Q.Why are amines basic? Compare basic strength of ammonia, ethylamine and diethylamine. OR How will you prepare ethylamine by using Hofmann bromide reaction and how will you convert ethylamine to ethylisocyanide?
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🔒 Start your 14-day free trial to unlock the full solution →Concept understanding — Amine Basicity Order
Amine Basicity Order – From Intuition to Precision
You already know that a base is something that accepts a proton (H+). An amine does this through the lone pair on its nitrogen. The more readily that lone pair grabs a proton, the stronger the base. So the question becomes: what makes that lone pair more or less willing to accept a proton?
The answer depends on three competing effects: inductive effect (electron pushing/pulling from nearby groups), steric hindrance (bulky groups blocking the proton), and solvation (how water molecules stabilise the protonated amine). And critically, the order flips depending on whether you are in the gas phase or in water.
The Intuition – What Would You Expect?
Imagine a nitrogen with three hydrogens: ammonia (NH3). Now replace one hydrogen with a methyl group (CH3). Methyl is an electron-donating group — it pushes electron density toward the nitrogen. That makes the lone pair richer, so it should grab a proton more easily. So methylamine (CH3NH2) should be a stronger base than ammonia.
Replace another hydrogen with a second methyl group. Now you have dimethylamine ((CH3)2NH). Even more electron density on nitrogen — stronger base still. Replace the third hydrogen: trimethylamine ((CH3)3N). Maximum electron donation — so you would expect it to be the strongest base of all.
That is the inductive effect prediction: more alkyl groups → stronger base. In the gas phase, this is exactly what happens. The order is:
Gas phase: NH3<1∘<2∘<3∘
But in water, the observed order is different. Why?
The Complication – Solvation and Steric Hindrance
When an amine accepts a proton, it becomes a positively charged ammonium ion (RNH3+). In water, that positive charge is stabilised by hydrogen bonding with water molecules. The more hydrogens on the nitrogen, the more hydrogen bonds it can form — and the more stable the protonated form becomes.
A primary amine (1∘) has three N–H hydrogens after protonation. A secondary (2∘) has two. A tertiary (3∘) has only one. So solvation stabilises the protonated form in the order: 1∘>2∘>3∘.
At the same time, bulky alkyl groups physically block the approach of a proton to the nitrogen — this is steric hindrance. A tertiary amine has three bulky groups crowding the nitrogen, making it harder for H+ to reach the lone pair.
So in water, two effects oppose the inductive effect: solvation (which favours more N–H bonds) and steric hindrance (which favours less crowding). The result is a compromise.
The Precise Statement – Aqueous Phase Order
In water, the typical order of basic strength for aliphatic amines is:
Aqueous phase: NH3<3∘<1∘<2∘
That is, secondary amines are the strongest bases in water, followed by primary, then tertiary, then ammonia.
The order in water is not simply "more alkyl groups = stronger base". The secondary amine wins because it has a good balance: enough electron donation from two alkyl groups, but still two N–H hydrogens for solvation, and not too much steric hindrance.
The Full Picture – A Table
| Amine | Gas-phase order (inductive only) | Aqueous order (all effects) | Reason |
|---|---|---|---|
| NH3 | Weakest | Weakest | No alkyl donation; only 3 H-bonds |
| 1∘ (RNH2) | Second | Second | One alkyl group donates; 3 H-bonds after protonation |
| 2∘ (R2NH) | Third | Strongest | Two alkyl groups donate; 2 H-bonds; steric hindrance still low |
| 3∘ (R3N) | Strongest | Third | Three alkyl groups donate most, but only 1 H-bond and high steric hindrance |
The basicity of an amine comes from the lone pair of electrons on its nitrogen atom, which becomes more available for donation as more electron-releasing alkyl groups are attached to it; separately, a primary amine can also be built up (by degrading an amide one carbon shorter) or converted into other nitrogen compounds through well-defined named reactions. …
Amines are basic due to the lone pair on nitrogen; in water, basicity rises as more alkyl groups are attached (up to a point): NH3 < C2H5NH2 < (C2H5)2NH.
Why amines are basic: the nitrogen atom in an amine has one lone pair of electrons not involved in bonding. This lone pair can be donated to a proton (H+) or to any electron-deficient species, so amines act as Lewis bases (and Bronsted bases, accepting a proton to form an ammonium-type cation). The more available/electron-dense this lone pair, the stronger the base.
Comparing basicity of ammonia, ethylamine, and diethylamine (aqueous solution): alkyl groups are electron-releasing (+I effect). As alkyl groups replace H atoms on nitrogen, they push electron density onto N, making the lone pair more available and the amine more basic.
- NH3 (no alkyl group) is the least basic of the three.
- C2H5NH2 (one ethyl group, primary amine) is more basic than NH3 due to the +I effect of the ethyl group.
- (C2H5)2NH (two ethyl groups, secondary amine) is more basic than C2H5NH2, since two alkyl groups donate more electron density than one.
(In water this simple inductive trend can be complicated further by solvation of the protonated ammonium ion and steric hindrance once tertiary amines are involved, but strictly among NH3, a primary, and a secondary amine, basicity rises as NH3 < RNH2 < R2NH.)
So: NH3 < C2H5NH2 < (C2H5)2NH (increasing base strength).
OR
Preparation of ethylamine by the Hofmann bromamide degradation reaction: this converts an amide into a primary amine with ONE LESS carbon (the carbonyl carbon is lost as CO2). To get ethylamine (CH3CH2NH2), start from propanamide (CH3CH2CONH2):
CH3CH2CONH2 + Br2 + 4KOH -> CH3CH2NH2 + 2KBr + K2CO3 + 2H2O
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Showing the 12 most recent of 19 on this concept.
- CBSE 2026Set V11 markMCQQ.Which of the following groups when present at para position increases the basic strength of aniline?(a) −NO2(b) −Br(c) −NH2(d) −COOH
›Reveal solutionSolution
An electron-donating para substituent raises aniline's basicity; among the options only –NH2 is electron-donating.
The basic strength of aniline depends on the availability of the lone pair on the nitrogen of the –NH2 group. Groups that push electron density into the ring (electron-donating, +R/+I) increase the electron density on nitrogen and therefore increase basicity; electron-withdrawing groups do the opposite.
Assessing the para substituents:
- −NO2: strongly electron-withdrawing (−R,−I) → decreases basicity.
- −Br: electron-withdrawing by induction → slightly decreases basicity. …
- CBSE 2026Set ANNUAL1 markQ.Fill in the blank: Amines behaves as ______ due to presence of an unshared pair of electron on Nitrogen atom.
›Reveal solutionSolution
Because of the nitrogen lone pair, amines behave as bases (and nucleophiles).
In an amine, the nitrogen atom carries an unshared (lone) pair of electrons. It can donate this lone pair to a proton (H+) or to an electron-deficient centre. Donating the lone pair to H+ makes the amine act as a Bronsted/Lewis base; donating it t …
- CBSE 2025Set ANNUAL1 markQ.Arrange the following in increasing order of their basic strength- C2H5NH2, (C2H5)2NH, (C2H5)3N, C6H5NH2
›Reveal solutionSolution
Aniline is the weakest (its lone pair is delocalised into the ring); among the ethylamines in water the accepted order is secondary > tertiary > primary, so diethylamine is the strongest and the increasing order is C6H5NH2 < C2H5NH2 < (C2H5)3N < (C2H5)2NH.
Basicity in aqueous solution is decided by the net effect of three factors: the electron-donating alkyl groups (+I effect, which raises the electron density on nitrogen and increases basicity), the steric hindrance to protonation together with the solvation (hydrogen bonding) of the resulting ammonium cation, and - for aniline only - resonance delocalisation of the nitrogen lone pair into the benzene ring, which sharply lowers its availability and hence its basicity.
C6H5NH2 (aniline) is the weakest base of the four, because its lone pair is delocalised into the aromatic ring and is much less available for protonation.
Among the three ethylamines, the order actually observed in aqueous solution (the balance of +I effect, steric crowding and cation solvation) is:
(C2H5)2NH>(C2H5)3N>C2H5NH2
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- CBSE 2025Set ANNUAL1 markMCQQ.Identify the most basic among the given amines:(a) C6H3NH2(b) (C2H5)2NH(c) (C2H5)3N(d) C2H5NH2
›Reveal solutionSolution
In water, basicity of these amines follows (C2H5)2NH > (C2H5)3N > C2H5NH2, so the most basic is diethylamine, (C2H5)2NH.
Basicity of an amine in aqueous solution is governed by three competing effects: (i) the +I (electron-releasing) effect of alkyl groups, which raises electron density on N and favours protonation; (ii) solvation of the resulting ammonium cation by water through H-bonding, which stabilises the cation and favours basicity; and (iii) steric hindrance of bulky alkyl groups around N, which hampers solvation.
- C2H5NH2 (1°): one ethyl group gives a modest +I effect; good solvation (two N-H bonds available). …
- CBSE 2025Set ANNUAL1 markQ.Arrange the following compounds in increasing order of their basic strength in aqueous solution: NH3, C2H5NH2, (C2H5)2NH, (C2H5)3N
›Reveal solutionSolution
In AQUEOUS solution, basicity of amines depends not just on the electron-donating (+I) effect of alkyl groups but also on steric hindrance and how well the resulting ammonium ion is stabilised by hydrogen-bonding with water (solvation); this combination gives the order NH3 < 3 degree < 1 degree < 2 degree amine for the ethyl series.
Factors affecting basicity in water:
- Inductive (+I) effect of alkyl groups: increases electron density on N, favouring basicity; increases with number of alkyl groups (3 degree > 2 degree > 1 degree > NH3 on this factor alone).
- Steric hindrance: bulky alkyl groups around N hinder the approach of a proton and hinder solvation of the resulting ammonium cation.
- Solvation (H-bonding) of the ammonium ion R-NH3+ (or its substituted forms) by water: more N-H bonds allow more hydrogen bonding with water, better stabilising the cation and boosting the observed basicity.
NH3 has no alkyl groups at all (weakest +I effect) - it is the weakest base of the four.
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- CBSE 2025Set ANNUAL1 markQ.Why do amines react as nucleophiles?
›Reveal solutionSolution
An available, reasonably accessible lone pair on N is exactly what defines a good nucleophile/Lewis base.
In an amine, R–NH₂ (or R₂NH, R₃N), the nitrogen is sp³ hybridized (approximately) with one lone pair of electrons not involved in any bond. This lone pair is available to attack an electron-deficient (electrophilic) carbon or other centre, forming a new bond — the defining behaviour of a nucleophile (and, correspondingly, amines also behave as Lewis/Brønsted bases, accepting a proton with this same lone pair). This is why amines readi …
- CBSE 2025Set ANNUAL1 markMCQQ.Which of the following is least basic ?(i) (CH₃)₂NH(ii) NH₃(iii) C₆H₅NH₂(iv) (CH₃)₃N
›Reveal solutionSolution
Aniline is least basic because the lone pair on its N atom is delocalised into the benzene ring, making it far less available to accept a proton than in the aliphatic amines.
Basicity of an amine depends on how freely available the nitrogen lone pair is to accept a proton (H⁺):
- (CH₃)₂NH (dimethylamine, 2° aliphatic amine): two +I (electron-donating) methyl groups increase electron density on N → quite basic.
- NH₃: no alkyl groups, moderate basicity, used as the reference.
- (CH₃)₃N (trimethylamine, 3° aliphatic amine): three +I methyl groups would suggest highest basicity electronically, though steric hindrance and poorer solvation of the resulting cation slightly reduce it — but it remains far more basic than aniline. …
- CBSE 2024Set 56/1/11 markMCQQ.Assertion (A): Aniline is a stronger base than ammonia. Reason (R): The unshared electron pair on nitrogen atom in aniline becomes less available for protonation due to resonance. [Codes (A)-(D) as in the Assertion-Reason instruction.]
›Reveal solutionSolution
Aniline is a weaker base than ammonia because the lone pair on nitrogen in aniline is delocalized into the benzene ring via resonance, making it less available for protonation. Therefore, Assertion (A) is false, and Reason (R) is true.
To understand the basicity of amines, we need to consider the availability of the lone pair of electrons on the nitrogen atom. A base, according to the Brønsted-Lowry definition, is a proton acceptor, and according to the Lewis definition, it is an electron pair donor. Therefore, the more readily available the lone pair on nitrogen is to accept a proton (or donate to an acid), the stronger the base.
Factors that increase the electron density on the nitrogen atom or localize the lone pair make it a stronger base. Conversely, factors that decrease the electron density on nitrogen or delocalize the lone pair make it a weaker base.
Let's analyze ammonia and aniline based on these principles.
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Basicity of Ammonia (NH3)
- In ammonia, the nitrogen atom has one lone pair of electrons.
- This lone pair is localized on the nitrogen atom and is readily available for donation to a proton (H+).
- There are no significant electron-withdrawing or electron-donating groups directly attached to the nitrogen that would extensively delocalize or concentrate this lone pair. Thus, ammonia serves as a reference point for basicity.
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Basicity of Aniline (C6H5NH2)
- Aniline consists of an amino (-NH2) group attached to a benzene ring.
- The nitrogen atom in the amino group also possesses a lone pair of electrons.
- However, this lone pair is in conjugation with the π-electron system of the benzene ring. This leads to resonance.
Resonance structures of Aniline:
C6H5NH2⟷C6H5NH2+ (with negative charge on ortho/para positions)
The lone pair on nitrogen can be delocalized into the benzene ring, as shown by these resonance structures:
NH2 / \ C C // \\ C C \ / C---C (Initial structure with lone pair on N) NH2(+) / \ C C(-) // \\ C C \ / C---C (Lone pair moves into ring, negative charge at ortho position) NH2(+) / \ C C // \\ C(-) C \ / C---C (Negative charge moves to para position) NH2(+) / \ C C(-) // \\ C C \ / C---C (Negative charge moves to other ortho position)- Due to this resonance, the lone pair of electrons on the nitrogen atom is not entirely localized on nitrogen; it is delocalized over the nitrogen and the ortho and para positions of the benzene ring.
- This delocalization makes the lone pair less available for donation to a proton.
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Comparison of Basicity …
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- CBSE 2024Set FZ1 markMCQQ.The compound having most basic strength is:(a) (CH3)2NH(b) CH3NH2(c) (CH3)3N(d) NH3
›Reveal solutionSolution
In water, dimethylamine is the strongest base of the four → option (a).
Concept. Basicity of an amine in water is decided by three factors: the electron-releasing (+I) effect of alkyl groups (raises basicity), steric hindrance around N (lowers it), and stabilisation of the protonated cation by H-bonding to water (more H on N = better solvation).
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- CBSE 2024Set ANNUAL1 markMCQQ.The compound showing highest basic strength in aqueous solution is -(a) (C2H5)3N(b) (C2H5)2NH(c) C2H5NH2(d) NH3
›Reveal solutionSolution
In water, basicity of alkylamines is governed by a balance of +I (electron-donating) effect, steric hindrance, and how well the protonated ammonium ion is stabilised by hydrogen bonding with water; for ethylamines this gives the order secondary > primary > tertiary > ammonia.
Electron-donating alkyl groups increase electron density on N (favouring basicity), which would suggest (C2H5)3N should be most basic. …
- CBSE 2024Set ANNUAL1 markMCQQ.Which of the following compounds is the most basic?(a) benzylamine (C6H5-CH2NH2)(b) aniline (C6H5-NH2)(c) p-nitroaniline (4-NH2-C6H4-NO2)(d) m-nitroaniline (3-NH2-C6H4-NO2)
›Reveal solutionSolution
Benzylamine is most basic because its nitrogen lone pair is not conjugated with the benzene ring, while all the anilines lose basicity because their -NH2 lone pair delocalises into the ring (and nitro groups withdraw electron density further).
In aniline, the nitrogen lone pair is conjugated (delocalised via resonance) into the aromatic ring. This delocalisation makes the lone pair much less available to accept a proton, so aniline is far less basic than an ordinary alkyl amine.
In benzylamine, the -CH2- group between the ring and -NH2 breaks this conjugation — the nitrogen behaves essentially like an aliphatic amine, with its lone pair fully available for protonation. This makes benzylamine considerably more basic than aniline.
The two nitroanilines are even less basic than aniline itself, because the electron-withdrawing -NO2 group further reduces electron density on nitrogen: …
- CBSE 2022Set ANNUAL1 markMCQQ.The amine having lowest pKb value is:(a) CH3NH2(b) (CH3)2NH(c) (CH3)3N(d) C6H5NH2
›Reveal solutionSolution
In aqueous solution, basicity of methylamines follows (CH3)2NH > CH3NH2 > (CH3)3N > C6H5NH2, because a balance of the electron-donating (+I) effect of methyl groups and steric hindrance to solvation (hydration) of the resulting ammonium ion determines the base strength; the secondary amine gives the best balance.
Basicity of an amine in water depends on two opposing factors:
- +I (electron-donating) effect of alkyl groups - increases electron density on N, increasing basicity as more methyl groups are added (favours 3-degree > 2-degree > 1-degree).
- Steric hindrance and reduced solvation (hydrogen bonding with water) of the ammonium cation - a more crowded ammonium ion is less stabilised by water, decreasing basicity (favours 1-degree > 2-degree > 3-degree). …
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