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.
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
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.....
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.
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
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?
U say that the formal charge is the number of electrons it brought - the number of electrons it has, but when U calculate that later, the sulphur actually gets a -6 F.C, I am confused ༼;´༎ຶ ༎ຶ༽
Christopher Sutton Technically yes, but steric factors, such as each electron's same charge repelling each other, keep atoms from completely filling up their d-shell
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.. 🤗🤗🤗
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.
moreover i dont understand this method oxygen must have 5 electrons after making bond with sulphur why did u just put total valence electrons after bonding
+Emma 1 Because it is in a bond, he uses a nice way to determine the formal charge; but you can actually use this formula if you're uncomfortable with his method - Formal Charge = V - L - 0.5*S V -> No. of valence electrons L -> No. of Lone Pair electrons S -> Electrons in bond formation
+Emma 1 think of it this way the electrons are moving around in the bond, there are two atoms sharing the electrons, and in average, if you divide the space the bond covers into the parts the atoms have themselves, the atoms have "half" the electrons on their own side. But they also have both the electrons in their clouds because they have them going back and forth in the bond
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!
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
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.
Anyone Here In 2024
🙋♀️
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 🙏
This is amazing. Even though English is not my native language I think this will save my exams
omg, the only video on TH-cam to actually explain FC
You are the best teacher man. Please continue to help people who had almost given up on chemistry !😊
Thank you! I just understood how the formal charges help to get a correct drawing and why.
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
Thank you so much. You helped me understand this when no one else could.
I wish I could get him as my chemistry teacher 😍😍😍
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
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?
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 :)
Super super teaching👍👍👍,thank you so much sir.From Manipur
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.....
Thank you so much, this video was only 6 minutes long but it cleared up an hour of confusion I had in class!
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.
Thanks teacher l al from morocco🇲🇦✌️
This video actually saved my life.. In the today's exam we had that👀
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..?
Im from Saudi Arabia and i wanna say that ur video is the bestttttt thaaaaaaaank u so soooo much😭😭😭😭❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️
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?
Thanks sir, I'm from Bangladesh,,love from my country ❤❤
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
only video that i've actually understood thank you
Excellent explaination 💟💟 God bless u sir
the most accurate explanation ngl love it!!!
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
omg i finally see the light.. thank you!
umm doesn't a bond count as 2 electrons? If each carbon brought 6 electrons + the bond wouldn't that be 8 electrons?
OMG! So helpful for my biochem undergrad
Thank you! :)
10 year old video and still helping a high schooler like me :3
beautiful explanaition, can i cry now?
I understood this thanks to you ! Keep up the good work
yaaaaaaaaaa
So we want the center atom the have zero or close to zero charge, like is that prioritized over the charge of other electrons?
Good explanation. Easy to understand, thanks. 👍👍
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
Thank u so muchhh. What my chem teacher didn't!!!
Oxygen has valence 6 and it is mention in the video, but why is it written/counted as only 4
I don't understand in SO4 here 4 is there for which thing either for valency or for electrons . Please tell!
You explained it in such simple terms thank u so much
the video was uploaded in 2013 but it's about to reach 2025, but it is helpful yet. that's so good.
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?
Tal vez no me entiendas pero ¿Por que no pudo generar dos enlaces dativos el "S"?
Your videos help me SO MUCH! THANK YOU!!!!!
thank you, it is very beneficial to prepare petrucci general chemistry chapter 10
But you have not talked about the -2 charge around the bracket
thank you for your video!THIS IS REALLY HELPFUL!
How is the octetrule fulfilled on the Oxygen and the Sulfur?
Can you please tell me the number of lone pair and bond pair of electrons in this ion... Please
what after when you draw the structure out, how do you know what to name it? The names consist of tetrahedral, pyramidal and stuff like that
Is there a list somewhere of which elements can break the octet rule?
Also my "people" (which is Aktiv Chemistry) say that 2 is the incorrect number of resonance structures.😭
Dang! Do they say it's 6 ? Which is EVERY combination of 2 double bonds + 2 single bonds around the sulfur?
@@chemistNATE Been a few days but yes, I think they wanted all 6
I am indian ...thank you very much for this video
You have really cleared my concept
the two additional electrons are from where?
U say that the formal charge is the number of electrons it brought - the number of electrons it has, but when U calculate that later, the sulphur actually gets a -6 F.C, I am confused ༼;´༎ຶ ༎ຶ༽
This was so helpful. I cannot thank you enough!
If the other oxygen has 1 bond why didnt u added another 2 bonds bw them
why is sulfur only allowed 6 bonds? shouldnt it be able to fill its d-shell, up to 18 electrons?
Christopher Sutton Technically yes, but steric factors, such as each electron's same charge repelling each other, keep atoms from completely filling up their d-shell
thanks for you , but I have question ..how no. of electron on O atom still 6 electron and form abond with S???
Because according to the octet rule, it tends to have 8 electrons around it's atom
mesa 3aleek :D
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...
Why must formal charge be as close to zero as possible?
This cleared my understanding of this topic
You didn't count the electrons afterwards to equal 32. Or explain.
Does this molecule has dative bond?????how???
Very helpful man. Thanks for helping me understand what my instructor didnt. Lol
Why we have to change the formal charge??? Please help me
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.
I think this video was made for me only ... ty soo much my doubt got clear ty
Amazing!! Você explica muito!!! Thank you!!
moreover i dont understand this method oxygen must have 5 electrons after making bond with sulphur why did u just put total valence electrons after bonding
Thorough and very helpful. Thank you!
THANK YOU
I finally get it!
Finally got it😊😊 Thank u soo much☺☺
Does it follow the octet rule ?
why didnt you just have double bonds on all four oxygens?
Thank you sir for the excellent explaination
Wow amazing thank you
Thank you Sir
Shouldn't we also consider number of bonds
you saved my life, thanks!!!
That was a great explanation, thank you!
WHYYYY YOU ARE NOT MY TEACHERRRRRRR WHYYYY .. Thank you so so very very much
Do the oxygen atoms remain in resonance ?????
Please reply. ...
I really want to Know .
And and and Your have such a great video .
bitch lasagna
EXCELLENT EXPLANATION 👍👍😃😃
why do you take 2 electrons and than take it like 1 electron?
+Emma 1
Because it is in a bond, he uses a nice way to determine the formal charge; but you can actually use this formula if you're uncomfortable with his method -
Formal Charge = V - L - 0.5*S
V -> No. of valence electrons
L -> No. of Lone Pair electrons
S -> Electrons in bond formation
Thnx Aditya Prakash
+Emma 1 think of it this way
the electrons are moving around in the bond, there are two atoms sharing the electrons, and in average, if you divide the space the bond covers into the parts the atoms have themselves, the atoms have "half" the electrons on their own side. But they also have both the electrons in their clouds because they have them going back and forth in the bond
+Braxium thnx
I think i love chemistry a little bit now :)
Hlo ,how to know no of dative bonds?
But Sir how sulphur can have 10 electrons there.........please please tell me please....I am very confused here please 🥺🥺🥺🥺🥺
Sir please tell me
תודה אחי. עזרת לי.
אתה מסביר מעולה.