In the hydrogen atom, transition takes place from n = 3 to n = 2 orbit. The wavelength of the emitted radiation lies in the _____ region.

Concept:

A spectral series is a collection of sequentially grouped wavelengths which describes light or any electromagnetic radiation released by energized atoms. Atomic hydrogen displays emission spectrum. This spectrum enfolds several spectral series. Once the electrons in the gas are excited, they transition between the energy levels.

Rydberg formula relates to the energy difference between the various levels of Bohr’s model and the wavelengths of absorbed or emitted photons. It is mathematically expressed as-

• \(\frac{1}{\lambda}=R_HZ^2(\frac{1}{n_l^2}-\frac{1}{{n_h^2}})\) where 

𝜆 is the wavelength

R is the Rydberg constant has the value \(R_H=1.09\times10^{7}m^{-1}\)

Z is the atomic number

\(n_l\) is the lower energy level

\(n_h\) is the higher energy level

Balmer series is displayed when electron transition takes place from higher energy states(\(n_h=3,4,5,6,...\)) to \(n_l=2\) energy state. All the wavelength of Balmer series falls in visible part of electromagnetic spectrum(400nm to 740nm).

Hence, the correct answer is Option-3-visible.