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How many different spectral lines would an element have if it only had two different electron...

How many different spectral lines would an element have if it only had two different electron energy levels (ground state and first excited state)? Explain answer and ignore ionization
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Answer #1

If you ignore ionization, then the electron can only jump from ground state to the first excited state and from the first excited state to the ground state. When the electron jumps from ground to the excited state it will absorb a light of wavelength

where E1 is the energy of the excited state and E0 is the energy of the ground state.

When the electron jumps from the excited state to the ground state, it will emit a photon with the same wavelength

Therefore there is just one spectral line whose wavelength is

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