Rhenium(VII) oxide

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Rhenium(VII) oxide
Rhenium(VII) oxide
Rhenium(VII) oxide
Names
Other names
Rhenium heptoxide
Identifiers
3D model (
JSmol
)
ECHA InfoCard
 100.013.857 Edit this at Wikidata
EC Number
  • 215-241-9
UNII
  • Key: NBGOSNNAAHDRLK-UHFFFAOYSA-N
  • InChI=1S/7O.2Re
SMILES
  • O=[Re](=O)(=O)O[Re](=O)(=O)=O
Properties
Re2O7
Molar mass 484.40298 g/mol
Appearance yellow crystalline powder
Density 6.103 g/cm3, solid
Melting point 360 °C (680 °F; 633 K)
Boiling point sublime
Hydrolyses
Hazards
GHS labelling:[1]
GHS05: Corrosive
Danger
H314
P260, P264, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P405, P501
Related compounds
Related compounds
Manganese(VII) oxide; technetium(VII) oxide; perrhenic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Rhenium(VII) oxide is the

anhydride of HOReO3. Perrhenic acid, Re2O7·2H2O, is closely related to Re2O7. Re2O7 is the raw material for all rhenium compounds, being the volatile fraction obtained upon roasting the host ore.[2]

Structure

Solid Re2O7 consists of alternating octahedral and tetrahedral Re centres. Upon heating, the polymer cracks to give molecular (nonpolymeric) Re2O7. This molecular species closely resembles manganese heptoxide, consisting of a pair of ReO4 tetrahedra that share a vertex, i.e., O3Re–O–ReO3.[3]

Synthesis and reactions

Rhenium(VII) oxide is formed when metallic rhenium or its oxides or sulfides are oxidized at 500–700 °C (900–1,300 °F) in air.[4]

Re2O7 dissolves in water to give perrhenic acid.

Heating Re2O7 gives

rhenium dioxide, a reaction signalled by the appearance of the dark blue coloration:[5]

2Re2O7 → 4ReO2 + 3O2

Using tetramethyltin, it converts to methylrhenium trioxide ("MTO"), a catalyst for oxidations:[6]

Re2O7 + 2Sn(CH3)4 → CH3ReO3 + (CH3)3SnOReO3

In a related reaction, it reacts with hexamethyldisiloxane to give the siloxide:[4]

Re2O7 + 2O(Si(CH3)3)2 → 2(CH3)3SiOReO3

Uses

Hydrogenation catalyst

Rhenium(VII) oxide finds some use in

catalyst for ethenolysis,[7] carbonyl reduction and amide reduction.[8]

References

  1. ^ "Rhenium(VII) oxide". pubchem.ncbi.nlm.nih.gov. Retrieved 14 December 2021.
  2. ISBN 3527306730
    .
  3. ISBN 0-19-855370-6
    .
  4. ^
    ISBN 9780470132401
    .
  5. ^ Glemser, O. (1963). "Rhenium". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry. Vol. 1 (2nd ed.). Academic Press. pp. 1476–1485.
  6. doi:10.1021/ar9601398
    .
  7. ISBN 9780471238966
  8. ISBN 978-0-471-39698-7
    .
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