All Questions
8
questions
9
votes
3
answers
1k
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How does an electrons's wave function change when it moves between energy levels?
I'm taking a class on QM and we're simulating the wave function of an electron in a box at the lowest energy level and I'm supposed to change the simulation to show the wave function for the next ...
-5
votes
1
answer
74
views
What is the energy difference between inner subshells?
For exemple, in silver the energy difference between the 4d 5s subshells is ≈ 4 eV (in the ultraviolet region, that's why it has no color, etc.), but what is the energy difference between some of its ...
-3
votes
1
answer
71
views
Stability of an atom in absence of EM field
According to Bohr model of atom, electrons move up an energy level in presence of EM field and emit a photon moving down the level.
In complete absence of any external EM field, shouldn't the electron ...
- 63
16
votes
4
answers
5k
views
Why do electrons jump back after absorbing energy and moving to a higher energy level?
Electrons in a shell absorb energy and move to higher energy levels, but they release their energy and jump back to the shell they originally were in. Why do they jump back? Why can they not keep ...
- 189
1
vote
2
answers
2k
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Why does a neutral atom of beryllium not have any electrons in a p orbital?
Here's what I understand about quantum number and orbitals, please correct me if anything is wrong:
Electrons enter into these different types of orbitals because they have a higher/lower amount of ...
- 31
2
votes
3
answers
6k
views
Are electron orbitals in a helium atom degenerate?
In a hydrogen atom, the presence of only one electron allows various orbitals' energy states to be dependent only on the principal quantum number and not on angular momentum. Orbital degeneracy and ...
- 123
4
votes
1
answer
2k
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How are subshells and shells arranged in an atom?
If $\mathrm{2s}$ and $\mathrm{2p}$ are in the second energy level, and $\mathrm{3s}$, $\mathrm{3p}$, and $\mathrm{3d}$ are in the next (3rd) energy level, how are these subshells arranged in space in ...
- 41
99
votes
7
answers
139k
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Why is the 2s orbital lower in energy than the 2p orbital when the electrons in 2s are usually farther from the nucleus?
My chemistry book explains that even though electrons in the $\mathrm{2p}$ orbital are closer to the nucleus on average, electrons from the $\mathrm{2s}$ orbital spend a very short time very close to ...
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