What Are the Last Four Jumps in Hydrogen's Spectral Lines?

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When a completely ionized hydrogen atom captures an electron, the electron can transition between energy levels, emitting light corresponding to specific spectral lines. The last four jumps in hydrogen's spectral lines relate to transitions between the lowest orbital energy levels, which are critical in understanding quantum mechanics. These transitions illustrate how atoms exist in discrete energy states and the resulting line spectra produced during electron excitation and relaxation. Quantum mechanics was developed to explain the stability of these orbits, countering classical physics predictions of energy loss. The discussion emphasizes the fundamental principles of quantum mechanics and their role in atomic behavior and spectral emissions.
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When a completely ionized atom of hydrogen captures an electron, the latter may conceivably cascade toward the nucleus by jumping successively from one permitted orbit to the next.
If we could watch the light emitted by this single atom, to what lines of the complete hydrogen spectrum will the last four jumps correspond?
 
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i cannot get the exact explanation from that link... please help me.
 
Do you know the 4 lowest orbital energy levels ?
 
then what are those?
 
This is the beginning of Quantum Mechanics. The fact that atoms can only exist in certain energy states and that they can only be excited to jump between those states accounts for the line spectra that they produce (and absorb).
The explanation is not just available in one paragraph.

QM had to be invented to explain away the fact that an electron in orbit (under acceleration) should, classically, be radiating energy constantly. This would cause its orbit to decay (like a satellite in a dense atmosphere). It doesn't. It goes on and on and on. You can 'explain' this by assuming that the electron, in this 'bound state' behaves like a wave. QM follows from this - along with line spectra etc. etc..
 

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