[adam_goalietender]

Right now we are learning about the history of the development of the quantum model of the atom and im not sure about the origins of the quantum numbers but i'm gona give it a go.

The primary quantum number n
-Bohr came to the conclusion that there must be discrete values for energy of electrons in obrit of the nucleus due to the specific energies absorbed/emitted as observed by the visible electomagnetic line spectra of the light produced by excited electrons dropping from an exicted state to a ground state.
-The idea of discrete values is supported by the solutions to Blackbody radiation and the Photoelectric effect that both use the idea of discrete values of energy, photons in the photoelectric effect (i still dont fully understand blackbody radiation, but it has to do something with the fact that a perfectly black object, that absorbs all visible light and reflects none, gives of light as a function of its temperature...?)
-Then DeBroglie stated that maybe the orbitals for electrons are really standing waves with specific energies given by the formula l/lambda = n, furthering the idea of discrete values, but in a different way. So, when the "electron wave" is excited do its standing waves temperily become longer due to the imput of engery and then when they return to their groud state length the emitted engery creates line spectra...?

Secondary Quantum number L
-Shows the different types of angular momentums of elecrtons/electron waves within the "main energy" of the primary quantum number.
-L = 0 to n-1   e.g. if n=2 then L= 0 and 1
- This was created due to the linespectra that was used in the primary quantum number actually is made up of multiple lines when observed under high resolution, as described first by arnold summerfield, desribing them as slightly eliptical orbits with varying eccenrticity.

mL and mS only sortof make sense to me as well but the answers to these questions will help me to understand them better:

so then if an n=1 line spectra line is viewed under high resolution it should have only 1 line spectra line becuase when n = 1, L = only 0 therefore only one possible angular momentum for the 2 elsctrons in this S orbital...?also in this example mL = 0 and mS= +1/2 and -1/2 and therefore in a magnetic field only one line spectra line, under low resolution, will be observed because mL only allows for one directional orientation of the subshells and under high resolution will have 2 line spectra for the opposite spinning electrons...?

Also if n=2 then L = 0,1 so therefore
-2 line spectra will be view with no magnetic field under low res
-mL = 0 and -1,0,1 so therefore in a magnetic field 3 line spectra will be observed
-will there be 8 spectra lines, observed under high res in a magnetic field, in this situation 2 accounting for mL = 0 (2s orbital) the other 6 accounting for mL= -1,0,1 the (2p orbital) ...?

any help is much appreiciated

[ARGOS++]

Dear adam_goalietender;

Your assumption is correct, if you can fulfil all required resonance conditions for all electrons.

But you have to keep in mind, that the 2s (n = 2, l = 0) and the 2p (n = 2, l = 1) transitions will not emit/absorb not at the “same” wavelength, so it may be a little complicate to observe all at the same time in a high resolution instrument.

You may also read on:     http://en.wikipedia.org/wiki/Zeeman_effect
(See also the picture on the page under:  Lyman alpha transition in hydrogen)


Good Luck!
                    ARGOS⁺⁺