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.
Answer: It has polar bonds and a symmetrical structure.
Explanation:
Formula used for calculating hybridization
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
The number of electrons is 3 that means the hybridization will be 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.