Uranyl chloride
[O=U=O]Cl2 | |
| Names | |
|---|---|
| IUPAC name
Dichlorodioxouranium | |
| Other names
Uranium(VI), dichlorodioxy Uranium(VI) dichloride dioxide | |
| Identifiers | |
3D model (JSmol) |
|
| ChemSpider | |
| ECHA InfoCard | 100.029.315 |
| EC Number |
|
PubChem CID |
|
| UNII | |
CompTox Dashboard (EPA) |
|
| |
| |
| Properties | |
| UO2Cl2 | |
| Molar mass | 340.93 g·mol−1 |
| Appearance | bright yellow large crystals[1] |
| Melting point | Decomposes |
| Boiling point | Decomposes |
| soluble[1] | |
| Solubility | Soluble in alcohols, acetone and ethers,[1] insoluble in benzene |
| Hazards | |
| Safety data sheet (SDS) | External MSDS |
| Related compounds | |
Other anions |
|
Other cations |
|
Related uranium chlorides |
|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Uranyl chloride is the inorganic compound with the chemical formula UO2Cl2. It is a fluorescent water soluble compound.[1] Uranyl chloride also refers to inorganic compounds with the formula UO2Cl2(H2O)n where n = 0, 1, 2, or 3. These are yellow salts.
Synthesis and structures
[edit]
Anhydrous uranyl chloride is a coordination polymer. It reacts and depolymerizes upon treatment with water. The hydrates are also obtained by treating aqueous uranyl sulfate or uranyl acetate with hydrochloric acid. Depending on the method of drying, one obtains the mono- or the trihydrate. The monohydrate is described as a yellow, sulfur-like powder. It is very hygroscopic.[3] The trihydrate is greenish-yellow. Both hydrates are fluorescent solids that are highly soluble in water.[4]
The anhydrous material can be obtained by the reaction of oxygen with uranium tetrachloride:[citation needed]
- UCl4 + O2 → UO2Cl2 + Cl2
The anhydrous material can also be obtained by the heating the hydrate under a stream of gaseous hydrogen chloride.ref name=Brauer/>
In terms of structures, all three of these compounds feature the uranyl center (trans-UO2+2) bound to five additional ligands, which can include (bridging) chloride, water, or another uranyl oxygen.[5][6]
Reactions
[edit]The aquo ligands can be replaced by a variety of donors, e.g. THF.[7] Uranyl chloride, and its two hydrates, (UO2Cl2·H2O and UO2Cl2·3H2O) decompose in the presence of light. This photosensitivity over the years, from time to time, has attracted scientific interest and there have been various unsuccessful attempts to develop applications in photography using these compounds.[1]
Safety
[edit]Uranyl chloride is radioactive.[1]
References
[edit]- 1 2 3 4 5 6 "SPI-Chem Uranyl Chloride Trihydrate CAS # 13867-67-9 (Depleted Uranium) | Z02411 | SPI Supplies". www.2spi.com. Retrieved 2026-07-14.
- ↑ Debets, P. C. (1968). "The structures of uranyl chloride and its hydrates". Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry. 24 (3): 400–402. Bibcode:1968AcCrB..24..400D. doi:10.1107/S056774086800244X.
- ↑ Hefley, Jack D.; Mathews, Daniel M.; Amis, Edward S. (1963). "Uranyl Chloride 1-Hydrate". Inorganic Syntheses. Vol. 7. pp. 146–148. doi:10.1002/9780470132388.ch41. ISBN 978-0-470-13238-8.
{{cite book}}: ISBN / Date incompatibility (help) - ↑ F. Hein, S. Herzog (1963). "Uranyl Chloride". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1439.
- ↑ Taylor, J. C.; Wilson, P. W. (1973). "The Structure of Anhydrous Uranyl Chloride by Powder Neutron Diffraction". Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry. 29 (5): 1073–1076. Bibcode:1973AcCrB..29.1073T. doi:10.1107/S0567740873003882.
- ↑ Leary, Joseph A.; Suttle, John F. (1957). "Uranyl Chloride". Inorganic Syntheses. Vol. 5. pp. 148–150. doi:10.1002/9780470132364.ch41. ISBN 978-0-470-13236-4.
{{cite book}}: ISBN / Date incompatibility (help) - ↑ Wilkerson, Marianne P.; Burns, Carol J.; Paine, Robert T.; Scott, Brian L. (1999). "Synthesis and Crystal Structure of UO2Cl2(THF)3: A Simple Preparation of an Anhydrous Uranyl Reagent". Inorganic Chemistry. 38 (18): 4156–4158. doi:10.1021/ic990159g.
- "Uranium". Encyclopædia Britannica. Vol. V27. 1911. p. 788.
- Heyes, S.J. (1998). "Lanthanides & Actinides". Four Lectures in 2nd Year Inorganic Chemistry. Archived from the original on 23 September 2017. Retrieved 22 November 2011.
External links
[edit]- Settle, Frank. "Nuclear Chemistry and the Community". www.chemcases.com: General Chemistry Case Studies. Archived from the original on 22 November 2011. Retrieved 22 November 2011.
