Why Beryllium 8 is unstable, and a new but expected idea of why electron orbitals are so odd.

The stable Isotope of Beryllium is B 9. The extra neutron allows an s1 orbital to form around two protons that come together into a managable attractive electron orbital bond, but this occurs in Beryllium 8 even more successfully. Why is Beryllium 8, then, so unstable it doesn’t last even one second, in fact, it self destructs at 0.00000000000000067 of a second?
I think this very fact gives us a hint at what is going on.
Of course the first two proton pairs, can create a stable orbital bond. But it resonates. And it resonates at an extremely great amplitude because the atoms are truly at a very stable horizontal level. This shrinks their orbital, making it even stronger. However, As the other protons attract electrons, they two form a very tight attractive electron orbital bond. Because of this, it too resonates greatly. Normally, this wouldn’t be a problem. But because it too tries to shrink, and becomes more solid, and resonates even more, it disturbs the first inner electron ring. This causes it to disrupt it, and destroy that first ring. As these rings are constantly being destroyed and rebuilt, the energies build up, and cause so much stress in the beryllium protons in the proton-neutron 8 point ring, that it destroys their bonds to the neutrons. two are held in check, and two protons are released, as would be expected if the smaller ring outlasts the outer ring.
From this we can deduce that outer orbitals can compress inner rings. But more importantly, that the pressures can disturb the proton-neutron chains. We can deduce from this, that the connections inside of the nucleus have to be really strong to withstand the forces that electron orbitals can place on them. Thus their structure has to be very organized, it can’t just be random blobs of neutrons here and protons there. It has to be structured.
And finally, we come to a new truth, that has been staring at us in the face all along. That electrons can always form successful orbitals.
If the structure is sound, and there isn’t undue pressure on the inner ring, then the electrons have no choice but to sling shot away from the nucleus in a cone pattern, instead of around the nucleus in a ring pattern. This would explain why molecules bond in orb regions instead of rings, for the most part.
This also explains why atoms have such a loose electron in its vicinity that it can share or give away to another atom.

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