Hydrogen Spectra: Electron Jumping & Emitting Lines

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    Hydrogen Spectra
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Discussion Overview

The discussion revolves around the behavior of an electron in a hydrogen atom when it is excited from the ground state to a higher energy level, specifically from level 1 to level 4. Participants explore whether the electron returns directly to the ground state or cascades down through intermediate levels, and the implications of these processes on the emitted spectral lines.

Discussion Character

  • Exploratory
  • Debate/contested
  • Conceptual clarification

Main Points Raised

  • One participant questions whether the electron jumps back immediately to the ground state or cascades down through intermediate levels, potentially emitting multiple spectral lines.
  • Another participant suggests that if the electron cascades, it could emit multiple photons corresponding to the transitions, but emphasizes that the observed spectrum may show only one line for the direct transition from 4 to 1.
  • Some participants propose that all possible transition routes can occur, including direct and cascading transitions, but the actual observed outcomes depend on probabilities.
  • A later reply asserts that the behavior of the electron is governed by quantum mechanics, which involves probabilities rather than certainties.
  • There is a mention of the Balmer and Lyman series in relation to the transitions, but no consensus on the specific behavior of the electron in this scenario.

Areas of Agreement / Disagreement

Participants express differing views on the behavior of the electron during the transition, with no consensus on whether it will jump directly or cascade. The discussion remains unresolved regarding the specific outcomes of the excitation process.

Contextual Notes

Participants note that the outcomes depend on probabilities and that quantum mechanics inherently involves uncertainty. There is no resolution on the exact nature of the transitions or the resulting spectral lines.

Bassalisk
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Hello,


When electron is excited in single atom hydrogen, it jumps to a certain level, let's say from 1 to 4.

My question here is, does this electron jump back immediately to 1 or does it cascade itself down to 3 to 2 to 1. and emits 3 lines instead of just 1.


Thanks
 
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Bassalisk said:
Hello,


When electron is excited in single atom hydrogen, it jumps to a certain level, let's say from 1 to 4.

My question here is, does this electron jump back immediately to 1 or does it cascade itself down to 3 to 2 to 1. and emits 3 lines instead of just 1.


Thanks

Haven't you just answered your own question? If it is the latter, then you would see 3 separate lines of different wavelength. Instead, you see only one, and the photons have the same energy as the 4-to-1 transition.

Now, it doesn't mean that the 3-to-2-to-1 transition doesn't occur in some cases. In fact, the 3-to-2 is part of the Balmer series. But the 4-to-1 transition isn't a result of a 3-to-2-to-1 transition. The Lyman series does occur.

Zz.
 
As long as the jumps are between levels all possible routes can happen.
.4 to 1(in other words in one jump)
.4 to 3 to 1
.4 to 2 to 1
.4 to 3 to 2 to 1
 
Look, i am asking, when i excite the electron from 1 to 4th level, in nature, what will happen...

I don't ask u what wave lengths i could get, but I'm asking you what will happen, what does happen...I know if electron jumps back from 4 to 1, emits a photon with energy difference from those 2 levels. And if it cascades we will get bigger wave lengths due to less energy, but we will see more lines.

I am asking you, what WILL happen, will the photon jump back from 4 to 1 and emit one photon or cascade down and emit 3 photons but with larger wave lengths, how does that effect behave?
 
No one can tell you what WILL happen, there are several possibilities; each one with a certain probability. If you observe a large number of atoms you will see lines corresponding to all these probabilities.
 
f95toli said:
No one can tell you what WILL happen, there are several possibilities; each one with a certain probability. If you observe a large number of atoms you will see lines corresponding to all these probabilities.

Hence the Heisenberg?
 
No, this has nothing as such to do with Heisenberg. It is just how quantum physics works: we are always dealing with probabilties and as far as we know this is just how nature works.
 

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