Calculate the frequency of the light emitted when an electron in a hydrogen atom makes each of the following transitions.

Question

Calculate the frequency of the light emitted when an electron in a hydrogen atom makes each of the following transitions. (Express in three sig. figs.)

n=7→n=3

n=5→n=1

n=9→n=5

Answer 1

must use the Rhydberg equation:

1/λ=R_h(1/n_f²-1/n_i²⁾

R_h=1.097E7 m^-1

nf is the final energy level and ni is the initial energy level

so transitioning from n=7 to n=3

1/λ=1.097E7(1/3²-1/7²)

λ=9.95E5 m

to convert wavelength to frequency use c=λf

where c is the speed of light 2.998E8m/s

2.998E8/9.95E5= 301.3 hz