Rhenium(IV) oxide

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Rhenium(IV) oxide
     Re      O
IUPAC name
Rhenium(IV) oxide
Other names
Rhenium dioxide
3D model (Jmol)
ECHA InfoCard 100.031.659
EC Number 234-839-0
Molar mass 218.206 g/mol
Appearance gray orthorhombic crystals
Density 11.4 g/cm3[1]
Melting point decomposes at 1000 °C[2]
Solubility in alkali insoluble
+44.0·10−6 cm3/mol
Orthorohmbic, oP12
Pbcn, No. 60
Safety data sheet Aldrich MSDS
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
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).
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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[edit]

It forms via comproportionation:[3]

2 Re2O7 + 3 Re → 7 ReO2

At high temperatures it undergoes disproportionation:

7 ReO2 → 2 Re2O7 + 3 Re

It forms perrhenates with alkaline hydrogen peroxide and oxidizing acids.[4] In molten sodium hydroxide it forms sodium rhenate:[5]

2 NaOH + ReO2 → Na2ReO3 + H2O


  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. ^ "RHENIUM DIOXIDE - Manufacturer". Aaamolybdenum.com. Retrieved 2012-08-06. 
  5. ^ G. Glemser "Sodium Rhenate (IV)" Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1483.