What Are the Limitations of Rydberg's Equation in Atomic Spectroscopy?

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Rydberg's equation is limited in atomic spectroscopy as it primarily applies to hydrogen-like atoms and does not account for electron-electron interactions in multi-electron systems. It assumes that electrons move in circular orbits, which oversimplifies their behavior and neglects quantum mechanical effects. Additionally, the equation fails to accurately predict spectral lines for complex atoms due to its reliance on fixed energy levels. Users are encouraged to demonstrate their problem-solving attempts to receive further assistance. Understanding these limitations is crucial for accurate analysis in atomic spectroscopy.
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The teacher told us to start with Bohrs equation, E=-2.18x10^-18(z^2/n^2).
Then using ΔE= E_f - E_i , and E=λv.

Also what are the limitations of using Rydberg's equation?

Thanks
 
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