Question
How many orbitals are available with the following combination of quantum
numbers?
1) n = 2; l = 0
2) n = 3; l = 2
3) n = 4; l = 3
I have figured that it is
1) 2s
2) 3d
3) 4f
but i don't know what to do after this.
numbers?
1) n = 2; l = 0
2) n = 3; l = 2
3) n = 4; l = 3
I have figured that it is
1) 2s
2) 3d
3) 4f
but i don't know what to do after this.
Answers
bobpursley
the number of orbitals in energy level n is n^2
a) n=2, n^2=4 ( 2s,2px,2py,2pz)
b) n=3, n^2=9 (3s,3px,3py,3pz,3d1,3d2,3d3,3d4,3d5)
a) n=2, n^2=4 ( 2s,2px,2py,2pz)
b) n=3, n^2=9 (3s,3px,3py,3pz,3d1,3d2,3d3,3d4,3d5)