Electron transition in bohr's model

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Discussion Overview

The discussion centers on electron transitions in Bohr's model of the atom, specifically how an atom can emit multiple wavelengths of light despite having a single electron. Participants explore the implications of energy absorption and emission during these transitions, as well as the practical aspects of spectroscopy in observing these phenomena.

Discussion Character

  • Exploratory, Technical explanation, Conceptual clarification, Debate/contested

Main Points Raised

  • One participant explains that in Bohr's model, electrons absorb energy to transition to higher energy levels and emit energy when returning to lower levels, with the emitted energy corresponding to the difference between these levels.
  • Another participant clarifies that while a single transition results in one specific wavelength, observing many atoms or multiple excitations of the same atom can yield multiple wavelengths.
  • A participant compares the situation to rolling multiple dice, where one die shows one number, but many dice show a range of numbers.
  • There is a mention of single-atom spectroscopy, which exists but is not applicable for the example discussed.
  • A question is raised about whether two different wavelengths in single-atom spectroscopy would indicate two different electrons transitioning or one electron making two transitions.
  • A later reply suggests that one electron could indeed make two jumps, implying a potential for multiple emissions from a single electron.

Areas of Agreement / Disagreement

Participants generally agree on the mechanics of electron transitions and the nature of emitted wavelengths, but there is some uncertainty regarding the implications of single-atom spectroscopy and how to interpret multiple wavelengths in that context.

Contextual Notes

Participants discuss the practical application of spectroscopy and the conditions under which multiple wavelengths can be observed, highlighting the dependence on the number of atoms and excitations involved.

Who May Find This Useful

This discussion may be useful for individuals interested in atomic physics, spectroscopy, and the Bohr model, particularly those exploring the nuances of electron transitions and their implications in experimental settings.

quicksilver123
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alright, so in bohr's model, an atom's electrons absorb energy and undergo electron transition. it jumps from a lower energy level (orbital) to a higher one.
in time, the attraction between the nucleus and the electron will pull the electron back to its original energy state (orbital).

when this happens, the electron emits its absorbed energy. the magnitude of said energy is equal to the difference between the two energy levels (orbitals) mentioned above.

that's my understanding of the concept.



hydrogen will release four different wavelengths. via spectroscopy, they are found to be (rounded):

410nm
434nm
486nm
656nm


how can an atom with a single electron release four different wavelengths of light? with the theory stated above, shouldn't there only be one wavelength released per electron?
 
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Those are possible wavelengths in a transition. A single transition will give just one specific wavelength, but usually you observe many atoms and/or many excitations of the same atom(s), so you can see all options (and some more).
 
how can an atom with a single electron release four different wavelengths of light? with the theory stated above, shouldn't there only be one wavelength released per electron?
The word "hydrogen" in
hydrogen will release four different wavelengths. via spectroscopy, ...
refers to the bulk material ... containing many many individual hydrogen atoms. Spectroscopy would use, at least, a glass tube filled with hydrogen gas ... you can also use the Sun.

It's a bit like how you roll one die once you only get one number but lots of them let you see lots of numbers.
 
thanks. i thought the given example only referred to a single atom viewed in a spectroscope.
this way is more practical, and makes more sense.
 
easy mistake to make ;)
single-atom spectroscopy exists btw - just not for this application.
 
just to confirm - in single atom spectroscopy, if an unknown substance were used, two different wavelengths would indicate that two different electrons had jumped orbitals?
 
Or one electron had made two jumps...
 

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