Antimony pentachloride

Antimony pentachloride
Antimony pentachloride
Names
	IUPAC names Antimony pentachloride; Antimony(V) chloride
	Other names Antimonic chloride; Antimony perchloride
Identifiers
CAS Number	7647-18-9 ;
3D model (JSmol)	Interactive image; Interactive image;
ChemSpider	10613049 ;
ECHA InfoCard	100.028.729
EC Number	231-601-8;
PubChem CID	24294;
RTECS number	CC5075000;
UNII	0S9308207L ;
CompTox Dashboard (EPA)	DTXSID30893043 ;
	InChI InChI=1S/5ClH.Sb/h51H;/q;;;;;+3/p-5 Key: PZVOXSCNPLCIRA-UHFFFAOYSA-I ; InChI=1/5ClH.Sb.3H/h51H;;;;/q;;;;;+3;;;/p-5/r5ClH.H3Sb/h51H;1H3/q;;;;;+3/p-5 Key: KUGFODPTKMDJNG-MEZDTJOHAL; InChI=1/5ClH.Sb/h51H;/q;;;;;+3/p-5 Key: PZVOXSCNPLCIRA-AACRGIKGAS;
	SMILES [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
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]
Magnetic susceptibility (χ)	-120.0·10−6 cm3/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
Heat capacity (C)	120.9 J/mol·K (gas)[3]
Std molar; entropy (So298)	295 J/mol·K[3]
Std enthalpy of; formation (ΔfH⦵298)	-437.2 kJ/mol[3]
Gibbs free energy (ΔfG˚)	-345.35 kJ/mol[3]
Hazards
GHS pictograms	[2]
GHS Signal word	Danger
GHS hazard statements	H314, H411[2]
GHS precautionary statements	P273, P280, P305+351+338, P310[2]
Inhalation hazard	Toxic
NFPA 704 (fire diamond)	0 3 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).
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	Infobox references

Antimony pentachloride is a chemical compound with the formula SbCl₅. It is a colourless oil, but typical samples are yellowish due to impurities. 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

Antimony pentachloride hydrolyses to give hydrochloric acid and antimony oxychlorides. This reaction is suppressed in the presence of a large excess of chloride, owing to the formation of the hexachloroantimonate complex ion:

SbCl₅ + Cl⁻ → [SbCl₆]⁻

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

This compound forms adducts with many Lewis bases. SbCl,₅ is a soft Lewis acid and its ECW model parameters are E_A = 3.64 and C_A = 10.42. It is used as the standard Lewis acid in the Gutmann scale of Lewis basicity.[7] However, Cramer-Bopp plots show that a one-parameter basicity scale is incomplete and that there is no single rank order of base strength. These plots show that to define the order of Lewis base strength (or Lewis acid strength) at least two properties must be considered.

It is also a strong oxidizing agent.[8]

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.[9]

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References

"Antimony pentachloride (UK PID)".
Sigma-Aldrich Co., Antimony(V) chloride. Retrieved on 2014-05-29.
"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), http://webbook.nist.gov (retrieved 2014-05-29)
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.
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.
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.
Shekarchi, M.; Behbahani, F. K Catal. Lett. 2017 147 2950. doi:10.1007/s10562-017-2194-2

External links

This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.

[inchem-1] "Antimony pentachloride (UK PID)".

[sigma-2] Sigma-Aldrich Co., Antimony(V) chloride. Retrieved on 2014-05-29.

[chemister-3] "Antimony(V) chloride".

[nist-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), http://webbook.nist.gov (retrieved 2014-05-29)

[PGCH-5] 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] 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.

[8] 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.

[9] Shekarchi, M.; Behbahani, F. K Catal. Lett. 2017 147 2950. doi:10.1007/s10562-017-2194-2