A) n=1 l=0 ml=0 ms=1/2
B) n=3 l=1 ml=-1 ms=1/2
C) n=2 l=0 ml=0 ms=-1/2
D) n=2 l=1 ml=0 ms=1/2
E) n=3 l=2 ml=0 ms=1/2
F) n=2 l=1 ml=1 ms=-1/2
Which of the above sets of quantum numbers could possibly describe an electron in the ground-state configurations of sulfur
16S = 1s2 2s2 2p6 3s2 3p4
What is it about this that you don't understand? Here are the rules.
n can be any whole number starting with 1.
l can be any whole number less than n-1.
ml can be -ell to +ell including 0.
ms can be either +1/2 or -1/2.
What I don't get is how do i determine the quantum numbers that match up with S's electron configuration
OK. Let's look at the two 1s electrons.
Remember those configurations give you n and l.
So for 1s2 n must be 1 and s electrons have ell = 0 and the two electrons of 1s2 can have +1/2 and other one -1/2
Therefore, one electron has
n = 1, l = 0 mL = 0 (see the rules;; i.e., since l = 0 then mL can be -l to +l incl 0 and in this case 0 is the only choice), then ms = +1/2
The other one of the pair is
n = 1, l = 0, ml = 0 and ms = -1/2.
For the 2s2.
n = 2, s means l = 0, ml = 0 and ms = +1/2 and =1/2.
You go through the electron progression just as I've done for the 1s2 and 2s2 but you cover the others. Remember the code: s means l = 0, p means l = 1, d means l = 2 and f means l = 3
I'll be glad to check your work if you want to post it.
A appears to be a choice. E can't be a choice because for l to be 2 we must have a d electrons and there aren't any d electrons in Sulfur. I'll be happy to answer any further questions. This can be very confusing; that's why you need to follow the rules.
To determine which set of quantum numbers could possibly describe an electron in the ground-state configuration of sulfur, we need to consider the allowed values for each quantum number.
The quantum number "n" represents the principal quantum number, which determines the energy level or shell of the electron. In the ground-state configuration, the electron occupies the lowest available energy level, so "n" should be the smallest possible value. Looking at the given set of quantum numbers, the only one with n=1 is A.
The quantum number "l" represents the azimuthal quantum number or the orbital angular momentum quantum number. It determines the shape of the orbital. The value of "l" ranges from 0 to (n-1), where n is the principal quantum number. For sulfur, which has atomic number 16, the ground-state electron configuration is 1s^22s^22p^63s^23p^4. In this configuration, there are electrons in the 1s, 2s, 2p, and 3s orbitals. So, the possible values for "l" in sulfur's ground-state configuration would be 0, 1, or 2. Looking at the given set of quantum numbers, B, D, and F have the correct values for "l".
The quantum number "ml" represents the magnetic quantum number, which determines the orientation of the orbital in space. The range of "ml" values depends on the value of "l" and can span from -l to +l, including zero. Looking at the given set of quantum numbers, all of them have ml values within the appropriate range for their corresponding l values.
The quantum number "ms" represents the spin quantum number, which describes the direction of electron's spin. The possible values for "ms" are +1/2 or -1/2. Looking at the given set of quantum numbers, all of them have ms values of ±1/2.
Based on the analysis above, the sets of quantum numbers that could possibly describe an electron in the ground-state configurations of sulfur are B) n=3, l=1, ml=-1, ms=1/2, and D) n=2, l=1, ml=0, ms=1/2.