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### Stable lewis structures

Posted: **Sun May 20, 2018 10:58 pm**

by **Husnia Safi - 1K**

So my TA mentioned something about when there is a formal charge of a -1 and a +1, a bond can be added to "even it out". Can someone explain to me why this is? Also Im not sure if I remembered this correctly so sorry if what I said is inaccurate.

### Re: Stable lewis structures

Posted: **Sun May 20, 2018 11:06 pm**

by **Chris Fults 1C**

Do you mean the way of double or triple bonds? For example in single bonded N-N there would be 6 lone pairs for each carbon which means the formal charge would be -2. If you were to triple bond nitrogen there would be 2 lone pairs and 3 shared electrons decreasing the formal charge to zero, therefore, making it more stable.

### Re: Stable lewis structures

Posted: **Tue May 22, 2018 12:19 pm**

by **Jennifer Ma 1G**

By adding another bond, you are able to make the formal charge of the molecule closer to 0, making it more stable. To help you figure out whether two atoms need another bond, just calculate the formal charge on each atom, and keep adding bonds wherever it is necessary in order to make the formal charge of the molecule the closest it can to 0, or even at 0.