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/x^2) Convert wavelength to meters. You know R, the 1/4 is 1/2^2. X will be the higher orbit.