The energy of electron in the nth orbit of hydrogen atom is expressed as `E_(n) = (-13.6)/(n^(2))eV`. The shortest and longest wavelength of Lyman series will be
The energy of an electron in the nth Bohr orbit of hydrogen atom is
Energy of the electron in nth orbit of hydrogen atom is given by E_(n) =-(13.6)/(n^(2))eV . The amount of energy needed to transfer electron from first orbit to third orbit is
The lagest and shortest wavelengths in the Lyman series for hydrogen
Calculate the shortest and longest wavelength in hydrogen spectrum of Lyman series.
An electron in the n = 1 orbit of hydrogen atom is bound by 13.6 eV energy is required to ionize it is
The ratio of the longest and shortest wavelengths of the Lyman series is approximately
Energy of an electron in a hydrogen atom is calculated as E_n=(-13.6)/n^2 eV. Is it possible for an electron in hydrogen atom to have energy of 2.8 eV
(a) Calculate the kinetic energy and potential energy of the electron in the first orbit of hydrogen atom. (b)Calculate the longest and shortest wavelength in the Balmer series of hydrogen atom.
According to Bohr theory, the electronic energy of hydrogen atom in the nth Bohr orbit is given by E_(n)=-(21.76xx10^(-19))/(n^(2))J . Calculate the longest wavelength of light that will be needed to remove an electron from the 2nd orbit of Li^(2+) ions.
