Difference between Balmer series and Brackett series
The origin of the spectral lines is comes from the Bohrs model. When electrons jump from higher energy states to lower energy state it release energy in the form of a photon. According to Bohr theory, the wavelengths of the hydrogen spectrum can be calculated by the Rydberg formula. The Balmer series, Bracket series are nothing but the different transition states for the hydrogen atom when an electron is excited. When electron is excited from one state to another state it will eventually lose energy. If electron is excited from n=2 state to n=4 state and return back by loosing energy to n=0 state then it is called Balmer series. For Balmer series it takes values from n = 3, 4, 5,6 ……to n = 2. Similarly for Brackett series when electron is excited from n=4 to n=6 then it will loose energy and return back to n=4 state then it is called Brackett series. Paschen series takes values from from n =5, 6, 7……to n = 4. We can see these spectral lines spectrum by spectroscope. The difference between them is as follows.
|1) The spectral lines of Balmer series is lie in the Visible region.
2) The wavelength of Balmer series is ranges from 4000- 6500 A°.
3) The wavelength of the first line of Balmer series is 6559.2 A°
4) The wavelength of series limit of Balmer series is 3644 A°
5) For Balmer series ni= 3,4,5,… and nf = 2.
|1) The spectral lines of Brackett series is lie in the infrared region.
2) The wavelength of Brackett series is ranges from 10450 – 40500 A°.
3) The wavelength of the first line of Brackett series is 40501 A°
4) The wavelength of series limit of Brackett series is 14580 A°
5) For Brackett series ni= 4,5,6,… and nf = 4.