Determine the wavelengh of light emitted when a hydrogen atom makes a transition from the n=6 to the n=2 energy level according to the Bohr model

Using Bohr's model , calculate the wavelength of the radiation emitted when an electron in a hydrogen atom make a transition from the fourth energy level to the second energy level

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 ? In which region of the electromagnetic spectrum does this radiation fall ?

What is the energy difference and the frequancy and the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from the energy level n = 4 to the energy n = 3 given that the value of Rydberg constant is 1.0974 xx 10^(7)m^(-1) ?

Calculate the wavelength of radiation emited when an electron in a hydrogen atom makes a transition from an energy level with n = 3 to a level with n= 2

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 ? (Given R_(H) = 109677 cm^(-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 ?

Determine the energy of the photon (in eV) emitted when the electron in a hydrogen atom undergoes a transition from the n = 8 level to then = 6 level.