A schematic of the energy levels of a hypothetical atom (not specifically hydrog

Question

A schematic of the energy levels of a hypothetical atom (not specifically hydrogen) is shown below. An electron has been excited from energy level 1 to energy level 5 by absorbing a photon. Note you may find that you use a specific transition to answer more than one question.

Which transition to lower energies represents the smallest energy change?

Which transition, as shown, is not possible?

Which of the transitions resulting in an emission line represents the reddest (or longest) wavelength?

Which of the transitions resulting in an emission line represents the bluest (or shortest) wavelength?

Which of the transitions resulting in an emission line results in a photon with the same energy as that absorbed originally?

Explanation / Answer

1) From the given diagram , for Transition E ( from n = 5 to n= 3) the energy change is smallest.

2) Transion D is not possible as it does not end up at a fixed energy level.

3) Minimum energy change corresponds to maximum wavelength ( reddest) . Therefore, Transition E represents the reddest wavelength.

4) Maximum energy change corresponds to minimum wavelength. Therefore, Transition B is the answer.

5) Electron jumped from n = 1 to n = 5 then came back to n = 1 . Transition B represents the same.

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