The Quantum Mechanical model of an atom
Sometimes, an unfamiliar researcher walks by who sees a theme in nature that others may miss altogether. Isaac Newton, for example, understood that the force behind a finished cannon ball is equal to that of the moon orbiting the earth. Ernest Rutherford was one such person. When he realized that iotas have a heavy core, he thought that the way the moon orbits the earth is the same as the electron orbiting the molecule. Newton was right. Rutherford now knows it was wrong. The particle did not look like something like this. But then we actually use Rutherford's model to illustrate what the particles look like. It is the most famous image we have of the iota. A real particle can look amazingly different from anything like this. Moreover, it would not be an empty space as you have been told. How exactly is a molecule the same? And, how can we find that? Why would an electron not fall into a ditch with the possibility of a gravitational pull? For what reason can you not press the particle? The correct answer expects us to look forward to the importance of quantum technology.
explain the quantum mechanical model of an atom
For what reason do we rely on quantum mechanics in any case? Moreover, have we emerged from this disclosure - perhaps the most straightforward and scientifically proven hypothesis. The correct answer comes at the moment ... In 1911, Ernest Rutherford proposed a model of the iota planet. According to the model, the nearby planetary group and the molecule were almost indivisible. In fact, like the moon's orbit around the earth because of its gravitational pull, the illuminated electron was captured by a circular orbit. The most attractive force was electromagnetism instead of gravity due to iota. This seemed good because Isaac Newton's law of general attraction was not clear in the colombomb law of electric power. This was fun. A beautiful night of nature. Well, well, it was ridiculous. Another big issue is that when the electrons move faster, as they will when they continue to adjust the course of the circular motion, they make electric waves in Maxwell's case. This means that the photons will be constantly transported from the electron, causing them to lose energy.
how does the quantum mechanical model of an atom describe electrons
A rainbow of tones could be seen, becoming greener and more upright as the electron moved closer to the core, until it landed on it. So applying the old particle rules did not work in case you took the Rutherford model. Great new progress was needed. In any case, Rutherford did not know that 11 years earlier, in 1900, Max Planck had successfully made this progress, showing that photon power was limited. Planck's hypothesis has shown that the matter only emits different radiation pathways, with the force E corresponding to the multiplication f - the solid equation h, since Planck's inconsistency. A young researcher by the name of Neils Bohr went on to join Rutherford's model and Planck's speculation that electrons might be present in certain supernatural circles without the transmission of energy. How could he think this? Bohr's observation is that Planck's stability has units of rakish energy. He therefore speculated that solitude such circles would be allowed when the precise power of the given electron value depends on Planck's level. In addition, he assumed that the smallest circle would be h / 2pi when 2pi appeared in the circles of circular circles. Also, any circle can exist as long as it was a different number of this number. So the next circle will be 2 x h / 2pi. At that point 3X of the following, etc.
What do atoms look-like Why
Also, Bohr thought that electrons might transfer or store energy when these electrons jump from one circle to the next. Either way, Bohr could not explain why electrons would not produce photons on a regular basis, or why these unusual circles should exist anywhere. However, if you think you are right, you can find the size of the electron circle using the coulomb law. Obviously, the smallest circle sweep can be .529 X 10 ^ -10 m, about the largest part of the angstrom. So now we know the magnitude of the molecule, which was previously a mystery. Recognizing this, the energy released by the electron as it changes circles can be determined. Views and views, power outages, confirmed this measurement. So Bohr's model was right. Since this model expects unreliable attributes, it was believed that this is it! This should be exactly what the molecules have in common.
conclusion
The problem was no one knew why Bohr was right. So this was not the final answer. Then came a wonderful French researcher named Louis de Broglie. He said: look, if the molecule is strong and has a related frequency due to Planck's stability, then the electron may wave. This requires a great deal of philosophical exaggeration, for the reason that here is someone raising such a strong issue - the things we can see and feel fully made in waves. Matter was somehow a molecule and a wave at the same time. De Broglie suggested that electrons can only exist in circles where their waves interfere. In addition, this may occur if the circuit circuit is equal to the frequency, or twice the frequency or the frequency multiplied by the frequency, or other numbers that set the frequency. This turned out well and really, and it clarified why the circles would be on the right radii, something Bohr couldn't do. Bohr's model seemed to be more realistic. In any case, there were still many questions right now. What is the meaning of these waves? How and w
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