Changes

If a electron in the ground state absorbed energy it would be able to be promoted to a higher energy orbit. After time it would fall back to its original state releasing a photon of light with energy corresponding to the gap between the two levels. The electron did not necessarily fall straight back, for example it could jump from n=1 to n=3 and either fall back from n=3 to n=1 or from n=3 to n=2 and then n=2 to n=1. As the energy levels between each level were different this allowed for a number of wavelengths to be emitted if a sample was exposed to a large energy source, however as the values were fixed only specific wavelengths were allowed hence explaining the discrete lines on the emission spectra of elements.

If a electron in the ground state absorbed energy it would be able to be promoted to a higher energy orbit. After time it would fall back to its original state releasing a photon of light with energy corresponding to the gap between the two levels. The electron did not necessarily fall straight back, for example it could jump from n=1 to n=3 and either fall back from n=3 to n=1 or from n=3 to n=2 and then n=2 to n=1. As the energy levels between each level were different this allowed for a number of wavelengths to be emitted if a sample was exposed to a large energy source, however as the values were fixed only specific wavelengths were allowed hence explaining the discrete lines on the emission spectra of elements.

Bohr modeled his atom on the emission spectrum of hydrogen. The [[Element|elemental]] 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 [[Infra red|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 - 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=7 to n=2 - 397.0nm (violet)

** n=7 to n=2 - 397.0nm (violet)

** n=8 to n=2 - 388.9nm (violet)

** n=8 to n=2 - 388.9nm (violet)

* Lymann Series - wavelength in the [[Ultra violet|UV]] range, when an electron falls from n=2 to n=1

* Lymann Series - wavelength in the [[Ultraviolet|UV]] range, when an electron falls from n=2 to n=1

==Limitations==

==Limitations==