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Ethyl bromoacetate

Ethyl bromoacetate
Skeletal formula of ethyl bromoacetate
Ball-and-stick model of ethyl bromoacetate
Preferred IUPAC name
Ethyl bromoacetate
Other names
Ethyl 2-bromoacetate
Bromoacetic acid, ethyl ester
Ethoxycarbonylmethyl bromide
3D model (JSmol)
ECHA InfoCard 100.002.992
RTECS number
  • AF6000000
Molar mass 167.002 g·mol−1
Appearance Colorless to yellow liquid[1]
Density 1.51 g/cm3
Melting point −38 °C (−36 °F; 235 K)[1]
Boiling point 158 °C (316 °F; 431 K)[1]
-82.8·10−6 cm3/mol
Very toxic (T+), Powerful lachrymator, Extremely harmful,
R-phrases (outdated) R26/27/28
S-phrases (outdated) (S1/2), S7/9, S26, S45
NFPA 704
Flammability code 0: Will not burn. E.g. waterHealth code 4: Very short exposure could cause death or major residual injury. E.g. VX gasReactivity code 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxideSpecial hazards (white): no codeNFPA 704 four-colored diamond
Flash point 47 °C (117 °F; 320 K)[1]
Related compounds
Other anions
Ethyl acetoacetate
Ethyl iodoacetate
Related esters
Methyl bromoacetate
Related compounds
Pepper spray
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Ethyl bromoacetate is the chemical compound with the formula CH2BrCO2C2H5. It is the ethyl ester of bromoacetic acid and is prepared in two steps from acetic acid.[2] It is a lachrymator and has a fruity, pungent odor.[3] It is also a highly toxic alkylating agent and may be fatal if inhaled.


Ethyl bromoacetate is listed by the World Health Organization as a riot control agent, and was first employed for that purpose by French police in 1912.[4] The French army used rifle grenades 'grenades lacrymogènes'[5] filled with this gas against the Germans beginning in August 1914, but the weapons were largely ineffective, even though Ethyl bromoacetate is twice as toxic as chlorine[6]. In the early months of the war the British also researched the weaponized use of tear gas agents and more toxic gasses including sulfur dioxide[7]. The German army then used this attack to justify their subsequent employment of it as odorant or warning agent in odorless, toxic gases and chemical weapons in 1915 under the German code Weisskreuz (White Cross).[8]

In organic synthesis, it is a versatile alkylating agent. Its major application involves the Reformatsky reaction, wherein it reacts with zinc to form a zinc enolate. The resulting BrZnCH2CO2Et condenses with carbonyl compounds to give a β-hydroxy-esters.

It is also the starting point for the preparation of several other reagents. For example, the related Wittig reagent (prepared by reaction with triphenylphosphine) is commonly used to prepare alpha,beta-unsaturated esters from carbonyl compounds such as benzaldehyde:[9]

Ethyl bromoacetate as the starting point for a Wittig reaction sequence


  1. ^ a b c d Chemicalland properties database (dead link 13 September 2018)
  2. ^ Natelson, S.; Gottfried, S. (1955). "Ethyl Bromoacetate". Organic Syntheses.CS1 maint: multiple names: authors list (link); Collective Volume, 3, p. 381
  3. ^ Criswell, DW; McClure, FL; Schaefer, R; Brower, KR (1980). "War gases as olfactory probes". Science. 210 (4468): 425–6. doi:10.1126/science.6968976. PMID 6968976.
  4. ^ Public health response to biological and chemical weapons, Chapter 3, Biological and Chemical agents, WHO Guidance]
  5. ^ []
  6. ^ []
  7. ^ []
  8. ^ Heller, Charles E. (September 1984). "Chemical Warfare in World War I: The American Experience, 1917-1918". Combat Studies Institute. Archived from the original on 2007-07-04. Retrieved 2007-08-02.
  9. ^ A student lab procedure for the Wittig sequence shown, only using the related methyl ester.

External links