What is the maximum number of electrons that can have n 4 L 2 and ML 1 in an atom?

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Johana Jeon 1A Posts: 30 Joined: Sun Feb 12, 2017 3:00 am

Postby Johana Jeon 1A » Thu Jun 29, 2017 9:47 pm

For Exercise 2.29 (Chapter 2 The Quantum Mechanics in Action: Atoms)How many electrons can have the following quantum numbers in an atom:a) n = 2, l = 1b) n = 4, l = 2, ml = -2c) n = 2d) n = 3, l = 2, ml = +1Does anyone know how to solve this problem?

Thank you in advance

Chem_Mod Posts: 21504 Joined: Thu Aug 04, 2011 1:53 pm Has upvoted: 1139 times

Postby Chem_Mod » Fri Jun 30, 2017 9:42 am

I will cover this in class in detail. This question is about 20 pages ahead of what we have covered.

derek1d Posts: 19 Joined: Wed Jun 28, 2017 3:00 am

Postby derek1d » Sun Jul 09, 2017 4:51 pm

For Problem 2.49"Predict the number of valence electrons present in each of the following atoms (include the outermost d-electrons: (a) N; (b) Ag; (c) Nb; (d) W."

What trend are we expected to see in order to identify the number of valence electrons? The atomic number? Is there also something else?

404768057 Posts: 20 Joined: Fri Jul 22, 2016 3:00 am

Postby 404768057 » Sun Jul 09, 2017 6:23 pm

In 2.29 part c), I don't understand why the maximum number of electrons is 8 if n=2. Can someone please explain?

104785906 Posts: 11 Joined: Wed Nov 16, 2016 3:04 am

Postby 104785906 » Mon Jul 10, 2017 7:56 pm

Chem_Mod wrote:I will cover this in class in detail. This question is about 20 pages ahead of what we have covered.

and with 2.25 which is similar and asks, "How many electrons can occupy, a) 4p-orbitals; b) 3d-orbitals; c) 1s-orbital; d)4f-orbital ?"

DavidEcheverri3J Posts: 36 Joined: Fri Sep 28, 2018 12:26 am

Postby DavidEcheverri3J » Tue Oct 23, 2018 1:34 pm

104785906 wrote:

Chem_Mod wrote:I will cover this in class in detail. This question is about 20 pages ahead of what we have covered.

I am confused with this question which asks "How many electrons can have the the following quantum numbers in an atom, a) n=2, l-1b)n=4, l=2, m1=-2c) n=2d) n=3, l=2, m1=+1 ?"

and with 2.25 which is similar and asks, "How many electrons can occupy, a) 4p-orbitals; b) 3d-orbitals; c) 1s-orbital; d)4f-orbital ?"

Andrew Lam 3B Posts: 30 Joined: Fri Sep 28, 2018 12:24 am

Postby Andrew Lam 3B » Tue Oct 23, 2018 1:59 pm

For Exercise 2.29 (Chapter 2 The Quantum Mechanics in Action: Atoms)How many electrons can have the following quantum numbers in an atom:a) n = 2, l = 1b) n = 4, l = 2, ml = -2c) n = 2d) n = 3, l = 2, ml = +1Does anyone know how to solve this problem? Thank you in advanceThe question varies in how specific the wave equation is solved to.In part a, we know the subshell in question is a 2p subshell, because n=2 and for p orbitals (l=1). We do not know which p-orbital (px,py,pz) we're speaking of,so there are 6 possible electrons that could have n=2, l=1 quantum numbers (ml and ms would make the question more specific).In Part B, we're told this time we're in the 4d subshell (n=4, l=2) but specifically the dxy orbital (ml=-2). Each orbital can hold two electrons; by Pauli Exclusion Principle they must spin in opposite directions (the last little bit is irrelevant to the question at hand).In Part C, all we know is that it is energy level 2. For all we know, it could be 2s or 2p, but between the two subshells, there are a total of 8 electrons present.

Part D can be solved the same way.

Andrew Lam 3B Posts: 30 Joined: Fri Sep 28, 2018 12:24 am

Postby Andrew Lam 3B » Tue Oct 23, 2018 2:00 pm

404768057 wrote:In 2.29 part c), I don't understand why the maximum number of electrons is 8 if n=2. Can someone please explain?

2+6=8.

Andrew Lam 3B Posts: 30 Joined: Fri Sep 28, 2018 12:24 am

Postby Andrew Lam 3B » Tue Oct 23, 2018 2:03 pm

derek1d wrote:For Problem 2.49"Predict the number of valence electrons present in each of the following atoms (include the outermost d-electrons: (a) N; (b) Ag; (c) Nb; (d) W."

What trend are we expected to see in order to identify the number of valence electrons? The atomic number? Is there also something else?

Ex: W has an electron configuration of [Kr] 6s2 4f14 5d3. The outermost valence electrons would be 6s (2) and 5d(3) for a total of 5.

Stevin1H Posts: 89 Joined: Fri Sep 28, 2018 12:17 am

Postby Stevin1H » Thu Oct 25, 2018 12:42 pm

To solve this problem, we need to know that each orbital holds 2 electrons and that ml= -l -> lSo, in this problem we are focusing on the magnetic quantum number. For example a) n=2, l=1 so ml = -1,0,1. Given that there are three orbitals in example a and that each orbital holds 2 electrons, there would be a total of 6 electrons for example a. For example b, n = 4, l=2,ml=-2. ml=-2 is the specified orbital for the quantum numbers, and since each orbital holds 2 electrons, there would be 2 electrons in the quantum numbers.

For example c, we are only given n=2. So l = 0,1. l=0 is the s orbital and l=1 is the p orbital. So for l=0 in the s orbital, ml=0. (there is one orbital so 2 electrons are present in s orbital). And for l=1, ml= -1, 0,1 (there are 3 orbitals here so there are 6 electrons in the p orbital). So when n=2, there is a total of 8 electrons present.

Bella Martin Posts: 47 Joined: Wed Sep 21, 2016 2:57 pm

Postby Bella Martin » Tue Jul 09, 2019 9:20 pm

Hello!
I'm having a bit of trouble with part D of this problem. The question states that n = 3, l = 2, and ml = +1. So from that, you are able to determine that it is the 3d orbital and ml is +1. I drew out a diagram with the different electrons in -2, -1, 0, +1, +2 sections, with up and down arrows to illustrate the spin. However, the answer key says the number of electrons in this specific atom are 2, however I calculated it out to be 4. Can anyone assist? Thank you!

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