## hw problem 1D.21

Joanna Mendoza 3J
Posts: 20
Joined: Sat Aug 24, 2019 12:17 am

### hw problem 1D.21

problem: Write the subshell notation (3d, for instance) and the number of orbitals having the following quantum numbers: (a) n=5, l=2; (b) n=1, l=0; (c) n=6, l=3; (d) n=2, l=1.

I know that to get the number of orbitals you use 2(l)+1 but can someone explain to me how to get/write the subshell notation?

Chem_Mod
Posts: 18739
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 635 times

### Re: hw problem 1D.21

Subshell notation is written as the shell number, followed by the type of orbital it belongs (Ex: 3p, 4s, 5d)

Angular momentum numbers correlate as follows:
l=0 --> s
l=1 --> p
l=2 --> d

For part a, since n=5 and l=2 (ie d), then the subshell is 5d.

AniP_2D
Posts: 95
Joined: Sat Aug 17, 2019 12:17 am

### Re: hw problem 1D.21

The subshell notation is basically the n-value and and the subshell that corresponds to l.
If l=0, s is the subshell, l=1 then p, l=2 then d, and l=3 f
So for (a) the subshell notation would be 5d and for (b) it would be 1s

For orbitals you would just look and see how many possible ml values the certain of quantum numbers would have, so for (a) since l=2, the possible ml values are -2, -1, 0, 1, 2, so there would be 5 orbitals. For (b) since l=0, the possible ml values are 0, so there would be only one orbital.