As the size of halogen atom increases, the acidic strength of boron halides increases. Thus, BF3 is the weakest Lewis acid. This is because of the pπ−pπ back bonding between the fully filled unutilised 2p-orbitals of F and vacant 2p-orbitals of boron which makes BF3 less electron deficient. Such backdonation is not possible in case of BCl3‌or‌B‌B‌r3 due to larger energy difference between their orbitals. Thus, these are more electron deficient. Since on moving down the group the energy difference increases, the Lewis acid character also increases. Thus, the tendency to behave as Lewis acid follows the order BBr3>BCl3>BF3