Grignard reaction

Grignard reaction
Named after	Victor Grignard
Reaction type	Coupling reaction
Identifiers
Organic Chemistry Portal	grignard-reaction
RSC ontology ID	RXNO:0000014

A solution of a carbonyl compound is added to a Grignard reagent. (See gallery below)

The Grignard reaction (pronounced /ɡriɲar/) is an organometallic chemical reaction in which alkyl, vinyl, or aryl-magnesium halides (Grignard reagents) add to a carbonyl group in an aldehyde or ketone. This reaction is an important tool for the formation of carbon–carbon bonds. The reaction of an organic halide with magnesium is not a Grignard reaction, but provides a Grignard reagent.

Grignard reactions and reagents were discovered by and are named after the French chemist François Auguste Victor Grignard (University of Nancy, France), who was awarded the 1912 Nobel Prize in Chemistry for this work. Grignard reagents are similar to organolithium reagents because both are strong nucleophiles that can form new carbon–carbon bonds.

Reaction mechanism

The Grignard reagent functions as a nucleophile, attacking the electrophilic carbon atom that is present within the polar bond of a carbonyl group. The addition of the Grignard reagent to the carbonyl typically proceeds through a six-membered ring transition state.

However, with hindered Grignard reagents, the reaction may proceed by single-electron transfer. Similar pathways are assumed for other reactions of Grignard reagents, e.g., in the formation of carbon–phosphorus, carbon–tin, carbon–silicon, carbon–boron and other carbon–heteroatom bonds.

Preparation of Grignard reagent

Grignard reagents form via the reaction of an alkyl or aryl halide with magnesium metal. The reaction is conducted by adding the organic halide to a suspension of magnesium in an etherial solvent, which provides ligands required to stabilize the organomagnesium compound. Empirical evidence suggests that the reaction takes place on the surface of the metal. The reaction proceeds through single electron transfer: In the Grignard formation reaction, radicals may be converted into carbanions through a second electron transfer.

R−X + Mg → R−X^•− + Mg^•+

R−X^•− → R^• + X⁻

R^• + Mg^•+ → RMg⁺

RMg⁺ + X⁻ → RMgX

A limitation of Grignard reagents is that they do not readily react with alkyl halides via an S_N2 mechanism. On the other hand, they readily participate in transmetalation reactions:

RMgX + AlX → AlR + MgX₂

For this purpose, commercially available Grignard reagents are especially useful because this route avoids the problem with initiation.

Reaction conditions

In reactions involving Grignard reagents, it is important to exclude water and air, which rapidly destroy the reagent by protonolysis or oxidation. Since most Grignard reactions are conducted in anhydrous diethyl ether or tetrahydrofuran, side-reactions with air are limited by the protective blanket provided by solvent vapors. Small-scale or quantitative preparations should be conducted under nitrogen or argon atmospheres, using air-free techniques. Although the reagents still need to be dry, ultrasound can allow Grignard reagents to form in wet solvents by activating the magnesium such that it consumes the water.

The organic halide

Grignard reactions often start slowly. As is common for reactions involving solids and solution, initiation follows an induction period during which reactive magnesium becomes exposed to the organic reagents. After this induction period, the reactions can be highly exothermic. Alkyl and aryl bromides and iodides are common, with chlorides being seen as well. However, fluorides are generally unreactive, except with specially activated magnesium.

Magnesium

Typical Grignard reactions involve the use of magnesium ribbon. All magnesium is coated with a passivating layer of magnesium oxide, which inhibits reactions with the organic halide. Specially activated magnesium, such as Rieke magnesium, circumvents this problem. The oxide layer can also be broken up using ultrasound, or by adding a few drops of iodine or 1,2-Diiodoethane.

Solvent

Usually Grignard reagents are written as RMgX, but in fact the magnesium(II) centre is tetrahedral when dissolved in Lewis basic solvents, as shown here for the bis-adduct of methylmagnesium chloride and THF.

Most Grignard reactions are conducted in ethereal solvents, especially diethyl ether and THF. With the chelating diether dioxane, some Grignard reagents undergo a redistribution reaction to give diorganomagnesium compounds (R = organic group, X = halide):

2 RMgX + dioxane ⇌ R₂Mg + MgX₂(dioxane)

This reaction is known as the Schlenk equilibrium.

Testing Grignard reagents

Because Grignard reagents are so sensitive to moisture and oxygen, many methods have been developed to test the quality of a batch. Typical tests involve titrations with weighable, anhydrous protic reagents, e.g. menthol in the presence of a color-indicator. The interaction of the Grignard reagent with phenanthroline or 2,2'-bipyridine causes a color change.

Initiation

Many methods have been developed to initiate sluggish Grignard reactions. These methods weaken the passivating layer of MgO, thereby exposing highly reactive magnesium to the organic halide. Mechanical methods include crushing of the Mg pieces in situ, rapid stirring, and sonication of the suspension. Iodine, methyl iodide, and 1,2-Dibromoethane are common activating agents. The use of 1,2-dibromoethane is particularly advantageous as its action can be monitored by the observation of bubbles of ethylene. Furthermore, the side-products are innocuous:

Mg + BrC₂H₄Br → C₂H₄ + MgBr₂

The amount of Mg consumed by these activating agents is usually insignificant. A small amount of mercuric chloride will amalgamate the surface of the metal, allowing it to react.

Industrial production

Grignard reagents are produced in industry for use in situ, or for sale. As with a bench-scale, the main problem is that of initiation; a portion of a previous batch of Grignard reagent is often used as the initiator. Grignard reactions are exothermic, and this exothermicity must be considered when a reaction is scaled-up from laboratory to production plant.

Many Grignard reagents such as methylmagnesium bromide, methylmagnesium chloride, phenylmagnesium bromide, and allylmagnesium bromide are available commercially as tetrahydrofuran or diethyl ether solutions.

Mg transfer reaction (halogen–Mg exchange)

An alternative preparation of Grignard reagents involves transfer of Mg from a preformed Grignard reagent to an organic halide. This method offers the advantage that the Mg transfer tolerates many functional groups. A typical reaction involves isopropylmagnesium chloride and aryl bromide or iodides.

Reactions of Grignard reagents

With carbonyl compounds

Grignard reagents react with a variety of carbonyl derivatives.

The most common application of Grignard reagents is the alkylation of aldehydes and ketones, i.e. the Grignard reaction:

Note that the acetal function (a protected carbonyl) does not react.

Such reactions usually involve an aqueous acidic workup, though this step is rarely shown in reaction schemes. In cases where the Grignard reagent is adding to an aldehyde or a prochiral ketone, the Felkin-Anh model or Cram's Rule can usually predict which stereoisomer will be formed. With easily deprotonated 1,3-diketones and related acidic substrates, the Grignard reagent RMgX functions merely as a base, giving the enolate anion and liberating the alkane RH.

Grignard reagents are nucleophiles in nucleophilic aliphatic substitutions for instance with alkyl halides in a key step in industrial Naproxen production:

Reactions as a base

Grignard reagents serve as a base for protic substrates (this scheme does not show workup conditions, which typically includes water). Grignard reagents are basic and react with alcohols, phenols, etc. to give alkoxides (ROMgBr). The phenoxide derivative is susceptible to formylation paraformaldehyde to give salicylaldehyde.

Formation of bonds to B, Si, P, Sn

Like organolithium compounds, Grignard reagents are useful for forming carbon–heteroatom bonds.

Reaction with transition metal halides

Grignard reagents react with many metal-based electrophiles. For example, they undergo transmetallation with cadmium chloride (CdCl₂) to give dialkylcadmium:

2 RMgX + CdCl₂ → R₂Cd + 2 Mg(X)Cl

Dialkylcadmium reagents are used for preparation of ketones from acyl halides:

2 R'C(O)Cl + R₂Cd → 2 R'C(O)R + CdCl₂

With organic halides

Grignard reagents do not typically react with organic halides, in contrast with their high reactivity with other main group halides. In the presence of metal catalysts, however, Grignard reagents participate in C-C coupling reactions. For example, nonylmagnesium bromide reacts with methyl p-chlorobenzoate to give p-nonylbenzoic acid, in the presence of Tris(acetylacetonato)iron(III) (Fe(acac)₃), after workup with NaOH to hydrolyze the ester, shown as follows. Without the Fe(acac)₃, the Grignard reagent would attack the ester group over the aryl halide.

For the coupling of aryl halides with aryl Grignard reagents, nickel chloride in tetrahydrofuran (THF) is also a good catalyst. Additionally, an effective catalyst for the couplings of alkyl halides is dilithium tetrachlorocuprate (Li₂CuCl₄), prepared by mixing lithium chloride (LiCl) and copper(II) chloride (CuCl₂) in THF. The Kumada-Corriu coupling gives access to [substituted] styrenes.

Oxidation

Treatment of a Grignard reagent with oxygen gives the magnesium organoperoxide. Hydrolysis of this material yields hydroperoxides or alcohol. These reactions involve radical intermediates.

The simple oxidation of Grignard reagents to give alcohols is of little practical import as yields are generally poor. In contrast, two-step sequence via a borane (vide supra) that is subsequently oxidized to the alcohol with hydrogen peroxide is of synthetic utility.

The synthetic utility of Grignard oxidations can be increased by a reaction of Grignard reagents with oxygen in presence of an alkene to an ethylene extended alcohol. This modification requires aryl or vinyl Grignards. Adding just the Grignard and the alkene does not result in a reaction demonstrating that the presence of oxygen is essential. The only drawback is the requirement of at least two equivalents of Grignard although this can partly be circumvented by the use of a dual Grignard system with a cheap reducing Grignard such as n-butylmagnesium bromide.

Elimination

In the Boord olefin synthesis, the addition of magnesium to certain β-haloethers results in an elimination reaction to the alkene. This reaction can limit the utility of Grignard reactions.

Degradation of Grignard reagents

At one time, the formation and hydrolysis of Grignard reagents was used in the determination of the number of halogen atoms in an organic compound. In modern usage Grignard degradation is used in the chemical analysis of certain triacylglycerols.

Industrial use

An example of the Grignard reaction is a key step in the (non-stereospecific) industrial production of Tamoxifen (currently used for the treatment of estrogen receptor positive breast cancer in women):

Gallery

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  Magnesium turnings are placed in a flask.

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  Tetrahydrofuran and a small piece of iodine are added.

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  A solution of alkyl bromide is added while heating.

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  After completion of the addition, the mixture is heated for a while.

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  Formation of the Grignard reagent is complete. A small amount of magnesium still remains in the flask.

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  The Grignard reagent thus prepared is cooled to 0°C before the addition of the carbonyl compound. The solution becomes cloudy as the Grignard reagent precipitates out.

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  A solution of carbonyl compound is added to the Grignard reagent.

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  The solution is warmed to room temperature. At this point the reaction is complete.

See also

• Wittig reaction
• Barbier reaction
• Bodroux-Chichibabin aldehyde synthesis
• Fujimoto-Belleau reaction
• Organolithium reagents
• Sakurai reaction
• Indium mediated allylation
• Alkynation

Further reading

• Mary McHale, "Grignard Reaction," Connexions, http://cnx.org/content/m15245/1.2/. 2007.
• Grignard knowledge: Alkyl coupling chemistry with inexpensive transition metals by Larry J. Westrum, Fine Chemistry November/December 2002, pp. 10–13 [1]