Tag Archives: atoms

Fluorine Atomic Structure

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.

(Update) 4-20-2016

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.


Neon Atomic Structure

When trying to find the Nitrogen atomic structure, based on my theory, I realized that it too was probably a reduction of the next fused atom in the star fusion chain. This put Neon or Magnesium as my next target to decipher. Finding that Neon was discovered to be more common in stars than previously thought, I realized that it was most likely to be the next in the fusion chain of element making found in stars. The fusion chain is H plus H makes He, or Helium. He plus He makes C, or Carbon. C plus C makes Ne, or Neon. Thus it was finally a matter of arranging all the neutrons to form the core of the atom, since protons repel each other, and neutrons help bind them together. But the design had to allow for the electron orbitals to have complete stability in their orbits because those orbitals are full and are not easily displaced, this makes the Nobel gasses inert and nonreactive. Finally, I had to incorporate the polar bonding system of the last structures according to my unified field theory, where neutrons and protons both have north and south poles. Finally, the best, most compact shape I could find, was not only viable, but I noticed that it looks very much like a carbon atom extended by addition of another carbon atom.

The red orbs are the bigger protons, the brown orbs are the smaller neutrons.


As you can see, my theory also supports why isotopes are not always viable structures, therefore a few elements have only one isotope. The electron orbitals put quite a strain on the inner structure’s ability to hold itself together, thus when forming, the atoms quickly deteriorate. I suspect that as the atoms increase in size, the structures will become more complicated, but the protons will almost always be on the outside part of the atom.

Element Nucleus Structures, Hydrogen thru Carbon…

Video of the pictures below, saying basically the same thing.

Hydrogen 1,


Helium 4,

After understanding that electron orbitals can compress other electron orbitals, I began to understand the shapes of the other atoms.  Helium 4’s shape, therefore, has its highest stability when the two electrons do not share one orbit, but instead, have their own orbits, parallel to each other, as shown below.  In nature, stability of form is very important.


The two orbitals form disks at either end of the nucleus, according to my understanding of my theory.  Please check in on this page from time to time, as I plan to add more elements to the page.  Thank you.

In star formation, Hydrogen fuses together to form Helium.  Then Helium fuses together to form Carbon.  It took me a while to understand that the Atoms above Hydrogen were not all helium derived, but instead, Carbon derivatives.  In other words, they were decay products of Carbon.  Thus they retained some of the Carbon structure, and were able to form very stable nuclei.

Lithium 7

This is our first example of electron orbitals compressing another electron orbital. Not only does it compress the orbital, but it makes the orbital so unstable, that the proton is sensed as still containing a positive charge, or unmarried state.


Beryllium 9,


Boron 11,


Carbon 12,


Model of Carbon 12 Isotope Nucleus Structure -Video Included

My theory, as stated a few posts ago, shows the inner structure of the carbon 12 Isotope nucleus and explains why the orbitals are shaped the way they are.

Here is a simple video I made showing the model….

Theory on Temperature and Loose Electron Orbitals

When electrons are too far away, or incapable of bonding to their proton partner, they still remain attracted to the proton, and inversely to its poles. This loose bonding means that the proton’s attraction is not one on one with the electron, instead it acts as a positive field area for the electron to be attracted to. The electron, respectively becomes held in this area, loosely, and because of nearby neutrons and other electron orbitals, its shape of influence alters. The closer the electron is to the proton, the more inverse its poles will be. Thus the electron will veer to electron orbitals in the area that are inverse to it, but will be repulsed by electrons in the area that are not inverse to it.

I will post pictures explaining this later.

I have also been working on the theory that electron orbitals determine energy absorption and dissipation, and that it is the way in which the orbitals react with the quanta fields that determine if an atom is a gas or solid or metal.

If I can discover the inner structure of Boron and Carbon, I think I can build upon that to discover why some atoms behave as gasses at room temperature and why some behave as a solid. Remember, as you well know, that the reason things are metals, solids, and gasses, at room temperature is because they are that way at room temperature. Temperature is simply a matter of energy levels of a given state. And since energy is the exchange of quanta in atomic quanta fields and mainly through electrons, the temperature will determine how they react to each other.

The more quanta in the area the more chances for reactions of attraction and repelling. This is heating, or increasing the temperature. Thus not only does this cause stress upon the quanta fields, this stresses electron orbitals and changes how well they attract or repel each other. The more energy in the system, the more quanta. This increases quanta field strength and size. While it may add chaos in some areas, the field strengths increase stability, but the stronger the fields in magnets, the smaller the size of the initial area of attraction. The orbitals may actually all shrink, thus repelling each other until the atoms, as energy is added, become a gas, then finally a form of plasma, the result is that the atoms act like inert objects that become more like electron charges than actual particles.

When you take away quanta, or energy, from the quanta fields electrons and their orbitals, which is what decreasing the temperature does, you cause the quanta fields to lose strength, they expand a bit in certain directions, and their attraction is weaker, but at the same time, more felt, for the attraction area is increased because the fields are less compressed.

So now we have very strong attraction fields because the window of attraction is open wider, and it is easy for the electron orbitals to form more solid bonds with other atoms, and they tend to crystallize, as their bonds are very strong.

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.