oxidise all the carbon to carbon dioxide and all the hydrogen to water. Ethanol therefore produces carbon dioxide and water."},{"text":"Carbon monoxide ($CO$) and water ($H_2O$).","correct":false,"explanation":"Carbon monoxide forms during incomplete combustion when oxygen is limited. Complete combustion of ethanol produces carbon dioxide and water instead."},{"text":"Carbon dioxide ($CO_2$) and hydrogen ($H_2$).","correct":false,"explanation":"Hydrogen gas is not the hydrogen-containing product of complete combustion. The hydrogen atoms are oxidised to water, while carbon forms carbon dioxide."},{"text":"Methane ($CH_4$) and water ($H_2O$).","correct":false,"explanation":"Methane is not produced by combustion of ethanol. Complete combustion fully oxidises ethanol, giving carbon dioxide from its carbon and water from its hydrogen."}]},{"id":"39027143-89da-4728-a49e-be3f1e651f38","cardType":"basic","points":2,"front":"State the balanced chemical equation for the complete combustion of ethanol.","back":"$$C_2H_5OH + 3O_2 \\rightarrow 2CO_2 + 3H_2O$","mcqOptions":[{"text":"$$C_2H_5OH + 3O_2 \\rightarrow 2CO_2 + 3H_2O$","correct":true,"explanation":"The equation balances two carbon atoms as $2CO_2$, six hydrogen atoms as $3H_2O$, and six oxygen atoms on each side. It therefore represents complete ethanol combustion."},{"text":"$$C_2H_5OH + 2O_2 \\rightarrow 2CO_2 + 3H_2O$","correct":false,"explanation":"The products contain eight oxygen atoms, but this equation provides only five on the reactant side. Three oxygen molecules are needed to balance complete combustion correctly."},{"text":"$$C_2H_5OH + 3O_2 \\rightarrow CO_2 + 3H_2O$","correct":false,"explanation":"One carbon atom is missing from the products. Ethanol contains two carbon atoms, so complete combustion requires $2CO_2$ as well as $3H_2O$."},{"text":"$$C_2H_5OH + 4O_2 \\rightarrow 2CO_2 + 3H_2O$","correct":false,"explanation":"Four oxygen molecules give too many oxygen atoms on the reactant side. Counting oxygen atoms shows that three $O_2$ molecules balance the equation."}]},{"id":"15f2c816-4f1f-4754-8900-222b7743750a","cardType":"basic","points":1,"front":"What substance is produced when ethanol undergoes microbial oxidation in air?","back":"Ethanoic acid ($CH_3COOH$)","mcqOptions":[{"text":"Ethanoic acid ($CH_3COOH$)","correct":true,"explanation":"Microbial oxidation of ethanol in air converts the alcohol into ethanoic acid. This is the acid responsible for the sour taste and smell of vinegar."},{"text":"Ethene ($C_2H_4$)","correct":false,"explanation":"Ethene is produced by dehydration of ethanol, not microbial oxidation in air. Microbial oxidation converts ethanol into ethanoic acid, $CH_3COOH$."},{"text":"Ethanal ($CH_3CHO$)","correct":false,"explanation":"Ethanal can be an intermediate formed during oxidation of ethanol, but microbial oxidation in air continues to ethanoic acid, $CH_3COOH$."},{"text":"Ethane ($C_2H_6$)","correct":false,"explanation":"Ethane is an alkane and is not the oxidation product of ethanol. Oxidation adds oxygen overall, producing ethanoic acid, $CH_3COOH$."}]},{"id":"552d383f-63a3-43c1-b9ec-48aec76b960b","cardType":"basic","points":2,"front":"Describe the colour change when ethanol is heated with acidified potassium dichromate(VI).","back":"From orange to green.","mcqOptions":[{"text":"From orange to green.","correct":true,"explanation":"Ethanol reduces acidified potassium dichromate(VI) during oxidation. Chromium(VI) ions are orange, while the chromium(III) ions formed are green."},{"text":"From green to orange.","correct":false,"explanation":"This reverses the observed change. Acidified potassium dichromate(VI) starts orange and is reduced to green chromium(III) ions as ethanol is oxidised."},{"text":"From purple to colourless.","correct":false,"explanation":"Purple to colourless describes some reactions involving permanganate, not acidified potassium dichromate(VI). Dichromate(VI) changes from orange to green during ethanol oxidation."},{"text":"From colourless to orange.","correct":false,"explanation":"The reagent is already orange before the reaction, so it does not become orange. Ethanol reduces dichromate(VI), changing the colour from orange to green."}]},{"id":"212c6c69-d468-4aeb-9d67-6675a438590b","cardType":"cloze","points":null,"front":"Heating ethanol with [ ] produces ethanoic acid and water.","back":"Heating ethanol with acidified potassium dichromate(VI) produces ethanoic acid and water.","mcqOptions":[{"text":"acidified potassium dichromate(VI)","correct":true,"explanation":"Acidified potassium dichromate(VI) is an oxidising agent that supplies oxygen to oxidise ethanol fully into ethanoic acid, with water also formed."},{"text":"concentrated phosphoric acid","correct":false,"explanation":"Concentrated phosphoric acid acts as a dehydration catalyst rather than the required oxidising agent. The correct reagent is acidified potassium dichromate(VI), which oxidises ethanol to ethanoic acid."},{"text":"aqueous sodium hydroxide","correct":false,"explanation":"Aqueous sodium hydroxide is an alkali and does not provide the oxygen needed for this reaction. Acidified potassium dichromate(VI) is the required oxidising agent."},{"text":"acidified potassium iodide","correct":false,"explanation":"Acidified potassium iodide is commonly used as a reducing agent test reagent, not to oxidise ethanol. Acidified potassium dichromate(VI) supplies the oxygen for oxidation."}]},{"id":"488822d0-d991-43df-89d4-2579e34f0ccf","cardType":"cloze","points":null,"front":"Heating ethanol with acidified potassium dichromate(VI) produces [ ] and water.","back":"Heating ethanol with acidified potassium dichromate(VI) produces ethanoic acid and water.","mcqOptions":[{"text":"ethanoic acid","correct":true,"explanation":"Heating ethanol with acidified potassium dichromate(VI) causes complete oxidation of the primary alcohol, producing ethanoic acid and water."},{"text":"ethanal","correct":false,"explanation":"Ethanal is the intermediate produced by controlled oxidation and immediate distillation. Heating ethanol for complete oxidation with acidified potassium dichromate(VI) produces ethanoic acid."},{"text":"methanoic acid","correct":false,"explanation":"Methanoic acid contains one carbon atom, so it cannot be formed by simply oxidising two-carbon ethanol. The complete oxidation product is ethanoic acid."},{"text":"propanoic acid","correct":false,"explanation":"Propanoic acid contains three carbon atoms, but oxidation does not add carbon atoms to ethanol. Two-carbon ethanol is oxidised to ethanoic acid."}]},{"id":"1781ae4d-1850-45a0-95dd-82d829a1edd9","cardType":"basic","points":1,"front":"What does the symbol [O] represent in simplified oxidation equations?","back":"Oxygen provided by an oxidising agent.","mcqOptions":[{"text":"Oxygen provided by an oxidising agent.","correct":true,"explanation":"In simplified organic equations, [O] denotes oxygen supplied by an oxidising agent. It represents oxidation without requiring the oxidising reagent’s full formula in the equation."},{"text":"Oxygen provided by a reducing agent.","correct":false,"explanation":"A reducing agent removes oxygen or supplies hydrogen rather than providing oxygen for oxidation. [O] represents oxygen supplied by an oxidising agent."},{"text":"Hydrogen provided by a reducing agent.","correct":false,"explanation":"The symbol [O] represents oxygen involved in oxidation, not hydrogen involved in reduction. This oxygen is supplied by an oxidising agent."},{"text":"Oxygen gas released by a catalyst.","correct":false,"explanation":"The brackets indicate oxygen available from an oxidising agent, not oxygen gas released by a catalyst. Catalysts speed reactions without supplying this oxygen."}]},{"id":"89e50605-d7ec-4fd2-b597-b0cbf10b36c1","cardType":"basic","points":2,"front":"State the reagents and catalyst used to manufacture ethanol from ethene.","back":"

Reagents: Ethene and steam
Catalyst: Phosphoric acid ($H_3PO_4$)

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

Reagents: Ethene and steam
Catalyst: Phosphoric acid ($H_3PO_4$)

","correct":true,"explanation":"Industrial hydration reacts ethene with steam over a phosphoric acid catalyst. The catalyst increases reaction rate without being consumed in the process."},{"text":"

Reagents: Ethene and steam
Catalyst: Sulfuric acid ($H_2SO_4$)

","correct":false,"explanation":"Ethene and steam are the correct reagents, but sulfuric acid is not the industrial hydration catalyst. Phosphoric acid, $H_3PO_4$, is used instead."},{"text":"

Reagents: Ethene and hydrogen
Catalyst: Nickel ($Ni$)

","correct":false,"explanation":"Ethene and hydrogen undergo hydrogenation rather than hydration, typically producing ethane. Ethanol manufacture uses ethene and steam with phosphoric acid as the catalyst."},{"text":"

Reagents: Glucose and water
Catalyst: Phosphoric acid ($H_3PO_4$)

","correct":false,"explanation":"Glucose and water are not the reactants for hydrating ethene. The industrial process reacts ethene with steam using phosphoric acid as its catalyst."}]},{"id":"eafa5500-f6fe-46c6-84f1-88c6bd2b886d","cardType":"cloze","points":null,"front":"The hydration of ethene requires a temperature of [ ] and a pressure of 60-70 atm.","back":"The hydration of ethene requires a temperature of 300 °C and a pressure of 60-70 atm.","mcqOptions":[{"text":"300 °C","correct":true,"explanation":"Industrial hydration of ethene is carried out at about 300 °C, providing a compromise between a sufficiently fast reaction and a favourable equilibrium yield."},{"text":"30 °C","correct":false,"explanation":"Confusing 300 °C with 30 °C makes the temperature ten times too small, leaving the reaction impractically slow. Industrial hydration uses approximately 300 °C."},{"text":"150 °C","correct":false,"explanation":"A temperature of 150 °C is below the specified industrial condition and gives a slower reaction rate. Ethene hydration is carried out at about 300 °C."},{"text":"450 °C","correct":false,"explanation":"Using 450 °C favours the reverse, endothermic direction more strongly and lowers the equilibrium ethanol yield. The standard compromise temperature is about 300 °C."}]},{"id":"e9c1a26a-aef3-40c7-926d-1bab02803142","cardType":"cloze","points":null,"front":"The hydration of ethene requires a temperature of 300 °C and a pressure of [ ].","back":"The hydration of ethene requires a temperature of 300 °C and a pressure of 60-70 atm.","mcqOptions":[{"text":"60-70 atm","correct":true,"explanation":"A pressure of 60-70 atm shifts the equilibrium towards ethanol because fewer gas molecules are present on the product side, while limiting compression costs."},{"text":"6-7 atm","correct":false,"explanation":"Dropping a zero gives a pressure far below the industrial condition, reducing both collision frequency and equilibrium yield. The process uses 60-70 atm."},{"text":"600-700 atm","correct":false,"explanation":"Adding an extra zero gives an unnecessarily high pressure with excessive equipment and compression costs. Industrial hydration uses the compromise pressure of 60-70 atm."},{"text":"1 atm","correct":false,"explanation":"Atmospheric pressure would give a low reaction rate and poor equilibrium yield because hydration is favoured by higher pressure. The specified range is 60-70 atm."}]},{"id":"4ec5f06c-f2c0-4697-b63b-301318e4a2ad","cardType":"basic","points":2,"front":"State the balanced chemical equation for the fermentation of glucose.","back":"$$C_6H_{12}O_6 \\rightarrow 2C_2H_5OH + 2CO_2$","mcqOptions":[{"text":"$$C_6H_{12}O_6 \\rightarrow 2C_2H_5OH + 2CO_2$","correct":true,"explanation":"One glucose molecule forms two ethanol molecules and two carbon dioxide molecules. These coefficients balance all six carbon, twelve hydrogen and six oxygen atoms."},{"text":"$$C_6H_{12}O_6 \\rightarrow C_2H_5OH + 2CO_2$","correct":false,"explanation":"Omitting the coefficient 2 before ethanol leaves carbon and hydrogen unbalanced. Fermentation forms two ethanol molecules and two carbon dioxide molecules per glucose molecule."},{"text":"$$C_6H_{12}O_6 + 6O_2 \\rightarrow 6CO_2 + 6H_2O$","correct":false,"explanation":"This is the equation for complete aerobic respiration because oxygen is consumed and only carbon dioxide and water form. Fermentation produces ethanol and carbon dioxide without oxygen."},{"text":"$$C_6H_{12}O_6 \\rightarrow 2C_2H_5OH + CO_2$","correct":false,"explanation":"Using only one carbon dioxide molecule leaves the carbon and oxygen atoms unbalanced. The balanced equation requires two ethanol and two carbon dioxide molecules."}]},{"id":"078015b6-4e53-4eed-8b1b-2c545d825be0","cardType":"basic","points":2,"front":"Why does fermentation require an absence of air?","back":"

To prevent aerobic respiration (which makes $CO_2$ and $H_2O$)
To prevent oxidation of ethanol into ethanoic acid

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

To prevent aerobic respiration (which makes $CO_2$ and $H_2O$)
To prevent oxidation of ethanol into ethanoic acid

","correct":true,"explanation":"Without air, yeast carries out anaerobic fermentation instead of aerobic respiration. Excluding oxygen also prevents the ethanol product from being oxidised further into ethanoic acid."},{"text":"

To prevent anaerobic respiration (which makes ethanol and $CO_2$)
To prevent glucose forming ethanol

","correct":false,"explanation":"Fermentation depends on anaerobic respiration, so preventing it would stop ethanol production. Air is excluded to prevent aerobic respiration and oxidation of ethanol to ethanoic acid."},{"text":"

To encourage aerobic respiration (which makes $CO_2$ and $H_2O$)
To oxidise ethanol into ethanoic acid

","correct":false,"explanation":"Air would encourage aerobic respiration rather than fermentation, and oxidising ethanol is undesirable. Oxygen is excluded to preserve ethanol and prevent respiration producing carbon dioxide and water."},{"text":"

To prevent yeast consuming glucose (which makes ethanol and $CO_2$)
To prevent the escape of carbon dioxide

","correct":false,"explanation":"Yeast must consume glucose for fermentation, and carbon dioxide escape does not explain excluding air. The absence of oxygen prevents aerobic respiration and ethanol oxidation."}]},{"id":"b4024153-9491-4557-93e8-5bc7bdf4e35e","cardType":"cloze","points":null,"front":"Fermentation uses [ ] at an optimum temperature of 30 °C.","back":"Fermentation uses yeast at an optimum temperature of 30 °C.","mcqOptions":[{"text":"yeast","correct":true,"explanation":"Yeast contains enzymes that catalyse the anaerobic conversion of glucose into ethanol and carbon dioxide, with activity typically highest around 30 °C."},{"text":"nickel","correct":false,"explanation":"Nickel catalyses reactions such as alkene hydrogenation, not fermentation. Alcoholic fermentation uses yeast, whose enzymes convert glucose into ethanol and carbon dioxide."},{"text":"phosphoric acid","correct":false,"explanation":"Phosphoric acid is the catalyst used for the industrial hydration of ethene. Fermentation instead uses yeast as the source of biological enzymes."},{"text":"oxygen","correct":false,"explanation":"Oxygen is not the biological agent used in fermentation, which is an anaerobic process. Yeast supplies the enzymes that break down glucose."}]},{"id":"5d4b5356-c5d5-4175-975f-983a870ab9b2","cardType":"cloze","points":null,"front":"Fermentation uses yeast at an optimum temperature of [ ].","back":"Fermentation uses yeast at an optimum temperature of 30 °C.","mcqOptions":[{"text":"30 °C","correct":true,"explanation":"Around 30 °C, yeast enzymes work efficiently without being denatured, so this is the optimum temperature normally stated for fermentation."},{"text":"20 °C","correct":false,"explanation":"At 20 °C, yeast enzymes work more slowly because particles have less kinetic energy. The typical optimum temperature for fermentation is 30 °C."},{"text":"40 °C","correct":false,"explanation":"At 40 °C, yeast enzymes may begin to denature, reducing fermentation rather than providing the optimum conditions. The stated optimum is 30 °C."},{"text":"60 °C","correct":false,"explanation":"At 60 °C, yeast enzymes are rapidly denatured and the yeast may be killed. Fermentation is normally carried out at about 30 °C."}]},{"id":"d8c40b98-7505-4944-be41-162110c59be0","cardType":"basic","points":2,"front":"Why does the rate of fermentation decrease if the temperature is significantly higher than 30 °C?","back":"The yeast enzymes denature (the active site changes shape).","mcqOptions":[{"text":"The yeast enzymes denature (the active site changes shape).","correct":true,"explanation":"High temperatures disrupt the bonds maintaining an enzyme’s shape. Its active site changes, so glucose no longer binds effectively and fermentation slows."},{"text":"The yeast enzymes are used up (no catalyst remains for the reaction).","correct":false,"explanation":"Enzymes are catalysts, so they are not consumed during fermentation. The rate falls because excessive heat denatures yeast enzymes and changes their active sites."},{"text":"The yeast enzymes evaporate (the catalyst leaves the mixture).","correct":false,"explanation":"Enzymes do not evaporate from the mixture at these temperatures. Excessive heat denatures them, altering their active sites so they cannot catalyse fermentation effectively."},{"text":"The glucose molecules denature (their active sites change shape).","correct":false,"explanation":"Glucose is a substrate and has no active site to denature. The yeast enzymes denature at excessive temperatures, changing the shape of their active sites."}]},{"id":"54b5fc2b-c754-4d02-be9f-b987da1e4f64","cardType":"cloze","points":null,"front":"In the naming of butan-1-ol, the \"1\" indicates that the [ ] is attached to the first carbon in the chain.","back":"In the naming of butan-1-ol, the \"1\" indicates that the -OH group is attached to the first carbon in the chain.","mcqOptions":[{"text":"-OH group","correct":true,"explanation":"The suffix -ol identifies an alcohol, and its locant gives the hydroxyl group’s position. In butan-1-ol, the -OH group is on carbon 1."},{"text":"-COOH group","correct":false,"explanation":"A -COOH group identifies a carboxylic acid and would require the suffix -oic acid. In butan-1-ol, the locant specifies the -OH group."},{"text":"C=C bond","correct":false,"explanation":"A C=C bond is identified by the suffix -ene, not -ol. The number in butan-1-ol gives the position of the -OH group."},{"text":"-CHO group","correct":false,"explanation":"A -CHO group identifies an aldehyde and normally gives the suffix -al. The functional group located by the 1 in butan-1-ol is -OH."}]},{"id":"97f43b8f-b941-4944-bbe7-e5910ebc0a4c","cardType":"cloze","points":null,"front":"In the naming of butan-1-ol, the \"1\" indicates that the -OH group is attached to the [ ] in the chain.","back":"In the naming of butan-1-ol, the \"1\" indicates that the -OH group is attached to the first carbon in the chain.","mcqOptions":[{"text":"first carbon","correct":true,"explanation":"The carbon chain is numbered from the end nearest the -OH group. A locant of 1 therefore places that group on the first carbon."},{"text":"second carbon","correct":false,"explanation":"An -OH group on carbon 2 would produce butan-2-ol, not butan-1-ol. The locant 1 places it on the first carbon."},{"text":"third carbon","correct":false,"explanation":"Numbering must begin from the end nearest the -OH group, so a position described as carbon 3 would be renumbered carbon 2. Butan-1-ol has it on carbon 1."},{"text":"both end carbons","correct":false,"explanation":"Butan-1-ol contains one hydroxyl group attached to one terminal carbon, not both ends of the chain. The locant identifies the first carbon."}]},{"id":"7b1f3a17-00c7-4947-957b-a1a902cd9cab","cardType":"basic","points":1,"front":"Why is the fermentation of glucose considered a biological process?","back":"It is catalysed by enzymes found in yeast.","mcqOptions":[{"text":"It is catalysed by enzymes found in yeast.","correct":true,"explanation":"Yeast is a living microorganism containing enzymes that catalyse glucose fermentation. Using these biologically produced catalysts makes fermentation a biological process."},{"text":"It is catalysed by phosphoric acid at 300 °C.","correct":false,"explanation":"Phosphoric acid and high temperature are associated with industrial ethene hydration, a chemical process. Fermentation is biological because yeast supplies the necessary enzymes."},{"text":"It is driven by oxygen found in air.","correct":false,"explanation":"Fermentation is anaerobic, so oxygen is not what makes it biological. Its biological character comes from enzymes produced by living yeast cells."},{"text":"It is catalysed by ethanol dissolved in water.","correct":false,"explanation":"Ethanol is a product of fermentation rather than its catalyst. The reaction is biological because enzymes in yeast catalyse the breakdown of glucose."}]},{"id":"03af235b-88e0-47e2-bc86-092a49f65848","cardType":"basic","points":3,"front":"What are the typical conditions for the hydration of ethene?","back":"

300 °C
60-70 atm pressure
Phosphoric acid catalyst

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

300 °C
60-70 atm pressure
Phosphoric acid catalyst

","correct":true,"explanation":"Industrial hydration reacts ethene with steam at about 300 °C and 60-70 atm, using phosphoric acid to catalyse the reversible reaction."},{"text":"

30 °C
1 atm pressure
Yeast catalyst

","correct":false,"explanation":"These resemble fermentation conditions, which use yeast at about 30 °C and low pressure. Ethene hydration requires 300 °C, 60-70 atm and phosphoric acid."},{"text":"

300 °C
1 atm pressure
Nickel catalyst

","correct":false,"explanation":"Nickel is used to hydrogenate alkenes, while low pressure is not typical for industrial ethene hydration. Hydration uses 300 °C, 60-70 atm and phosphoric acid."},{"text":"

450 °C
200 atm pressure
Iron catalyst

","correct":false,"explanation":"These are associated with the Haber process rather than ethene hydration. Hydration is carried out at 300 °C and 60-70 atm with phosphoric acid."}]},{"id":"90d2a05f-4c33-428f-ba75-504f14c12af7","cardType":"cloze","points":null,"front":"Wine turning into vinegar when left open is an example of [ ].","back":"Wine turning into vinegar when left open is an example of microbial oxidation.","mcqOptions":[{"text":"microbial oxidation","correct":true,"explanation":"When wine is exposed to air, microorganisms use oxygen to oxidise its ethanol into ethanoic acid, the acid responsible for vinegar’s properties."},{"text":"anaerobic fermentation","correct":false,"explanation":"Anaerobic fermentation converts sugars into ethanol without oxygen; it does not turn ethanol into vinegar. Exposed wine undergoes microbial oxidation to form ethanoic acid."},{"text":"catalytic hydration","correct":false,"explanation":"Catalytic hydration is the industrial reaction of ethene with steam to make ethanol. Wine becomes vinegar through microbial oxidation of ethanol to ethanoic acid."},{"text":"thermal decomposition","correct":false,"explanation":"The change does not result from heating a substance until it breaks down. Microorganisms instead oxidise ethanol using oxygen from the air, producing ethanoic acid."}]}]}],"examCountdown":{"examDate":"2027-05-19","paperLabel":"Paper 1"},"heading":"Alcohols","title":"Alcohols Flashcards","topbar":{"backHref":"/igcse/chemistry/edexcel/flashcards"},"topicSidebar":"$L36"}]}],"topicId":"d5d6d4a2-692a-5721-9f83-2c07d0472001","walled":"$L37"}],"$L38","$L39"]