Arsenic trifluoride

Arsenic trifluoride
Names
IUPAC name
Arsenic(III) fluoride
Other names
Arsenic trifluoride, trifluoroarsane, TL-156
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.145 Edit this at Wikidata
EC Number
  • 232-060-0
RTECS number
  • CG5775000
UNII
  • InChI=1S/AsF3/c2-1(3)4 checkY
    Key: JCMGUODNZMETBM-UHFFFAOYSA-N checkY
  • InChI=1/AsF3/c2-1(3)4
    Key: JCMGUODNZMETBM-UHFFFAOYAJ
  • F[As](F)F
Properties
AsF3
Molar mass 131.9168 g/mol
Appearance colorless oily liquid
Density 2.666 g/cm3 (0 °C)[1]
Melting point −8.5 °C (16.7 °F; 264.6 K)
Boiling point 60.4 °C (140.7 °F; 333.5 K)
decomposes
Solubility soluble in alcohol, ether, benzene and ammonia solution
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Toxic, corrosive
GHS labelling:
GHS06: Toxic
Danger
H301, H311, H331
P261, P264, P270, P271, P280, P301+P310, P302+P352, P304+P340, P311, P312, P321, P322, P330, P361, P363, P403+P233, P405, P501
NIOSH (US health exposure limits):
PEL (Permissible)
 [1910.1018] TWA 0.010 mg/m3[2]
REL (Recommended)
 Ca C 0.002 mg/m3 [15-minute][2]
IDLH (Immediate danger)
 Ca [5 mg/m3 (as As)][2]
Thermochemistry
-821.3 kJ/mol
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Arsenic trifluoride is a chemical compound of arsenic and fluorine with the chemical formula AsF3. It is a colorless liquid which reacts readily with water.[3] Like other inorganic arsenic compounds, it is highly toxic.

Preparation and properties

It can be prepared by reacting hydrogen fluoride, HF, with arsenic trioxide:[3]

6HF + As2O3 → 2AsF3 + 3H2O

It has a pyramidal molecular structure in the gas phase which is also present in the solid.[3] In the gas phase the As-F bond length is 170.6 pm and the F-As-F bond angle 96.2°.[4]

Arsenic trifluoride is used as a fluorinating agent for the conversion of non-metal chlorides to fluorides, in this respect it is less reactive than SbF3.[3]

Salts containing AsF4− anion can be prepared for example CsAsF4.[5] the potassium salt KAs2F7 prepared from KF and AsF3 contains AsF4− and AsF3 molecules with evidence of interaction between the AsF3 molecule and the anion.[6]

AsF3 reacts with SbF5. The product obtained could be described as the ionic compound AsF2+ SbF6−. However, the authors conclude the formed product cannot be viewed only as an ionic compound nor entirely as the neutral adduct AsF3SbF5. The crystal structure displays characteristics of both an ionic pair, and a neutral adduct, taking the middle ground in between both models. [7]

References

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  2. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0038". National Institute for Occupational Safety and Health (NIOSH).
  3. ^ a b c d Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  4. ^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  5. ^ New alkali metal and tetramethylammonium tetrafluoroarsenates(III), their vibrational spectra and crystal structure of caesium tetrafluoroarsenate(III) Klampfer P, Benkič P, Lesar A, Volavšek B, Ponikvar M, Jesih A., Collect. Czech. Chem. Commun. 2004, 69, 339-350 doi:10.1135/cccc20040339
  6. ^ Alkali-metal heptafluorodiarsenates(III): their preparation and the crystal structure of the potassium salt, Edwards A.J., Patel S.N., J. Chem. Soc., Dalton Trans., 1980, 1630-1632, doi:10.1039/DT9800001630
  7. ^ Fluoride crystal structures. Part XV. Arsenic trifluoride–antimony pentafluoride, Edwards A. J., Sills R. J. C. J. Chem. Soc. A, 1971, 942 - 945, doi:10.1039/J19710000942