## Formal Charge

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

Izzie Capra 2E
Posts: 103
Joined: Sat Sep 07, 2019 12:19 am

### Formal Charge

How do you recognize when an atom can have a "better" representation or more stable structure? Should you complete formal charge calculations for each structure you draw or only for atoms involving P, S and Cl?

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

### Re: Formal Charge

We should calculate the formal charge on any compound that has a resonance structure. Through this we are able to determine which of the multiple structures will be the most stable and therefore the most favorable for us. The structure that has the least amount of charged atoms and the lesser strength of charge will be the better one. Hope this helps!
Last edited by Mashkinadze_1D on Mon Oct 28, 2019 9:24 pm, edited 1 time in total.

Nyari Muchaka_Discussion 4A
Posts: 53
Joined: Thu Sep 19, 2019 12:17 am

### Re: Formal Charge

The safest bet is to do formal charge calculations for all your structures. However, this is more necessary for those atoms as they have a d-orbital, and are thus able to hold more than eight electrons versus the atoms without the d orbital who adhere to the octet rule. Any atom above period 3 has a d orbital and thus acts in the same manner as P,Cl, and S in that they can have more than eight electrons however for this class I believe we only have to be concerned with those three.

Lauren Tanaka 1A
Posts: 109
Joined: Sat Aug 17, 2019 12:18 am

### Re: Formal Charge

You should calculate the formal charge of the structures to find which structure would be the most stable. The formal charge will then tell you if the structure is stable if the number is closest to 0.

Tiffany_Chen 2K
Posts: 106
Joined: Fri Aug 30, 2019 12:15 am

### Re: Formal Charge

I would say perform formal charge calculations to structures where you are uncertain of the middle atom (such as OHCl, where formal charges can determine whether O or Cl would be in the middle).