[2][3][4] Despite being isoelectronic to the triple-bonded species CO and N2, computational studies generally agree that the true bond order is much lower than 3.

[5] BF is unusual in that the dipole moment is inverted with fluorine having a positive charge even though it is the more electronegative element.

Backbonding, or the transfer of π orbital electrons for the fluorine atom, is not required to explain the polarization.

[10] A naïve analysis would suggest that BF is isoelectronic with carbon monoxide (CO) and so could form similar compounds to metal carbonyls.

As discussed above (see § Structure), BF has a much lower bond order, so that the valence shell around boron is unfilled.

[15] To make the compound, Vidovic and Aldridge reacted NaRu(CO)2(C5H5) with (Et2O)·BF3; the boron monofluoride ligand then formed in-place.

[2] Hafnium, thorium, titanium, and zirconium can form a difluoride with a BF ligand at the low temperature of 6K.

[2] The first fully characterized molecule featuring BF as a terminal ligand was synthesized by Drance and Figueroa in 2019, by sterically hindering the formation of a dimer.