Fluorine is more electronegative than either | vedclass

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(D) The $BF_3$ molecule has a dipole moment of $0$ because it has a planar triangular geometry,where the bond dipoles cancel each other out due to sym

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The $BF_3$ molecule must be planar triangular

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(D) The $BF_3$ molecule has a dipole moment of $0$ because it has a planar triangular geometry,where the bond dipoles cancel each other out due to symmetry.In contrast,$PF_3$ has a pyramidal geometry due to the presence of a lone pair on the phosphorus atom,which results in a net dipole moment.Therefore,the fact that $BF_3$ has no dipole moment implies that it must be planar triangular.

Fluorine is more electronegative than either boron or phosphorus. What conclusion can be drawn from the fact that $BF_3$ has no dipole moment but $PF_3$ does?

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