Any Chemistry majors out there???

Question

Normal Quantum Number Values are
primary-N: 1 to infinity
secondary-L: 0 to (N-1)
magnetic-M:-L to +L
spin-S: +1/2, 0, -1/2
What if I change some of them, and my new set of quantum number values is:
primary-N: 1 to infinity
secondary-L: 0 to N
magnetic-M:-L to +L
spin-S: +1, 0, -1

Can you please tell me how this would change the electron configuration of an element, and therefore how the location would change on the periodic table of elements?

Can you please five me the old and new electron configurations for some elements of your choice so that I can understand better?


Thanks soooo much!!!

I think the change in spin has something to do with one vs. two electrons per orbital....something like that. Please help!!!

I know what the significance of each original quantum number is, but we are now changing that. If all other factors remain constant, and just the quantum numbers are changed, what would happen? I am not talking Earth here, but in general. The new spin is +1, 0, and -1. That is a change. What happens because of this?

I have a typo in one of my requests above.
Can you please give me the old and new electron configurations for some elements of your choice so that I can understand better?

This is an AP Chemistry challenge problem. Please do not post responses saying that it is not possible or anything, because I know that. This is discussing hypotheticals.

Answer 1

The principal quantum number (n) will remain integers starting as 1 and increasing. This would mean that the relative size of the electron cloud distribution would remain about the same.

If the angular quantum number (l) is limited to n and not (n-1), then an additional shape for the electrons at that level would be allowed. This would mean that the elements in the first row of the periodic table would not be limited to just a single s-orbital (l=0, holding 2 electrons) but p-orbitals (l=1, each holding 2 electrons) as well. Additional elements would be added to each row as the new angular quantum number would allow.

If the magnetic quantum number (m) keeps the original constraints, the the shape of the sub-orbitals would remain the same. S-orbitals would be spherical, p=orbitals tear-drop shaped, etc.

The new values for spin may have no direct effect. The numerical +/- 1/2 were originally arbitrary to denote clockwise and counter-clockwise spin. Perhaps paramagnetic elements (those with unpaired electrons) may behave differently, but this would not effect electron configurations.

I do not know if there is a direct correlation to be made using known elements. One consequence of the new quantum numbers would require a change in Hund's Rule. The initial electrons would go into the 1s orbit, but now a 1p orbit (with three p-orbitals) would be needed to complete the first row on the periodic table.

Hydrogen and Helium would be followed by Elements 3,4,5,6,7 and 8 but these would have different properties than Lithium through Oxygen. These elements would have a different number of electrons in their outer orbitals.

For example Element 8 (Oxygen) is currently 1s^2 2s^2 2p^4. In the new system, it would be 1s^2 1p^6. It would have it's outer orbitals filled and be chemically like a noble gas (if it would be a gas).

Additional: spin = + 1/2 or - 1/2 changing to spin = +1 or 0 or - 1. Yes, three spin states (no matter what the numbers might be) would allow 3 electrons per orbital instead of just 2.

The new 1s could hold Elements 1, 2 and 3. The new 1p could then hold Elements 4,5,6,7,8,9,10,11,12. Oxygen (Element 8) would be 1s^3 1p^5.

Since zero spin is usually not allowed, you teacher could have wanted the spin quantum numbers to just be twice the original (s = +1, +1/2, -1/2, -1) allowing for 4 electrons per orbital instead of two.

This would mean that the new 1s could hold 4 electrons (Elements 1,2,3 &4) and the new 1p could hold 12 electrons (Elements 5 through 16). Now Oxygen would be 1s^4 1p^4.

Answer 2

Spin can only be +/- 1/2, since only two electrons can go into one orbital.

The quantum numbers deal with solutions to the Schrodinger equation, which describes the mathematical possibilities as to where the electron is located vaguely in terms of its position and precisely in terms of its energy (Heisenberg Uncertainty Principle comes into play). As a result, the secondary quantum number L can not be equal to N.

Answer 3

L or Angular quantum number dictates partition of electrons into orbitals. Changing it would include higher energy levels into lower orbits.