Carboxylic acids Flashcards
Physical properties of carboxylic acids and derivatives
Structure: Simple molecular structure
1. Higher BP than alkenes (hydrogen bond between carboxylic acid molecules > idid)
2. BP increases down the group
3. Higher BP than alcohols with same alkyl chain
( Alcohols have electron withdrawing carbonyl group –> -OH group more polarised –> carboxylic acid forms stronger intermolecular hydrogen bonds than alcohols –> more energy needed )
4. Higher BP than acyl chlorides and esters
(Hydrogen bond vs pdpd)
5. Soluble in water
6. Insoluble in organic solvents
Structure and bonding of acyl chlorides and esters
For both:
Bonding: pdpd
Structure: simple molecular structure
Synthesis of carboxylic acid
- oxidative cleavage of alkenes
- oxidation of primary alcohols
- oxidation of aldehydes
- acidic hydrolysis of nitriles
- hydrolysis of acyl chlorides
- hydrolysis of esters
- hydrolysis of amides
- side-chain oxidation to give benzoic acid
oxidative cleavage of alkenes
Hot KMnO4, H2SO4(aq)
oxidation of aldehyde
K2Cr2O7/KMnO4, H2SO4(aq), heat under reflux
oxidation of primary alcohol
K2Cr2O7/KMnO4,H2SO4(aq), heat under reflux
Side-chain oxidation to give benzoic acid
KMnO4, H2SO4(aq), heat under reflux
–> white ppt of benzoic acid
Acidic hydrolysis of nitriles
HCl/H2SO4(aq), heat under reflux
Hydrolysis of amides
(Synthesis of carboxylic acids)
H2SO4(aq), heat under reflux
Hydrolysis of acyl chlorides
H2O(l), rtp (milder conditions because acyl chlorides are very reactive)
Hydrolysis of esters
HCl/H2SO4(aq), heat under reflux
Reactions of carboxylic acids
- condensation to form esters
- nucleophilic substitution to form acyl chlorides
- redox (acid-metal)
- Acid-base
- Acid-carbonate
- oxidation of ethanedioic acid
- oxidation of methanoic acid
- reduction to form alcohols
Condensation to form esters
(carboxylic acid)
alcohol, concentrated H2SO4, heat under reflux
Nucleophilic substitution to form acyl chloride
(carboxylic acid)
PCl5, room temperature OR
PCl3, heat under reflux OR
SOCl2, heat under reflux
Redox (acid-metal)
(carboxylic acid)
Na(s) ,produce H2 gas
OH –> O-Na+
Acid-base
(carboxylic acid)
NaOH(aq), produce H2O
OH–>O-Na+
Acid-carbonate
(carboxylic acid)
Na2CO3(aq), produce CO2 and H2O
OH–>O-Na+
Oxidation of methanoic acid
(carboxylic acid)
K2Cr2O7/KMnO4, H2SO4(aq), heat under reflux
–> must have H on C atom thus oxidation occurs
Oxidation of ethanedioic acid
(carboxylic acid)
*special case for strong oxidation
KMnO4, H2SO4(aq), heat under reflux
Reduction of alcohols
(carboxylic acid)
LiAlH4 in dry ether
Synthesis of acyl chlorides + reagents
Nucleophilic substitution (carboxylic acid)
- PCl5, room temperature OR
PCl3, heat under reflux
SOCl2, heat under reflux
Reactions of acyl chlorides
- Hydrolysis of acyl chlorides (synthesis of carboxylic acids)
- H2O(l), rtp - Condensation of acyl chlorides to form amides
- condensation of acyl chlorides to form esters
Condensation of acyl chlorides to form amides
NH3/amine, rtp
Condensation of acyl chlorides to form esters
alcohol+acyl chlorides, rtp
acyl chlorides + phenol:
1. NaOH(aq)
2. add acyl chloride, rtp
Why does carboxylic acids not react with phenols?
- Phenols are weak nucleophiles because the LP of electrons on O delocalises into benzene ring
- electrons on O less available for donation to the carbon deficient C in carboxylic acid
Why acyl chlorides react with phenols?
Carbonyl carbon in acyl chloride is highly electron deficient
Synthesis of esters
- condensation of alcohols and carboxylic acid
- condensation of acyl chlorides and alcohols
- condensation of acyl chlorides and phenols
Reactions of esters
- acidic hydrolysis
HCl/H2SO4(aq), heat under reflux - alkaline hydrolysis
NaOH(aq), heat under reflux - reduction to form CH2OH and alcohol
LiAlH4 in dry ether
Why acyl chlorides most reactive?
- Cl is electron-withdrawing via the inductive effect (due to EN difference)
- OH, -OR, and -NH2 are all electron-donating via the resonance effect (due to delocalisation of electrons)
- C in Cl most electron-deficient, thus most susceptible to nucleophilic attack
Why amides less reactive than esters
- N is less EN than O
- LP of electrons on N delocalises across C=O to a larger extent
- C in amides less electron deficient than C in esters
- attracts nucleophile less readily than esters
Distinguishing tests for carboxylic acids
acid-carbonate reaction
Na2CO3(aq)
effervescence of CO2 gas which forms white ppt in Ca(OH)2.
why are carboxylic acids acidic?
- electron-withdrawing COOH group
- disperses negative charge
- more stable conjugate base
- more acidic