Selenium oxydichloride

Selenium oxydichloride
Names
IUPAC name
Selenium oxychloride
Other names
Seleninyl chloride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.313
EC Number 232-244-0
RTECS number VS7000000
Properties
SeOCl2
Molar mass 165.87 g/mol
Appearance colorless liquid
Density 2.43 g/cm3, liquid
Melting point 10.9 °C (51.6 °F; 284.0 K)
Boiling point 177.2 °C (351.0 °F; 450.3 K)
1.651 (20 °C)
Structure
trigonal pyramidal
Hazards
R-phrases (outdated) 14-23/25-33-35-50/53
S-phrases (outdated) 26-36/37/39-45-60-61
NFPA 704
Flammability code 0: Will not burn. E.g., waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gasReactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calciumSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
3
1
Lethal dose or concentration (LD, LC):
2 mg/kg (rabbit, dermal)[1]
Related compounds
Related compounds
 SOCl2, POCl3
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Selenium oxydichloride is the inorganic compound with the formula SeOCl2. It is a colorless liquid. With a high dielectric constant (55) and high specific conductance, it is an attractive solvent. Structurally, it is a close chemical relative of thionyl chloride SOCl2, being a pyramidal molecule.

Preparation and reactions

Selenium oxydichloride can be prepared by several methods, and a popular one involves the conversion of selenium dioxide to dichloroselenious acid followed by dehydration:[2]

SeO2 + 2 HCl → Se(OH)2Cl2
Se(OH)2Cl2 → SeOCl2 + H2O

The original synthesis involved the redistribution reaction of selenium dioxide and selenium tetrachloride.

The compound hydrolyzes readily to form hydrogen chloride and selenium dioxide.

See also

References

  1. ↑ "Selenium compounds (as Se)". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  2. ↑ Smith, G. B. L.; Jackson, Julius (1950). "Selenium(IV) Oxychloride". Inorganic Syntheses. 3: 130–137. doi:10.1002/9780470132340.ch34.
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