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$\ce{BCF}$ (boron carbofluoride, or carbon borofluoride, not to be confused with another so-called BCF molecule that has nothing to do with it) should exist as a vapor molecule with the bonds $\ce{B≡C-F}$, it's simple; but it doesn't seem to exist, or I can't find any information (I just found a heavy thesis where $\ce{H2··FCB}$ —a theoretical molecule with Van Der Waals forces— is computationally studied, but it turns to be quite unstable even with the help of $\ce{H2}$). Instead, other molecules like $\ce{C2O}$, $\ce{FBO}$, $\ce{NCF}$, vapor $\ce{BN}$, etc, do exist.

Why not $\ce{BCF}$ or $\ce{BCCl}$?

Victor Graus
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    Even C=B-F would be much more viable. – Mithoron May 22 '20 at 14:44
  • @Mithoron You are right about C=B-F, now I've read a few papers which state that computationally it is 100 - 200 kJ/mol more favorable than BCF. Anyway even C=B-F seems to be quite unstable. So in your opinion, as a thought experiment, if we could engineer to obtain BCF, we would just get C=B-F? It's a sound idea. – Victor Graus May 23 '20 at 19:16
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    FCB molecule wouldn't survive perhaps even single collision with another FCB, and probably even H2 - instant addition on first occasion. Your FCB would be absurdly strong Lewis acid. – Mithoron May 23 '20 at 19:34

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