Question- the emission lines of hydrogen observed in the visible region belong to the Balmer series. They correspond to transition of electrons in the hydrogen atom (n=6 to n=2, n=5 to n=2, n=4 to n=2, n=3 to n=2). How do the theoretical energy values you calculated compare to the experimental energy you found by observation? Determine which energy transitions corresponds to which spectral line in the hydrogen emission spectrum?
The experimental energy values are Green -2.63*10^19, yellow- 3.37 * 10^-19., Red -3.03*10^-20.
I merely calculated the theoretical energy values using the formula E=-Rhc(1/(n^2)^2-1/(n1)^2)
I want proficient help to solve the above problem