phosphine

Phosphine
IUPAC name	Phosphane
Other names	Phosphamine Phosphorus trihydride Phosphorated hydrogen
Identifiers
CAS number	7803-51-2 Y
PubChem	24404
EC number	232-260-8
UN number	2199
RTECS number	SY7525000
Properties
Molecular formula	PH3
Molar mass	33.99758 g/mol
Appearance	colorless gas
Density	1.379 g/l, gas (25 °C)
Melting point	-132.8 °C, 140 K, -207 °F
Boiling point	-87.7 °C, 185 K, -126 °F
Solubility in water	31.2 mg/100 ml (17 °C)
Viscosity	1.1 x 10-5 Pa s
Structure
Molecular shape	Trigonal pyramidal
Dipole moment	0.58 D
Hazards
MSDS	ICSC 0694
EU Index	015-181-00-1
EU classification	Highly flammable (F+) Very toxic (T+) Corrosive (C) Dangerous for the environment (N)
R-phrases	R12, R17, R26, R34, R50
S-phrases	(S1/2), S28, S36/37, S45, S61, S63
NFPA 704	4 4 2
Flash point	flammable gas
Autoignition temperature	38 °C (see text)
Related compounds
Other cations	Ammonia Arsine Stibine Bismuthine
Related compounds	Trimethylphosphine Triphenylphosphine
Y (what is this?)  (verify) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Phosphine is the common name for phosphorus trihydride (PH₃), also known by the IUPAC name phosphane and, occasionally, phosphamine. It is a colorless, flammable gas with a boiling point of −88 °C at standard pressure. Pure phosphine is odourless, but technical grade phosphine has a highly unpleasant odor like garlic or rotting fish, due to the presence of substituted phosphine and diphosphine (P₂H₄). Phosphines are also a group of substituted phosphines, with the structure R₃P, where other functional groups replace hydrogens. They are important in catalysts where they complex to various metal ions; a chiral metal phosphine complex can catalyze a reaction to give chiral products. It is sometimes confused with the unrelated chemical phosgene.

Phosphine is highly toxic; it kills at low concentrations. Because of this, the gas is used for pest control by fumigation. For farm use, it is often sold in the form of aluminium phosphide, calcium phosphide, or zinc phosphide pellets, which yield phosphine on contact with atmospheric water or rodents' stomach acid. These pellets also contain other chemicals which evolve ammonia which helps to reduce the potential for spontaneous ignition or explosion of the phosphine gas. They may also contain other agents, such as methanethiol, to give the gas a detectable garlic smell to help warn against its presence in the atmosphere.

Phosphine is also used as a dopant in the semiconductor industry, and a precursor for the deposition of compound semiconductors. Recently high purity tertiary butyl phosphine (TBP) has been developed as a less hazardous liquid alternative to highly toxic phosphine gas, for application in Metalorganic Vapor Phase Epitaxy (MOVPE) of III-V compound semiconductors. Alternatively phosphine can be packaged in a cylinder containing a solid microporous adsorbent at 0 PSIG. The system is called a sub-atmospheric gas source. This type of packaging permits the gas to be stored without pressure which significantly reduces the risk of a phosphine gas leak from the cylinder. The system is able to deliver gas by applying vacuum to the cylinder valve outlet. For semiconductor manufacturing, this is a practical approach as the processes usually operate under high vacuum.

Phosphine is probably a normally occurring constituent of the atmosphere at very low and highly variable concentrations and hence may contribute to the global phosphorus biochemical cycle^[1]. The origin(s) of atmospheric phosphine is not certain. Possible sources include bacterial reduction of phosphate in decaying organic matter, although this is not thermodynamically favorable, and processes related to corrosion of metals containing phosphorus impurities.^[2]

History

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 by describing it as “hydruyet of phosphorus, or phosphuret of hydrogen”^{[citation needed]}.

Ernst von Meyer (1891) described the early history of phosphine research thus: "The discovery of phosphuretted hydrogen (PH₃) by Gengembre in 1783, and the examination of it by Pelletier (who was the first to prepare it pure), only became fruitful after Humphry Davy’s investigations; and the last-named elucidated the composition of this gas, and pointed out its analogy to ammonia, this being emphasised still more sharply by H. Rose later on."^{[citation needed]}

Thénard (1845) 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 colour that can form on surfaces, which is a polymerisation product. 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.

Structure and properties

PH₃ is a trigonal pyramidal molecule with C_3v molecular symmetry. The length of the P-H bond 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 the lone pair contributes only a little to the molecular orbitals. The high positive chemical shift of the P atom in³¹P NMR spectrum accords with the conclusion that the lone pair electrons occupy the 3s orbital and so are close to the P atom (Fluck, 1973). This electronic structure leads to a lack of nucleophilicity and an inability to form hydrogen bonds.

The aqueous solubility of PH₃ is slight; 0.22 mL of gas dissolve in 1 mL of water. Phosphine dissolves more readily in non-polar solvents than in water because of the non-polar P-H bonds. It acts as neither an acid nor a base in water. Proton exchange proceeds via a phosphonium (PH₄⁺) ion in acidic solutions and via PH₂⁻ at high pH, with equilibrium constants K_b = 4 × 10⁻²⁸ and K_z = 41.6 × 10⁻²⁹.

Chemistry

Phosphine may be prepared in a variety of ways.^[3] Industrially it can be made by the reaction of white phosphorus with sodium hydroxide, producing sodium hypophosphite and sodium phosphite as a by-product. Alternatively the acid-catalyzed disproportioning of white phosphorus may be used, which yields phosphoric acid and phosphine. Both routes have industrial significance, with the acid route as the preferred method if further reaction of the phosphine to substituted phosphines is needed. This latter step 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).

Phosphines

Related to PH₃ is the class of organophosphorus compounds commonly called "phosphines." These alkyl and aryl derivatives of phosphine are analogous to organic amines. Common examples include triphenylphosphine ((C₆H₅)₃P) and BINAP, both used as a ligands in homogeneous catalysis or triisopropylphosphine. Phosphines are easily oxidized to phosphine oxides as exemplified by the directed synthesis of a phospha-crown, the phosphorus analogue of an aza crown^[4] where it is not possible to isolate the phosphine itself.^[5]

When modified with suitable substituents as in certain (rare) diazaphospholenes (scheme 3) the polarity of the P-H bond can be inverted (see: umpolung) and the resulting phosphine hydride can reduce a carbonyl group as in the example of benzophenone in yet another way.^[6]

Use as a fumigant

Phosphine is highly toxic to organisms undergoing oxidative respiration, but is non toxic to organisms kept under low oxygen (<1%) or that can anaerobically respire (i.e. ferment). Because of these characteristics, phosphine is widely used as a fumigant of metabolically dormant stored products such as grain. The toxicity of phosphine kills insect pests that might infest the grain, but does not affect the viability of the dormant grain.

Because continued use of the previously widely used fumigant methyl bromide has been banned 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 developing high levels of resistance toward phosphine have become commonplace in many countries of Asia and in Australia as well. Active research into the mode of action of phosphine and the mechanisms whereby insects acquire resistance is being conducted in Australia.

Production during illicit drug manufacturing

During the illicit production of methamphetamine the principal chemicals are ephedrine or pseudoephedrine, iodine, and hypophosphorous acid. Known as the “hypo method,” this method results in a high yield of methamphetamine and usually is used only when red phosphorus or hydriodic acid are in limited supply. This method is particularly dangerous, often resulting in explosions and fires because of the phosphine produced.

See also

• Phosphine oxide, R₃PO
• Phosphorane, R₃PR₂
• Phosphinite, R₂(RO)P
• Phosphonite, R(RO)₂P
• Phosphite, (RO)₃P
• Phosphinate, R₂P(RO)O
• Phosphonate, RP(RO)₂O
• Phosphate, P(RO)₃O

References

External links

• International Chemical Safety Card 0694