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Selenium oxydichloride

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Selenium oxydichloride
Structure of the selenium oxydichloride molecule
Structure of the selenium oxydichloride molecule
3D model of the selenium oxydichloride molecule
3D model of the selenium oxydichloride molecule
Names
IUPAC name
Selenium oxychloride
Other names
Seleninyl chloride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.313 Edit this at Wikidata
EC Number
  • 232-244-0
RTECS number
  • VS7000000
UNII
  • InChI=1S/Cl2OSe/c1-4(2)3 ☒N
    Key: LIRMPIXWGWLNND-UHFFFAOYSA-N ☒N
  • InChI=1/Cl2OSe/c1-4(2)3
    Key: LIRMPIXWGWLNND-UHFFFAOYAX
  • O=[Se](Cl)Cl
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
GHS labelling:[2]
GHS05: CorrosiveGHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard
Warning
H301, H314, H331, H373, H410
P260, P261, P264, P270, P271, P273, P280, P301+P310, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P311, P314, P321, P330, P363, P391, P403+P233, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
3
0
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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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

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Selenium oxydichloride can be prepared by several methods, and a common one involves the conversion of selenium dioxide to dichloroselenious acid followed by dehydration:[3]

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

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

Pure selenium oxydichloride autoionizes to a dimer:[4]

SeOCl2 ↔ (SeO)2Cl+
3 + Cl−

The SeOCl2 is generally a labile Lewis acid and solutions of sulfur trioxide in SeOCl2 likely form [SeOCl]+[SO3Cl]− the same way.[5]

The compound hydrolyzes readily to form hydrogen chloride and selenium dioxide,[citation needed] and very few organic compounds dissolve in it without reaction. At elevated temperatures, it is a strong oxidizer, yielding a chloride, selenium dioxide, and diselenium dichloride.[6]

See also

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References

[edit]
  1. ^ "Selenium compounds (as Se)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  2. ^ "Selenium oxychloride". pubchem.ncbi.nlm.nih.gov. Retrieved 12 December 2021.
  3. ^ Smith, G. B. L.; Jackson, Julius (1950). "Selenium(IV) Oxychloride". Inorganic Syntheses. Vol. 3. pp. 130–137. doi:10.1002/9780470132340.ch34. ISBN 9780470132340.
  4. ^ Audrieth & Kleinberg 1953, p. 237.
  5. ^ Audrieth & Kleinberg 1953, pp. 239–242.
  6. ^ Audrieth, Ludwig F.; Kleinberg, Jacob (1953). Non-aqueous solvents. New York: John Wiley & Sons. pp. 235–6. LCCN 52-12057.
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