Bromination of Alkenes: The Mechanism

by James

in AlkeneCC, Alkenes, Alkyl Halides, Organic Chemistry 1, Organic Reactions

In the last post of this series we showed how the mechanism for bromination of alkenes can’t possibly go through a carbocation intermediate.

0-brom

Why not? We have at least 3 good reasons:

  • The two atoms that form new bonds to carbon add to opposite faces of the alkene (“anti” stereoselectivity)
  • The reaction is stereospecific – (Z)-2-butene gives different product(s) than does (E)-2-butene (in fact, the products are stereoisomers of each other).
  • No rearrangements are observed, as they are for, say, the reactions of H-Cl with certain alkenes

There is one other detail to explain: when using water as a solvent, the reaction proceeds with “Markovnikov” regioselectivity. That is, the C-O bond is formed on the most substituted carbon of the alkene.

Back in 1937, Roberts and Kimball used similar observations to point out the deficiency of a free-carbocation mechanism proposed earlier by Robinson [Note below]. They argued that a free carbocation would allow for rotation about the carbon-carbon bond, and that this was inconsistent with the products observed in this reaction.

Instead, they invoked the intermediacy of a 3-membered ring structure with a positive charge on the halogen, which is “isoelectronic” (i.e. has the same electronic configuration) as a member of the oxygen family [epoxides, for instance].  Importantly, they said:

Since the two carbons in [the structure] are joined by a single bond and by a halogen bridge, free rotation is not to be expected

Furthermore, this proposal also explains the stereochemistry of the reaction:

This second step, which may be the addition of either a halogen ion X- or some other atom or molecule, is probably a simple “three-atom” reaction… In this case the new atom will approach one of the carbon atoms from the side opposite to the X atom already present. A bond to this carbon will be formed while the bond from the original X to the carbon is broken, with simultaneous neutralization of the charge of the ion. This process will always lead to trans addition

The final issue – regioselectivity – was not specifically addressed in this paper, but makes sense when you consider that it is the carbonwhich are electrophiles in this structure, not bromine [despite the positive formal charge on bromine ! recall that bromine is more electronegative than carbon!] and  the reaction will proceed at the carbon best able to stabilize positive charge.

Here’s what it looks like graphically:

1-brom

 

So in this reaction, the alkene acts as a nucleophile, attacking the electrophilic bromine, giving rise to a 3-membered ring intermediate. This is then attacked from the back side [similar to the backside attack in the SN2] at the carbon best able to stabilize positive charge,  to give the trans product. [Note that, like a flat coin that can land on “heads” or “tails” with equal likelihood, the bromine can “land” on either face of the alkene – this gives rise to enantiomers in this case].

If we use a solvent which can potentially act as a nucleophile such as water or an alcohol, the intermediate halonium ion can be “trapped” by solvent, giving rise to “halohydrin” products in the case where the solvent is water. Again, note that the water molecule attacks the most substituted carbon:

2-brom

 

Alright – so this “halonium ion” proposal seems to explain these results well enough. It’s a nice idea.  But is there any hard evidence that has come to light since 1937 that helps us to know if they really exist?

As a matter of fact, yes: halonium ions have actually been observed in the wild! The halonium ion from the reaction below is particularly stable. [think about it for a second – why might this be?]

4-adamantyl

 

Furthermore, R.S. Brown and co-workers succeeded in using X-ray diffraction to obtain a crystal structure of this molecule. Here’s the iodonium ion portion of the structure:

Screen shot 2013-03-04 at 2.03.45 PM

Figure adapted from R.S. Brown et. al., Journal of the American Chemical Society, 1994, 116, 2448-2456. Used with permission.

 

In chemistry, obtaining an X-ray crystal structure of a molecule is considered to be near-definite “proof” of its existence.  Although mechanisms can never be “proven”, this crystal structure represents about as close to a conclusive piece of evidence as you can get.

In the next post we’ll expand this idea of intermediate bridging ions to explain the results of a whole host of other reactions.

NEXT POST: Alkene Addition Pattern #2 – The “3 Membered Ring” Pathway

*1952 Nobel Prize winner Robinson, (of Robinson Annulation fame), was a brilliant man, but he was wrong about the mechanism of this reaction according to a reference that I cannot obtain at the moment but is apparently referenced here [Ingold, Chem. Rev., 15, 225, 1934]  This is instructive: looking backward, it seems obvious that the halonium proposal is correct, but in science we move forward gazing through a foggy windshield.

moc-elite-1

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{ 8 comments… read them below or add one }

Soji

Hey Prof., I get everything and you explain everything in a simpler way, but I don’t understand the part about “the reaction will proceed at the carbon best able to stabilize positive charge?” Could you perhaps show me that it is that C with greater partial charge in the corresponding example by using partial charge symbols?

Thanks,
Soji

Reply

James

It would be the most substituted carbon – think about carbocation stability, which follows the trend tertiary (most stable) > secondary > primary (least stable)

Reply

Owen

I was wondering about this, too. Thanks for taking time to explain it.

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Charles

Is there any reason why in case of water, H2O reacts before Br- does? H2O should be a weaker nucleophile than Br-.

Reply

James

Water is the solvent, so it is present in tremendously high concentration (pure water has a concentration of 55 M !). This explains why water attacks preferentially over Br-, which otherwise is a much better nucleophile.

Reply

ANAS KHAN

This is complicated by the fact that the major product isn’t 1,2-dibromoethane. The water also gets involved in the reaction, and most of the product is 2-bromoethanol.

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Idan

Something I don’t understand (my professor couldn’t explain it well either): logically I would assume that the second attack be on the less substituted carbon as there would be less steric hindrance. Also, being more substituted (more neighboring carbons) means that these carbons would donate more of their electron density to that same carbon, which would make it more negative (hence less electrophilic and less reactive).

I noticed you didn’t go into more detail than “[…] the reaction will proceed at the carbon best able to stabilize positive charge.” Is there a deeper explanation to this?

Reply

JAYANTA SARKAR

How can i synthesis only cis dibromo alkane from an alkene ?

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