For the series of spectral lines of atomic hydrogen with n1 = 3, which of the fo

Question

For the series of spectral lines of atomic hydrogen with n1 = 3, which of the following wavelengths does not correspond to a wavelength predicted by the Rydberg equation? Rydberg equation: 1/? = (1.097 x 107 m-1) x (1/n12 - 1/n22) ----- A. 1875 nm B. 1282 nm C. 1184 nm D. 1094 nm E. 1005 nm

Explanation / Answer

There are a couple of forms of the Rydberg equation. What you partially show is this one I beleive 1/lambda = R(1/n1^2 - 1/n2^2) where lambda is the wavelength in m and R is the Rydberg constant 1.097 x 10^7 m^-1. For the series of spectral lines with n1 = 3 you are looking at the series of electronic transitions n2 --> n1 4 ----> 3 5 ----> 3 6 ----> 3 7 ----> 3 8 ----> 3 etc. So to answer this question you need to calculate the wavelength from the equation for each possible transition and find the one that doesn't match. Note - the equation gives wavelengths in m you then need to convert to nm

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