A hydrogen atom in its excited state emits radiations of wavelengths 1218\AA and 974.3\AA when it finally comes to the ground state. Identify the energy levels from where transitions occur. Given Rydberg constant R=1.1\times 10^{7}\; m^{-1}. Also specify the spectral series to which these lines belong.

 

 
 
 
 
 

Answers (1)
S safeer

\lambda _{1}=1218\; \AA

\lambda _{2}=974.3\; \AA

Rydberg const, R=1.1\times 10^{7}\; m^{-1}

\frac{1}{1218\times 10^{-10}}=1.1\times 10^{7}\left ( \frac{1}{1^2}-\frac{1}{n^{2}} \right )

n^{2}=\frac{1}{0.2536}

n^{2}=3.9429               \therefore n=1.98\cong 2

 given \lambda _{2}=974.3\; \AA 

\frac{1}{974.3\times 10^{-10}}=1.1\times 10^{^{-1}}\left ( \frac{1}{1^{2}}-\frac{1}{n^{2}} \right )

n^{2}=\frac{1}{0.0669}

n^{2}=14.9411

\therefore n=3.86\cong 4

These lines belong to layman series

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