@@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.
I hope you know that your videos have been helping me since I took general chemistry in highschool. I'm now, finally, taking organic chemistry in my second year of college and these videos continue to save me every day
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.
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
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.
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!
I know you probably hear this a lot, but you are seriously the best. You saved me in trigonometry and now chemistry. People, if you haven't supported this guys patreon, do it.
I m extremely happy with his simple and clear explanation of all science and mathematics concepts. Thank such a terrific doubtless tutor in your organic chemistry channel. I wish I have watch his video before then I think I would have excelled in all science subsubjectsat I have undertaken during my secondary study. May the good Lord continue to bless and hunstain you more in due time in your work. HELPFUL❤ Thank you sir organic science HERO tutor for your tremendous video❤.
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.
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
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.
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.
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
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.
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
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.
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.
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
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?
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
in SO2, how does left oxygen atom can have 6 dots and one bond at the same time? I mean 6 dots mean 6 V-electron which O in total has. Can sm1 please explain this to me? & how come in CN anion C also have 1 lone pair like nitrogen?
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?
11:57 I don't unerstand why because O is more electronegative than N, the 2nde configuration (the one with O) is more stable than the 1st (the one with N), can someone explain this to me please?
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.
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.
I suggest you draw out the Lewis dot structure for this polyatomic ion, namely,the hydronium ion,H3O +.O has 6 VE,one for each H,gives 9VE,but you subtract one e due to the plus one charge on this ion.You now have 8VE to draw this structure.You will have 3 bonded pairs,and one lone pair.Hence 6-5 =1,the FC is assigned to O of plus one.Good luck,you need to get a good tutor.
How do you know how many lone pairs to add to an atom that still doesn't have a completed octet? My teacher gave me some names of molecules and told me that there was a charge on each either positive or negative.
at 6 min 20 sec... what does Carbon has a pair of electrons left although it was a triple bond to N? Wouldnt that leave it with a single electron remaining?
Molecular Geometry - Free Formula Sheet: bit.ly/3YgxHkf
Chemistry 1 Final Exam Review: th-cam.com/video/5yw1YH7YA7c/w-d-xo.html
Formal Charge: www.video-tutor.net/how-to-calculate-formal-charge.html
you are such a blessing. whenever i search a chemistry topic, i always look out for your videos first
Are u also preparing jee???
fr fr
me too i always look up for him coz he makes things simple. what a blessing
Me too!
Indeed.
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.
How can I know the number of dots to be put in an element and the type of bond to be put
look at his lewis structure videos
@@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.
I hope you know that your videos have been helping me since I took general chemistry in highschool. I'm now, finally, taking organic chemistry in my second year of college and these videos continue to save me every day
No bullshit! Straight to the point! Your video's help me a tremendous amount during my exams! Keep up the good work!
For the CN- confusionistas out there: 6:50
When drawing the Lewis structure, be aware of the charges in the formula given: CN-
Tyyy❤
out of curiosity what language do you learn chemistry with
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.
Wow, i really like this Man's Voice.It's soothing and it seems like all my anxieties about Chemistry and Calculus dissapears whenever i listen to him.
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
It's interesting how something so simple can be complicated so much. Since formal charge can be calculated with just a simple equation.
Seriously, I learned all my chemistry through this channel! Thank you so much!
You're a hero.
Thanks
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!
yeah my professor gave me some bs formula that takes much more work but this is easy
31 dislikes from professors who overcomplicate things
dude lmao love the profile picture
lol this
@@kennyo4230 ahhhh the simple times when there was a dislike count
much better times when dislikes appeared.
Back when you could see dislikes on videos
"If you don't use it you are gonna forget it" love it😊
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.
missed the lecture on formal charge for my chem class and have been struggling ever since, THANK YOU for such a clear explanation
I like how you always address any lingering questions the viewer might have which might trip them off during exams.
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
I got a 100 on my quiz 😭 thank you ❤️
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!
I know you probably hear this a lot, but you are seriously the best. You saved me in trigonometry and now chemistry. People, if you haven't supported this guys patreon, do it.
thanks sir , that sound seems more relaxing than i used to hear across
You just saved my rank in a competitive exam...
Thanks
I m extremely happy with his simple and clear explanation of all science and mathematics concepts. Thank such a terrific doubtless tutor in your organic chemistry channel.
I wish I have watch his video before then I think I would have excelled in all science subsubjectsat I have undertaken during my secondary study.
May the good Lord continue to bless and hunstain you more in due time in your work. HELPFUL❤
Thank you sir organic science HERO tutor for your tremendous video❤.
Best Chemistry TH-camr in the world;
Keep making content like this bro, Love you 😀😍🤩😃😀😃😍🤩
Holy crap way easier than what my professor gave us. I love how you dumbed it down. Way easier than what she showed us
I actually learned new things while learning about formal charges... thank you so much
Your videos are so helpful! Thank you so much😭❤️
Great video! Easy to understand and straight to the point
why do professors have to complicate things.. such simple things.... smh
because they are dumb
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
Andrew Mullins whaaaa
@@convicted5506 bro I just want to pass
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.
Thank you so much! I can watch these and be able to help others in my classes!
Someone verify this man
Thanks!
your formula was way better than my text books! Thank you for sharing! I appreciate you.
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
Thanx a bunch.....👌👌👌👌👌👌👌 he really made dis concept DAMN EASY...
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.
3:00- how is it possible for O to bond 3 Hs with its two e's spared??
very helpful. Thank you for teaching what professors should in class teach us.
FINALLY, I now understand why some lewis structures have double bonds for apparently no reason (SO4 -2 and PO4 -3). Thank you so much
I just watched this 7 mins before my exam thank you so much
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.
very good tutor
ur the reason why i love chemistry
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
This is the best video on TH-cam
I was answering my quiz while the time is running while I was watching your video. Thank you so much. I got 18/20 score. Not bad.🤣❤
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.
to draw its Lewis dot structure
you do the stuff in such a cool manner
Love your work.
One criticism though... I always have to turn up my volume, you often post your videos with audio volume too low.
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.
Love your videos..so helpful..but could you please increase the volume of your voice. Thanks for all your wonderful vidoes
Thank you so much!!! Helped me sooo much more than my professor!
You video is tremendously helpful. Thanks
Thank God 🙏
I hope you add Arabic subtitles for arab student and thank you for your help ❤️
3:29 Why is he using that lewis structure for S02 when it should be where S forms 4 bonds with 1 lone pair?
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
Your are a gift for us from God may u live long and thanks for explaining that how we can find the charge
thank you man you really helped me in my end term high school exams
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 .
good channel for pre university!!
I have a question in these questions do we have to count the no. Of bonds or no. Of bonded electrons ?
Plzz do reply
for the Cyanide example, why is the carbon still have 2 lone pairs with a triple bond to Nitrogen? thanks!!
For the CN- why is the extra electron added to C and not N since N has a greater Electronegativity value
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.
You’re incredible, you’re my idol
In h30+ molecule there will be three unpaired electron so it should be like this (6-(3+3))=0 ?
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.
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
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
I have the same question
Where do the R and H mean at 0:33?
76👎 likes from Australia.. you are such a blessing❣️
You’re the best, thank you so much
@3:09 doesn't oxygen have six valence electrons so shouldn't there be three dots instead of 2
Thankyou bro I was able to solve my hw with this omm you god
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?
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
Woop man loved it❤❤❤
in SO2, how does left oxygen atom can have 6 dots and one bond at the same time? I mean 6 dots mean 6 V-electron which O in total has. Can sm1 please explain this to me? & how come in CN anion C also have 1 lone pair like nitrogen?
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?
+1 means lose and -1 means gain :)
It's 5-4=+1 that's why the positive 1 charge
Thank you so much ..you have really helped me.....God bless you
You tube channel of the millennium 👏👏✊
11:57 I don't unerstand why because O is more electronegative than N, the 2nde configuration (the one with O) is more stable than the 1st (the one with N), can someone explain this to me please?
Thank god for you!!!❤️🙏🏻
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.
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.
You are very smart. You have a gift of taking something complex and making it simple. God bless you. God is good.
is having a net charge of 0 in the molecule the same as not processing a formal charge?
Couldn't I add another bond in the SO2 structure to the right oxygen to balance out the +1 and -1 formal charges? Sulfur is an exception to octet.
thanks very very much! never got it before this
You sir are a life saver
This dude is pro.
this has really helped me
Hey oxygen has 6 valency and it has 3 bonds with H that means its go 3 lone electrons right ?
6-(3+3) ?
I suggest you draw out the Lewis dot structure for this polyatomic ion, namely,the hydronium ion,H3O +.O has 6 VE,one for each H,gives 9VE,but you subtract one e due to the plus one charge on this ion.You now have 8VE to draw this structure.You will have 3 bonded pairs,and one lone pair.Hence 6-5 =1,the FC is assigned to O of plus one.Good luck,you need to get a good tutor.
@@ronlal652 i got it ron its been 11 months xD
So that's the end of the video, thanks for watching and have a great day. I got you coach!!
thanks buddy good work helped me a lot
How do you know how many lone pairs to add to an atom that still doesn't have a completed octet? My teacher gave me some names of molecules and told me that there was a charge on each either positive or negative.
at 6 min 20 sec... what does Carbon has a pair of electrons left although it was a triple bond to N? Wouldnt that leave it with a single electron remaining?
you have to add one e to account for the the minus one charge on this ion.
Your voice is soothing
The king has saved me once again
Thank you for dumbing it down for me
this helped me so much