Alkylation of Amines (Sucks!)
Last updated: November 1st, 2022 |
Why Alkylation Of Amines (aka “The Williamson Ether Synthesis, But For Amines” ) Usually Doesn’t Pan Out
- Making a more-substituted amine from a less-substituted amine through treatment with an alkyl halide often fails, because the product amine is more nucleophilic than the starting amine.
- In some cases this is desired, as in the formation of alkylammonium salts with an excess of alkyl halide (e.g. CH3I)
- In other cases, the best approach to making a more substituted amine from a less substituted amine is generally reductive amination.
Table of Contents
- “The Williamson Ether Synthesis, But For Amines” : Why Does This Reaction Suck?
- The Runaway Train of Amine Alkylation, Step 1: SN2
- Step 2: Alkylation Is Followed By An Acid-Base Reaction…
- …Liberating An Amine That Is A Better Nucleophile: Step 3: A Second SN2
- Step 4: Another Acid-Base Reaction Makes An Even Better Nucleophile
- The Runaway Train Continues
- The Reaction Tends To Stop At Tertiary Amines. Usually.
- Summary: Alkylation Of Amines Generally Sucks. Here Are Some Workarounds
- Notes, plus “Exhaustive Methylation”
- (Advanced) References and Further Reading
1. Why Does This Reaction Suck?
Trends in the basicity of amines provide a classic example of why chemistry is so interesting; it’s deciphering the delicate trade-offs between various general factors in specific cases that gives chemists a buzz. The miraculous starts looking obvious.
– The Curious Wavefunction (Ash Jogalekar)
Today, let’s talk about how to make amines. It’s not as straightforward as you might think.
See if you can fill in the blank in the following skill-testing question:
Let’s walk through the thought process. We need to form a C-N bond. The N of NH3 has a lone pair and is a good nucleophile. So, much like the Williamson ether synthesis, maybe we can use an alkyl halide like ethyl bromide (CH3CH2Br) and boom! done.
It doesn’t quite turn out that way. In the words of the scientist who investigated this thoroughly:
“The interaction of ethyl bromide and ammonia… conduces largely to the formation of triethylamine”.
[ref: Werner, J. Chem. Soc. 1918, p. 899]
Formation of a primary amine through alkylation of ammonia turns out to be a pretty low-yielding reaction. (For reasons of economy, we generally want to use reactions that form one dominant product in high yield to avoid tedious separations: this doesn’t qualify.)
This is part of the fun* of learning organic chemistry. Just when you think you might have things figured out, along comes a curveball.
Why does this reaction. for lack of a better word, suck?
2. The Runaway Train of Amine Alkylation, Step 1: SN2
Let’s look at the first reaction that would happen the moment that a solution of ammonia is combined with ethyl bromide: nucleophilic substitution (via the SN2 mechanism)
3. Step 2: Alkylation Is Followed By An Acid Base Reaction
So far so good. We’ve formed our C-N bond. Since the reaction is in excess ammonia, an acid-base reaction can then lead to the neutralization of at least some of the ammonium salt, yielding us our neutral primary amine.
So now we have the primary amine. We’re done, right?
Not so fast. See, relative to substitution reactions, acid-base reactions are fast, so this deprotonation event will occur before the first substitution reaction has consumed all of the remaining ethyl bromide.
That means that ethylamine will be present in the same flask with ethyl bromide.
4. Step 3: The Acid-Base Reaction Liberates An Amine Nucleophile That Is Even Better Than The Starting Amine
Well, ethylamine is itself a good nucleophile. In fact, it’s an even better nucleophile than ammonia itself, because of the electron-donating alkyl group [Link: 5 factors that affect the basicity of amines]
How much better? If we use pKaH as a proxy for nucleophilicity (reasonable, since steric hindrance isn’t a factor here) we have a pKaH of 10.7 for ethylamine versus 9.2 for NH3. That’s about 101.5 = 30 times more nucleophilic.
The ethylamine created by the first SN2 will start gobbling up the ethyl bromide… instead of NH3!
We’ve created a monster!
Even if we try to stack the deck with (say) a 15-fold excess of NH3, the reaction of ethylamine will still be faster by a factor of (30/15) = 2. [That’s what Werner did, above; the yield of EtNH2 was 34% under those conditions, versus 11% for just 1 equiv of NH3.]
5. Step 4: Another Acid-Base Reaction Makes An Even Better Nucleophile
Now we have the diethylammonium product in the presence of excess base, which will lead to at least some formation of diethylamine.
You know what that means? Another nucleophile has been produced that will compete with NH3 for the remaining ethyl bromide.
How does the nucleophilicity compare to ammonia and ethylamine?
The pKaH of diethylamine is about 11.0, making it slightly more nucleophilic than ethylamine!
6. The Runaway Train Continues
Diethylamine, being a stronger nucleophile than both ammonia and ethylamine, will react faster with the remaining ethyl bromide than either of those two species. This will form triethylammonium bromide, which can then be deprotonated (using any one of the amine bases in solution) to form neutral triethylamine.
Now we have three nucleophilic amine species all swimming around in solution at the same time, before all of our ethyl bromide has been consumed.
This soup containing multiple amine products is the kind of reaction that my friend Jeff would describe in his lab notebook as a “BFM”. (The “B” is for “big”, and the “M” is for “mess”….)
7. The Reaction Tends To Stop At Tertiary Amines…
The “runaway train” usually stops at the tertiary amine stage. In this specific case, the pKaH of triethylamine is 10.75, a little less than diethylamine. [Recall that pKaH refers to basicity, not nucleophilicity: the basicity of NEt3 is attenuated here due to the lowered solubility of the conjugate acid in water. [more here]. ]
The nucleophilicity of triethylamine is less than that of diethyl amine largely because the triethylamine nitrogen is tertiary, which will increase steric hindrance and slow down the reaction rate.
For this reason, formation of tertiary amines from secondary amines via alkylation is thus, for the most part, exempt from our broad “amine alkylation is crap” statement.
8. Summary: Alkylation of Amines Generally Sucks. Here Are Some Workarounds
Otherwise, workarounds must be used. There are plenty. Azides are good nucleophiles for example, and they can be alkylated without incident and reduced to amines afterwards. The Gabriel Synthesis is another workaround.
What about our skill-testing question from the top of the article?
Here’s a reaction that most organic chemists would consider to be the best general way to make amines: a reaction called reductive amination.
Here’s a little sneak preview.
We’ll talk about how this reaction works in the next post , on reductive amination.
Note 1. Alkylation of ammonia mostly stopped at the tertiary amine stage.
Although tertiary amines tend to be less nucleophilic than secondary amines, they are still nucleophiles, and when treated with excess alkyl halide under forcing conditions they can be converted to quaternary ammonium salts.
The best example of this is with methyl iodide, in a reaction called exhaustive methylation. Recall that methyl halides are the fastest-reacting alkyl halides in SN2 reactions due to their low steric hindrance.
Treatment of amines with a large excess of methyl iodide leads to their quaternary ammonium salts. As we’ll see in a future post, these quaternary ammonium salts can behave as excellent leaving groups in elimination reactions (and, rarely, substitution reactions) to give alkenes, particularly in the Hofmann elimination.
(Advanced) References and Further Reading
- —The preparation of ethylamine and of diethylamine
Emil Alphonse Werner
J. Chem. Soc. Trans. 1918, 113, 899-902
An early report on the synthesis of alkylamines by alkylation of ammonia with ethyl bromide, and the second paragraph begins with “This is a faulty procedure, since it conduces largely to the formation of the less useful triethylamine, with consequent loss in the yields of the primary and secondary bases”.
- Cesium Effect: High Chemoselectivity in Direct N-Alkylation of Amines
Ralph Nicholas Salvatore, Advait S. Nagle, and Kyung Woon Jung
The Journal of Organic Chemistry 2002, 67 (3), 674-683
The selective monoalkylation of amines is possible, provided you know how.
- Efficient and selective N-alkylation of amines with alcohols catalysed by manganese pincer complexes
Saravanakumar Elangovan, Jacob Neumann, Jean-Baptiste Sortais, Kathrin Junge, Christophe Darcel & Matthias Beller
Nature Communications 2016, 7:12641
- Selective Synthesis of Secondary and Tertiary Amines by Reductive N‐Alkylation of Nitriles and N‐Alkylation of Amines and Ammonium Formate Catalyzed by Ruthenium Complex
Iryna D. Alshakova, Dr. Georgii I. Nikonov
ChemCatChem 2019, 11 (21), 5370-5378
Both papers are on essentially the same reaction. The mechanism of these reactions shows that it is basically a ‘one-pot’ reductive amination. The alcohol is oxidized in situ and an excess of alcohol serves as a reductant.
- Aqueous N-alkylation of amines using alkyl halides: direct generation of tertiary amines under microwave irradiation
Yuhong Jua and Rajender S. Varma
Green Chem., 2004, 6, 219-221
This paper demonstrates that alkylation of secondary amines yields tertiary amines, obviously. But more importantly, quaternary ammonium salts are only formed with difficulty; this paper does not report any quaternary ammonium salt formation even after extended microwave heating of a secondary amine with excess alkyl halide.
5 thoughts on “Alkylation of Amines (Sucks!)”
Dr.James greetings from my side.I have read lot of articles by you on different topics of organic chemistry and i really appreciate the way you make the students understand organic chemistry like a breeze.
I also refer your blogs to my students when they are stuck with some really difficult topics like complex mechanisms of the reactions and other topics.
Thank you very much, this is the only article through which I understood the above reaction.
This [site](https://www.chemguide.co.uk/organicprops/haloalkanes/nh3.html) says primary amine to be the major product in excess of ammonia. Is it wrong?
Werner, J. Chem. Soc. 1918, p. 899 tried a 16:1 ratio of NH3 to ethylamine and got 34% yield of the amine. Maybe if you used a 50:1 or 100:1 ratio of NH3 to alkyl halide, then it would have a higher yield. But that’s starting to get to be a fairly impractical process.
Dear Dr Ashenhurst,
I was wondering whether the link you added about why tertiary amines are less basic than secondary amines paints a full picture regarding the formation of a quaternary ammonium salt. Whereas one could rightly make the argument that triethylamine is slightly less basic than diethylamine in an aqueous medium, the SN2 reaction could be performed using a polar solvent that isn’t water, right? So couldn’t the comparitively more polar nature of the pentacoordinate transition state and ionic nature of the subsequent salt be stabilised in a sufficiently polar solvent that isn’t water? I ask this because I was taught in my second year of undergrad that the rate of reaction of n-Pr3N + MeI (SN2) could be increased by increasing the polarity of the solvent used due to the reason the increased polarity of the TS compared to the reactants.