Which of the following structures represents | vedclass

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(C) Boron trifluoride $(BF_3)$ is an electron-deficient molecule where the boron atom has only $6$ electrons in its valence shell. To achieve stabilit

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(C) Boron trifluoride $(BF_3)$ is an electron-deficient molecule where the boron atom has only $6$ electrons in its valence shell. To achieve stability,the lone pair of electrons from the fluorine atom is donated to the empty $p$-orbital of the boron atom,forming a $p\pi-p\pi$ back-bonding. This results in resonance structures where a double bond character exists between the boron and one of the fluorine atoms. The correct resonance structures involve the formal charges on the atoms,where the boron atom carries a positive charge $(B^+)$ and the fluorine atom involved in the double bond carries a negative charge $(F^-)$. Option $C$ correctly depicts these resonance structures with the appropriate formal charges and double bond character.

Which of the following structures represents the correct resonance structures of boron trifluoride $(BF_3)$?

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