- Carboxylic acids are carbon compounds with a –COOH group and have acidic nature.
- Types:
- Monocarboxylic acids have one –COOH group (e.g., formic acid, acetic acid)
- Dicarboxylic acids have two –COOH groups (e.g., oxalic acid) - IUPAC Naming: Replace the ‘e’ of the corresponding alkane with ‘oic acid’ (e.g., ethane → ethanoic acid); also called alkanoic acids.
Definitions [3]
Definition: Esterification
Alcohols and phenols form esters by reaction with carboxylic acid, acid halides and acid anhydrides. This reaction is called esterification.
Definition: Carbonyl Compound
Organic compounds containing carbon-oxygen double bond, i.e. \[\mathrm{>C=O}\] group, are known as carbonyl compounds.
Definition: Carboxylic Acid
An organic compound containing the carboxyl group (-COOH) is known as carboxylic acid. These compounds possess acidic properties.
Formulae [1]
Formula: Carboxylic Acid
General formula: CnH2n+1COOH (or RCOOH)
Functional group:
Key Points
Key Points: Alcohols, Phenols and Ethers
- Alcohols: Compounds with one or more –OH groups attached directly to a carbon chain. General formula: C₂H₂ₙ₊₁OH.
- Phenols: Compounds where –OH group is directly bonded to an aromatic (benzene) ring.
- Ethers: Compounds with general formula R–O–R'. If R = R', it is a symmetrical ether; if R ≠ R', it is an unsymmetrical ether.
Types of Alcohols
| Type | Meaning | Position of —OH |
|---|---|---|
| Allylic Alcohol | —OH attached to sp³-hybridised carbon next to C=C double bond | Carbon next to C=C |
| Benzylic Alcohol | —OH attached to sp³-hybridised carbon next to aromatic ring | Benzylic carbon |
| Vinylic Alcohol | —OH attached directly to a vinylic carbon (CH₂=CH—) or aryl carbon | On C=C bond |
Key Points: Classification of Alcohols, Phenols and Ethers
Classification of Alcohols
Based on number of —OH groups
| Type | —OH Groups | Example |
|---|---|---|
| Monohydric | 1 | Ethanol (CH₃CH₂OH) |
| Dihydric | 2 | Ethylene glycol (CH₂OH–CH₂OH) |
| Trihydric | 3 | Glycerol |
| Polyhydric | More than 3 | Glucose |
Based on hybridisation of carbon bearing —OH (Monohydric only):
| Type | Description | Example |
|---|---|---|
| Primary (1°) | —OH on primary carbon | R–CH₂–OH |
| Secondary (2°) | —OH on secondary carbon | R–CH(OH)–R |
| Tertiary (3°) | —OH on tertiary carbon | R–C(OH)(R)–R |
| Allylic | —OH on sp³ carbon next to C=C | CH₂=CH–CH₂OH |
| Vinylic | —OH directly on sp² carbon of C=C | CH₂=CH–OH |
| Benzylic | —OH on sp³ carbon next to aromatic ring | C₆H₅–CH₂–OH |
Classification of Phenols
| Type | —OH Groups | Example |
|---|---|---|
| Monohydric | 1 | Phenol |
| Dihydric | 2 | Catechol (Benzene-1,2-diol) |
| Trihydric | 3 | Phloroglucinol (Benzene-1,3,5-triol) |
Classification of Ethers
| Type | Description | Example |
|---|---|---|
| Simple / Symmetrical | Same alkyl/aryl groups on both sides of O | CH₃–O–CH₃ (Dimethyl ether), C₆H₅–O–C₆H₅ (Diphenyl ether) |
| Mixed / Unsymmetrical | Different alkyl/aryl groups on both sides of O | CH₃–O–C₂H₅ (Ethyl methyl ether), C₂H₅–O–C₆H₅ (Ethyl phenyl ether) |
Key Points: Nomenclature of Alcohols, Phenols and Ethers
- Alcohol names are derived from alkanes by replacing ‘e’ with ‘ol’ (e.g., methane → methanol).
- In alcohols, the longest chain containing –OH is selected and numbered to give the lowest locant to the –OH group.
- Phenol is the simplest aromatic alcohol; substituted phenols use ortho (1,2), meta (1,3), and para (1,4) positions.
- Ethers are named as alkoxyalkanes in IUPAC; the smaller group becomes the alkoxy prefix.
- Common names: Alcohol → alkyl + alcohol, Ether → alkyl groups + ether
Key Points: Structures of Functional Groups of Alcohols, Phenols and Ethers
- Alcohols: O atom is sp³ hybridised; two bond pairs + two lone pairs; bent structure.
- Phenols: –OH directly on benzene ring; lone pair on O delocalised into ring → more acidic than alcohols.
- Ethers: O is sp³ hybridised. Two O–C sigma bonds + two lone pairs. Structure similar to water molecule. Bent/angular shape.
Key Points: Chemical Properties of Alcohols and Phenols
- Litmus Test — Aqueous alcohols are neutral to litmus, while aqueous phenols turn blue litmus red, confirming the acidic character of phenols.
- Reaction with Bases — Phenols react with NaOH to form water-soluble sodium phenoxide (regenerated on acidification with HCl) but do not react with NaHCO₃, since phenol is a weak acid.
- Esterification — Alcohols/phenols react with carboxylic acids (conc. H₂SO₄ catalyst), acid anhydrides (H⁺ catalyst), or acid chlorides (in pyridine) to form esters; Aspirin is the acetyl derivative of salicylic acid formed using acetic anhydride.
- Reactivity with Hydrogen Halides — Order of alcohol reactivity: 3° > 2° > 1°; order of HX reactivity: HI > HBr > HCl (HCl needs anhydrous ZnCl₂ catalyst).
- Oxidation of Alcohols — 1° alcohol → aldehyde (with PCC, best reagent) → further to carboxylic acid (with KMnO₄/K₂Cr₂O₇/HNO₃); 2° alcohol → ketone (with CrO₃); 3° alcohols resist oxidation and break C–C bonds only at high temperature.
Key Points: Commercially Important Alcohols
Methanol (Wood Spirit):
-
Produced by catalytic hydrogenation of CO:
\[\ce{CO + 2H2 ->[ZnO/Cr2O3, 200-300atm, 573-673K] CH3OH}\]
-
Highly poisonous; used as a solvent in paints and varnishes.
Ethanol:
-
Produced by fermentation of sugar:
\[\ce{C12H22O11 + H2O ->[Invertase] \underset{Glucose}{C6H12O6} + \underset{Fructose}{C6H12O6}}\]
-
Used as a solvent and in the preparation of carbon compounds.
Differentiation between Methanol & Ethanol:
-
Iodoform test: Ethanol gives yellow ppt (CHI₃); methanol gives no reaction.
-
With salicylic acid + H₂SO₄: Methanol forms methyl salicylate (characteristic odour); ethanol gives no specific odour.
Key Points: Preparation of Ethers
-
Williamson Synthesis (most important): R–O–Na + X–R' → R–O–R' + NaX. Primary alkyl halide is preferred (SN2 mechanism; 2° or 3° alkyl halide gives elimination).
-
Acid-catalysed dehydration of alcohols:
\[\ce{2R - OH ->[H2SO4, 413K] R - O - R + H2O}\]
(works best for symmetrical ethers)
-
From alcohols by catalytic dehydration:
\[\ce{2C2H5OH ->[Al2O3, 513-523K] C2H5 - O - C2H5 + H2O}\]
-
Alkoxy mercuration-demercuration: \[\begin{array}{cc}
\phantom{}\ce{CH3 - CH = CH2 + C2H5OH + Hg(OCOCF3)2 -> CH3 - CH - CH2 - HgOCOCF3 ->[NaBH4/OH^{-}] CH3 - CH - CH3}\\
\phantom{................................................................................}|\phantom{.....................................................................}|\phantom{.}\\
\phantom{............................................................................................}\ce{OC2H5}\phantom{...........................................................}\ce{O-C2H5}\phantom{.}
\end{array}\]
Key Points: Physical Properties of Ethers
- Colourless liquids (except dimethyl ether and diethyl ether, which are gases).
- Polar due to bent structure (like a water molecule).
- Low boiling point due to the absence of H-bonding between ether molecules.
- Slightly soluble in water due to H-bonding with water; more soluble in organic solvents.
- Structure: O is sp³ hybridised; two sp³ orbitals form O–C sigma bonds; two sp³ orbitals have lone pairs.
Key Points: Physical Properties of Ethers
- Methods of preparation of ethers: Acid-catalysed dehydration of alcohols (conc. H₂SO₄, 443 K); catalytic dehydration (Al₂O₃, 250°C); Williamson synthesis (alkyl halide + sodium alkoxide, Sₙ2); reaction of alkyl halides with dry Ag₂O.
- Preparation of Diethyl Ether (Simple Ether): From ethanol using conc. H₂SO₄ / H₃PO₄ at 413 K; or by Williamson's synthesis from C₂H₅ONa + BrCH₂CH₃ under heat.
- Reactions of Diethyl Ether: O₂ (long contact) → peroxide; dil. H₂SO₄ → 2 C₂H₅OH; PCl₅ → C₂H₅OH + C₂H₅Cl; hot HI → C₂H₅I + C₂H₅OH; excess HI → 2 C₂H₅I.
- Preparation of Anisole (Mixed Ether): CH₃Br + sodium phenoxide (C₆H₅ONa) → Methyl phenyl ether (Anisole) on heating.
- Reactions of Anisole: HI (398 K) → phenol + CH₃I; Br₂/CH₃COOH → p-bromoanisole (major) + o-bromoanisole (minor); conc. HNO₃ + conc. H₂SO₄ → 4-nitroanisole (major) + 2-nitroanisole (minor); CH₃Cl/AlCl₃ → 4-methoxytoluene (major) + 2-methoxytoluene (minor); CH₃COCl/AlCl₃ → 4-methoxyacetophenone (major) + 2-methoxyacetophenone (minor).
Key Points: Chemical Reactions of Ethers – Cleavage of C–O Bond
- Ethers are generally very unreactive (no H-bonding between ether molecules).
- When excess HX is added → C–O bond cleaves → alkyl halides.
- Reactivity of HX: HI > HBr > HCl
- If 1° or 2° alkyl groups: Smaller alkyl group forms alkyl iodide. (e.g., C₂H₅–O–CH₃ + HI → C₂H₅OH + CH₃I)
- If one alkyl group is 3°: Forms tertiary alkyl halide (SN1 pathway).
Reaction with conc. HI:
- With excess HI: Both groups convert to iodo compounds
- e.g., \[\ce{C2H5OC2H5 + HI ->[Cold] C2H5I + C2H5OH}\]
Key Points: Chemical Reactions of Ethers – Electrophilic Substitution
Substitution Reactions in Aromatic Ether: The alkoxу group in ether activates the aromatic ring at ortho and para positions for electrophilic substitution. Common electrophilic substitution reactions are halogenation, Friedel-Crafts reaction, etc.
Key Points: Concepts of Aldehydes, Ketones, and Carboxylic Acids
- Carbonyl group: The ≻C=O group (carbonyl carbon + carbonyl oxygen) — a key functional group in organic chemistry.
- Carbonyl compounds: Aldehydes and ketones, both containing ≻C=O as their functional group.
- Aldehydes: –CHO (formyl group); carbonyl C bonded to at least one H.
- Ketones: ≻C=O (ketonic carbonyl group); carbonyl C bonded to two alkyl/aryl groups (R=R′ or R≠R′).
- Carboxylic acids: –COOH (carboxyl group); –OH attached to ≻C=O makes them distinct from aldehydes/ketones.
Key Points: Nomenclature of Aldehydes and Ketones
In IUPAC system in aldehyde the suffix ‘e’ of alkane is replaced by ‘al’, e.g.,
CH₃—CH₂—CH=O; Propanal
\[ \underset{\text{2-methylpropanal}}{\mathrm{CH}_3 - \underset{\underset{\displaystyle \mathrm{CH}_3}{|}}{\mathrm{CH}} - \mathrm{CH} = \mathrm{O}} \]
In ketones, the suffix ‘e’ of alkane is replaced by ‘one’.
For example,
\[ \underset{\text{Butan-2-one}}{\mathrm{CH}_3 - \mathrm{CH}_2 - \overset{\displaystyle \mathrm{O}}{\overset{||}{\mathrm{C}}} - \mathrm{CH}_3} \quad \quad \underset{\text{Propanone (Acetone)}}{\mathrm{CH}_3\mathrm{COCH}_3} \]
Key Points: Structure of the Carbonyl Group
- Carbon is sp² hybridised (trigonal planar, bond angle ≈ 120°).
- C = O bond consists of one σ bond and one π bond.
- Oxygen is more electronegative, so it pulls electron density towards itself →
C gets a partial positive charge (δ⁺) and O gets a partial negative charge (δ⁻). - This makes the carbonyl group polar.
- Hence, the carbon atom becomes electrophilic and is susceptible to nucleophilic attack.
Key Points: Preparation of Aldehydes and Ketones
Preparation of aliphatic aldehydes and ketones
By oxidation of alcohols:
\[\ \begin{array}{r@{\;}c@{\;}l} \mathrm{R} & & \\ & \backslash & \\ & & \mathrm{CH}-\mathrm{OH} \\ & / & \\ \mathrm{R}' & & \end{array} + [\mathrm{O}] \xrightarrow[\text{Or KMnO}_4]{\text{K}_2\text{Cr}_2\text{O}_7/\text{H}_2\text{SO}_4} \begin{array}{r@{\;}c@{\;}l} \mathrm{R} & & \\ & \backslash & \\ & & \mathrm{C}=\mathrm{O} \\ & / & \\ \mathrm{R}' & & \end{array} + \mathrm{H}_2\mathrm{O}\]
When,
- R' = H then 1° alcohol to aldehyde.
- R' = alkyl group then 2º alcohol to ketone.
By dehydrogenation of alcohols:
\[ \begin{array}{r@{\;}c@{\;}l} \mathrm{R} & & \\ & \backslash & \\ & & \mathrm{CH}-\mathrm{OH} \\ & / & \\ \mathrm{R}' & & \end{array} \xrightarrow[\text{573 K}]{\text{Cu}} \begin{array}{r@{\;}c@{\;}l} \mathrm{R} & & \\ & \backslash & \\ & & \mathrm{C}=\mathrm{O} \\ & / & \\ \mathrm{R}' & & \end{array} + \mathrm{H}_2 \]
When
- R' = H then 1° alcohol to aldehyde.
- R' = alkyl group the 2° alcohol to ketone.
By acid chloride:
\[ \mathrm{R} - \overset{\displaystyle \mathrm{O}}{\overset{||}{\mathrm{C}}} - \mathrm{Cl} + \mathrm{H}_2 \xrightarrow[\text{Rosenmund Reduction}]{\text{Pd}-\text{BaSO}_4} \underset{\text{Aldehyde}}{\mathrm{R} - \overset{\displaystyle \mathrm{O}}{\overset{||}{\mathrm{C}}} - \mathrm{H}} + \mathrm{HCl} \]
2RMgX + CdCl2 → R2Cd + 2MgXCl
\[\ 2\mathrm{R}' - \overset{\displaystyle \mathrm{O}}{\overset{||}{\mathrm{C}}} - \mathrm{Cl} + \mathrm{R}_2\mathrm{Cd} \longrightarrow 2\mathrm{R}' - \underset{\text{Ketone}}{\overset{\displaystyle \mathrm{O}}{\overset{||}{\mathrm{C}}}} - \mathrm{R} + \mathrm{CdCl}_2 \]
From nitriles and esters:
\[ \mathrm{R} - \mathrm{CN} \xrightarrow[\text{(ii) }\mathrm{H}_2\mathrm{O}]{\text{(i) }\mathrm{AlH}(i\text{Bu})_2} \underset{\text{Aldehyde}}{\mathrm{R} - \mathrm{CHO}} \]
\[ \mathrm{CH}_3(\mathrm{CH}_2)_9 - \overset{\displaystyle \mathrm{O}}{\overset{||}{\mathrm{C}}} - \mathrm{OC}_2\mathrm{H}_5 \xrightarrow[\text{(ii) }\mathrm{H}_2\mathrm{O}]{\text{(i) DIBAL-H}} \mathrm{CH}_3(\mathrm{CH}_2)_9 - \underset{\text{Aldehyde}}{\overset{\displaystyle \mathrm{O}}{\overset{||}{\mathrm{C}}} - \mathrm{H}} \]
From hydrocarbons
By ozonolysis:
By hydration:
Key Points: Physical Properties of Aldehydes and Ketones
- Most aldehydes are liquids (except HCHO = gas); ketones of lower order are colourless liquids with a pleasant odour.
- Higher BP than corresponding hydrocarbons but lower than alcohols (no H-bonding between molecules, but dipole-dipole interactions).
- Lower members are soluble in water (H-bonding with water); higher members are insoluble (large alkyl groups).
Key Points: Chemical Reactions of Aldehydes and Ketones - Nucleophilic Addition Reactions
Addition of HCN:
\[\text{HCN} + \text{OH}^- \rightleftharpoons :\text{CN}^- + \text{H}_2\text{O}\]
Addition of NaHSO3:
Addition of Grignard reagent:
Addition of alcohols:
Key Points: Chemical Reactions of Aldehydes and Ketones - Reduction
\[\text{R}-\text{CHO} + 2[\text{H}] \xrightarrow[\text{or BH}_3]{\text{LiAlH}_4} \text{RCH}_2\text{OH}\]
\[\begin{array}{r@{\;}c@{\;}l r@{\;}c@{\;}l} \ce{R} & & & \ce{R} & & \\ & \backslash & & & \backslash & \\ & & \ce{C=O + H2 ->[Ni or Pt]} & & & \ce{CH2OH} \\ & / & & & / & \\ \ce{R} & & & \ce{R} & & \end{array}\]
Clemmensen reduction:
\begin{array}{r@{\;}c@{\;}l c r@{\;}c@{\;}l} & & & & & & \\ & \backslash & & & & \backslash & \\ & & \ce{C=O} & \xrightarrow[\text{HCl}]{\text{Zn-Hg}} & & & \ce{CH2 + H2O} \\ & / & & & & / & \\ & & & & & & \end{array}
Wolff-Kishner reduction:
\begin{array}{r@{\;}c@{\;}l c r@{\;}c@{\;}l c r@{\;}c@{\;}l} & & & & & & & & & & \\ & \backslash & & & & \backslash & & & & \backslash & \\ & & \ce{C=O} & \xrightarrow[-\ce{H2O}]{\ce{NH2NH2}} & & & \ce{C=NNH2} & \xrightarrow{\text{KOH ethylene Glycol, }\Delta} & & & \ce{CH2 + N2} \\ & / & & & & / & & & & / & \\ & & & & & & & & & & \end{array}
Key Points: Chemical Reactions of Aldehydes and Ketones - Oxidation
\[\underset{\text{Aldehyde}}{\ce{R-CHO}} + \ce{[O]} \xrightarrow[\text{or }\ce{KMnO4/H2SO4}]{\ce{K2Cr2O7/H2SO4}} \underset{\text{Carboxylic acid}}{\ce{R-COOH}}\]
Key Points: Chemical Reactions of Aldehydes and Ketones - Reactions Due to α-hydrogen
Aldol condensation:
\[\ce{CH3 - \overset{\displaystyle O}{\overset{||}{C}} - H + H - CH2 - \overset{\displaystyle O}{\overset{||}{C}} - H} \xrightarrow{\text{dil. NaOH}} \ce{H3C - \underset{\underset{\displaystyle OH}{|}}{CH} - \underset{\underset{\displaystyle H}{|}}{CH} - \overset{\displaystyle O}{\overset{||}{C}} - H} \\ \xrightarrow{\text{dil. }\ce{H2SO4}\Delta, \ce{-H2O}} \ce{CH3 - CH = CH - \overset{\displaystyle O}{\overset{||}{C}} - H}\]
Mechanism:
Cross aldol condensation:
\[\begin{array}{ccccccccccccc} & \ce{O} & & \ce{O} & & & & \ce{OH} & & \ce{O} & & & \\ & || & & || & & & & | & & || & & & \\ \ce{C6H5 -} & \ce{C} & \ce{+ HCH2 -} & \ce{C} & \ce{- H} & \overset{\text{dil. NaOH}}{\rightleftharpoons} & \ce{C6H5 -} & \ce{C} & \ce{- CH2 -} & \ce{C} & \ce{- H} & \xrightarrow[\Delta]{\ce{H2O}} & \ce{C6H5CH=CHCHO} \\ & | & & & & & & | & & & & & \text{Cinnamaldehyde} \\ & \ce{H} & & & & & & \ce{H} & & & & & \end{array}\]
Cannizzaro reaction: It is a self-oxidation reduction reaction.
\[\begin{array}{r@{\;}c@{\;}l} \ce{H} & & \\ & \backslash & \\ & & \ce{C=O} \\ & / & \\ \ce{H} & & \end{array} + \begin{array}{r@{\;}c@{\;}l} \ce{H} & & \\ & \backslash & \\ & & \ce{C=O} \\ & / & \\ \ce{H} & & \end{array} + \text{conc. KOH} \xrightarrow{\Delta} \ce{H - \underset{\underset{\displaystyle H}{|}}{\overset{\overset{\displaystyle H}{|}}{C}} - OH} + \ce{H - \overset{\displaystyle O}{\overset{||}{C}} - OK}\]
Haloform Reaction:
The reaction can be used to transform acetyl groups into carboxyl groups or to produce chloroform or iodoform. This reaction has been used in qualitative analysis to indicate the presence of a methyl ketone in which excess iodine is used to halogenate the compound. The product iodoform precipitates as a yellow-coloured substance and has a characteristic odour.
\[\underset{\substack{\text{Acetone} \\ \text{Iodoform Test}}}{\ce{H3C - \overset{\displaystyle O}{\overset{||}{C}} - CH3}} \xrightarrow[4\ce{NaOH}]{3\ce{Cl2}} \underset{\text{Sodium acetate}}{\ce{H3C - \overset{\displaystyle O}{\overset{||}{C}} - O^\ominus Na^\oplus}} + \underset{\text{Chloroform}}{\ce{CHCl3}}\]
Key Points: Uses of Aldehydes and Ketones
- Formaldehyde: Used in making Bakelite (phenol-formaldehyde resin), as a preservative (formalin = 40% HCHO).
- Acetaldehyde: Used in the preparation of acetic acid and ethanol.
- Acetone: Solvent (nail polish remover), used in the manufacture of chloroform.
- Benzaldehyde: Used in perfumes and dyes.
Key Points: Carboxylic Acid
Key Points: Preparation of Carboxylic Acids
- Special preparations: Benzoic acid from cumene (KMnO₄/KOH, Δ → H₃O⁺); adipic acid from cyclohexene (KMnO₄/dil. H₂SO₄, Δ).
- Aldehyde preparation: From 1° alcohol (K₂Cr₂O₇/H₂SO₄ or Cu/573 K), alkene (ozonolysis), alkyne (dil. H₂SO₄/HgSO₄), acid chloride (Rosenmund), nitrile (Stephen/DIBAL-H); aromatic via Etard, CrO₃/(CH₃CO)₂O, Cl₂/hν, Gatterman–Koch.
- Aldehyde reactions: HCN → cyanohydrin; NaHSO₃ → bisulphite adduct; R′OH → acetal; RMgBr → 2° alcohol; NH₂OH → aldoxime; NH₂NH₂ → hydrazone; K₂Cr₂O₇ → COOH; Clemmensen/Wolf–Kishner → alkane.
- Carboxylic acid preparation: From nitriles (hydrolysis), acyl chloride/anhydride/ester + H₂O, CO₂ + RMgX (dry ether, H₃O⁺), alkylbenzene (KMnO₄–KOH).
- Carboxylic acid reactions: PCl₅/SOCl₂ → RCOCl; NH₃ → amide; P₂O₅ → anhydride; NaOH + CaO (Δ) → alkane; LiAlH₄ → 1° alcohol; ROH/conc. H₂SO₄ → ester.
Key Points: Physical Properties of Carboxylic Acids
- Solubility: Decreases with an increase in the size of the hydrocarbon part.
- Miscibility: Lower carboxylic acids (up to 4 C atoms) are miscible with water due to H-bonding.
- Boiling point: Carboxylic acids have higher B.P. than ketones, aldehydes, and alcohols of comparable molecular mass due to intermolecular H-bonding.
- Order of B.P. (carboxylic acids & aldehydes): Valeric > Butyric > Propionic > Acetic > Formic acid; Hexanal > Pentanal > Butanal > Propanal.
- Order of B.P. (ketones): Hexan-2-one > Pentan-2-one > Butan-2-one > Propanone.
Key Points: Uses of Carboxylic Acids
- Methanoic acid (Formic acid): Leather tanning, dyeing and finishing in textiles.
- Ethanoic acid (Acetic acid): Manufacturing of rayon and plastic; used as vinegar in cooking.
- Benzoic acid: Used as a food preservative and in perfumery.
- Salicylic acid: Used in the preparation of Aspirin (analgesic/antipyretic), Salol, and Oil of Wintergreen (methyl salicylate).
- Aspirin = acetylsalicylic acid; anti-pyretic and pain killer.
- Methyl salicylate = Oil of wintergreen (from methanol + salicylic acid).
Concepts [42]
- Introduction of Organic Compounds Containing Oxygen
- Concept of Alcohols, Phenols and Ethers
- Classification of Alcohols, Phenols and Ethers
- Nomenclature of Alcohols, Phenols and Ethers
- Structures of Functional Groups of Alcohols, Phenols and Ethers
- Identification of Primary, Secondary, and Tertiary Alcohols
- Methods of Preparation of Alcohols
- Methods of Preparation of Phenols
- Chemical Properties of Alcohols and Phenols
- Chemical Reactions of Alcohols and Phenols
- Reactions Involving Cleavage of O-H Bond
- Reactions Involving Cleavage of Carbon–Oxygen (C–O) Bond in Alcohols
- Reactions of Phenols
- Commercially Important Alcohols
- Preparation of Ethers
- Physical Properties of Ethers
- Chemical Reaction of Ethers - Cleavege of C-O Bonds
- Chemical Reaction of Ethers - Electrophilic Substitution
- Concepts of Aldehydes, Ketones, and Carboxylic Acids
- Nomenclature of Aldehydes and Ketones
- Structure of Carbonyl Group
- Preparation of Aldehydes
- Preparation of Ketones
- Preparation of Aldehydes and Ketones
- Physical Properties of Aldehydes and Ketones
- Chemical Reactions of Aldehydes and Ketones - Nucleophilic Addition Reactions
- Chemical Reactions of Aldehydes and Ketones - Reduction
- Chemical Reactions of Aldehydes and Ketones - Oxidation
- Chemical Reactions of Aldehydes and Ketones - Reactions Due to α-hydrogen
- Chemical Reactions of Aldehydes and Ketones - Other Reactions
- Relative Reactivities of Aldehydes and Ketones
- Uses of Aldehydes and Ketones
- Carboxylic Acids
- Nomenclature of Carboxylic Acids
- Structure of the Carboxyl group
- Methods of Preparation of Carboxylic Acids
- Physical Properties of Carboxylic Acids
- Chemical Reactions of Carboxylic Acids - Reactions Involving Cleavege of O-H Bond
- Chemical Reactions of Carboxylic Acids - Reactions Involving Cleavege of C-OH Bond
- Chemical Reactions of Carboxylic Acids - Reactions Involving –COOH Group
- Chemical Reactions of Carboxylic Acids - Substitution Reactions in the Hydrocarbon Part
- Uses of Carboxylic Acids
