Arsine
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Names | |||
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IUPAC names
Arsenic trihydride
Arsane Trihydridoarsenic | |||
Other names
Arseniuretted hydrogen,
Arsenous hydride, Hydrogen arsenide Arsenic hydride | |||
Identifiers | |||
3D model (
JSmol ) |
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ChEBI | |||
ChEMBL | |||
ChemSpider | |||
ECHA InfoCard
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100.029.151 | ||
EC Number |
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599 | |||
KEGG | |||
PubChem CID
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RTECS number
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UNII | |||
UN number | 2188 | ||
CompTox Dashboard (EPA)
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Properties | |||
AsH3 | |||
Molar mass | 77.9454 g/mol | ||
Appearance | Colourless gas | ||
Odor | Faint, garlic-like | ||
Density | 4.93 g/L, gas; 1.640 g/mL (−64 °C) | ||
Melting point | −111.2 °C (−168.2 °F; 162.0 K) | ||
Boiling point | −62.5 °C (−80.5 °F; 210.7 K) | ||
0.2 g/100 mL (20 °C)[1] 0.07 g/100 mL (25 °C) | |||
Solubility | soluble in chloroform, benzene | ||
Vapor pressure | 14.9 atm[1] | ||
Conjugate acid
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Arsonium | ||
Structure | |||
Trigonal pyramidal | |||
0.20 D | |||
Thermochemistry | |||
Std molar
entropy (S⦵298) |
223 J⋅K−1⋅mol−1 | ||
Std enthalpy of (ΔfH⦵298)formation |
+66.4 kJ/mol | ||
Hazards | |||
Occupational safety and health (OHS/OSH): | |||
Main hazards
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Extremely toxic, explosive, flammable, potential occupational carcinogen[1] | ||
GHS labelling: | |||
Danger | |||
H220, H330, H373, H410 | |||
P210, P260, P271, P273, P284, P304+P340, P310, P314, P320, P377, P381, P391, P403, P403+P233, P405, P501 | |||
NFPA 704 (fire diamond) | |||
Flash point | −62 °C (−80 °F; 211 K) | ||
Explosive limits
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5.1–78%[1] | ||
Lethal dose or concentration (LD, LC): | |||
LD50 (median dose)
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2.5 mg/kg (intravenous)[2] | ||
LC50 (median concentration)
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LCLo (lowest published)
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NIOSH (US health exposure limits): | |||
PEL (Permissible)
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TWA 0.05 ppm (0.2 mg/m3)[1] | ||
REL (Recommended)
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C 0.002 mg/m3 [15-minute][1] | ||
IDLH (Immediate danger) |
3 ppm[1] | ||
Related compounds | |||
Related hydrides
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Ammonia; phosphine; stibine; bismuthine | ||
Supplementary data page | |||
Arsine (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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Arsine (
General properties
In its standard state arsine is a colorless, denser-than-air gas that is slightly soluble in
AsH3 is a
Discovery and synthesis
AsH3 is generally prepared by the reaction of As3+ sources with H− equivalents.[10]
- 4 AsCl3 + 3 NaBH4 → 4 AsH3 + 3 NaCl + 3 BCl3
As reported in 1775,
Alternatively, sources of As3− react with protonic reagents to also produce this gas. Zinc arsenide and sodium arsenide are suitable precursors:[12]
- Zn3As2 + 6 H+ → 2 AsH3 + 3 Zn2+
- Na3As + 3 HBr → AsH3 + 3 NaBr
Reactions
The understanding of the chemical properties of AsH3 is well developed and can be anticipated based on an average of the behavior of pnictogen counterparts, such as PH3 and SbH3.
Thermal decomposition
Typical for a heavy hydride (e.g., SbH3, H2Te, SnH4), AsH3 is unstable with respect to its elements. In other words, AsH3 is stable kinetically but not thermodynamically.
- 2 AsH3 → 3 H2 + 2 As
This decomposition reaction is the basis of the Marsh test, which detects the elemental As.
Oxidation
Continuing the analogy to SbH3, AsH3 is readily
- 2 AsH3 + 3 O2 → As2O3 + 3 H2O
Arsine will react violently in presence of strong oxidizing agents, such as potassium permanganate, sodium hypochlorite, or nitric acid.[8]
Precursor to metallic derivatives
AsH3 is used as a precursor to metal complexes of "naked" (or "nearly naked") arsenic. An example is the dimanganese species [(C5H5)Mn(CO)2]2AsH, wherein the Mn2AsH core is planar.[13]
Gutzeit test
A characteristic test for arsenic involves the reaction of AsH3 with Ag+, called the Gutzeit test for arsenic.[14] Although this test has become obsolete in analytical chemistry, the underlying reactions further illustrate the affinity of AsH3 for "soft" metal cations. In the Gutzeit test, AsH3 is generated by reduction of aqueous arsenic compounds, typically arsenites, with Zn in the presence of H2SO4. The evolved gaseous AsH3 is then exposed to AgNO3 either as powder or as a solution. With solid AgNO3, AsH3 reacts to produce yellow Ag4AsNO3, whereas AsH3 reacts with a solution of AgNO3 to give black Ag3As.
Acid-base reactions
The acidic properties of the As–H bond are often exploited. Thus, AsH3 can be deprotonated:
- AsH3 + NaNH2 → NaAsH2 + NH3
Upon reaction with the aluminium trialkyls, AsH3 gives the trimeric [R2AlAsH2]3, where R = (CH3)3C.[15] This reaction is relevant to the mechanism by which GaAs forms from AsH3 (see below).
AsH3 is generally considered non-basic, but it can be protonated by superacids to give isolable salts of the tetrahedral species [AsH4]+.[16]
Reaction with halogen compounds
Reactions of arsine with the halogens (fluorine and chlorine) or some of their compounds, such as nitrogen trichloride, are extremely dangerous and can result in explosions.[8]
Catenation
In contrast to the behavior of PH3, AsH3 does not form stable chains, although diarsine (or diarsane) H2As–AsH2, and even triarsane H2As–As(H)–AsH2 have been detected. The diarsine is unstable above −100 °C.
Applications
Microelectronics applications
AsH3 is used in the synthesis of semiconducting materials related to
- Ga(CH3)3 + AsH3 → GaAs + 3 CH4
For microelectronic applications, arsine can be provided via a
Chemical warfare
Since before
Forensic science and the Marsh test
AsH3 is also well known in forensic science because it is a chemical intermediate in the detection of arsenic poisoning. The old (but extremely sensitive) Marsh test generates AsH3 in the presence of arsenic.[4] This procedure, published in 1836 by James Marsh,[18] is based upon treating an As-containing sample of a victim's body (typically the stomach contents) with As-free zinc and dilute sulfuric acid: if the sample contains arsenic, gaseous arsine will form. The gas is swept into a glass tube and decomposed by means of heating around 250–300 °C. The presence of As is indicated by formation of a deposit in the heated part of the equipment. On the other hand, the appearance of a black mirror deposit in the cool part of the equipment indicates the presence of antimony (the highly unstable SbH3 decomposes even at low temperatures).
The Marsh test was widely used by the end of the 19th century and the start of the 20th; nowadays more sophisticated techniques such as atomic spectroscopy, inductively coupled plasma, and x-ray fluorescence analysis are employed in the forensic field. Though neutron activation analysis was used to detect trace levels of arsenic in the mid 20th century, it has since fallen out of use in modern forensics.
Toxicology
The toxicity of arsine is distinct from that of other arsenic compounds. The main route of exposure is by inhalation, although poisoning after skin contact has also been described. Arsine attacks hemoglobin in the red blood cells, causing them to be destroyed by the body.[19][20]
The first signs of exposure, which can take several hours to become apparent, are
Exposure to arsine concentrations of 250 ppm is rapidly fatal: concentrations of 25–30 ppm are fatal for 30 min exposure, and concentrations of 10 ppm can be fatal at longer exposure times.
Arsine can cause pneumonia in two different ways either the "extensive edema of the acute stage may become diffusely infiltrated with polymorphonuclear leucocytes, and the edema may change to ringed with leucocytes, their epithelium degenerated, their walls infiltrated, and each bronchiole the center of a small focus or nodule of pneumonic consolidation", and In the second Case "the areas involved are practically always the anterior tips of the middle and upper lobes, while the posterior portions of these lobes and the whole of the lower lobes present an air-containing and emphysematous condition, sometimes with slight congestion, sometimes with none." which can result in death.[21]
It is classified as an
Occupational exposure limits
Country | Limit[23] |
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Argentina | Confirmed human carcinogen |
Australia | TWA 0.05 ppm (0.16 mg/m3) |
Belgium | TWA 0.05 ppm (0.16 mg/m3) |
Bulgaria | Confirmed human carcinogen |
British Columbia, Canada
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TWA 0.005 ppm (0.02 mg/m3) |
Colombia | Confirmed human carcinogen |
Denmark | TWA 0.01 ppm (0.03 mg/m3) |
Egypt | TWA 0.05 ppm (0.2 mg/m3) |
France |
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Hungary | TWA 0.2 mg/m3STEL 0.8 mg/m3 |
Japan |
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Jordan | Confirmed human carcinogen |
Mexico | TWA 0.05 ppm (0.2 mg/m3) |
Netherlands | MAC-TCG 0.2 mg/m3 |
New Zealand | TWA 0.05 ppm (0.16 mg/m3) |
Norway | TWA 0.003 ppm (0.01 mg/m3) |
Philippines | TWA 0.05 ppm (0.16 mg/m3) |
Poland | TWA 0.2 mg/m3 STEL 0.6 mg/m3 |
Russia | STEL 0.1 mg/m3 |
Singapore | Confirmed human carcinogen |
South Korea | TWA 0.05 ppm (0.2 mg/m3) |
Sweden | TWA 0.02 ppm (0.05 mg/m3) |
Switzerland | MAK-week 0.05 ppm (0.16 mg/m3) |
Thailand | TWA 0.05 ppm (0.2 mg/m3) |
Turkey | TWA 0.05 ppm (0.2 mg/m3) |
United Kingdom | TWA 0.05 ppm (0.16 mg/m3) |
United States | 0.05 ppm (0.2 mg/m3) |
Vietnam | Confirmed human carcinogen |
See also
- Cacodylic acid
- Cacodyl oxide
- Devarda's alloy, also used to produce arsine in the lab
- List of highly toxic gases
- Scheele's Green, a pigment popularly used in the early 19th century
References
- ^ a b c d e f g h i NIOSH Pocket Guide to Chemical Hazards. "#0040". National Institute for Occupational Safety and Health (NIOSH).
- PMID 19108099.
- ^ a b c "Arsine". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
- ^ ISBN 0-12-352651-5.
- ISBN 978-0-08-045043-8.
While arsine itself is odourless, its oxidation by air may produce a slight, garlic-like scent. However, it is lethal in concentrations far lower than those required to produce this smell.
- ^ "Medical Management Guidelines for Arsine (AsH3)". Agency for Toxic Substances & Disease Registry. Archived from the original on January 24, 2012.
- ^ Hartman, Robert James (1947). Briscoe, Herman Thompson (ed.). Colloid Chemistry (2 ed.). Houghton Mifflin Company. p. 124.
- ^ a b c d Institut National de Recherche et de Sécurité (2000). Fiche toxicologique nº 53: Trihydrure d'arsenic (PDF) (Report) (in French). Archived from the original (PDF) on 2006-11-26. Retrieved 2006-09-06.
- .
- .
- ^ Scheele, Carl Wilhelm (1775) "Om Arsenik och dess syra" Archived 2016-01-05 at the Wayback Machine (On arsenic and its acid), Kongliga Vetenskaps Academiens Handlingar (Proceedings of the Royal Scientific Academy [of Sweden]), 36: 263-294. From p. 290: "Med Zinck. 30. (a) Denna år den endaste af alla så hela som halfva Metaller, som i digestion met Arsenik-syra effervescerar." (With zinc. 30. (a) This is the only [metal] of all whole- as well as semi-metals that effervesces on digestion with arsenic acid.) Scheele collected the arsine and put a mixture of arsine and air into a cylinder. From p. 291: "3:0, Då et tåndt ljus kom når o̊pningen, tåndes luften i kolfven med en småll, lågan for mot handen, denna blef o̊fvedragen med brun fårg, ... " (3:0, Then as [the] lit candle came near the opening [of the cylinder], the gases in [the] cylinder ignited with a bang; [the] flame [rushed] towards my hand, which became coated with [a] brown color, ... )
- ^ "Arsine" in Handbook of Preparative Inorganic Chemistry, 2nd ed., G. Brauer (ed.), Academic Press, 1963, NY, Vol. 1. p. 493.
- .
- ^ King, E. J. (1959) Qualitative Analysis and Electrolytic Solutions Harcourt, Brace, and World; New York
- .
- .
- ^ Suchard, Jeffrey R. (March 2006). "CBRNE — Arsenicals, Arsine". EMedicine. Archived from the original on 2006-06-23. Retrieved 2006-09-05.
- ^ Marsh, James (1836). "Account of a method of separating small quantities of arsenic from substances with which it may be mixed". Edinburgh New Philosophical Journal. 21: 229–236.
- PMID 4608634.
- PMID 8598571.
- ^ "Collected Studies on the Pathology of War Gas Poisoning, from the Department of Bacteriology and Pathology, Medical Science Section, Chemical Warfare Service, under the direction of M. C. Winternitz, major, M. C., U. S. A. Yale University Press". books.google.com. Yale University press. 1920. Retrieved 28 September 2022.
- ^ 40 C.F.R.: Appendix A to Part 355—The List of Extremely Hazardous Substances and Their Threshold Planning Quantities (PDF) (Report) (July 1, 2008 ed.). Government Printing Office. Archived from the original (PDF) on February 25, 2012. Retrieved October 29, 2011.
- ^ "Arsine". RTECS. National Institute for Occupational Safety and Health (NIOSH). Archived from the original on 2017-06-08. Retrieved 2017-09-08.
External links
- International Chemical Safety Card 0222
- IARC Monograph "Arsenic and Arsenic Compounds"
- NIOSH Pocket Guide to Chemical Hazards
- Institut national de recherche et de sécurité (2000). "Trihydrure d'arsenic." Fiche toxicologique n° 53. Paris:INRS. (in French)
- Data on arsine from Air Liquide