Here it says give the set a full quantum numbers for the 6th electron of the oxygen atom. So here it says provide the electron orbital diagram for the element or ion. All right. So oxygen atom means oxygen is neutral. Oxygen has an atomic number of 6 here. Its electron configuration would be 1 S 2 2S22P4, filling in this electron orbital diagram 1S2SO1UP1 down to S21UP1 down.
The next 4 electrons are found within our 2P set of orbitals. Since they're all 2P electrons, they all have the same energy. So following Hun's rule, we half fill first up, up, up and here is my 7th or my 4th electron. Now Step 2. Use the number and letters for the set of orbitals to determine its N and L values. All right, so we're looking for the 6th electron. So this is 1234, half built, 1st 567, and then back around 8:00. So our 6th electron is right here.
All right, So we're going to say here that that electron that we're looking at, it is within a two set of orbitals. Because the number is 2, N equals 2. Because the letter is P, that means l = 1. Remember, if you know the sublevel letter, then you know what L is. So if it's PL. Is 1. Next, locate the specific orbital for the electron to determine its M sub L value. The electron we're looking at is in the 0 orbital that is equal to the M sub L and then finally determine if the electron spins up or spins down to determine the M sub S value it is pointing up.
That means Ms = + 12. So the four quantum numbers for the 6th electron with an oxygen would be n = 2, L equals one, M sub l = 0 and M sub s = + 12. But remember, we can't do this unless we're able to correctly number the electrons as they appear within the electron orbital diagram.