Phosphine

Source: Wikipedia, the free encyclopedia.
This article is about PH3. For organic derivatives, see Organophosphine. For the visual phenomenon, see phosphene. For the star, see Kepler-289.
Not to be confused with Phosgene.

Phosphine
Skeletal formula of phosphine
Ball-and-stick model of phosphine
Ball-and-stick model of phosphine
Spacefill model of phosphine
Spacefill model of phosphine
  Phosphorus, P
  Hydrogen, H
Names
IUPAC name
Phosphane
Other names
Hydrogen phosphide
Phosphamine
Phosphorus trihydride
Phosphorated hydrogen
Identifiers
3D model (
JSmol
)
ChEBI
ChemSpider
ECHA InfoCard
 100.029.328 Edit this at Wikidata
EC Number
  • 232-260-8
287
RTECS number
  • SY7525000
UNII
UN number 2199
  • InChI=1S/H3P/h1H3 checkY
    Key: XYFCBTPGUUZFHI-UHFFFAOYSA-N checkY
  • InChI=1/H3P/h1H3
    Key: XYFCBTPGUUZFHI-UHFFFAOYAP
  • P
Properties
PH3
Molar mass 33.99758 g/mol
Appearance Colourless gas
Odor odorless as pure compound; fish-like or garlic-like commercially[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/100 ml (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)
2.144
Viscosity 1.1×10−5 Pa⋅s
Structure
Trigonal pyramidal
0.58 D
Thermochemistry
37 J/mol⋅K
210 J/mol⋅K[2]
Std enthalpy of
formation
(ΔfH⦵298)
 5 kJ/mol[2]
13 kJ/mol
Hazards
GHS labelling:
GHS02: Flammable GHS06: Toxic GHS05: Corrosive GHS09: Environmental hazard
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 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. propaneInstability 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 code
4
4
2
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]
Safety data sheet (SDS) ICSC 0694
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).
checkY verify (what is checkY☒N ?)

Phosphine (

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.

Phosphines are compounds that include PH3 and the organophosphines, which are derived from PH3 by substituting one or more hydrogen atoms with organic groups.[4] They have the general formula PH3−nRn. Phosphanes are saturated phosphorus hydrides of the form PnHn+2, such as triphosphane.[5] Phosphine, PH3, is the smallest of the phosphines and the smallest of the phosphanes.

History

Philippe Gengembre (1764–1838), a student of

white phosphorus in an aqueous solution of potash (potassium carbonate).[6][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.[7] 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][8] The gas PH3 was named "phosphine" by 1865 (or earlier).[9]

Structure and reactions

PH3 is a

hydrogen bonds.[11]

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 (PH−2) at high pH, with equilibrium constants Kb = 4×10−28 and Ka = 41.6×10−29. Phosphine reacts with water only at high pressure and temperature, producing phosphoric acid and hydrogen:[12][13]

PH3 + 4H2O pressure & temperature→H3PO4 + 4H2

Burning phosphine in the air produces phosphoric acid):[14][12]

2 PH3 + 4 O2 → 2 H3PO4

Preparation and occurrence

Phosphine may be prepared in a variety of ways.[15] 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
3 NaOH + P4 + 3 H2O → 3 NaH2PO2 + 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.

Laboratory routes

It is prepared in the laboratory by disproportionation of phosphorous acid:[16]

4 H3PO3 → PH3 + 3 H3PO4 Phosphine evolution occurs at around 200 °C.

Alternative methods are the hydrolysis of tris(trimethylsilyl)phosphine, or of metal phosphides such as aluminium phosphide, or calcium phosphide:

Ca3P2 + 6 H2O → 3 Ca(OH)2 + 2 PH3

Pure samples of phosphine, free from P2H4, may be prepared using the action of potassium hydroxide on phosphonium iodide:

[PH4]I + KOH → PH3 + KI + H2O

Occurrence

Phosphine is a worldwide constituent of the Earth's atmosphere at very low and highly variable concentrations.

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.[18]

It is also found in Jupiter's atmosphere.[19]

Possible extraterrestrial biosignature

See also: Life on Venus

In 2020 a spectroscopic analysis was reported to show signs of phosphine in the

disputed – discuss
]

Applications

Organophosphorus chemistry

Phosphine is a precursor to many

Michael acceptors. Thus with acrylonitrile, it reacts to give tris(cyanoethyl)phosphine:[26]

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

where R is CH3, alkyl, etc.

Microelectronics

Phosphine is used as a

compound semiconductors. Commercially significant products include gallium phosphide and indium phosphide.[27]

Fumigant (pest control)

See also: Fumigation

Phosphine is an attractive fumigant because it is lethal to insects and rodents, but degrades to phosphoric acid, which is non-toxic. As sources of phosphine, for farm use, pellets of aluminium phosphide (AlP), calcium phosphide (Ca
3P
2), or zinc phosphide (Zn
3P
2) are used. These phosphides release phosphine upon contact with atmospheric water or rodents' stomach acid. These pellets also contain reagents to reduce the potential for ignition or explosion of the released phosphine.

An 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.

One problem with phosphine fumigants is the increased resistance by insects.[28]

Toxicity and safety

Further information: Aluminium phosphide poisoning
See also: White phosphorus munitions

Deaths have resulted from accidental exposure to fumigation materials containing aluminium phosphide or phosphine.[29][30][31][32] It can be absorbed either by inhalation or transdermally.[29] As a respiratory poison, it affects the transport of oxygen or interferes with the utilization of oxygen by various cells in the body.[31] Exposure results in pulmonary edema (the lungs fill with fluid).[32] Phosphine gas is heavier than air so it stays near the floor.[33]

Phosphine appears to be mainly a redox toxin, causing cell damage by inducing oxidative stress and mitochondrial dysfunction.[34] Resistance in insects is caused by a mutation in a mitochondrial metabolic gene.[28]

Phosphine can be absorbed into the body by inhalation. The main target organ of phosphine gas is the respiratory tract.

dyspnea (breathing difficulty), muscle pain, chills, stupor or syncope, and pulmonary edema.[36][37] 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.[38]

Fumigation hazards

Phosphine is used for pest control, but its usage is strictly regulated due to high toxicity.[39][40] Gas from phosphine has high mortality rate[41] and has caused deaths in Sweden and other countries.[42][43][44]

Because the previously popular

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.[28]
Identification of this gene now allows rapid molecular identification of resistant insects.

Explosiveness

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.[12]

In popular culture

In the 2008 pilot of the crime drama television series Breaking Bad, Walter White poisons two rival gangsters by adding red phosphorus to boiling water to produce phosphine gas. However, this reaction in reality would require white phosphorus instead, and for the water to contain sodium hydroxide.[45] An episode of Homicide: Life on the Street depicted a murder suspect who adulterated beverages, including Sacramental wine, with a poison called "Phosphozine."

See also

Notes

  1. ^ For further information about the early history of phosphine, see:
  2. ^ Note:
    • On p. 222 Archived 24 April 2017 at the Wayback Machine 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 Archived 24 April 2017 at the Wayback Machine, 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).

References

  1. ^ a b c d e f NIOSH Pocket Guide to Chemical Hazards. "#0505". National Institute for Occupational Safety and Health (NIOSH).
  2. ^
    ISBN 978-0-618-94690-7
    .
  3. ^ a b "Phosphine". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  4. doi:10.1351/goldbook.P04553
  5. doi:10.1351/goldbook.P04548
  6. ^ Gengembre (1783) "Mémoire sur un nouveau gas obtenu, par l'action des substances alkalines, sur le phosphore de Kunckel" (Memoir on a new gas obtained by the action of alkaline substances on Kunckel's phosphorus), Mémoires de mathématique et de physique, 10 : 651–658.
  7. ^ Paul Thénard (1844) "Mémoire sur les combinaisons du phosphore avec l'hydrogène" Archived 15 October 2015 at the Wayback Machine (Memoir on the compounds of phosphorus with hydrogen), Comptes rendus, 18 : 652–655.
  8. ^ A.W. Hofmann; Auguste Cahours (1857). "Researches on the phosphorus bases". Proceedings of the Royal Society of London (8): 523–527. Archived from the original on 10 February 2022. 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, ...
  9. ^ William Odling, A Course of Practical Chemistry Arranged for the Use of Medical Students, 2nd ed. (London, England: Longmans, Green, and Co., 1865), pp. 227, 230.
  10. ISBN 9789385998898
    .
  11. doi:10.1021/j100070a006
    .
  12. ^ a b c Material Safety Data Sheet: Phosphine/hydrogen Gas Mixture (PDF) (Report). Matheson Tri-Gas. 8 September 2008. Archived from the original (PDF) on 5 July 2022. Retrieved 4 July 2022.
  13. S2CID 4195473
    .
  14. ^ "Phosphine: Lung Damaging Agent". United States: National Institute for Occupational Safety and Health (NIOSH). 8 July 2021. Retrieved 4 July 2022.
  15. ^ Toy, A. D. F. (1973). The Chemistry of Phosphorus. Oxford, UK: Pergamon Press.
  16. ISBN 978-0-470-13168-8
    .
  17. S2CID 32611695
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  18. PMID 11499578
    .
  19. ^ Kaplan, Sarah (11 July 2016). "The first water clouds are found outside our solar system – around a failed star". The Washington Post. Archived from the original on 15 September 2020. Retrieved 14 September 2020.
  20. S2CID 204401807
    .
  21. ^ Chu, Jennifer (18 December 2019). "A sign that aliens could stink". MIT News. Archived from the original on 18 February 2021. Retrieved 14 September 2020.
  22. ^ "Phosphine Could Signal Existence of Alien Anaerobic Life on Rocky Planets". Sci-News. 26 December 2019. Archived from the original on 14 September 2020. Retrieved 15 September 2020.
  23. S2CID 224803085
    .
  24. S2CID 225103303
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  25. S2CID 233296859
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  26. S2CID 250775640
    .
  27. ISBN 978-3527306732
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  28. ^
    S2CID 10390339
    .
  29. ^ a b Ido Efrati; Nir Hasson (22 January 2014). "Two toddlers die after Jerusalem home sprayed for pests". Haaretz. Archived from the original on 23 January 2014. Retrieved 23 January 2014.
  30. ^ "La familia de Alcalá de Guadaíra murió tras inhalar fosfina de unos tapones". RTVE.es (in Spanish). Radio y Televisión Española. EFE. 3 February 2014. Archived from the original on 2 March 2014. Retrieved 23 July 2014.
  31. ^ a b Julia Sisler (13 March 2014). "Deaths of Quebec women in Thailand may have been caused by pesticide". CBC News. Archived from the original on 4 April 2017. Retrieved 3 April 2017.
  32. ^ a b Amy B Wang (3 January 2017). "4 children killed after pesticide released toxic gas underneath their home, police say". Washington Post. Archived from the original on 25 June 2018. Retrieved 6 January 2017.
  33. ^ "Pesticide blamed in 8-month-old's death in Fort McMurray". CBC News. 23 February 2015. Archived from the original on 24 February 2015. Retrieved 23 February 2015.
  34. PMID 21776261
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  35. ^ "NIOSH Emergency Response Card". CDC. Archived from the original on 2 October 2017. Retrieved 6 April 2010.
  36. ^ "NIOSH pocket guide". CDC. 3 February 2009. Archived from the original on 11 May 2017. Retrieved 6 April 2010.
  37. ^ "WHO – Data Sheets on Pesticides – No. 46: Phosphine". Inchem.org. Archived from the original on 18 February 2010. Retrieved 6 April 2010.
  38. doi:10.26616/nioshpub99126. Archived
    from the original on 19 June 2017. Retrieved 6 April 2010.
  39. ^ Wallstén, Beata (13 February 2024). "Åklagaren bekräftar: Familjen i Söderhamn förgiftades av fosfin". DN.se (in Swedish). Archived from the original on 13 February 2024. Retrieved 13 February 2024.
  40. ^ European Agency for Safety and Health at Work. "Hälsorisker och förebyggande rutiner vid hantering av fumigerade containrar" (PDF). Archived from the original (PDF) on 13 February 2024. Retrieved 13 February 2024.
  41. PMID 34871510
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  42. ^ Nyheter, S. V. T. (13 February 2024). "Giftgåtan i Söderhamn: Gas tros ha dödat flickan". SVT Nyheter (in Swedish). Archived from the original on 13 February 2024. Retrieved 13 February 2024.
  43. PMID 10408124
    . Retrieved 13 February 2024.
  44. PMID 37438888
    .
  45. ^ Hare, Jonathan (1 March 2011). "Breaking Bad – poisoning gangsters with phosphine gas". education in chemistry. Royal Society of Chemistry. Archived from the original on 24 September 2023.

Further reading

External links

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