Which statement is true about BF3, a nonpolar molecule? It has nonpolar bonds and a symmetrical structure. It has nonpolar bonds and an asymmetrical structure. It has polar bonds and a symmetrical structure. It has polar bonds and an asymmetrical structure. It has ionic bonds and symmetrical structure.

I think the correct answer is the first option. It has nonpolar bonds and a symmetrical structure. The structure of a BF3 molecule shows a symmetrical trigonal geometry. The net dipole moment of the molecule is zero therefore it is polar.

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kobenhavn kobenhavn · Answer 2 · 2019-03-16T06:15:17+01:00

Answer: It has polar bonds and a symmetrical structure.

Explanation:

Formula used for calculating hybridization

[tex]:{\text{Number of electrons}} =\frac{1}{2}[V+N-C+A][/tex]

where, V = number of valence electrons present in central atom i.e. boron= 3

N = number of monovalent atoms bonded to central atom=3

C = charge of cation = 0

A = charge of anion = 0

[tex]BF_3[/tex]

[tex]{\text{Number of electrons}} =\frac{1}{2}[3+3-0+0]=3[/tex]

The number of electrons is 3 that means the hybridization will be [tex]sp^2[/tex] and the electronic geometry of the molecule will be trigonal planar.

Thus as there are no lone pair of electrons, there is no distortion and the molecule is symmetrical. The B-F bonds are polar due to electronegativity difference but the polarities cancel due to symmetrical structure.