Question 2.19 part b and c [ENDORSED]

[jillianduffield_2D]

2.19
b) How many values of m sub l are allowed for an electron in a 6d-subshell?
c) How many values of m sub l are allowed for an electron in a 3p-subshell?
I am confused on how to get the answers to these questions

[Brandon_Phan_3J]

b) The relationship between the angular momentum quantum number (L) and the magnetic quantum number (m sub L) is that m sub L can take on values of L, L-1,..., -L. Since the question is asking for m sub L values for an electron in a 6d subshell, that would mean that L=2. Because we know that L=2, we can say that the values m sub L can have are: -2, -1, 0, 1, and 2.

c) The same thing applies for this question. The question is asking for m sub L values for an electron in a 3p subshell so that means L=1. Since L=1, we can say that m sub L can have the values of -1, 0, 1.

Hope this helps!

[isabelle ruedisueli 1j]

Hi. Could someone also explain 2.17? It reads: How many orbitals are in subshells with l equal to (a) 0; (b) 2; (c) 1; (d) 3?

[Shushanna S 3F]

For #19, one thing you need to know is that n (principle quantum number) = shell, l (angular momentum quantum number) = subshell, and that m sub l (the magnetic quantum number)=orbital. You know that m sub l = l, l-1,... -l. Using the value of l, you find the values of m sub l and count how many values there are. That's how you get the answer.

I hope this helps.

[isabelle ruedisueli 1j]

Yes! Thanks so much for your help :)

[Jineava_To_3N]

What exactly does it mean when m sub l is -2, -1, 0, 1, 2 compared to when m sub l is -1, 0, 1 for when l=1?

[Lauren_Bui_1A]

When m sub l is -2, -1, 0, 1, 2, l=2 which are the d-orbitals.
m sub l for when l=1 are the p-orbitals.