The wavelength of emitted photons:

$\overline{)\frac{\mathbf{1}}{\mathbf{\lambda}}{\mathbf{=}}{\mathbf{R}}{\mathbf{(}}\frac{\mathbf{1}}{{{\mathbf{n}}_{\mathbf{1}}}^{\mathbf{2}}}{\mathbf{-}}\frac{\mathbf{1}}{{{\mathbf{n}}_{\mathbf{2}}}^{\mathbf{2}}}{\mathbf{)}}}$

The bluer section of the hydrogen spectrum is characterized by short wavelengths. It is therefore in the Lyman series. For the Lyman series, n_{1} = 1

n_{2} has values of 2, 3, 4, 5, 6...

In the hydrogen atom, why do the lines get closer together as you go bluer?

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