The ground state energy of hydrogen atom is `-13.6eV`. If an electron makes a transition form an energy level `-0.85 eV` to `-3.4 eV`, calculate the wavelength of spectral line emitted. To which series of hydrogen spectrum does this wavelength belongs?

Answer

`4853Å`, Balmer series

Explanation

In the given transition, energy emitted,
`E=E_(2)-E_(1)=-0.85-(-3.4)=2.55eV`.
`(hc)/lambda=2.55xx1.6xx10^(-19)J`,
`lambda=(hc)/(2.55xx1.6xx10^(-19))m=(6.6xx10^(-34)xx3xx10^(8))/(2.55xx1.6xx10^(-19))`
`=4.853xx10^(-7)m=4853Å`
This wavelength belongs to Balmer series of hydrogen atom.