In the formation of a Grignard reagent from a compound possessing both bromine and chlorine, magnesium preferentially inserts into the C–Br bond over the C–Cl bond. For example, the formation of a Grignard reagent from 1-bromo-2-chloroethane proceeds with good selectivity:[1]

Grignard formation from 1-bromo-2-chloroethane and subsequent transmetallation to tin

How can this be explained? Can it be rationalised using a reaction mechanism?

  1. Simon, P. Y.-R.; Oreal, H.; Audran, G.; Schulz, M.; Joly, J.-P.; Siri, D.; Siri, A. Proteasome Inhibiting β-Lactam Prodrugs Useful for the Treatment of Cancer and Neurodegenerative Disorders. World Patent WO 2018/115497 A1, June 28, 2018.
  • 12
    $\begingroup$ Simply put the C-Br bond is weaker than C-Cl, so oxidative addition occurs much faster. Oxidative addition is treated in more depth in any textbook on organometallic chemistry (the usual context is transition metals but it applies equally well to Mg). $\endgroup$
    – orthocresol
    Apr 4 '17 at 17:44

As noted earlier, the determining factor is the greater strength of the carbon-chlorine bond versus carbon-bromine, which leads to a higher activation energy for the magnesium to react with the former.

The strength of a carbon-halogen bond, and therefore the activation energy required for magnesium to form a Grignard reagent, is greatest with fluorine and decreases progressively with heavier halogens. The reactivity sequence between carbon-halogen bonds and magnesium may therefore be extended:

$\ce{C-F < C-Cl < C-Br < C-I}$

We might amend the first Inequality to read $<<$ rather than just $<$, as carbon-fluorine bonds are completely unreactive with normal procedures. Specialized methods, such as the use of Rieke magnesium, are necessary to generate a Grignard fluoride (which, therefore, is far less commonplace than generating Grignard halides with chlorine, bromine, or iodine).

The hydrocarbon group, too, can impact reactivity. Chlorine, bromine and iodine can all couple their nonbonding pairs with an aromatic ring, strengthening the bond of the halogen to the ring. Thus aryl halides react less rapidly than alkyl halides with a given halogen. Encyclopedia Britannica, combining the substrate and halogen effects reports:

Organohalogens vary greatly in their rates of reaction with magnesium. For example, alkyl iodides generally react very rapidly, whereas most aryl chlorides react very slowly, if at all.

This may be used to advantage, for instance if an aryl compound with both chlorine and bromine is exposed to magnesium, the chloroarylmagnesium bromide is formed with good selectivity.


There are a few reasons:

  1. C-Br bond is weaker than and thus more easily cleaved than C-Cl bond.

  2. Mg-Br is more stable than Mg-Cl. The electron cloud of Br is more polarisable than that of Cl, due to Br having not just a larger number of electrons but also larger atomic radius, over which its electrons are distributed. The Mg-Br covalent bond formed will thus have a greater partial ionic character than Mg-Cl bond, which confers additional stability by electrostatic attraction.

  • 5
    $\begingroup$ I'd stick with (1). $\endgroup$ Nov 22 '21 at 10:42
  • 2
    $\begingroup$ Unfortunately I can only upvote @OscarLanzi once $\endgroup$
    – Ian Bush
    Nov 22 '21 at 12:08
  • $\begingroup$ Mg-Br covalent bond? Highly suspicious $\endgroup$ Nov 24 '21 at 13:50

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.