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IUPAC name Iodomethane
Other names Methyl iodide, Monoiodomethane, Methyl iodine, MeI, Halon 10001, UN 2644
CAS number 74-88-4
PubChem 6328
EINECS number 200-819-5
RTECS number PA9450000
InChI InChI=1/CH3I/c1-2/h1H3
Molecular formula CH3I
Molar mass 141.94 g/mol
Appearance Clear colourless liquid with acrid odor
Density 2.2789 g/cm3 at 20 °C
Melting point

-66.45 °C (206.70 K)

Boiling point

42.43 °C (315.58 K)

Solubility in water 14 g/l at 20 °C
log P 1.51
Vapor pressure 50 kPa at 20 °C

53.32 at 25.3 °C 166.1 kPa at 55 °C

EU classification Toxic (T), Carc. Cat. 3
NFPA 704
R-phrases R21, R23/25, R37/38, R40
S-phrases (S1/2), S36/37, S38, S45
Flash point -28 °C
352 °C
Explosive limits 8.5 - 66%
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Iodomethane, commonly called methyl iodide and commonly abbreviated "MeI", is the chemical compound with the formula CH3I. This dense volatile liquid is related to methane by replacement of one hydrogen atom by an atom of iodine and its dipole moment is 1.59 D. Refractive index is 1.5304 (20 °C, D), 1.5293 (21 °C, D). It is miscible with common organic solvents. It is colourless, although upon exposure to light, samples develop a purplish tinge caused by the presence of I2. Storage over copper metal absorbs the iodine. Methyl iodide is widely used in organic synthesis to deliver a methyl group, via the transformation called methylation. It is naturally emitted by rice plantations in small amounts.[1]

Additional recommended knowledge


Chemical properties

Methyl iodide is an excellent substrate for SN2 substitution reactions. It is sterically open for attack by nucleophiles, and iodide is a good leaving group. For example, it can be used for the methylation of phenols or carboxylic acids:[2]

In these examples, the base (K2CO3 or Li2CO3) removes the acidic proton to form the carboxylate or phenoxide anion, which serves as the nucleophile in the SN2 substitution.

Iodide is a "soft" anion which means that methylation with MeI tends to occur at the "softer" end of an ambidentate nucleophile. For example, reaction with thiocyanate ion favours attack at S rather than "hard" N, leading mainly to methyl thiocyanate (CH3SCN) rather than CH3NCS. This behavior is relevant to the methylation of stabilized enolates such as those derived from 1,3-dicarbonyl compounds. Methylation of these and related enolates can occur on the harder oxygen atom or the (usually desired) carbon atom. With methyl iodide, C-alkylation nearly always predominates.

MeI is also an important precursor to methylmagnesium iodide or "MeMgI", which is a common reagent. Because MeMgI forms readily, it is often prepared in instructional laboratories as an illustration of Grignard reagents. The use of MeMgI has been somewhat superseded by the commercially available methyl lithium.

In the Monsanto process, MeI forms in situ from the reaction of methanol and hydrogen iodide. The CH3I then reacts with carbon monoxide in the presence of a rhodium complex to form acetyl iodide, the precursor to acetic acid after hydrolysis. Most acetic acid is prepared by this method.

MeI hydrolyzes at 270 °C forming hydrogen iodide, carbon monoxide and carbon dioxide.


Iodomethane is formed via the exothermic reaction that occurs when iodine is added to a mixture of methanol with red phosphorus:[3]

5 CH3OH + P + 2.5 I2 → 5 CH3I + H3PO4 + H2O

The iodinating reagent is phosphorus triiodide that is formed in situ. Alternatively, it is prepared from the reaction of dimethyl sulfate with potassium iodide in the presence of calcium carbonate:[3]

(CH3O)2SO2 + KI → K2SO4 + 2 CH3I

The CH3I can easily be purified by distillation followed by washing with Na2S2O3 (to remove iodine) and then water, aq. Na2CO3.

Methyl iodide can be formed during nuclear accidents by the reaction of organic matter with the "fission iodine."

Choice of iodomethane as a methylating agent

Iodomethane is an excellent reagent for methylation, but there are some disadvantages to its use. It has a high equivalent weight: one mole of MeI weighs almost three times as much as one mole of methyl chloride. However, the chloride is a gas (as is methyl bromide), making it more awkward to work with than liquid MeI. Methyl chloride is a poorer methylating reagent than MeI, though it is often adequate.

Iodides are generally expensive relative to the more common chlorides and bromides, though iodomethane is reasonably affordable; on a commercial scale the toxic dimethyl sulfate is preferred, since it is both cheap and liquid. The iodide leaving group in MeI may cause side reactions, as it is a powerful nucleophile. Finally, being highly reactive, MeI is more dangerous for laboratory workers than related chlorides and bromides. When considering alternatives to MeI, it is necessary to consider cost, handling, risk, chemical selectivity, and ease of reaction work-up.


Besides use as a methylation agent, there have been proposals of its use as a fungicide, herbicide, insecticide or nematicide and as a fire extinguisher. Further it can be used as a soil disinfectant, replacing bromomethane (which was banned under the Montreal Protocol), and in microscopy due to properties related to refraction index. In a controversial October 2007 decision, the United States Environmental Protection Agency approved its use as a soil fumigant in some cases, although it cannot yet be used in California (a major potential market) due to lack of state approval.[4]

Biological effects

Iodomethane has LD50 for oral administration to rats 76 mg/kg and in the liver it undergoes rapid conversion to S-methylglutathione.[5]

Breathing iodomethane fumes can cause lung, liver, kidney and central nervous system damage. It causes nausea, dizziness, coughing and vomiting. Prolonged contact with skin causes burns. Massive inhalation causes pulmonary edema.

See also

Methylating reagents


  1. ^ K. R. Redeker, N.-Y. Wang, J. C. Low, A. McMillan, S. C. Tyler, and R. J. Cicerone (2000). "Emissions of Methyl Halides and Methane from Rice Paddies". Science 290: 966-969. doi:10.1126/science.290.5493.966.
  2. ^ Avila-Zárraga, J. G., Martínez, R. (January 2001). "Efficient methylation of carboxylic acids with potassium hydroxide/methyl sulfoxide and iodomethane". Synthetic Communications 31 (14): 2177 - 2183. doi:10.1081/SCC-100104469.
  3. ^ a b King, C. S.; Hartman, W. W. (1943). "Methyl Iodide". Org. Synth.; Coll. Vol. 2: 399. 
  4. ^ "EPA approves new pesticide despite scientists' concerns", Los Angeles Times, October 6, 2007. 
  5. ^ Johnson, M. K. (1966). "Metabolism of iodomethane in the rat". Biochem. J. 98: 38-43.
  • March, J. (1992). Advanced Organic Chemistry, 4th Edn., New York: Wiley. ISBN 0-471-60180-2. 
  • Sulikowski, G. A.; Sulikowski, M. M. (1999). in Coates, R.M.; Denmark, S. E. (Eds.) Handbook of Reagents for Organic Synthesis, Volume 1: Reagents, Auxiliaries and Catalysts for C-C Bond Formation New York: Wiley, pp. 423–26.
  • Bolt H. M., Gansewendt B. (1993). "Mechanisms of carcinogenicity of methyl halides.". Crit Rev Toxicol. 23 (3): 237-53.
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Iodomethane". A list of authors is available in Wikipedia.
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