I was solving questions about writing the quantum numbers of the last electron of an element.
For Ions like Na+ , Na , O , Cl it was easy.
But for elements like Scandium , Yttrium , Iron I am having difficulty.
Electronic configuration respectively of each element = $3d^1$ $4s^2$ , $4d^1$ $5s^2$ , $3d^6$ $4s^2$.
Now, according to the answer in my textbook + online I rechecked. The quantum numbers of the last electron respectively are:
- For Sc : n = 3 , l = 2 , m = -2 , s = +1/2. This clearly shows that the last electron is not of 4s orbital but of 3d. Why is it that if according to the electronic configuration , $4s^2$ is the last orbital we have written,
Similarly , for other 2 as well:
For Fe , n = 3 & not 4
For Y , n = 4 & not 5.
I couldn’t find any explanation for it but I am guessing.For example :
We can notice all these elements are exceptions to electronic configuration.
In case of Sc , d orbital is not filled & has only 1 e- but the $4s^2$ orbital is filled. Therefore , we choose the electron of 3d. But still , it is not the last electron but the 1st unpaired electron we can say.
If it is right , then in case when we have $Sc^+$. We will have outer electronic configuration = $4s^1$. In this case , which electron would we choose
The 3d orbital or 4s ?
To brief my questions:
Why is the set of quantum numbers in case of elements like Sc,Fe,Y are different to write than Na,O,Na+.
What is the reason for such thing to happen?
I have made a guess above which is not theoretical but mathematical , if that guess is correct. How would we write set of quantum numbers for $Sc^+$.