# Justifying the tremendous −I effect of trimethylammonium group by molecular orbital theory

The $$\ce{-[NMe3]+}$$ group is ranked almost at the first position in the −I effect series, which is often given at the very beginning of the teaching of general organic chemistry.

I know this can be justified by hyperconjugation, but I am interested in a rigorous justification by molecular orbital theory.

• This group has a positive charge, any molecular orbital effect will be negligible compared to that. – Martin - マーチン Aug 1 '18 at 16:02

Powerful electron withdrawing substituents, like $$\ce{-NO2}$$ can be interpreted as having a large effect on the $$\pu{\pi}$$-system of an aromatic ring. Resonance structures can be drawn that put a positive charge at the ortho and para positions and put the electron out in the nitro group, on an oxygen.

This must be adjusted for $$\ce{-N(CH3)3+}$$, because it has no $$\pu{\pi}$$ electrons, and we can't draw structures with a double bond between the nitrogen and the ring carbon. It works thru a very strong $$\ce{-I}$$ effect. However, if we use the concept of hyperconjugation, and donate a $$\pu{\pi}$$ electron from the ring to the nitrogen and then a methyl group (making it $$\ce{-CH3}$$), unbounded to any other atom, we can imagine the oxygens in the picture replaced with methyls and will get the same distribution of charge in the ring: a positive charge at the ortho and para positions. This will result in meta substitution if any reaction does occur.

For $$\ce{-N(CH3)3}$$, it's like hyperconjugation in reverse. Interestingly, while $$\ce{-N(CH3)3}$$ makes it very difficult to substitute, and always meta, $$\ce{-NH3+}$$ is only a weak meta director.

Reference

1. Advanced Organic Chemistry, L.F. Fieser, 1961, p628
• Thanks for the edit help! – James Gaidis Jun 10 '20 at 14:41

The question is so good that maybe it deserves another correct answer. While my answer above attempts to answer using the criterion mentioned by user57048 (hyperconjugation), hyperconjugation is generally a small effect, but the $$-I$$ effect of $$-N(CH3)3+$$ is so large that maybe an entirely different approach could be appealing - not that you could necessarily distinguish between them.

The inductive effect is not in question, and does not need hyperconjugation to explain it. But the $$meta$$ directing effect, without the possibility of a double bond between carbon #1 on the ring and the nitrogen presents a problem. The reference I used in my first answer also discusses this at length, but I'd like to expand it a bit.

The question mentions the $$-N(CH3)3)+$$ group, but we need one more thing: an aryl group attached to the nitrogen. And we need one more thing for explaining the $$meta$$ direction: the transition state. This is what is brought up in the discussion by Fieser, but without using the specific words $$transition state$$. While in the example of the $$-NO2$$ group, a charge separation is generated such that it can minimize the $$pi$$ electron density on the $$ortho$$ and $$para$$ positions, with $$-N(CH3)3+$$, we only have to consider the inductive effect as far as carbon #1. The incoming electrophile carries the positive charge that resonates around the ring and directs it to the $$meta$$ positions because attaching to the other positions puts a positive charge on the #1 carbon, which would be highly unfavored because it places two positive charges next to each other.

The question seems to have been of long standing. The idea of aronium ion intermediates was put forth by Pfeiffer and Wizinger. The structures shown as aronium ions $$a$$ and $$b$$ in the picture are the ones that do not lead to product; $$c$$ leads to product, and would seem to be a transition state (or close to it) rather than a true intermediate.

Reference: P. Pfeiffer and R. Wizinger, Ann., 461, 132 (1928)

$\ce{Me}$ is a pushing group which pushes electron towards the nitrogen atom. As a result electron concentration is towards the nitrogen atom.

The anti bonding electrons of nitrogen are shifted to the bonding orbital of nitrogen. This is because the bonding orbitals are closer to the more electronegative atom which in this case is nitrogen.

So nitrogen becomes more "electron hungry" and in order to stabilize itself tries to pull electron towards itself and thereby renders a -I effect.

• Will somebody explain what i have done wrong in this answer. – Pole_Star Jan 4 '18 at 6:19
• This is super hand wavy and probably not what the OP wanted. – ringo Jul 2 '18 at 13:34
• Relative to what you did wrong: methyl does indeed push; there are two methyls pushing toward the N in -NMe2. However, when you add the third methyl (Me+) to make NMe3+, it becomes an electron withdrawer, and this FAR outweighs the two little electron pusher methyls. They all average out, pulling on the N, which then is a big puller from whatever it is connected to. – James Gaidis Jun 5 '20 at 14:11
• @JamesGaidis could you please write an answer for this. – user57048 Jun 8 '20 at 14:30