Reactions of Aromatic Molecules
Activating and Deactivating Groups In Electrophilic Aromatic Substitution
Last updated: February 3rd, 2023 |
Activating and Deactivating Groups in Electrophilic Aromatic Substitution
- The rate of electrophilic aromatic substitution (EAS) reactions is greatly affected by the groups attached to the ring. The more electron-rich the aromatic ring, the faster the reaction
- Groups that can donate electron density to the ring make EAS reactions faster.
- If a substituent increases the rate of reaction relative to H it is called activating. If it decreases the rate relative to H it is called deactivating. (These rates need to be measured by experiment).
- Important! Groups like OR and NR2 that seem like they should be deactivating because of their electronegativity are actually activating since they can donate a lone pair of electrons into the ring through resonance.
There’s a lot to this post, so here’s a quick index:
Table of Contents
- Activating And Deactivating Groups
- Measuring Reaction Rates Can Provide Insight Into The Mechanism
- “Activating” and “Deactivating” Groups – A Definition
- “Sigma” (σ) donors and acceptors (otherwise known as “inductive effects”)
- Pi ( π) Donors and Acceptors (often just called “Resonance”)
- Oxygen And Nitrogens Containing Lone Pairs Are Highly Activating When Bonded Directly To The Ring
- Halogens (F, Cl, Br, I) Are Deactivating
- Pi Acceptor Groups Are Strongly Deactivating
- A Table of Activating and Deactivating Groups
- Summary: What Does This Tell Us About The Mechanism Of Electrophilic Aromatic Substitution?
- (Advanced) References and Further Reading
Last post in this series we introduced electrophilic aromatic substitution. Here’s the general case:
Why is this a substitution reaction, you ask? Because we’re forming and breaking a bond on the same carbon. We form C–E (where “E” is a generic term for “electrophilic atom”) and we break C–H.
[As for the specific identity of “E”, we mentioned six key electrophilic aromatic substitution reactions in the last post (bromination, chlorination, nitration, sulfonylation, Friedel-Crafts alkylation and Friedel-Crafts acylation) that we’ll eventually dig into in detail. But not yet. ]
So if that’s the summary of what happens, the next obvious question is: how does it happen?
In other words, what’s the mechanism?
Obligatory pre-mechanism speech: You can’t determine the mechanism of a chemical reaction merely through logical deduction from first principles. Sure, you can make guesses – even good ones! But the ultimate test of a mechanistic hypothesis is how well it fits with experiment, and that typically involves a lot of lab work. What you’re taught in an introductory course is the tippy-topmost layer of snow on the iceberg. We give you the best answer, and in retrospect it looks obvious. What you don’t see is all the failure, wrong turns, and false hypotheses that happened along the path towards determining the correct mechanism. However, the mechanisms of these reactions that you will learn about weren’t obvious to most of their discoverers, who were among the brightest and best chemists of their time. Remember that.
As far as determining mechanisms is concerned, one of the best tools we have in our experimental arsenal is the ability to measure reaction rates.
By measuring the effect that slight tweaks in the experimental conditions (e.g. structure of reactant, temperature, solvent) have upon the rate, we can gather useful insights about how a reaction operates “under the hood”.
Of the parameters mentioned above, changing the substrate (reactant) is probably the most powerful way to probe a mechanism, because it allows you to tune how electron-rich (nucleophilic) or electron-poor (electrophilic) it is.
Let me show you what I mean.
Let’s arbitrarily pick one electrophilic aromatic substitution reaction: nitration.
- We know that by adding nitric acid and H2SO4, benzene can undergo nitration to form nitrobenzene (break C-H, form C-NO2)
- We can even measure the rate of this reaction at a given temperature, concentration, and solvent.
- Using the exact same experimental conditions we can then measure the rate of the reaction when toluene (methylbenzene, C6H5CH3) is used as the substrate instead of benzene.
- The nitration of toluene is 23 times faster than it is for benzene. [Ref 1]
- Using the exact same experimental conditions, we can also use trifluoromethylbenzene (C6H5CF3) as the substrate, and measure the reaction rate.
- The nitration of trifluoromethylbenzene is 40,000 times slower than it is for benzene (2.5 × 10-5).
This pattern turns out to be general for other electrophilic aromatic substitution reactions as well (chlorination, bromination, Friedel-Crafts, and others).
Let’s call a group activating that increases the rate of an electrophilic aromatic substitution reaction, relative to hydrogen. As we just saw, CH3 is a perfect example of an activating group; when we substitute a hydrogen on benzene for CH3, the rate of nitration is increased.
A deactivating group, on the other hand, decreases the rate of an electrophilic aromatic substitution reaction, relative to hydrogen. The trifluoromethyl group, CF3 , drastically decreases the rate of nitration when substituted for a hydrogen on benzene.
This definition is ultimately based on experimental reaction rate data. It doesn’t tell us why each group accelerates or decreases the rate. “Activating” and “deactivating” just refers to the effect of each substituent on the rate, relative to H.
OK then. So why might CH3 increase the rate of reaction, and CF3 decrease it?
Let’s quickly think back to what we know about alkyl groups (such as CH3) and haloalkyl groups (such as CF3), and try to address this question.
In CH3, the carbon atom is more electronegative (2.5) than hydrogen (2.2). This means that the carbon attracts a bit more than an equal share of electron-density from the covalent bond with H, resulting in a partial negative charge (δ–) on carbon and a partial positive charge (δ+) on hydrogen. This partial negative charge is then available to be donated to an adjacent atom. Hence, we tend to think of CH3 as an electron-rich species; an electron–donor.
In CF3 the electrons are pulled in the opposite direction. Three highly electronegative (4.0) fluorine atoms pull electron density away from the carbon atom (2.5), resulting in a partial positive charge (δ+) on carbon. Rather than donate electron density, the carbon tends to accept (pull away) electron density from adjacent atoms (this is the familiar inductive effect) We generally consider CF3 to be an electron-poor species; an electron-acceptor.
Since these inductive effects operate solely through single bonds (“sigma”, or σ bonds) this behaviour is sometimes called “sigma donation” (as for CH3) or “sigma accepting” (for CF3).
So it seems like a good hypothesis that
- activating groups are electron-donating (relative to H), and
- deactivating groups are electron-withdrawing (relative to H)
Sigma donation and acceptance helps us to understand the effect of alkyl groups on electrophilic aromatic substitution. So what about other functional groups? What effect might, say, a hydroxyl group have on the rate of nitration?
Quiz time. Do you think –OH would be activating (increase the rate) or deactivating (decrease the rate) for electrophilic aromatic substitution (such as nitration)? Guessing is OK!
Based on what we just said, it’s fully understandable if you said, “deactivating”. After all, oxygen is highly electronegative (3.4) and through induction, pulls away electron density through the bond. In other words, it’s a sigma-acceptor.
The fact is, however, that OH greatly accelerates the rate, orders of magnitude more than CH3 does. In fact I couldn’t find good rate data comparing OH to CH3 because in the case of -OH, the reaction is what’s called, “diffusion controlled”. That roughly means, “as soon as the reactant comes in contact with the electrophile, a reaction occurs.” In other words, the –OH group is highly activating.
Clearly, something else must be going on here besides the inductive effect of oxygen!
6. Oxygen And Nitrogens Containing Lone Pairs Are Highly Activating When Bonded Directly To The Ring
As we saw in our chapter way back on resonance, hydroxyl groups are excellent pi donors. The lone pairs on the oxygen atom can form a pi bond with an adjacent atom containing an available p-orbital.
This donation effect (or “resonance”) must outweigh electron-withdrawal via inductive effects, otherwise we’d observe that hydroxyl groups are deactivating.
The same is true for nitrogen groups with lone pairs, such as amines and amides (below).
[One measure of the importance of pi-donation in the activating nature of amines is seen in their behavior under strongly acidic conditions. If the nitrogen lone pair is either protonated with strong acid or undergoes a substitution reaction to form NR3+ , pi-donation is impossible and the group becomes strongly deactivating (see table below). ]
Not all groups capable of pi donation are activating groups. For example, halogens (F, Cl, Br, I) tend to be deactivating. The rates of electrophilic aromatic substitution reactions on fluorobenzene, chlorobenzene, bromobenzene, and iodobenzene are all slower than they are for benzene itself. In these cases, inductive effects (“sigma accepting”) would appear to have a greater effect on the rate than any pi-donation from the lone pairs. [pi donation < sigma acceptance]. [Why?]
A good rule of thumb for pi-donation ability is the basicity of the lone pair. Amines tend to be better bases than oxygens, which are far better bases than halogens.
Alright. What if electrons flow in the opposite direction? Is there an opposite of “pi donor” ?
Yes! As you may already know, the opposite of a “pi-donor” is a “pi acceptor”. Certain functional groups can accept, rather than donate, a pi bond from the ring, resulting in a new lone pair on a substituent atom. Examples are NO2, carbonyl groups (C=O), sulfonyl, cyano (CN) among others. These groups are universally deactivating, slowing the rate of electrophilic aromatic substitution.
In terms of resonance, one can draw a pi bond from the aromatic ring forming a pi bond with the atom bound to the ring, resulting in formation of a new lone pair on an electronegative atom on the substituent. Note how this results in a positive charge on the ring!
So how do we keep all of these factors straight?
This is an example of why I say that resonance is the most important key concept to review for Org 2. In the section on aromatic chemistry it comes back with a vengeance.
Now seems like the right time to present a big table of activating and deactivating groups. It’s hard to rank exactly by power since the effect is averaged over several types of reactions.
I would suggest five main “buckets”, below:
- Nitrogen and oxygens with lone pairs – amines (NH2, NHR, NR2), phenol (OH) and its conjugate base O– are very strong activating groups due to pi-donation (resonance). Alkoxy, amide, ester groups less strongly activating.
- Alkyl Groups – (with no electron withdrawing groups). Moderately activating through inductive effect.
- Halogens – Moderately deactivating. Electron withdrawing (highly electronegative) nature outweighs donation of electron density through a lone pair.
- Atoms with pi-bonds to electronegative groups – Strongly deactivating. NO2, CN, SO3H, CHO, COR, COOH, COOR, CONH2. All pi-acceptors.
- Electron withdrawing groups with no pi bonds or lone pairs – Strongly deactivating. CF3, CCl3, and NR3(+). Pure inductive effect.
Once you remember the somewhat counterintuitive fact that O and N-bonded functional groups with lone pairs are activating, and halogens are deactivating, the rest is fairly straightforward.
One final word. Our table of “activating” and “deactivating” groups turns out to be a little bit like a pKa table. How? We can evaluate several factors that have an impact on pKa, but the ultimate test of which factor is more important is experimental measurement of an equilibrium constant. Likewise, with activating and deactivating groups, we can identify factors which may or may not make a certain group activating or deactivating, but in the end, its position on the chart comes down to experimental measurements of reaction rates.
OK. So what does all of this tell us?
Since the rate is so sensitive to whether the group is electron donating or electron withdrawing (“electronic effects”, as organic chemists might quickly summarize it) it would suggest that the rate determining step is the formation of a fairly unstable electron-poor species, such as a carbocation.
Recall CH3 and CF3. You may recall that the order of carbocation stability (tertiary > secondary > primary) is due to the fact that carbocations are stabilized by adjacent alkyl groups (such as CH3), and, conversely, are destabilized by adjacent electron withdrawing groups (like CF3).
Likewise, carbocations are stabilized by adjacent atoms that can donate lone pairs (e.g. O and N) through resonance, and destabilized by pi acceptors such as C=O, NO2, and so on.
A likely first step would be something like this:
We’ll go into the full mechanism of electrophilic aromatic substitution in the next post, but will fill in additional detail in a bonus topic below.
1. [Advanced] No deuterium isotope effect is observed in electrophilic aromatic substitution
In electrophilic aromatic substitution a C-H bond is broken. One way to probe the mechanisms of reactions that involve C-H bond cleavage is to use deuterium (D) labelling. In reactions where C-H bond breakage is a rate-determining step (e.g. E2 elimination) a C-H bond can break up to 6-7 times faster than a C-D bond. This is called a deuterium isotope effect and it is measurable.
Electrophilic aromatic substitution reactions have no significant deuterium isotope effects. [Note] This strongly suggests that C-H bond breakage is not the rate determining step.
2. Carbocation intermediates have been isolated that strongly support the proposed mechanism
Here’s a species that’s been observed when 1,3,5-trimethylbenzene (mesitylene) is treated with ethyl fluoride and boron trifluoride at –80°C (this is a Friedel-Crafts alkylation reaction, by the way).
The carbocation intermediate (called an “arenium ion” or “Wheland intermediate” was isolated as a white solid with melting point –15°C, and analyzed by NMR spectroscopy.
As Eric Jacobsen might say: “mechanisms can never be proven, but….” . (this pretty much seals the deal). We’ll go into in more detail in the next post.
Note 2. Why? Interestingly, fluorine is the most activating of the halogens. The reason is likely that the overlap of the lone pair in the fluorine 2p orbital with the p orbital on carbon is much better (resulting in a stronger pi-bond) than is donation with the 3p (and higher) p orbitals of chlorine, bromine, and iodine.
Note 3. Actually a white lie; some electrophilic aromatic substitution reactions do have very small deuterium isotope effects, but we’re not touching that topic, nosiree. [partitioning effects, see March’s Advanced Organic Chemistry, 5th ed., p. 679]
As mentioned, this topic is useful for all types of EAS reactions – Friedel-Crafts alkylation/acylation, halogenation, nitration, etc.
- —The chlorination of anilides. The directing influence of the acylamido-group
Kennedy Joseph Previté Orton and Alan Edwin Bradfield
J. Chem. Soc. 1927, 986-997
An early paper discussing the ortho/para product distribution obtained by electrophilic chlorination of anilides (generally 65% para/35% ortho). Unfortunately this paper does not have data comparing the rate of chlorination to benzene.
- Kinetics and mechanism of some electrophilic benzene substitution reactions
Alan E. Bradfield and Brynmor Jones
Faraday Soc. 1941, 37, 726-743
Table I in this paper contains partial rate factors for nitration of benzene and related compounds. Chlorobenzene and bromobenzene are around 1-3% as reactive as benzene, whereas ethyl benzoate is significantly deactivated – it is around 0.1-0.2% as reactive as benzene! Toluene is 40-50 times as reactive as benzene.
- The kinetics of aromatic halogen substitution. Part IX. Relative reactivities of monosubstituted benzenes
P. W. Robertson, P. B. D. de la Mare, and B. E. Swedlund
J. Chem. Soc. 1953, 782-788
Pg. 783 in this paper contains data for reaction rates of halogenation of various benzene derivatives. This spans the gamut of extreme activating substituents (N,N-dimethylaniline is 1018 times more reactive than benzene!) and deactivating substituents (nitrobenzene is 10-6 times less reactive than benzene).
- The influence of the methoxyl group in aromatic substitution
P. B. D. de la Mare and C. A. Vernon
J. Chem. Soc. 1951, 1764-1767
This paper examines the effect of -OMe in electrophilic aromatic substitution (e.g. anisole and related compounds vs. benzene). Overall, anisole is 108 times more reactive than benzene, and as a result, o/p selectivity in reactions is very low.
- Rates of Bromination of Anisole and Certain Derivatives. Partial Rate Factors for the Bromination Reaction. The Application of the Selectivity Relationship to the Substitution Reactions of Anisole
Leon M. Stock and Herbert C. Brown
Journal of the American Chemical Society 1960, 82 (8), 1942-1947
This paper is a more rigorous study of the bromination of anisole by Nobel Laureate Prof. H. C. Brown. The o/p selectivity of anisole is actually rather high – bromination gives 1.6% o– and 98.4% p-bromoanisole. The relative reaction of anisole:benzene is also measured to be 1.79 x 109:1.00. This paper also shows that s+ values (electrophilic Hammett constants) measured this way are comparable to Hammett values measured through other methods, and that the Hammett values also provide a good measure of how a substituent will effect EAS reactions as well.
- —Influence of directing groups on nuclear reactivity in oriented aromatic substitutions. Part II. Nitration of toluene
Christopher Kelk Ingold, Arthur Lapworth, Eugene Rothstein, and Denis Ward
J. Chem. Soc. 1931, 1959-1982
This is the first paper to introduce the term ‘partial rate factor’ (usually denoted by fp, fo, fm) to denote the amount by which a specific position on a substituted benzene may be more or less reactive compared to benzene. Table IV shows in this paper that toluene can be anywhere from 1.2 – 10 times more reactive than benzene.
- Effects of Alkyl Groups in Electrophilic Additions and Substitutions
COHN, H., HUGHES, E., JONES, M. and PEELING, M. G.
Nature 1952, 169, 291
This paper has data comparing the nitration of t-butylbenzene and toluene. T-butylbenzene is much more p-directing than toluene (79.5% para for t-butylbenzene vs. 40% para for toluene), which is likely due to sterics (ortho approach is blocked by the bulkier t-butyl group).
- The transmission of polar effects through aromatic systems. Part II. The nitration of benzyl derivatives
J. R. Knowles and R. O. C. Norman
J. Chem. Soc. 1961, 2938-2947
J. R. Knowles went on to become a Professor at Harvard, specializing in enzymology. The knowledge of kinetics that one gets from doing physical organic chemistry is applicable in a wide variety of areas! In this paper, Table 2 is interesting, and shows that the empirical reactivity difference between toluene and benzene is 25x, which is what is commonly found in textbooks today. T-butylbenzene is less reactive than toluene, but still 15x more reactive than benzene.
- Influence of directing groups on nuclear reactivity in oriented aromatic substitutions. Part IV. Nitration of the halogenobenzenes
Marjorie L. Bird and Christopher K. Ingold
J. Chem. Soc. 1938, 918
Table I in this paper shows that overall, chlorobenzene and bromobenzene are around 2-3% as reactive as benzene towards nitration under a wide variety of conditions.
- Some aspects of the nitration of the mononitrotoluenes
J. G. Tillett
J. Chem. Soc. 1962, 5142-5148
Pg. 5148 in this paper shows that in nitrotoluenes, the deactivating nature of nitro wins out over the activating nature of the methyl group. Interestingly, in m-nitrotoluene, the meta position to the nitro group is less reactive than the other positions, due to resonance effects. Note that these compounds are also precursors to the common explosive TNT!
- Substituent effects of positive poles in aromatic substitution. Part I. The nitration of the anilinium ion in 90—100% sulphuric acid
Madeline Brickman and J. H. Ridd
J. Chem. Soc. 1965, 6845-6851
- Substituent effects of positive poles in aromatic substitution. Part II. The nitration of N-methylated anilinium ions
Madeline Brickman, J. H. P. Utley, and J. H. Ridd
J. Chem. Soc. 1965, 6851-6857
In contrast to aniline, which is very reactive in EAS compared to benzene, the anilinium ion (which is easily formed in acidic media) is deactivated. As the acidity of the medium increases, the amount of meta product obtained from nitration of aniline increases, indicating that the reaction is proceeding via the anilinium ion (PhNH3+). Reaction rates also decrease with increasing acidity, as the amount of free aniline available in the reaction gets lower and lower.
- Aromatic substitution. 53. Electrophilic nitration, halogenation, acylation, and alkylation of (.alpha.,.alpha.,.alpha.-trifluoromethoxy)benzene
George A. Olah, Takehiko Yamato, Toshihiko Hashimoto, Joseph G. Shih, Nirupam Trivedi, Brij P. Singh, Marc Piteau, and Judith A. Olah
Journal of the American Chemical Society 1987, 109 (12), 3708-3713
The -OCF3 substituent is not commonly encountered in undergraduate chemistry courses, but is used in medicinal chemistry. This paper by Nobel Laureate Prof. George A. Olah and his wife Judith, covers the directing effects and reactivity of PhOCF3 in a variety of EAS reactions. Overall, PhOCF3 is around 3-10% as reactive as benzene in EAS (see Tables VI-VIII).
- A Quantum Mechanical Investigation of the Orientation of Substituents in Aromatic Molecules
G. W. Wheland
Journal of the American Chemical Society 1942, 64 (4), 900-908
This discusses the structure of the arenium ion that gets formed in EAS reactions, also known as the s-complex or Wheland intermediate, after the author here who first proposed it.
- Isolation of the Stable Boron Trifluoride – Hydrogen Fluoride Complexes of the Methyl-benzenes ; the Onium Salt (or σ-Complex) Structure of the Friedel-Crafts Complexes
OLÁH, G., KUHN, S. & PAVLÁTH, A.
Nature 1956, 178, 693–694
- The Benzotrifluoride–Nitryl Fluoride–Boron Trifluoride Complex
OLÁH, G., NOSZKÓ, L. & PAVLÁTH, A.
Nature 1957, 179, 146–147
- Isolation of the Stable Boron Trifluoride-ethylfluoride and Boron Trifluoride-formylfluoride Complexes of the Methylbenzenes: Mechanism of the Friedel–Crafts Reactions
OLÁH, G., KUHN, S.
Nature 1956, 178, 1344–1345
These papers by Nobel Laureate Prof. G. A. Olah describe the isolation and characterization of the intermediate ions (‘Wheland intermediates’) from various electrophilic aromatic substitution reactions – alkylation, nitration, and even protonation (by HBF4!)
- A Quantitative Treatment of Directive Effects in Aromatic Substitution
Leon M. Stock, Herbert C. Brown
Phys. Org. Chem. 1963, 1, 35-154
This is a very comprehensive review for its time, summarizing work on directing effects in EAS (e.g. determining which groups are o/p-directing vs. meta-directing, and to what extent they direct/deactivate).
- Stable carbocations. CLXX. Ethylbenzenium ions and the heptaethylbenzenium ion
George A. Olah, Robert J. Spear, Guisseppe Messina, and Phillip W. Westerman
Journal of the American Chemical Society 1975, 97 (14), 4051-4055
This paper discusses the characterization of benzenium ions, which are intermediates in EAS, and the characterization of the heptaethylbenzenium ion, which is a stable species because it lacks a proton and therefore eliminates with difficulty.
- The Anomalous Reactivity of Fluorobenzene in Electrophilic Aromatic Substitution and Related Phenomena
Joel Rosenthal and David I. Schuster
Journal of Chemical Education 2003, 80 (6), 679
A very interesting paper, suitable for curious undergrads, and discusses something that most practicing organic chemists will know empirically – fluorobenzene is almost as reactive as benzene in EAS or Friedel-Crafts reactions, which is counterintuitive when one considers electronic effects.