It's been 8 years since I took high school chemistry. I'm a junior in college now. My Chem professor said, "If you don't remember how to do high school chem you're going to struggle in this class. And I did. Then I remembered you're channel existed and have had no problems learning the material. I'm starting to think that she was just trying to make excuses for not actually teaching the material.
I was totally confused after attending my teacher's lecture on Resonance Structures. I couldn't understand a single thing, I got so irritated and came here and within 10 mins 30 seconds I have now mastered the concept! (okay, yeah, atleast to some extent) He is so calm, composed and clear headed that his attitude reflects into yours too, even through the virtual medium! I'm not the kind that usually posts comments but this video definitely deserves applause... Way to go sir @The Organic Chemistry Tutor
Professor Organic Chemistry Tutor, thank you for a basic Introduction into Resonance Structures in AP/General Chemistry. Drawing the resonance hybrid is not a difficult process, however moving the electrons / lone pairs around can be problematic. In drawing resonance forms, you can only move the electrons. This is an error free video/lecture on UA-cam TV with the Organic Chemistry Tutor.
Our prof is redirecting us to you. We do not use platforms for online lectures due to poor internet connection. Should we give you her salary to you instead?
I was at first trying to relocate certain atoms and ions to other parts of the structure, but realized that that would turn the molecule into another molecule or a molecule that doesn't exist. So better do it the more labor intense way and draw all the resonance forms:)
How do you know where to place the charges on the structure? I know you said oxygen always has a - charge if it has 1 bond and 3 lone pairs, but does that rule apply to other elements? thanks!
I have found a more developed way to get the number of lone pairs, here’s how it works - First count the number of valence electrons, just like he does but if you have have Hydrogen in the molecule, count its valence electrons as ‘7’. Now that you have the total valence electrons, divide it by 8. Now you will have a quotient and a remainder, the quotient tells you about the number of sigma bonds in the molecule and then divide the remainder by 2 and it will give you the number of lone pairs on the molecule(Just try it once, although it only works on single central atom species). You can even use this to get the HYBRIDIZATION of a molecule. For example take NO2- , here VE(N) = 5, VE(O)=6 and count the electron as 1, so total we get 5 + 2 x 6 + 1 = 18, now divide by 8 we get 2 as quotient and 2 as remainder, that means, there are two sigma bonds and 2/2=1 lone pair on the central atom, And the fun part is if you add 2(sigma bonds) and 1(lone pair) you get three which states that it is a sp2 hybridized molecule. ( 2= sp , 3=sp2, 4=sp3 and so on) good tryy ittt. Thank you for reading and do try it with a hydrogen species as well, just remember to count its valence as 7. And channel owner sir please pin it as well so others can be helped as well😷👍
thank you for telling me that lone pair formula only works if hydrogen isnt present... legit been asking why this formula he showed isnt working on a number of problems I have been working on.
The aim of chemical bonding is to attain octect Structure. N has five electrons on its outermost shell, on forming three bonds, it gains three more electrons and hence, 8. .. :N• This was the initial position of the bonds until they were bonded to oxygen.
When you break the first N-O double bond, are you not supposed to evenly distribute the two electrons from that bond between N and O, in which case the oxygen ends up having 2 lone pairs and one unpaired electron instead of the 3 lone pairs on the diagram??
Hi I have a question. How would you know that building a resonance structure would stop at a certain point? Foe example, in your 1st ex the Co3 2- you got 3, but in No2 you only got 2?
If the same resonance structure with which we started repeats then we can come to a conclusion that there are no more resonance structures possible for the given molecule
The comment above me is correct. This is because Co3 2- has THREE oxygen atoms, so the double bond will move between three oxygens. But No2 has TWO oxygen atoms, so the double bond will move between two oxygens only. Hence, Co3 2- has three resonance structures, and No2 has two. Hope this helped. :)
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Chapter 8 - Video Lessons: www.video-tutor.net/chemical-bonding.html
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Thank you so much for your kind comment on our videos. I'm hoping you are now a Chem 1 master.
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It's been 8 years since I took high school chemistry. I'm a junior in college now. My Chem professor said, "If you don't remember how to do high school chem you're going to struggle in this class. And I did. Then I remembered you're channel existed and have had no problems learning the material. I'm starting to think that she was just trying to make excuses for not actually teaching the material.
I was totally confused after attending my teacher's lecture on Resonance Structures. I couldn't understand a single thing, I got so irritated and came here and within 10 mins 30 seconds I have now mastered the concept! (okay, yeah, atleast to some extent) He is so calm, composed and clear headed that his attitude reflects into yours too, even through the virtual medium! I'm not the kind that usually posts comments but this video definitely deserves applause... Way to go sir @The Organic Chemistry Tutor
I don't understand it, maybe I'm missing something 🤔
What my prof taught in half a lecture, you taught me in 3 minutes. Literally at the 3min mark the lightbulb went off in my head, thank you kind sir.🙏🏻
My goal is to finish watching (learning from) every video you've uploaded (regarding chemistry) before completing my senior secondary edu 🐸
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You are the reason I am passing General Chemistry. Thank you so much
incredibly helpful ......your videos are the only reason to make me enable to pass my course of organic chemistry
Hi, i am 13 yrs old and you helped me for my researches about resonanse structures, thank you
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i honestly needed this for my midterm, thank you!!!!
Thank you so much! You make me love chemistry even more!
I’m finally taking o chem!! Even though I’ve been watching my whole college career for stats, algebra, and other math courses! Thank you
The way a UA-camr explains a difficult topic is just like raising a new born baby by her parents.
Btw thanks a lot
love u bro. always helping out others
Bro thank you for the kind comment but we, the Organic Chemistry Tutor, don't love you.
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This guy has taught more people than some professors lol
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when i practice exam i always look at ur videos when im facing difficult questions and its helping me alot
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From the night right before the exam 😅😂
Genuinely taught me more than my teachers at school.. now i finally understand why we gotta find lone pairs and stuff
He really simplified it!
my ochem professor makes us not put lone pairs on the resonance hybrid. maybe just a preference thing? patron here. best science videos ever!
Professor Organic Chemistry Tutor, thank you for a basic Introduction into Resonance Structures in AP/General Chemistry. Drawing the resonance hybrid is not a difficult process, however moving the electrons / lone pairs around can be problematic. In drawing resonance forms, you can only move the electrons. This is an error free video/lecture on UA-cam TV with the Organic Chemistry Tutor.
Our prof is redirecting us to you. We do not use platforms for online lectures due to poor internet connection. Should we give you her salary to you instead?
😂
Most definitely
OMG thank you this was such a huge help
Always great videos. I've watched you for algebra too!
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I follow you forever. From a ChemE student.
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He's got more now. 2.8M
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4.55 :)
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thank you so match, had a hard time to understand that until now
You are so match welcome!
I was at first trying to relocate certain atoms and ions to other parts of the structure, but realized that that would turn the molecule into another molecule or a molecule that doesn't exist. So better do it the more labor intense way and draw all the resonance forms:)
Thanku sir i have learned draw resonance structure finally
Thank you so much for your help,your videos really are helpful
How do you know where to place the charges on the structure? I know you said oxygen always has a - charge if it has 1 bond and 3 lone pairs, but does that rule apply to other elements? thanks!
You are making difference in peoples life thank you teacher
Thank you so much you saved my life
At 5:58 he says to draw the nitrate structure but writes down the nitrite NO2- ion 😅
BEST CHEM TEACHER 🙏🙏🙏🙏
I’m wondering why the hell no one has ever taught me that center atom lone pairs trick before? It’s so helpful!
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easy and good explanation
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It's literally 1 a.m and i hav my exam in 6h and am here
it is really helpful for my midterm!!!!! Thank you so much!!!🥹🥹
finally i can really understand itttt
many thx
I really understood this thank you very much
my chem exam is in 2 hours and im cramming 😵💫
In really appreciated this vedio...tnx very much
Short and simple. Thank you.
I have found a more developed way to get the number of lone pairs, here’s how it works - First count the number of valence electrons, just like he does but if you have have Hydrogen in the molecule, count its valence electrons as ‘7’. Now that you have the total valence electrons, divide it by 8. Now you will have a quotient and a remainder, the quotient tells you about the number of sigma bonds in the molecule and then divide the remainder by 2 and it will give you the number of lone pairs on the molecule(Just try it once, although it only works on single central atom species). You can even use this to get the HYBRIDIZATION of a molecule. For example take NO2- , here VE(N) = 5, VE(O)=6 and count the electron as 1, so total we get 5 + 2 x 6 + 1 = 18, now divide by 8 we get 2 as quotient and 2 as remainder, that means, there are two sigma bonds and 2/2=1 lone pair on the central atom, And the fun part is if you add 2(sigma bonds) and 1(lone pair) you get three which states that it is a sp2 hybridized molecule. ( 2= sp , 3=sp2, 4=sp3 and so on) good tryy ittt. Thank you for reading and do try it with a hydrogen species as well, just remember to count its valence as 7. And channel owner sir please pin it as well so others can be helped as well😷👍
Does this work with ammonia NH3??
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thank you for telling me that lone pair formula only works if hydrogen isnt present... legit been asking why this formula he showed isnt working on a number of problems I have been working on.
At 2:03, is there a reason for why Oxygen has a (-) when it has 3 lone pairs?
I think you'll find the answer in a video about "formal charges".
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Like 👍 if he is better than your highly paid chemistry lecturer.
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Can someone explain why on 7:28 he mentions that Nitrogen has 8 electrons?
The aim of chemical bonding is to attain octect Structure. N has five electrons on its outermost shell, on forming three bonds, it gains three more electrons and hence, 8.
..
:N•
This was the initial position of the bonds until they were bonded to oxygen.
Thanks for your offer
Thank you sir🙏🙏🙏🙏
amazing video
Please don't use dark-blue colored pens on a black background. It's hard to distinguish between the two. Great video.
fuck u bitch. why dont u make the video then
@@PHILLYMEDIC69 he asked him politely and shared his opinion. there's no need to be harsh on him.
lol he's so mad
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Thank you!!!
Will this also work for ap chem?
Can we all agree that traditional chemistry professors basically suck at what they do
like wtf. This guy makes it so simple.
Thank you so much; I benefit from your video by building highly effective learning.
Good luck with chapter 8 😂❤️
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Please make a vedio of showing how to draw resonance structure for NO2+( nitronium ion) I'm so confused With it.
How to know if a lewis structure really needs resonance?
1:59 is there any way to know that? Or is it memorization
Good efforts 🥹🫶🏻
bless ur soul
Thanks you so much for everything but I wanna you to do a video of how to identify the number of canonical structures
Love your videos.. that’s nitrite not nitrate..
When you break the first N-O double bond, are you not supposed to evenly distribute the two electrons from that bond between N and O, in which case the oxygen ends up having 2 lone pairs and one unpaired electron instead of the 3 lone pairs on the diagram??
Why don't you put the negative charge of NO2- on O but in brackets... ?
Hi I have a question. How would you know that building a resonance structure would stop at a certain point? Foe example, in your 1st ex the Co3 2- you got 3, but in No2 you only got 2?
If the same resonance structure with which we started repeats then we can come to a conclusion that there are no more resonance structures possible for the given molecule
The comment above me is correct. This is because Co3 2- has THREE oxygen atoms, so the double bond will move between three oxygens. But No2 has TWO oxygen atoms, so the double bond will move between two oxygens only. Hence, Co3 2- has three resonance structures, and No2 has two.
Hope this helped. :)
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@@anabanana8518 Oh my gosh, Ana that's cool!
Thank you