CHMA10H3 Lecture Notes - Lecture 20: Louis De Broglie, Balmer Series, Photon
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Bohr"s model of atoms helps us understand the observed line emission spectra: Planck"s equation relates the energy of a photon to the wavelength of light: n = 1 is the most stable, ground state https://onedrive. live. com/edit. aspx/documents/chemistry?cid=4612573e81e7633b&id=documents&wd=target%281. 1%20october. one%7cefd34092-1f66-4f 1/7. If supplied more energy, it goes to higher energy fields. Using bohr"s model, one can calculate the energy difference. In the visible range, for h, we only see 4 lines. Those lines are excited states coming back to second stable form, not the first stable form (balmer series) Energy levels within the lower level states are also invisible to us, we can"t see them. So other lines do exist, we just can"t see them. So in balmer"s equation, there was a 22 bc the energies went back to 2nd state. If you know energy, you can calculate wavelength. ***some kind of question like this on final exam*** The 121 nm fits with the wavelength calculation above https://onedrive. live. com/edit. aspx/documents/chemistry?cid=4612573e81e7633b&id=documents&wd=target%281. 1%20october. one%7cefd34092-1f66-4f 2/7.
