Antimony trifluoride

| Structural formula | space-filling model

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| Unit cell | Unit cell of antimony trifluoride. The distorted-octahedral coordination of the fluorine relative to the antimony is visualized.

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Names
Preferred IUPAC name

Antimony(III) fluoride

Systematic IUPAC name

Trifluorostibane

Other names

Trifluoroantimony

Identifiers

CAS Number

* 7783-56-4 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 22960 Y

EC Number |

* 232-009-2

PubChem CID

* 24554

RTECS number |

* CC5150000

UNII |

* VWM00O92AM Y

UN number | UN 2923

InChI

* InChI=1S/3FH.Sb/h3*1H;/q;;;+3/p-3 Y

Key: GUNJVIDCYZYFGV-UHFFFAOYSA-K Y

* InChI=1S/3FH.Sb/h3*1H;/q;;;+3/p-3

Key: GUNJVIDCYZYFGV-UHFFFAOYSA-K

* InChI=1/3FH.Sb/h3*1H;/q;;;+3/p-3

Key: GUNJVIDCYZYFGV-DFZHHIFOAW

SMILES

* F[Sb](F)F

Properties

Chemical formula

| SbF3
Molar mass | 178.76 g/mol
Appearance  | light gray to white crystals
Odor | pungent
Density | 4.379 g/cm3
Melting point |  292 °C (558 °F; 565 K)
Boiling point |  376 °C (709 °F; 649 K)

Solubility in water

| 385 g/100 mL (0 °C)
443 g/100 mL (20 °C)
562 g/100 mL (30 °C)
Solubility | soluble in methanol, acetone
insoluble in ammonia

Magnetic susceptibility (χ)

| −46.0·10−6 cm3/mol
Structure

Crystal structure

| Orthorhombic, oS16

Space group

| Ama2, No. 40
Hazards
NFPA 704 (fire diamond)  |

Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 100 mg/kg
NIOSH (US health exposure limits):

PEL (Permissible)

| TWA 0.5 mg/m3 (as Sb)[1]

REL (Recommended)

| TWA 0.5 mg/m3 (as Sb)[1]
Related compounds

Other anions

| Antimony trichloride
Antimony tribromide
Antimony triiodide

Other cations

| Nitrogen trifluoride
Phosphorus trifluoride
Arsenic trifluoride
Bismuth fluoride

Related compounds

| Antimony pentafluoride

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

Antimony trifluoride is the inorganic compound with the formula SbF3. Sometimes called Swarts' reagent, it is one of two principal fluorides of antimony, the other being SbF5. It appears as a white solid. As well as some industrial applications,[2] it is used as a reagent in inorganic and organofluorine chemistry.

## Contents

* 1 Preparation and structure
* 2 Applications
* 3 Safety
* 4 References
* 5 External links

## Preparation and structure

In solid SbF3, the Sb centres have octahedral molecular geometry and are linked by bridging fluoride ligands. Three Sb–F bonds are short (192 pm) and three are long (261 pm). Because it is a polymer, SbF3 is far less volatile than related compounds AsF3 and SbCl3.[3]

SbF3 is prepared by treating antimony trioxide with hydrogen fluoride:[4]

Sb2O3 \+ 6 HF → 2 SbF3 \+ 3 H2O

The compound is a mild Lewis acid, hydrolyzing slowly in water. With fluorine, it is oxidized to give antimony pentafluoride.

SbF3 \+ F2 → SbF5

## Applications

It is used as a fluorination reagent in organic chemistry.[5] This application was reported by the Belgian chemist Frédéric Jean Edmond Swarts in 1892,[6] who demonstrated its usefulness for converting chloride compounds to fluorides. The method involved treatment with antimony trifluoride with chlorine or with antimony pentachloride to give the active species antimony trifluorodichloride (SbCl2F3). This compound can also be produced in bulk.[7] The Swarts reaction is generally applied to the synthesis of organofluorine compounds, but experiments have been performed using silanes.[8] It was once used for the industrial production of freon. Other fluorine-containing Lewis acids serve as fluorinating agents in conjunction with hydrogen fluoride.

SbF3 is used in dyeing and in pottery, to make ceramic enamels and glazes.

## Safety

The lethal minimum dose (guinea pig, oral) is 100 mg/kg.[9]

## References

1. ↑ 1.0 1.1 NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0036.html.
2. ↑ Sabina C. Grund, Kunibert Hanusch, Hans J. Breunig, Hans Uwe Wolf "Antimony and Antimony Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2006, Wiley-VCH, Weinheim. doi:10.1002/14356007.a03_055.pub2
3. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
4. ↑ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 199.
5. ↑ Tariq Mahmood and Charles B. Lindahl Fluorine Compounds, Inorganic, Antimony in Kirk‑Othmer Encyclopedia of Chemical Technology.doi:10.1002/0471238961.0114200913010813.a01
6. ↑ Swarts (1892). "none". Acad. Roy. Belg 3 (24): 474.
7. ↑ US patent 4438088
8. ↑ Booth, Harold Simmons; Suttle, John Francis (1946). "IV. The Preparation and Fluorination of Dimethyl and Trimethyl Chlorosilanes". J. Am. Chem. Soc. 68 (12): 2658–2660. doi:10.1021/ja01216a072.
9. ↑ Sabina C. Grund, Kunibert Hanusch, Hans J. Breunig, Hans Uwe Wolf “Antimony and Antimony Compounds” in Ullmann's Encyclopedia of Industrial Chemistry 2006, Wiley-VCH, Weinheim. doi: 10.1002/14356007.a03_055.pub2

## External links

* WebBook page for SbF3

* v
* t
* e

Antimony compounds

* SbBr3
* Sb(C2H3O2)3
* SbCl3
* SbCl5
* SbF3
* SbF5
* SbH3
* SbI3
* Sb2O3
* Sb2O4
* Sb2O5
* Sb2S3
* Sb2S5
* Sb2(SO4)3
* Sb2Se3
* Sb2Te3

* v
* t
* e

Salts and covalent derivatives of the fluoride ion

HF |  |  |  | He

|
|
|
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LiF | BeF2 | BF
BF3
B2F4 | CF4
other compounds | NF3
FN3
N2F2
N2F4
NF5§  | F2O
F2O2
other compounds | F2 | Ne
NaF | MgF2 | AlF
AlF3 | SiF4 | P2F4
PF3
PF5 | S2F2
SF2
SF4
SF6 | ClF
ClF3
ClF5 | Ar
KF | CaF
CaF2 | ScF3 | TiF2
TiF3
TiF4 | VF2
VF3
VF4
VF5 | CrF2
CrF3
CrF4
CrF5
CrF6§  | MnF2 | FeF2
FeF3 | CoF2
CoF3 | NiF2 | CuF
CuF2 | ZnF2 | GaF2
GaF3 | GeF2
GeF4 | AsF3
AsF5 | Se2F2
SeF4
SeF6 | BrF
BrF3
BrF5 | KrF2
RbF | SrF
SrF2 | YF3 | ZrF3
ZrF4 | NbF4
NbF5 | MoF2
MoF3
MoF4
MoF5
MoF6 | TcF4
TcF6 | RuF3
RuF5
RuF6 | RhF3
RhF5
RhF6 | PdF2 | AgF | CdF2 | InF
InF2
InF3 | SnF2
SnF4 | SbF3
SbF5 | Te3F2
TeF4
TeF6 | IF
IF3</br>IF5</br>IF7 | XeF2
XeF4
XeF6
CsF | BaF2 |  | HfF4 | TaF5 | WF2
WF3
WF4
WF5
WF6 | Re3F9
ReF4
ReF5
ReF6
ReF7 | OsF4
OsF5
OsF6 | IrF2
IrF3
IrF4
IrF5
IrF6 | PtF2
PtF4
PtF5
PtF6 | AuF
AuF3
Au2F10
AuF5•F2 | Hg2F2
HgF2
HgF4 | TlF | PbF2
PbF4 | BiF3
BiF5 | PoF2
PoF4
PoF6 | AtF  | RnF2
FrF | RaF2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaF3 | CeF3
CeF4 | PrF3 | NdF2,
NdF3 | PmF3 | SmF2,
SmF3 | EuF2,
EuF3 | GdF3 | TbF3 | DyF2,
DyF3 | HoF3 | ErF3 | TmF2
TmF3 | YbF2
YbF3 | LuF3
AcF3 | ThF4 | PaF5 | UF3
UF4
UF5
UF6 | NpF4
NpF6 | PuF3
PuF6 | AmF2
AmF3 | CmF3 | BkF3 | CfF3 | EsF3 | Fm  | Md  | No  | LrF3

§ means the substance has not been made.

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