Which one of the following molecules has zero dipole moment.
Correct answer: C. BF3
- A. NH3
- B. NF3
- C. BF3
- D. H2O
Explanation
The dipole moment of BF3 is zero because the molecule is symmetrical. The three B-F bonds are arranged in a trigonal planar configuration, and the electronegativity of boron and fluorine are similar. This means that the partial charges on the boron and fluorine atoms are equal in magnitude and opposite in direction, so they cancel each other out.
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Chemical bonding explains molecular shape through VSEPR theory and distinguishes sigma bonds from pi bonds. Questions involve hybridization, bond angles, dipole moment and bond energy, including how electron-pair repulsion determines geometry and how bond polarity differs from the overall polarity of a molecule.
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