# Chemistry

List all the quantum numbers for each of the 9 electrons in fluorine
n L m sub L m sub s
1.
2.
3.
4.
5.
6.
7.
8.
9.

1. 👍
2. 👎
3. 👁
4. ℹ️
5. 🚩
1. You need to learn to do these. Here are the rules.
n can be any whole positive number beginning with 1, 2, 3, etc.
l(ell) can be any positive whole number beginning with zero but can't be larger than n-1
ml can have values from -ell to + ell.
ms may have either of two values; i.e., +1/2 or -1/2

1. 👍
2. 👎
3. ℹ️
4. 🚩
2. What does each stand for? So if I am doing it for fluorine, what would n, l, ml, and ms represent? For instance, is n the sublevel or what? I'm rather confused.

1. 👍
2. 👎
3. ℹ️
4. 🚩
3. n is the principal quantum number and in general terms is the old Bohr shell.
l (ell) is the azimuthal quantum number and describes the ellipticity (how elliptical) of the orbit.
ml describes how the orbit is arranged in space
ms describes the spin of the electron; i.e., clockwise or counterclockwise.

1. 👍
2. 👎
3. ℹ️
4. 🚩
4. so would it be
n=4 since that is the largest outer shell
ms= + 1/2, -1/2 since it has 2 electrons in 4s but what would happen if it was 3d? Would that be times by 5?
and I'm still a little confused on what the two others represent. I'm sorry for being such a bother!

1. 👍
2. 👎
3. ℹ️
4. 🚩
5. I think your part way there but I don't think you grasp the problem. And n =2 is the last shell of F.
First, the electronic configuration of F is 1s2 2s2 2p5. You can see from this, and the problem restates that, that there are 9 electrons in the F atom. Thr problem is asking you to show all four quantum numbers for EACH electron. So for the 1s2 electrons,
n = 1
ell = 0
Mell = 0
Ms = +1/2 for 1 electron and -1/2 for the other. This completes n,l,ml and ms for the 1s2 electrons.

Next shell is n = 2
So for the 2s2 electrons you have
n = 1
ell = 0
Mell = 0
Ms = +1/2 for 1 electron and -1/2 for the other.

In the same n = 2 shell, there are 5p electrons in addition to the 2s electrons.
These 5 p electrons will have different quantum numbers. No two electrons can have the same four quantum numbers in the same atom. If they are paired up (as in the 1s2 and 2s2 levels) they will have the same n,l and ml, but the ms values will be different (one electrons is +1/2 and the other electron is -1/2)
So the frst p electron will have
n = 2
ell = 1 (we've used zero already) and it can't have anything larger than 1 because of the n-1 rule)
Mell = -1, or 0, or +
Ms can have +1/2 or -1/2 for each of these. You can draw those 5 electrons individually if you wish. Hope this helps.

1. 👍
2. 👎
3. ℹ️
4. 🚩
6. This post has gotten pretty far down the list and I may not see it by tomorrow. If you're still confused please post a new question at the top of the page.

1. 👍
2. 👎
3. ℹ️
4. 🚩
7. Thank you so much for your help. It means the world!

1. 👍
2. 👎
3. ℹ️
4. 🚩

## Similar Questions

1. ### Chemistry

How many electrons can be described by the quantum numbers n = 2, l = 1, ml = -1? a.) 2 b.) 14 c.) 6 d.) 10 e.) 0 I thought it was 6 but here's my reasoning n = 2 energy levels l = 1 (p orbital) ml = -1 (I don't think this is

2. ### chemistry

Suppose you take a trip to a distant universe and find that the periodic table there is derived from an arrangement of quantum numbers different from the one on Earth. The rules in that universe are: 1. principal quantum number n

3. ### Chem

What 4 quantum numbers describes one of the outermost electrons in a strontium atom in ground state? 5,0,0,1/2 Is my answer correct?

4. ### Chemistry

How many valence electrons does molybdenum have? (give only 1 answer) Go to this site and look for the electrons available in the outside shells. Click on element #42 and scroll down the menu on the left side until you come to

1. ### Chem

What is the set of quantum numbers for the last three electrons in an iodine atom?

2. ### chem

There are eight markers in a full set, but Flora and Frank each only have seven markers.Flora is missing the red marker, and Frank is missing the blue marker.What can they do so that each has a full set of markers? * steal the

3. ### Chemistry

Quantum numbers arise naturally from the mathematics used to describe the possible states of an electron in an atom. The four quantum numbers, the principal quantum number (n), the angular momentum quantum number (ℓ), the

4. ### Chem

The only stable isotope of fluorine is fluorine-19. Predict possible modes of decay for fluorine-21, fluorine-18, and fluorine-17. Would it just be alpha-particle production, beta-particle production, gamma-ray production, and

1. ### Chemistry, Periodic Table

Very brieﬂy explain the main horizontal and vertical features of the Periodic Table in terms of the electronic structure and relevant quantum numbers? -------------- Am I being asked to state for instance in the case of Halogens