In the hydrogen spectrum,the wavelengths of l | vedclass

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(B) The Rydberg formula for the hydrogen spectrum is given by $\frac{1}{\lambda} = R \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right)$.Comparing this

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Brackett,infrared

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(B) The Rydberg formula for the hydrogen spectrum is given by $\frac{1}{\lambda} = R \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right)$.Comparing this with the given equation $\frac{1}{\lambda} = R \left( \frac{1}{4^2} - \frac{1}{n^2} \right)$,we find that $n_1 = 4$.The spectral series corresponding to $n_1 = 4$ is the Brackett series.The Brackett series transitions occur between higher energy levels $(n_2 = 5, 6, 7, \ldots)$ and the $n_1 = 4$ level.This series lies in the infrared region of the electromagnetic spectrum.

In the hydrogen spectrum,the wavelengths of light emitted in a series of spectral lines is given by the equation,$\frac{1}{\lambda}=R\left(\frac{1}{4^{2}}-\frac{1}{n^{2}}\right)$,where $n=5, 6, 7, \ldots$ and $R$ is Rydberg's constant. Identify the series and wavelength region.

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