## Formula Provided

$FC=V-(L+\frac{S}{2})$

ZachMoore1C
Posts: 30
Joined: Fri Apr 06, 2018 11:04 am

### Formula Provided

Will the formula be provided for formal charge on the next test or is that something we ought to just have memorized?

Elizabeth Parker 1K
Posts: 33
Joined: Wed Nov 15, 2017 3:00 am

### Re: Formula Provided

I'm not sure if it will be provided but I would memorize it just in case. Formal charge = [# of valence electrons] – [electrons in lone pairs + 1/2 the number of bonding electrons]

sharonvivianv
Posts: 63
Joined: Fri Apr 06, 2018 11:05 am

### Re: Formula Provided

There is also an easier way to tell. If you get the number of valence electrons and subtract the electrons "directly surrounding it", you will find the formal charge.

Ex: CH4
C: 4 valence electrons - 4 electrons around it = 0
H: 1 valence electron - 1 electron around it = 0
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ZachMoore1C
Posts: 30
Joined: Fri Apr 06, 2018 11:04 am

### Re: Formula Provided

Thank you!

Johanna Caprietta 1E
Posts: 30
Joined: Fri Apr 06, 2018 11:02 am

### Re: Formula Provided

Just a follow-up question. What is the importance of the formal charge when it comes to drawing a Lewis structure?

Mariah Guerrero 1J
Posts: 32
Joined: Fri Apr 06, 2018 11:03 am

### Re: Formula Provided

Formal charge can be used to determine if a structure is stable. In drawing lewis structures for tests, the correct answer would be a lewis structure of a molecule with the formal charge of 0 (or close to zero).

Kara Justeson 1B
Posts: 31
Joined: Fri Apr 06, 2018 11:03 am

### Re: Formula Provided

In response to the question right above this one, the formal charge also lets you know which structure would be correct since there as sometimes multiple ways you could draw the structure. Since the correct structure is the one thats the most stable (or with the formal charge they give you in that instance), you can calculate the formal charge to make sure you're answering with the right one.