Trimethyl borate

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]

Green fire of boric acid in methanol
Trimethyl borate
Names
Other names
trimethoxyborane, boron trimethoxide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.004.063
EC Number
  • 204-468-9
UNII
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
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).
Y verify (what is YN ?)
Infobox references

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


Applications

Trimethyl borate is the main precursor to sodium borohydride by its reaction with sodium hydride:

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


gollark: I could buy all diamonds, if someone lowered the price to about .001KST.
gollark: not possible
gollark: no financial incentive
gollark: Again:
gollark: *Gollark's Tiny Diamond Store: Exploiting 5cn's ridiculous plans since 27 BC*

References
  1. Robert J. Brotherton, C. Joseph Weber, Clarence R. Guibert, John L. Little (2000). "Boron Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH.CS1 maint: uses authors parameter (link)
  2. M.A. Beckett, G.C. Strickland, J.R. Holland, and K.S. Varma, "A convenient NMR method for the measurement of Lewis acidity at boron centres: correlation of reaction rates of Lewis acid initiated epoxide polymerizations with Lewis acidity", Polymer, 1996, 37, 4629–4631. doi: 10.1016/0032-3861(96)00323-0
  3. Kazuaki Ishihara, Suguru Ohara, Hisashi Yamamoto (2002). "3,4,5-Trifluorophenylboronic Acid". Organic Syntheses. 79: 176.CS1 maint: multiple names: authors list (link); Collective Volume, 10, p. 80
  4. R. L. Kidwell, M. Murphy, and S. D. Darling (1969). "Phenols: 6-Methoxy-2-naphthol". Organic Syntheses. 49: 90.CS1 maint: multiple names: authors list (link); Collective Volume, 10, p. 80
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.