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I understand that the orbital is a probability field of the highest likelihood of the atoms position, however, is the probability uniform throughout the orbital or is it more likely to be near the nucleus and why?
Not totally sure, but I think that the probability is uniform because of the energy of the electrons going around the orbital, and at that point the pull from the nucleus doesn't make a difference in the location of the electron.
The probability depends on the shape of the shell itself. Some orbitals have nodal planes or areas where the probability density is equal to 0. This means that there is no possibility of finding an electron in these areas. An s-orbital, however, has a symmetrical electron probability density that is not uniform, but denser near the nucleus. I believe this might be due to the attraction between the positively-charged nucleus and the electron.
For p-orbitals, for example, it is unlikely to be near the nucleus because they have a nodal plane at the nucleus which means there is zero probability of finding an electron there. Due to the fact that p-orbitals, unlike s-orbitals, have angular momentum which pushes the electron away from the nucleus.
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