In my textbook, it states that the maximum number of electrons that have the right to fit in any kind of given covering is provided by 2n². This would average 2 electrons might fit in the very first shell, 8 can fit in the 2nd shell, 18 in the 3rd shell, and 32 in the fourth shell.

However, i was formerly taught that the maximum number of electrons in the an initial orbital is 2, 8 in the 2nd orbital, 8 in the third shell, 18 in the fourth orbital, 18 in the 5th orbital, 32 in the sixth orbital. I am reasonably sure the orbitals and also shells space the exact same thing.

Which of this two techniques is correct and should be supplied to find the number of electrons in an orbital?

I am in high college so please try to simplify your answer and also use reasonably basic terms.

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Melanie Shebel♦
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Shells and also orbitals space not the same. In regards to quantum numbers, electrons in different shells will have various values of principal quantum number n.

To answer your question...

In the first shell (n=1), us have:

The 1s orbital

In the 2nd shell (n=2), us have:

The 2s orbitalThe 2p orbitals

In the 3rd shell (n=3), us have:

The 3s orbitalThe 3p orbitalsThe 3d orbitals

In the fourth shell (n=4), we have:

The 4s orbitalThe 4p orbitalsThe 4d orbitalsThe 4f orbitals

So one more kind that orbitals (s, p, d, f) becomes obtainable as us go to a covering with greater n. The number in former of the letter signifies which shell the orbital(s) are in. Therefore the 7s orbital will be in the 7th shell.

Now because that the different kinds of orbitalsEach kind of orbital has actually a various "shape", together you have the right to see on the photo below. Friend can additionally see that:

The s-kind has only one orbitalThe p-kind has actually three orbitalsThe d-kind has five orbitalsThe f-kind has seven orbitals

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Each orbital deserve to hold two electrons. One spin-up and also one spin-down. This method that the 1s, 2s, 3s, 4s, etc., can each organize two electrons because they each have actually only one orbital.

The 2p, 3p, 4p, etc., have the right to each host six electrons since they each have actually three orbitals, that deserve to hold two electrons every (3*2=6).

The 3d, 4d etc., have the right to each organize ten electrons, since they each have actually five orbitals, and each orbital have the right to hold two electrons (5*2=10).

Thus, to discover the variety of electrons feasible per shell

First, we look at the n=1 covering (the an initial shell). That has:

The 1s orbital

An s-orbital hold 2 electrons. Hence n=1 shell deserve to hold 2 electrons.

The n=2 (second) covering has:

The 2s orbitalThe 2p orbitals

s-orbitals deserve to hold 2 electrons, the p-orbitals deserve to hold 6 electrons. Thus, the second shell deserve to have 8 electrons.

The n=3 (third) covering has:

The 3s orbitalThe 3p orbitalsThe 3d orbitals

s-orbitals deserve to hold 2 electrons, p-orbitals have the right to hold 6, and also d-orbitals deserve to hold 10, because that a full of 18 electrons.

Therefore, the formula $2n^2$ holds! What is the difference in between your 2 methods?

There"s an essential distinction in between "the variety of electrons feasible in a shell" and "the variety of valence electrons possible for a duration of elements".

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There"s an are for $18 \texte^-$ in the third shell: $3s + 3p + 3d = 2 + 6 + 10 = 18$, however, aspects in the third period only have up to 8 valence electrons. This is due to the fact that the $3d$-orbitals aren"t filled till we gain to elements from the 4th period - ie. Elements from the third period don"t to fill the third shell.

The orbitals are filled so that the persons of lowest energy are filled first. The power is approximately like this: