Answer:
Both of them are Lewis acids but
because of\[p\pi -p\pi \] back bonding, the electron density on boron atom
increases and the Lewis acid strength of the halides decreases. Now, \[2p\]orbitals
of boron and fluorine that are involved in back bonding have comparable
energies, while \[2p\]orbitals of boron and \[4p\] orbitals of bromine differ
largely in energy and the back bonding is not so effective. Therefore, \[BB{{r}_{3}}\]
is a stronger acid than\[B{{F}_{3}}.\]
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