Acids in the Geocubic Model
by Tom Gilmore
All graphics by Tom Gilmore
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An acid is generally an aqueous solution with the ability to react with certain metals, bases, or alkalis (and may form salts). Most acidic compounds contain Hydrogen. It is conventionally thought that a Hydrogen atom from the acidic compound is transferred to the water molecule and forms “Hydronium” (H3O), but the Geocubic Model shows that this is a fallacy. The Hydronium hypothesis is also contradicted by the fact that Carbon dioxide (CO2) will dissolve in water to create a carbonic acidic aqueous solution, and there is no Hydrogen atom in carbon dioxide, so there would be no 3rd Hydrogen atom supposedly making Hydronium.
Void Nuclide Attraction
In the Geocubic Model a Hydrogen atom will always be bonded, and either have 2 Spheres or no Spheres (Void). When a Hydrogen atom is Void (empty) it projects a weak intermolecular attraction that certain active Elements respond to. This is utilized in the genetic coding of DNA, where the nucleobases holding the DNA strands together are linked by the weak intermolecular attraction, allowing the strands of DNA to easily separate in the process of cell reproduction.
In the Geocubic Model the acidic solution results from the linkages (caused by the Void Hydrogen in water) attracting the active Elements of an acidic molecule.
The Nuclide of an atom is not the Baryons (Protons and Neutrons) themselves, but a weak energy bundle taken from the Baryons. In atomic bonding, Protons are loaned and borrowed, and the Nucleonic deficit pulls on the loaned Protons. Only a Hydrogen atom can be Void in a bond. When the Hydrogen atom is Void the pull of the Nuclide has no Nucleon to center it, and the pull results in an intermolecular attraction.
The intermolecular attraction is represented in the water molecule diagram below by green arrows (each Void Hydrogen can form only one link).
In the simplified bonding diagrams in this article the Atomic Number of the Element (the number of Protons in the Nuclide) is in black, arrows show transfers of Protons, and the bonded Proton counts are in red.
Acidity is conventionally measured by the acidic activity level. A logarithmic scale is used called the pH (percentage Hydronium). A pH of 7 is neutral, and lower is acidic (if higher, called a base).
Hydrochloric Acid (HCl) is:
Hydrogen(1)Empty-form(0) + Chlorine(17)Argon-form(18),
There is a dual linkage in the acidic solution of HCl. The Void Hydrogen atom in the Hydrochloric acidic molecule attracts the Oxygen atom in a water molecule, and a Void Hydrogen atom of the water molecule attracts the Chlorine atom of the Hydrochloric molecule. In the diagram below of the acidic solution, the intermolecular attraction linkages are shown with green arrows.
Nitrogen(7), Oxygen(8), and the Halogen Elements (such as Fluorine(9) and Chlorine(17)), are subject to intermolecular attraction.
Although Phosphorus(15) and Sulfur(16) are active Elements (in that they have no independent valid Sphere arrangement), they are immune to the attraction. This is evident from their hydro-molecules as demonstrated following.
With Sulfur(16), two Void Hydrogen atoms are
attached in Hydrogen Sulfide (H2S), but it is not acidic. However when 4 Oxygen(8)
atoms are incorporated in the Sulfide, the Sulfur’s bonded form drops back an
octave (to S(16,10), making Sulfuric Acid (H2SO4).
In shorthand, [2H(1,0)+S(16,18)], drops back to [2H(1,0)+S(16,10)+4O(8,10)].
The Oxygen atoms in the Sulfuric acidic molecule link to the Void Hydrogen atoms in water, and the Oxygen atoms in water link to Void Hydrogen atoms in the Sulfuric acidic molecule. The multiple linkage locations allow Sulfuric acid and water molecules to link in chains.
In stepping back another atomic number, to Phosphorus(15), the chemical Phosphine (H3P) is not acidic, but becomes phosphoric acid (H3PO4) by adding 4 Oxygen(8) to drop Phosphorus back an octave in form.
[3H(1,0)+P(15,18)] drops to [3H(1.0)+P(15,10)+4O(8,10)].
One of the super-strong acids is Fluorosulfuric acid (HSO3F)