Rhenium(IV) oxide
The topic of Rhenium(IV) oxide is one that has been widely discussed over the years. With divergent opinions and varied points of view, Rhenium(IV) oxide has captured the interest of experts and enthusiasts alike. In this article, we will explore the different facets of Rhenium(IV) oxide, offering a comprehensive analysis covering its history, impact, and possible implications for the future. From its origin to its current evolution, Rhenium(IV) oxide has left a significant mark on the world that deserves meticulous and detailed attention.
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| Names | |
|---|---|
| IUPAC name
Rhenium(IV) oxide
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| Other names
Rhenium dioxide
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.031.659 |
| EC Number |
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PubChem CID
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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
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Rhenium(VII) oxide Rhenium(III) oxide Rhenium(III) chloride |
Other cations
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manganese(IV) oxide Technetium(IV) oxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).
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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
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
- ^ 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. Wiley. 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.