An electron in an excited state of a hydrogen atom emits two photons in succession, the first at 2165 nm and the second at 97.20 nm, to return to the ground state (n=1). For a given transition, the wavelength of the emitted photon corresponds to the difference in energy between the two energy levels.

What were the principal quantum numbers of the initial and intermediate excited states involved?

Question

An electron in an excited state of a hydrogen atom emits two photons in succession, the first at 2165 nm and the second at 97.20 nm, to return to the ground state (n=1). For a given transition, the wavelength of the emitted photon corresponds to the difference in energy between the two energy levels.



What were the principal quantum numbers of the initial and intermediate excited states involved?

anonymous · Answer

Use the rydberg formula: 1λ=E=R(1n2f−1n2i)

R=1.097∗107m−1

anonymous · Answer

I'm looking for two answers though

anonymous · Answer

n initial and n intermediate

anonymous · Answer

u need the definition

anonymous · Answer

Pardon? The definition of what?

anonymous · Answer

inn initial and n intermediate

anonymous · Answer

Could you assist me in how to do it?

anonymous · Answer

i will but u need to help me do u need the definition

anonymous · Answer

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