Diboron tetrafluoride

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Diboron tetrafluoride
Stick model of diboron tetrafluoride
Space-filling model of the diboron tetrafluoride molecule
Names
Preferred IUPAC name
Diboron tetrafluoride
Systematic IUPAC name
Tetrafluorodiborane
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/B2F4/c3-1(4)2(5)6
    Key: WUWOPJNIAKTBSJ-UHFFFAOYSA-N
  • FB(F)B(F)F
Properties
Chemical formula
 B2F4
Molar mass 97.616 g/mol
Appearance Colorless gas
Density 4.3 kg/m3 (gas)
Melting point −56 °C (−69 °F; 217 K)
Boiling point −34 °C (−29 °F; 239 K)
Thermochemistry
79.1 J/mol K
317.3 J/mol K
Std enthalpy of
formation (ΔfH⦵298)
 -1440.1 kJ/mol
Gibbs free energy (ΔfG˚)
 -1410.4 kJ/mol
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Diboron tetrafluoride is the inorganic compound with the formula (BF2)2. A colorless gas, the compound has a halflife of days at room temperature. It is the most stable of the diboron tetrahalides.[1]

Structure and bonding[]

Diboron tetrafluoride is a planar molecule with a B-B bond distance of 172 pm.[1] Although it is electron-deficient, the unsaturated boron centers are stabilized by pi-bonding with the terminal fluoride ligands. The compound is isoelectronic with oxalate.

Synthesis and reactions[]

Diboron tetrafluoride can be formed by treating boron monofluoride with boron trifluoride at low temperatures, taking care not to form higher polymers.[2]

Addition of diboron tetrafluoride to Vaska's complex was employed to produce an early example of a transition metal boryl complex:[3]

2 B2F4 + IrCl(CO)(PPh3)2 → Ir(BF2)3(CO)(PPh3)2 + ClBF2

Historical literature[]

  • Louis Trefonas and William N. Lipscomb (1958). "Crystal and Molecular Structure of Diboron Tetrafluoride, B2F4". J. Chem. Phys. 28 (1): 54–55. doi:10.1063/1.1744079.
  • Gayles, J. N.; Self, J. (1964). "Infrared Spectrum of Diboron Tetrafluoride in the Gaseous and Solid States". Journal of Chemical Physics. 40 (12): 3530–3539. doi:10.1063/1.1725048.
  • Arthur Finch and Hermann Irving Schlesinger (1958). "Diboron Tetrafluoride". J. Am. Chem. Soc. 80 (14): 3573–3574. doi:10.1021/ja01547a020.
  • A. K. Holliday; F. B. Taylor (1964). "Diboron tetrafluoride. Part II. Reactions with some oxides and organometallic compounds". J. Chem. Soc.: 2731–2734. doi:10.1039/JR9640002731.
  • Vernon H. Dibeler; Susan K. Liston (1968). "Mass-spectrometric study of photoionization. XII. Boron trifluoride and diboron tetrafluoride". J. Chem. Soc. 7 (9): 1742–1746. doi:10.1021/ic50067a010.

References[]

  1. ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  2. ^ P. L. Timms (1972). Low Temperature Condensation. Advances in Inorganic Chemistry and Radiochemistry. p. 143. ISBN 0-12-023614-1.
  3. ^ Neeve, Emily C.; Geier, Stephen J.; Mkhalid, Ibraheem A. I.; Westcott, Stephen A.; Marder, Todd B. (2016). "Diboron(4) Compounds: From Structural Curiosity to Synthetic Workhorse". Chemical Reviews. 116 (16): 9091–9161. doi:10.1021/acs.chemrev.6b00193. PMID 27434758.


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