You are a really good teacher ! I switched over "completely" to your videos after I seen the comments you posted on the mistakes made by Kahn academy. Anyway, when I was 16, I won first place on a questionnaire contest about chemistry, spec. the periodic table. Over the years after the military, and going from job to job, and then kids, found myself a 47 year old, still a fan of science, physics, biology, astronomy, and especially Chemistry. Wanted to refresh my knowledge of what I knew 30 years ago and learn even more than ever before. Your videos are informative and refreshing. You speak clearly, and get right to the point. Will donate to you in a month or so, after I get out of this slump ! Thanks again Dave ...
that's a heck of a success story for the passion of learning! many rounds of applause. thanks for watching! haha maybe i should leave a bunch more comments on the khan content, i didn't know it was getting me viewers!
Professor Dave Explains well it needed to be done ! One assumes that a course being taught is by the right person ! I MYSELF caught mistakes, but I'm sure he left a Hydrogen out. Also, I always thought Carbon was a stickler for the octet rule. That guy had a moment or short period of Carbon having a fifth Bond, I thought it couldn't, not even for a split second ... thanks again, See ya !
I've commented the following comment about 5 times in other Prof. Dave comment sections. The quality of your content is so dang high that I believe you've earned a PhD. I'm calling it now: in the near future, I think a university will reward you for your hard work. You 100% deserve it. In the meantime, I hope this channel earns you wealth & happiness. Thanks for making this, the educating of others, your life.
theres always someone trying to make it more complicated than it has to be xD... OR someone smarter who boils it down to its essence through understanding ;)
Seriously, the most HELPFUL and easy-to-understand person out there. I grasped the concept within 4 minutes of watching your video. Something my Chem professor couldn't properly teach and help me understand within an hour and a half. THANK YOU!
in the video C2H4 shown on the left has lines which represent bonds, since carbon is at the ends of lines the bonds shown would not be carbon-hydrogen but instead carbon-carbon.
Oh, you are very right. I found an other mistake which I will tell him separately. The resonance structure with the positive charge on the carbon isn't the more important. The resonance structure with the positive charge on the oxygen atom is the more important, because when carbon bears a positive charge, it hasn't got a filled octet. And it is more important to have a full octet than to have a positive charge on the less electronegative atom.
thank you sir through this video I got these concepts cleared in my mind : -formal charge -appropriate Lewis dot structure - and definitely resonance hybrid and canonical structure thanks a lot!
I wish i had found your channel when I was preparing for NEET. I'm a fy B Pharmacy student now and i have a lot of these concepts in Pharmaceutical Organic Chemistry. Thank you, professor for helping me understand these concepts easily! Your way of teaching is really good, I have my POC exam in 3 days, your channel is helping me a lot. TYSM. ✨️✨️✨️✨️✨️
At 9:48, wouldn't the + still be more stable on an oxygen compared to a carbon? Because a positively charged carbon has an incomplete octet whereas a positively charged oxygen has a complete octet.
@@ProfessorDaveExplains Your teaching is absolutely great Prof. Dave. But here, I have to tell you, that you are totally wrong. You can also check it with WebMO calculations, that kasra.b3316 is right with his assumption that the resonance structure with the positive charge on the carbon isn't the more important. The resonance structure with the positive charge on the oxygen atom is the more important, because when carbon bears a positive charge, it hasn't got a filled octet. And it is more important to have a full octet than to have a positive charge on the less electronegative atom. Ah, I see. There isn't a hydrogene bonded to the oxygene atom. Then you are right Dave. But this molecule probably won't exist or? Would it be more stable than a methyl cation?
@@ProfessorDaveExplains Yes, yes. As I edited above under my comment, I did see something wrong and you were right. I have seen a hydrogen bound on the oxygen (which isn't there). Probably I have seen the acid catalyzed mechanism of nucleophilic addition on carbonyl group too often ;-)
Thank YOU! Im currently trying to teach my self OChem. my book rushes to the point so i start to guess and then later become confused. Now i fully understand what im reading. This was probably the best academic video tutorial that i have seen. Very Clear and enjoyable!
@@keatodiet There was a lot to remember, but I'd say overall it went okay. I took ochem 1 and 2 as well as the lab in undergrad and I think I got at least B's. Now I work at a community college and mostly tutor students there, and it's been fun to revisit and brush up on some subjects. That's why I find myself coming back to these educational channels regularly.
at the beginning when you flipped the molecule(in order to view it edge on) why did you bound each of the two carbons to two hydrogen atoms aren't they supposed to be bound to carbon atoms (since you said in a previous class that the end points and vertex in the line notation of the molecule are carbon atoms )
ah i see what you mean, yes technically those are two different molecules! but i'm really just trying to illustrate how the orbitals work to make the pi bond so it's not really the focus there.
Professor dave you are really great but can you do a series of acids bases and the factors effecting them like inductive, steric effect etc etc. It will be a huge favour thank you.
Sir add some more video on organic nomenclature. some of it may be on aromatic amines , aldehyde or ke tones. and all that you know better, indeed because in our syllabus carbonyl and amines form a major section
Hello! I really appreciate your work, I'm currently studying biotech and your courses have been fundamental in my studying. I share your content with my classmates and teachers. Hope you continue to do great and happy new year!
*Help!* Something doesn't add up with C2O2 shown in 5:49 : If Oxigen has sp2 hybridization and 7 electrons, each of its three SP orbitals would bear a pair of electrons and the P orbital just one (so the pi bond is possible). However, if the 3 SP orbitals have each a pair of electrons the sigma bond would not be possible anymore (because the C wants to share its electron but the SP orbital of the O is already full). How does it work then? Thanks Prof Dave Explains community!
Hi thanks for the excellent explanation ❤️, but I have a doubt; In the nitrate ion what would be the most stable resonant form? Or they are equally stable?
when you explained how to determine if an atom would bear a formal charge, you said that you use the lewis dot structure and compare/contrast that to the typical valence electron number for that element. with that in mind, how come the oxygen atom that you demonstrated couldn't have also been deciphered as having a positive charge of 1? are we never to assume that it could have less than the typical valence unless the math makes that clear as in the case of the Nitrogen?
when drawing mechanisms, we sometimes start an arrow from a negative charge, in which case we are depicting the movement of a pair of electrons, but yes in the strictest sense, like on a monoatomic ion, it means one electron beyond its typical valence.
8:42 isn't the structure on the right with a positive formal charge on the oxygen invalid? the oxygen atom there has only 6 electrons and therefore it doesn't fullfill the octet rule
Assigning formal charge? More like "The educational quality of these videos is large!" Thanks again so much for making so many great videos on such a wide array of topics.
I have a question please answer Question in my book says choose a compound for which we can write a resonance structure? a)o3 (b)Nh3 (c)ch4 (d)h20 Answer is 03 But Nh3 can have resonance as well with N(-)double bond with one h having minus Help
@3.00 Why does the first Oxygen w/ the double bond get 2 lone pairs but the one w/ the single bond get 3? Must e- exist always in either bonds or pairs? Thanks a ton!
Sir;I have a doubt that in resonating structures when more electronegative element has positive charge and lesser one has negative charge then in that situation how does charge separation makes significance to it?I will feel glad if u answer my question.
With counting the electron pairs to determine formal charges, how do you know to add 2 or 3 electron pairs on Oxygen? For example in the part about resonance structures, you show 2 ions with the same structure, but different charges on the oxygen. One has 7 electrons in total 3 pairs and one sigma e, the other one had five, and thus a positive charge
Hey professor Dave , I didn't get you at 5:23 .You told that the negative sign is just a lone pair (2 electrons) , but "-1" means it has one electron more than it's valence electrons, so is it one electron or a pair of electrons?
It's both kind of! Oxygen has six valence electrons, so when it shows seven, from one covalent bond and three lone pairs, it has a negative charge. Then we sometimes draw arrows from a negative charge to indicate the activity of a lone pair. So the negative charge results in an extra lone pair.
I know it's been a long long while, but if you wanted to practice naming complex compounds, you can use this program: marvinjs-demo.chemaxon.com/latest/demo.html If you click the save button, and then select "Name" from the dropdown box, it'll show you the IUPAC name.
Professor I am from India . I am preparing for neet but I have totally confused in drawing lining Stuture of aromatic compounds please suggest me your video for this ❓❓❓❓❓✍️✍️✍️
I know it's been a long long time, but if you still wanted to practice naming complex compounds, you can use this program: marvinjs-demo.chemaxon.com/latest/demo.html If you click the save button, and then select "Name" from the dropdown box, it'll show you the IUPAC name.
@8:43 the first example with the primary carbocation, how were you able to move the pi electrons between oxygen and the central carbon without violating the octet rule on oxygen? It does not seem like it would be a reasonable resonance structure.
prof.Dave, in the last structure which includes Nitrogen in it, is there any reason for the electron came out from Nitrogen atom stopped its way on the middle of the structure, not going to the end just like other examples?
I think they mean how the curved arrow points from the positively charged nitrogen to the middle of the structure or where the carbon atom is. I have the same question, why does it go from that Nitrogen to the Carbon? Is it just because Carbon can be more electropositive?
oh, i see, so in that last one the arrow originates in the middle of the pi bond, and those pi electrons go over to the carbon. but this is a very poor resonance structure because there are two formal charges as opposed to a neutral molecule so it is almost not at all contributing to the overall structure.
Hey Prof. At 7:17 can we write delta -(ve) on both the oxygen atoms in the composite structure ?? And at 8:28 N=+(ve) while Oxygens have delta -(ve) ??
+yash pant kind of, you could put a half a charge on each oxygen, but really we just prefer to put a dashed line everywhere there's pi electron density and then just signify the magnitude of the formal charge outside of the brackets.
![[Re:all TREASURE] EP.6 in 방콕ㅣ🚩 쩡캠의 방콕 투어 빵 마이 와이 👍](http://i.ytimg.com/vi/uyFw-nItA_s/mqdefault.jpg)
Need OChem help? Find me and all the resources you need on Chemmunity: chemmunity.info/dave
You are a really good teacher ! I switched over "completely" to your videos after I seen the comments you posted on the mistakes made by Kahn academy. Anyway, when I was 16, I won first place on a questionnaire contest about chemistry, spec. the periodic table. Over the years after the military, and going from job to job, and then kids, found myself a 47 year old, still a fan of science, physics, biology, astronomy, and especially Chemistry. Wanted to refresh my knowledge of what I knew 30 years ago and learn even more than ever before. Your videos are informative and refreshing. You speak clearly, and get right to the point. Will donate to you in a month or so, after I get out of this slump ! Thanks again Dave ...
that's a heck of a success story for the passion of learning! many rounds of applause. thanks for watching! haha maybe i should leave a bunch more comments on the khan content, i didn't know it was getting me viewers!
Professor Dave Explains well it needed to be done ! One assumes that a course being taught is by the right person ! I MYSELF caught mistakes, but I'm sure he left a Hydrogen out. Also, I always thought Carbon was a stickler for the octet rule. That guy had a moment or short period of Carbon having a fifth Bond, I thought it couldn't, not even for a split second ... thanks again, See ya !
Damn...
@@pianodna-james3147 fr what a life
@@seanbergeron4251you are 54 now sir so how's your journey going 😊 ?
I would feel so much more justified if my tuition were going to you rather than my school
i will gladly take any monies that you are offering!
real talk
You should support him on patreon if you can.
I know it's been awhile, but I was just curious; how did college go?
This was so incredibly helpful! Professors forget the very basics sometimes and this made more complicated ideas much more manageable.
on the structure with nitrogen at 11:49 where did the electrons from the double bond go because they are not shown on the other structure.
This guy is the man. 10/10
I've commented the following comment about 5 times in other Prof. Dave comment sections. The quality of your content is so dang high that I believe you've earned a PhD. I'm calling it now: in the near future, I think a university will reward you for your hard work. You 100% deserve it.
In the meantime, I hope this channel earns you wealth & happiness. Thanks for making this, the educating of others, your life.
I like this way of finding formal charges WAY more than the arithmetic method. Thanks!
theres always someone trying to make it more complicated than it has to be xD... OR someone smarter who boils it down to its essence through understanding ;)
I must say.....your videos are helpful....our teachers in school suck..bt atleast you helped us...
So thank you...
Sahil Singh whats the name of your school and where are you from?
Life saver. Please keep being awesome. I think you're gonna be able to help me survive organic chemistry. Subcribed!
I got full marks in Organic Chemistry in Class 10 thanks to Professor Dave's Organic Chemistry playist .
@@ritsuafk How have your studies been going since then?
I know it's been a long long time, but I came across your comment and was curious. Did you indeed survive ochem?
Seriously, the most HELPFUL and easy-to-understand person out there. I grasped the concept within 4 minutes of watching your video. Something my Chem professor couldn't properly teach and help me understand within an hour and a half. THANK YOU!
Just lie down and learn chemistry. I do not even have to concentrate much because it goes straught into the mind. EQ and IQ together are potent!
When Christ returns to save your Chemistry Grade
not funny. you need to repent to God, sinner
Nikita Solomon go fuck yourself
@@Whitelivesmatter148ate You like your own reply .
Nice joke . Christ . XD Even Jesus will be laughing at it .
Some people instead of focusing on the love He showed us find pleasure in joking... it’s sad.
you officially just taught me more in ten minutes than two weeks of a ucla chem lecture did
You go to UCLA?!....can u write me some things u think got u in pls?
in the video C2H4 shown on the left has lines which represent bonds, since carbon is at the ends of lines the bonds shown would not be carbon-hydrogen but instead carbon-carbon.
Oh, you are very right. I found an other mistake which I will tell him separately. The resonance structure with the positive charge on the carbon isn't the more important. The resonance structure with the positive charge on the oxygen atom is the more important, because when carbon bears a positive charge, it hasn't got a filled octet. And it is more important to have a full octet than to have a positive charge on the less electronegative atom.
thank you sir through this video I got these concepts cleared in my mind :
-formal charge
-appropriate Lewis dot structure
- and definitely resonance hybrid and canonical structure
thanks a lot!
Everything Everything ........
u are way better than my university organic chemistry instructor.
I know it's been a long long time, but how did the rest of your ochem class(es) go?
Very very useful to me.thank you sir .from India 🇮🇳
thank you chemistry jeasus, your apprentice youtube led me to my needful video finally
Im from Germany and These explanations are mostly better and easier to understand than explanations in German
Love your intro and content. The intro lightens the mood and the content appears much easier to understand
🤐No words to explain how nicely u explained professor Dave you are great, 😀
🙌hands off sir
💗Love from India from your small fan💗
Does the hybridization of each atom remains the same for all the resonant structures?
nope it changes! so in the composite structure atoms sometimes have intermediate hybridizations, some character of one and some of another.
thankyou very much
I wish i had found your channel when I was preparing for NEET.
I'm a fy B Pharmacy student now and i have a lot of these concepts in Pharmaceutical Organic Chemistry. Thank you, professor for helping me understand these concepts easily! Your way of teaching is really good, I have my POC exam in 3 days, your channel is helping me a lot. TYSM. ✨️✨️✨️✨️✨️
sir plzx upload more videos on benzene reactions n other organic reactions
n ty soo much for all these videos ..they r very helpful
At 9:48, wouldn't the + still be more stable on an oxygen compared to a carbon? Because a positively charged carbon has an incomplete octet whereas a positively charged oxygen has a complete octet.
more stable on a carbon
@@ProfessorDaveExplains Your teaching is absolutely great Prof. Dave. But here, I have to tell you, that you are totally wrong. You can also check it with WebMO calculations, that kasra.b3316 is right with his assumption that the resonance structure with the positive charge on the carbon isn't the more important. The resonance structure with the positive charge on the oxygen atom is the more important, because when carbon bears a positive charge, it hasn't got a filled octet. And it is more important to have a full octet than to have a positive charge on the less electronegative atom.
Ah, I see. There isn't a hydrogene bonded to the oxygene atom. Then you are right Dave.
But this molecule probably won't exist or? Would it be more stable than a methyl cation?
@@nilsnickname4455 If that pi bond left the oxygen it also would not have an octet. The one with the carbocation is more stable.
@@ProfessorDaveExplains
Yes, yes. As I edited above under my comment, I did see something wrong and you were right.
I have seen a hydrogen bound on the oxygen (which isn't there).
Probably I have seen the acid catalyzed mechanism of nucleophilic addition on carbonyl group too often ;-)
Thank YOU! Im currently trying to teach my self OChem. my book rushes to the point so i start to guess and then later become confused. Now i fully understand what im reading. This was probably the best academic video tutorial that i have seen. Very Clear and enjoyable!
Yeah I agree Professor Dave is the best! I know it's been awhile, but I was just curious; how did learning ochem go?
@@PunmasterSTP left bro hanging 😢
@@keatodiet Yeah, not everyone gets back to me. But I have heard from a few people after more than a decade!
@@PunmasterSTP well then traveller, how did YOUR ochem journey go?
@@keatodiet There was a lot to remember, but I'd say overall it went okay. I took ochem 1 and 2 as well as the lab in undergrad and I think I got at least B's. Now I work at a community college and mostly tutor students there, and it's been fun to revisit and brush up on some subjects. That's why I find myself coming back to these educational channels regularly.
Even does the 'hang-loose' sign for the cooler members of his class at 38 sec and 50 sec... well done relating to your class.
at the beginning when you flipped the molecule(in order to view it edge on) why did you bound each of the two carbons to two hydrogen atoms aren't they supposed to be bound to carbon atoms (since you said in a previous class that the end points and vertex in the line notation of the molecule are carbon atoms )
ah i see what you mean, yes technically those are two different molecules! but i'm really just trying to illustrate how the orbitals work to make the pi bond so it's not really the focus there.
Pls sir which atom should be at d centre, is it the more electro positive or more electronegative
What an excellent explanation! It is tremendously satisfactory to be enlightened about such a confuse and a usually incorrectly presented topic.
Professor dave you are really great but can you do a series of acids bases and the factors effecting them like inductive, steric effect etc etc. It will be a huge favour thank you.
Sir add some more video on organic nomenclature. some of it may be on aromatic amines , aldehyde or ke tones. and all that you know better, indeed because in our syllabus carbonyl and amines form a major section
Hello! I really appreciate your work, I'm currently studying biotech and your courses have been fundamental in my studying. I share your content with my classmates and teachers. Hope you continue to do great and happy new year!
Hello
Professor, how would we represent the more "skewed" composite structures on diagrams? Do we just draw the more likely structure?
Great teacher. Love from India
*Help!* Something doesn't add up with C2O2 shown in 5:49 :
If Oxigen has sp2 hybridization and 7 electrons, each of its three SP orbitals would bear a pair of electrons and the P orbital just one (so the pi bond is possible). However, if the 3 SP orbitals have each a pair of electrons the sigma bond would not be possible anymore (because the C wants to share its electron but the SP orbital of the O is already full). How does it work then?
Thanks Prof Dave Explains community!
Hi thanks for the excellent explanation ❤️, but I have a doubt;
In the nitrate ion what would be the most stable resonant form? Or they are equally stable?
all equivalent
Precise and concise . Good work dave
when you explained how to determine if an atom would bear a formal charge, you said that you use the lewis dot structure and compare/contrast that to the typical valence electron number for that element. with that in mind, how come the oxygen atom that you demonstrated couldn't have also been deciphered as having a positive charge of 1? are we never to assume that it could have less than the typical valence unless the math makes that clear as in the case of the Nitrogen?
nm. went back and watched lewis dot structure tutorial you posted and it answered my question i think
@5:22, Prof. said that the negative charge implies a lone pair. But isn't it just an extra electron (not a pair)? Plz clarify!
when drawing mechanisms, we sometimes start an arrow from a negative charge, in which case we are depicting the movement of a pair of electrons, but yes in the strictest sense, like on a monoatomic ion, it means one electron beyond its typical valence.
@@ProfessorDaveExplains ❤
Best chem teacher on the net
I tried to understand this with another video, and I got confused. This was perfect. I'll come back for more chemistry.
8:42 isn't the structure on the right with a positive formal charge on the oxygen invalid? the oxygen atom there has only 6 electrons and therefore it doesn't fullfill the octet rule
Carbocations don't have a full octet either. Don't worry about the octet rule, it's sort of meaningless.
What a beautiful man.
I literally cannot focus lol been "watching" for 5 minutes and actually didn't listen a single word lmao
thanks for explaining what my professor didn't
you just explained this so fast and so easily!!! phewks, I can now do my O.chem exam, thanks!
I know it's been awhile, but how did your exam go?
U teach good with very less time feeling so interested to listen ur lectures keep going
Thank you very much DAVE !!!!!!!
I finally understand this. THANK YOU DAVE!
Thank you very much for nice explanation
Assigning formal charge? More like "The educational quality of these videos is large!" Thanks again so much for making so many great videos on such a wide array of topics.
I have a question please answer
Question in my book says choose a compound for which we can write a resonance structure?
a)o3 (b)Nh3 (c)ch4 (d)h20
Answer is 03
But Nh3 can have resonance as well with N(-)double bond with one h having minus
Help
nope, hydrogen can't accommodate a second bond!
@@ProfessorDaveExplains oookk
Yeah thanks for replying though appreciate it!
I love your teaching. ❤
But please can I get a statement of what the resonance theory is? The “theory “
Please 🙏.
Thank you so much for your helpful videos!
Your point at #11:03 really cleared things up. THANKS! told about these videos to my classmates and they like it!
Your biochemistry videos are excellent really!
I know it's been a long long time, but how did your classes go?
Still Legendary!! Helped me understand a topic I have been struggling with for so long.
The professors at the university where I studied could've learned a thing or two from this professor.
@3.00 Why does the first Oxygen w/ the double bond get 2 lone pairs but the one w/ the single bond get 3? Must e- exist always in either bonds or pairs? Thanks a ton!
Usually, unpaired electrons exist in radicals, those show up later in the playlist.
@@ProfessorDaveExplains Thanks for the fast reply, I appreciate it professor Dave!
Sir;I have a doubt that in resonating structures when more electronegative element has positive charge and lesser one has negative charge then in that situation how does charge separation makes significance to it?I will feel glad if u answer my question.
i'm not sure i understand the question, i just know that electronegative elements are better at accommodating negative charge than positive
Very nicely explained Sir🙏
With counting the electron pairs to determine formal charges, how do you know to add 2 or 3 electron pairs on Oxygen? For example in the part about resonance structures, you show 2 ions with the same structure, but different charges on the oxygen. One has 7 electrons in total 3 pairs and one sigma e, the other one had five, and thus a positive charge
Sir , is it possible to calculate the number of resonating structures of a molecule without even drawing these stuffs ??
hmm, not that i'm aware of, it's not really calculation-based, you just have to push electrons around!
this channel helps me a lot , really . thank you so much, gonna recommend this to some friends.😉😉😉
woohoo! tell them to subscribe!
You are saving my life!!! Thank you so much - watching all your videos
How have your studies been going?
no one can compete this man
#ProfesserDaveThe Best
i love the way it starts....
Tyler Dewitt is the best any ways
Beautiful lecture
Hey professor Dave , I didn't get you at 5:23 .You told that the negative sign is just a lone pair (2 electrons) , but "-1" means it has one electron more than it's valence electrons, so is it one electron or a pair of electrons?
It's both kind of! Oxygen has six valence electrons, so when it shows seven, from one covalent bond and three lone pairs, it has a negative charge. Then we sometimes draw arrows from a negative charge to indicate the activity of a lone pair. So the negative charge results in an extra lone pair.
Professor Dave Explains Thank you so much Professor Dave! Thanks for replying so quick ! You are the best!
Thank you very much for your sincere efforts.
thank you soooo much!! it is amazing that I understood it so easily!!!
김현숙 안녕하세요! 한국 사람??
Guess i should have paid you than pay for my school. This man is so much better than my teachers. Thank you so much, Professor Dave.
i will gladly accept any monetary gratitudes at my patreon page!!
Thank you so much professor...this helped a lot.
Thanks sir 👍
I have a CLEP test today. Thank you so much!
one suggestion please upload complex compounds also
otherwise it is very good
I know it's been a long long while, but if you wanted to practice naming complex compounds, you can use this program:
marvinjs-demo.chemaxon.com/latest/demo.html
If you click the save button, and then select "Name" from the dropdown box, it'll show you the IUPAC name.
Professor I am from India . I am preparing for neet but I have totally confused in drawing lining Stuture of aromatic compounds please suggest me your video for this ❓❓❓❓❓✍️✍️✍️
Materi ttg sigma, pi, dan formal charge ada di GC Lewis dot structure
wish I knew about your classes earlier..anyway glad I found this now😀
this is your best video so far
could you please make a video on the iupac naming of polyfunctional group containing organic compounds.
i've got 5 tutorials on IUPAC nomenclature! check them out.
I know it's been a long long time, but if you still wanted to practice naming complex compounds, you can use this program:
marvinjs-demo.chemaxon.com/latest/demo.html
If you click the save button, and then select "Name" from the dropdown box, it'll show you the IUPAC name.
@8:43 the first example with the primary carbocation, how were you able to move the pi electrons between oxygen and the central carbon without violating the octet rule on oxygen? It does not seem like it would be a reasonable resonance structure.
u are really saving me in my first year in med school
Sir how to determine stability of resonance structure
Dave, my friend, you are my hero. Thank you !
so beautifully explained...
prof.Dave, in the last structure which includes Nitrogen in it, is there any reason for the electron came out from Nitrogen atom stopped its way on the middle of the structure, not going to the end just like other examples?
+Hyein Song i'm not sure i understand, going to the end of what?
I think they mean how the curved arrow points from the positively charged nitrogen to the middle of the structure or where the carbon atom is. I have the same question, why does it go from that Nitrogen to the Carbon? Is it just because Carbon can be more electropositive?
oh, i see, so in that last one the arrow originates in the middle of the pi bond, and those pi electrons go over to the carbon. but this is a very poor resonance structure because there are two formal charges as opposed to a neutral molecule so it is almost not at all contributing to the overall structure.
Got it now! Thank you! You're saving my Ochem test grade for tomorrow! haha
@@beesbee1 I know it's been a long long time, but I just came across your comment and was curious. How did your ochem test go?
You are great sir
In the last question 11:25 , is sp2 C more electronegative than sp2 nitrogen? Bcoz you shifted the pi electron to sp2 C atom.
studying for a big ap chem test tomorrow... totally forgot what formal charge was. god bless.
Thank you Professor Jesus for the explanation 🥺
thank you so much prof Dave
Hey Prof. At 7:17 can we write delta -(ve) on both the oxygen atoms in the composite structure ?? And at 8:28 N=+(ve) while Oxygens have delta -(ve) ??
+yash pant kind of, you could put a half a charge on each oxygen, but really we just prefer to put a dashed line everywhere there's pi electron density and then just signify the magnitude of the formal charge outside of the brackets.
Finally understanding this! Thanks so much :)
Ah so this is gonna be my professor for the next 4 months!
How'd your classes go?
So well explained, thanks Dave!
thank you you are save me you are so amazing 😍 another time thank you 👨🏫
You're awesome prof!
You made so easy thank you
sir plz can you explain about hyperconjugation?
sir u are a life saver
He teaches the short topic better than many college professors.
What about s-p mixing in NO3-