Antimony pentachloride
Antimony pentachloride
Antimony pentachloride
Names
IUPAC names
Antimony pentachloride
Antimony(V) chloride
Other names
Antimonic chloride
Antimony perchloride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.028.729
EC Number
  • 231-601-8
RTECS number
  • CC5075000
UNII
  • InChI=1S/5ClH.Sb/h5*1H;/q;;;;;+3/p-5 checkY
    Key: PZVOXSCNPLCIRA-UHFFFAOYSA-I checkY
  • InChI=1/5ClH.Sb.3H/h5*1H;;;;/q;;;;;+3;;;/p-5/r5ClH.H3Sb/h5*1H;1H3/q;;;;;+3/p-5
    Key: KUGFODPTKMDJNG-MEZDTJOHAL
  • InChI=1/5ClH.Sb/h5*1H;/q;;;;;+3/p-5
    Key: PZVOXSCNPLCIRA-AACRGIKGAS
  • [Cl-].[Cl-].[Cl-].[Cl-].[Cl-].[SbH3+3]
  • [SbH3+3].[Cl-].[Cl-].[Cl-].[Cl-].[Cl-]
Properties
Cl5Sb
Molar mass 299.01 g·mol−1
Appearance colorless or reddish-yellow (fuming) liquid, oily
Odor pungent, offensive
Density 2.336 g/cm3 (20 °C)[1]
2.36 g/cm3 (25 °C)[2]
Melting point 2.8 °C (37.0 °F; 275.9 K)
Boiling point 140 °C (284 °F; 413 K)
decomposes from 106 °C[3]
79 °C (174 °F; 352 K)
at 22 mmHg[1]
92 °C (198 °F; 365 K)
at 30 mmHg[2]
reacts
Solubility soluble in alcohol, HCl, tartaric acid, CHCl3, CS2, CCl4
Solubility in selenium(IV) oxychloride 62.97 g/100 g (25 °C)
Vapor pressure 0.16 kPa (25 °C)
4 kPa (40 °C)
7.7 kPa (100 °C)[4]
-120.0·10−6 cm3/mol
1.59255
Viscosity 2.034 cP (29.4 °C)[1]
1.91 cP (35 °C)
Structure
Trigonal bipyramidal
0 D
Thermochemistry[3]
120.9 J/mol·K (gas)
295 J/mol·K
-437.2 kJ/mol
-345.35 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):
Inhalation hazards
 Toxic
GHS labelling:[2]
GHS05: Corrosive GHS09: Environmental hazard
Danger
H314, H411
P273, P280, P305+P351+P338, P310
NFPA 704 (fire diamond)
NFPA 704 four-colored diamond
4
0
1
W
Flash point 77 °C (171 °F; 350 K)
Lethal dose or concentration (LD, LC):
1115 mg/kg, (rat, oral)[3]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.5 mg/m3 (as Sb)[5]
REL (Recommended)
 TWA 0.5 mg/m3 (as Sb)[5]
Related compounds
Other anions
 Antimony pentafluoride
Other cations
 Phosphorus pentachloride
Related compounds
 Antimony trichloride
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 ?)
Infobox references

Antimony pentachloride is a chemical compound with the formula SbCl5. It is a colourless oil, but typical samples are yellowish due to dissolved chlorine. Owing to its tendency to hydrolyse to hydrochloric acid, SbCl5 is a highly corrosive substance and must be stored in glass or PTFE containers.

Preparation and structure

Antimony pentachloride is prepared by passing chlorine gas into molten antimony trichloride:

SbCl3 + Cl2 → SbCl5

Gaseous SbCl5 has a trigonal bipyramidal structure.[6]

Reactions

This compounds reacts with water to form antimony pentoxide and hydrochloric acid:[7]

2 SbCl5 + 5 H2O → Sb2O5 + 10 HCl

The mono- and tetrahydrates are known, SbCl5·H2O and SbCl5·4H2O.

This compound forms adducts with many Lewis bases. SbCl5 is a soft Lewis acid and its ECW model parameters are EA = 3.64 and CA = 10.42. It is used as the standard Lewis acid in the Gutmann scale of Lewis basicity.[8][9]

It is also a strong oxidizing agent.[10] For example aromatic ethers are oxidized to their radical cations according to the following stoichiometry:[11]

3 SbCl5 + 2 ArH → 2 (ArH+)(SbCl6−) + SbCl3

Applications

Antimony pentachloride is used as a polymerization catalyst and for the chlorination of organic compounds.

Precautions

Antimony pentachloride is a highly corrosive substance that should be stored away from heat and moisture. It is a chlorinating agent and, in the presence of moisture, it releases hydrogen chloride gas. Because of this, it may etch even stainless-steel tools (such as needles), if handled in a moist atmosphere. It should not be handled with non-fluorinated plastics (such as plastic syringes, plastic septa, or needles with plastic fittings), since it melts and carbonizes plastic materials.[12]

References

  1. 1 2 3 "Antimony pentachloride (UK PID)".
  2. 1 2 3 Sigma-Aldrich Co., Antimony(V) chloride. Retrieved on 2014-05-29.
  3. 1 2 3 "Antimony(V) chloride".
  4. ↑ Antimony pentachloride in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD) (retrieved 2014-05-29)
  5. 1 2 NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  6. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  7. ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  8. ↑ V. Gutmann (1976). "Solvent effects on the reactivities of organometallic compounds". Coord. Chem. Rev. 18 (2): 225–255. doi:10.1016/S0010-8545(00)82045-7.
  9. ↑ Cramer, R. E.; Bopp, T. T. (1977). "Graphical display of the enthalpies of adduct formation for Lewis acids and bases". Journal of Chemical Education. 54: 612–613. doi:10.1021/ed054p612. The plots shown in this paper used older parameters. Improved E&C parameters are listed in ECW model.
  10. ↑ Connelly, N. G.; Geiger, W. E. (1996). "Chemical Redox Agents for Organometallic Chemistry". Chem. Rev. 96 (2): 877–922. doi:10.1021/cr940053x. PMID 11848774.
  11. ↑ Rathore, R.; Kumar, A. S.; Lindeman, S. V.; Kochi, J. K. (1998). "Preparation and Structures of Crystalline Aromatic Cation-Radical Salts. Triethyloxonium Hexachloroantimonate as a Novel (One-Electron) Oxidant". The Journal of Organic Chemistry. 63 (17): 5847–5856. doi:10.1021/jo980407a. PMID 11672186.
  12. ↑ Shekarchi, M.; Behbahani, F. K Catal. Lett. 2017 147 2950. doi:10.1007/s10562-017-2194-2
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