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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Melissa, I grew up in a cult where we weren't allowed to learn Science at all. I recently started college and was terrified of how I'd do. Over the summer I watched all of your videos to prepare and I just took my first Chemistry test ever and got a 95%. Thank you!!!!

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Melissa, you put in a lot of sincere efforts in preparation and lucid teaching.. Kudos..

[@Lina-vf1ky]

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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This was so helpful in understanding everything especially formal charge!!!!

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

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Using this adding formula instead of the fraction formula is so much easier. Thank you.

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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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This is the only Lewis Structure practice video that went slow enough for my slow brain to comprehend. Thank you 😊

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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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[@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.

[@hsal8797]

Thank you soooooooo much!!!!!

[@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 !!!

[@Learn_with_Dynasty]

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

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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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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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this is the first time i ever understood lewis structures. have my exam on Monday wish me luck💔

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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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[@chloe817-eq3ee]

Hi! I know this video is older, but your videos help so much. I was wondering if the specific shape you do Lewis structures matter? I have seen it done in several different ways. For example, if I had a molecule with 4 species (ex. PCl3), would it matter if I put one of the Cls above or below the P? P has a lone pair in this structure, but I usually put species below the main least electronegative atom, not above. I also noticed that, with IF5, your student was specific in trying to represent geometry. I usually do 5 bonds and do not worry about representing the structure, just my ability to recognize and label it. Is this super important? Thanks!!

[@JovenC123]

Thanks

[@Iddo97]

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

[@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

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i was like genuinely clueless about lewis structures but now i have such a clear understanding of them that's crazy

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thanku mam it helps a lot

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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?

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

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it was good..