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BBr3 is the currect answer!!
Boron tribromide is the STRONGEST Lewis acid known…and this is the experimental fact despite the reduced electronegativity of bromine as compared to fluorine, and chlorine. So why so? For boron trifluoride, and the trichloride, donation from the lone pairs of the halogen to the empty p-orbital on boron is fairly effective. In the case of bromine, the lone pairs are larger and more diffuse and LESS capable of this donation….and as a result the boron centre is more electropositive, and Lewis-acidic…. Of course, we might also finger boron triiodide as a strong Lewis acid by this same argument, however, (and I have NEVER used this reagent!), it tends not to figure in these scenarios perhaps because of the expense, and its particularly high molar mass.
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Boron tribromide is the STRONGEST Lewis acid known…and this is the experimental fact despite the reduced electronegativity of bromine as compared to fluorine, and chlorine. So why so? For boron trifluoride, and the trichloride, donation from the lone pairs of the halogen to the empty p-orbital on boron is fairly effective. In the case of bromine, the lone pairs are larger and more diffuse and LESS capable of this donation….and as a result the boron centre is more electropositive, and Lewis-acidic…. Of course, we might also finger boron triiodide as a strong Lewis acid by this same argument, however, (and I have NEVER used this reagent!), it tends not to figure in these scenarios perhaps because of the expense, and its particularly high molar mass.
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BBr3
is the answer
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is the answer
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