The shape of the boron trifluoride molecule, BF3, is
- A. pyramidal
- B. bent
- C. tetrahedral
- D. trigonal planar with bond angles of 120 degrees
Explanation
Boron forms three bonds and has no lone pair, so the three electron regions lie flat at 120 degrees, and the molecule is an exception to the octet rule with only six electrons round the central atom. That electron deficiency is why boron trifluoride readily accepts a lone pair and acts as a Lewis acid. Ammonia looks similar on paper but is pyramidal because of its lone pair.
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