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### Course: MCAT > Unit 8

Lesson 23: Electronic structure- Electronic structure questions
- Photoelectric effect
- Bohr model radii (derivation using physics)
- Bohr model radii
- Bohr model energy levels (derivation using physics)
- Bohr model energy levels
- Absorption and emission
- Emission spectrum of hydrogen
- Heisenberg uncertainty principle
- Quantum numbers
- Quantum numbers for the first four shells
- Electron configurations for the first period
- Electron configurations for the second period
- Electron configurations for the third and fourth periods
- Electron configurations of the 3d transition metals
- Paramagnetism and diamagnetism
- Electron configurations article

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# Quantum numbers for the first four shells

Calculates number of orbitals and number of electrons in different kinds of orbitals for n = 1 to 4. Explains that only two electrons are allowed per orbital, and gives shortcuts for calculating number of orbitals and total number of electrons for a given n. Created by Jay.

## Want to join the conversation?

- Are orbitals and sub shells the same?(19 votes)
- They are not same. Sub-shell is the l value (Azimuthal Quantum No.) e.g. s, p, d, f, etc, whereas oribitals are within the subshell with same n (Principal Quantum No.) and l. Example: 2py is an orbital in the p subshell.

But generally, they are used synonymously.(36 votes)

- Can the number of electrons in an orbital be increased?or does it just have to be 2?(13 votes)
- Two is maximum number of electrons in an orbital, because the electrons repel each other. If you try to put three electrons in an orbital, the atom wouldn't be stable.(26 votes)

- when electrons are in orbitals, then possess a charge which is cancel out so why they do not slam with nucleus?(8 votes)
- Excellent question. The electron would collapse into the nucleus if we applied classical electrodynamics. This was one of the central problems which quantum mechanics solved. With quantum mechanics, the motion of the electron is replaced with a wave function as described by Schrodinger's equation and solutions to that equation result in quantized energy states that the electron can occupy, and none of those states allow for the electron to collapse into the nucleus due to the boundary conditions required for the wave function to exist.(11 votes)

- I've learned that the formula to determine the no. of elecrons in each shell-2n^2 is only applicable till the elements having atomic no. 20. It was given by Bohr and was proved incorrect. But here, in the video, it seems to be fully correct. I'm confused. Please explain.(8 votes)
- That formula represents the maximum number of electrons per shell, NOT the actual number in any element's particular shells. Most notably, there is no element massive enough to have more than 32 electrons in any of its shells, even though, hypothetically, shells beginning with shell 5 could have more than that number of electrons.

Shells 1 and 2 fill up completely before any higher shells begin filling, but that is not the case thereafter. Starting with scandium, the electrons fill in complicated ways, with higher numbered shells beginning to fill before lower numbered shells are complete.(13 votes)

- how dose the d and the f orbital look like?(10 votes)
- d-orbital looks like a double-dumbbell

f-orbital looks like a triple-dumbbell

Check this out:http: //http://www.angelfire.com/falcon2/dirgni/orbitals.html(4 votes)

- please tell me if i am right or wrong...

every orbital can hold only 2 electrons. and one of the electrons have up spin and the other down spin.

and the number of orbitals in a shell is given by n^2 where n is the shell number.(4 votes)- Yes, everything you said is correct. Although, strictly speaking, "spin up" and "spin down" are not official terms.

However, beginning with shell n=3, the shells do NOT completely fill up before the next higher shell begins to fill.

NOTE: there is no element with a large enough atomic number to contain more than 32 electrons (16 orbitals) in any shell. The higher level orbitals (g, h, etc.) do exist but only as excited states. The first theoretical element that would be predicted to have an electron in a g orbital would be Element-125, which does not exist in nature and we do not current know whether it is even possible to make artificially.

So, in summary, although shells 5 and above theoretically could have electrons in 25 or more orbitals, there is no known element that is massive enough for this to actually happen.(9 votes)

- I'm a little confused on the orbitals an atom has as we increase in n shells.

Do, the s,p,d,f, orbitals DIFFER as we go from shell to shell? (I was thinking yes since as 'n' increases we have bigger radius so 's' orbital in n=1 is smaller than 's' orbital in n=2)

Also lets say we took an atom that had n=3. Does that mean it has orbitals of only those in n=3 or does that INCLUDE all the orbitals from n=1 and n=2? (i.e. sulfur atom has a total of 14(1+4+9) different orbitals in which you can find electrons?(7 votes)- Your both ideas are correct. The s orbital in the first shell has a smaller radius than the s orbital in the second shell, and so on (it is valid for all of the orbitals). An atom can have a lot of orbitals (it just depends on its number of electrons), so, if you have three shells in the atom, you're gonna have all the orbitals from n=1 to n=3, because each electron will be in a specific orbital.(3 votes)

- I've not found this anywhere else, so I doubt if it even exists....But are there subshells after 'f' and correspondingly are values of L>3 posiible?(3 votes)
- Yes and No.

There is no element massive enough to have an electron in the g or higher subshell in its ground state. The first element (should it be possible to create it artificially) predicted to have a ground state g subshell with an electron in it would be Element 125.

However, in excited states a lighter element can have an electron in a g or higher subshell. So, in that sense, there is such a thing as a g subshell and higher.(6 votes)

- could you please explain the shape of p and d orbitals because its not explained very well and i could not understand it(2 votes)
- We usually describe a p orbital as being dumbbell shaped.

I usually say that four of the d orbitals look like four-leaf clovers and the fifth one looks like a big p orbital with a doughnut around its middle.

Remember that the orbitals are 3-dimensional in shape.

Go to

http://winter.group.shef.ac.uk/orbitron/AOs/2p/index.html

and

http://winter.group.shef.ac.uk/orbitron/AOs/3d/index.html

to see their computer-generated shapes.(5 votes)

- why can we fit only 2 electrons in one orbital (1:55)?(1 vote)
- The Pauli exclusion principal states no two particles with identical quantum properties can occupy the same space.

Electrons share identical properties with other electrons. The only property they can differ by is quantum spin, which they can be either spin up or spin down. So, if you have an electron in a orbital, the only way another electron can occupy the same orbital is if it has an opposite spin at which point, no other electrons can occupy that orbital.

https://www.khanacademy.org/science/physics/quantum-physics/quantum-numbers-and-orbitals/v/quantum-numbers(7 votes)

## Video transcript

- Now that we understand the four quantum numbers, let's get some more practice using the quantum numbers and thinking about the first four shells, the first four energy levels. So we'll start with n is equal to one. So when n is equal to one, the principle quantum
number is equal to one, we're talking about the first energy level or the first shell. The angular momentum
quantum number depends upon the principle quantum number and so when n is equal to one, let's think about the allowed values for l. So l goes from zero, one and all the way up to n minus one. Well n minus one, if n is equal to one and minus one, one minus
one is equal to zero and so that's the only allowed value for the angular momentum quantum number. And we know l is equal to zero refers to an s orbital. So we're talking about an s orbital here. Alright, the next quantum number is the magnetic quantum number. So ml. So the magnetic quantum number depends on the angular
momentum quantum number and it goes from negative l to positive l. So if l is equal to zero, we only get one value for the magnetic quantum number. If l is equal to zero, the only possible value we could get is zero. And remember, this tells
us the orientation. So we only have one possible orientation. We have only one s orbital. So there's an s orbital, there's only one of them here. We know an s orbital is
shaped like a sphere. So remember, an orbital is the region where you're most likely
to find an electron here. So there's a total of one orbital in the first energy level and you could have gotten that by using n squared. So when n is equal to one, one squared is equal to one, that's the total number of orbitals that you're going to find in
the first energy level here. Let's move on to electrons in the orbital. So you can fit a maximum of two electrons in one orbital. So the fourth quantum number, alright, the fourth quantum number says, the spin of an electron
can either be positive one half or it can be negative one half. And so if you have two electrons in one orbital, one electron has to spin a positive one half and one electron has a spin of negative one half. So there's a maximum of two electrons in one orbital, we have a maximum of two electrons in this one s orbital in the first energy level. And since that's the only orbital in this energy level or this shell, that's also the total number
of electrons in the shell. So the total number of electrons is equal to two. And you could have gotten
that using two n squared. So if n is equal to one, so one squared is equal to one times two
which is equal to two. So that's the first energy level or the first shell. Let's move on to the second shell. So this is where n is equal to two. So if n is equal to two, the principle quantum
number is equal to two, the angular momentum quantum number, what are the allowed values? Well you start with zero and you go all the way up to n minus one. So we start with zero, n minus one, that would be two minus
one, that would be one. So we go from zero and then we go to one and then we have to stop. So we have only two allowed values for the angular momentum quantum number. So if you have n equal to two, you get two allowed values here. We already talked about what l is equal to zero means, l is equal to zero refers to an s orbital. And there's one s orbital. So in the second energy level, there's another s orbital. This is different from the s orbital in the first energy level that we just talked about. So there's another s orbital here. It too is shaped liked a sphere. What I drew here is misleading. I drew this as being a little bit smaller then the one before. Remember, when n is equal
to two, you're further away. You're electron is on average further away from your nucleus here, l is equal to one so if l is equal to one, what is the allowed values for the magnetic quantum number? So remember, the magnetic quantum number goes from negative l to positive l. So negative l would be negative one, and then we include zero and then we go to positive one. So there are three possible values for the magnetic quantum number. One, two, three, the
magnetic quantum number told us the orientation so there are three different orientations. And we talked about l is equal to one is referring to a p orbital which is shaped like a dumbbell. So we have three different orientations, we have three different p orbitals in the second energy level. One of them goes along the x-axis, one of them the y and one of them the z. So we talked about this
in the previous video. So a total of three p orbitals here. So how many orbitals are there in the second energy level? Well we have one s orbital
and three p orbitals. So one plus three gives us four. We could have done this math, n squared, so two is n squared which gives us four. Alright, let's do electrons now. So four, let's go back
to the s orbital here. Remember, there's one orbital so we can fit a maximum of two
electrons in one orbital. For the p orbitals, we
have three p orbitals. If each p orbital's holding a maximum of two electrons, three times two gives us six, so we have a total of eight electrons in the
second energy level. So eight electrons and we can get that from two n squared again right? Because if n is equal to two, square that and you get four, multiply that by two and you get eight. Alright, let's go to
the third energy level or the third shell here. So when n is equal to three what are the allowed values for the angular momentum quantum number l? So remember l goes from zero all the way up to n minus one. So l goes from zero all
the way to n minus one. So l is equal to zero, l is equal to one and l is equal to two
because three minus one is equal to two, so if we
have n is equal to three, we have three possible values for l. Zero, one and two. We already talked about what l is equal to zero means, l is equal to zero is an s orbital and there's one of them, l is equal to one is a p orbital and with three allowed values for the magnetic quantum number, we can have three p orbitals in the third energy level. So let's focus in on l is equal to two. So when l is equal to two, what are the allowed values for the magnetic quantum number? Well those go from
negative l to positive l. So if l is equal to two, let me use a different color here. So if l is equal to two, we could go negative two, negative
one, zero, one and two. So that's a total of
one, two, three, four, five, five values. So five different
orientations for this orbital and when l is equal to two, we call this a d orbital. So five different orientations so five d orbitals. So I'm going to write a five here. So the total number of
orbitals that we have in this energy level, that would be one plus three plus
five and so that's nine which we could have
gotten from three squared. So the total number of
orbitals equal to n squared, if n is equal to three,
three squared gives us nine. Alright, how many electrons can we fit in each one of those orbitals? Well, let me once again
use a different color. So we have the s orbital,
we have one of those, so we can fit a maximum of two electrons into that s orbital. For the p orbitals in
the third energy level, we have three of them, so
each one of those orbitals could fit a maximum of two. So three times two gives us six and then we go to the d orbitals. Alright, so five orbitals. Each one can hold a
maximum of two electrons so five times two gives us ten. So what's the total number of electrons that we can fit in this third shell here? So that would be two plus six plus ten, that's 18. Alright and again, we could have used this little formula over here. So two n squared, so
if n is equal to three, square that that's nine
times two, this gives us 18. Alright, let's do one
more and before I do that, we already talked about the shape of an s orbital, we talked about the shape of a p orbital, when you get in to things like d orbitals, you
start to get a little bit complicated and it's a little bit tricky for me to draw. So I'm not going to attempt do draw all the d orbitals in the five different orientations,
so let's just move on to n is equal to four. I went ahead and rewrote
what we were going for here. So we're going to go for n, so we're going for n is equal to four now, n is equal to four. What are the allowed values for l? So that's zero all the
way up to n minus one. So l is equal to zero, l is equal to one, l is equal to two and then n minus one, that's four minus one,
that's equal to three. So that's the last allowed value for l, the angular momentum quantum number. And once again, if you have four here, you get four allowed values. Alright, when l is equal to zero, we said that's an s orbital. When l is equal to one, we
said that was a p orbital. When l is equal to two, we call that a d orbital and when l is equal to three, we're going to call this an f orbital. And s, p, d and f come from old nomenclature used in atomic spectroscopy and so it's kind of... It's not really used anymore but like the s, I think, used to stand for sharp and so that's where your
letters come from here. We used them to think about the orbitals and the different shapes here. So an s orbital is shaped like a sphere, we know we have one of those. A p orbital is shaped like a dumbbell, we know we have three of those. D orbitals, we just talked about the fact that we have five of them. So five different
possible values here fore the magnetic quantum number. So we have five d orbitals in the fourth energy level and then finally f alright? So an f orbital when l is equal to three, what are the allowed values for the magnetic quantum number? So ml, so what are the allowed values? Well they go from
negative l to positive l. So if l is equal to three, I'm going to use a different color. If l is equal to three we could get negative three, negative
two, negative one, zero, one, two and three. So how many different orbitals are we talking about now. That would be one, two, three, four, five, six, seven. So seven f orbitals in
the fourth energy level. Alright, maximum number of
electrons in the orbital. We have only one. Let me use, what color should I use here? Let's use magenta. So I have one s orbital,
maximum two electrons. So two electrons here. Three p orbitals, two times three is six. Five d orbitals in the fourth shell or the fourth energy level, so five times two gives us ten. And then we just talked about f orbitals which would be way too difficult for me to draw so you can get some nice pictures of f orbitals online or in your textbook here. So if we have seven f orbitals, seven times two gives us a total of 14, so we could have a maximum of 14 electrons in the f orbitals. Alright, what's that total? So we add all those up. So two plus six plus
ten plus 14, that's 32. So there's 32 electrons
in the fourth shell, in the fourth energy level and once again, we could have used our formula here. So two n squared, so
when n is equal to four, we square that and we get 16, we'll divide that by two and we get 32. And so hopefully this give you some experience playing with
the quantum numbers. So you have to be, this
is a very useful exercise. So just sit down and think about how the quantum numbers
depend on each other. So l depends on n and ml, the magnetic quantum
number depends on this. And so it's going to allow you to understand the periodic table and electron configurations.