Rhenium(IV) oxide

  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
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
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).
☒N verify (what is checkY☒N ?)

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

  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". Single Crystals of Transition-Metal Dioxides. Inorganic Syntheses. Vol. XIII. pp. 135–145. doi:10.1002/9780470132449.ch27. ISBN 9780470131725.
  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.
Categories