Question

In the Balmer series of lines of the hydrogen spectrum, the third line from the red end corresponds to which one of the following inter-orbit jumps of the electrons for Bohr's orbits in an atom of hydrogen?

Answer 1

Hint: We know that the balmer series is a series of spectrum emission lines of hydrogen atom which results when electron transition occurs from higher level down to energy level with principal quantum number $ 2. $ Paschen series is a series of spectrum emission lines of hydrogen atom which results when electron transition occurs from higher level down to energy level with principal quantum number $ 3. $

Complete answer:
The Bohr model was introduced by Neil’s Bohr in $ 1913. $ It is a system consisting of a small, dense nucleus surrounded by orbiting electrons. It is similar to the structure of the solar system but it provides attraction of electrostatic forces instead of gravity. The atom will be completely stable in the state with the smallest orbit after that there is no orbit of lower energy into which the electron can jump.
Atoms, molecules or ions that absorb radiations are called excited. Spectrum of visible light is continuous. Spectrum of atoms in gaseous state does not show continuous spectrum but they emit light at specific wavelengths with dark spaces between them. Such spectrum is called line spectrum or atomic spectrum. Line emission spectrums are important to understand electronic structure; each element has a unique line emission spectrum. When an electric discharge is passed through gaseous hydrogen, hydrogen molecules dissociate and energetically excited hydrogen atoms produce electromagnetic radiations of discrete frequencies.
The Hydrogen spectrum consists of several series of lines named after discoveries. Balmer showed when spectral lines are expressed in terms of wavenumber, then visible lines of hydrogen spectrum. Where n is an integral equal to or greater than three Series of lines described by this formula $ \bar{v}=109.67\left( \dfrac{1}{{{2}^{2}}}-\dfrac{1}{{{n}^{2}}} \right)c{{m}^{-1}}, $ are called Balmer series. Balmer series are only lines in the hydrogen spectrum which appear in visible regions.
Here the line at red end suggests that,
First line in the Balmer series is $ n=3 $ to $ n=2. $
Second line in the Balmer series is $ n=4 $ to $ n=2. $
Third line in the Balmer series is $ n=5 $ to $ n=2. $
Therefore, the electrons jump from $ n=5 $ to $ n=2. $ .

Note:
Remember that Spectrum of visible light is continuous. Spectrums of atoms in gaseous state do not show continuous spectrum but they emit light at specific wavelengths with dark spaces between them. Such spectrum is called line spectrum or atomic spectrum. Balmer showed when spectral lines are expressed in terms of wavenumber, then visible lines of hydrogen spectrum. As we move away from the nucleus, the energy of the orbit increases. Bohr’s orbit is a hypothetical path of an electron about the nucleus of the Bohr atom.