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Why is #BF_3# considered to be a non-polar molecule, any yet #B-F# bonds are polar?

Answer 1

Molecular polarity results from the #"vector sum"# of the individual bond dipoles.

We know (i) the the #B-F# bond is polar; and (ii) that the #/_F-B-F# bond angles are #120""^@#. When the individual bond dipoles are summed in a vector fashion, the resultant is necessarily #0#. Thus boron trifluoride is non-polar. Capisce?

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Answer 2

Cameron Andrews

BF3 is considered a non-polar molecule because its molecular geometry is trigonal planar, meaning the B-F bond dipoles cancel each other out due to symmetry, resulting in no net dipole moment. Although B-F bonds are polar due to the difference in electronegativity between boron and fluorine, the symmetrical arrangement of the bonds in BF3 leads to a non-polar overall molecule.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.