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Finally, in selected cases, magnesium will react with acidic hydrocarbons such as cyclopentadienyl at high temperatures (600 °C).


In the vapor phase dialkyl magnesium compounds are generally monomeric linear compounds. In solution, in the absence of coordinating solvents R 2 Mg form a variety of oligomers ( [link] a-c) in solution as determined by molecular weight measurements. In the presence of coordinating solvents 4-coordinate monomers predominate ( [link] d).

Solution structure of R 2 Mg (R = Me, Et) in (a – c) non-coordinating solvents, and (d) diethyl ether.

As similar trend is observed in the solid state, where polymers have been characterized in the absence of coordinating solvents ( [link] a), while monomers or dimmers are generally observed when crystallized from a coordinating solvent ( [link] b and c).

Solid state structure of R 2 Mg (R = Me, Et) crystallized in (a) the absence and (b and c) the presence of a coordinating solvents.

The use of organomagnesium compounds in organic synthesis

Grignard compounds react with water to give the hydrocarbon, [link] , they also react with other hydroxylic compounds such as alcohols and carboxylic acids. One important use of the hydrolysis reaction is specifically deuteration, [link] .

The hydrogen atom on a terminal alkyne is sufficiently acidic that the reaction with Grignards occurs in an analogous manner to that of hydrolysis.

Once formed the alkynyl Grignard undergoes the same hydrolysis reaction.

Reaction with co 2

Grignards react readily with carbon dioxide to form the carboxylate, which yields the associated carboxylic acid upon hydrolysis, [link] .

Reaction with carbonyls

Organomagnesium compounds react with organic carbonyls (aldehydes, ketones, and esters) to yield the alcohol on hydrolysis, [link] . This synthetic route is useful for the formation of primary, secondary and terminal alcohols.

Unfortunately, for some carbonyls there is a competing side reaction of enolization, where the starting ketone is reformed upon hydrolysis.

When the Grignard reagent has a β-hydrogen another side reaction occurs in which the carbonyl group is reduced and an alkene is formed.

Both the enolization and reduction occur via similar 6-membered cyclic transition states ( [link] ).

Representation of the 6-membered transition state reaction for enolization of a ketone.

Grignards react with α,β-unsaturated ketones to give either the 1,2-addition product or the 1,4-addition product, or both.

Reaction with acyl halides

Acyl halides react with Grignards to give ketones, [link] . Best results are obtained if the reaction is carried out at low temperature and in the presence of a Lewis acid catalysts (e.g., FeCl 3 ).

Reaction with epoxides

Oxirane (epoxide) rings are opened by Grignards, [link] , in a useful reaction that extends the carbon chain of the Grignard by two carbon atoms. This reaction is best performed with ethylene oxide since the magnesium halide formed is a Lewis acid catalyst for further reactions in the case of substituted oxiranes.

Reaction with salts

One of the most useful methods of preparing organometallic compounds is the exchange reaction of one organometallic compound with a salt of a different metal, [link] . This is an equilibrium process, whose equilibrium constant is defined by the reduction potential of both metals. In general the reaction will proceed so that the more electropositive metal will form the more ionic salt (usually chloride).

Grignard reagents are particularly useful in this regard, and may be used to prepare a wide range of organometallic compounds. For example:

The reaction with a Grignard is milder than the analogous reaction with lithium reagents, and leads to a lower incident of side-products.


  • H. Bader and N. M. Smyth, J. Org. Chem . , 1964, 29 , 953.
  • C. L. Hill, J. B. Vander Sande, G. M. Whitesides, J. Org. Chem. , 1980, 45 , 1020.
  • E. Weiss, J. Organomet. Chem. , 1964, 2 , 314.
  • A. R. Barron, J. Chem. Soc., Dalton Trans. , 1989, 1625.

Questions & Answers

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Commplementary angles
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The answer is neither. The function, 2 = 0 cannot exist. Hence, the function is undefined.
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Differences Between Laspeyres and Paasche Indices
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At high concentrations (>0.01 M), the relation between absorptivity coefficient and absorbance is no longer linear. This is due to the electrostatic interactions between the quantum dots in close proximity. If the concentration of the solution is high, another effect that is seen is the scattering of light from the large number of quantum dots. This assumption only works at low concentrations of the analyte. Presence of stray light.
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the Beer law works very well for dilute solutions but fails for very high concentrations. why?
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Source:  OpenStax, Chemistry of the main group elements. OpenStax CNX. Aug 20, 2010 Download for free at http://cnx.org/content/col11124/1.25
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