When the electron of hydrogen atom transitions from n=4 energy level to n=2 energy level then...

The wavelength of the spectral line when the electron is the hydrogen atom undergoes a transition from the energy level 4 to energy level 2 is.

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 ?

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 ?

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 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 ?

An electron in a hydrogen atom jumps from n = 5 energy level to n = 1 energy level. What are the maximum number of photons that can be emitted ?

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) ?