Chemistry Lewis Structure (Boron and Fluorine)

Question

What is the correct Lewis Structure for BF₂^- ?

I thought Boron was an exception to the Octet rule and that Fluorine could not be double bonded but I am not sure if that is correct.

Is it boron with two electrons single bonded to each fluorine and each fluorine having six additional electrons or is boron with two electrons double bonded to one Fluorine with four additional electrons and boron single bonded to the other Fluorine with six additional electrons.

Answer 1

I made a video above to help answer this question. Hope this helps. Feel free to reach out if. I can be of further assistance! :)

-Courtney

Answer 2

Boron is an exception to the octet rule, often forming stable compounds with fewer than 8 electrons. In BF2−_2^-2−​, Boron has 8 electrons around it due to the negative charge.

Fluorine typically does not form double bonds as it is highly electronegative and prefers to complete its octet with lone pairs.

Thus, the correct Lewis structure for BF2− has Boron single-bonded to each Fluorine, with each Fluorine having three lone pairs of electrons, and Boron having a pair of electrons for the negative charge.