Rhenium(IV) oxide
From Wikipedia the free encyclopedia
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| Names | |
|---|---|
| IUPAC name Rhenium(IV) oxide | |
| Other names Rhenium dioxide | |
| Identifiers | |
3D model (JSmol) | |
| ECHA InfoCard | 100.031.659 |
| EC Number |
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PubChem CID | |
CompTox Dashboard (EPA) | |
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| Properties | |
| ReO2 | |
| Molar mass | 218.206 g/mol |
| Appearance | gray orthorhombic crystals |
| Density | 11.4 g/cm3[1] |
| Melting point | decomposes at 1000 °C[2] |
| insoluble | |
| Solubility in alkali | insoluble |
| +44.0·10−6 cm3/mol | |
| Structure | |
| Orthorohmbic, oP12 | |
| Pbcn, No. 60 | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Safety data sheet (SDS) | Aldrich MSDS |
| Related compounds | |
Other anions | Rhenium(VII) oxide Rhenium(III) oxide Rhenium(III) chloride |
Other cations | manganese(IV) oxide Technetium(IV) oxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
Rhenium(IV) oxide or rhenium dioxide is the inorganic compound with the formula ReO2. This gray to black crystalline solid is a laboratory reagent that can be used as a catalyst. It adopts the rutile structure.
Synthesis and reactions
[edit]It forms via comproportionation:[3]
- 2 Re2O7 + 3 Re → 7 ReO2
Single crystals are obtained by chemical transport, using iodine as the transporting agent.:[4]
- ReO2 + I2 ⇌ ReO2I2
At high temperatures it undergoes disproportionation:
- 7 ReO2 → 2 Re2O7 + 3 Re
It forms rhenates with alkaline hydrogen peroxide and oxidizing acids.[5] In molten sodium hydroxide it forms sodium rhenate:[6]
- 2 NaOH + ReO2 → Na2ReO3 + H2O
References
[edit]- ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). CRC Press. p. 484. ISBN 0-8493-0594-2. Retrieved 2008-06-05.
- ^ Perry, Dale L.; Phillips, Sidney L. (1995). Handbook of Inorganic Compounds. San Diego: CRC Press. p. 328. ISBN 0-8493-8671-3. Retrieved 2008-06-05.
- ^ G. Glemser "Rhenium (IV) Oxide" Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1480.
- ^ Rogers, D. B.; Butler, S. R.; Shannon, R. D. (1972). Single Crystals of Transition-Metal Dioxides. Inorganic Syntheses. Vol. XIII. pp. 135–145. doi:10.1002/9780470132449.ch27. ISBN 9780470131725.
- ^ "RHENIUM DIOXIDE - Manufacturer". Aaamolybdenum.com. Archived from the original on 2003-02-09. Retrieved 2012-08-06.
- ^ G. Glemser "Sodium Rhenate (IV)" Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1483.