« on: 11/06/2017 23:05:29 »
The first thing to get out of the way is that the exponential functions governing the wave functions of electrons are just heuristics.What so you mean by that precisely.
There is a probability of 1:4.17 x 10^42 that the electron will appear at at least some distance beyond the Van Der Waals radius of the atom to which it belongs. So this is a tiny probability that the electron volume probability density of an atom extends somewhere beyond the Van Der Waals radius, i.e. an electron can pop-up somewhere beyond the radius of the atom for a very brief amount of time before it interacts with a photon and changes position again.That is incorrect. You misinterpreted the probability incorrectly. The probability associated with the wavefunction refers to the probability of finding an electron in a specified volume of space when the position of the particle is measured. It doesn't refer to the electron popping up somewhere nor does it mean that a photon will collide with it changing its position.
I strongly recommend learning more about the wave function and its correct interpretation. See:
I also recommend that you learn the philosophy of physics and why the notion of proof is not part of science. Here's a place to start. The following video is of Alan Guth, an MIT cosmologist/particle physicist. Highly respected and well-known in his fields.
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