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Per NCERT §4.3.6 + Table 4.5, why is the dipole moment of BF₃ ZERO although each B-F bond is polar?
ATrigonal-planar geometry — the three equal B-F bond dipoles at 120° give a vector sum of zero
BF is less electronegative than B
CB-F bonds are non-polar
DBF₃ is ionic
Answer & Solution
Correct answer: A. Trigonal-planar geometry — the three equal B-F bond dipoles at 120° give a vector sum of zero
Per NCERT §4.3.6, BF₃ trigonal planar. Three equal bond dipoles at 120° → resultant 0. Similarly CO₂ (linear) μ = 0.
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