Difluorocarbene
Names
Preferred IUPAC name
Difluoromethylidene
Other names
Difluoromethylene
Identifiers
ECHA InfoCard 100.128.429
  • InChI=1S/CF2/c2-1-3
    Key: LTVOKYUPTHZZQH-UHFFFAOYSA-N
  • [C](F)F
Properties
CF2
Molar mass 50.008 g·mol−1
Related compounds
Other anions
 Methylene
Dichlorocarbene
Dibromocarbene
Diiodocarbene
Other cations
 Difluorosilylene
Difluorogermylene
Stannous fluoride
Plumbous fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Difluorocarbene is the chemical compound with formula CF2. It has a short half-life, 0.5 and 20 ms, in solution and in the gas phase, respectively.[1] Although highly reactive, difluorocarbene is an intermediate in the production of tetrafluoroethylene, which is produced on an industrial scale as the precursor to Teflon (PTFE).

Bonding in difluorocarbene

Fig. 1: The electron distribution in a singlet carbene. The empty p-orbital perpendicular to the plane of the other bonds is not shown
Fig. 2: Molecular orbitals for three contributing p-orbitals

In general, carbenes exist in either singlet or triplet states, which are often quite close in energy. Singlet carbenes have spin-paired electrons and a higher energy empty 2p orbital. In a triplet carbene, one electron occupies the hybrid orbital and the other is promoted to the 2p orbital.[2] For most carbenes, the triplet state is more stable than the corresponding singlet. In the case of fluorinated carbenes, however, the singlet is lower energy than the triplet.[3] The difference in energy between the singlet ground state and the first excited triplet state is 56.6 kcal per mol.[3] In singlet difluorocarbene, the C-F bond length is measured as 1.300 Å and F-C-F bond angle is measured as 104.94° (almost tetrahedral). On the other hand for the triplet state, the C-F bond length is measured as 1.320 Å and F-C-F bond angle is measured as 122.3° (slightly more, due to steric repulsion, than expected in an sp2 carbon).

The reasoning for the difference between the two carbenes is outlined in the two figures on the left. Figure 1 depicts the electron distribution in a singlet carbene, figure 2 shows the orbitals available to π-electrons. The molecular orbitals are built from an empty p-orbital on the central carbon atom and two orbitals on the fluorine atoms. Four electrons, the carbon orbital is empty, the fluorine orbitals both carry two electrons, need to find a place, thus filling the lower two of the MO-set. The non-bonding electrons of the carbene now need to be placed either double in the rather low energy sp2 orbital on carbon or in the highest anti-bonding level of the MO-system. Clearly in CF2 the singlet is the most favorable state.

In ordinary carbene, no π-MO-system is present, so the two non-bonding electrons can be placed in the two non-bonding orbitals on the carbon atom. Here avoiding the double negative charge in one orbital leads to a triplet carbene.

Preparation

Thermolysis of sodium chlorodifluoroacetate was established as the first method of the preparation of difluorocarbene. The generation of difluorocarbene involves loss of carbon dioxide and chloride.[2] [4]

ClF
2CCO
2− → CO
2+ ClF
2C−
ClF
2C− → CF
2+ Cl−

Alternatively, dehydrohalogenation of chlorodifluoromethane or bromodifluoromethane using alkoxides or alkyllithium also produces difluorocarbene:

NaOR + HCF
2Cl → CF
2+ HOR + NaCl

A variant of this reaction is using ethylene oxide in conjunction with a catalytic amount of quaternary ammonium halide at elevated temperature. In equilibrium a small amount of β-haloalkoxide is present that acts as a base. This avoids an excess concentration of base that will destroy the carbene just formed.

Thermolysis of hexafluoropropylenoxide at 190 °C gives difluorocarbene and trifluoroacetyl fluoride. This is an attractive method for the synthesis of difluorocyclopropanes as hexafluoropropylenoxide is inexpensive and the byproduct trifluoroacetyl fluoride is a gas.

Application

The thermolysis of chlorodifluomethane between 600 and 800 °C gives 1,1,2,2-tetrafluoroethylene (TFE).[2][4] The required CHClF
2 is generated by fluorination of chloroform.

CHCl
3+ 2 HF → CHClF
2+ 2 HCl
2 CHClF
2 → C
2F
4+ 2 HCl

TFE, tetrafluoroethylene C
2F
4, is also produced by dehalogenation of bromofluoro-, or iodofluoroalkanes with zinc and alcohol, by dehydrohalogenation of hydrogen-containing haloalkenes with alcoholic alkali, or by heating.[5] The industrial annual production of PTFE, generated by polymerization of tetrafluoroethylene (TFE), in 1991 was 9000 tons.[4]

Difluorocarbene is used to generate geminal difluorocyclopropanes.

See also

References

  1. ↑ Douglas A Jean Osteraas "Difluorocarbene Modification of Polymer and Fiber Surfaces," Journal of Applied Polymer1969, volume 13, 1523-1535. doi:10.1002/app.1969.070130715
  2. 1 2 3 Jones. Maitland.Organic Chemistry, 3rd ed, W. W. Norton, 2005, 460-465. ISBN 0-393-92408-4.
  3. 1 2 Dana Lyn S. Brahms, William P. Dailey. "Fluorinated Carbenes," Chem. Rev., American Chemical Society, 1996, 96, 1585-1632 doi:10.1021/cr941141k
  4. 1 2 3 Subhash V. Gangal."Fluorine-Containing Polymers, Polytetrafluoroethylene," Encyclopedia of Chemical Technology, John Wiley & Sons, New York, 1994. doi:10.1002/0471238961.1615122507011407.a01
  5. ↑ William X. Bajzer "Fluorine Compounds, Organic," Kirk-Othmer Encyclopedia of Chemical Technology, John Wiley & Sons, New York, 2004. doi:10.1002/0471238961.0914201802011026.a01.pub2
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