## 2.19 Part B

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### 2.19 Part B

Can someone please explain part b of 2.19?
How many values of m1 are allowed for an electron in a 6d-subshell?
Thank You

Laura Riccardelli
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Joined: Fri Sep 29, 2017 7:04 am

### Re: 2.19 Part B

I was also a little confused by this question but I believe that because it is talking about "d" orbitals which can have 5 different lobes each lobe can have a different sub-shell value so their would be 5 possible ml or sub-shell values.

Justin Chu 1G
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### Re: 2.19 Part B

That is correct. For the d-orbital, you can have 5 different numbers for your magnetic quantum number, specifically -2, -1, 0, 1, 2.

MichelleKaku1H
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### Re: 2.19 Part B

Justin Chu 1C wrote:That is correct. For the d-orbital, you can have 5 different numbers for your magnetic quantum number, specifically -2, -1, 0, 1, 2.

Can someone please explain how you get the magnetic quantum numbers of -2, -1, 0, 1, 2?

Justin Chu 1G
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### Re: 2.19 Part B

MichelleKaku1H wrote:
Justin Chu 1C wrote:That is correct. For the d-orbital, you can have 5 different numbers for your magnetic quantum number, specifically -2, -1, 0, 1, 2.

Can someone please explain how you get the magnetic quantum numbers of -2, -1, 0, 1, 2?

So basically for the magnetic quantum number, you can have values of l, -l, and everything in between. So for d-orbital, since l=2, you can have values of 2, 1, 0, 1, and -2. For p-orbital (l=1) you can have 1,0,-1. For l=0 (s-orbital) you can only have 0. F-orbital (l=3) can have 3,2,1,0,-1,-2,-3.

Gabriela Carrillo 1B
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### 2.43 part e

What is the ground sate electron configuration for (e) tungsten??
I understand that you start with [Xe] but I'm lost on how the 4f^14 5d^4 6s^2 was attained
First of all will d-block n value always be one less than that of s block???
Secondly, do we plug in the f-block to the periodic table to get the 4f^14 value??