Rhenium(IV) oxide

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Rhenium(IV) oxide
Rutile-unit-cell-3D-balls.png
  Re   O
Names
IUPAC name
Rhenium(IV) oxide
Other names
Rhenium dioxide
Identifiers
3D model (JSmol)
ECHA InfoCard 100.031.659 Edit this at Wikidata
EC Number
  • 234-839-0
  • InChI=1S/2O.Re
  • O=[Re]=O
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
Safety data sheet (SDS) Aldrich MSDS
NFPA 704 (fire diamond)
1
0
0
Related compounds
Other anions
 Rhenium(VII) oxide

Rhenium(III) chloride
Other cations
 manganese(IV) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

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 perrhenates with alkaline hydrogen peroxide and oxidizing acids.[5] In molten sodium hydroxide it forms sodium rhenate:[6]

2 NaOH + ReO2 → Na2ReO3 + H2O

References[]

  1. ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). CRC Press. p. 484. ISBN 0-8493-0594-2. Retrieved 2008-06-05.
  2. ^ 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.
  3. ^ G. Glemser "Rhenium (IV) Oxide" Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1480.
  4. ^ Rogers, D. B.; Butler, S. R.; Shannon, R. D. (1972). "Single Crystals of Transition-Metal Dioxides". Inorganic Syntheses. XIII: 135–145. doi:10.1002/9780470132449.ch27.
  5. ^ "RHENIUM DIOXIDE - Manufacturer". Aaamolybdenum.com. Archived from the original on 2003-02-09. Retrieved 2012-08-06.
  6. ^ G. Glemser "Sodium Rhenate (IV)" Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1483.


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