why dipole moment of BF3 is zero
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Explanation:
- Boron trifluoride is has zero dipole moment although it has three polar B—F bonds.
- This is because BF3 has sp2 hybridisation and regular trigonal planal geometry.
- And the individual dipole moments of polar bonds get cancelled and overall dipole moment is zero.
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❤.NF3 is apolar molecule with polar bonds.
NF3 has unsymmetrical,three dimensional pyramidal structures,with a lone pair of electron.so the net dipole moment ofNF3 is always positive.
❤.BF3 is a non - polar molecule with polar bonds.
BF3 has symmetrical and trigonal plannar structure,with no lone pair of electrons.
So the net dipole moment of BF3is zero.
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