Unit Introduction

This is your gateway to understanding organic chemistry - the study of carbon-based compounds that make up everything from petrol to perfumes. You'll master the art of naming molecules and recognising patterns in their behaviour.

The key to success here is learning to spot the structural patterns that determine how molecules behave. Once you've cracked the code, you'll see chemistry everywhere around you.

Quick Tip: Keep the naming rules handy - they're your roadmap through this entire topic!

Homologous Series

Ever wondered why petrol burns differently to cooking oil? It's all about homologous series - families of compounds that share similar structures and properties. Think of them as chemical cousins with the same general formula but different sizes.

The main families you need to know are alkanes (like methane), alkenes (like ethene), cycloalkanes, alcohols, and carboxylic acids. Each has its own general formula that acts like a mathematical recipe for building molecules.

When naming branched molecules, follow the four golden rules: find the longest chain, identify branches, number carbons to get the lowest numbers, then list branches alphabetically. Remember "McBride Educates People By Pretending He Has Oscars" for the carbon chain lengths.

Isomers are like molecular twins - same formula, different arrangement. They're crucial because even tiny structural changes can completely alter a compound's properties.

Memory Hook: Use the mnemonic to nail those carbon chain prefixes - it'll save you marks in exams!

Saturation and Addition Reactions

Here's where chemistry gets exciting - saturated compounds are like fully packed suitcases (only single bonds), while unsaturated compounds have room for more (contain double bonds). This difference completely changes how they react.

The bromine test is your go-to method for spotting unsaturated compounds. Add bromine water and watch - if it goes from orange to colourless, you've got double bonds present. It's like a chemical detective test.

Addition reactions happen when small molecules crash into double bonds and stick there. Whether it's bromination, hydrogenation, chlorination, or hydration, the pattern is always the same - the double bond breaks and new atoms join the party.

Understanding these reactions isn't just academic - they're used to make everything from margarine (hydrogenation) to plastics (polymerisation).

Real World: Hydrogenation turns liquid oils into solid margarine - that's addition reactions in your kitchen!

Aromatic Compounds

Meet benzene - chemistry's rebel that breaks all the rules you've just learned. Despite looking like it has double bonds, benzene doesn't behave like other unsaturated compounds. It's got delocalised electrons that make it incredibly stable.

This stability means benzene won't react with bromine like other unsaturated compounds. Think of it as chemistry's equivalent of a perfectly balanced spinning top - it's happy as it is and doesn't want to change.

Phenol and phenyl groups are benzene's derivatives that pop up everywhere in organic chemistry. Phenol is benzene with an -OH group attached, making it useful for everything from antiseptics to plastics.

The key insight here is that aromatic compounds march to their own beat - they prefer substitution reactions over addition reactions because they want to keep their stable ring structure.

Key Point: Benzene's stability comes from electron delocalisation - imagine electrons spread like butter across the entire ring rather than stuck between specific atoms.

Introduction to Alcohols

Alcohols are the party molecules of organic chemistry - they contain the hydroxyl group $-OH$ that makes them incredibly versatile. From the ethanol in hand sanitiser to the glycerol in soap, alcohols are everywhere.

The general formula CₙH₂ₙ₊₁OH is your key to identifying any alcohol. But chemistry loves variety, so you'll also meet diols $two -OH groups$ and triols $three -OH groups$ like glycerol.

Glycerol $propane-1,2,3-triol$ is particularly important - it's the backbone of fats and oils in your body. Understanding its structure helps explain why fats behave the way they do.

The position of that -OH group matters enormously. Moving it just one carbon along the chain can change a molecule from a useful fuel additive to a toxic poison.

Fun Fact: Glycerol is what makes soap slippery and helps keep your skin moisturised!

Types of Alcohols

Not all alcohols are created equal - they come in three distinct types based on where that hydroxyl group attaches. Primary alcohols have the -OH attached to a carbon with only one other carbon neighbour. Think of them as the end-of-the-line molecules.

Secondary alcohols are the middle children - their -OH sits on a carbon with two carbon neighbours. These often make great solvents and appear in many household products.

Tertiary alcohols are the crowded ones - three carbon atoms surround the carbon bearing the -OH group. This crowding makes them behave very differently in reactions, often making them more resistant to oxidation.

Why does this matter? Each type reacts differently when you try to oxidise them, producing different products. Primary alcohols can become carboxylic acids, secondary become ketones, but tertiary alcohols stubbornly refuse to oxidise under normal conditions.

Memory Trick: Primary = one neighbour, Secondary = two neighbours, Tertiary = three neighbours. Simple!

Properties of Alcohols

Ever wondered why alcohols have such different properties from their alkane cousins? It all comes down to that polar hydroxyl group and its ability to form hydrogen bonds. These are like molecular handshakes that hold molecules together more tightly.

Melting and boiling points of alcohols are much higher than equivalent alkanes because hydrogen bonds are stronger than the weak London dispersion forces in alkanes. Breaking hydrogen bonds requires more energy, hence higher temperatures.

This explains why ethanol (alcohol) boils at 78°C while ethane boils at -89°C, despite having similar molecular weights. The hydrogen bonding makes all the difference.

As alcohol molecules get larger, they become less polar overall. The hydrocarbon chain grows while the -OH group stays the same size, gradually changing the molecule's personality from polar to non-polar.

Key Insight: Hydrogen bonds are the strongest intermolecular forces - they're what make alcohols so different from hydrocarbons.

Solubility and Trends

Solubility in water follows a clear pattern - short-chain alcohols dissolve brilliantly because they can form hydrogen bonds with water molecules. But as the carbon chain grows longer, the non-polar hydrocarbon part takes over and solubility drops dramatically.

Ethanol mixes with water in any proportion (that's why alcoholic drinks exist!), but try dissolving octanol and you'll be waiting forever. The long hydrocarbon chain makes it behave more like oil than alcohol.

This creates fascinating trends as you move up the alcohol series. Flammability decreases, molecular mass increases, solubility in water drops, and melting/boiling points rise steadily.

Understanding these trends helps explain why methanol is used as a fuel, ethanol for drinks and antiseptics, and longer alcohols for industrial solvents and lubricants.

Real World: This is why vodka (40% ethanol) mixes with water, but cooking oil doesn't - it's all about polarity and hydrogen bonding!

Carboxylic Acids

Carboxylic acids are the sour molecules of chemistry, containing the distinctive carboxyl group $-COOH$. From the acetic acid in vinegar to the fatty acids in your cell membranes, these compounds are essential to life.

The general formula CₙH₂ₙ₊₁COOH covers everything from formic acid (ant venom) to complex fatty acids. Unlike other functional groups, the carboxyl group is always at the end of the chain, so you never need to number its position.

Neutralisation reactions are where carboxylic acids really shine. They react with alkalis to form salts and water, following the classic acid-base pattern. These reactions are crucial in everything from antacid tablets to soap making.

The carboxyl group is actually two functional groups merged together - a carbonyl $C=O$ and a hydroxyl $-OH$. This combination creates unique properties that neither group has alone.

Daily Life: Every time you eat vinegar or citrus fruit, you're experiencing carboxylic acids in action!

Esters

Esters are chemistry's perfume makers - they're responsible for most fruity smells and flavours you encounter. They form through condensation reactions between carboxylic acids and alcohols, where water is eliminated to create the ester link $-COO-$.

Esterification is reversible, meaning esters can break back down into their parent alcohol and acid. This equilibrium is crucial in biological processes like fat digestion and metabolism.

Naming esters follows a simple two-step dance: change the alcohol name to end in "-yl" and the acid name to end in "-oate", then put alcohol first, acid second. So methanol + ethanoic acid becomes methyl ethanoate.

The general formula CₙH₂ₙO₂ applies to simple esters, though more complex ones exist. Esters are everywhere - in fruit flavourings, perfumes, and even the polyester in your clothes.

Smell Test: Next time you smell banana flavouring, you're detecting isoamyl acetate - a classic ester that tricks your nose!