Basing the structure on the deconstruction of Neon, we find two things. One, an electron orbital is pressed far out of shape, giving Fluorine’s charge a -1, an electron that is easily exchangeable with other atoms. It also gives us a rigid structure that would fall apart under the electron orbital stresses if it had less neutrons, thus explaining, perhaps, why there are no other isotopes of Fluorine but this one….
In this picture we see the two atoms side by side, Neon and Fluorine, with their most abundant isotopes. A removal of the front top right proton causes the rear top right proton’s electron orbit to expand downward and allowing it to take up space left from the removal of the proton and its electron. This causes instability which makes the electron orbital easily effected by other atoms nearby who might be missing an electron. I will be working on Oxygen next. Interestingly, it has only three isotopes, and the one with the highest number of neutrons matches that of neon and fluorine, O 18, z 8 n10. Though it is rare, it is still very likely to be the first true deconstruction of fluorine.
The structure is still sound, but the internal neutrons are found to repel each other when placed in the current configuration. Instead, there is a tighter bond of neutrons when the two inner rings have their polarities reversed, the first four being put opposite and to the side of the second four, in a locked gear-like arrangement. This makes them closer together and also reverses the polarity of the end proton and electrons, making fluorine and neon non-polar, in other words, their two ends would push away from each other instead of being attracted to each other.