The energy levels of a hypothetical one - electron atom system are given by `E_n = 16/(n^2) eV`, where `n = 1, 2, 3,…….` . The wavelength of emitted photom corresponding to the transtition from first excited level to ground level is about

The energy levels of a hypothetical one electron atom are given by E_n = -(18.0)/(n^2) eV where n = 1,2,3,…. (a) Compute the four lowest energy levels and construct the energy levels diagram. (b) What is the first excitation potential (c ) What wavelength (Å) can be emitted when these atoms in the ground state are bombarged by electrons that have been accelerated through a potential difference of 16.2 V? (e) what is the photoelectric threshold wavelength of this atom?

The energy levels of a hypothetical one electron atom are given by E_n = -(18.0)/(n^2) eV where n = 1,2,3,…. (a) Compute the four lowest energy levels and construct the energy levels diagram. (b) What is the first excitation potential (c ) What wavelength (Å) can be emitted when these atoms in the ground state are bombarged by electrons that have been accelerated through a potential difference of 16.2 V? (e) what is the photoelectric threshold wavelength of this atom?

The energy levels of a hypothetical one electron atom are given E_(n) = - (18.0)/(n^(2)) eV , where n = 1,2,3 … a Cumpete the four lowest energy levels and construct the energy level diagram . b What is the excitation potential of the state n = 2 ? c What wavelengths (Å) can be emitted when these atoms in the ground stste are bombarded by electron that have been accelerate through a potential difference of 16.2 V d If these atoms are in the ground state , can they absorb radiation having a wavelength of 2000 Å ? e what is the photoclectric threshold wavelength of this atom ?

what is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n=4 to and energy level with n=2 ?

what is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n=4 to and energy level with n=2 ?

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from the energy level with n=4 to the energy level with n=1 ?

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from the energy level with n=4 to the energy level with n=1 ?

Energy levels of H atom are given by : E_(n)=(13.6)/(n^(2))eV , where n is principal quantum number. Calculate the wavelength of electromagnetic radiation emitted by hydrogen atom resulting from the transition : n=2 to n = 1.