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 :')
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 :)
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
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.
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 ༼;´༎ຶ ༎ຶ༽
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..?
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.
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?
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.
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
Yep. Americans say sulfur British English say sulphur kind of like gray and grey. Honestly speak though no one really uses Sulphur anymore. It's obsolete and even google's spell check is telling me sulphur is misspelled as I type this and recommending Sulfur instead. Kind of like how gay isn't used as a synonym of happy, people don't use sulphur to describe the element... unless you're old as dirt. Sorry to the other guy, I mean no harm... just saying...
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.....
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
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
You're the only one that made this make sense! Thank you so much
Anyone Here In 2024
🙋♀️
You're an excellent teacher. Thanks for breaking this down step by step and using such clear language! :)
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.
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
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 :')
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 :)
the most accurate explanation ngl love it!!!
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
Oh finally, a sigh of relief. That was a great explanation!
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.
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 ༼;´༎ຶ ༎ຶ༽
so sulfur has 12 electrons
It’s an example of expanded octet......one of the limitations of LDS......such as in IF7.....SF6 etc....
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
only video that i've actually understood thank you
You explained it in such simple terms thank u so much
You have really cleared my concept
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..?
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?
This was so helpful. I cannot thank you enough!
I'm French and you're my chem savior. Thank you, thank you, THANK YOU.
bro bless up my teacher is too stupid to explain this
But sir you should draw 2 lines to indicate double bond
umm doesn't a bond count as 2 electrons? If each carbon brought 6 electrons + the bond wouldn't that be 8 electrons?
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.
omg i finally see the light.. thank you!
Thanks teacher l al from morocco🇲🇦✌️
I wish I could get him as my chemistry teacher 😍😍😍
Thank you sir for the excellent explaination
Thank you! I just understood how the formal charges help to get a correct drawing and why.
Thorough and very helpful. Thank you!
I am indian ...thank you very much for this video
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?
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
Very helpful man. Thanks for helping me understand what my instructor didnt. Lol
THANK YOU
I finally get it!
Hindi wala hai kya koi 😂 full english smjh nhi ayi... Smjhaya to acha th .. 😅
Shouldn't we also consider number of bonds
If the other oxygen has 1 bond why didnt u added another 2 bonds bw them
finally got it, thank you so much!
WHYYYY YOU ARE NOT MY TEACHERRRRRRR WHYYYY .. Thank you so so very very much
I don't understand in SO4 here 4 is there for which thing either for valency or for electrons . Please tell!
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 are the best teacher man. Please continue to help people who had almost given up on chemistry !😊
Thank you Sir
Wow amazing thank you
Excellent explaination 💟💟 God bless u sir
I think i love chemistry a little bit now :)
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.
Does this molecule has dative bond?????how???
thank you for your video!THIS IS REALLY HELPFUL!
Amazing!! Você explica muito!!! Thank you!!
Excellent 👍
Thanks sir, I'm from Bangladesh,,love from my country ❤❤
You didn't count the electrons afterwards to equal 32. Or explain.
Your videos help me SO MUCH! THANK YOU!!!!!
When this video was uploaded I was not that tym on earth 😂
I understood this thanks to you ! Keep up the good work
yaaaaaaaaaa
Oxygen has valence 6 and it is mention in the video, but why is it written/counted as only 4
Thank you so much its helped me a lot
I got this question wrong on my test. Apparently 2 double bonds is wrong 🤔
Can you please tell me the number of lone pair and bond pair of electrons in this ion... Please
awesome expliantion
I think this video was made for me only ... ty soo much my doubt got clear ty
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 is the octetrule fulfilled on the Oxygen and the Sulfur?
But oxygen brought 7 electrons and had 8 later on
I don't understand 🙄
10 year old video and still helping a high schooler like me :3
But you have not talked about the -2 charge around the bracket
24+2 is 26 how did 32 come
so sulfur has 12 electrons
Jujulay Ju *sulphur
Spelled both ways actually.
LOL
Yep. Americans say sulfur British English say sulphur kind of like gray and grey. Honestly speak though no one really uses Sulphur anymore. It's obsolete and even google's spell check is telling me sulphur is misspelled as I type this and recommending Sulfur instead. Kind of like how gay isn't used as a synonym of happy, people don't use sulphur to describe the element... unless you're old as dirt. Sorry to the other guy, I mean no harm... just saying...
yeap. thanks john. :) >_
But Sir how sulphur can have 10 electrons there.........please please tell me please....I am very confused here please 🥺🥺🥺🥺🥺
Sir please tell me
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 u so muchhh. What my chem teacher didn't!!!
Why must formal charge be as close to zero as possible?
Sir, "Electrons brought" means "valence electrons"????😓
Wow wonderfull I understand it easily
lets go Mr.oldridge aka Chemist Nate
There are more than 2 resonance structures for sulfate!
So we want the center atom the have zero or close to zero charge, like is that prioritized over the charge of other electrons?
Thank you😊.
So confusing why sulphur has 10 electrons and how oxygen has 6 valence electrons which remains with him and shares the 7 th how is this possible
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
Bro why is the sulfur not following octet
Super super teaching👍👍👍,thank you so much sir.From Manipur
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😭😭😭😭❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️❤️
Bless you!
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
I don't understand why S have 6
Very gamer of you. Thanks.
I just saw this right now, thank youu
It actually has 6 Resonance structure.
+Sadegh Ayoubi Agreed. There should be six resonance structures if we go through all the possible arrangements.
your hands look like a pale version of donald trump's hands
THANK YOU SO MUCH! this cleared my doubt
especially u even told the formal charge on sulfur
But how so4 has 2 negative ion
Hlo ,how to know no of dative bonds?
Seen once. Shall be seen again.