In the spectrum of a specific element, there is a line with a wavelength of 656 nm. Use the Rydberg equation to calculate the value of n for the higher energy Bohr orbit involved in the emission of this light. Assume the value for the lower energy orbit equals 2.

Question

In the spectrum of a specific element, there is a line with a wavelength of  656  nm. Use the Rydberg equation to calculate the value of n for the higher energy Bohr orbit involved in the emission of this light. Assume the value for the lower energy orbit equals 2.

DrBob222 · Answer

1/wavelength = R(1/4 - 1/n^2) 1/4 is 1/2^2