Charge Levels and Charge Motions

Charge Levels and Charge Motions

Charge motions and charge levels (energy) fit together
with the complementarity of harmonics.

Einstein predicted that light from a star which would pass near
the sun would be deflected by the mass of the sun.
This showed an interaction between electromagnetic radiation,
the light, and gravitation, the mass of the sun.
This can be generalized to say that the electromagnetic
interacts with the nucleomagnetic.
That is, gravitation is a nucleomagnetic force.
Gravitation involves the motion of the charge fractions
within the nucleus.

The charge fractions within the nucleus are the “up”quarks
and the “down” quarks.
These two charge fractions combine in ratios of two to one.
Two “up quarks combine with one “down” quark
to form the proton.
Two “down” quarks combine with one “up” quark
to form the neutron.
This two to one ratio exemplifies the complementarity
of charge motions and charge levels.

The plus (+) two thirds charge level of the “up” quark
harmonically combines with the minus (-) one third level
of the “down” quark.
When the two (2) plus (+) two thirds (2/3) charges
of the “up” quark combine
with the one (1) minus (-) one third (1/3) charge
of the “down” quark, it yields a proton,
with a so called whole unit charge.

The charge constitutes a closure, a loop,
an emission-absorption loop.
The wave-like properties of electromagnetic
and nucleomagnetic radiation occurs when the loop opens
and is described by Planck’s equation:
E (energy) equals (=) Planck’s constant (m)
times (x) frequency (u),

E = m u

In general, the higher the frequency, the higher the energy.
However, all frequencies or all increments of energy
do not form charges.
The charges which do form are related
to geometries of interaction at certain ranges.
This is the realm of quantum mechanics.

We characterize the species of atomic elements
according to atomic number.
Atomic number minus the number of protons
and electrons which constitute the atoms
of a particular atomic element.
The atomic numbers are organized
into periods and groups.
The periods constitute the rows in an inordinate system.
The group constitutes the columns.

The periods show the number of subshells in each period,
which constitutes a whole shell tabulation.
Each period, then, shows a progression
from one principal shell containing one subshell
and a single orbital to the second principal shell
containing two subshells, the second of which subshell
contains three orbitals.
The third principal shell contains three subshells,
the third of which subshell contains five orbitals.
The fourth principal shell, the fourth period
contains four subshells, the fourth of which subshells
contains seven orbitals.

An orbital contains two electrons.
This then indicates the progression in atomic number,
the filling of the orbitals characterized by the subshell.

Hydrogen is the first atomic element
in the first principal shell, with one subshell
and one orbital containing only one electron.
This makes hydrogen ambivalent.
That means the cadence or kind of degree of balance
or completion can either be gained
by donating its sole electron,
especially to an element needing only one electron
to complete its most external and accessible orbital
in its outermost subshell of hydrogen
can be an electron acceptor,
completing its single orbital capacity for two electrons
but disbalancing the proton / electron ratio.
This disbalance makes a hydrogen atom
which has accepted an electron quite reactive.

However, having a single electron in an orbital
with a capacity for two also makes hydrogen reactive.
Hydrogen attaches to other elements easily and extensively.
When it does so, it is said the element has been reduced.
That means that the charge the element held
towards accepting an electron,
its role as an electron acceptor, has been reduced.
When two hydrogens combine with one oxygen,
the oxygen functions as an electron acceptor.
The hydrogen has reduced the oxygen
in the formation of H2O, water.

Another reactive event has also occured:
the oxygen has oxidized the hydrogen
in the formation of H2O or water.
The function of accepting electrons is the reactive event
called oxidation.

When hydrogen combines with chloride to form hydrochloric acid,
the hydrogen is oxidized by the chloride
and the chloride is reduced by the hydrogen.
The energy level which characterizes the bond of combining,
forming a compound is called the oxidation-reduction potential.

In the case where salts form, with what is called an ionic bond,
the one element simply transfers its donated electron
to the electron accepting element and they form the association,
a crystalline association called the ionic bond.
The one element empties its asymmetrically filled orbital
and the other element accepts the donated electron
to symmetrically fill its most external or outermost orbital
despite the charge disbalance which is satisfied
by the crystalline association.

In the case of the metallic bond the atoms associate
to release electrons to the whole crystalline structure.
These released electrons then move through the corridors
of the crystal making the crystalline structure conductive.

The whole periodic table can be organized
in terms of conductors, insulators and semi-conductors.
When, where and as the atomic elements associate
and are able to involve all of their electrons
in orbitals with motion around the nucleus,
the atomic element is said to be an insulator.
Sulfur hexafluoride is an excellent insulator.
It binds or holds its associated electrons in very tight,
highly bound orbitals.
Silver or copper, however
associate to form very good conductors.

There are even bonds that create what is called superconduction.
This means that the electrons move through the corridors
of the crystalline lattice with little resistance.

When one atomic element combines with another atomic element,
both of which are metals and which associate
using the metallic bond, they are conductors.

There is another class of chemical bond called the covalent bond.
When two atoms combine using the covalent bond,
the charge moves from an orbital around one of the atoms
to an orbital around the other atom.
The covalent bond is characterized by the shared charge.

Another way of viewing the periodic table
is in terms of metals and non-metals.
Metals are the atomic elements which tend to lie
towards the left and the bottom of the periodic table.
Non-metals lie towards the right and the top
of the periodic table.
Metals are electron donors.
Non-metals are electron acceptors.
These roles, however, are relative.
In the case of sulfur hexafluoride, sulfur,
an electron acceptor, combines powerfully
with fluoride an electron acceptor
of even greater power or negative value.

The geometry of the periodic table
reflects the progression of the principal shells,
the subshells and their orbitals.

The first period, the first principal shell,
with only one subshell and only one orbital,
contains only two atomic elements,
atomic number one and atomic number two, respectively.

The second period, the second principal shell
with two subshells, the second of which has
both the one orbital subshell
and the three orbital subshell,
contains eight atomic elements.

copyright 2011, 2014, ECOhealth / Eve Revere