Spectrum of singly ionised helium

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Ionized helium, with two protons, has a line spectrum that differs from hydrogen due to the increased attraction of the electron, which is doubled at the same distance. The energies in the spectrum are not entirely different; they are multiplied by a factor of four due to the increased nuclear charge. To compare the frequencies of the first lines in the hydrogen and singly ionized helium spectra, the Rydberg formula can be applied, where the factor of Z² accounts for the differences, with Z being 1 for hydrogen and 2 for helium. Understanding this relationship helps clarify the spectral differences between these two elements. Utilizing the Rydberg formula will facilitate further comprehension of the topic.
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Dear Friends!
We know ionized helium has two protons in its nucleus, whereas hydrogen has one. This changes the line spectrum completely.
Why? Thank You in advance!
 
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The attraction of the electron doubles at the same distance.
The line spectrum is not completely different, all energies are multiplied by a factor of 4.
 
Thank You!
Frequency corresponding to first line in Laymen series in hydrogen spectrum is to be compared to the corresponding line in single ionised helium.
How to proceed to find the solution if relevant.
I am studying this subject after a long time ,but am keen.
I hope to accelerate my understanding with your expert guidance!
Thanks!
 
Just use the Rydberg formula. You'll see a factor of Z2 there. It is 1 for hydrogen and 22=4 for helium, everything else stays the same.
 

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