## Electron Configurations

Posts: 72
Joined: Wed Sep 18, 2019 12:18 am

### Electron Configurations

Hi can somebody please explain to me how you know the order when writing an electron configuration? For example, 1s, 2s, 2p....Is there a trick to remember the order? Also, how do you know how many electrons will fit in that orbital? Let me know if I have to clarify any parts of the question. Thank you :)

Posts: 87
Joined: Sat Aug 24, 2019 12:15 am

### Re: Electron Configurations

Hello, so if we were to google the "electron configuration" there is a chart that we go by with arrows, but this is the more tedious and often confusing method to understand this. Generally the best way to understand this is all elements in groups 1-2 are s, all elements in groups 13-18 are p, all elements from 3-12 are d, and all elements from 57-80 along with 89-112 are f. Hope this helps!

Wendy 1E
Posts: 111
Joined: Sat Aug 17, 2019 12:17 am
Been upvoted: 2 times

### Re: Electron Configurations

As to your question on how many electrons will fit into a specific orbital, each orbital consists of two electrons. There is one s-orbital, thus there are 2 electrons in the s-sublevel. There are 3 p-orbitals, thus there are 6 electrons in the p-sublevel (3 p-orbitals* 2 e- per orbital). There are a total of 5 d-orbitals, thus there are 10 electrons in the d-sublevel. There are a total of 7 f-orbitals, thus there are 14 electrons in the f-sublevel.

Emma Popescu 1L
Posts: 105
Joined: Wed Sep 11, 2019 12:16 am

### Re: Electron Configurations

Eunice Nguyen 4I
Posts: 100
Joined: Sat Aug 17, 2019 12:17 am

### Re: Electron Configurations

When looking at the periodic table, you kinda just go left to right and then down to the next row. The first two elements of each row on the left will be s, and the last 6 of the row are going to be p (except for the first row which is just 1s2 in total). You just go 1s2,2s2,2p6,3s2,3p6,... and so forth :) but then after the 3rd row, you'll also hit the d-block, which goes up to xd10 (x being row number-1).

### Who is online

Users browsing this forum: No registered users and 1 guest