The discussion focuses on calculating the wavelengths of photons emitted during specific transitions in the hydrogen atom's spectral series: the 3rd line in the Lyman series, the 2nd line in the Balmer series, and the 1st line in the Paschen series. The Lyman series involves transitions from n ≥ 2 to n = 1, the Balmer series from n ≥ 3 to n = 2, and the Paschen series from n ≥ 4 to n = 3. The Rydberg formula is the key tool for calculating these wavelengths, with the specific transitions identified as n=4 for the 3rd line in Lyman, n=4 for the 2nd line in Balmer, and n=4 for the 1st line in Paschen.
PREREQUISITESStudents of physics, educators teaching atomic structure, and anyone interested in the quantization of energy levels in hydrogen and other elements.
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?