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Question

Boron trifluoride (BF3) has no dipole moment (μ=0D). Explain how this observation confirms the geometry of BF3 predicted by VSEPR theory.

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Solution

The BF3 molecule has a symmetrical trigonal planar geometry, like the SO3 molecule.

In such a structure, the resultant moment of any two BF dipoles is equal in magnitude but opposite in direction to the moment of the third one.

So, the net dipole moment of the BF3 molecule is zero, and it is non-polar.


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