Ethylene dione

Source: Wikipedia, the free encyclopedia.
Not to be confused with Ethylene oxide.
Ethylene dione
Ball-and-stick model of ethylene dione
Names
IUPAC name
Ethene-1,2-dione
Systematic IUPAC name
Ethenedione
Other names
    • Dicarbon dioxide
    • Dimeric carbon monoxide
    • Dimeric carbonous oxide
    • Dimeric carbon(II) oxide
    • Ethylenedione
    • Oxygen percarbide
Identifiers
3D model (
JSmol
)
ChemSpider
UNII
  • InChI=1S/C2O2/c3-1-2-4
    Key: FONOSWYYBCBQGN-UHFFFAOYSA-N
  • O=C=C=O
Properties
C2O2
Molar mass 56.020 g·mol−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Ethylene dione or ethylenedione, also called dicarbon dioxide, Carbon peroxide, ethenedione, or ethene-1,2-dione, is a

dimer of carbon monoxide.[1] It can also be thought of as the dehydrated form of glyoxylic acid (H(C=O)COOH), or a ketone of ethenone
H2C=C=O.

Synthesis attempts

The existence of ethylenedione was first suggested in 1913.

hypothetical compound, or at best an "exceedingly coy molecule".[3]

In 2015, a research group reported the creation of ethylenedione — by using

anion C2O−2 — and its spectroscopic characterization.[4] However, the reported spectrum was later found to match that of the oxyallyl diradical, (H2C•)2CO, formed by rearrangement or disproportionation under the high-energy experimental conditions rather than simple electron loss.[5]

Theoretical investigations

Despite the existence of the

electronic structure motif similar to the oxygen molecule. However, when the molecule is distorted away from its equilibrium geometry, the potential surfaces of the triplet and singlet states intersect, allowing for intersystem crossing to the singlet state, which is unbound and dissociates to two ground-state CO molecules. The timescale of the intersystem crossing was predicted to be 0.5 ns,[6]
making triplet ethylenedione a transient, yet spectroscopically long-lived molecule.

On the other hand, the mono

anion of ethylenedione, OCCO−, as well as the dianion C
2O2−
2, called acetylenediolate, are both stable.[7][8]

Recent theoretical computations suggest that the in situ preparation and characterization of ethylenedione may be possible through low-energy free-electron induced single-molecule engineering.[1]

Koch's glyoxylide

In the 1940s,

FDA.[9]

See also

References

  1. ^
    PMID 28249449
    .
  2. ^ H. Staudinger, E. Anthes, Ber. Dtsch. Chem. Ges. 1913, 46, 1426.
  3. Bibcode:2008moma.book.....L
  4. doi:10.1002/anie.201503423
    .
  5. doi:10.1002/anie.201801848
  6. ^ D. Schröder, C. Heinemann, H. Schwarz, J. N. Harvey, S. Dua, S. J. Blanksby, and John, H. Bowie, "Ethylenedione: An Intrinsically Short-Lived Molecule", Chem. Eur. J., 4, 2550-2557 (1998).
  7. ^ J. R. Thomas, B. J. DeLeeuw, P. O’Leary, H. F. Schaefer III, B. J. Duke, B. O’Leary "The ethylenedione anion: Elucidation of the intricate potential energy hypersurface", J. Chem. Phys, 102, 6525-6536(1995).
  8. ^ P. Pyykkö and N. Runeberg, "Ab initio studies of bonding trends: Part 8. The 26-electron A≡B-C≡Dn and the 30-electron A=B=C=Dn systems", J. Mol. Struct. THEOCHEM, 234, 269-277(1991).
  9. ^ Goodrich, William W. (October 15–16, 1986). "FDA Oral History Interview, Goodrich" (PDF) (Interview). Interviewed by Ronald T. Ottes and Fred L. Lofsvold. p. 31.
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