## Orbitals

Ben 1B
Posts: 55
Joined: Sat Aug 17, 2019 12:16 am

### Orbitals

How do you solve 1D.23 which asks how many orbitals can have the following quantum numbers in an atom? Is there a shortcut to finding out how many orbitals can have certain quantum numbers? Thanks!

SnehinRajkumar1L
Posts: 101
Joined: Thu Jul 11, 2019 12:15 am

### Re: Orbitals

Well, in the case of the question, we can look at part a.
You know that n = 2 and l = 1, meaning that it is in the p orbital. So, the orientation of the p orbitals doesn't matter and thus, there are 3 possible orbitals.
For part b, there is only one that can have those three quantum numbers because it specifies the orientation as well.

Nikki Razal 1L
Posts: 116
Joined: Fri Aug 30, 2019 12:17 am
Been upvoted: 1 time

### Re: Orbitals

Once you find out what "l" is, you can figure out how many orbitals there are because to find the number of orbitals you can plug "l" into the equation 2*l+1, and that will give you the number of orbitals. Or you can think that ml=-l,...0...,+l, and the number of values you get also = the number of orbitals.. For example, if l=1, ml= -1,0,1, and because there are 3 values for ml, you have 3 orbitals