Changes

Bohr modeled his atom on the emission spectrum of hydrogen. The [[element]]al atom of hydrogen at ground state contains an electron in the first electron orbit, n=1. When the atom is excited the electron can jump into a higher state including energy levels n=2, n=3, n=4, n=5, n=6, and then would fall back to its ground state. Bohr calculated a number of transitions were possible, including:

Bohr modeled his atom on the emission spectrum of hydrogen. The [[element]]al atom of hydrogen at ground state contains an electron in the first electron orbit, n=1. When the atom is excited the electron can jump into a higher state including energy levels n=2, n=3, n=4, n=5, n=6, and then would fall back to its ground state. Bohr calculated a number of transitions were possible, including:

* Paschen Series - wavelength in the [[Infrared|IR]] range, when an electron falls to n=3 from a higher orbit

* Paschen Series - wavelength in the [[Infrared|IR]] range, when an electron falls to n=3 from a higher orbit

* Balmer Series - wavelength in the visible range, when an electron falls to n=2 from a higher orbit, specifically

* [[Balmer series|Balmer Series]] - wavelength in the visible range, when an electron falls to n=2 from a higher orbit, specifically

** n=3 to n=2 - 656.3nm (red)  

** n=3 to n=2 - 656.3nm (red)  

** n=4 to n=2 - 486.1nm (blue)

** n=4 to n=2 - 486.1nm (blue)