Alcohols, Phenols and Ethers — Class 12 Chemistry Notes & Practice

If you have opened this page because Alcohols, Phenols and Ethers Class 12 Chemistry looks like a wall of forty unrelated reactions, take a breath. It is not forty reactions. It is one idea, wearing forty costumes. Every single thing this chapter asks you to remember — why phenol dissolves in sodium hydroxide but ethanol does not, why the Lucas test takes five minutes for one alcohol and no time at all for another, why a nitro group on a ring changes everything — comes back to a single question: once the oxygen has let go of its hydrogen, how comfortable is the negative charge left behind?

That question is what we are going to call the acidity ladder, and it is the spine of this whole page. We will build the ladder early, then hang every preparation, every property and every named reaction off it. By the end you will not be reciting reactions; you will be predicting them. That is the difference between six marks and two.

This is Unit 7 of the CBSE Class 12 Chemistry course for 2026-27 and it carries 6 marks in the 70-mark theory paper. Along the way you will get Alcohols, Phenols and Ethers with solved examples, a full reaction and reagent list, the identification tests laid out as a single lab-bench decision flow, and a practice worksheet with worked answers. Read it slowly. Nothing here needs to be memorised twice.

What You’ll Learn

Your Game Plan

1. Spend fifteen minutes on the acidity ladder alone. Do not move on until you can draw it from memory and say why each rung sits where it does.
2. Learn nomenclature next. Half the marks lost in this unit are lost on names, not on chemistry.
3. Do the preparations as a table, not as prose — reagent in the left column, product in the right.
4. Attack the reactions of phenol in one sitting, because they are all consequences of the same ring.
5. Finish with ethers. They are the short, easy marks, and students routinely leave them for a day that never comes.
6. Then close the book and walk through the identification decision flow in your head, twice.

Study Notes

Classification of Alcohols, Phenols and Ethers

Three families, one shared feature: a carbon atom joined to an oxygen atom by a single bond. What changes is what else that oxygen is holding, and what kind of carbon it is attached to.

An alcohol has –OH sitting on an sp³ (tetrahedral, single-bonded) carbon. A phenol has –OH sitting directly on an sp² carbon of an aromatic ring. An ether has the oxygen sandwiched between two carbon groups with no hydrogen of its own: R–O–R′. That last detail — no O–H — is the reason ethers behave so differently, and it is worth writing on the inside cover of your notebook.

Alcohols are sorted three ways. First by how many –OH groups: monohydric (ethanol), dihydric (ethane-1,2-diol), trihydric (propane-1,2,3-triol), and polyhydric beyond that. Second by which carbon carries the –OH: primary (1°) if that carbon is attached to one other carbon, secondary (2°) if two, tertiary (3°) if three. Third, by the neighbourhood: an allylic alcohol has the –OH carbon next door to a C=C double bond, and a benzylic alcohol has it next door to a benzene ring.

Phenols are sorted only by count: monohydric (phenol), dihydric (benzene-1,2-diol, benzene-1,3-diol, benzene-1,4-diol), trihydric (benzene-1,2,3-triol). Ethers are sorted by symmetry: symmetrical or simple when both groups are identical (ethoxyethane), unsymmetrical or mixed when they differ (methoxyethane), and an alkyl aryl ether when one of the two is a ring (methoxybenzene).

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IUPAC Nomenclature and the Structure of the Functional Groups

Naming is the cheapest mark in the unit and the one most often thrown away. There are only four habits to build.

1. Alcohols: find the longest carbon chain that contains the –OH carbon, drop the final “e” of the alkane and add “-ol”. Number the chain so the –OH gets the lowest possible locant — the –OH beats a double bond and beats an alkyl branch.
2. Two or more –OH groups: keep the final “e” and add -diol, -triol. So it is ethane-1,2-diol, not ethan-1,2-diol.
3. Phenols: the parent name is simply phenol, and the carbon carrying the –OH is C-1 by definition. Substituents are then numbered to get the lowest set.
4. Ethers: the larger group is the parent alkane; the smaller one becomes an alkoxy prefix. CH₃–O–CH₂CH₃ is methoxyethane, not ethoxymethane.

Structure of the functional groups. In an alcohol the oxygen is sp³ hybridised, so the C–O–H arrangement is bent, with an angle a little smaller than the perfect tetrahedral 109.5°. Two lone pairs on the oxygen crowd the bonding pairs and squeeze the angle shut. In an ether, R–O–R′, the same oxygen now has two bulky carbon groups instead of one carbon and one small hydrogen, so they push apart and the C–O–C angle opens out slightly beyond the tetrahedral value.

In a phenol the picture changes qualitatively. The –OH is attached to an sp² ring carbon, and one lone pair of the oxygen overlaps with the ring’s π system. That overlap gives the C–O bond partial double-bond character, so the C–O bond in phenol is measurably shorter than the C–O bond in methanol. It also builds a small positive charge on the oxygen — and an oxygen carrying a partial positive charge is far more willing to let its hydrogen go. Hold onto that sentence; it is the entire acidity story in advance.

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The Acidity Ladder — the Master Idea

Here is the ladder, and here is the single rule that builds it. When an O–H bond breaks, the hydrogen leaves as H⁺ and a negatively charged oxygen is left behind — the conjugate base. If that negative charge can be shared out over several atoms, the conjugate base is comfortable, it forms readily, and the parent compound is a stronger acid. If the charge is stuck on one lonely oxygen, the conjugate base is unhappy, it does not form easily, and the parent is a weak acid. That is the whole mechanism of this chapter, stated once.

Climb the rungs from the bottom.

• Alcohols (bottom rung). R–O⁻ keeps the entire charge on one oxygen, and the alkyl group actually pushes electron density towards that oxygen (+I effect), making the crowding worse. Alcohols are therefore weaker acids than water. Among alcohols the order is CH₃OH > 1° > 2° > 3°, because each extra alkyl group pushes a little more.
• Water. HO⁻ has no alkyl group pushing at it, so it is slightly better off than an alkoxide. Water sits just above alcohols.
• Phenol. Now the ring joins in. In the phenoxide ion the negative charge is delocalised from the oxygen into the ring, appearing at the ortho and para carbons. Charge shared over four centres instead of one — a huge jump. Phenol is roughly a million times more acidic than ethanol.
• Substituted phenols. Add an electron-withdrawing group such as –NO₂ at the ortho or para position and it pulls even more charge away; the phenoxide gets even more comfortable and acidity rises again. Add an electron-donating group such as –CH₃ or –OCH₃ and it pushes charge back, so acidity falls slightly below plain phenol.
• Carboxylic acids (top rung). In RCOO⁻ the charge is split equally between two identical oxygen atoms — the two C–O bonds become exactly the same length. Nothing in this chapter beats that.

The ladder immediately pays for itself with a reagent trick. Sodium metal is aggressive enough to react with anything from rung 1 upwards, so it fizzes with alcohols, phenols and carboxylic acids alike. Sodium hydroxide can only deprotonate things above water — so phenol dissolves in NaOH but ethanol does not. Sodium hydrogencarbonate is weaker still and only reacts with the top rung — so a carboxylic acid gives brisk CO₂ effervescence and phenol gives nothing at all. Three bottles, three rungs, one clean separation.

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Preparation of Alcohols

Three families of route, and each one answers a different design question: where do I want the –OH to land?

(a) From alkenes — acid-catalysed hydration. Bubble the alkene through dilute acid and water adds across the double bond following Markovnikov’s rule: the –OH ends up on the more substituted carbon. The mechanism has three steps. The π electrons grab a proton to give the more stable carbocation; a water molecule attacks that carbocation; a second water molecule removes the extra proton. Because a carbocation is involved, rearrangements are possible — and that is exactly why the second method exists.

(b) From alkenes — hydroboration–oxidation. Treat the alkene with diborane, B₂H₆, to get a trialkylborane, then oxidise with alkaline hydrogen peroxide (H₂O₂ / OH⁻). The –OH lands on the less substituted carbon — an anti-Markovnikov result — and because no carbocation is ever formed, nothing rearranges. Boron and hydrogen add to the same face of the double bond, so the addition is syn.

(c) From carbonyl compounds by reduction. Feeding hydrogen into a C=O group knocks it down to C–OH. An aldehyde gives a 1° alcohol; a ketone gives a 2° alcohol. Any of H₂ with a metal catalyst (Ni, Pd or Pt), sodium borohydride (NaBH₄) or lithium aluminium hydride (LiAlH₄) will do the job. Carboxylic acids are harder to reduce and need LiAlH₄; industrially they are first converted to esters and the ester is then hydrogenated, because LiAlH₄ is expensive.

(d) From Grignard reagents. This is the carbon-chain builder. R–Mg–X, made from an alkyl halide and magnesium in dry ether, attacks the carbonyl carbon; the adduct is then hydrolysed with dilute acid to release the alcohol. The class of alcohol you get is decided entirely by the carbonyl partner:

• Grignard + methanal (HCHO) → a 1° alcohol with one carbon more than the Grignard.
• Grignard + any other aldehyde → a 2° alcohol.
• Grignard + a ketone → a 3° alcohol.

If the arrow-pushing behind carbocation stability still feels shaky, the substitution and elimination groundwork sits one chapter earlier — work through our chapter on Haloalkanes and Haloarenes before you go further, because SN1, SN2 and carbocation rearrangement all reappear here in new clothes.

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Preparation of Phenols

Four routes. Two are laboratory routes that force an –OH onto a ring; two are industrial. Learn them as reagent-plus-condition pairs, because that is exactly how they are examined.

The haloarene route needs brutal conditions because the C–Cl bond in chlorobenzene has partial double-bond character and refuses to give up its chlorine easily. The sulphonic acid route works because the –SO₃H group can be displaced by hydroxide when NaOH is molten. The diazonium route is the gentlest and cleanest — the diazonium group is such a good leaving group (it leaves as nitrogen gas) that warm water is all the reagent you need.

The cumene route is the one industry actually uses, and the reason is economic rather than chemical: it produces propanone (acetone) as a valuable by-product. That by-product is a favourite one-mark question, so do not let it slip past you.

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Physical Properties: Hydrogen Bonding, Boiling Point, Solubility

One picture explains this whole section. An O–H group is a molecular hook: the oxygen is strongly electronegative, so the hydrogen carries a real partial positive charge and reaches out to the lone pair on a neighbouring oxygen. That is a hydrogen bond, and it means alcohol and phenol molecules cling to one another. An ether has no O–H hook at all, so ether molecules simply do not hold hands.

The consequence is dramatic. Ethanol and methoxymethane have exactly the same molecular formula, C₂H₆O, and exactly the same molar mass of 46 g mol⁻¹. Ethanol is a liquid at room temperature that boils at around 78 °C. Methoxymethane is a gas — it boils far below room temperature. Same atoms, same mass, opposite states of matter, and the only difference is hydrogen bonding.

Boiling point within a set of isomers. For isomeric alcohols the order is 1° > 2° > 3°. Branching makes a molecule more spherical, which shrinks the contact area between neighbouring molecules and weakens the van der Waals forces, so the more branched isomer boils lowest. Across a homologous series, boiling point rises steadily with molar mass because there is simply more surface to attract.

Solubility in water. A small alcohol is essentially a water molecule wearing a short carbon coat — methanol, ethanol and propan-1-ol mix with water in all proportions. As the carbon chain lengthens the greasy hydrocarbon part starts to dominate and solubility falls away. Branching, oddly, helps: a branched alcohol has less surface area to hide from water, so 2-methylpropan-2-ol is more soluble than butan-1-ol.

Ethers are the interesting case. They cannot hydrogen-bond to each other, so their boiling points are low. But they can accept a hydrogen bond from a water molecule, so their solubility in water is roughly the same as that of the isomeric alcohol. Low boiling point, decent water solubility — the two facts feel contradictory until you separate “can it bond to its own kind?” from “can it bond to water?”

Hydrogen bonding is also the reason alcohols behave so unusually as solvents and why their solutions show the deviations you met earlier — the treatment of ideal and non-ideal behaviour in our chapter on Solutions is the same physics seen from a different angle.

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Chemical Reactions of Alcohols

An alcohol can be attacked in two completely different places, and sorting a reaction into one of these two boxes is most of the battle.

• Cleavage of the O–H bond. The hydrogen leaves. This is acid-like behaviour: reaction with sodium, and esterification.
• Cleavage of the C–O bond. The whole –OH leaves. This is substitution and elimination: reaction with HX, with PCl₅, with SOCl₂, and dehydration.

1. Reaction with active metals. 2 R–OH + 2 Na → 2 R–O⁻Na⁺ + H₂. The product is a sodium alkoxide, and hydrogen gas fizzes off. Rate of reaction follows the acidity order: 1° > 2° > 3°.

2. Esterification. R–OH + R′COOH, warmed with a trace of concentrated H₂SO₄, gives the ester R′COOR plus water. The reaction is reversible, so the acid catalyst is also there to pull the equilibrium along, and removing water drives it further right. Acid chlorides and acid anhydrides do the same job irreversibly and faster; a base such as pyridine is added to mop up the HCl produced.

3. Reaction with hydrogen halides. R–OH + HX → R–X + H₂O. The –OH is a poor leaving group, so it is first protonated to –OH₂⁺, which leaves happily as water. Reactivity of the alcohol runs 3° > 2° > 1°, and of the halide acid HI > HBr > HCl. When the halide is chloride the reaction needs help, and that help is anhydrous zinc chloride — the Lucas reagent, which we come to in the next section.

4. Reaction with PCl₅, PCl₃ and SOCl₂. These are the clean laboratory ways to swap –OH for –Cl. R–OH + PCl₅ → R–Cl + POCl₃ + HCl. 3 R–OH + PCl₃ → 3 R–Cl + H₃PO₃. R–OH + SOCl₂ → R–Cl + SO₂ + HCl, which is the tidiest of all because both by-products are gases and escape, leaving pure alkyl chloride.

5. Dehydration. Heat ethanol with concentrated sulphuric acid at about 443 K and you get ethene. The mechanism is worth writing out in full, because CBSE asks for it by name.

1. Protonation. The lone pair on the alcohol oxygen picks up a proton from the acid, giving a protonated alcohol, R–OH₂⁺. Fast and reversible.
2. Loss of water. The C–O bond breaks heterolytically and a water molecule departs, leaving a carbocation. This is the slow, rate-determining step.
3. Loss of a proton. A base (a bisulphate ion or another alcohol molecule) removes a hydrogen from the carbon next to the positive centre, and the electrons of that C–H bond swing across to make the π bond. The alkene is formed and the catalyst is regenerated.

Because step 2 makes a carbocation, ease of dehydration follows carbocation stability: 3° > 2° > 1°. And when more than one alkene is possible, the more highly substituted alkene is the major product (Saytzeff’s rule). The idea of a rate-determining step is exactly the one you met in our chapter on Chemical Kinetics — the slowest step sets the pace for the whole sequence.

6. Oxidation and dehydrogenation. Oxidation here means adding oxygen or removing hydrogen from the carbon that carries the –OH. What you get depends on how many hydrogens that carbon has to give.

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Telling 1°, 2° and 3° Alcohols Apart

Three bottles of colourless liquid, all smelling faintly of hospital corridors. How do you tell which is which? There are three standard methods and each one exploits a different consequence of the acidity-and-carbocation story.

Method 1 — the Lucas test. Lucas reagent is concentrated hydrochloric acid plus anhydrous zinc chloride. Zinc chloride is a Lewis acid; it grips the oxygen and helps water leave, so a carbocation forms. The alkyl chloride produced is insoluble in the reagent, so it shows up as a cloudiness or turbidity. How fast the cloud appears tells you the class of alcohol, because it tells you how easily that carbocation forms.

Method 2 — oxidation. Warm each alcohol with acidified potassium dichromate. A 1° alcohol turns the orange solution green and yields first an aldehyde and then a carboxylic acid. A 2° alcohol also turns it green but stops at a ketone. A 3° alcohol leaves the solution stubbornly orange.

Method 3 — catalytic dehydrogenation over copper at 573 K. This is the cleanest discriminator of all because each class gives a chemically different kind of product: a 1° alcohol gives an aldehyde, a 2° alcohol gives a ketone, and a 3° alcohol does not dehydrogenate at all — it dehydrates instead, giving an alkene. Aldehyde, ketone, alkene: three different answers, no ambiguity.

The bonus test — iodoform. Warm the alcohol with iodine and sodium hydroxide. A yellow precipitate of iodoform, CHI₃, appears only if the molecule contains the CH₃–CH(OH)– unit, that is, a methyl group attached to the carbinol carbon which still carries a hydrogen. Ethanol, propan-2-ol and butan-2-ol are positive. Methanol and propan-1-ol are negative. 2-Methylpropan-2-ol is negative too, because its carbinol carbon has no hydrogen at all.

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Chemical Reactions of Phenols

Phenol has a split personality, and both halves come from the same resonance. The oxygen’s lone pair pushes into the ring. That makes the O–H more acidic (charge can leave the oxygen) and simultaneously makes the ring electron-rich (charge arrives at the ortho and para carbons). So phenol is an unusually good acid and an unusually eager partner for electrophiles. Every reaction below is one of those two things.

1. Acidity. Phenol dissolves in aqueous sodium hydroxide to give sodium phenoxide and water. It does not react with sodium hydrogencarbonate, so no carbon dioxide is evolved. That single negative result is what separates phenol from a carboxylic acid in every board question ever written on the topic.

2. Esterification (acylation). Phenol reacts with acetic anhydride, or with ethanoyl chloride in the presence of a base, to give phenyl ethanoate (phenyl acetate). Phenols are poorer nucleophiles than alcohols, which is why the more reactive anhydride or acid chloride is used rather than the carboxylic acid itself.

3. Electrophilic substitution. The –OH group is strongly activating and ortho, para-directing.

• Nitration. With dilute nitric acid at low temperature, phenol gives a mixture of 2-nitrophenol and 4-nitrophenol. The two are separated by steam distillation: the ortho isomer forms an intramolecular hydrogen bond (a private handshake inside its own molecule), so it does not cling to its neighbours and travels over with the steam; the para isomer forms intermolecular hydrogen bonds and stays behind. With concentrated nitric acid the reaction goes all the way to 2,4,6-trinitrophenol, picric acid.
• Halogenation. This one is a two-condition question. Phenol with bromine in a non-polar solvent such as carbon disulphide at 273 K gives mainly 4-bromophenol. Phenol with bromine water gives an immediate white precipitate of 2,4,6-tribromophenol. The difference is polarity: in water phenol ionises a little to phenoxide, which is even more activated, so all three positions are attacked at once.

4. Kolbe’s reaction. Sodium phenoxide is heated with carbon dioxide under pressure (about 400 K, 4–7 atm). Carbon dioxide is a weak electrophile, but phenoxide is a strong enough nucleophile to attack it. The product, after acidification, is 2-hydroxybenzoic acid — salicylic acid, the parent of aspirin.

5. Reimer–Tiemann reaction. Phenol is treated with chloroform and aqueous sodium hydroxide at about 340 K. The hydroxide strips a proton from chloroform to generate dichlorocarbene, :CCl₂, which is the real electrophile. It attacks the ortho position, and hydrolysis of the resulting intermediate gives 2-hydroxybenzaldehyde — salicylaldehyde.

6. Reaction with zinc dust. Distil phenol with zinc dust and the oxygen is stripped off altogether: you get benzene and zinc oxide. It is a neat way of walking a substituent back off the ring.

7. Oxidation. Phenol is oxidised by sodium dichromate in sulphuric acid to benzene-1,4-dione (para-benzoquinone), a bright conjugated diketone. Old phenol samples go pink for the same reason — slow air oxidation. If keeping track of what is being oxidised and what is being reduced still trips you up, the electron bookkeeping in our chapter on Electrochemistry is the cleanest place to rebuild that habit.

8. The ferric chloride test. Add neutral ferric chloride solution to phenol and a violet colouration appears, from a coloured iron–phenoxide complex. Alcohols give nothing. This is the fastest single test for a phenolic –OH on the bench.

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Preparation of Ethers

Two methods, and one of them comes with a design trap that examiners set almost every year.

(a) Dehydration of alcohols. Heat an alcohol with concentrated sulphuric acid at about 413 K and two molecules join with the loss of water: 2 R–OH → R–O–R + H₂O. This is nucleophilic substitution — a second alcohol molecule attacks the protonated first one — and because it is essentially an SN2 process it works well only for primary alcohols. Secondary and tertiary alcohols eliminate instead and hand you an alkene. It also only ever gives symmetrical ethers, since there is just one alcohol in the flask.

(b) Williamson synthesis. An alkoxide (or a phenoxide) attacks an alkyl halide: R–O⁻Na⁺ + R′–X → R–O–R′ + NaX. This is a clean SN2 reaction and it is the general method — it will build symmetrical and unsymmetrical ethers, and alkyl aryl ethers too.

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Properties and Reactions of Ethers

An ether has no O–H, so it is chemically quiet: it does not react with sodium, it is not acidic, and it will happily sit in a flask as a solvent while more dramatic chemistry happens around it. That is precisely why diethyl ether is the traditional Grignard solvent. But the ether oxygen still has lone pairs, and under acidic conditions those lone pairs are its weak point.

1. Cleavage of the C–O bond by hydrogen halides. Heat an ether with a hydrogen halide and it splits. Reactivity of the acid is HI > HBr > HCl. The oxygen is protonated first, then a halide ion attacks a carbon. Which carbon it attacks is the whole question.

• Both groups primary or secondary → SN2. The iodide attacks the less hindered carbon. So methoxyethane + HI gives iodomethane + ethanol. With excess HI and heat, the ethanol goes on to become iodoethane.
• One group tertiary → SN1. A stable tertiary carbocation forms, so the halide bonds to the tertiary carbon. So 2-methoxy-2-methylpropane + HI gives 2-iodo-2-methylpropane + methanol.
• Alkyl aryl ethers → always phenol + alkyl halide. The C(aryl)–O bond has partial double-bond character and its carbon is sp², so it is never attacked. Anisole + HI gives phenol + iodomethane, never iodobenzene and methanol.

2. Electrophilic substitution on aromatic ethers. In an alkyl aryl ether the –OR group behaves like –OH: it pushes electron density into the ring, so it is activating and ortho, para-directing. Because the methoxy group is bulky, the para product usually dominates.

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Some Commercially Important Alcohols

The syllabus names this section explicitly, and it is genuinely easy marks — two molecules, a handful of facts each.

Methanol, CH₃OH. Historically it was made by the destructive distillation of wood, which is why it is still called wood spirit. Industrially it is produced by passing carbon monoxide and hydrogen over a zinc oxide–chromium oxide catalyst at high temperature and pressure. It is used as a solvent, as an antifreeze, and as the raw material for methanal. It is also seriously poisonous: ingesting even small quantities causes blindness, and larger amounts are fatal. This is exactly why industrial ethanol is deliberately contaminated with methanol.

Ethanol, C₂H₅OH. Made industrially by the fermentation of sugars. The enzyme invertase in yeast first splits sucrose into glucose and fructose; the enzyme zymase then converts those sugars into ethanol and carbon dioxide. Ethanol is a solvent, a fuel additive, an antiseptic in dilute solution, and a starting material for a long list of chemicals.

• Denatured or methylated spirit — ethanol made undrinkable by adding methanol together with a dye such as copper sulphate and a little pyridine, so that it can be sold cheaply for industrial use without attracting excise duty.
• Absolute alcohol — ethanol from which essentially all the water has been removed.
• Power alcohol — ethanol blended with petrol as a fuel.

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The Lab-Bench Identification Decision Flow

This is where the whole chapter earns its keep. Imagine a labelled-only-as-“X” bottle containing a colourless liquid known to hold nothing but carbon, hydrogen and oxygen. Four tests, run in this order, will name it. Run them in the wrong order and you will waste reagent and confuse yourself, so the order matters.

1. Sodium metal. Drop in a small clean piece. Bubbles of hydrogen mean an acidic O–H is present, so X is an alcohol, a phenol or a carboxylic acid. No bubbles is already an answer: X is an ether.
2. Neutral ferric chloride. A violet, blue or green colouration means a phenol. Confirm by shaking with sodium hydroxide solution (phenol dissolves) and with bromine water (a white precipitate of 2,4,6-tribromophenol appears).
3. Lucas reagent. Now that X is known to be an alcohol, this sorts the class. Cloudiness at once means 3°; cloudiness after about five minutes means 2°; a clear solution in the cold means 1°.
4. Iodine and sodium hydroxide, warmed. A yellow precipitate of iodoform pins down the exact skeleton: X contains the CH₃–CH(OH)– unit. This is what separates ethanol from methanol, and butan-2-ol from butan-1-ol.

If at step 1 you also want to exclude a carboxylic acid, slip in a fifth bottle: sodium hydrogencarbonate. Brisk effervescence of carbon dioxide means a carboxylic acid, and nothing else in this chapter does that. On the acidity ladder you are simply asking whether X stands above or below carbonic acid.

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Alcohols, Phenols and Ethers Class 12 Chemistry Important Questions — the Reaction and Reagent List

Almost every Alcohols, Phenols and Ethers formula and reaction list question, and most of the NCERT intext exercises, reduces to recognising a reagent. Here is the whole chapter as reagent-in, product-out. Cover the right-hand column and test yourself; when you can fill it in from memory you are ready for the paper.

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Practice Worksheet

Ten questions, written for this page and not lifted from anywhere. Do them with the notes closed, then open each answer. If you get one wrong, go back to the section it came from rather than simply reading the solution again.

One Last Thing

You will not master this chapter in an evening, and you are not supposed to. Tomorrow, come back and try to draw the acidity ladder from memory before you read anything. The day after, write the reagent table with the right-hand column covered. Small, boring, daily gains are what separate a 6 from a 3 in this unit — not a heroic all-nighter. Get one more reaction right today than you did yesterday, and let that be enough.