Acyl Halide

In organic chemistry, an acyl halide (also known as an acid halide) is a chemical compound derived from an oxoacid[1] by replacing a hydroxyl group (−OH) with a halide group (−X, where X is a halogen).[2]

If the acid is a carboxylic acid (−C(=O)OH), the compound contains a −C(=O)X functional group, which consists of a carbonyl group (C=O) singly bonded to a halogen atom.[3] The general formula for such an acyl halide can be written RCOX, where R may be, for example, an alkyl group, CO is the carbonyl group, and X represents the halide, such as chloride. Acyl chlorides are the most commonly encountered acyl halides, but acetyl iodide is the one produced (transiently) on the largest scale. Billions of kilograms are generated annually in the production of acetic acid.[4]


Aliphatic acyl halides

On an industrial scale, the reaction of acetic anhydride with hydrogen chloride produces a mixture of acetyl chloride and acetic acid:[5]

Common syntheses of acyl chlorides also entail the reaction of carboxylic acids with phosgene, thionyl chloride,[6] and phosphorus trichloride[7] Phosphorus pentabromide is used for acyl bromides, which are rarely of value.

Aromatic acyl chlorides

Benzoyl chloride is produced from benzotrichloride using either water or benzoic acid:[8]

As with other acyl chlorides, it can be generated from the parent acid and other chlorinating agents phosphorus pentachloride or thionyl chloride.

Representative laboratory routes to aromatic acyl halides are comparable to those for aliphatic acyl halides.[9] For example, chloroformylation, a specific type of Friedel-Crafts acylation which uses formaldehyde as a reagent[citation needed], or by the direct chlorination of benzaldehyde derivatives.[10]

Acyl fluorides

Of commercial interest, acyl chlorides react with HF to give acyl fluorides.[11] Aromatic (as well as aliphatic) acyl fluorides are conveniently prepared directly from carboxylic acids, using stable, inexpensive commodity chemicals: PPh3, NBS and Et3N-3HF in a bench-top protocol.[12] Cyanuric fluoride converts carboxylic acids to acyl fluorides.

Acyl bromides and iodides

Acyl bromides and iodides are synthesized accordingly but are less common.[13]


Acyl halides are rather reactive compounds often synthesized to be used as intermediates in the synthesis of other organic compounds. For example, an acyl halide can react with:

In the above reactions, HX (hydrogen halide or hydrohalic acid) is also formed. For example, if the acyl halide is an acyl chloride, HCl (hydrogen chloride or hydrochloric acid) is also formed.

Multiple functional groups

Adipoyl chloride

A molecule can have more than one acyl halide functional group. For example, "adipoyl dichloride", usually simply called adipoyl chloride, has two acyl chloride functional groups; see the structure at right. It is the dichloride (i.e., double chloride) of the 6-carbon dicarboxylic acid adipic acid. An important use of adipoyl chloride is polymerization with an organic di-amino compound to form a polyamide called nylon or polymerization with certain other organic compounds to form polyesters.

Phosgene (carbonyl dichloride, Cl–CO–Cl) is a very toxic gas that is the dichloride of carbonic acid (HO–CO–OH). Both chlorine atoms in phosgene can undergo reactions analogous to the preceding reactions of acyl halides. Phosgene is used a reactant in the production of polycarbonate polymers, among other industrial applications.

General hazards

Volatile acyl halides are lachrymatory because they can react with water at the surface of the eye producing hydrohalic and organic acids irritating to the eye. Similar problems can result if one inhales acyl halide vapors. In general, acyl halides (even non-volatile compounds such as tosyl chloride) are irritants to the eyes, skin and mucous membranes.


  1. ^ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "acyl groups". doi:10.1351/goldbook.A00123
  2. ^ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "acyl halides". doi:10.1351/goldbook.A00124
  3. ^ Saul Patai, ed. (1972). Acyl Halides. PATAI'S Chemistry of Functional Groups. doi:10.1002/9780470771273. ISBN 9780470771273.
  4. ^ Hosea Cheung, Robin S. Tanke, G. Paul Torrence "Acetic Acid" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a01_045
  5. ^ Cheung, Hosea; Tanke, Robin S.; Torrence, G. Paul (2000). "Acetic Acid". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a01_045.
  6. ^ Helferich, B.; Schaefer, W. (1929). "n-Butyrl chloride". Organic Syntheses. 9: 32. doi:10.15227/orgsyn.009.0032.
  7. ^ a b Allen, C. F. H.; Barker, W. E. (1932). "Desoxybenzoin". Organic Syntheses. 12: 16. doi:10.15227/orgsyn.012.0016.
  8. ^ Maki, Takao; Takeda, Kazuo (2000). "Benzoic Acid and Derivatives". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_555.
  9. ^ Adams, Roger (1923). "p-Nitrobenzoyl chloride". Organic Syntheses. 3: 75. doi:10.15227/orgsyn.003.0075.
  10. ^ Clarke, H. T.; Taylor, E. R. (1929). "o-Chlorobenzoyl chloride". Organic Syntheses. 9: 34. doi:10.15227/orgsyn.009.0034.
  11. ^ Olah G, Kuhn S (1961). "Preparation of Acyl Fluorides with Anhydrous Hydrogen Fluoride. The General Use of the Method of Colson and Fredenhagen". J. Org. Chem. 26: 237–238. doi:10.1021/jo01060a600.
  12. ^ Munoz, Socrates B.; Dang, Huong; Ispizua-Rodriguez, Xanath; Mathew, Thomas; Prakash, G. K. Surya (2019-03-15). "Direct Access to Acyl Fluorides from Carboxylic Acids Using a Phosphine/Fluoride Deoxyfluorination Reagent System". Organic Letters. 21 (6): 1659–1663. doi:10.1021/acs.orglett.9b00197. ISSN 1523-7060. PMID 30840474. S2CID 73481495.
  13. ^ Keinan, Ehud; Sahai, M. (June 1990). "Diiodosilane. 3. Direct synthesis of acyl iodides from carboxylic acids, esters, lactones, acyl chlorides and anhydrides". The Journal of Organic Chemistry. 55 (12): 3922–3926. doi:10.1021/jo00299a042. ISSN 0022-3263.
  14. ^ Allen, C. F. H.; Kibler, C. J.; McLachlin, D. M.; Wilson, C. V. (1946). "Acid Anhydrides". Organic Syntheses. 26: 1–3. doi:10.15227/orgsyn.026.0001. PMID 20280752.