dlp-8 Molecule Anatomy. Electon Can Split Itself? Real Unified Theory of Everything

DLP-8 Molecule Anatomy

Orbital Stability

First ionization energy (FIE) is the amount of energy required to remove first electron from an atom.

The periodic table is primarily organized based on FIE.

Electron shells of noble gases are fully filled,
and thus are the most stable.
(except when it gets too big).


As previously mentioned, Electron can split itself, with proton as a pivot.
But usually Electron don’t like to split, in order to maintain its “sync equilibrium”.

* Neon 10
All slots in the outer most shell are filled,
Electrons do not need to split, & the system is stable.

* Flourine 9
An unfilled slot in outer shell,
requires 7 Electrons in the shell to “split” to attend to.
It has high tendency to absorb 1 Electron to cover the slot.

* Sodium 11
A lone valence Electron need multiple splits to fill multiple slots.
It has high tendency to jump out of the shell.

Ionic Bond

* Sodium flouride

So 1 Electron from sodium’s 3rd shell jumps to flourine’s 2nd shell,
completing both atoms’ 2nd-shells.
Then Na’s positive charge attracts F’s Electron,
to balance charge (trajectories),
forming an ionic bond.

Covalent Bond

* Ethene

Orbital hybridization is the adjustments of electron orbitals’ angles & sizes,
to the most energy conserving config,
under different conditions (usually to form bonds).

Covalent Sigma Bond is 2 Electrons of same spin fused to become 1, connecting both nucleus.

It is the strongest type of bond.

The Electron borrows Momentum from its paired Electron,
to conserve with the nucleus’s Protons,
as it needs more Momentum to interact with 2 nucleus instead of 1.
Also, the Electron lending Momentum,
contracts to reduce repulsion from, expanded neighbouring Electrons.

Covalent ‘pi’ bonds

A sigma bond can bring two parallel ‘p’ orbitals close enough to form connecting belts,
this is the pi bond.

Only Electrons with same spin can form sigma/pi bond.

Metallic Bond

Metallic Bond occurs in atoms with incomplete outer shell,
thus Electrons in outer shell are unstable.

When a group of such atoms cluster together,
the loosely gripped Electrons in outer shell may connect with other nucleus,
and get expelled from its own shell.

The atom losing the Electrons becomes an positive ion,
attracting nearby Electrons, and the process repeats.
Eventually developing into a sea of +ions attracting Electrons,
but unable to keep them in outer shell.

In such structure, Electrons free to move & orientate,
connecting multiple ions at all angles, at stretchable distances.

Giving such molecule higher potential to,
bend & stretch & spring
(flexible connection angles, stretchable distances),
transmit heat & electricity (electron vibrations),
and be ferromagnetic (electron rotation).

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