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Antimony triiodide

From Wikipedia, the free encyclopedia

Antimony triiodide
Names
IUPAC name
Antimony triiodide, Antimony(III) iodide
Systematic IUPAC name
Triiodostibane
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.278 Edit this at Wikidata
EC Number
  • 232-205-8
UNII
  • InChI=1S/3HI.Sb/h3*1H;/q;;;+3/p-3 checkY
    Key: KWQLUUQBTAXYCB-UHFFFAOYSA-K checkY
  • InChI=1/3HI.Sb.3H/h3*1H;;;;/q;;;+3;;;/p-3/r3HI.H3Sb/h3*1H;1H3/q;;;+3/p-3
    Key: JYIUOADDPFDEAV-GODZFDHEAT
  • InChI=1/3HI.Sb/h3*1H;/q;;;+3/p-3
    Key: KWQLUUQBTAXYCB-DFZHHIFOAA
  • [SbH3+3].[I-].[I-].[I-]
  • I[Sb](I)I
Properties
I3Sb
Molar mass 502.473 g·mol−1
Appearance red crystals
Density 4.921 g/cm3
Melting point 170.5 °C (338.9 °F; 443.6 K)
Boiling point 401.6 °C (754.9 °F; 674.8 K)
soluble, partially hydrolyses
Solubility soluble in benzene, alcohol, acetone, CS2, HCl, KI, SnCl4, C2H7N
,HI,alkali metal triiodides 
insoluble in CHCl3, CCl4[1]
Solubility in diiodomethane 10.15% v/v (12 °C)[2]
-147.0·10−6 cm3/mol
Structure
Rhombohedral, hR24,
R-3, No. 148
1.58 D
Thermochemistry
81.6 J/mol·K (gas)[1]
-100.4 kJ/mol[1]
Hazards
GHS labelling:[4]
GHS07: Exclamation mark
GHS09: Environmental hazard
Warning
H302, H332, H411
P273
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.5 mg/m3 (as Sb)[3]
REL (Recommended)
 TWA 0.5 mg/m3 (as Sb)[3]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
Antimony triiodide
Antimony triiodide cristalline
Antimony triiodide
Antimony triiodide milled

Antimony triiodide is the chemical compound with the formula SbI3. This ruby-red solid is the only characterized "binary" iodide of antimony, i.e. the sole compound isolated with the formula SbxIy. It contains antimony in its +3 oxidation state. Like many iodides of the heavier main group elements, its structure depends on the phase. Gaseous SbI3 is a molecular, pyramidal species as anticipated by VSEPR theory. In the solid state, however, the Sb center is surrounded by an octahedron of six iodide ligands, three of which are closer and three more distant.[5] For the related compound BiI3, all six Bi—I distances are equal.[6]

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Transcription

Production

It may be formed by the reaction of antimony with elemental iodine, or the reaction of antimony trioxide with hydroiodic acid.

Alternatively, it may be prepared by the interaction of antimony and iodine in boiling benzene or tetrachloroethane.

Uses

SbI3 has been used as a dopant in the preparation of thermoelectric materials.[7]

References

  1. ^ a b c "Antimony triiodide".
  2. ^ Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand. Retrieved 18 May 2017.
  3. ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  4. ^ Sigma-Aldrich Co., Antimony(III) iodide. Retrieved on 2014-05-29.
  5. ^ Hsueh, H.C.; Chen, R.K.; Vass, H.; Clark, S.J.; Ackland, G.J.; Poon, W.C.K.; Crain, J. (1998). "Compression mechanisms in quasimolecular XI3 (X = As, Sb, Bi) solids" (PDF). Physical Review B. 58 (22): 14812–14822. Bibcode:1998PhRvB..5814812H. doi:10.1103/PhysRevB.58.14812. hdl:20.500.11820/6b565e3e-900c-465c-a037-6929e8a7c18b. S2CID 121883973.
  6. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  7. ^ D.-Y. Chung; T. Hogan; P. Brazis; M. Rocci-Lane; C. Kannewurf; M. Bastea; C. Uher; M. G. Kanatzidis (2000). "CsBi4Te6: A High-Performance Thermoelectric Material for Low-Temperature Applications". Science. 287 (5455): 1024–7. Bibcode:2000Sci...287.1024C. doi:10.1126/science.287.5455.1024. PMID 10669411.

External links

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This page was last edited on 21 January 2024, at 14:10
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