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Trimethyldiborane

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Trimethyldiborane
Names
IUPAC name
1,1,2-Trimethyldiborane
Other names
Trimethyldiborane(6)
Identifiers
3D model (JSmol)
  • InChI=1S/C3H12B2/c1-4-6-5(2,3)7-4/h4H,1-3H3
    Key: JDPNBQILNNVWNW-UHFFFAOYSA-N[1]
  • C[B]1(C)[H][BH](C)[H]1
Properties
(CH
3)
3B
2H
3
Molar mass 69.75 g mol−1
Appearance Colorless pyrophoric liquid
Melting point −122.9 °C (−189.2 °F; 150.2 K)
Boiling point 45.5 °C (113.9 °F; 318.6 K)
Thermochemistry
48 kcal/mol
Related compounds
Related alkyl boranes
 trimethylborane
tetramethyldiborane
dimethyldiborane
methyldiborane
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N (what is checkY☒N ?)

Trimethyldiborane, (CH3)3B2H3 is a molecule containing boron carbon and hydrogen. It is an alkylborane, consisting of three methyl group substituted for a hydrogen in diborane. It can be considered a mixed dimer: (CH3)2BH2BH(CH3) or dimethylborane and methylborane.[1] called 1,2-dimethyldiborane.[2] Other combinations of methylation occur on diborane, including monomethyldiborane, 1,2-dimethyldiborane, tetramethyldiborane, 1,1-dimethylborane and trimethylborane. At room temperature the substance is at equilibrium between these forms, so it is difficult to keep it pure.[3] The methylboranes were first prepared by H. I. Schlesinger and A. O. Walker in the 1930s.[4][5]

Formation

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Trimethylborane is formed by the reaction of diborane and trimethylborane. This reaction produces four different substitution of methyl with hydrogen on diborane. Produced is 1-methyldiborane, 1,1-dimethyldborane, 1,1,2-trimethyldiborane and 1,1,2,2-tetramethyldiborane. By reacting monomethyldiborane with ether, dimethylether borine is formed [(CH3)2O].BH3 leaving methylborane which rapidly dimerises to 1,2-dimethyldiborane.[3] The reaction is complex.[6] The yield of trimethyldiborane is maximised with ratio of 1 of diborane to 3 of trimethylborane.[7]

Tetramethyl lead can react with diborane in a 1,2-dimethoxyethane solvent at room temperature to make a range of methyl substituted diboranes, ending up at trimethylborane, but including 1,1-di, tridiborane. The other outputs of the reaction are hydrogen gas and lead metal.[8]

Other methods to form methyldiboranes include reacting hydrogen with trimethylborane between 80 and 200 °C under pressure, or reacting a metal borohydride with trimethylborane in the presence of hydrogen chloride, aluminium chloride or boron trichloride. If the borohydride is sodium borohydride, then methane is a side product. If the metal is lithium then no methane is produced.[4] Dimethylchloroborane and methyldichloroborane are also produced as gaseous products.[4]

When Cp2Zr(CH3)2 reacts with borane dissolved in tetrahydrofuran, a borohydro group inserts into the zirconium carbon bond, and methyl diboranes are produced.[9]

Properties

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Trimethyldiborane has two methyl groups on one boron atom, and one methyl and a hydrogen on the second boron atom. A bridge of two hydrogen atoms links the boron atoms together. The molecule is expected to have a Cs point group due to rapid rotation of the methyls. The infrared spectrum of trimethyldiborane has a strong absorption band at 2509 cm−1 due to the non-bridge boron-hydrogen bond.[10] It has a vapour pressure of 51 mm Hg at -22.8 °C; 61 mm Hg at -18.4 °C and[7] 83 mm Hg at 0 °C.[11] Vapour pressure can be approximated by Log P = 7.673 - (1527/T).[12] The boiling point is 45.5 °C, and the melting point is -122.9.[12]

The predicted heat of formation for liquid trimethyldiborane is ΔH0f=-48 kcal/mol, and for the gas -41 kcal/mol. Heat of vapourisation ΔHvap was measured at 7.0 kcal/mol.[13]

A gas chromatograph can be used to determine the amounts of the methyl boranes in a mixture. The order they pass through are diborane, monomethyldiborane, trimethylborane, 1,1-dimethyldiborane, 1,2-dimethyldiborane, trimethyldiborane, and lastly tetramethyldiborane.[14]

The nuclear resonance shift for the bridge hydrogen is 9.27 ppm, compared to 10.49 for diborane.[15]

Reactions

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Trimethyldiborane partially disproportionates over a period of hours at room temperature to yield tetramethyldiborane and 1,2-dimethyldiborane. Over a period of weeks 1,1-dimethyldiborane appears as well.[16]

3[1,1-(CH3)3B2H4] ⇌ 2 (CH3)3B2H3 + B2H6 K=0.00027[17]
4(CH3)3B2H3 ⇌ (CH3)4B2H2 + B2H6 K=0.0067[17]

Trimethyldiborane is hydrolyzed in water to methylboronic acid CH3B(OH)2 and dimethylborinic acid (CH3)2B(OH).[3]

Trimethyldiborane spontaneously inflames when exposed to air.[18]

Trimethyldiborane reacts with liquid ammonia initially forming methylborohydride anions and (CH3)2B(N3)2+ cations.[19][20][21]

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Trimethylborane (CH3)3B has a similar-sounding name, and many similar properties, but only has one boron atom.[4] Trimethylhydroborate (CH3)3BH− is an anion with one boron atom. It can form a lithium salt.[22]

References

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  1. ^ Srebnik, Morris; Cole, Thomas E.; Brown, Herbert C. (January 1987). "Methylborane - a remarkable unhindered monoalkylborane which achieves the controlled sequential hydroboration of representative alkenes". Tetrahedron Letters. 28 (33): 3771–3774. doi:10.1016/s0040-4039(00)96380-9.
  2. ^ Low, M. J. D. (1968). "Characteristic Infrared Frequencies of Methyldiboranes". The Journal of Chemical Physics. 48 (5): 2386–2387. Bibcode:1968JChPh..48.2386L. doi:10.1063/1.1669454.
  3. ^ a b c Bell, R. P.; Emeléus, H. J. (1948). "The boron hydrides and related compounds". Quarterly Reviews, Chemical Society. 2 (2): 132. doi:10.1039/QR9480200132.
  4. ^ a b c d Long, L. H.; Wallbridge, M. G. H. (1965). "646. The chemistry of boron. Part VI. New preparative methods and decomposition studies relating to methyldiboranes". Journal of the Chemical Society (Resumed): 3513–3520. doi:10.1039/JR9650003513. (subscription required)
  5. ^ Schlesinger, H. I.; Walker, A. O. (April 1935). "Hydrides of Boron. IV. The Methyl Derivatives of Diborane". Journal of the American Chemical Society. 57 (4): 621–625. doi:10.1021/ja01307a009.
  6. ^ van Aalten, Lloyd; Seely, G. R.; Oliver, Juhn; Ritter, D. M. (1 June 1961). Kinetics and Equilibria in the Alkylation of Diborane Preliminary Report (PDF). Advances in Chemistry. Vol. 32. American Chemical Society. pp. 107–114. doi:10.1021/ba-1961-0032.ch012. ISBN 0-8412-0033-5.
  7. ^ a b Carpenter, J.H.; Jones, W.J.; Jotham, R.W.; Long, L.H. (September 1971). "The Raman spectra of the methyldiboranes—II Monomethyldiborane and trimethyldiborane, and characteristic frequencies of the methyldiboranes". Spectrochimica Acta Part A: Molecular Spectroscopy. 27 (9): 1721–1734. Bibcode:1971AcSpA..27.1721C. doi:10.1016/0584-8539(71)80227-1.
  8. ^ Holliday, A.K.; N. Jessop, G. (November 1967). "The reaction of tetramethyllead with diborane". Journal of Organometallic Chemistry. 10 (2): 291–293. doi:10.1016/s0022-328x(00)93089-4.
  9. ^ Marsella, John A.; Caulton, Kenneth G. (May 1982). "Dealkylation of zirconium(IV) by borane: the intimate mechanism of an alkyl transfer reaction". Journal of the American Chemical Society. 104 (9): 2361–2365. doi:10.1021/ja00373a005.
  10. ^ Cowan, R. D. (1949). "The Infra-Red Spectra of Borine Carbonyl and Tetramethyldiborane". The Journal of Chemical Physics. 17 (2): 218. Bibcode:1949JChPh..17..218C. doi:10.1063/1.1747225.
  11. ^ Lamneck, John H. Jr; Kaye, Samuel (4 September 1958). "Thermal reaction of diborane with trimethylborane". National Advisory Committee for Aeronautics.
  12. ^ a b Onak, Thomas (1 January 1966). Stone, F. G. A.; West, Robert (eds.). Advances in Organometallic Chemistry. New York, London: Academic Press. p. 284. ISBN 9780080580043. Retrieved 14 August 2015.
  13. ^ Altschuller, Aubrey P. (4 October 1955). "Calculated Heats of Formation and Combustion of Boron Compounds (Boron, Hydrogen, Carbon, Silicon)" (PDF). NACA Research Memorandum. Cleveland, Ohio: National Advisory Committee for Aeronautics. p. 22. Retrieved 14 August 2015.
  14. ^ Seely, G. R.; Oliver, J. P.; Ritter, D. M. (December 1959). "Gas-Liquid Chromatographic Analysis of Mixtures Containing Methyldiboranes". Analytical Chemistry. 31 (12): 1993–1995. doi:10.1021/ac60156a032.
  15. ^ Leach, John B.; Ungermann, Charles B.; Onak, Thomas P. (January 1972). "Proton magnetic resonance studies on methyl and chloro substituted diboranes". Journal of Magnetic Resonance. 6 (1): 74–83. Bibcode:1972JMagR...6...74L. doi:10.1016/0022-2364(72)90088-1.
  16. ^ Lehmann, Walter J.; Wilson, Charles O.; Shapiro, I. (1961). "Infrared Spectra of Alkyldiboranes. V. Tri- and Tetramethyl- and Ethyldiboranes". The Journal of Chemical Physics. 34 (3): 783. Bibcode:1961JChPh..34..783L. doi:10.1063/1.1731675.
  17. ^ a b Onak, Thomas (1 January 1966). "Carboranes and Organo-Substituted Boron Hydrides". In Stone, F. G. A.; West, Robert (eds.). Advances in Organometallic Chemistry. New York, London: Academic Press. p. 284. ISBN 9780080580043. Retrieved 19 August 2015.
  18. ^ Urben, Peter; Pitt, M. J., eds. (2007). Bretherick's Handbook of Reactive Chemical Hazards (7th ed.). Amsterdam: Elsevier. p. 527. ISBN 978-0-12-373945-2.
  19. ^ Jungfleisch, Francis (1973). "Reactions of Methyl Substituted Diboranes and 2,2-Dimethyltetraborane with Amine Bases". Ohio State University. p. 64. Retrieved 15 August 2015.
  20. ^ Sheldon, J. C.; Smith, B. C. (1960). "The borazoles". Quarterly Reviews, Chemical Society. 14 (2): 202. doi:10.1039/QR9601400200.
  21. ^ Schlesinger, H. I.; Horvitz, Leo; Burg, A. B. (March 1936). "Hydrides of Boron. VI. The Action of Ammonia on the Methyl Diboranes". Journal of the American Chemical Society. 58 (3): 409–414. doi:10.1021/ja01294a008.
  22. ^ "inorganic materials research division - The Berkeley Lab" (PDF).

Extra reading

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  • Carpenter, J. H.; Jones, W. J.; Jotham, R. W.; Long, L. H. (1968). "Laser-source Raman spectroscopy and the Raman spectra of the methyldiboranes". Chemical Communications (15): 881. doi:10.1039/C19680000881.
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