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24:[["$","$L33",null,{"feature":"flashcards"}],"$L34",["$","$L35",null,{"href":"/igcse/chemistry/cie/alkanes/flashcards","label":"Alkanes","subjectCode":"igcse_chemistry__cie","surface":"flashcards"}],["$","$L36",null,{"runner":["$","div",null,{"className":"min-h-0 flex-1 overflow-hidden bg-background","children":["$","$L37",null,{"decks":[{"id":"b9e17fd5-10ff-4024-96a5-75803ee75de2","title":"Alkanes Flashcards","topicId":"4fd65917-f500-5602-a287-715cae3a9f55","topicSlug":"alkanes","cards":[{"id":"73d7997d-8ff7-4dec-bd1e-b0201434f319","cardType":"basic","points":1,"front":"What two elements are the only components of a hydrocarbon?","back":"

Carbon
Hydrogen

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

Carbon
Hydrogen

","correct":true,"explanation":"Hydrocarbons contain carbon atoms bonded to hydrogen atoms and no other elements. Their name combines “hydro”, referring to hydrogen, with “carbon”."},{"text":"

Carbon
Oxygen

","correct":false,"explanation":"Including oxygen would make the substance an oxygen-containing organic compound rather than a hydrocarbon. A hydrocarbon consists solely of carbon and hydrogen."},{"text":"

Carbon
Nitrogen

","correct":false,"explanation":"Nitrogen is present in compounds such as amines, not in hydrocarbons. The only elements permitted in a hydrocarbon are carbon and hydrogen."},{"text":"

Hydrogen
Oxygen

","correct":false,"explanation":"Hydrogen and oxygen together form compounds such as water, but a hydrocarbon must contain carbon. Its only two elements are carbon and hydrogen."}]},{"id":"e6c0619c-02e7-4db0-91af-e353b26b723a","cardType":"cloze","points":null,"front":"Alkanes are described as [ ] because they contain only single carbon-carbon bonds.","back":"Alkanes are described as saturated because they contain only single carbon-carbon bonds.","mcqOptions":[{"text":"saturated","correct":true,"explanation":"Alkanes are saturated because every carbon-carbon bond is single. Each carbon therefore holds the maximum possible number of hydrogen atoms for an open-chain hydrocarbon."},{"text":"unsaturated","correct":false,"explanation":"Unsaturated hydrocarbons contain at least one carbon-carbon double or triple bond. Alkanes contain only single carbon-carbon bonds, so they are described as saturated."},{"text":"aromatic","correct":false,"explanation":"Aromatic compounds contain a stable ring system with delocalised electrons, such as benzene. Alkanes have only single carbon-carbon bonds and are therefore saturated."},{"text":"polyunsaturated","correct":false,"explanation":"Polyunsaturated substances contain multiple carbon-carbon double bonds. Alkanes have no double or triple bonds, so the correct description is saturated."}]},{"id":"a219edd9-0882-45a9-bc70-db4d0207325d","cardType":"cloze","points":null,"front":"Alkanes are described as saturated because they contain only [ ] carbon-carbon bonds.","back":"Alkanes are described as saturated because they contain only single carbon-carbon bonds.","mcqOptions":[{"text":"single","correct":true,"explanation":"Saturated hydrocarbons contain only single bonds between their carbon atoms. A double or triple carbon-carbon bond would make the compound unsaturated."},{"text":"double","correct":false,"explanation":"A carbon-carbon double bond indicates an unsaturated hydrocarbon, such as an alkene. Alkanes are saturated because all their carbon-carbon bonds are single."},{"text":"triple","correct":false,"explanation":"A carbon-carbon triple bond is characteristic of an alkyne and makes it unsaturated. Alkanes instead contain only single carbon-carbon bonds."},{"text":"alternating","correct":false,"explanation":"Alternating bond types may be associated with representations of some unsaturated systems, not alkanes. Every carbon-carbon bond in an alkane is single."}]},{"id":"0be3898c-213a-4a73-9e7c-c099b56c0570","cardType":"basic","points":1,"front":"What is the general formula for alkanes?","back":"$$C_nH_{2n+2}$","mcqOptions":[{"text":"$$C_nH_{2n+2}$","correct":true,"explanation":"An open-chain alkane with $n$ carbon atoms has $2n+2$ hydrogen atoms because every carbon forms four covalent bonds and all carbon-carbon bonds are single."},{"text":"$$C_nH_{2n}$","correct":false,"explanation":"The formula $C_nH_{2n}$ applies to open-chain alkenes and cycloalkanes. Saturated open-chain alkanes have two additional hydrogen atoms, giving $C_nH_{2n+2}$."},{"text":"$$C_nH_{2n-2}$","correct":false,"explanation":"The formula $C_nH_{2n-2}$ represents hydrocarbons with two degrees of unsaturation, such as an alkyne. An alkane’s general formula is $C_nH_{2n+2}$."},{"text":"$$C_nH_{2n+1}$","correct":false,"explanation":"The formula $C_nH_{2n+1}$ describes an alkyl group formed by removing one hydrogen from an alkane. A complete alkane has formula $C_nH_{2n+2}$."}]},{"id":"520ce80c-e056-4b12-aecf-73b5c7369e6e","cardType":"basic","points":1,"front":"State the names of the first four alkanes.","back":"

Methane
Ethane
Propane
Butane

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

Methane
Ethane
Propane
Butane

","correct":true,"explanation":"The alkane names follow increasing carbon-chain length: methane has one carbon, ethane two, propane three and butane four."},{"text":"

Methane
Ethane
Propane
Pentane

","correct":false,"explanation":"Pentane has five carbon atoms, so it is the fifth alkane rather than the fourth. The first four end with butane."},{"text":"

Ethane
Propane
Butane
Pentane

","correct":false,"explanation":"This sequence omits methane, the one-carbon alkane, and therefore shifts every position. The first four are methane, ethane, propane and butane."},{"text":"

Methane
Ethene
Propene
Butene

","correct":false,"explanation":"The “-ene” endings identify alkenes containing carbon-carbon double bonds. The first four alkanes are methane, ethane, propane and butane."}]},{"id":"ca5713eb-ebaf-41f6-8329-a0426c01ddf6","cardType":"cloze","points":null,"front":"A [ ] formula shows the number of atoms (e.g. $C_2H_6$), whereas a displayed formula shows every atom and bond.","back":"A molecular formula shows the number of atoms (e.g. $C_2H_6$), whereas a displayed formula shows every atom and bond.","mcqOptions":[{"text":"molecular","correct":true,"explanation":"A molecular formula gives the actual number of atoms of each element in one molecule. For example, ethane’s molecular formula is $C_2H_6$."},{"text":"empirical","correct":false,"explanation":"An empirical formula gives the simplest whole-number ratio of atoms, so ethane would be $CH_3$ rather than $C_2H_6$. The required term is molecular."},{"text":"structural","correct":false,"explanation":"A structural formula indicates how atoms or groups are connected, rather than merely giving their numbers. A formula such as $C_2H_6$ is molecular."},{"text":"skeletal","correct":false,"explanation":"A skeletal formula represents the carbon framework while omitting carbon labels and most attached hydrogens. The formula recording actual atom numbers is molecular."}]},{"id":"447ee4f5-fe59-4cd3-951f-8012c243f333","cardType":"cloze","points":null,"front":"A molecular formula shows the number of atoms (e.g. $C_2H_6$), whereas a [ ] formula shows every atom and bond.","back":"A molecular formula shows the number of atoms (e.g. $C_2H_6$), whereas a displayed formula shows every atom and bond.","mcqOptions":[{"text":"displayed","correct":true,"explanation":"A displayed formula draws every atom and every covalent bond explicitly. This provides more structural detail than a molecular formula such as $C_2H_6$."},{"text":"structural","correct":false,"explanation":"A structural formula may use condensed groups and does not necessarily draw every individual bond. The specific formula showing every atom and bond is displayed."},{"text":"molecular","correct":false,"explanation":"A molecular formula records only how many atoms of each element are present, such as $C_2H_6$. A displayed formula shows every atom and bond."},{"text":"empirical","correct":false,"explanation":"An empirical formula shows the simplest ratio of elements and provides no complete bonding diagram. A displayed formula is the one that shows every atom and bond."}]},{"id":"46ea8332-9a94-49e0-9a7a-05aad503f471","cardType":"basic","points":1,"front":"How many covalent bonds does a carbon atom always form in an alkane?","back":"Four","mcqOptions":[{"text":"Four","correct":true,"explanation":"Carbon is tetravalent, meaning it forms four covalent bonds. In an alkane, these bonds connect carbon to hydrogen atoms or other carbon atoms."},{"text":"Two","correct":false,"explanation":"Two bonds would leave a carbon atom below its normal valency in an alkane. Carbon is tetravalent and therefore always forms four covalent bonds."},{"text":"Three","correct":false,"explanation":"Three bonds are typical of neutral nitrogen, not carbon in an alkane. Each alkane carbon completes its outer shell by forming four covalent bonds."},{"text":"Six","correct":false,"explanation":"Six bonds would exceed carbon’s valency and its outer-shell capacity. Carbon atoms in alkanes are tetravalent, so each forms exactly four covalent bonds."}]},{"id":"cba0c69a-cbca-465b-a4b2-163d3df0536a","cardType":"basic","points":2,"front":"Why are alkanes generally unreactive?","back":"

C-C and C-H bonds are strong
They have no reactive functional group

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

C-C and C-H bonds are strong
They have no reactive functional group

","correct":true,"explanation":"Strong C-C and C-H bonds require considerable energy to break, while the absence of a reactive functional group gives alkanes few sites where reactions can begin."},{"text":"

C-C and C-H bonds are weak
They contain a reactive hydroxyl group

","correct":false,"explanation":"Weak bonds and a hydroxyl group would make a substance more reactive. Alkanes are unreactive because their C-C and C-H bonds are strong and they lack a functional group."},{"text":"

C-C and C-H bonds are ionic
They contain a reactive carbonyl group

","correct":false,"explanation":"Alkane bonds are covalent, not ionic, and alkanes contain no carbonyl group. Their low reactivity results from strong C-C and C-H bonds and no reactive functional group."},{"text":"

C-C and C-H bonds are easily broken
They contain a reactive double bond

","correct":false,"explanation":"Easily broken bonds and a C=C double bond would produce greater reactivity, as in alkenes. Alkanes instead have strong single bonds and no reactive functional group."}]},{"id":"ba28fe9f-fe95-4fde-8496-cba319810ef9","cardType":"basic","points":1,"front":"Name the two products of the complete combustion of an alkane.","back":"

Carbon dioxide ($CO_2$)
Water ($H_2O$)

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

Carbon dioxide ($CO_2$)
Water ($H_2O$)

","correct":true,"explanation":"With excess oxygen, all carbon atoms in an alkane are fully oxidised to carbon dioxide and all hydrogen atoms are oxidised to water."},{"text":"

Carbon monoxide ($CO$)
Water ($H_2O$)

","correct":false,"explanation":"Carbon monoxide forms when the oxygen supply is insufficient, so this describes incomplete combustion. Complete combustion produces carbon dioxide and water."},{"text":"

Carbon ($C$)
Water ($H_2O$)

","correct":false,"explanation":"Solid carbon, observed as soot, can form during incomplete combustion with very limited oxygen. Complete combustion oxidises the carbon fully, producing carbon dioxide and water."},{"text":"

Carbon dioxide ($CO_2$)
Hydrogen ($H_2$)

","correct":false,"explanation":"Hydrogen is not released as an element during combustion; it is oxidised by oxygen. The two products of complete alkane combustion are carbon dioxide and water."}]},{"id":"489f4ac5-b1d9-4b23-8efc-c21e61a01544","cardType":"cloze","points":null,"front":"Combustion is an [ ] reaction because it releases energy to the surroundings.","back":"Combustion is an exothermic reaction because it releases energy to the surroundings.","mcqOptions":[{"text":"exothermic","correct":true,"explanation":"An exothermic reaction transfers energy from the reacting chemicals to the surroundings, commonly causing the surroundings to become warmer."},{"text":"endothermic","correct":false,"explanation":"Endothermic reactions absorb energy from the surroundings rather than releasing it. Because combustion transfers energy to the surroundings, it is classified as exothermic."},{"text":"isothermal","correct":false,"explanation":"Isothermal describes a process occurring at constant temperature, not one classified by energy release. Combustion releases energy to the surroundings, so it is exothermic."},{"text":"non-energetic","correct":false,"explanation":"Combustion clearly involves an energy transfer, often producing heat and light. A reaction that releases energy to the surroundings is described as exothermic."}]},{"id":"ca598686-a355-49fd-801d-4b64e26dbde4","cardType":"cloze","points":null,"front":"Combustion is an exothermic reaction because it [ ] energy to the surroundings.","back":"Combustion is an exothermic reaction because it releases energy to the surroundings.","mcqOptions":[{"text":"releases","correct":true,"explanation":"Combustion transfers chemical energy from the fuel to the surroundings, usually as heat and light, so it releases energy and is exothermic."},{"text":"absorbs","correct":false,"explanation":"Absorbing energy from the surroundings defines an endothermic reaction. Combustion is exothermic because it releases energy to the surroundings instead."},{"text":"stores","correct":false,"explanation":"Combustion converts stored chemical energy and transfers it to the surroundings; it does not store additional energy. It is exothermic because it releases energy."},{"text":"destroys","correct":false,"explanation":"Energy is conserved and cannot be destroyed during a chemical reaction. Combustion releases stored chemical energy by transferring it to the surroundings."}]},{"id":"732cc0ba-04ea-4438-af02-54a4d022926e","cardType":"basic","points":1,"front":"What toxic gas is produced during the incomplete combustion of alkanes?","back":"Carbon monoxide ($CO$)","mcqOptions":[{"text":"Carbon monoxide ($CO$)","correct":true,"explanation":"Insufficient oxygen can prevent carbon from being fully oxidised to carbon dioxide, producing carbon monoxide instead. Carbon monoxide is toxic because it reduces the blood’s oxygen-carrying capacity."},{"text":"Sulfur dioxide ($SO_2$)","correct":false,"explanation":"Sulfur dioxide forms when sulfur-containing substances burn, but alkanes contain only carbon and hydrogen. Incomplete alkane combustion can produce toxic carbon monoxide."},{"text":"Nitrogen monoxide ($NO$)","correct":false,"explanation":"Nitrogen monoxide may form from atmospheric nitrogen at very high temperatures, but it is not the characteristic toxic product of incomplete alkane combustion. That product is carbon monoxide."},{"text":"Chlorine ($Cl_2$)","correct":false,"explanation":"Chlorine cannot be a combustion product of an alkane because neither the alkane nor oxygen supplies chlorine atoms. The toxic gas formed by incomplete combustion is carbon monoxide."}]},{"id":"358f8e9b-29f5-4de5-9c20-485849fd1acb","cardType":"basic","points":1,"front":"What type of reaction occurs when an alkane reacts with chlorine?","back":"Substitution","mcqOptions":[{"text":"Substitution","correct":true,"explanation":"In ultraviolet light, a chlorine atom replaces a hydrogen atom in the alkane. Replacing one atom with another makes this a substitution reaction."},{"text":"Addition","correct":false,"explanation":"Addition reactions occur across multiple bonds, such as the C=C bond in an alkene. Alkanes have only single bonds and react with chlorine by substitution."},{"text":"Neutralisation","correct":false,"explanation":"Neutralisation is the reaction of an acid with a base, usually forming salt and water. Chlorination of an alkane instead involves substitution of hydrogen by chlorine."},{"text":"Polymerisation","correct":false,"explanation":"Polymerisation joins many small molecules into a long-chain molecule and commonly involves alkenes. An alkane reacting with chlorine undergoes substitution, not polymerisation."}]},{"id":"dcb73e3f-9df1-4968-bfa5-8b7c1a7d95ca","cardType":"cloze","points":null,"front":"In a substitution reaction, one [ ] atom in the alkane is replaced by one chlorine atom.","back":"In a substitution reaction, one hydrogen atom in the alkane is replaced by one chlorine atom.","mcqOptions":[{"text":"hydrogen","correct":true,"explanation":"During chlorination, a C-H bond is broken and one hydrogen atom is replaced by chlorine, producing a chloroalkane and hydrogen chloride."},{"text":"carbon","correct":false,"explanation":"The carbon skeleton of the alkane remains intact during substitution; a carbon atom is not removed. Chlorine replaces one hydrogen atom attached to carbon."},{"text":"oxygen","correct":false,"explanation":"Alkanes contain only carbon and hydrogen, so there is no oxygen atom available for replacement. In chlorination, one hydrogen atom is replaced by chlorine."},{"text":"nitrogen","correct":false,"explanation":"Nitrogen is not present in an alkane, which contains only carbon and hydrogen. A substitution reaction with chlorine replaces one of the alkane’s hydrogen atoms."}]},{"id":"675f8280-66a5-4ee0-880e-39dbca267fbf","cardType":"cloze","points":null,"front":"In a substitution reaction, one hydrogen atom in the alkane is replaced by one [ ] atom.","back":"In a substitution reaction, one hydrogen atom in the alkane is replaced by one chlorine atom.","mcqOptions":[{"text":"chlorine","correct":true,"explanation":"In the substitution reaction between an alkane and chlorine, a chlorine atom takes the place of one hydrogen atom, forming a chloroalkane."},{"text":"oxygen","correct":false,"explanation":"Replacing hydrogen with oxygen does not describe the chlorination of an alkane. In this substitution reaction, the incoming atom is chlorine."},{"text":"carbon","correct":false,"explanation":"Carbon atoms form the alkane’s existing chain and are not substituted for hydrogen in chlorination. One hydrogen atom is replaced by a chlorine atom."},{"text":"nitrogen","correct":false,"explanation":"Nitrogen does not enter the alkane during its reaction with chlorine. The substitution specifically replaces one hydrogen atom with one chlorine atom."}]},{"id":"3e74b697-438b-4ddf-b971-e3433748d1a9","cardType":"basic","points":1,"front":"What specific condition is required for the chlorination of alkanes?","back":"Ultraviolet (UV) light","mcqOptions":[{"text":"Ultraviolet (UV) light","correct":true,"explanation":"Ultraviolet light supplies the energy needed to break the chlorine molecule into reactive radicals, initiating the substitution reaction with an alkane."},{"text":"Heat","correct":false,"explanation":"Heating is not the specific condition required for alkane chlorination at this level. The reaction is initiated by ultraviolet (UV) light, which starts radical formation."},{"text":"High pressure","correct":false,"explanation":"Pressure does not initiate the substitution of an alkane by chlorine. The required condition is ultraviolet (UV) light, which provides energy for the reaction to start."},{"text":"A nickel catalyst","correct":false,"explanation":"Nickel catalyses hydrogenation reactions rather than initiating chlorination of alkanes. Alkane chlorination requires ultraviolet (UV) light to begin the radical substitution process."}]},{"id":"e226a0f3-73cb-428c-a045-8a89d5f23441","cardType":"basic","points":1,"front":"Why is the reaction between alkanes and chlorine described as photochemical?","back":"The reaction is started by light (specifically UV light).","mcqOptions":[{"text":"The reaction is started by light (specifically UV light).","correct":true,"explanation":"The reaction is photochemical because ultraviolet light provides the energy needed to split chlorine molecules into reactive radicals, starting the substitution mechanism."},{"text":"The reaction is stopped by light (specifically UV light).","correct":false,"explanation":"Ultraviolet light does not stop chlorination; it initiates it by supplying energy to form reactive chlorine radicals. This light-started behaviour is why the reaction is photochemical."},{"text":"The reaction is started by heat (specifically boiling).","correct":false,"explanation":"Boiling is not the stated trigger for alkane chlorination. It is ultraviolet light that starts the reaction by supplying energy to break chlorine molecules into radicals."},{"text":"The reaction is started by a catalyst (specifically nickel).","correct":false,"explanation":"A nickel catalyst is associated with hydrogenation, not chlorination of alkanes. The chlorination reaction is started by ultraviolet light, giving it its photochemical description."}]},{"id":"6e9a524f-975a-4dd2-b99b-e8468581fc17","cardType":"cloze","points":null,"front":"In chlorination, ultraviolet light provides the [ ] ($E_a$) needed to start the reaction.","back":"In chlorination, ultraviolet light provides the activation energy ($E_a$) needed to start the reaction.","mcqOptions":[{"text":"activation energy","correct":true,"explanation":"Activation energy is the minimum energy needed for reacting particles to overcome the energy barrier. Ultraviolet light supplies this energy at the start of chlorination."},{"text":"bond energy","correct":false,"explanation":"Bond energy is the energy needed to break a particular chemical bond, not the general energy barrier for a reaction. The missing term is activation energy."},{"text":"kinetic energy","correct":false,"explanation":"Kinetic energy is energy associated with movement, although particles may use it during collisions. The specific minimum energy needed to start reaction is activation energy."},{"text":"thermal energy","correct":false,"explanation":"Thermal energy is energy transferred because of temperature and is not the named reaction threshold here. Ultraviolet light provides the activation energy needed to begin chlorination."}]},{"id":"d96e4942-b790-4f7a-900e-a4cd85e39588","cardType":"basic","points":2,"front":"Identify the two products formed when methane reacts with chlorine in UV light.","back":"

Chloromethane ($CH_3Cl$)
Hydrogen chloride ($HCl$)

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

Chloromethane ($CH_3Cl$)
Hydrogen chloride ($HCl$)

","correct":true,"explanation":"Chlorine substitutes for one hydrogen atom in methane, producing chloromethane. The displaced hydrogen combines with the other chlorine atom to form hydrogen chloride."},{"text":"

Chloroethane ($C_2H_5Cl$)
Hydrogen chloride ($HCl$)

","correct":false,"explanation":"Chloroethane comes from substituting hydrogen in ethane, not methane. Methane chlorination produces chloromethane and hydrogen chloride because methane contains one carbon atom."},{"text":"

Methanol ($CH_3OH$)
Hydrogen chloride ($HCl$)

","correct":false,"explanation":"Methanol contains an oxygen atom and is not formed when chlorine substitutes into methane. The organic product is chloromethane, alongside hydrogen chloride."},{"text":"

Chloromethane ($CH_3Cl$)
Hydrogen ($H_2$)

","correct":false,"explanation":"The displaced hydrogen does not form hydrogen gas because it reacts with chlorine. The second product is hydrogen chloride, so the pair is chloromethane and HCl."}]},{"id":"bff78d25-f215-4ead-94ab-8a95c06d8fe0","cardType":"cloze","points":null,"front":"The organic product of the substitution of ethane with chlorine is [ ] (formula: $C_2H_5Cl$).","back":"The organic product of the substitution of ethane with chlorine is chloroethane (formula: $C_2H_5Cl$).","mcqOptions":[{"text":"chloroethane","correct":true,"explanation":"Substitution replaces one hydrogen atom in ethane with chlorine. The two-carbon product is therefore chloroethane, with formula $C_2H_5Cl$."},{"text":"chloromethane","correct":false,"explanation":"Chloromethane is formed from methane, which has one carbon atom. Starting with ethane gives the two-carbon substitution product chloroethane, $C_2H_5Cl$."},{"text":"ethene","correct":false,"explanation":"Ethene is an unsaturated hydrocarbon formed by elimination, not by replacing a hydrogen atom in ethane with chlorine. Substitution produces chloroethane."},{"text":"ethanol","correct":false,"explanation":"Ethanol contains an -OH group and is not the product of chlorination. Replacing one hydrogen in ethane with chlorine gives chloroethane, $C_2H_5Cl$."}]},{"id":"1b4a2fb6-4ecf-4b1d-ab22-9f9d1d40d5a5","cardType":"cloze","points":null,"front":"The organic product of the substitution of ethane with chlorine is chloroethane (formula: [ ]).","back":"The organic product of the substitution of ethane with chlorine is chloroethane (formula: $C_2H_5Cl$).","mcqOptions":[{"text":"$$C_2H_5Cl$","correct":true,"explanation":"Ethane has formula $C_2H_6$. Replacing one hydrogen atom with chlorine gives $C_2H_5Cl$, the formula of chloroethane."},{"text":"$$C_2H_6$","correct":false,"explanation":"This is the formula of ethane before substitution. Replacing one hydrogen atom with chlorine changes it to $C_2H_5Cl$, which is chloroethane."},{"text":"$$C_2H_4Cl_2$","correct":false,"explanation":"This formula represents replacement of two hydrogen atoms by chlorine, producing a dichloro compound. Single substitution of ethane gives $C_2H_5Cl$."},{"text":"$$CH_3Cl$","correct":false,"explanation":"$$CH_3Cl$ is chloromethane and contains only one carbon atom. Chloroethane retains ethane’s two-carbon chain, so its formula is $C_2H_5Cl$."}]},{"id":"73af24a9-c060-40ea-b9af-bce1fe568451","cardType":"basic","points":1,"front":"Define activation energy ($E_a$).","back":"The minimum energy particles must have to react.","mcqOptions":[{"text":"The minimum energy particles must have to react.","correct":true,"explanation":"Activation energy is the minimum energy reacting particles must possess for successful collisions. Collisions below this threshold do not result in a chemical reaction."},{"text":"The maximum energy particles can have before reacting.","correct":false,"explanation":"There is no maximum-energy limit defining activation energy. It is the minimum energy particles must have for collisions to lead to a reaction."},{"text":"The average energy particles have during a reaction.","correct":false,"explanation":"Average particle energy relates to temperature and does not define the reaction barrier. Activation energy is the minimum energy required for particles to react."},{"text":"The energy released when particles react.","correct":false,"explanation":"Energy released describes an energy change during a reaction, not the energy barrier before it occurs. Activation energy is the minimum energy particles must have to react."}]},{"id":"0d777f0d-994d-4311-b314-19bfa536743b","cardType":"basic","points":1,"front":"How many hydrogen atoms are in an alkane with 5 carbon atoms?","back":"12","mcqOptions":[{"text":"12","correct":true,"explanation":"Alkanes follow the general formula $C_nH_{2n+2}$. With five carbon atoms, the number of hydrogens is $2(5)+2=12$."},{"text":"10","correct":false,"explanation":"Using $2n$ gives 10 hydrogen atoms, but that is the alkene pattern. Alkanes follow $C_nH_{2n+2}$, so five carbons require 12 hydrogens."},{"text":"14","correct":false,"explanation":"Adding four instead of two to $2n$ gives 14, an arithmetic or formula slip. The alkane formula is $C_nH_{2n+2}$, giving 12 hydrogens for five carbons."},{"text":"5","correct":false,"explanation":"This copies the number of carbon atoms rather than applying the alkane formula. For $n=5$, $2n+2$ gives 12 hydrogen atoms."}]},{"id":"b464bd8e-7ca3-4963-bfde-376130355a54","cardType":"basic","points":2,"front":"Contrast saturated and unsaturated molecules in organic chemistry.","back":"

Saturated: only single carbon-carbon bonds
Unsaturated: at least one double carbon-carbon bond

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

Saturated: only single carbon-carbon bonds
Unsaturated: at least one double carbon-carbon bond

","correct":true,"explanation":"Saturated organic molecules contain only single carbon-carbon bonds. Unsaturated molecules contain at least one carbon-carbon double bond, which can undergo addition reactions."},{"text":"

Saturated: at least one double carbon-carbon bond
Unsaturated: only single carbon-carbon bonds

","correct":false,"explanation":"This reverses the definitions. Saturated molecules have only single carbon-carbon bonds, whereas unsaturated molecules have at least one carbon-carbon double bond."},{"text":"

Saturated: only single carbon-hydrogen bonds
Unsaturated: at least one double carbon-oxygen bond

","correct":false,"explanation":"Saturation concerns bonds between carbon atoms, not whether carbon-hydrogen or carbon-oxygen bonds are present. Saturated molecules have only single carbon-carbon bonds; unsaturated molecules have a carbon-carbon double bond."},{"text":"

Saturated: an even number of carbon atoms
Unsaturated: an odd number of carbon atoms

","correct":false,"explanation":"The number of carbon atoms does not determine whether an organic molecule is saturated. The distinction is between only single carbon-carbon bonds and having at least one double carbon-carbon bond."}]}]}],"examCountdown":null,"heading":"Alkanes","title":"Alkanes Flashcards","topbar":{"backHref":"/igcse/chemistry/cie/flashcards"},"topicSidebar":"$L38"}]}],"topicId":"4fd65917-f500-5602-a287-715cae3a9f55","walled":"$L39"}],"$L3a","$L3b"]