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 ?

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 transitition from first excited level to ground level is about

The energy levels of a hypothetical one electron atom are shown in figure Find the ionization potential of the atom.

The energy levels of a hypotherical one electron atom are shown in figure Find the excitation potential for the state n = 3 .

The energy levels of a hypotherical one electron atom are shown in figure Find the excitation potential for the state n = 3 .

What is the wavelength of light emitted when the electron of a hydrogen atom undergoes a transition from an energy level with n= 4 to an energy level with n = 2 ? .What is the colour corresponding to this wavelength ?

What is the wavelength of light emitted when the electron of a hydrogen atom undergoes a transition from an energy level with n= 4 to an energy level with n = 2 ? .What is the colour corresponding to this wavelength ?

Suppose the energy of a hydrogen- like atom is given as E_(n) = (-54.4)/(n^(2))eV where ninN . Calculate the following: (a) Sketch the energy levels for this atom and compute its atomic number. (b) If the atom is in ground state, compute its first excitation potential and also its ionization potential. (c) When a photon with energy 42 eV and another photon with energy 56 eV are made to collide with this atom, does this atom absorb these photons? (d) Determine the radius of its first Bohr orbit. (e) Calculate the kinetic and potential energies in the ground state.