Boron monofluoride monoxide

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Boron oxyfluoride
Names
IUPAC name
Fluoro(oxo)borane
Other names
boron monofluoride monoxide
Identifiers
3D model (
JSmol
)
ChemSpider
  • InChI=1/BFO/c2-1-3
    Key: FHYICEHKTRQYRP-UHFFFAOYSA-N
  • B(=O)F
Properties
BFO
Molar mass 45.81 g·mol−1
Appearance Gas
Thermochemistry
Std enthalpy of
formation
(ΔfH⦵298)
 48.0 ± 3.0 kcal/mol[1]
Related compounds
Related oxyhalides
 boron oxychloride
Related compounds
 boron monofluoride
boron monoxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Boron monofluoride monoxide or oxoboryl fluoride

inert gas matrix, and has been condensed in solid neon and argon.[3] When an attempt is made to condense the gas to a solid in bulk, a polymeric glass is formed, which is deficient in fluoride, and when heated forms a glassy froth like popcorn.[4][5] Boron fluoride oxide has been studied because of its production in high energy rocket fuels that contain boron and fluorine, and in the form of an oxyfluoride glass. BOF glass is unusual in that it can condense directly from gas.[6]

Properties

Monomer

The FBO molecule is linear with structure F-B=O. The F-B bond length is 1.283 Å, and B-O bond is 1.207 Å.[7]

The infrared spectrum of BFO has vibrational bands at 1900, 1050, and 500 cm−1.[8] Spectroscopic constants of the 10BFO molecule are B=9349.2711 MHz D=3.5335 kHz and for 11BFO molecule they are B=9347.3843 MHz D=3.5273 kHz[9] The monomer is stable either at low pressures, or temperatures over 1000 °C. Below this temperature, the monomers associate to form a trimer[10] called trifluoroboroxole.[11]

Heat of formation ΔfH⦵
298 K is predicted to be -146.1 kcal/mol. Proton affinity 149.6 kcal/mol.[12]

Trimer

If a hot BFO gas is cooled slowly it dismutates back into B2O3 and BF3.[13] At room temperature this dismutation completes in an hour.[13]

Boron fluoride oxide forms a trimer with a ring composed of alternating oxygen and boron atoms, with fluorine bonded to the boron. (BFO)3. The ring structure puts it in the class of boroxols.[14] This is also called trifluoroboroxin. The trimer is the predominant form in gas at 1000K.[13] When heated to 1200K it mostly converts to the monomer BFO.[13] Boron oxyfluoride can be condensed from vapour to a fluorine deficient glass at temperatures below 190° by very rapid cooling. When heated this deposit has a temperature at which it loses more BF3 to form a frothy or porous glass that resembles popcorn. The glass deposited at lower temperatures has a higher proportion of fluorine. Deposits at -40 °C are predicted to have a 1:1 ratio of fluorine to oxygen.[5] Below -135° (BFO)3 is stable.[15]

The heat of formation of the trimer from the monomer (BFO)3 → 3BFO is 131 kcal/mol.[16]

Glass

Boron oxyfluoride glass is transparent and colourless. It is stable in dry air, but it is hygroscopic and in normal air becomes white and opaque. When heated the glass will encounter a glass transition temperature (Tg) at which it ceases to be a glass, and produces BF3 gas and a boron oxyfluoride with less fluorine is left behind. This glass transition temperature is determined from where the pressure of BF3 produced exceeds the strength of the glass. The hypothetical structure of BOF glass, is of long chains of B-O-B-O with fluorine attached to each boron. These can be considered as BO2F triangles linked in a chain by O atoms. These chains are tangled up like spaghetti in the glass. When the substance becomes fluorine deficient, crosslinks with oxygen form between the chains, and it becomes more two dimensional in structure.[17] BF3 is produced when the terminals of two linear −(BF)O− chains join with each other.[6] These ends contain -O-BF2, and when two meet, BF3 can be eliminated and the chain extended with oxygen.[18]

Occurrence

BFO is expected to form in supernovae II output in gas between 1,000 and 2,000 °C and pressures around 10−7 bar.[19]

Preparation

Otto Ruff noticed that a mixture of BF3 and SiF4 passing over molten B2O3 produced some SiO2 and redistributed B2O3 into cold parts of the reaction tube. He speculated that there must be some heat stable intermediate that converted back into the original components on cooling.[20][21] Several years later, Paul Baumgarten and Werner Bruns made the boron oxyfluoride trimer by passing BF3 over solid B2O3 at 450 °C.[20][22]

BFO is an intermediate in the hydrolysis of BF3 along with BF(OH)2, BF2OH and boric acid.

  • BF3 + H2O → BFO + 2HF;
  • BF2OH → BFO + HF;
  • BF(OH)2 → BFO + H2O[23]

Another way in which BFO can be made is to vapourise B2O3 with BF3.[5]

When BF3 is heated with air, BFO gas predominates from 2800° to 4000 °C, being a maximum at 3200°. Above 4000 °C BO dominates.[8]

Hot BF3 passed over some oxides such as SiO2 forms BFO.

alumina.[25]

In the plasma phase HF reacts with BO2H+
2, B2OH+, B3O+
4, B2O+
4, B2O+
2, B2OH+ to make FBO, and other products including FBOH and FBO+.[26]

Related

The B-O-F molecule theoretically exists but it releases energy when it rearranges to F-B-O.[27][28] A related molecule is BOF2.[29] Molecules related to the trimer include B3O3ClF2, B3O3Cl2F, and (BOCl)3.[30]

FBO is predicted to be able to insert noble gas atoms between the fluorine and boron atom yielding FArBO, FKrBO and FXeBO. The molecules are predicted to be linear.[31]

Uses

Boron oxyfluoride could be used in boriding steel. By using a gas, sticking solids onto the steel is avoided. Also this method allows control of the boron concentration, and mostly forms Fe2B instead of the more brittle FeB.[25] Burning boron releases much energy, so its use in explosives or fuel is being researched. To maximise energy output, both fluorine and oxygen are used to react, and thus FBO and related molecules are formed and may be in the exhaust.[26]

References

  1. doi:10.1021/ic00271a011. Retrieved 20 May 2015. {{cite journal}}: Cite journal requires |journal= (help
    )
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  7. doi:10.1063/1.453175
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  9. PMID 9645936
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  10. doi:10.1039/TF9625802090
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  11. ^ Thevenot, Francois H. J.; Goeuriot, Patrice M. V.; Driver, Julian H.; Lebrun, Jean-Paul R. (1982). "Apparatus for the boronizing of pieces made of metal or cermet and surface-bornished pieces".
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    doi:10.1016/0073-8085(68)80019-1
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  14. doi:10.1002/zaac.19522670102
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  15. ^ Fisher, H. D.; Kiehl, J.; Cane, A. (June 1961). "Infrared Spectra and Thermodynamic Properties of Trifluoroboroxine (FBO)3 Final Report HTC-61-90". Culver City, California: Hughs Tool Company Aircraft Division. Archived from the original on December 27, 2016. Retrieved 27 November 2016.
  16. doi:10.1063/1.1734569
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  17. doi:10.1016/0022-3093(95)00183-2
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  22. doi:10.1002/cber.19410740717
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  23. S2CID 91517483
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  24. doi:10.1016/0043-1648(83)90083-2
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  25. ^
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  26. ^ a b Smolanoff, Jason; Lapicki, Adom; Anderson, Scott L.; Sowa-Resat, Marianne (26 Dec 1994). "A Cluster Beam Study of Boron Oxide Chemistry With HF". Retrieved 1 December 2016.[dead link]
  27. doi:10.1016/0166-1280(85)80091-9
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  28. doi:10.1021/j100017a039
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  29. doi:10.1016/0022-2852(66)90242-6
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  30. doi:10.1016/0584-8539(67)80210-1
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  31. doi:10.1016/j.cplett.2004.12.090
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