The question of the nature of matter has plagued scientists and philosophers since the beginning of history. Are there some first principles of Nature that describes the structure of the atom on the atomic level?

A significant event in the development of atomic theory took place when Sir Joseph J. Thomson showed beyond doubt that cathode rays in a discharge tube actually do consist of negatively charged particles. Thomson constructed a discharge tube, with a fairly high vacuum, which contained an auxiliary electrode that was connected to an electroscope. Thomson used a magnet to deflect the rays to strike the auxiliary electrode of the electroscope which registered the presence of negatively charged particles.

In 1902 English physicist Lord Kelvin proposed a model of the atom but was so strongly supported by Thomson that it became known as the Thomson atom. In this model the electrons were embedded in a positive sphere in various equilibrium positions, much like raisins in a pudding.

Another major event in the development of the structure of the atom occurred in 1910 when two researchers, under the supervision or direction of Ernest Rutherford, bombarded some very thin metal foils with alpha particles and found some of the particles were scattered from the foil at wide angles and even in a backward direction. Lord Rutherford stated, "It was almost as incredible as if you fired a 15-inch shell at a piece of tissue paper and it came back and hit you." With subsequent experiments came the realization that the nucleus was a small positive core no larger than 1/10,000 of the atomic diameter. Furthermore, the number of electrons outside of the core equaled the number of positive charges in the nucleus.

The results of the scattering experiments led Rutheford to establish the model of the atom as a small, positively, charged, massive nucleus surrounded by a cloud of electrons that provided electrical neutrality. At this point Thomson's idea of the atom had to be abandoned.

Rutherford's discovery of the nucleus created a major dilemma: how can the atom exist for any length of time with the electrons, being negatively charged, and strongly electrostatically attracted to the positively charged nucleus? The first thing one immediately thinks of is the solar system where gravity provides the centripetal force which keeps the Earth circling the sun. The assumption that the motion of the electrons, which follows a curved path and is in a state of revolving around the nucleus, balances the force of attraction between the opposite electrical charges leads to grave difficulty.

James Clerk Maxwell (1865), a student and assistant of Michael Faraday, firmly established mathematically and by prediction that any vibrating or oscillating electrical charge must emit or send out a train of electromagnetic waves that travel with an enormous velocity. Heinrich Hertz in 1888 produced a beam of electromagnetic waves by driving electrical charges rapidly back and forth through a wire.

A negative charged electron accelerating around its orbit, much as the Earth revolves around the Sun (planetary atomic model), should lose energy, become unstable, emit radiation continually at a frequency equal to that of its orbital motion, and within one hundred-millionth of a second fall into the nucleus. Rutherford stated: "I was perfectly aware when I put forward the theory of the nuclear atom that according to classical theory the electron ought to fall into the nucleus..."

Here is an apparently insuperable major dilemma': if atomic electrons are at rest, electrostatic attraction will draw them into the nucleus; if they are not at rest then in order to stay in the atom they must have acceleration and Maxwell's electrodynamics dictate immediate atomic collapse.

Something was wrong; two seemingly impossible options confronted physicists at that time. In retrospect, they simply did not have an experimental repertoire necessary to solve the dilemma; they did not know that magnets could float above a superconducting material.

The solution to the dilemma, without breaking any physical laws, necessitates only a minor arbitrary assumption: the nucleus acts as a superconductor. It is possible for a magnet to float above a superconductor and on the atomic level the electron acts as a magnet. The electron supplies its own magnetic field. On the atomic level the electron "floats" above the nucleus. The electron does not go around the nucleus but is suspended, free floating, at a precise, stable, stationary region above the superconducting nucleus.

Stable levitation is possible for superconducting bodies in a static magnetic field, which requires no energy input, and is exceedingly stable and quiet. Truly stable levitation without consumption of energy is possible only in magnetic fields. [1]

With this new atomic model it becomes possible to describe the phenomenon of atomic emission of discrete frequencies or definite line spectra in simplistic terms. Thermal, electromagnetic radiation, or mechanical kinetic (by collisions) energy when added to the atomic system causes the floating electron, in its quiet stable region at equilibrium position, to become displaced "vertically" and to vibrate harmonically around this equilibrium point which then radiates much like a radio antenna; a precise high frequency sinusoidal electromagnetic wave train in the form of light is emitted.

Additionally, if an inner electron is knocked out of its position or is moved to a higher energy stable state by a photon then an outer electron can fall "vertically" into that vacant position- The electron may either jump directly to the innermost position or may reach the innermost energy state by successive jumps with stopovers in intermediate positions. A vertical drop of a cascading electron emits the characteristic line spectra.

Evidence supporting the concept of this floating electron atomic model would be the chemist's description of the filled p subshell containing six electrons (three pairs) geometrically oriented so that the three p orbitals involves bi-spherical or dumbbell-shaped charge distribution about an axis that passes through the nucleus. The axes of the p orbitals are so arranged that they are at right angles to each other. The sum of the electronic distributions of these three p orbitals when filled adds up to a spherically symmetrical distribution about the nucleus. In filled orbitals the floating electrons each strongly repel all the other floating electrons therefore they orient themselves in order to maximize the distance between each other.

With the very intense electric and magnetic fields inside the atom the configuration of electrons is precise and this is exemplified when an atom interacts or bonds with other atoms. For example, the bond angle of the hydrogen-carbon-hydrogen of the four p orbitals of the carbon atom in a molecule of methane, prescribing a regular tetrahedron, measures 109.5 degrees. The four valence electrons repel each other with equal strength and the four covalent bonds are directed toward the four vertices with the carbon atom at its center.

The floating electron model allows for precise bond distances because the electrons reside at precise equilibrium points. In the diamond atomic crystal each carbon atom is connected by means of a single covalent bond to each of the four other atoms located at the corners of a regular tetrahedron. The distance between the carbon atoms is 1.54 angstrom units. Crystalline and chemical structures are very precise; atoms always bond in certain configurations and ratios.

This new model of the atom describes the covalent bond as being magnetic. The two valence electrons are attracted to each other like bar magnets; the north poles of the electrons are attracted to the south poles of each other.

In 1925, Samuel Goudsmit and George Uhlenbeck proposed that the electron inside the atom can be aligned with or against the lines of force of an applied magnetic field which gives two states of different energy. [2] The floating electron model would literally allow the electron to spin on its axis much in the same way that the earth spins on its axis. The concept of spin-up and spin-down would be allowed by this new model. This spin-on-its-axis of the electron produces effects which gives rise to a small magnetic moment.

In helium the filled s orbital would have an electron on the opposite sides of the nucleus. The north pole and south pole of the one electron would couple with the south pole and north pole of the other electron respectively. The atom would be electronically and magnetically balanced. This configuration of electrons would permit only the two s electrons and would describe the reason for the existence of the s orbitals. In the floating electron model two electrons can also couple north pole to south pole and south pole to north pole and thus be spinning in the opposite directions. The Pauli exclusion principle, however, does not apply to the p shell electrons because a filled shell has six electrons all at the exact same distance from the nucleus.

The new floating electron model allows for all the physical laws that apply to the macroscopic level of our physical world to apply to the microscopic level.

And that's all I have to say about that