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| Names | |
|---|---|
| Other names
Arsenic(III) chloride, Arsenous trichloride, Arsine trichloride, Butter of arsenic, de Valagin's solution, Trichloroarsine
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.029.144 |
| EC Number |
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PubChem CID
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| RTECS number |
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| UNII | |
| UN number | 1560 |
CompTox Dashboard (EPA)
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| Properties | |
| AsCl3 | |
| Molar mass | 181.28 g/mol |
| Appearance | colourless oily liquid |
| Density | 2.163 g/cm3, liquid |
| Melting point | −13 °C (9 °F; 260 K) |
| Boiling point | 181 °C (358 °F; 454 K) |
| Hydrolyzes | |
| Solubility | soluble in alcohol, ether, HCl, HBr, chloroform, CCl4[1] |
| -79.9·10−6 cm3/mol | |
Refractive index (nD)
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1.6006 |
| Viscosity | 9.77 x 10−6 Pa s |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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Very toxic, carcinogen, corrosive, decomposes on contact with water releasing HCl |
| GHS labelling: | |
   
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| Danger | |
| H301, H310, H314, H331, H350, H410 | |
| P201, P202, P260, P261, P262, P264, P270, P271, P273, P280, P281, P301+P310, P301+P330+P331, P302+P350, P303+P361+P353, P304+P340, P305+P351+P338, P308+P313, P310, P311, P321, P322, P330, P361, P363, P391, P403+P233, P405, P501 | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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48 mg/kg |
LCLo (lowest published)
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100 mg/m3 (cat, 1 hr) 200 mg/m3 (cat, 20 min) 338 ppm (rat, 10 min)[3] |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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[1910.1018] TWA 0.010 mg/m3[2] |
REL (Recommended)
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Ca C 0.002 mg/m3 [15-minute][2] |
IDLH (Immediate danger)
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Ca [5 mg/m3 (as As)][2] |
| Related compounds | |
Other anions
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Arsenic trioxide, Arsenic trifluoride |
Other cations
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Antimony trichloride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Arsenic trichloride is an inorganic compound with the formula AsCl3, also known as arsenous chloride or butter of arsenic. This poisonous oil is colourless, although impure samples may appear yellow. It is an intermediate in the manufacture of organoarsenic compounds.[4]
YouTube Encyclopedic
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1/5Views:16 1141 2621 071771702
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AsCl3 Lewis Structure: How to Draw the Lewis Dot Structure for AsCl3
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Arsenic trioxide | Wikipedia audio article
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Lewisite
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เคมี เพิ่ม ม.4 เล่ม1 (2560) | บทที่3 พันธะเคมี : แบบฝึกหัด 3.7 ข้อ 03
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As toxicology
Transcription
This is the AsCl3 Lewis structure. For the Arsenic atom, we have 5 valence electrons, plus 7 for the Chlorine, we have 3 Chlorine atoms; for a total of 26 valence electrons. Arsenic is the least electronegative, we'll put that in the center and then we'll put the Chlorines around the outside. We have a total of 26 valence electrons. We'll put 2 between atoms to form chemical bonds, and then we'll go around the outside of the outer atoms to complete their octets. So 2, 4, 6, 8, 10, and 24. Then we'll come back to the central atom and we'll put 2 valence electrons there, 26. We've used all 26 valence electrons. So now the Chlorine atoms, and they're all the same, they have 8 valence electrons, so their octets are full. And the central Arsenic atom, that also has 8 valence electrons, so its octet is full, as well. So we've used all 26 valence electrons and each of the atoms has an octet. So this is the correct Lewis structure for AsCl3, arsenic trichloride. This is Dr. B., and thanks for watching.
Structure
AsCl3 is a pyramidal molecule with C3v symmetry. The As-Cl bond is 2.161 Å and the angle Cl-As-Cl is 98° 25'±30.[5][6] AsCl3 has four normal modes of vibration: ν1(A1) 416, ν2(A1) 192, ν3 393, and ν4(E) 152 cm−1.[7]
Synthesis
This colourless liquid is prepared by treatment of arsenic(III) oxide with hydrogen chloride followed by distillation:
- As2O3 + 6 HCl → 2 AsCl3 + 3 H2O
It can also be prepared by chlorination of arsenic at 80–85 °C, but this method requires elemental arsenic.[4]
- 2 As + 3 Cl2 → 2 AsCl3
Arsenic trichloride can be prepared by the reaction of arsenic oxide and sulfur monochloride. This method requires simple apparatus and proceeds efficiently:[8]
- 2 As2O3 + 6 S2Cl2 → 4 AsCl3 + 3 SO2 + 9 S
A convenient laboratory method is refluxing arsenic(III) oxide with thionyl chloride:[9]
- 2 As2O3 + 3 SOCl2 → 2 AsCl3 + 3 SO2
Arsenic trichloride can also be prepared by the reaction of hydrochloric acid and arsenic(III) sulfide.
- As2S3 + 6 HCl → 2 AsCl3 + 3 H2S
Reactions
Hydrolysis gives arsenous acid and hydrochloric acid:
- AsCl3 + 3 H2O → As(OH)3 + 3 HCl
Although AsCl3 is less moisture sensitive than PCl3, it still fumes in moist air.[10]
AsCl3 undergoes redistribution upon treatment with As2O3 to give the inorganic polymer AsOCl. With chloride sources, AsCl3 also forms salts containing the anion [AsCl4]−. Reaction with potassium bromide and potassium iodide give arsenic tribromide and arsenic triiodide, respectively.
AsCl3 is useful in organoarsenic chemistry, for example triphenylarsine is derived from AsCl3:[11]
- AsCl3 + 6 Na + C6H5Cl → As(C6H5)3 + 6 NaCl
The chemical weapons called Lewisites are prepared by the addition of arsenic trichloride to acetylene:
- AsCl3 + C2H2 → ClCH=CHAsCl2
Safety
Inorganic arsenic compounds are highly toxic,[4] and AsCl3 especially so because of its volatility and solubility (in water).
It is classified as an extremely hazardous substance in the United States as defined in Section 302 of the U.S. Emergency Planning and Community Right-to-Know Act (42 U.S.C. 11002), and is subject to strict reporting requirements by facilities which produce, store, or use it in significant quantities.[12]
References
- ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99th ed.). CRC Press. pp. 4–41. ISBN 978-1138561632.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0038". National Institute for Occupational Safety and Health (NIOSH).
- ^ "Arsenic (inorganic compounds, as As)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
- ^ a b c Sabina C. Grund, Kunibert Hanusch, Hans Uwe Wolf "Arsenic and Arsenic Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, VCH-Wiley, 2008, Weinheim.doi:10.1002/14356007.a03_113.pub2
- ^ P. Kisliuk; C. H. Townes. "The Microwave Spectra and Molecular Structure of Phosphorus and Arsenic Trichloride". J. Chem. Phys. 1950, 18.
- ^ Jean Galy; Renee Enjalbertl Pierre Lecante; Andrzej Burian "AsCl3: From the crystalline to the liquid state. XRD (176< T (K) < 250) and WAXS (295K) studies" Inorg. Chem 2002, volume 41, pp. 693–698.doi:10.1021/ic0102788
- ^ Klapoetke, Thomas M. "The vibrational spectrum of arsenic trichloride" Main Group Metal Chemistry 1997, volume 20, pp. 81–83.
- ^ R. C. Smith, "Manufacture of Arsenic trichloride" The Journal of Industrial and Engineering Chemistry 1919, volume 11, pp. 109–110. doi:10.1021/ie50110a009
- ^ Pandey, S. K.; Steiner, A.; Roesky, H. W. (1997). "Arsenic(III) chloride". Inorganic Synthesis. 31: 148-150. doi:10.1002/9780470132623.ch24.
- ^ Holleman, A. F.; Wiberg, E. Inorganic Chemistry Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Shriner, R. L.; Wolf, C. N. (1963). "Tetraphenylarsonium Chloride Hydrochloride". Organic Syntheses; Collected Volumes, vol. 4, p. 910.. Describes the preparation of As(C6H5)3.
- ^ 40 C.F.R.: Appendix A to Part 355—The List of Extremely Hazardous Substances and Their Threshold Planning Quantities (PDF) (Report) (July 1, 2008 ed.). Government Printing Office. Archived from the original (PDF) on February 25, 2012. Retrieved October 29, 2011.
This page was last edited on 25 April 2024, at 05:12