This video was posted in 2013, but in 2021 - It's helping me to fully ingest some key points I missed when I first took gen-chem in undergrad. Thank you.
This is ABSOLUTELY the ONLY video I have ever seen that completely explains formal charges in resonance structures!!!!!! THANK YOU THANK YOU THANK YOU. I could cry of happiness :')
Hey, thank you so much. You don't know how great your help have been during these lockdown days. I pray that you are safe. Thanks for showing it step by step. I couldn't grasp in my class and I was very scared to ask the teacher. I can't thank you enough for this.
Thank you!!! This helped so much! I was always confused as to why the molecules would become a double bond but now it’s all clear. Thanks great teaching :)
What about dative bond...? Sir I'm from India....I don't see any other videos of you ....but by waching only this video I'm very sure that ur a best chemistry tr.....thank uu sir.....
Elements in Period 3 and higher (i.e. periods 4, 5..) can "expand the octet". In simple terms, their outer shells can accommodate more than 8 electrons. It happens commonly in P, S, Cl, Br and I
great video!! I have a question though... when drawing the lewis structure you put the element with the least electronegativity in the middle? or the most electronegative? my professor told us the most electronegative..?
Hi sir, your videos is very much useful, I have doubt that how can we know that the formal charge should be used & also how can we confirm that the picture of sulphur to oxygen in a single bond is correct or wrong, please can you clarify my doubt Thanking you
You said that there was only one resonance structure, Would it not work if any of the two bonds were double bonds? in which case there would be 6 structures that fit.
PLZ help with chem. I got some questions. 1. When counting the original number of electrons, you add the plus two from the extra two electrons. Why is that? Do you just go with it because it's given? Is there a reason as to why the extra two electrons are there to begin with? Like... where tf did they come from? 2. Why is the octet rule being broken for Sulfur? Is it because of the row it's in? 3.Originally I thought that once the Sulfur had 8 electrons when connected to Oxygens (at the beginning), the remaining two electrons Sulfur had would transfer over to an oxygen. I know this wouldn't work, but could someone explain why? Chemistry is one of those subjects that I consider so easy... that it's insanely difficult. Be it from overthinking or from thinking of something unrelated when looking at chem.
Hello Sir as you have explained that F.C. = no. Of e-* brought minus no. Of e- have or has but sir actually the fomula is like this F.C. = total no. Of e- minus total no. Of non bonding e- minus half of no. Of no bonding e-.. (*e- is electron)..Actually I was trying to draw Lewis structure clf3 molecule at that time come across this formula..from above your mentioned formula we cant draw Lewis structure for CLF 3.. 🤗🤗🤗
How can you have cumulated pi bonds on sulfur without forcing a linear bond geometry? I am especially confused since it has been shown (about 1990) that d orbitals do not actually participate in hybridization?
This video was posted in 2013, but in 2021 - It's helping me to fully ingest some key points I missed when I first took gen-chem in undergrad. Thank you.
Bro can u tell me how many lone and bond pairs are present in so4^2-
So do i 🤣😇🥰
@@theunderdogstg808
bond pair = 6
Lone pair = 10
Now 2023 😮
@@AnshuEXCELnow 2024
This is ABSOLUTELY the ONLY video I have ever seen that completely explains formal charges in resonance structures!!!!!! THANK YOU THANK YOU THANK YOU. I could cry of happiness :')
You're an excellent teacher. Thanks for breaking this down step by step and using such clear language! :)
You're the only one that made this make sense! Thank you so much
Hey, thank you so much. You don't know how great your help have been during these lockdown days. I pray that you are safe. Thanks for showing it step by step. I couldn't grasp in my class and I was very scared to ask the teacher. I can't thank you enough for this.
Self teaching is getting huge right now. Thanks for the encouragement.
I'm French and you're my chem savior. Thank you, thank you, THANK YOU.
Oh finally, a sigh of relief. That was a great explanation!
Thanks! This was one of those few videos which was perfect for me. It was crisp and precise and delivered what it had to. Thanks once again.
OMG, THIS IS THE BESTexplanation video ever and the SMARTEST. Omg, I can't believe how simple and clear it is now for me to understand. THANK YOU
You are the best teacher man. Please continue to help people who had almost given up on chemistry !😊
For anyone that may be confused, 3rd period elements and beyond can sometimes have their d orbitals become involved in bonding.
+DefeatedSkeptic I don't think people learning this have learned about hybridization and pi-bonding with the lone d-orbital yet
One of the easiest way to write Lewis dot structure I have ever found in youtube 👍👍thank you so much sir 🙏
omg, the only video on RUclips to actually explain FC
Thank you very much! I wish you were at my college as a Chem tutor you're so helpful!
meeoun adjani Thanks! What College, and are they hiring? :D
+chemistNATE
so sulfur has 12 electrons
college? lol i have to study this shit at school
Yup
Welcome to crazy lol
Anyone Here In 2024
🙋♀️
and now 2025😮
Thank you! I just understood how the formal charges help to get a correct drawing and why.
This is amazing. Even though English is not my native language I think this will save my exams
Thank you!!! This helped so much! I was always confused as to why the molecules would become a double bond but now it’s all clear. Thanks great teaching :)
Thank you so much, this video was only 6 minutes long but it cleared up an hour of confusion I had in class!
Thank you so much. You helped me understand this when no one else could.
I wish I could get him as my chemistry teacher 😍😍😍
Thanks teacher l al from morocco🇲🇦✌️
THANK YOU SO MUCH! this cleared my doubt
especially u even told the formal charge on sulfur
years ago , i watched some of ur videos and aced my chemistry exam ,
u literally saved my life back then ! :D
the most accurate explanation ngl love it!!!
Super super teaching👍👍👍,thank you so much sir.From Manipur
only video that i've actually understood thank you
This video actually saved my life.. In the today's exam we had that👀
Im from Saudi Arabia and i wanna say that ur video is the bestttttt thaaaaaaaank u so soooo much😭😭😭😭❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️
Thank u so muchhh. What my chem teacher didn't!!!
Excellent explaination 💟💟 God bless u sir
the video was uploaded in 2013 but it's about to reach 2025, but it is helpful yet. that's so good.
omg i finally see the light.. thank you!
I understood this thanks to you ! Keep up the good work
yaaaaaaaaaa
You explained it in such simple terms thank u so much
What about dative bond...?
Sir I'm from India....I don't see any other videos of you ....but by waching only this video I'm very sure that ur a best chemistry tr.....thank uu sir.....
Thanks sir, I'm from Bangladesh,,love from my country ❤❤
You have really cleared my concept
OMG! So helpful for my biochem undergrad
Thank you! :)
Good explanation. Easy to understand, thanks. 👍👍
Thank you Sir
Thank you for the video. I have a question though. Why can't we have 4 double bonds instead and thus only S will have -2 formal charge?
beautiful explanaition, can i cry now?
Your videos help me SO MUCH! THANK YOU!!!!!
why sulphur has 12 electrons in the outermost shell where u can only have 8 electrons
As mentioned by him, sulphur can break the octate rule
It has 3d orbital which can accommodate more electrons
Elements in Period 3 and higher (i.e. periods 4, 5..) can "expand the octet". In simple terms, their outer shells can accommodate more than 8 electrons. It happens commonly in P, S, Cl, Br and I
Sulphur has valence shell no equal to 3 so it also has 3d orbital in which it can accommodate extra electron
Wow amazing thank you
thank you for your video!THIS IS REALLY HELPFUL!
thank you, it is very beneficial to prepare petrucci general chemistry chapter 10
great video!! I have a question though... when drawing the lewis structure you put the element with the least electronegativity in the middle? or the most electronegative? my professor told us the most electronegative..?
Hi sir, your videos is very much useful, I have doubt that how can we know that the formal charge should be used & also how can we confirm that the picture of sulphur to oxygen in a single bond is correct or wrong, please can you clarify my doubt
Thanking you
You said that there was only one resonance structure, Would it not work if any of the two bonds were double bonds? in which case there would be 6 structures that fit.
This was so helpful. I cannot thank you enough!
If we make third oxygen double bond along with the two we have made. Wudnt it further lower the formal charge.. And sulphur can expand octet
This cleared my understanding of this topic
When this video was uploaded I was not that tym on earth 😂
Amazing!! Você explica muito!!! Thank you!!
THANK YOU
I finally get it!
Very helpful man. Thanks for helping me understand what my instructor didnt. Lol
תודה אחי. עזרת לי.
אתה מסביר מעולה.
I just saw this right now, thank youu
The sulfate ion now does not satisfy the covalency. Sulphate has covalence two, but now in this drawing 4 electron pairs. How is that possible?
I am confused by that also. Has 6 valence electrons but how did he get only 4?
Finally got it😊😊 Thank u soo much☺☺
I think this video was made for me only ... ty soo much my doubt got clear ty
finally got it, thank you so much!
Thank you sir for the excellent explaination
you saved my life, thanks!!!
umm doesn't a bond count as 2 electrons? If each carbon brought 6 electrons + the bond wouldn't that be 8 electrons?
Thorough and very helpful. Thank you!
EXCELLENT EXPLANATION 👍👍😃😃
Excellent
How is the octetrule fulfilled on the Oxygen and the Sulfur?
Oxygen has valence 6 and it is mention in the video, but why is it written/counted as only 4
the best I have seen
But you have not talked about the -2 charge around the bracket
That was a great explanation, thank you!
Excellent 👍
I am indian ...thank you very much for this video
I think i love chemistry a little bit now :)
Thank you !!! It's way more clear now !!!
bro bless up my teacher is too stupid to explain this
PLZ help with chem. I got some questions.
1. When counting the original number of electrons, you add the plus two from the extra two electrons. Why is that? Do you just go with it because it's given? Is there a reason as to why the extra two electrons are there to begin with? Like... where tf did they come from?
2. Why is the octet rule being broken for Sulfur? Is it because of the row it's in?
3.Originally I thought that once the Sulfur had 8 electrons when connected to Oxygens (at the beginning), the remaining two electrons Sulfur had would transfer over to an oxygen. I know this wouldn't work, but could someone explain why?
Chemistry is one of those subjects that I consider so easy... that it's insanely difficult. Be it from overthinking or from thinking of something unrelated when looking at chem.
lets go Mr.oldridge aka Chemist Nate
So we want the center atom the have zero or close to zero charge, like is that prioritized over the charge of other electrons?
I don't understand in SO4 here 4 is there for which thing either for valency or for electrons . Please tell!
Iam from lraq ,thank you very much 💜
the two additional electrons are from where?
Great video it's help me very much !
Why must formal charge be as close to zero as possible?
Hello Sir as you have explained that F.C. = no. Of e-* brought minus no. Of e- have or has but sir actually the fomula is like this
F.C. = total no. Of e- minus total no. Of non bonding e- minus half of no. Of no bonding e-..
(*e- is electron)..Actually I was trying to draw Lewis structure clf3 molecule at that time come across this formula..from above your mentioned formula we cant draw Lewis structure for CLF 3.. 🤗🤗🤗
that comes to exactly the same...
Thank you so much its helped me a lot
Many thanks for this great video! xoxo
How can you have cumulated pi bonds on sulfur without forcing a linear bond geometry? I am especially confused since it has been shown (about 1990) that d orbitals do not actually participate in hybridization?
You didn't count the electrons afterwards to equal 32. Or explain.
Can you please tell me the number of lone pair and bond pair of electrons in this ion... Please
That was awesome 💯👏
you're the best.
WHYYYY YOU ARE NOT MY TEACHERRRRRRR WHYYYY .. Thank you so so very very much
This video is too good
Very gamer of you. Thanks.
So clear❤❤