Trimethyl borate

Trimethyl borate
Names
IUPAC name
Trimethyl borate
Other names
Trimethoxyborane
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.004.063
EC Number
  • 204-468-9
UNII
  • InChI=1S/C3H9BO3/c1-5-4(6-2)7-3/h1-3H3 checkY
    Key: WRECIMRULFAWHA-UHFFFAOYSA-N checkY
  • InChI=1/C3H9BO3/c1-5-4(6-2)7-3/h1-3H3
    Key: WRECIMRULFAWHA-UHFFFAOYAY
  • O(B(OC)OC)C
Properties
C3H9BO3
Molar mass 103.91 g·mol−1
Appearance colourless liquid
Density 0.932 g/ml
Melting point −34 °C (−29 °F; 239 K)
Boiling point 68 to 69 °C (154 to 156 °F; 341 to 342 K)
decomposition
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 flammable
Related compounds
Other cations
 Trimethyl phosphite
Tetramethyl orthosilicate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Trimethyl borate is the organoboron compound with the formula B(OCH3)3. It is a colourless liquid that burns with a green flame.[1] It is an intermediate in the preparation of sodium borohydride and is a popular reagent in organic chemistry. It is a weak Lewis acid (AN = 23, Gutmann-Beckett method).[2]

This chemical is quite flammable and burns with a green flame

Borate esters are prepared by heating boric acid or related boron oxides with alcohols under conditions where water is removed by azeotropic distillation. [1]

Applications

Trimethyl borate is the main precursor to sodium borohydride by its reaction with sodium hydride in the Brown-Schlesinger process:

4 NaH + B(OCH3)3 → NaBH4 + 3 NaOCH3

It is a gaseous anti-oxidant in brazing and solder flux. Otherwise, trimethyl borate has no announced commercial applications. It has been explored as a fire retardant, as well as being examined as an additive to some polymers.[1]

Organic synthesis

It is a useful reagent in organic synthesis, as a precursor to boronic acids, which are used in Suzuki couplings. These boronic acids are prepared via reaction of the trimethyl borate with Grignard reagents followed by hydrolysis:.[3][4]

ArMgBr + B(OCH3)3 → MgBrOCH3 + ArB(OCH3)2
ArB(OCH3)2 + 2 H2O → ArB(OH)2 + 2 HOCH3

References

  1. ^ a b c Robert J. Brotherton; C. Joseph Weber; Clarence R. Guibert; John L. Little (2000). "Boron Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. ISBN 978-3-527-30673-2.
  2. ^ Beckett, M. A.; Strickland, G. C.; Holland, J. R.; Varma, K. S. (September 1996). "A convenient n.m.r. method for the measurement of Lewis acidity at boron centres: correlation of reaction rates of Lewis acid initiated epoxide polymerizations with Lewis acidity". Polymer. 37 (20): 4629–4631. doi:10.1016/0032-3861(96)00323-0.
  3. ^ Ishihara, Kazuaki; Ohara, Suguru; Yamamoto, Hisashi (2002). "3,4,5-Trifluorophenylboronic Acid". Organic Syntheses. 79: 176; Collected Volumes, vol. 10, p. 80.
  4. ^ Kidwell, R. L.; Murphy, M.; Darling, S. D. (1969). "Phenols: 6-Methoxy-2-naphthol". Organic Syntheses. 49: 90; Collected Volumes, vol. 10, p. 80.
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