Organic chemistry might seem complex, but it's actually about understanding...
Chemistry666 views·Updated 19 Jul 2026·6 pagesComprehensive Chemistry Notes on Alkenes, Alkanes, and Polymers
Annabel@annabel_xo
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1
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Alkenes and Their Properties
Alkenes are unsaturated hydrocarbons that contain a carbon-carbon double bond , which makes them much more reactive than alkanes. The first four alkenes you need to know are ethene, propene, butene, and pentene, and they all follow the general formula CₙH₂ₙ.
What makes alkenes special is their ability to undergo addition reactions. The double bond can "open up" to allow other atoms to attach, turning the unsaturated alkene into a saturated compound. This is something alkanes simply can't do because they only have single bonds.
When alkenes burn, they produce smoky flames due to incomplete combustion. This happens because the double bonds make it harder for complete combustion to occur, which is why alkenes aren't typically used as fuels despite being hydrocarbons.
Key Point: The C=C double bond is what gives alkenes their reactive nature - it's like a "hook" that other molecules can attach to!
2
of 6
Addition Reactions of Alkenes
Alkenes can undergo three main types of addition reactions, each producing different useful products. Hydrogenation involves adding hydrogen gas with a nickel catalyst to produce alkanes - this process is used in making margarine from vegetable oils.
Hydration adds steam (water) at about 300°C with a catalyst to create alcohols. This is actually how industrial ethanol is produced for use in chemicals and fuels.
Halogenation involves adding halogens like bromine or chlorine to create halogenoalkanes. This reaction is particularly important for testing - when you add bromine water to an alkene, it changes from orange-brown to colourless, proving an alkene is present.
Test Tip: Remember the bromine water test - it's colourless with alkenes but stays orange-brown with alkanes. This often comes up in exams!
3
of 6
Alcohols and Their Reactions
Alcohols contain the functional group -OH (hydroxyl group) and follow the general formula CₙH₂ₙ₊₁OH. The ones you'll encounter most are methanol, ethanol, propanol, and butanol - notice how the names end in "-ol".
Alcohols are surprisingly reactive and undergo several important reactions. When mixed with strong oxidising agents, they form carboxylic acids. They react with sodium metal to produce hydrogen gas, and they dissolve in water to give neutral solutions.
Fermentation is a crucial process for producing ethanol using yeast and sugar. The ideal conditions are 37°C (body temperature), slightly acidic conditions, and no oxygen present (anaerobic). This ancient process is still used today for making alcoholic beverages and biofuels.
Real-World Connection: Fermentation happens in your kitchen when you make bread - the yeast produces both alcohol (which evaporates) and CO₂ (which makes the bread rise)!
4
of 6
Carboxylic Acids
Carboxylic acids contain the -COOH (carboxyl group) and have the general formula CₙH₂ₙ₊₁COOH. Common examples include methanoic acid (HCOOH) and ethanoic acid (CH₃COOH) - you'll recognise ethanoic acid as the main component in vinegar.
These are weak acids because they only partially ionise in water, making them less dangerous than strong acids like hydrochloric acid. When dissolved in water, they create acidic solutions but won't burn through your skin like concentrated strong acids would.
Carboxylic acids react with alcohols (using an acid catalyst) to form esters and water. They also react with carbonates to produce a salt, carbon dioxide, and water - just like other acids do.
Memory Trick: Remember "COOH" sounds like "COO" - carboxylic acids are the ones that make vinegar smell and taste sharp!
5
of 6
Polymerisation
Polymerisation is the process of joining small molecules (monomers) together to create long chains called polymers - think of it like connecting LEGO bricks to build something massive. There are two main types you need to understand.
Addition polymerisation uses alkenes as monomers because their C=C double bonds can open up and link together. The polymer contains exactly the same atoms as the original monomers - nothing is lost. Poly(ethene) plastic bags are made this way from ethene monomers.
Condensation polymerisation involves monomers with two functional groups that join together whilst producing small molecules like water as by-products. Amino acids (which have both -NH₂ and -COOH groups) use this process to form proteins and polypeptides in your body.
Think About It: Your hair, muscles, and even the enzymes in your digestive system are all polymers made from amino acids through condensation polymerisation!
6
of 6
Key Alkene Reactions Summary
Understanding alkene reactions becomes much easier when you focus on the specific conditions and products for each reaction type. Hydrogenation requires a nickel catalyst and produces alkanes, whilst hydration needs high temperatures (around 300°C) and a catalyst to form alcohols.
The halogenation reaction is particularly useful for identification purposes. When alkenes react with halogens like bromine, the orange-brown bromine water becomes colourless, creating compounds like dibromoethane from ethene and bromine.
Remember that alkenes aren't used as fuels because their double bonds cause incomplete combustion, resulting in sooty, smoky flames. This makes them less efficient and more polluting than alkanes for energy production.
Exam Success: Practice drawing the structural formulas for these reactions - examiners love testing whether you can show the before and after structures correctly!
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Chemistry666 views·Updated 19 Jul 2026·6 pagesComprehensive Chemistry Notes on Alkenes, Alkanes, and Polymers
Annabel@annabel_xo
Organic chemistry might seem complex, but it's actually about understanding how different groups of carbon-based molecules behave and react with each other. You'll discover how alkenes, alcohols, carboxylic acids, and polymers each have their own unique properties and reactions that...
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Alkenes and Their Properties
Alkenes are unsaturated hydrocarbons that contain a carbon-carbon double bond , which makes them much more reactive than alkanes. The first four alkenes you need to know are ethene, propene, butene, and pentene, and they all follow the general formula CₙH₂ₙ.
What makes alkenes special is their ability to undergo addition reactions. The double bond can "open up" to allow other atoms to attach, turning the unsaturated alkene into a saturated compound. This is something alkanes simply can't do because they only have single bonds.
When alkenes burn, they produce smoky flames due to incomplete combustion. This happens because the double bonds make it harder for complete combustion to occur, which is why alkenes aren't typically used as fuels despite being hydrocarbons.
Key Point: The C=C double bond is what gives alkenes their reactive nature - it's like a "hook" that other molecules can attach to!
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Addition Reactions of Alkenes
Alkenes can undergo three main types of addition reactions, each producing different useful products. Hydrogenation involves adding hydrogen gas with a nickel catalyst to produce alkanes - this process is used in making margarine from vegetable oils.
Hydration adds steam (water) at about 300°C with a catalyst to create alcohols. This is actually how industrial ethanol is produced for use in chemicals and fuels.
Halogenation involves adding halogens like bromine or chlorine to create halogenoalkanes. This reaction is particularly important for testing - when you add bromine water to an alkene, it changes from orange-brown to colourless, proving an alkene is present.
Test Tip: Remember the bromine water test - it's colourless with alkenes but stays orange-brown with alkanes. This often comes up in exams!
3
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Alcohols and Their Reactions
Alcohols contain the functional group -OH (hydroxyl group) and follow the general formula CₙH₂ₙ₊₁OH. The ones you'll encounter most are methanol, ethanol, propanol, and butanol - notice how the names end in "-ol".
Alcohols are surprisingly reactive and undergo several important reactions. When mixed with strong oxidising agents, they form carboxylic acids. They react with sodium metal to produce hydrogen gas, and they dissolve in water to give neutral solutions.
Fermentation is a crucial process for producing ethanol using yeast and sugar. The ideal conditions are 37°C (body temperature), slightly acidic conditions, and no oxygen present (anaerobic). This ancient process is still used today for making alcoholic beverages and biofuels.
Real-World Connection: Fermentation happens in your kitchen when you make bread - the yeast produces both alcohol (which evaporates) and CO₂ (which makes the bread rise)!
4
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Carboxylic Acids
Carboxylic acids contain the -COOH (carboxyl group) and have the general formula CₙH₂ₙ₊₁COOH. Common examples include methanoic acid (HCOOH) and ethanoic acid (CH₃COOH) - you'll recognise ethanoic acid as the main component in vinegar.
These are weak acids because they only partially ionise in water, making them less dangerous than strong acids like hydrochloric acid. When dissolved in water, they create acidic solutions but won't burn through your skin like concentrated strong acids would.
Carboxylic acids react with alcohols (using an acid catalyst) to form esters and water. They also react with carbonates to produce a salt, carbon dioxide, and water - just like other acids do.
Memory Trick: Remember "COOH" sounds like "COO" - carboxylic acids are the ones that make vinegar smell and taste sharp!
5
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Polymerisation
Polymerisation is the process of joining small molecules (monomers) together to create long chains called polymers - think of it like connecting LEGO bricks to build something massive. There are two main types you need to understand.
Addition polymerisation uses alkenes as monomers because their C=C double bonds can open up and link together. The polymer contains exactly the same atoms as the original monomers - nothing is lost. Poly(ethene) plastic bags are made this way from ethene monomers.
Condensation polymerisation involves monomers with two functional groups that join together whilst producing small molecules like water as by-products. Amino acids (which have both -NH₂ and -COOH groups) use this process to form proteins and polypeptides in your body.
Think About It: Your hair, muscles, and even the enzymes in your digestive system are all polymers made from amino acids through condensation polymerisation!
6
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Key Alkene Reactions Summary
Understanding alkene reactions becomes much easier when you focus on the specific conditions and products for each reaction type. Hydrogenation requires a nickel catalyst and produces alkanes, whilst hydration needs high temperatures (around 300°C) and a catalyst to form alcohols.
The halogenation reaction is particularly useful for identification purposes. When alkenes react with halogens like bromine, the orange-brown bromine water becomes colourless, creating compounds like dibromoethane from ethene and bromine.
Remember that alkenes aren't used as fuels because their double bonds cause incomplete combustion, resulting in sooty, smoky flames. This makes them less efficient and more polluting than alkanes for energy production.
Exam Success: Practice drawing the structural formulas for these reactions - examiners love testing whether you can show the before and after structures correctly!
We thought you’d never ask...
Our AI Companion is a student-focused AI tool that offers more than just answers. Built on millions of Knowunity resources, it provides relevant information, personalised study plans, quizzes, and content directly in the chat, adapting to your individual learning journey.
You can download the app from Google Play Store and Apple App Store.
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