Link to PDF Article
Above is a link to the article entitled Modeling hydrogen spectral lines published in June 2009 in Physics Essays a publishing of AIP. This article presents an alternative theory to the Bohr model and the quantum mechanics model of the hydrogen atom theorizing that the secondary electron of the hydride ion arranged in a dipole configuration is the entity reponsible for hydrogen's spectral lines and not the bound electron of the hydrogen atom as most eloquently questioned by Schrodinger.
Once we have become aware of this state of affairs, the epistemological question: "Do the electrons really exist in these orbits within the atom?" is to be answered with a decisive No, unless we prefer to say that the putting of the question itself has absolutely no meaning. __Erin Schrodinger.
In the case of the hydrogen atom, the electron is either bound or unbound with no intermediate excited energy states. To solve Schrodinger's equation a complex wave function is necessary because Schrodinger attempted to describe hydrogen's spectral lines in a field in which they do not exist, that is the point charge field. The nonradiating energy states observed are produced from the secondary electron in a dipole field of the hydride ion and unlike the current theories predicts that the angular momentun of the excited electron is constant and equal to h-bar, classically explains electron spin, and asserts that the intrinsic angular momentum or electron spin for an electron at rest (n = infinity) is also h-bar. Thus, there is no need to arbitrarily introduce a 4th quantum number.
Click to Link to Physics Essays's Web Site
Friday, November 13, 2009
Saturday, November 7, 2009
An Explanation for the Stability of the Hydrogen Atom
Early models of the hydrogen atom such as the Bohr model and quantum mechanics model failed to explain the stability of the ground state electron bound to the nucleus of the hydrogen atom. In the article entitled Modeling hydrogen’s spectral lines , the exited states for this atom can be explained by the hydride ion model. Now the question is: “Why doesn’t the electron in the ground state fall into the nucleus of the atom?” as predicted by classical physics. The hydrogen atom with its bound electron is stable to radiation, an obvious experimental fact, and it is assumed there must be classical mechanism that explains this stability.
First, it is fundamental to our understanding of the atom that the laws and principles of classical physics apply, and hence, the derivation of the potential and kinetic energy equations of Niels Bohr are valid equations. However, one may with justification question his postulates. It is interesting to note that Bohr was able to predict both the ground state radius of .529 angstrom and the angular momentum of the electron of h-bar and both of these values are verified by the hydride ion model. Considering Bohr's findings and the predictions of the hydride ion model for momentum of a free electron of h-bar, it is clear that a negatively charged unbound electron spiraling toward a positively charged proton will radiate energy until it reaches a state in which the angular momentum is again h-bar, thus obeying the law of conservation of angular momentum. No other values of the angular momentum are physically possible.
Second, a spiraling electron is assumed to stop radiating energy once it reaches the Bohr radius. This phenomenon can happen only if the positively charged proton of the nucleus of the atom senses a charged ring produced by the spiraling electron with sufficient velocity to uniformly distribute the charge of the electron around the ring. Under these the conditions, the mathematics of the charged ring prevail and the electric potential of the electron is E(r=0) = E(r=infinity) = 0, where r is the distance from the ring to the proton. Thus, mathematically there exits a minimum potential somewhere in between these extremes and it can be shown that this minimum potential occurs at the Bohr radius. A free electron will immediately “snap” to this location external to the proton without the ability to move closer and must stop radiating energy given the fact when an electron radiates energy away it must move closer to the nucleus, a necessary requirement for conservation of angular momentum.
First, it is fundamental to our understanding of the atom that the laws and principles of classical physics apply, and hence, the derivation of the potential and kinetic energy equations of Niels Bohr are valid equations. However, one may with justification question his postulates. It is interesting to note that Bohr was able to predict both the ground state radius of .529 angstrom and the angular momentum of the electron of h-bar and both of these values are verified by the hydride ion model. Considering Bohr's findings and the predictions of the hydride ion model for momentum of a free electron of h-bar, it is clear that a negatively charged unbound electron spiraling toward a positively charged proton will radiate energy until it reaches a state in which the angular momentum is again h-bar, thus obeying the law of conservation of angular momentum. No other values of the angular momentum are physically possible.
Second, a spiraling electron is assumed to stop radiating energy once it reaches the Bohr radius. This phenomenon can happen only if the positively charged proton of the nucleus of the atom senses a charged ring produced by the spiraling electron with sufficient velocity to uniformly distribute the charge of the electron around the ring. Under these the conditions, the mathematics of the charged ring prevail and the electric potential of the electron is E(r=0) = E(r=infinity) = 0, where r is the distance from the ring to the proton. Thus, mathematically there exits a minimum potential somewhere in between these extremes and it can be shown that this minimum potential occurs at the Bohr radius. A free electron will immediately “snap” to this location external to the proton without the ability to move closer and must stop radiating energy given the fact when an electron radiates energy away it must move closer to the nucleus, a necessary requirement for conservation of angular momentum.
Thursday, October 22, 2009
Electronic Configuration Pattern Found in Pascal's Triangle-JCE 1996 (73) 742 [Aug]
Link to Electronic Configuration Pattern
This site reveals the discovery of the Electronic Configuration Pattern within Pascal's Triangle. This is a mouse-over applet that displays the electronic configuration when the mouse is placed over elements of Pascal's Triangle. This discovery may lead to a better understanding of quantum theory.
This site reveals the discovery of the Electronic Configuration Pattern within Pascal's Triangle. This is a mouse-over applet that displays the electronic configuration when the mouse is placed over elements of Pascal's Triangle. This discovery may lead to a better understanding of quantum theory.
Periodic Table of the Elements
Link to the Periodic Table of Elements
The Periodic Table of the Elements (published in JCE) describes a unique representation of the Periodic Table placing the semimetals in a vertical column, thus separating the metals from the nonmetals. Notice the impressive symmetry of the elements.
The Periodic Table of the Elements (published in JCE) describes a unique representation of the Periodic Table placing the semimetals in a vertical column, thus separating the metals from the nonmetals. Notice the impressive symmetry of the elements.
The Geometry of the Nuclear Atom
Link to the Geometry of the Nuclear Atom
The is a link to an interactive online paper that contains vrml files. A plug-in such as Cortona 3D or Cosmos Player is needed which can be downloaded from the internet. This is essential for fully grasping the construction of atoms and bond sites. Also, note that at this time Mozilla Firefox is the preferred browser. The paper describes a very unique way of modeling the outer shell of the periodic atoms. Explored are the hydrogen atom and the carbon atom depicting single, double, and triple bonds. Bond length determinations for selected organic compounds are given to demonstrate the predictive power of this theory.
The is a link to an interactive online paper that contains vrml files. A plug-in such as Cortona 3D or Cosmos Player is needed which can be downloaded from the internet. This is essential for fully grasping the construction of atoms and bond sites. Also, note that at this time Mozilla Firefox is the preferred browser. The paper describes a very unique way of modeling the outer shell of the periodic atoms. Explored are the hydrogen atom and the carbon atom depicting single, double, and triple bonds. Bond length determinations for selected organic compounds are given to demonstrate the predictive power of this theory.
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