Assume that the structure of BF₃ (boron trifluoride, or trifluoroborane) is correctly predicted by the VSEPR rules.
1. What is the predicted structure? (Show all unpaired valence electrons.)
2. The B-F bond is exceptionally strong. This suggests that it has some double-bond character. Draw resonance structures for BF₃ that show that the three B-F bonds share some double-bond character. Be sure to show formal charges and all unshared electrons.
3. What is the polarity of the B-F bond? (In which direction is the bond dipole?) How do you know?

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The Answer of Assume that the structure of BF₃ (boron trifluoride, or trifluoroborane) is correctly predicted by the VSEPR rules. 1. What is the predicted structure? (Show all unpaired valence electrons.) 2. The B-F bond is exceptionally strong. This suggests that it has some double-bond character. Draw resonance structures for BF₃ that show that the three B-F bonds share some double-bond character. Be sure to show formal charges and all unshared electrons. 3. What is the polarity of the B-F bond? (In which direction is the bond dipole?) How do you know?

Assume That the Structure of BF3 (Boron Trifluoride, or Trifluoroborane)

Assume That the Structure of BF₃ (Boron Trifluoride, or Trifluoroborane)