The hydrogen emission spectrum has four series (or sets) of lines named Balmer, Brackett, Paschen, and Lyman. Indicate the energy (infrared, ultraviolet, or visible), the nf value for each series, and all possible ni values up to 7
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To determine the energy range (infrared, ultraviolet, or visible), the nf value, and all possible ni values for each series in the hydrogen emission spectrum, we need to understand the energy levels involved and the transitions that occur.
1. Balmer series:
- Energy: Visible light
- nf value: 2 (as Balmer series corresponds to the transition level where the electron jumps to the second energy level)
- Possible ni values up to 7: 3, 4, 5, 6, 7
2. Brackett series:
- Energy: Infrared light
- nf value: 4
- Possible ni values up to 7: 5, 6, 7
3. Paschen series:
- Energy: Infrared light
- nf value: 3
- Possible ni values up to 7: 4, 5, 6, 7
4. Lyman series:
- Energy: Ultraviolet light
- nf value: 1
- Possible ni values up to 7: 2, 3, 4, 5, 6, 7
The pattern in the hydrogen emission spectrum arises from the electron transitioning between energy levels in the hydrogen atom. Each series corresponds to a different final energy level (nf value), and the possible initial energy levels (ni values) depend on the specific series.
To find this information, you can refer to the Rydberg formula:
1/λ = R * (1/nf^2 - 1/ni^2)
where λ is the wavelength, R is the Rydberg constant, nf is the final energy level, and ni is the initial energy level.
By applying this formula and analyzing the resulting wavelengths, you can identify the energy range for each series, the nf value, and the possible ni values up to 7.