Explain the origin of spectral lines of hydrogen using Bohr’s theory?

Explanation

The radiation of particular wavelength or frequency are emitted when electrons jump from higher energy ievel to lower energy level. These radiations are called spectral lines. The wavelength of these spectral lines depend upon the energies between two energy levels in which transition of electron takes place. A group of spectral lines arising from the transition of electrons from the higher energy states to a particular lower energy state form a spectral series.
Hydrogen spectrum consists of the following five series: (i) Lyman series When a electron jumps from any higher orbit to first orbit, the series obtained is called Lyman series. Its wavelength is given by
`(1)/(lambda)=R(1)/(I^(2))-(1)/(n_(i)^(2))` where `n_(i) =2,3,4,5` the series lies in ultraviolet region
(ii) Balmer series When an electron jumps from any higher orbit so second orbit, the series obtained called Balmer series. Its wavelength is given by
`(1)/(lambda)=R(1)/(2^(2))-(1)/(n_(i)^(2))` where `n_(i) =3,4,5` the series lies in visible region
(iii) Paschen series When an electron jumps from any higher orbit to third orbit, the series obtained is called Paschen series. Its wavelength is given by
(iv) Bracket series When an electron jumps from any higher orbit to fourth orbit, the series obtained is called Bracket series. Its wavelength is given by
(v) pfund series When an electron jumps from any higher orbit to fifth orbit, the series obtained is called Pfund series. Its wavelength is given by
`(1)/(lambda)=R(1)/(5^(2))-(1)/(n_(i)^(2))` where `n_(i) =6,7,8 `... The series lies in far infraraed region