Orbitals  [ENDORSED]

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Postby Kiara1F » Fri Jun 24, 2016 11:44 am

In lecture it was mentioned that after the f orbital ..(it was some type of trick question) that there was another orbital -- can anyone explain this?

I think he called it a g-orbital or state..? Does this mean that the electrons just end up back in the ground energy state?

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Re: Orbitals

Postby 104890318 » Fri Jun 24, 2016 2:52 pm

F-orbitals are more complicated than any other orbital(i.e. p-, d-). there are seven different types of f orbitals. For f-orbitals n=2, l=3, and ml=-1,0,1.
Now the tricky thing about G-orbitals is that n has to equal 5 so that l=4. However, this can never occur while in ground state. G-orbitals can only occur in higher levels of energy.

jeree pucan
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Re: Orbitals

Postby jeree pucan » Fri Jun 24, 2016 3:47 pm

I think essentially he was trying to say that L can be 0,1,2,3,4,... however the corresponding orbitals were s,p,d, and f so there was no further orbital for any value after 3. It is possible for the L-value to have values greater than 3 however they occur at a higher level.

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Re: Orbitals  [ENDORSED]

Postby Chem_Mod » Sun Jun 26, 2016 2:10 pm

There is nothing tricky about the orbitals beyond f. The rules for possible quantum numbers n, l, and ml are results of solving the Schrodinger Equation, and there is no reason why l cannot be 4 or higher since this is an allowed number according to the rules. So, there definitely are g-orbitals and even more complicated orbitals. The point that he wanted to make clear is that we do not currently know of any element (recall the periodic table stops around ~115) which have electrons occupying the g-orbital in the ground state.

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