excited state EC of boron is 1s2 2s1 2px1 2py1. so it undergoes sp2 type of hybrydisation and has trigonal planar shape.
BF3 is Non-Polar :)
BF3 is the compound Boron Triflouride
.. .. : F - B - F : .. .. :F:
BF3 has polar covalent bonds. It is planar and symmetric so the net dipole moment of the molecule is zero.
NH3 is a 3D object (like an open umbrella) but BF3 is all on one plane in a triangle.In the second case the dipoles cancel each other
No. The individual bonds are polar, but BF3 is trigonal planar so the overall molecule is not polar.
SO2 is bent shaped and has a net dipole moment.
BF3 is a planar molecule with bond angle 120 0 . The bonds are polar but the bond dipoles cancel one another out - think of it as symmetry or vector addition or that they pull equally in opposite directions.
The shape of this molecule is Trigonal Planar. this is because it has no lone pairs of electrons so it maintains a 2D shape.
Boron trifluoride BF3 reacts with F- ion to form the BF4- ion. BF3 has only 6 electrons around the B atom, is planar, and is a Lewis acid (as it will accept electrons from an electron pair donor such as F-. BF4- is a tetrahedral ion- all four bonds are equivalent.
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The geometry of XeCl2 is linear with a symmetric charge distribution.Therefore this molecule is nonpolar.