The discussion revolves around determining the wavelengths of photons emitted in specific transitions of the hydrogen atom, focusing on the Lyman, Balmer, and Paschen series. The original poster expresses confusion regarding the meaning of "line" in this context.
Some participants have provided clarifications regarding the transitions for each series, and there appears to be a productive exchange of understanding about the spectral lines. However, the original poster's interpretation of the specific lines remains unconfirmed, as they seek validation of their reasoning.
There is an emphasis on understanding the definitions and transitions within the spectral series, with participants referencing external sources for additional context. The discussion does not resolve the original poster's confusion but highlights the need for clarity on the definitions used in the problem.
ojs said:The 'line' is a spectral line (see http://en.wikipedia.org/wiki/Hydrogen_spectral_series), for the Lyman series it is the transitions from n >= 2 to the n = 1 state, for Balmer series its from n >= 3 to the n = 2 state and the Paschen series are transitions from n >= 4 to n = 3 state. The first line in each series is the transition from the next lowest number in the series to the lowest (so in the Lyman series the first line would be from n=2 to n=1) and the second line would be from from the third lowest to the lowest (in Lyman it would be n=3 to n=1) etc etc.
To calculate the wavelength you can use the Rydberg formula.
Nope said:I see,
3rd line in the Lyman series --> ni=4
2nd line in the Balmer series --> ni=4
1st line in the Paschen series ---> ni=4
am i right?