Antimony pentachloride

Chemical compound

Antimony pentachloride  | Antimony pentachloride |

|

Names
IUPAC names

Antimony pentachloride
Antimony(V) chloride

Other names

Antimonic chloride
Antimony perchloride

Identifiers

CAS Number

* 7647-18-9 Y

3D model (JSmol)

* Interactive image
* Interactive image

ChemSpider |

* 10613049 Y

ECHA InfoCard | 100.028.729
EC Number |

* 231-601-8

PubChem CID

* 24294

RTECS number |

* CC5075000

UNII |

* 0S9308207L Y

CompTox Dashboard (EPA)

* DTXSID30893043

InChI

* InChI=1S/5ClH.Sb/h5*1H;/q;;;;;+3/p-5 Y

Key: PZVOXSCNPLCIRA-UHFFFAOYSA-I Y

* 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

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[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

Signal word

| Danger

Hazard statements

| H314, H411

Precautionary statements

| P273, P280, P305+P351+P338, P310
NFPA 704 (fire diamond)  |

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 YN ?)

Infobox references

Chemical compound

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

[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)".
2. ^ a b c Sigma-Aldrich Co., Antimony(V) chloride. Retrieved on 2014-05-29.
3. ^ a b c "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. ^ a b 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)82045-7.225-255&rft.date=1976&rft_id=info:doi/10.1016/S0010-8545(00)82045-7&rft.au=V.+Gutmann&rfr_id=info:sid/en.wikipedia.org:Antimony+pentachloride" class="Z3988">
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/ed054p612.612-613&rft.date=1977&rft_id=info:doi/10.1021/ed054p612&rft.au=Cramer,+R.+E.&rft.au=Bopp,+T.+T.&rfr_id=info:sid/en.wikipedia.org:Antimony+pentachloride" class="Z3988"> 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 11848774.877-922&rft.date=1996&rft_id=info:doi/10.1021/cr940053x&rft_id=info:pmid/11848774&rft.au=Connelly,+N.+G.&rft.au=Geiger,+W.+E.&rfr_id=info:sid/en.wikipedia.org:Antimony+pentachloride" class="Z3988">
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 11672186.5847-5856&rft.date=1998&rft_id=info:doi/10.1021/jo980407a&rft_id=info:pmid/11672186&rft.aulast=Rathore&rft.aufirst=R.&rft.au=Kumar,+A.+S.&rft.au=Lindeman,+S.+V.&rft.au=Kochi,+J.+K.&rft_id=https://epublications.marquette.edu/cgi/viewcontent.cgi?article=1696&context;=chem_fac&rfr_id=info:sid/en.wikipedia.org:Antimony+pentachloride" class="Z3988">
12. ^ Shekarchi, M.; Behbahani, F. K Catal. Lett. 2017 147 2950\. doi:10.1007/s10562-017-2194-2

## External links

[edit]

Wikimedia Commons has media related to Antimony pentachloride.

* v
* t
* e

Antimony compounds

Antimonides|

* AlSb
* Bi1-xSbx
* DySb
* GaSb
* HoSb
* HoSb2
* InSb
* PrSb
* SmSb
* YSb
* ZnSb

Sb(III)|

* SbBr3
* Sb(C2H3O2)3
* SbCl3
* SbF3
* Sb4O4(OH)2(NO3)2
* SbH3
* SbI3
* SbN
* Sb2O3
* Sb2S3
* Sb2(SO4)3
* Sb2Se3
* Sb2Te3

| Organoantimony(III) compounds|

* Sb(CH3)3
* Sb(C6H5)3

|

Sb(III,V)|

* Sb2O4

Sb(V)|

* SbCl5
* SbF5
* Sb2O5
* Sb2S5

| Organoantimony(V) compounds|

* Sb(CH3)5
* Sb(C6H5)5

|

* v
* t
* e

Salts and covalent derivatives of the chloride ion

| HCl |  |  |  | He

|
|
|
|

LiCl | BeCl2 | B4Cl4
B12Cl12
BCl3
B2Cl4
+BO3 | C2Cl2
C2Cl4
C2Cl6
CCl4

+CO3 | NCl3
ClN3

+NO3 | ClxOy
Cl2O
Cl2O2
ClO
ClO2
Cl2O4
Cl2O6
Cl2O7
ClO4
+O | ClF
ClF3
ClF5 | Ne
NaCl | MgCl2 | AlCl
AlCl3 | Si5Cl12
Si2Cl6
SiCl4 | P2Cl4
PCl3
PCl5
+P | S2Cl2
SCl2
SCl4
+SO4 | Cl2 | Ar
KCl | CaCl
CaCl2 |  | ScCl3 | TiCl2
TiCl3
TiCl4 | VCl2
VCl3
VCl4
VCl5 | CrCl2
CrCl3
CrCl4 | MnCl2
MnCl3 | FeCl2
FeCl3 | CoCl2
CoCl3 | NiCl2 | CuCl
CuCl2 | ZnCl2 | GaCl
GaCl3 | GeCl2
GeCl4 | AsCl3
AsCl5
+As | Se2Cl2
SeCl2
SeCl4 | BrCl | Kr
RbCl | SrCl2 |  | YCl3 | ZrCl2
ZrCl3
ZrCl4 | NbCl3
NbCl4
NbCl5 | MoCl2
MoCl3
MoCl4
MoCl5
MoCl6 | TcCl3
TcCl4 | RuCl2
RuCl3
RuCl4 | RhCl3 | PdCl2 | AgCl | CdCl2 | InCl
InCl2
InCl3 | SnCl2
SnCl4 | SbCl3
SbCl5 | Te3Cl2
TeCl2
TeCl4 | ICl
ICl3 | XeCl
XeCl2
XeCl4
CsCl | BaCl2 | *  | LuCl3 | HfCl4 | TaCl3
TaCl4
TaCl5 | WCl2
WCl3
WCl4
WCl5
WCl6 | ReCl3
ReCl4
ReCl5
ReCl6 | OsCl2
OsCl3
OsCl4
OsCl5 | IrCl2
IrCl3
IrCl4 | PtCl2
PtCl4 | AuCl
(Au[AuCl4])2
AuCl3 | Hg2Cl2
HgCl2 | TlCl
TlCl3 | PbCl2
PbCl4 | BiCl3 | PoCl2
PoCl4 | AtCl | Rn
FrCl | RaCl2 | **  | LrCl3 | RfCl4 | DbCl5 | SgO2Cl2 | BhO3Cl | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og

*  | LaCl3 | CeCl3 | PrCl3 | NdCl2
NdCl3 | PmCl3 | SmCl2
SmCl3 | EuCl2
EuCl3 | GdCl3 | TbCl3 | DyCl2
DyCl3 | HoCl3 | ErCl3 | TmCl2
TmCl3 | YbCl2
YbCl3
**  | AcCl3 | ThCl3
ThCl4 | PaCl4
PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl3 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3
CfCl2 | EsCl2
EsCl3 | FmCl2 | MdCl2 | NoCl2
*[CID]: Compound ID
*[EPA]: U.S. Environmental Protection Agency
*[H314]: H314: Causes severe skin burns and eye damage
*[H411]: H411: Toxic to aquatic life with long lasting effects
*[P273]: P273: Avoid release to the environment.
*[P280]: P280: Wear protective gloves/protective clothing/eye protection/face protection.
*[P305+P351+P338]: P305+P351+P338: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do. Continue rinsing.
*[P310]: P310: Immediately call a POISON CENTER or doctor/physician.
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