Arsenic trifluoride
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| IUPAC name Arsenic(III) fluoride | |||
| Other names Arsenic trifluoride, trifluoroarsane, TL-156 | |||
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| ECHA InfoCard | 100.029.145  | ||
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| Properties | |||
Chemical formula | 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) | ||
Solubility in water | decomposes | ||
| Solubility | soluble in alcohol, ether, benzene and ammonia solution | ||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards | Toxic, corrosive | ||
| GHS labelling: | |||
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| 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 | |||
Std enthalpy of formation (ΔfH⦵298) | -821.3 kJ/mol | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).  Y verify (what is  Y N ?) Infobox references | |||
Chemical compound
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]
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
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0038". National Institute for Occupational Safety and Health (NIOSH).
- ^ a b c d Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
- ^ 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
- ^ 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
- ^ 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
