Page 1 of 1

### Text Book Problem 2.29 (d)

Posted: Tue Jul 11, 2017 3:39 pm
How many electron can have the following quantum numbers in an atom:
n=2

To find 'l' you use (n-1) which gives you "1" that makes it a p-orbital (0,1). 'ml' is -1,0,1. That means that there are 6 electrons that can have that quantum number. But the book answer says there are 8 electrons. How is it 8 electrons?

### Re: Text Book Problem 2.29 (d)

Posted: Tue Jul 11, 2017 3:49 pm
The question is asking about how many electrons can have the quantum number of n=2, meaning the 2nd shell. Since the 2nd shell possesses only s and p subshells, those subshells are the only ones that can have the number n=2. We learned that s- subshells have one orbital and that each orbital can hold up to two electrons (Pauli Exclusion Principle). Furthermore, the p- subshell has 3 orbitals that can hold up to 2 electrons each, producing 6 electrons. With 2 electrons in the 2s subshell and 6 in the 2p subshell, the answer is 8.

### Re: Text Book Problem 2.29 (d)

Posted: Tue Jul 11, 2017 4:06 pm
It's 8 because n = 2 is s & p orbitals
s can hold 2 + p can hold 6 = 8

### Re: Text Book Problem 2.29 (d)

Posted: Tue Jul 11, 2017 4:20 pm
I see. So if you're given the quantum number "l" like in problem "a" then there would be 6 electron because it specifically asks for that orbital?