[josepk2]

I am wondering about the hydrogen emmission spectrum. So my chemistry book says that the given values from the spectrum which are 410nm, 434nm, 486nm, and 656nm, are the only wavelengths that are allowed for the electrons of hydrogen, and also says that the Bohr's model fits the energy levels of the hydrogen. deltaE= (-2.178 x 10^-18) (Z^2 /n^2) But the calculated wave lengths using the Bohr model are giving wave lengths that are not even close to the allowed wavelengths. For example the calculated wave length needed for hydrogen to go from N=1 to N=2 is 1.216E-7M or 121.6nm. This value that we get is not even close to any of the discrete line spectrum... I dont understand what is going on can someone please clarify why the wave length associated with the electrons going from N=1 to N=2 does not correspond to the line spectrum as it says it should?

Its not my math either because this is straight out of a example in the book

[Borek]

410nm, 434nm, 486nm, and 656nm

http://en.wikipedia.org/wiki/Balmer_series