If you look at a radial probability chart for a given electron sublevel (excluding n=1), there is a probability of an electron in that sublevel being closer to the nucleus. The electron should lose energy if it is closer to the nucleus because it experiences a greater force of attraction to the nucleus, but how is this possible if all electrons in a given sublevel have the same energy?
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2$\begingroup$ Stop thinking of probability as probability. An electron is not here or there; it is everywhere at once. $\endgroup$– Ivan NeretinOct 10 '17 at 16:13
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$\begingroup$ No, it doesn't. If you believe in electron orbits imagine it to be elliptical like in B-S model. $\endgroup$– MithoronOct 10 '17 at 17:07
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You are trying to apply macroscopic understanding to the world of quantum mechanics. This thinking is doomed to fail. The energy of an electron occupying a specific orbital is that orbital’s energy. Full stop. Unless it changes its orbital it does not change energy.
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1$\begingroup$ The electron does not occupy the orbital, it IS the orbital! $\endgroup$– FeodoranOct 11 '17 at 7:24