Lewis Structures and Formal Charges Practice Problems | Study Chemistry With Us

Practice drawing these lewis structures and don't worry we will go over all the answers step by step. This video will explain how to find the formal charges of each element in a structure, what formal charges are best, and why formal charges can be used to draw the best lewis structure.
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Thank u very much, that helps me alot, this is the first time i understand why there are more than one Lewis structure for polyatomic ions.

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i think i need a little more practice and ill be where I need to be to get that A !!!

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Thanks, I have better understanding for formal charges after watching your video.

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Thank you so much. I just found this one when I am very stuck with Lewis structure

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[@graceorji6423]

Their is a trick I got from this whole lesson
That is ,that when their is just a single minus sign that means I will have just one single bond in the structure and that also implies to the sign of minus 2
Thanks for this great video

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[@reginas4009]

Hi, thank you so much I get it more! But one question, I thought that the formal charge formula looks like: FC= #valance electrons -(#non-bonding + 1/2 bonding electrons) because that’s what I’ve been learning. So is the 1/2 not necessary?
Thank you so much though !!!

[@danielhonour-god4916]

1/2×5 is the same this as 1/2×5/1
So the 1 times the bonding electrons

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[@AG-kn9gn]

What do you do if, in order to make the central atom have a formal charge of zero, you can't meet the octet rule? Which is more important if you can't do both? For example- CCl2. To make carbon have a FC of zero, carbon will be left with only 6 valence electrons and carbon is not an exception to the octet rule.

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Thank you so much✨✨
I understand much more💕💕

[@joshcowles2745]

At 7.01, how come the oxygen atoms have 6 lone pairs of electrons attached, as well as the one bonding with Sulphur, which adds up to 7, if it only has 6 valence electrons?

[@hassinagayapershad7402]

I have the same question

[@sarahbender8251]

Thank you for your content! It has been very helpful!
I actually am confused about the very last problem. Why wouldn't nitrogen and oxygen have a double bond and then fill in the lone pair for oxygen? When do you use double bonds versus lone pairs?

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Thank you so much

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Thank you melissa it was really helpful!!❤ i could nt understand one part at 24:48 why one of the Fluorine atoms have only two lone pairs i understand why the other Fs have 3 lone pairs but i don t get why this F has 2 lone pairs

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Your formal charge equation I prefer over the book! Thank you so much I understood it better practicing with you.

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HIIII Melissa, I just wanted to ask if it matters where we put the hydrogen for the oxygen in the last problem?

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Can you make a video about functional groups? PLEASE AND THANK YOU!!!

[@yasmeenyas4056]

Thank you for this video. However, I just had a quick question I thought that the central atom always has to have a charge of zero. Because for No3- the charge on the nitrogen is 1 and thats the right structure. So how would you know if the central atom is supposed to be zero or have a charge on it? Thank you in advance

[@bone5200]

Can anyone explain when she does [SO4]-2, why sulfer does not form only 2 bonds? i thought since it was in group 16, it would only want to form 2 bonds, not 4. Thank you!

[@Iddo97]

why is it more favourable to have a neutral formal charge on the central atom? do you have a video about this?

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Thanks

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[@estheralaba1195]

Melissa pls explain why sulphur is having 6 bonds because it only makes a bond

[@silashollis6630]

On the NH2OH problem, could we have triple bonded oxygen and nitrogen with oxygen having one lone pair?

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no, because in this Nitrogen will have 10 electrons around it and it cannot expand the octet.

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What do we do if the formula has an element like Ti in it? Like TiCl4

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Ma'am how can we draw lewis dot structure for Br3O8 ma'am? can u pls explain it?

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any have an idea why the last question at 27:50 can't have a double bond between the Nitrogen and the Oxygen with the Oxygen having 4 electrons on it still

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so helpful!

[@ezbuz]

why does cl go next to C and not next to H??? I dont know if my question makes sense lol, but like I wanted to draw the hydrogens around the carbon then put clorine next to one of the H but here you say to still have the hydrogens around C but leave a space open to attach that Cl

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What is the device you use to show this awesome exercise online?

[@走言走语]

I applied the formal charge rule and in most cases, it worked. However, it is not working for NO3-. I thought there should be 5 bonded electrons attach to N but the correct one is actually 4 bonded electrons attach to N.

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Love u Melissa ❤️

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thank you!

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Please upload a video on acids and bases,my favorite teacher

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it was good..