Arsine

Arsenic, As   Hydrogen, H
Names
IUPAC names Arsenic trihydride Arsane Trihydridoarsenic
Other names Arseniuretted hydrogen, Arsenous hydride, Hydrogen arsenide Arsenic hydride
Identifiers
CAS Number	7784-42-1 Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:47217 Y
ChEMBL	ChEMBL1231052
ChemSpider	22408 Y
ECHA InfoCard	100.029.151
EC Number	232-066-3
Gmelin Reference	599
KEGG	C06269
PubChem CID	23969
RTECS number	CG6475000
UNII	V1I29R0RJQ Y
UN number	2188
CompTox Dashboard (EPA)	DTXSID3023760
InChI InChI=1S/AsH3/h1H3 Y Key: RBFQJDQYXXHULB-UHFFFAOYSA-N Y InChI=1/AsH3/h1H3 Key: RBFQJDQYXXHULB-UHFFFAOYAH
SMILES [AsH3]
Properties
Chemical formula	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)
Solubility in water	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	Arsonium
Structure
Molecular shape	Trigonal pyramidal
Dipole moment	0.20 D
Thermochemistry
Std molar entropy (S⦵298)	223 J⋅K−1⋅mol−1
Std enthalpy of formation (ΔfH⦵298)	+66.4 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	Extremely toxic, explosive, flammable, potential occupational carcinogen[1]
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H220, H330, H373, H410
Precautionary statements	P210, P260, P271, P273, P284, P304+P340, P310, P314, P320, P377, P381, P391, P403, P403+P233, P405, P501
NFPA 704 (fire diamond)	4 4 2
Flash point	−62 °C (−80 °F; 211 K)
Explosive limits	5.1–78%[1]
Lethal dose or concentration (LD, LC):
LD50 (median dose)	2.5 mg/kg (intravenous)[2]
LC50 (median concentration)	120 ppm (rat, 10 min) 77 ppm (mouse, 10 min) 201 ppm (rabbit, 10 min) 108 ppm (dog, 10 min)[3]
LCLo (lowest published)	250 ppm (human, 30 min) 300 ppm (human, 5 min) 25 ppm (human, 30 min)[3]
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 0.05 ppm (0.2 mg/m3)[1]
REL (Recommended)	C 0.002 mg/m3 [15-minute][1]
IDLH (Immediate danger)	3 ppm[1]
Related compounds
Related hydrides	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). N verify (what is YN ?) Infobox references

Arsine (IUPAC name: arsane) is an inorganic compound with the formula AsH₃. This flammable, pyrophoric, and highly toxic pnictogen hydride gas is one of the simplest compounds of arsenic.^[4] Despite its lethality, it finds some applications in the semiconductor industry and for the synthesis of organoarsenic compounds. The term arsine is commonly used to describe a class of organoarsenic compounds of the formula AsH_3−xR_x, where R = aryl or alkyl. For example, As(C₆H₅)₃, called triphenylarsine, is referred to as "an arsine".

General properties

At its standard state, arsine is a colorless, denser-than-air gas that is slightly soluble in water (20% at 20 °C)^[1] and in many organic solvents as well.^{[citation needed]} Whereas arsine itself is odorless,^[5] owing to its oxidation by air, it is possible to smell a slight garlic or fish-like scent when the compound is present above 0.5 ppm.^[6] This compound is kinetically stable: at room temperature it decomposes only slowly. At temperatures of ca. 230 °C, decomposition to arsenic and hydrogen is sufficiently rapid to be the basis of the Marsh test. Similar to stibine, the decomposition of arsine is autocatalytic, as the arsenic freed during the reaction acts as a catalyst for the same reaction.^[7] Several other factors, such as humidity, presence of light and certain catalysts (namely alumina) facilitate the rate of decomposition.^[8]

AsH₃ is a trigonal pyramidal molecule with H–As–H angles of 91.8° and three equivalent As–H bonds, each of 1.519 Å length.^[9]

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, Carl Scheele reduced arsenic(III) oxide with zinc in the presence of acid.^[11] This reaction is a prelude to the Marsh test.

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 oxidized by concentrated O₂ or the dilute O₂ concentration in air:

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 microelectronics and solid-state lasers. Related to phosphorus, arsenic is an n-dopant for silicon and germanium.^[8] More importantly, AsH₃ is used to make the semiconductor GaAs by chemical vapor deposition (CVD) at 700–900 °C:

Ga(CH₃)₃ + AsH₃ → GaAs + 3 CH₄

For microelectronic applications, arsine can be provided via a sub-atmospheric gas source. In this type of gas package, the arsine is adsorbed on a solid microporous adsorbent inside a gas cylinder. This method allows the gas to be stored without pressure, significantly reducing the risk of an arsine gas leak from the cylinder. With this apparatus, arsine is obtained by applying vacuum to the gas cylinder valve outlet. For semiconductor manufacturing, this method is feasible, as processes such as ion implantation operate under high vacuum.

Chemical warfare

Since before WWII AsH₃ was proposed as a possible chemical warfare weapon. The gas is colorless, almost odorless, and 2.5 times denser than air, as required for a blanketing effect sought in chemical warfare. It is also lethal in concentrations far lower than those required to smell its garlic-like scent. In spite of these characteristics, arsine was never officially used as a weapon, because of its high flammability and its lower efficacy when compared to the non-flammable alternative phosgene. On the other hand, several organic compounds based on arsine, such as lewisite (β-chlorovinyldichloroarsine), adamsite (diphenylaminechloroarsine), Clark 1 (diphenylchloroarsine) and Clark 2 (diphenylcyanoarsine) have been effectively developed for use in chemical warfare.^[17]

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 headaches, vertigo, and nausea, followed by the symptoms of haemolytic anaemia (high levels of unconjugated bilirubin), haemoglobinuria and nephropathy. In severe cases, the damage to the kidneys can be long-lasting.^[1]

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.^[3] Symptoms of poisoning appear after exposure to concentrations of 0.5 ppm. There is little information on the chronic toxicity of arsine, although it is reasonable to assume that, in common with other arsenic compounds, a long-term exposure could lead to arsenicosis.^{[citation needed]}

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 extremely hazardous substance in the United States as defined in Section 302 of the U.S. Emergency Planning and Community Right-to-Know Act (42 U.S.C. 11002), and is subject to strict reporting requirements by facilities which produce, store, or use it in significant quantities.^[22]

Occupational exposure limits