Bismuth chloride

Names
IUPAC name

Bismuth chloride

Other names

Bismuth trichloride, Trichlorobismuth, Trichlorobismuthine, Bismuth(III) chloride

Identifiers

CAS Number

* 7787-60-2 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 22993 Y

ECHA InfoCard | 100.029.203

PubChem CID

* 24591

RTECS number |

* EB2690000

UNII |

* 4X6566U3SD Y

CompTox Dashboard (EPA)

* DTXSID3064851

InChI

* InChI=1S/Bi.3ClH/h;3*1H/q+3;;;/p-3 Y

Key: JHXKRIRFYBPWGE-UHFFFAOYSA-K Y

* InChI=1/Bi.3ClH/h;3*1H/q+3;;;/p-3

Key: JHXKRIRFYBPWGE-DFZHHIFOAJ

SMILES

* Cl[Bi](Cl)Cl

Properties

Chemical formula

| BiCl3
Molar mass | 315.34 g/mol
Appearance  | hygroscopic white to yellow crystals
Density | 4.75 g/cm3
Melting point | 227 °C (441 °F; 500 K)
Boiling point | 447 °C (837 °F; 720 K)

Solubility in water

| Soluble,hydrolyses
Solubility | soluble in methanol, diethyl ether, acetone

Magnetic susceptibility (χ)

| -26.5·10−6 cm3/mol
Structure

Crystal structure

| cubic
Thermochemistry

Heat capacity (C)

| 0.333 J/(g K)

Std molar
entropy (S⦵298)

| 82.9 J/(K mol)

Std enthalpy of
formation (ΔfH⦵298)

| -1.202 kJ/g
Hazards
NFPA 704 (fire diamond)  |

Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 3324 mg/kg, oral (rat)
Safety data sheet (SDS)  | JT Baker
Related compounds

Other anions

| bismuth fluoride, bismuth subsalicylate, bismuth trioxide

Other cations

| iron(III) chloride, manganese(II) chloride, cobalt(II) chloride

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

Bismuth chloride (or butter of bismuth) is an inorganic compound with the chemical formula BiCl3. It is a covalent compound and is the common source of the Bi3+ ion. In the gas phase and in the crystal, the species adopts a pyramidal structure, in accord with VSEPR theory.

## Preparation[edit]

Bismuth chloride can be synthesized directly by passing chlorine over bismuth.

2 Bi + 3 Cl2 → 2 BiCl3

or by dissolving bismuth metal in aqua regia, evaporating the mixture to give BiCl3·2H2O, which can be distilled to form the anhydrous trichloride.[1]

Alternatively, it may be prepared by adding hydrochloric acid to bismuth oxide and evaporating the solution.

Bi2O3 \+ 6 HCl → 2 BiCl3 \+ 3 H2O

Also, the compound can be prepared by dissolving bismuth in concentrated nitric acid and then adding solid sodium chloride into this solution.[2]

Bi + 6 HNO3 → Bi(NO3)3 \+ 3 H2O + 3 NO2
Bi(NO3)3 \+ 3 NaCl → BiCl3 \+ 3 NaNO3

## Structure[edit]

In the gas phase BiCl3 is pyramidal with a Cl–Bi–Cl angle of 97.5° and a bond length of 242 pm.[3] In the solid state, each Bi atom has three near neighbors at 250 pm, two at 324 pm and three at a mean of 336 pm,[4] the image above highlights the three closest neighbours. This structure is similar to that of AsCl3, AsBr3, SbCl3 and SbBr3.

## Chemistry[edit]

Bismuth chloride is hydrolyzed readily to bismuth oxychloride, BiOCl:[5]

Bi3+
(aq) + Cl−
(aq) + H
2O(l) ⇌ BiOCl (s) + 2 H+
(aq)

This reaction can be reversed by adding an acid, such as hydrochloric acid.[6]

Reaction of solid BiCl3 with water vapour below 50 °C has been shown to produce the intermediate monohydrate, BiCl3·H2O.[7]

Bismuth chloride is an oxidizing agent, being readily reduced to metallic bismuth by reducing agents.

### Chloro complexes[edit]

In contrast to the usual expectation by consistency with periodic trends, BiCl3 is a Lewis acid, forming a variety of chloro complexes such as [BiCl6]3− that strongly violates the octet rule. Furthermore, the octahedral structure of this coordination complex does not follow the predictions of VSEPR theory, since the lone pair on bismuth is unexpectedly stereochemically inactive. The dianionic complex [BiCl5]2− does however adopt the expected square pyramidal structure.[8]

|  |

|
|

Cs3[BiCl6] | Cs3[BiCl6] | [BiCl6]3−

### Organic catalysis[edit]

Bismuth chloride is used as a catalyst in organic synthesis. In particular, it catalyzes the Michael reaction and the Mukaiyama aldol reaction. The addition of other metal iodides increases its catalytic activity.[9]

## References[edit]

1. ^ Godfrey, S. M.; McAuliffe, C. A.; Mackie, A. G.; Pritchard, R. G. (1998). Nicholas C. Norman (ed.). Chemistry of arsenic, antimony, and bismuth. Springer. p. 90\. ISBN 0-7514-0389-X.
2. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
3. ^ Töke, Orsolya, and Magdolna Hargittai. "Molecular structure of bismuth trichloride from combined electron diffraction and vibrational spectroscopic study." Structural Chemistry 6.2 (1995): 127–130.
4. ^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition, pp. 879–884, Oxford Science Publications, ISBN 0-19-855370-6
5. ^ Joel Henry Hildebrand (2008). Principles of Chemistry. BiblioBazaar, LLC. p. 191\. ISBN 978-0-559-31877-1.
6. ^ Frank Welcher (2008). Chemical Solutions. READ BOOKS. p. 48\. ISBN 978-1-4437-2907-9.
7. ^ Wosylus, Aron; Hoffmann, Stefan; Schmidt, Marcus; Ruck, Michael (2010). "In-situ Study of the Solid-Gas Reaction of BiCl3 to BiOCl via the Intermediate Hydrate BiCl3·H2O". European Journal of Inorganic Chemistry. 2010 (10): 1469–1471. doi:10.1002/ejic.201000032. ISSN 1434-1948.
8. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
9. ^ Hitomi Suzuki; Yoshihiro Matano (2001). Organobismuth chemistry. Elsevier. pp. 403–404. ISBN 0-444-20528-4.

* v
* t
* e

Bismuth compounds

Bismuth(III)|

* Bi(CH3COO)3
* BiBr3
* BiCl3
* Bi4Ge3O12
* BiOCl
* BiOI
* BiONO3
* BiAs
* Bi2Se3
* Bi12SiO20
* Bi2O2(CO3)
* Bi2Te3
* BiF3
* BiI3
* Bi2(SO4)3
* Bi(NO3)3
* BiVO4
* Bi(IO3)3
* Bi2O3
* BiP
* BiMn
* Bi(OH)3
* Bi2S3
* BiH3
* BiFeO3
* subsalicylate
* subcitrate
* C7H5BiO6

| Organobismuth(III)|

* C4H4BiH

|

Bismuth(V)|

* NaBiO3
* BiF5
* Bi2O5

| Organobismuth(V)|

* Bi(CH3)5
* Bi(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 | 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 | ThCl4 | PaCl4
PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl3 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3 | EsCl2
EsCl3 | FmCl2 | MdCl2 | NoCl2

Authority control databases: National |

* Germany

|

*[CID]: Compound ID
*[EPA]: U.S. Environmental Protection Agency
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template