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Contents

   



(Top)
  


1 Preparation and structure  




2 Reactions  




3 Applications  




4 Precautions  




5 References  




6 External links  













Antimony pentachloride






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From Wikipedia, the free encyclopedia
  

Antimony pentachloride
Antimony pentachloride
Antimony pentachloride
Names
IUPAC names

Antimony pentachloride
Antimony(V) chloride

Other names

Antimonic chloride
Antimony perchloride

Identifiers

CAS Number

3D model (JSmol)
  • Interactive image
    • ChemSpider
    ECHA InfoCard 100.028.729 Edit this at Wikidata
    EC Number
    • 231-601-8

    PubChem CID
    RTECS number
    • CC5075000
    UNII

    CompTox Dashboard (EPA)

    • 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

    Chemical formula

    		 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]

    Solubility in water

    		 reacts
    Solubility soluble in alcohol, HCl, tartaric acid, CHCl3, CS2, CCl4
    Solubilityinselenium(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]

    Magnetic susceptibility (χ)

    		 -120.0·10−6cm3/mol

    Refractive index (nD)

    		 1.59255
    Viscosity 2.034 cP (29.4 °C)[1]
    1.91 cP (35 °C)
    Structure

    Molecular shape

    		 Trigonal bipyramidal

    Dipole moment

    		 0 D
    Thermochemistry[3]

    Heat capacity (C)

    		 120.9 J/mol·K (gas)

    Std molar
    entropy     (S⦵298)

    		 295 J/mol·K

    Std enthalpy of
    formation     (ΔfH⦵298)

    		 -437.2 kJ/mol

    Gibbs free energy (ΔfG⦵)

    		 -345.35 kJ/mol
    Hazards
    Occupational safety and health (OHS/OSH):

    Inhalation hazards

    		 Toxic
    GHS labelling:[2]

    Pictograms

    		 GHS05: Corrosive GHS09: Environmental hazard

    Signal word

    		 Danger

    Hazard statements

    		 H314, H411

    Precautionary statements

    		 P273, P280, P305+P351+P338, P310
    NFPA 704 (fire diamond)
    NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acid
    4
    0
    1
    W
    Flash point 77 °C (171 °F; 350 K)
    Lethal dose or concentration (LD, LC):

    LD50 (median dose)

    		 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 hydrolysetohydrochloric acid, SbCl5 is a highly corrosive substance and must be stored in glass or PTFE containers.

    Preparation and structure

    [edit]

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

    SbCl3 + Cl2 → SbCl5

    Gaseous SbCl5 has a trigonal bipyramidal structure.[6]

    Reactions

    [edit]

    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

    [edit]

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

    Precautions

    [edit]

    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

    [edit]
    1. ^ a b c "Antimony pentachloride (UK PID)".
  • ^ a b c Sigma-Aldrich Co., Antimony(V) chloride. Retrieved on 2014-05-29.
  • ^ a b c "Antimony(V) chloride".
  • ^ 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)
  • ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  • ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  • ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  • ^ 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.
  • ^ 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.
  • ^ 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.
  • ^ 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.
  • ^ Shekarchi, M.; Behbahani, F. K Catal. Lett. 2017 147 2950. doi:10.1007/s10562-017-2194-2
    • [edit]
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