Hypothetical atom + Rydberg equation

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The discussion centers on calculating photon wavelengths and energies for a hypothetical atom with specified energy levels. To find the wavelength for exciting an electron from E1 to E4, the Rydberg equation must be adapted for hydrogen-like ions by incorporating the atomic number (Z). Participants express confusion about applying the equation correctly, noting that the standard form is limited to hydrogen. The conversation emphasizes the need for a modified version of the equation to accommodate the unique properties of the hypothetical atom. Understanding these adjustments is crucial for solving the homework problems effectively.
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Homework Statement



Consider the following energy levels of a hypothetical atom.
E4 -1.0 10-19 J

E3 -5.0 10-19 J

E2 -10 10-19 J

E1 -15 10-19 J
(a) What is the wavelength of the photon needed to excite an electron from E1 to E4?
_______nm
(b) What is the energy (in joules) a photon must have in order to excite an electron from E2 to E3?
_______J
(c) When an electron drops from the E3 level to the E1 level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process.
_______nm

Homework Equations



1/lambda= R(1/n^2-1/n^2)

The Attempt at a Solution


I have no idea where to start other than that equation... I did the ones that involved hydrogen but I'm stuck on these on... can you point me in the right direction?
 
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This is an almost good equation. Problem is, as written it holds only for a hydrogen atom, while this is an "hydrogen-like" ion. There is a slightly modified version of the formula that includes Z (atomic number) and holds in this case.
 
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