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Short description: Chemical compound hydrogen phosphide
IUPAC name
Other names
Phosphorus trihydride
Phosphorated hydrogen
3D model (JSmol)
EC Number
  • 232-260-8
RTECS number
  • SY7525000
UN number 2199
Molar mass 33.99758 g/mol
Appearance Colourless gas
Odor fish-like or garlic-like[1]
Density 1.379 g/l, gas (25 °C)
Melting point −132.8 °C (−207.0 °F; 140.3 K)
Boiling point −87.7 °C (−125.9 °F; 185.5 K)
31.2 mg/100ml (17 °C)
Solubility Soluble in alcohol, ether, CS2
slightly soluble in benzene, chloroform, ethanol
Vapor pressure 41.3 atm (20 °C)[1]
Conjugate acid Phosphonium (chemical formula PH+4)
Viscosity 1.1×10−5 Pa⋅s
Trigonal pyramidal
0.58 D
37 J/mol⋅K
210 J/mol⋅K[2]
5 kJ/mol[2]
13 kJ/mol
Safety data sheet ICSC 0694
GHS pictograms GHS02: Flammable GHS06: Toxic GHS05: Corrosive GHS09: Environmental hazard
NFPA 704 (fire diamond)
Flammability code 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneHealth code 4: Very short exposure could cause death or major residual injury. E.g. VX gasReactivity code 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazards (white): no codeNFPA 704 four-colored diamond
Flash point Flammable gas
38 °C (100 °F; 311 K) (see text)
Explosive limits 1.79–98%[1]
Lethal dose or concentration (LD, LC):
3.03 mg/kg (rat, oral)
11 ppm (rat, 4 hr)[3]
1000 ppm (mammal, 5 min)
270 ppm (mouse, 2 hr)
100 ppm (guinea pig, 4 hr)
50 ppm (cat, 2 hr)
2500 ppm (rabbit, 20 min)
1000 ppm (human, 5 min)[3]
NIOSH (US health exposure limits):
PEL (Permissible)
TWA 0.3 ppm (0.4 mg/m3)[1]
REL (Recommended)
TWA 0.3 ppm (0.4 mg/m3), ST 1 ppm (1 mg/m3)[1]
IDLH (Immediate danger)
50 ppm[1]
Related compounds
Other cations
Related compounds
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

Phosphine (IUPAC name: phosphane) is a colorless, flammable, very toxic gas compound with the chemical formula PH3, classed as a pnictogen hydride. Pure phosphine is odorless, but technical grade samples have a highly unpleasant odor like rotting fish, due to the presence of substituted phosphine and diphosphane (P2H4). With traces of P2H4 present, PH3 is spontaneously flammable in air (pyrophoric), burning with a luminous flame. Phosphine is a highly toxic respiratory poison, and is immediately dangerous to life or health at 50 ppm. Phosphine has a trigonal pyramidal structure.

Phosphine is also the general name given to the class of organophosphorus compounds in which one or all of hydrogen atoms in PH3 been replaced with organic derivative, having a general formula PH3−nRn. Organophosphines are important in catalysts.


Philippe Gengembre (1764–1838), a student of Lavoisier, first obtained phosphine in 1783 by heating white phosphorus in an aqueous solution of potash (potassium carbonate).[4][NB 1]

Perhaps because of its strong association with elemental phosphorus, phosphine was once regarded as a gaseous form of the element, but Lavoisier (1789) recognised it as a combination of phosphorus with hydrogen and described it as phosphure d'hydrogène (phosphide of hydrogen).[NB 2]

In 1844, Paul Thénard, son of the French chemist Louis Jacques Thénard, used a cold trap to separate diphosphine from phosphine that had been generated from calcium phosphide, thereby demonstrating that P2H4 is responsible for spontaneous flammability associated with PH3, and also for the characteristic orange/brown color that can form on surfaces, which is a polymerisation product.[5] He considered diphosphine's formula to be PH2, and thus an intermediate between elemental phosphorus, the higher polymers, and phosphine. Calcium phosphide (nominally Ca3P2) produces more P2H4 than other phosphides because of the preponderance of P-P bonds in the starting material.

The name "phosphine" was first used for organophosphorus compounds in 1857, being analogous to organic amines (NR3).[NB 3][6] The gas PH3 was named "phosphine" by 1865 (or earlier).[7]

Structure and properties

PH3 is a trigonal pyramidal molecule with C3v molecular symmetry. The length of the P−H bond is 1.42 Å, the H−P−H bond angles are 93.5°. The dipole moment is 0.58 D, which increases with substitution of methyl groups in the series: CH3PH2, 1.10 D; (CH3)2PH, 1.23 D; (CH3)3P, 1.19 D. In contrast, the dipole moments of amines decrease with substitution, starting with ammonia, which has a dipole moment of 1.47 D. The low dipole moment and almost orthogonal bond angles lead to the conclusion that in PH3 the P−H bonds are almost entirely pσ(P) – sσ(H) and phosphorus 3s orbital contributes little to the bonding between phosphorus and hydrogen in this molecule. For this reason, the lone pair on phosphorus may be regarded as predominantly formed by the 3s orbital of phosphorus. The upfield chemical shift of the phosphorus atom in the 31P NMR spectrum accords with the conclusion that the lone pair electrons occupy the 3s orbital (Fluck, 1973). This electronic structure leads to a lack of nucleophilicity in general and lack of basicity in particular (pKaH = –14),[8] as well as an ability to form only weak hydrogen bonds.[9]

The aqueous solubility of PH3 is slight; 0.22 cm3 of gas dissolves in 1 cm3 of water. Phosphine dissolves more readily in non-polar solvents than in water because of the non-polar P−H bonds. It is technically amphoteric in water, but acid and base activity is poor. Proton exchange proceeds via a phosphonium (PH+4) ion in acidic solutions and via phosphanide (PH2) at high pH, with equilibrium constants Kb = 4×10−28 and Ka = 41.6×10−29.

Phosphine burns producing a dense white cloud of phosphoric acid:

PH3 + 2 O2 → H3PO4

Preparation and occurrence

Phosphine may be prepared in a variety of ways.[10] Industrially it can be made by the reaction of white phosphorus with sodium or potassium hydroxide, producing potassium or sodium hypophosphite as a by-product.

3 KOH + P4 + 3 H2O → 3 KH2PO2 + PH3

Alternatively, the acid-catalyzed disproportionation of white phosphorus yields phosphoric acid and phosphine. Both routes have industrial significance; the acid route is the preferred method if further reaction of the phosphine to substituted phosphines is needed. The acid route requires purification and pressurizing. It can also be made (as described above) by the hydrolysis of a metal phosphide, such as aluminium phosphide or calcium phosphide. Pure samples of phosphine, free from P2H4, may be prepared using the action of potassium hydroxide on phosphonium iodide (PH4I).

Laboratory routes

It is prepared in the laboratory by disproportionation of phosphorous acid[11]

4 H3PO3 → PH3 + 3 H3PO4

Phosphine evolution occurs at around 200 °C. Alternative methods involve the hydrolysis of aluminium phosphide, calcium phosphide, and tris(trimethylsilyl)phosphine.


Phosphine is a constituent of the Earth's atmosphere at very low and highly variable concentrations.[12] It may contribute significantly to the global phosphorus biochemical cycle. The most likely source is reduction of phosphate in decaying organic matter, possibly via partial reductions and disproportionations, since environmental systems do not have known reducing agents of sufficient strength to directly convert phosphate to phosphine.[13]

It is also found in Jupiter's atmosphere.[14]

Possible extraterrestrial biosignature

In 2020 a spectroscopic analysis was reported to show signs of phosphine in the atmosphere of Venus in quantities that could not be explained by known abiotic processes.[15][16][17] Later re-analysis of this work showed interpolation errors had been made, re-analysis of data with the fixed algorithm either do not result in the detection of phosphine[18][19] or detect it with a much lower concentration of 1 ppb.[20]


Organophosphorus chemistry

Phosphine is a precursor to many organophosphorus compounds. It reacts with formaldehyde in the presence of hydrogen chloride to give tetrakis(hydroxymethyl)phosphonium chloride, which is used in textiles. The hydrophosphination of alkenes is versatile route to a variety of phosphines. For example, in the presence of basic catalysts PH3 adds of Michael acceptors. Thus with acrylonitrile, it reacts to give tris(cyanoethyl)phosphine:[21]

PH3 + 3 CH2=CHZ → P(CH2CH2Z)3 (Z is NO2, CN, or C(O)NH2)

Acid catalysis is applicable to hydrophosphination with isobutylene and related analogues:

PH3 + R2C=CH2 → R2(CH3)CPH2 (R is Me, alkyl, etc.)


Phosphine is used as a dopant in the semiconductor industry, and a precursor for the deposition of compound semiconductors. Commercially significant products include gallium phosphide and indium phosphide.[22]


For farm use, pellets of aluminium phosphide, calcium phosphide, or zinc phosphide release phosphine upon contact with atmospheric water or rodents' stomach acid. These pellets also contain agents to reduce the potential for ignition or explosion of the released phosphine. A more recent alternative is the use of phosphine gas itself which requires dilution with either CO2 or N2 or even air to bring it below the flammability point. Use of the gas avoids the issues related with the solid residues left by metal phosphide and results in faster, more efficient control of the target pests.

Because the previously popular fumigant methyl bromide has been phased out in some countries under the Montreal Protocol, phosphine is the only widely used, cost-effective, rapidly acting fumigant that does not leave residues on the stored product. Pests with high levels of resistance toward phosphine have become common in Asia, Australia and Brazil. High level resistance is also likely to occur in other regions, but has not been as closely monitored. Genetic variants that contribute to high level resistance to phosphine have been identified in the dihydrolipoamide dehydrogenase gene.[23] Identification of this gene now allows rapid molecular identification of resistant insects.

Toxicity and safety

Deaths have resulted from accidental exposure to fumigation materials containing aluminium phosphide or phosphine.[24][25][26][27] It can be absorbed either by inhalation or transdermally.[24] As a respiratory poison, it affects the transport of oxygen or interferes with the utilization of oxygen by various cells in the body.[26] Exposure results in pulmonary edema (the lungs fill with fluid).[27] Phosphine gas is heavier than air so stays nearer the floor.[28]

Phosphine appears to be mainly a redox toxin, causing cell damage by inducing oxidative stress and mitochondrial dysfunction.[29] Resistance in insects is caused by a mutation in a mitochondrial metabolic gene.[23]

Phosphine gas is denser than air and hence may collect in low-lying areas. It can form explosive mixtures with air, and may also self-ignite.

Phosphine can be absorbed into the body by inhalation. Direct contact with phosphine liquid – although unlikely to occur – may cause frostbite, like other cryogenic liquids. The main target organ of phosphine gas is the respiratory tract.[30] According to the 2009 U.S. National Institute for Occupational Safety and Health (NIOSH) pocket guide, and U.S. Occupational Safety and Health Administration (OSHA) regulation, the 8 hour average respiratory exposure should not exceed 0.3 ppm. NIOSH recommends that the short term respiratory exposure to phosphine gas should not exceed 1 ppm. The Immediately Dangerous to Life or Health level is 50 ppm. Overexposure to phosphine gas causes nausea, vomiting, abdominal pain, diarrhea, thirst, chest tightness, dyspnea (breathing difficulty), muscle pain, chills, stupor or syncope, and pulmonary edema.[31][32] Phosphine has been reported to have the odor of decaying fish or garlic at concentrations below 0.3 ppm. The smell is normally restricted to laboratory areas or phosphine processing since the smell comes from the way the phosphine is extracted from the environment. However, it may occur elsewhere, such as in industrial waste landfills. Exposure to higher concentrations may cause olfactory fatigue.[33]

See also

  • Diphosphane, H2PPH2, simplified to H4P2
  • Diphosphene, HP=PH


  1. For further information about the early history of phosphine, see:
    • The Encyclopædia Britannica (1911 edition), vol. 21, p. 480: Phosphorus: Phosphine.
    • Thomas Thomson, A System of Chemistry, 6th ed. (London, England: Baldwin, Cradock, and Joy, 1820), vol. 1, p. 272.
  2. Note:
    • On p. 222 of his Traité élémentaire de chimie, vol. 1, (Paris, France: Cuchet, 1789), Lavoisier calls the compound of phosphorus and hydrogen "phosphure d'hydrogène" (hydrogen phosphide). However, on p. 216 , he calls the compound of hydrogen and phosphorus "Combinaison inconnue." (unknown combination), yet in a footnote, he says about the reactions of hydrogen with sulfur and with phosphorus: "Ces combinaisons ont lieu dans l'état de gaz & il en résulte du gaz hydrogène sulfurisé & phosphorisé." (These combinations occur in the gaseous state, and there results from them sulfurized and phosphorized hydrogen gas.)
    • In Robert Kerr's 1790 English translation of Lavoisier's Traité élémentaire de chimie ... — namely, Lavoisier with Robert Kerr, trans., Elements of Chemistry ... (Edinburgh, Scotland: William Creech, 1790) — Kerr translates Lavoisier's "phosphure d'hydrogène" as "phosphuret of hydrogen" (p. 204), and whereas Lavoisier — on p. 216 of his Traité élémentaire de chimie ... — gave no name to the combination of hydrogen and phosphorus, Kerr calls it "hydruret of phosphorus, or phosphuret of hydrogen" (p. 198). Lavoisier's note about this compound — "Combinaison inconnue." — is translated: "Hitherto unknown." Lavoisier's footnote is translated as: "These combinations take place in the state of gas, and form, respectively, sulphurated and phosphorated oxygen gas." The word "oxygen" in the translation is an error because the original text clearly reads "hydrogène" (hydrogen). (The error was corrected in subsequent editions.)
  3. In 1857, August Wilhelm von Hofmann announced the synthesis of organic compounds containing phosphorus, which he named "trimethylphosphine" and "triethylphosphine", in analogy with "amine" (organo-nitrogen compounds), "arsine" (organo-arsenic compounds), and "stibine" (organo-antimony compounds).


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  5. Paul Thénard (1844) "Mémoire sur les combinaisons du phosphore avec l'hydrogène" (Memoir on the compounds of phosphorus with hydrogen), Comptes rendus, 18 : 652–655.
  6. A.W. Hofmann; Auguste Cahours (1857). "Researches on the phosphorus bases". Proceedings of the Royal Society of London (8): 523–527. Retrieved 19 November 2020. "(From page 524:) The bases Me3P and E3P, the products of this reaction, which we propose to call respectively trimethylphosphine and triethylphosphine, ...". 
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  9. Sennikov, P. G. (1994). "Weak H-Bonding by Second-Row (PH3, H2S) and Third-Row (AsH3, H2Se) Hydrides". Journal of Physical Chemistry 98 (19): 4973–4981. doi:10.1021/j100070a006. 
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  13. Roels, J.; Verstraete, W. (2001). "Biological formation of volatile phosphorus compounds, a review paper". Bioresource Technology 79 (3): 243–250. doi:10.1016/S0960-8524(01)00032-3. PMID 11499578. 
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  16. Chu, Jennifer (18 December 2019). "A sign that aliens could stink". MIT News. 
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  18. Snellen, I. A. G.; Guzman-Ramirez, L.; Hogerheijde, M. R.; Hygate, A. P. S.; van der Tak, F. F. S. (2020), "Re-analysis of the 267-GHz ALMA observations of Venus No statistically significant detection of phosphine", Astronomy and Astrophysics 644: L2, doi:10.1051/0004-6361/202039717, Bibcode2020A&A...644L...2S 
  19. Thompson, M. A. (2021), "The statistical reliability of 267 GHz JCMT observations of Venus: No significant evidence for phosphine absorption", Monthly Notices of the Royal Astronomical Society: Letters 501 (1): L18–L22, doi:10.1093/mnrasl/slaa187, Bibcode2021MNRAS.501L..18T 
  20. Greaves, Jane S.; Richards, Anita M. S.; Bains, William; Rimmer, Paul B.; Clements, David L.; Seager, Sara; Petkowski, Janusz J.; Sousa-Silva, Clara et al. (2021), "Reply to: No evidence of phosphine in the atmosphere of Venus from independent analyses", Nature Astronomy 5 (7): 636–639, doi:10.1038/s41550-021-01424-x, Bibcode2021NatAs...5..636G 
  21. Trofimov, Boris A.; Arbuzova, Svetlana N.; Gusarova, Nina K. (1999). "Phosphine in the Synthesis of Organophosphorus Compounds". Russian Chemical Reviews 68 (3): 215–227. doi:10.1070/RC1999v068n03ABEH000464. Bibcode1999RuCRv..68..215T. 
  22. Bettermann, G.; Krause, W.; Riess, G.; Hofmann, T. (2002). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_527. 
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  24. 24.0 24.1 Ido Efrati; Nir Hasson (2014-01-22). "Two toddlers die after Jerusalem home sprayed for pests". Haaretz. 
  25. "La familia de Alcalá de Guadaíra murió tras inhalar fosfina de unos tapones" (in es). Radio y Televisión Española. 2014-02-03. 
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  29. Nath, NS; Bhattacharya, I; Tuck, AG; Schlipalius, DI; Ebert, PR (2011). "Mechanisms of phosphine toxicity". Journal of Toxicology 2011: 494168. doi:10.1155/2011/494168. PMID 21776261. 
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  32. "WHO – Data Sheets on Pesticides – No. 46: Phosphine". 
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Further reading

External links