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### 1D 11

Posted: Tue Oct 15, 2019 5:58 pm
I am struggling with this problem. Can someone explain how to find the orbitals in subshells and what the differences are between l, m, and n?

"How many orbitals are in subshells with l equal to (a) 0; (b) 2; (c) 1; (d) 3? "

### Re: 1D 11

Posted: Tue Oct 15, 2019 6:36 pm
I just try to memorize the what orbitals each l value corresponds to. l=0 is a s-orbital, l=1 is a p-orbital, l=2 is a d-orbital, and l=3 is for f orbital. S-orbitals have 1 orbital, p orbitals have 3 orbitals, d-orbitals have 5, and f-orbitals have 7.

### Re: 1D 11

Posted: Tue Oct 15, 2019 6:56 pm
l, which is the angular quantum number, represents the shape of the orbital.
m shows the number of orbitals in a sublevel. For example, m=-1,0,+1 shows that there is 3 orbitals in the p sublevel.
n is the energy level of the orbital.

### Re: 1D 11

Posted: Wed Oct 16, 2019 2:10 pm
n is the principal quantum number that represents energy. Its values can be anything greater than one.

l is the angular momentum quantum number, and it describes shape. Its values can be anything from 0 to n-1.
0 represents the s subshell.
1 represents the p subshell.
2 represents the d subshell.
3 represents the f subshell, and so on.

ml is the magnetic quantum number that represents orientation, and its values can range from -l to l. It represents the different orbitals in a subshell.

To answer the question, look at the quantum number l.
a) 0 - this represents s so there is one orbital.
b) 2 - this represents d so there are five orbitals.
c) 1 - this represents p so there are three orbitals.
d) 3 - this represents f so there are seven orbitals.

### Re: 1D 11

Posted: Wed Oct 16, 2019 2:23 pm
Just remember that the values of m and l are related. The values of m range from l, l-1, ..., -l. When asking about orbitals, you want to think about the m value. So if l =0, you can only have one orbital. If l=1, you can have 3 orbitals. When l=2, you can have 5 orbitals. When l=3, you can have 7 orbitals.