Calculating NO3- Formal Charges: Calculating Formal Charges for NO3-

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In order to calculate the formal charges for NO3- we'll use the equation

Formal charge = [# of valence electrons] - [nonbonding val electrons] - [bonding electrons / 2]

The number of valence electrons for the atom of interest is found on the Periodic Table.

Nonbonding valence electrons are those around the atom of interest that are not involved in chemical bonds (they aren't being shared with another atom).

Bonding valence electrons are the ones shared between atoms. We'll divide this number by two.

Some things to note about NO3- Formal Charges:
- Formal charge is not the actual charge. It is different from the oxidation number.
- If you can exceed the octet rule for the central atom it's a good idea to check the formal charges.
- If we have isomers or resonance -- formal charges will help us determine most stable structure.
- The closer the formal charges are to zero the more likely we have the most probable Lewis structure for the molecule.
- We write the formal charges in (). E.g. (-1)

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Seriously you are saving me right now, thank you!!

chobani

Thank you so much, I had to watch this a few times but now I understand!!!! Thanks again so very much my final is coming up and with your help I'll ace it!!!

larrainejohnson

At @1:23 you say all the N electrons are involved in a bond. But N had 5 valence electrons. Only 4 of them are involved in bonds. That should 1 as an unbonded electron.

ssarkar

If oxygen has 6 valance electrons, and one of them is shared won't it make the unshared electrons 5 instead of 6???

hermelamoges

You gained a suscriber❤
Just what i was looking for

oluwagbemigaotunaiya

The video is amazing. Now I know to find formal charges yay !
But got a doubt..
how does nitrogen has 4 bonds when it has 5 electrons ?
dont we have to consider that non bonding valence electron as 1 ?

rabiyantashi

i salute you sire, finally someone that could explain why the negative charge!!!

ISLAMguidanceful

Man …. you’re so much better than my D1 professor

stevencody

N=+1
O=-1
Why can't we move the two electrons from O to N until the charges N and O are equal to zero?

halaashraf

I am confused. I thought that the oxygen had 6 valence electrons, and to form a bond with nitrogen, it needed to use one of its valence electrons and so did nitrogen.

How can oxygen have 6 valence electrons after having a bond with nitrogen?

shrutishete

It´s weird that nitrogene has five valens e- and 4 bonds, meaning that 4 electrons are involved in those bonds and one is not, but still you say that it has no non-bonding valens e-. Or do you only consider lone pairs and not lone e-?

khalidraouz