Bismuth chloride
| |
| |
| Names | |
|---|---|
| IUPAC name
Bismuth chloride
| |
| Other names
Bismuth trichloride, Trichlorobismuth, Trichlorobismuthine, Bismuth(III) chloride
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.029.203 |
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| 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) |
| Decomposes to bismuth oxychloride | |
| Solubility | soluble in methanol, diethyl ether, acetone |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
|
3324 mg/kg, oral (rat) |
| 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).
| |
Bismuth chloride is an inorganic compound with the chemical formula BiCl3. It is a 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
Bismuth chloride is synthesized directly by passing chlorine over bismuth.
- 2 Bi + 3 Cl2 → 2 BiCl3
Alternatively, the chloride salt 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. [1]
- Bi + 6 HNO3 → Bi(NO3)3 + 3 H2O + 3 NO2
- Bi(NO3)3 + 3 NaCl → BiCl3 + 3 NaNO3
Chemistry
Bismuth chloride is hydrolyzed readily to bismuth oxychloride, BiOCl:[2]
- Bi3+
+ Cl−
+ H
2O → BiOCl (s) + 2 H+
This reaction can be suppressed by adding an acid, such as hydrochloric acid.[3]
Bismuth chloride is an oxidizing agent, being readily reduced to metallic bismuth by reducing agents.
Chloro complexes
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.[4]
 |
 |
 |
Organic catalysis
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.[5]
Uses
Bismuth chloride is an excellent water soluble crystalline source of bismuth. Its aqueous solution conducts electricity as does the molten material. It is used to prepare several other bismuth salts, and is a constituent in pigments and cosmetics.
Safety
Bismuth chloride is toxic. It causes irritation to the gastrointestinal and respiratory tract. Contact with skin may cause burns.
References
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
- ^ Joel Henry Hildebrand (2008). Principles of Chemistry. BiblioBazaar, LLC. p. 191. ISBN 0559318774.
- ^ Frank Welcher (2008). Chemical Solutions. READ BOOKS. p. 48. ISBN 1443729078.
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Hitomi Suzuki; Yoshihiro Matano (2001). Organobismuth chemistry. Elsevier. pp. 403–404. ISBN 0444205284.
 | This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |