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Free Radical Reactions

By James Ashenhurst

Allylic Bromination

Last updated: February 27th, 2020 |

Allylic Bromination and Benzylic Bromination: What Is It,  And How Does It Work?

In previous posts on radicals, we’ve seen how bromine can selectively react with tertiary C-H bonds (bond strength 93 kcal/mol) over secondary (96 kcal/mol) and primary (100 kcal/mol) C–H bonds.

If you recall that bond dissociation energies are a good guide for predicting radical stability, then you won’t be surprised to learn that “benzylic” and “allyllic” C–H bonds can also be brominated selectively. These C-H bonds are particularly weak because the radical formed through the homolytic  breaking of C-H  is stabilized by resonance.

Table of Contents

  1. Allylic and Benzylic Bromination: Examples
  2. Free Radicals Are Stabilized By Resonance
  3. The Mechanism of Benzylic Bromination With Br2 and Light/Heat
  4. Br2 Is Not An Appropriate Reagent For Allylic Bromination Since It Forms Vicinal Dibromides
  5. Using N-Bromo Succinimide (NBS) Ensures A Low Concentration Of Br
  6. Notes
  7. (Advanced) References and Further Reading

1. Allylic and Benzylic Bromination: Examples

So what is allylic and benzylic halogenation, anyway?  Here’s an example of each.

Take toluene and treat with either Br2 in the presence of light, as per this procedure, or N-Bromosuccinimide (NBS) in the presence of a radical initiator + heat (or  light) and one of the benzylic C–H bonds is replaced with C–Br.

(Note that the “benzylic” position is the carbon attached to the benzene ring; the C-H bonds of the  benzene ring itself are the “phenyl” C-H bonds). 


Here’s an example of the allylic bromination of propene, this time using NBS and peroxides (or heat)


We’ve spent a considerable amount of time discussing the stability of free radicals, particularly that primary radicals are particularly unstable.

So what’s different in this case? And what’s this “NBS” stuff?

2. Free Radicals Are Stabilized By Resonance

Recall that free radicals are stabilized by resonance, and bond dissociation energies (BDE’s) aka “bond strengths” measure homolytic bond cleavage.

So the methyl  groups (above) aren’t ordinary methyl groups – the resulting radicals are greatly stabilized by resonance!

Therefore when we look at bond dissociation energies for benzylic and allylic C–H bonds it should not be surprising to find that these bond strengths  are quite weak  (89-90 kcal/mol for a primary allylic or benzylic radical) relative to tertiary C-H bonds (93 kcal/mol).


So how might allylic or benzylic bromination work?

3. The Mechanism of Benzylic Bromination With Br2 and Light/Heat

For benzylic bromination, hopefully imagining the mechanism will be straightforward: after initiation (by heat or light), bromine radical then breaks the C-H bond (forming the benzylic radical) [propagation step #1] and the benzylic radical attacks Br2 to re-generate bromine radical [propagation step #2]. These two steps repeat until the concentration of Br2 runs low, whereupon radical chain termination will occur.

[See Initiation, Propagation, Termination]


4. Br2 Is Not An Appropriate Reagent For Allylic Bromination Since It Forms Vicinal Dibromides

Let’s turn to allylic bromination. Do you see any reason why treating the molecule below with Br2 might lead to problems?


You might recall that alkenes react with Br2 to form vicinal dibromides, and that is in fact exactly what would occur if we were to just dump in 1 equivalent of Br2 with an alkene.

At issue here is the fact that we have 1 equivalent of Br2 swimming around, of which only a small proportion at any given time will exist as bromine radical [due to the initiation step].

How might we solve this problem and favour the radical substitution over the dibromination?

Imagine, if you will, we had a very low concentration of Br2. If the concentration of Br2 is kept low, not only will the rate of dibromination be lower, the relative concentration of bromine radical relative to Br2 will increase. Therefore, the rate of C-H abstraction relative to dibromination will increase, which will allow our allylic bromination product to be formed in a higher yield. *

Of course, this creates a new question: how do we generate a low, constant concentration of Br2?

5. Using N-Bromo Succinimide (NBS) Ensures A Low Concentration Of Br

As it turns out, there’s a way. If the bromonium ion source N-bromosuccinimide (NBS) is present with a trace amount of acid (HBr), HBr will react with NBS to give succinimide and Br2.**

Since one equivalent of HBr generates one equivalent of Br2,  Br2 will be generated only after the completion of Propagation Step #1.*** This keeps the concentration of Br2 low and allows the free-radical reaction to out-compete the alkene addition reaction.



In all other respects the allylic bromination reaction is identical to the benzylic bromination reaction mechanism shown above. However in *some* situations there is an extra twist, which we will briefly discuss in the next post.

Next Post: Allylic Rearrangement


*  If this explanation sounds somewhat unsatisfactory, you’re on to something. After all, doesn’t this decrease the concentration of Br• as well? One additional complication is that theoretical studies show strong evidence for a termolecular rate determining step in formation of the bromonium ion (that is, involvement by the alkene and two molecules of Br2). Decreasing the concentration of Br2 would therefore vastly decrease the rate of bromonium ion formation (and thus dibromination) relative to free radical halogenation.

** As it happens, NBS which has been left out for awhile will usually be contaminated with trace HBr (as well as Br2, which gives it a yellow or orange colour). For this reason if doing a radical reaction with NBS it’s common to avoid recrystallizing it before use, as it will remove the trace acid that jump starts the reaction in the first place.

*** As long as the initial concentration of HBr is low (i.e. it is used as a catalyst)

(Advanced) References and Further Reading

  1. The Peroxide Effect in the Addition of Reagents to Unsaturated Compounds. I. The Addition of Hydrogen Bromide to Allyl Bromide
    S. Kharasch and Frank R. Mayo  Journal of the American Chemical Society 1933 55 (6), 2468-2496
    DOI: 10.1021/ja01333a041
    This paper by the legendary chemist M. S. Kharasch (U. Chicago) and student F. Mayo, describes the first observation of free-radical addition of bromine to allylic systems. The paper also shows how Mayo exhaustively tested a lot of reaction conditions before observing the effect that oxygen had on the reactivity (O2 can create Br radicals from Br2).
  2. The evolution of free radical chemistry at Chicago
    Frank R. Mayo
    Journal of Chemical Education 1986 63 (2), 97
    DOI: 1021/ed063p97
    For those interested in the history of science, this retrospective by Mayo tells the story of how he and Kharasch discovered the ‘peroxide effect’ and thereby a new area of organic chemistry. M. S. Kharasch also founded the Journal of Organic Chemistry in order to expedite publishing his work, since he felt JACS was too slow!
  3. Mechanisms of Benzylic Bromination
    Glen A. Russell, Charles. DeBoer, and Kathleen M. Desmond
    Journal of the American Chemical Society 1963 85 (3), 365-366
    DOI: 1021/ja00886a040
    Benzylic bromination follows the same mechanism as allylic bromination, as this paper explains.NBS (N-Bromosuccinimide) is a convenient reagent for free-radical bromination, and the following papers are mechanistic studies involving NBS:
  4. The Mechanism of Benzylic Bromination with N-Bromosuccinimide
    E. Pearson and J. C. Martin
    Journal of the American Chemical Society 1963 85 (3), 354-355
    These papers by Prof J. C. Martin (UIUC) were early in his career, before he did the work that he is most well-known for (studies on ‘hypervalent’ molecules, including the development of the ‘Dess-Martin Periodinane’).
  5. The Identity of the Chain-Carrying Species in Brominations with N-Bromosuccinimide: Selectivity of Substituted N-Bromosuccinimides toward Substituted Toluenes
    E. Pearson and J. C. Martin
    Journal of the American Chemical Society 1963 85 (20), 3142-3146
    DOI: 10.1021/ja00903a021
  6. N-bromosuccinimide. Mechanisms of allylic bromination and related reactions
    H. Incremona and James Cullen Martin
    Journal of the American Chemical Society 1970 92 (3), 627-634
    DOI: 10.1021/ja00706a034
  7. Radical Bromination of Cyclohexene in CCl4 by Bromine: Addition versus Substitution
    W. McMillen and John B. Grutzner
    The Journal of Organic Chemistry 1994 59 (16), 4516-4528
    DOI: 10.1021/jo00095a029
    This paper describes careful kinetic studies that demonstrate that a low concentration of Br2 (such as that provided by impure NBS) will favor radical substitution over a polar addition reaction.
    L. Greenwood, M. D. Kellert, and J. Sedlak
    Org. Synth. Vol. 38, p.8 (1958).
    DOI: 10.115227/orgsyn.038.0008
    A reliable procedure for allylic bromination with NBS in Organic Syntheses.
    Emily F. M. Stephenson
    Org. Synth. Vol. 34, p.100 (1954)
    A reliable procedure for benzylic bromination with Br2 in Organic Syntheses.
  10. Kinetics and Mechanism Of The Reaction of Cyclohexene With Bromine in the Presence of Pyridine: Competition Between Different Electrophiles
    Giuseppe Bellucci, Giancarlo Berti, Roberto Bianchini, Giovanni Ingrosso, and Roberto Ambrosetti
    Journal of the American Chemical Society 1980 102 (25), 7480-7486

    DOI: 10.1021/ja00545a014
    So why does addition of HBr to alkenes occur at low concentrations of Br2 and not bromination itself? This paper observes that in a non-polar solvent like ClCH2CH2Cl, bromination is second-order in [Br2] and third order overall, which makes it considerably slower for low concentrations of [Br2].


Comment section

34 thoughts on “Allylic Bromination

  1. Hey James,

    Would I be correct in assuming that unless strict conditions are employed such as 1 equivalent of NBS, a second bromine addition will take place? Or will the EWG nature of the first bromide affect a second addition?

    Also the physics student in me would like to point out that light is represented by h(nu) not h(gamma). Quite trivial I know.

    1. Bromonium ion formation is reversible so as long as no strong nucleophiles are present to open it, it’s possible to get away with an excess of NBS. What often happens is that you need to keep adding the radical initiator (like AIBN or peroxides) over time if the reaction stops.

      Thanks for the correction!

      1. James,
        In the allylic bromination, after the initiation step, bromine radicals are formed. They have one electron less than their requirement and so they want to pick one electron. Then why don’t they cleave the pi bond, which has loosely bound electron, and take it from there?

        1. What you’re describing is addition of bromine radical to a pi bond, which is what happens when you treat an alkene with peroxides and HBr. In that reaction, once Br• adds to the pi bond, you obtain a radical on a carbon. If plenty of HBr is present, then the radical attacks the H of HBr and the cycle continues.

          However in the case of allylic bromination, that reaction is (ideally) a cul-de-sac. Once Br• radical addds to the double bond, forming that carbon-based radical, there is (ideally) nothing for it to react with since we’re not adding HBr and we’re keeping the concentration of Br2 low. Therefore the addition will revert back to the double bond and Br radical, and eventually the Br• will abstract a hydrogen from the allylic position.

          1. The same question came up in class today, and a quick bond energy calculation suggests the addition of Br2 across the double bond might be more favorable. The propagation step of allylic H abstraction is slightly endothermic, while the propagation step in “competing” radical addition to the C=C pi bond is slightly exothermic.
            This had me confused for a while, but a trip to my old graduate physical organic text (Lowry & Richardson, 1981, pp. 717-726) suggested that the Arrhenius collision orientation factor for abstraction is much more favorable than that for pi-addition, even though the activation energy is a bit less. The net result is a difference in rate constants of a factor of ~5 at 300 K. At the typical reaction temperature (refluxing CCl4, ~350 K) the difference is about a factor of 13.

  2. wouldn’t Br• attack on the vinylic carbon just like it does in the peroxide effect and the resulting radical would further start a chain reaction by attacking on Br2

    1. The vinyl C-H bonds have a bond dissociation energy of around 111 kcal/mol and the allyl C-H bonds have a bond dissociation energy of around 90 kcal/mol so it’s easier to break the allyl C-H bond and form the radical there.

  3. Hi James–

    As I understood, allylic means the molecule two away from the double bond, not directly attached, and vinylic means it is attached to the double bond. Therefore wouldn’t the radical on the 3rd carbon of 1-propene be vinylic?

    1. A vinylic radical would be directly attached to the double bond – i.e. sp2 hybridized . For example a radical on the 1 or 2 carbon of 1-propene would be vinylic. The adjacent carbon (carbon 3) is allylic. If there was a 4th carbon that position would be called, “homoallylic”.

      1. Dear james,
        Can you please tell me what will be the product when 3 methyl cyclohexene reacts with NBS/br2.
        Thank you

  4. Hi,

    Can I use DCM (dichlormethan) as a solvent instead of PhCl? Radical reactions are often not very selective. Why can brominate anyway selective just at the benzylposition and not somewhere else?

    Many thinks

    1. Usually you want a solvent that has a reasonably high boiling point since the initiation step requires heat. Dichloromethane is pretty low boiling. You could go for dichloroethane instead. (83 C° versus 40 C°)

  5. Hi james
    why wouldn’t Br• attack on the vinylic carbon instead of allylic carbon just like it does in the peroxide effect ?
    And for the reason u give why would be it not applicable in peroxide effect?

  6. If you were to have a molecule with a t-butyl substituent and a methyl substituent, with which group would the Br radical be more likely to react with?

    The particular molecule that brought up this question is 1-methyl-3-tert-butylbenzene.

  7. how can one selectively brominate one benzylic site out of two different sites……say if i want to slectively brominate the benzylic -CH2- group of p-ethyltoluene instead of the benzylic -CH3 group?

  8. Hi James
    I’ve a question about para ethyltoluene,(4-ethyltoluene) what will happen when it reacts with HBR, i can’t figure out where the bromation will take place,

    what happens if chlorobenzene reacts with KI ? is there any reaction? if yes where does it take place? i’ve an orgnic examen ,and i really don’t know how to handle those kinds of reactions.

    1. Bromination will not happen using HBr as a reagent. In that case all that will happen is that you will (transiently) protonate the ring.
      Chlorobenzene plus KI under (extraordinarily) forcing conditions MAY yield iodobenzene via nucleophilic aromatic substitution, but there are much better ways to do it.

    1. Nice and high boiling. If it takes heat to initiate the reaction it’s useful to choose a solvent which has a relatively high boiling point. There’s also no C-H bonds which can potentially react with free radicals.

  9. If On product 3 bromo cyclo pentene further addition of Br2, is done then what will be the product ?
    Bromination is possible ??

  10. I’m a little bit confused. It seems like your explanation to achieve a low concentration of Br2 to avoid dibromination is to react a trace amount of HBr with NBS to get a small amount of Br2, and then react Br2 in the presence of a solvent and with light to end up with an allylic brominated product. Why can’t we just start with a small amount of Br2 and react that with light in the first place? Why do we have to start with HBr and NBS?

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