Orbitals
Moderators: Chem_Mod, Chem_Admin
-
- 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.
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.
-
- 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
-
- Posts: 103
- Joined: Wed Sep 30, 2020 9:34 pm
Re: Orbitals
Finding the number of orbitals doesn't have a short cut to my knowledge, but it's not super hard to do. Know that l=0 is an s orbital, l=1 is a p, l=2 is a d orbital, and l=3 is an f-orbital. so, spdf. Btw, we get the l from the n or the shell number and l always is less than n. So for n=2 , for instance, l= 0,1. To find the number of orbitals, find the ml number which is just, (l, l-1, and -l) which gives you the "range of values" your orbitals can be. So for l=2, a d-orbital we have ml =(2,1,-2), so a range of (-2,-1, 0, 1, 2). Therefore, it has 5 orbitals!
-
- Posts: 116
- Joined: Wed Sep 30, 2020 9:37 pm
Return to “Wave Functions and s-, p-, d-, f- Orbitals”
Who is online
Users browsing this forum: No registered users and 6 guests