3 posts • Page 1 of 1
Bohr's model shows that electrons move from one orbit to another based on whether or not the energy of the photons is equivalent to the energy difference between the orbits. Thus, the spectral line is essentially a representation of this condition.
The bohr frequency condition states that the energy of the photon must match the energy needed to bring an electron to a higher energy state exactly in order to be absorbed, so the wavelengths shown on the spectrums just show which ones fit this condition because certain wavelengths correspond to specific frequencies and therefore specific energies (that must fit bohr's frequency condition).
Who is online
Users browsing this forum: No registered users and 2 guests