The discussion focuses on the spectral emissions of CH* molecules in a candle flame, specifically the violet emission at 432 nm. This emission is attributed to chemiluminescence, where the energies of emitted photons correspond to specific wavelengths as described by the equation E = hc/λ. The conversation also draws parallels to the Balmer lines in the hydrogen spectrum, emphasizing the discrete nature of spectral lines and the underlying atomic and molecular energy differences.
PREREQUISITESStudents and educators in chemistry and physics, researchers interested in spectral analysis, and anyone studying the properties of light emissions from chemical reactions.
Kamakiri said:Homework Statement
In the spectrum of the blue part in a candle flame, there’s a violet emission at 432 nm due to excited CH* molecules (chemiluminescence). Why 432? Why not 400 or 500? There are emissions at 436, 475 and 520 nm too. Why these numbers?
2. The attempt at a solution
Is it because the energies of the photons emitted correspond to these wavelengths, as E = hc/λ?
I read about Balmer lines. The H-alpha spectral line of hydrogen gas is red, since the energy of the photons emitted correspond to 656.3 nm, as E = hc/λ. Is that right?Quantum Defect said:Why do the Balmer lines in the Hydrogen spectrum have the wavelengths that they have? If you know the answer to that question, you know why CH* emits at the wavelengths that it does.
Kamakiri said:I read about Balmer lines. The H-alpha spectral line of hydrogen gas is red, since the energy of the photons emitted correspond to 656.3 nm, as E = hc/λ. Is that right?