Hydrogen selenide

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Hydrogen selenide
Structural diagram of the hydrogen selenide molecule
Space-filling model of the hydrogen selenide molecule
Names
IUPAC name
Hydrogen selenide
Other names
Hydroselenic acid
selane
selenium hydride
Identifiers
7783-07-5 YesY
ChEBI CHEBI:16503 YesY
ChemSpider 518 YesY
Jmol-3D images Image
KEGG C01528 YesY
PubChem 533
RTECS number X1050000
UN number 2202
Properties
H2Se
Molar mass 80.98 g/mol
Appearance Colorless gas
Odor horseradish
Density 3.553 g/cm3
Melting point −65.73 °C (−86.31 °F; 207.42 K)
Boiling point −41.25 °C (−42.25 °F; 231.90 K)
0.70 g/100 mL
Solubility soluble in CS2, phosgene
Acidity (pKa) 3.89
Structure
Molecular shape Bent
Hazards
MSDS ICSC 0284
EU Index 034-002-00-8
EU classification Highly Flammable (F+)
Toxic (T)
Dangerous for the environment (N)
R-phrases R23/25, R33, R50/53
S-phrases (S1/2), S20/21, S28, S45, S60, S61
NFPA 704
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., propane Health code 4: Very short exposure could cause death or major residual injury. E.g., VX gas Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Flash point flammable gas
Related compounds
Other anions
H2O
H2S
H2Te
H2Po
Other cations
Na2Se
Ag2Se
Related compounds
Arsine
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Hydrogen selenide is an inorganic compound with the formula H2Se. It is the simplest (and virtually the only) hydride of selenium. H2Se is a colorless, flammable gas under standard conditions. It is the most toxic selenium compound[1] with an exposure limit of 0.05 ppm over an 8 hour period.[2][3] Even at extremely low concentrations this compound has a very irritating smell resembling that of decayed horseradish or 'leaking gas', but smells of rotten eggs at higher concentrations.

Structure and properties[edit]

H2Se adopts a "bent" structure with a H-Se-H bond angle of 91°. Consistent with this structure, three IR-active vibrational bands are observed: 2358, 2345, and 1034 cm−1.

The properties of H2S and H2Se are similar, although the selenide is more acidic with pKa = 3.89, and the second pKa = 11.0 at 25 °C. Reflecting its acidity, H2Se is soluble in water.

Preparation[edit]

Industrially, it is produced by treating elemental selenium at T > 300 °C with hydrogen gas.[4] A number of routes to H2Se have been reported, which are suitable for both large and small scale preparations. In the laboratory, H2Se is usually prepared by the action of water on Al2Se3, concomitant with formation of hydrated alumina. A related reaction involves the acid hydrolysis of FeSe.[5]

Al2Se3 + 6 H2O 2 Al(OH)3 + 3 H2Se

H2Se can also be prepared by means of different methods based on the in situ generation in aqueous solution using boron hydride, Marsh test and Devarda's alloy. According to the Sonoda method, H2Se is generated from the reaction of H2O and CO on Se in the presence of Et3N.[6] H2Se can be purchased in cylinders.

Reactions[edit]

Elemental selenium can be recovered from H2Se through a reaction with aqueous sulfur dioxide (SO2).

2 H2Se + SO2 2 H2O + Se + S

Its decomposition is used to prepare highly pure Se metal.

Applications[edit]

H2Se is commonly used in the synthesis of Se-containing compounds. It adds across alkenes. Illustrative is the synthesis of selenoureas from cyanamides.[7]

Selenourea reaction

H2Se gas is used to dope semiconductors with selenium.

Safety[edit]

Hydrogen selenide is hazardous, being the most toxic selenium compound[1] and far more toxic than its congener hydrogen sulfide. The threshold limit value is 0.05 ppm. The gas acts as an irritant at concentrations higher than 0.3 ppm, which is the main warning sign of exposure; below 1 ppm, this is "insufficient to prevent exposure", while at 1.5 ppm the irritation is "intolerable".[3] Exposure at high concentrations, even for less than a minute, causes the gas to attack the eyes and mucous membranes; this causes cold-like symptoms for at least a few days afterwards. In Germany, the limit in drinking water is 0.008 mg/L, and the US EPA recommends a maximum contamination of 0.01 mg/L.[4][8]

Despite being highly toxic, no human fatalities have yet been reported. It is suspected that this is due to the gas' tendency to oxidise to form red selenium in mucous membranes; elemental selenium is less toxic than selenides are.[2]

References[edit]

  1. ^ a b http://www.epa.gov/ttnatw01/hlthef/selenium.html, US Environmental Protection Agency, Air Toxins website
  2. ^ a b http://www.cdc.gov/niosh/idlh/7783075.html, Documentation of Immediately Dangerous to Life or Health Concentrations: Hydrogen Selenide, The National Institute for Occupational Safety and Health
  3. ^ a b http://www.cdc.gov/niosh/docs/81-123/pdfs/0336.pdf Occupational Health Guideline for Hydrogen Selenide, The National Institute for Occupational Safety and Health, 1978
  4. ^ a b Bernd E. Langner "Selenium and Selenium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a23_525.
  5. ^ Féher, F. In "Handbook of Preparative Inorganic Chemistry"; Brauer, E., Ed.; Academic: New York, 1963; 1, p 418.
  6. ^ Sonoda, N.; Kondo K.; Nagano, K.; Kambe, N.; Morimoto, F. Angewandte Chemie, International Edition English 1980, vol. 19, page 308
  7. ^ V.I. Cohen "A Convenient Synthesis of Mono-, N,N′-Di-, and Trisubstituted Selenoureas from Methyl Carbamimidothioates (S-Methylpseudothioureas)" Synthesis, 1980, 60-3 (1980).
  8. ^ http://www.osha.gov/dts/chemicalsampling/data/CH_246700.html, OSHA GENERAL INDUSTRY PEL: 0.05 ppm, 0.2 mg/m3 ,OSHA CONSTRUCTION INDUSTRY PEL: 0.05 ppm, 0.2 mg/m3 TWA

External links[edit]