# What is the mechanism of trialkylborane oxidation with hydroperoxide?

This is the mechanism of trialkylborane. In this mechanism I can't understand why should the -OH group leave and the -R group enter in its place to form borate ester. Can someone please explain me that step?

• The carbon migrates because peroxide bonds are generally weak and dissociate quite easily. – Gokul Apr 28 '15 at 16:57
• Also, the mechanism is drawn poorly. In the species labeled "Unstable intermediate," the left arrow should not point towards the boron or the bond; the arrow head should terminate at the left oxygen. – Zhe Oct 19 '16 at 17:47
• @Zhe Yes. In the upper mechanism, curved arrows are drawn in a wrong way. The arrowhead should be placed pointing towards boron in two of the curved arrows. – Apoorv Potnis Mar 11 '18 at 12:38

One aspect is the release of the stable anion $\ce{OH-}$.
Another aspect is that $\ce{B-O}$ bonds are much stronger than $\ce{B-C}$ bonds because the empty p-orbital of boron overlaps with one p-orbital with a lone electron pair of oxygen.
$\ce{B-C}$ $D_{298}^ \circ = 448 \pm 29\ \mathrm{kJ\ mol^{-1}}$
$\ce{B-O}$ $D_{298}^ \circ = 809\ \mathrm{kJ\ mol^{-1}}$