Phosphorus tribromide is a colourless liquid with the formula PBr3. The liquid fumes in moist air due to hydrolysis and has a penetrating odour. It is used in the laboratory for the conversion of alcohols to alkyl bromides.
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| Names | |
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| IUPAC name
Phosphorus tribromide
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| Other names
phosphorus(III) bromide,
phosphorous bromide, tribromophosphine | |
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3D model (JSmol)
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| ECHA InfoCard | 100.029.253 |
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CompTox Dashboard (EPA)
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| Properties | |
| PBr3 | |
| Molar mass | 270.69 g/mol |
| Appearance | clear, colourless liquid |
| Density | 2.852 g/cm3 |
| Melting point | −41.5 °C (−42.7 °F; 231.7 K) |
| Boiling point | 173.2 °C (343.8 °F; 446.3 K) |
| rapid hydrolysis | |
Refractive index (nD)
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1.697 |
| Viscosity | 0.001302 Pas |
| Structure | |
| trigonal pyramidal | |
| Hazards | |
| GHS labelling: | |
 
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| Danger | |
| H314, H335 | |
| P260, P261, P264, P271, P280, P301 P330 P331, P303 P361 P353, P304 P340, P305 P351 P338, P310, P312, P321, P363, P403 P233, P405, P501 | |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other anions
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phosphorus trifluoride phosphorus trichloride phosphorus triiodide |
Other cations
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nitrogen tribromide arsenic tribromide antimony tribromide |
Related compounds
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phosphorus pentabromide phosphorus oxybromide |
| Supplementary data page | |
| Phosphorus tribromide (data page) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Preparation
editPBr3 is prepared by treating red phosphorus with bromine. An excess of phosphorus is used in order to prevent formation of PBr5:[1][2]
- P4 6 Br2 → 4 PBr3
Because the reaction is highly exothermic, it is often conducted in the presence of a diluent such as PBr3. Phosphorus tribromide is also generated in situ from red phosphorus and bromine.[3]
Reactions
editPhosphorus tribromide, like PCl3 and PF3, has both properties of a Lewis base and a Lewis acid. For example, with a Lewis acid such as boron tribromide it forms stable 1 :1 adducts such as Br3B · PBr3. At the same time PBr3 can react as an electrophile or Lewis acid in many of its reactions, for example with amines.
An important reaction of PBr3 is with alcohols, where it replaces an OH group with a bromine atom to produce an alkyl bromide. All three bromides can be transferred.[4]
- PBr3 3 (CH3)2CHCH2OH → 3 (CH3)2CHCH2Br HP(O)(OH)2
Several detailed procedures are available.[5][6] In some cases, triphenylphosphine/Br2 is superior to PBr3.[7]
The mechanism for a primary alcohol involves formation of a phosphorous ester (to form a good leaving group), followed by an SN2 substitution.
Because of the SN2 substitution step, the reaction generally works well for primary and secondary alcohols, but fails for tertiary alcohols. If the reacting carbon centre is chiral, the reaction usually occurs with inversion of configuration at the carbon alpha to the alcohol, as is usual with an SN2 reaction.
In a similar reaction, PBr3 also converts carboxylic acids to acyl bromides:[8]
- PBr3 3 RCO2H → 3 RCOBr HP(O)(OH)2
Applications
editThe main use for phosphorus tribromide is for conversion of primary or secondary alcohols to alkyl bromides,[9] as described above. PBr3 usually gives higher yields than hydrobromic acid, and it avoids problems of carbocation rearrangement- for example even neopentyl bromide can be made from the alcohol in 60% yield.[10]
Another use for PBr3 is as a catalyst for the α-bromination of carboxylic acids. Although acyl bromides are rarely made in comparison with acyl chlorides, they are used as intermediates in Hell-Volhard-Zelinsky halogenation.[11] Initially PBr3 reacts with the carboxylic acid to form the acyl bromide, which is more reactive towards bromination. The overall process can be represented as
On a commercial scale, phosphorus tribromide is used in the manufacture of pharmaceuticals such as alprazolam, methohexital and fenoprofen. It is also a potent fire suppression agent marketed under the name PhostrEx.
Phosphorus tribromide is used for doping in microelectronics.[12]
Precautions
editPBr3 evolves corrosive HBr, which is toxic, and reacts violently with water and alcohols.
- PBr3 3 H2O → H3PO3 3 HBr
In reactions that produce phosphorous acid as a by-product, when working up by distillation be aware that this can decompose above about 160 °C to give phosphine which can cause explosions in contact with air.[9]
References
edit- ^ Gay, J. F.; Maxson, R. N.; Kleinberg, J.; Haan, R. E. (1946). "Phosphorus(III) Bromide". Inorganic Syntheses. Vol. 2. pp. 147–151. doi:10.1002/9780470132333.ch43. ISBN 978-0-470-13161-9.
- ^ Burton, T. M.; Degerping, E. F. (1940). "The Preparation of Acetyl Bromide". Journal of the American Chemical Society. 62 (1): 227. doi:10.1021/ja01858a502.
- ^ Géza Braun (1934). "Glycerol α,γ-Dibromohydrin". Organic Syntheses. 14: 42. doi:10.15227/orgsyn.014.0042.
- ^ C. R. Noller, R. Dinsmore (1933). "Isobutyl Bromide". Organic Syntheses. 13: 20. doi:10.15227/orgsyn.013.0020.
- ^ George C. Harrison, Harvey Diehl (1943). "β-Ethoxyethyl Bromide". Organic Syntheses. 23: 32. doi:10.15227/orgsyn.023.0032.
- ^ H. B. Schurink (1937). "Pentaerythrityl Bromide and Iodide". Organic Syntheses. 17: 73. doi:10.15227/orgsyn.017.0073.
- ^ John P. Schaefer, J. G. Higgins, P. K. Shenoy (1968). "Cinnamyl Bromide". Organic Syntheses. 48: 51. doi:10.15227/orgsyn.048.0051.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ C. W. Smith, D. G. Norton (1953). "Dimethylketene". Organic Syntheses. 33: 29. doi:10.15227/orgsyn.033.0029.
- ^ a b Harrison, G. C.; Diehl, H. (1955). "β-Ethoxyethyl Bromide". Organic Syntheses; Collected Volumes, vol. 3, p. 370.
- ^ Wade, L. G. Jr. (2005). Organic Chemistry (6th ed.). Upper Saddle River, NJ, USA: Pearson/Prentice Hall. p. 477.
- ^ Wade, L. G. Jr. (2005). Organic Chemistry (6th ed.). Upper Saddle River, NJ, USA: Pearson/Prentice Hall. p. 1051.
- ^ Knoell, R. V.; Murarka, S. P. (1985-02-15). "Epitaxial growth induced by phosphorus tribromide doping of polycrystalline silicon films on silicon". Journal of Applied Physics. 57 (4). AIP Publishing: 1322–1327. Bibcode:1985JAP....57.1322K. doi:10.1063/1.334533. ISSN 0021-8979.
Further reading
edit- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- Lide, D. R., ed. (1990). Handbook of Chemistry and Physics (71st ed.). Ann Arbor, MI: CRC Press. ISBN 978-0849304712.
- March, J. (1992). Advanced Organic Chemistry (4th ed.). New York: Wiley. p. 723. ISBN 978-0471601807.
- Stecher, P. G., ed. (1960). The Merck Index (7th ed.). Rahway, NJ, USA: Merck & Co.
- Holmes, R. R. (1960). "An Examination of the Basic Nature of the Trihalides of Phosphorus, Arsenic and Antimony". Journal of Inorganic and Nuclear Chemistry. 12 (3–4): 266–275. doi:10.1016/0022-1902(60)80372-7.