How To Calculate The Formal Charge of an Atom - Chemistry

[@TheOrganicChemistryTutor]

Molecular Geometry - Free Formula Sheet: bit.ly/3YgxHkf Chemistry 1 Final Exam Review: kzbin.info/www/bejne/a6raYox-bL50bcU Formal Charge: www.video-tutor.net/how-to-calculate-formal-charge.html

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Me too!

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Indeed.

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You’re kidding. I spent a week confusing myself on formal charge and I finally understand it 1 minute into this video? You’re a blessing.

[@esnartmwanza7071]

How can I know the number of dots to be put in an element and the type of bond to be put

[@Glidingwithdolphins]

look at his lewis structure videos

[@RicJiang]

@@esnartmwanza7071 “u just have to know” is what my professor said. “It’s obvious” The organic chm guy says that Hydrogen has 1 and so does everything below it Beryllium has 2 and so does everything below it Boron has 3 and so does everything below it Carbon has 4 and so does everything below it Nitrogen has 5 and so does everything below it Oxygen has 6 and so does everything below it Florine has 7 and so does everything below it Neon has 8 and so does everything below it Helium has 2 it’s an exception.

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[@theo3027]

For the CN- confusionistas out there: 6:50 When drawing the Lewis structure, be aware of the charges in the formula given: CN-

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out of curiosity what language do you learn chemistry with

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I'm taking an advanced biochemistry course as a senior that relies on concepts I learned in gen chem as a freshman like formal charge. I've been watching your videos for years and they've genuinely been a lifesaver for concepts that went over my head.

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AN HOUR LONG ASYNCH LECTURE WAS ABOUT THIS AND I DIDNT GET IT,,,,,,,,,, BUT I LITERALLY UNDERSTAND IT NOW AFTER A 13 MIN VIDEO 😭 why r we even paying for uni at this point smh

[@Veronicz]

It's interesting how something so simple can be complicated so much. Since formal charge can be calculated with just a simple equation.

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31 dislikes from professors who overcomplicate things

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much better times when dislikes appeared.

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Back when you could see dislikes on videos

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You're a hero.

[@TheOrganicChemistryTutor]

Thanks

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2021 is here and I am watching this video now. Honestly, the formula is the best so far and it is way easier to remember, so thanks for sharing!

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yeah my professor gave me some bs formula that takes much more work but this is easy

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Listen you have been an absolute lifeline for me trying to learn chem from an online course.... Thank god for you or I'd have failed

[@georgesadler7830]

Professor Organic Chemistry Tutor, thank you for an outstanding Introduction into How to calculate the formal charge of an atom or element in a Lewis structure. Calculating the formal charge is simple to follow and understand, however drawing the Lewis structure is problematic. Thanks to the viewers for finding and correcting the errors with the Lewis structures in AP/General Chemistry.

[@senny-]

I like how you always address any lingering questions the viewer might have which might trip them off during exams.

[@br1ghtl1ght]

missed the lecture on formal charge for my chem class and have been struggling ever since, THANK YOU for such a clear explanation

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[@wmm100]

Thanks for your help, graciously appreciated! I was finding it quite frustrating, trying to understand how to calculate Lewis' formal charge. You've made it a delight to move forward!! Doing a good job!

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why do professors have to complicate things.. such simple things.... smh

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because they are dumb

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Juan Piñeres no... because in the real world things aren’t going to be easy. They want you to TRULY make a connection and understand

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[@مريَم-ط5م7غ]

@@convicted5506 bro I just want to pass

[@convicted5506]

Gone In A Wisp formal charge does connect to a lot of other things in chemistry.. and you also have to read in your text book. You can’t walk into a class not prepared and expect to understand a foreign concept almost instantly. That’s not realistic.

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Someone verify this man

[@ael019]

thanks sir , that sound seems more relaxing than i used to hear across

[@Cole_pie]

Holy crap way easier than what my professor gave us. I love how you dumbed it down. Way easier than what she showed us

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[@Baron-nv1ez]

Craxy how I learnt more in 13 minutes than in an 1 1/2 hr long lecture. It's like the professor was speaking in a foreign language .

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Great video! Easy to understand and straight to the point

[@matthew6762]

I just watched this 7 mins before my exam thank you so much

[@greaterthanlife]

Good video But there's a slight mistake here tho the FC for the Oxygen on the right is also 0 because O has a valencyn of 6 so it uses one of those 6 to bond leaving it with 5 hence d for the oxygen on the right is 5

[@ianhuskins2491]

Thank you so much! I can watch these and be able to help others in my classes!

[@gwendolynnfernstrom6247]

your formula was way better than my text books! Thank you for sharing! I appreciate you.

[@ivanpedro9151]

FINALLY, I now understand why some lewis structures have double bonds for apparently no reason (SO4 -2 and PO4 -3). Thank you so much

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I really appreciated this video, before to see this this section is very difficult and complicated to me but now i understand how easy and interesting part. Thank you

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I actually learned new things while learning about formal charges... thank you so much

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very helpful. Thank you for teaching what professors should in class teach us.

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[@5kunk157h35h17]

Great that you added the thing about electronegativity at the end. I would have thought that the priority of the bonds would have gone to O if i had stumbled upon this problem on my own, since O is known to want to form 2 bonds and the formal charge didn't differ between example 1 and 2.

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76👎 likes from Australia.. you are such a blessing❣️

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god bless omg literally first day of o chem we talk about formal charge- NO EXPLANATION on how to do it, just straight into examples problems :l... and he was mad cuz no one answering the question like bruh

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This is the best video on KZbin

[@ronlal652]

The common sense method is the best way to figure out the formal charge.Since N is a group five element it has five VE in its non bounded neutral ground state.If it has more or less than five VE than it will incur a formal charge.Assume that R is another H,then you will get the amide ion which has a formal charge of -1 on the N,since N accounts for six of total of eight VE around the central atom.All of LP are counted and only half of the bounded pair since H accounts for the other two.In the case of ammonia,there is no formal charge on N,since it has five,the same as it its ground state.One LP plus one half of six gives you 5.In the ammonium ion,N will have a formal charge of plus one,since there are no LP,all of the bounded pairs will have to be divided by two,hence eight electrons around the central atom N,cut in half is 4.But it is supposed to have five in its ground state,hence 5-4 is one.H does not incur a formal charge in any of the examples since it has only one its magic number.

[@9th.class.chemistry]

Your are a gift for us from God may u live long and thanks for explaining that how we can find the charge

[@daliaashraf7068]

i wonder why we calculated the num. of valence e- first on the example of OCN- Also, thank you so much. it's a real tutor.

[@ronlal652]

to draw its Lewis dot structure

[@4pharaoh]

Love your work. One criticism though... I always have to turn up my volume, you often post your videos with audio volume too low.

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Thanks!

[@ndiengalamedionysius2121]

you do the stuff in such a cool manner

[@zack_120]

3:00- how is it possible for O to bond 3 Hs with its two e's spared??

[@angeliq596]

Love your videos..so helpful..but could you please increase the volume of your voice. Thanks for all your wonderful vidoes

[@johmcg64]

Apply the octet rule for nitrogen and then the duet rule for hydrogen before calculating the formal charge. He applied the octet rule when he put in the x's around the nitrogen atom.

[@Mister-l3j]

3:42 , Sorry sir but are you sure that dots of Oxygen of right side should have 6 dots, shouldn’t it contain 5, since it gave one of its dots to bond with Sulfur

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[@ayasamer7731]

Thanks It's soo helpful ❤ But I want to learn more about Lewis structure and how can I know the number of dots and bonds

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The king has saved me once again

[@gabrielpetit2911]

Another way to look at it is if the atom is making more or fewer bonds than its valency then it will have a formal charge. Every "extra" bond means a negative charge and every "missing" bond means a positive charge. This kinda breaks down when the octet rule is broken, so like Xenon Difluoride, but it works well for molecules with atoms from periods 1 and 2.

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My professor (“Dr” Denton) who doesn’t even have a doctoral degree just expected us to figure this out on our own.

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Did u figure out

[@kalanicoria362]

You’re the best, thank you so much

[@sprihaa899]

I have a question in these questions do we have to count the no. Of bonds or no. Of bonded electrons ? Plzz do reply

[@mathewspuente3510]

3:29 Why is he using that lewis structure for S02 when it should be where S forms 4 bonds with 1 lone pair?

[@eljefe3794]

So that's the end of the video, thanks for watching and have a great day. I got you coach!!

[@sarmiento123]

Thank you for dumbing it down for me

[@kholofelomonene4440]

For the CN- why is the extra electron added to C and not N since N has a greater Electronegativity value

[@clairedantzlerward4266]

Where do the R and H mean at 0:33?

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You sir are a life saver

[@chauhinchong3324]

for the Cyanide example, why is the carbon still have 2 lone pairs with a triple bond to Nitrogen? thanks!!

[@devsiwach100]

thanks buddy good work helped me a lot

[@gitmemed2668]

i have a question, when he does the lewis dot, why is it always short one dot? the oxygen has 6 valence electrons but i only count 5, same to the other elements

[@westrice6539]

I have the same question

[@zarinah16]

How are you supposed to know that the Sulfur dioxide has a double bond? Is that something we are just supposed to know or is that something you can figure out?

[@chrislliatsos]

im new to organic chemistry and have a question. when it comes to the cn- (cyanide), why are you using an alkenes, triple binding, instead of an alkanes, double binding? thanks.

[@ronlal652]

Before you can assign FC on a polyatomic ion you have to first draw its Lewis dot structure. N has 5 VE, C has four VE ,and you will have to add one e to account for the -1 charge, thus giving you 10 VE for this structure.This is the best way to complete the ocet .With triple bond both C and N will have 8 VE around it.For this ion C will be assigned the -1 FC not N,since N has 5 VE in its ground state,and this is the same as in this ion,half the bonded e plus the LP will equal 5,and 5-5=0 hence no FC on N,the C gets the FC of -1.See my above explaination to assign FC.

[@contentgeek4673]

in the first example with the R-N-H, where did the 4th electron come from? N in nature has 5 valence e, R bonds N leaving N with 4e and then H comes along and takes 1e leaving N with 3 valence e. Hence 3 dots representing 3 electrons, not 4.

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Does this work always cause I am going to use this on a nationalnlevel exam

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Great videos, however I would greatly appreciate fixing the volume, when the ads pop out, they are so loud because I have to put the volume up to hear your videos.

[@shreeramjha5073]

In h30+ molecule there will be three unpaired electron so it should be like this (6-(3+3))=0 ?

[@japantradingmachinery9782]

Very very vvvvvery helpful lecture

[@cayanlamanna]

is having a net charge of 0 in the molecule the same as not processing a formal charge?

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Woop man loved it❤❤❤

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[@superfightingrobotmkx7776]

7:08 I'm confused. If Nitrogen has 5 valence electrons and the hydrogen atoms each subtract 1 through covalent bonding, why does it have a +1 charge? Shouldn't it be a -1 charge since there's 1 electron left over?

[@advin6159]

+1 means lose and -1 means gain :)

[@gunamuthu9284]

It's 5-4=+1 that's why the positive 1 charge