Why Are There Only 4 Visible Emission Lines in the Bohr Model for Hydrogen?

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The discussion centers on the confusion regarding the limited number of visible emission lines observed in the hydrogen atom when applying the Bohr model. While the model indicates that energy levels extend infinitely, only four visible lines are typically noted due to the wavelengths emitted beyond the visible spectrum when energy levels exceed n=4. The focus is on the Balmer series, which includes visible wavelengths from transitions between specific energy levels (n=3 to n=6). Beyond these levels, emissions fall into the ultraviolet range, which is not visible to the human eye. Additionally, the conversation highlights the existence of other spectral series beyond the Balmer series, emphasizing that a deeper understanding of atomic behavior may require moving beyond the Bohr model, although it remains sufficient for foundational chemistry applications.
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I am feeling a little stupid asking this considering I am about to graduate with my BS in chemistry. But I have never given this much thought, nor do I remember learning this and I can't figure out a proper explanation. I am sure I am overlooking a simple detail, but I can not figure it out.

Ok, so I understand the bohr model and the principles behind photon absorption/emission perfectly fine. But one thing that is puzzling to me is why is it when the bohr model is applied to an atom such as hydrogen, only 4 emission lines observed? Can't it have more? I ask this because, the energy levels, n, go from n=0,1,2,3,4,...,infinity, right? So obviously there are more than 4 different energy levels that are capable of emitting a photon. Anybody have an answer?

*edit*

I think I figured it out...is it due to when n>4 that the only wavelength emitted are beyond the visible spectrum, thus meaning it is not visible to us?
 
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Essentially, you have answered your own question, I think. However, it will be easiest to restrict our attention to the Balmer series, especially to the spectral lines H-alpha to H-gamma. Where λ >400nm (i.e. (n=3) to (n=6)) the photon emitted lies within the visible spectrum.

There are many series in addition to Balmer, even where n-prime is greater than 6.

There are series constructed entirely within the UV portion of the spectrum, for example.

If you are interested in physical fundamentals, you will have to go beyond the Bohr model, however for the purposes of the foundations of chemistry this could be unnecessary. Most applications of partially quantised classical theories and models are fine (i.e. work) within certain scales.
 
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