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mercury
2005-Mar-30, 06:42 AM
Here are a few questions about quantum mechanics (Bohr’s atomic model).
1. An electron is a particle revolving around the nucleus. So it should radiate energy (by classical mechanics). But if this energy comes from the orbital, it must finally become 0 and the electron must crash into the nucleus. Why does this not happen?
2. Why does the energy in the orbits remain constant?
3. During quantum jumping or an electron traveling between any 2 orbits, the electron must lose energy when it is between them in the atomic vacuum. Does this really happen?

astromark
2005-Mar-30, 09:20 AM
Orbital rules, gravaty even electromagnetic forces just dont apply to sub atomic particals and there behavior in and around the nuclie of the atom. Its not orbital machanics at all.
They have there own set of parimaters (rules)and we dont know all the rules yet.

alfchemist
2005-Mar-31, 02:39 PM
Hello, Mercury! The Bohr's model assumes quantization of energy in the atom such that in these "allowed" energy states, the electron does not radiate energy so that it will not spiral into the nucleus. "Jumping" from a higher energy state to a lower energy state means lowering of energy of electron so that this is accompanied by photon emission with frequency corresponding to the energy difference between the two energy states. "Jumping" from lower energy state to a higher energy state means increasing the energy of the electron such that this is accompanied by absorption of photon of energy, again equal to the difference between the two energy levels. But if I understood the model right, Bohr used a planetary model with orbits of fixed radii. This means that the position in space and the energy of electron corresponding to that position can be simultaneously known. This goes against the Heisenberg Uncertainty principle such that for a particular energy state, the exact position was replaced by probability density function which is your familiar "orbital", the s,p,d, and f orbitals