Electrons occupying a subshell  [ENDORSED]

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Electrons occupying a subshell

Postby 804991762_4A » Sun Apr 29, 2018 11:33 pm

How can you find how many electrons can occupy a subshell with a given value of L?

Alicia Yu 1A
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Joined: Thu Feb 22, 2018 3:02 am

Re: Electrons occupying a subshell  [ENDORSED]

Postby Alicia Yu 1A » Mon Apr 30, 2018 6:54 am

Given l (the type of subshell), you can use it to find the magentic quantum number ml=-l...0...+l. This number divides the subshell into individual orbitals (s,p,d,f) which hold the electrons; there are 2l+1 orbitals in each subshell. Thus the s subshell has only one orbital, the p subshell has three orbitals, etc.
Because each orbital can hold 2 e-, the s-orbitals can hold 2 electrons, p-orbitals can hold 6, and d-orbitals can hold 10, for a total of 18 electrons.

A general formula you can follow is 2n^2 to find the number of e- in each subshell.

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