## 2.27 [ENDORSED]

alexagreco1A
Posts: 34
Joined: Fri Apr 06, 2018 11:03 am

### 2.27

Write the subshell notation and the number of orbitals having the following quantum numbers:

When it asks for the number of orbitals, is that the same as asking for the number of subshells? If not, how do you solve for this?

ramayyala1G
Posts: 31
Joined: Fri Feb 02, 2018 3:02 am

### Re: 2.27

Orbitals and subshell are not the same thing. It is asking you to find the number of orbitals within the subshell. So lets look at (a). it gives you n= 5 and l=2. If n=5 you know it is on the 5th energy level and l=2 means that is it on the d-block hence 5d is the subshell notation. We know l=2 correlates to the d-block because l=1 is the s-block and l=0 is the p-block. In order to find the number of orbitals, the easiest thing to do is understand that the d-block as 10 electrons meaning that it will have 5 orbitals. Just count the number of elements on the period table in one row of the d block. There is 10 elements meaning that there is 10 electrons to fill in the d-block. Divide the 10/2 to get 5 orbitals.

victoriatanaka1C
Posts: 38
Joined: Fri Apr 06, 2018 11:05 am

### Re: 2.27

Orbitals and subshells are not the same thing!

Shells are determined by the value of n.

Subshells are determined by the value of l (which can go from 0 to the value of n-1).

Orbitals are determined by the value of m (which are valued between l and -l).

So if you're given n = 4 and l = 1, m can be 1, 0 or -1.

Chem_Mod
Posts: 18161
Joined: Thu Aug 04, 2011 1:53 pm
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### Re: 2.27  [ENDORSED]

I just want to correct a portion of Ramay's response. l=0 is the s orbital and l=1 is the p orbital.

Katie_Duong_1D
Posts: 69
Joined: Fri Sep 28, 2018 12:27 am

### Re: 2.27

In sub shell notation, n refers to the coefficient.

For example,

a. n = 5, l = 2 would be 5d. This is because n=5, so the coefficient would be 5, and l = 2 corresponds with d. There are 5 possible electrons with that quantum number because l=2, so the possible electrons would be -l and +1 (-2, -1, 0, 1, 2)