Hmmm.... how to explain this...
I'll try.
Quote:
What is the total number of atomic orbitals possible at n =3?
I thought the answer would be 5 but it's actually 9, can someone explain why there are 9 orbitals?
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Okay, if n=3, then it means that there are 3 azimuthal quantum values (l): 0, 1 and 2, as given by the statement 0 <= l < n (l = n-1).
Anyway,
l = 1 includes 1 type "s" orbital.
l = 2 includes 3 type "P" orbitals.
l = 3 includes 5 type "d" orbitals. If you add the total number of orbitals up (1+3+5), you get
9.
Quote:
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How many electrons in an atom can have the following sets of numbers: n= 4 and m(subscript l)= +2/-2? The answer is 8 while I thought it was 14. Can someone also explain this?
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Hmmm... again, it's rather hard to explain.
Basically, there are 4 orbitals that fulfil those requirements (+2/-2) when n = 4. There are m=+2/-2 orbitals in the
l = 2 subshell, and m=+2/-2 orbitals in the
l= 3 subshell. (4*2) = 8.
I hope this helps!
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