Molecular Geometry - Free Formula Sheet: bit.ly/3YgxHkf Final Exams and Video Playlists: www.video-tutor.net/ Full-Length Videos & Worksheets: www.patreon.com/MathScienceTutor/collections Chemistry PDF Worksheets: www.video-tutor.net/chemistry-basic-introduction.html
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
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 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😷👍
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:)
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.
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!
btw could a more general Lone Pair formula be: (#total electrons - (#valence electrons if outer energy level is filled)*(#noncentral atoms))/2 ? Note I wrote #total electrons, not #valence electrons as you named it because formal charge should be added to valence electrons to give total electrons.
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. :)
Molecular Geometry - Free Formula Sheet: bit.ly/3YgxHkf
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Full-Length Videos & Worksheets: www.patreon.com/MathScienceTutor/collections
Chemistry PDF Worksheets: www.video-tutor.net/chemistry-basic-introduction.html
how does it feel to be a legendary chemistry teacher
he's a jack of all trade actually!
He just pure legendary he taught Virgin Mary how to have a baby and remain a virgin
Feels damn gooood !! Thanks for asking
@@Sir_Emo i didnt know wether to like ur coment or go to heaven
I learned Calculus from him before I learned chemistry, this man is truly the best teacher on UA-cam
This man has so much power in my life. He could totally tell me the wrong this and I would believe it without question
He can't say anything wrong
hi just letting you know that your videos are the only reason I'm passing gen chem 1. you're the best.
Thank you so much for your kind comment on our videos. I'm hoping you are now a Chem 1 master.
@@musick4288 who da fook is this guy
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.🙏🏻
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.
Hi, i am 13 yrs old and you helped me for my researches about resonanse structures, thank you
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My goal is to finish watching (learning from) every video you've uploaded (regarding chemistry) before completing my senior secondary edu 🐸
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
This guy has taught me everything I know and I don't even know what he looks like lollll. Man needs a university named after him.
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😷👍
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
Bro no bullshit, u deserve a noble peace prize for helping thousands of chem students pass they’re exams
It is really sister
Genuinely taught me more than my teachers at school.. now i finally understand why we gotta find lone pairs and stuff
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.
i honestly needed this for my midterm, thank you!!!!
Thank you so much! You make me love chemistry even more!
The way a UA-camr explains a difficult topic is just like raising a new born baby by her parents.
Btw thanks a lot
when i practice exam i always look at ur videos when im facing difficult questions and its helping me alot
so thanks
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
Thank you so much! ❤
From the night right before the exam 😅😂
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:)
This guy has taught more people than some professors lol
plus more easier to understand than most professors lol.
some? more like most lmao
my ochem professor makes us not put lone pairs on the resonance hybrid. maybe just a preference thing? patron here. best science videos ever!
..... You're the next Albert Einstein 📉🧠🖤😅
You the best bro
I’m wondering why the hell no one has ever taught me that center atom lone pairs trick before? It’s so helpful!
U deserves 2.3 M subscribers❤️
He's got more now. 2.8M
@@anvayaiyer5614 ❤️🤩
4.55 :)
8.52 now!
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I follow you forever. From a ChemE student.
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
@@fromir6619 JEBAITED
@@PHILLYMEDIC69 LOL GET THE STRAP
Can we all agree that traditional chemistry professors basically suck at what they do
like wtf. This guy makes it so simple.
love u bro. always helping out others
Bro thank you for the kind comment but we, the Organic Chemistry Tutor, don't love you.
@@musick4288 impostor😂
@@dab3stbb Nah, I'm a crewmate. hihihi
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.
He really simplified it!
You are making difference in peoples life thank you teacher
my chem exam is in 2 hours and im cramming 😵💫
You speak to my polymath heart!
Thanku sir i have learned draw resonance structure finally
u are the only god i praise
Always great videos. I've watched you for algebra too!
thank you so match, had a hard time to understand that until now
You are so match welcome!
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Y????
Mad one !
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BEST CHEM TEACHER 🙏🙏🙏🙏
Believe me or not but your voice is so beautiful 🤩
Thank you so much for your help,your videos really are helpful
OMG thank you this was such a huge help
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 😅
you saved my life.
Like 👍 if he is better than your highly paid chemistry lecturer.
Good luck with chapter 8 😂❤️
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!
It helps me a lot😊😊
You help me alot man keep it up!!! ❤️❤️
Thank you so much; I benefit from your video by building highly effective learning.
Thanks! Incredibly helpful!
Excellent service
easy and good explanation
Short and simple. Thank you.
Thank you!!!
You make it a lot easier to understand :)
Please make a vedio of showing how to draw resonance structure for NO2+( nitronium ion) I'm so confused With it.
Learned in only 8 minutes than the prof. taught in 1 hour
finally i can really understand itttt
many thx
Great help. Thank you.
In really appreciated this vedio...tnx very much
great teacher... thank you soooo much
Love your videos.. that’s nitrite not nitrate..
I really understood this thank you very much
You my best man
Thanks you so much for everything but I wanna you to do a video of how to identify the number of canonical structures
Will this also work for ap chem?
thank you very much for this video
amazing video
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".
How to know if a lewis structure really needs resonance?
THANK YOU THANK YOU THANK YOU
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Wish you were my school teacher.....
what is the difference between resonance structure and lewis structure? I really need to know in order to survive on my midterm test🙏🏻
thank you so much
very helpful
How do you know carbon can only form 4 bonds?
❤❤❤you are the best
Good efforts 🥹🫶🏻
can someone explain like what is the overall goal in resonance structures like how do we know which e- is going to which atom
btw could a more general Lone Pair formula be: (#total electrons - (#valence electrons if outer energy level is filled)*(#noncentral atoms))/2 ?
Note I wrote #total electrons, not #valence electrons as you named it because formal charge should be added to valence electrons to give total electrons.
Wow,,your awesome,,thanks❤
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??
Thank you!!!
It's literally 1 a.m and i hav my exam in 6h and am here
Thank you sir🙏🙏🙏🙏
bless ur soul
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. :)
@@anabanana8518 thanks guys. I'm now at 2nd year college. I think we're having a biochemistry course next sem after this pandemic.
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@@anabanana8518 Oh my gosh, Ana that's cool!
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I love you