Lewis Structure of SO2 (sulfur dioxide)

[@nourahkhaled6161]

Imagine this man explaining life to me

[@helixrelicsshow9651]

Respect

[@kabeersahu3017]

Nice pic of kaneki ken!😏

[@moncefalger5596]

M9stihach

[@little_fish_x]

Hey weeb...😂😂

[@itriied5027]

A simple 5-minute lesson on SO2 cleared up EVERYTHING. Thank you so much! :)

[@BlueKermit27]

Same, I couldn’t understand why only one oxygen had a double bond, and therefore I didn’t know why it was a bent rather than linear VSEPR. Looks like I have to review my Lewis structures!

[@maglev2000]

I am so confused right now. Everything I know about chemistry is a lie.

[@shirishaaloorkar6487]

It's true

[@SanjivKumar-bf1oz]

I am also confused

[@quanhonson9746]

This is actually pretty easy

[@equinoxboy]

XD your right

[@आयुष-न5ब]

@Luis Chavez share the 2 electron with 2 electron of any other element

[@ahintea]

This depends if you have learned about formal charge. This is correct for earlier stages of learning chemistry. I even asked my teacher about resonacne and formal charge, and they wont teach it to us, i dont know why but that means that structures we draw are actually wrong.

[@divya6050]

I really wish my chemistry teachers were more like you...thank you for the video!!

[@dfshjb44]

This seems correct to me. I always learned valence electrons desired - valence electrons available = valence electrons needed/2 = # of bonds in the structure. So S and O want 8 electrons, so that's 24 electrons desired. They're both in group 6, so S=6, (2)O=12. 6+12=18 electrons available. 24-18=6. 6/2=3 bonds used in the structure. The structure in the video has 3 bonds.

[@TheCANALpololey]

You learned me in 4 minutes something that my chemistry teacher hasn’t be able to explain me at all. Thanks a lot ! PS: I’m french and you speak very clearly so it’s easy for me to understand, thanks again

[@swarnimranabhat4]

Me tooo

[@rakshita888]

Ohh bonjour ❤

[@قاسمابوالخير-ظ1ض]

I am Palestinian. You explained this very clearly. Thank you 🤍🤍

[@donkeyparadise9276]

What is Palestine

[@seanhipe]

It's because of the octet rule, thanks for the explanation.

[@driraasch2951]

You made me learn something that i never undestood, i can't believe that i finally got it, thanks!!!! btw, im from brazil, so thanks for speak very clearly

[@talesamaral3744]

Salve

[@guilhermevitalidecamargo6371]

Salve

[@gamerplus9884]

Hi I like you can we talk?

[@Mr-ep2qi]

Damn he punked us at the end lol

[@davideisenstadt3745]

I believe this is wrong, Sulfur can utilize d orbitals to expand it's octet, so both oxygens would be double bonded to sulfur WITH a lone pair on sulfur as well as to have no formal charge on anything.

[@Elcompalui712]

yes hes wrong

[@AdityaSingh-ly9ku]

I am not saying that this structure is wrong but it is less stable and in competitive exams your marks will be deduced for this kind of structure, there will be two double bond between oxygen and sulfer atom, sulfer atom will have 10 electrons which is the most stable as sulfer is stable at covalency 2 4 6 and here it is 4. While octect rule is not followed here having extended octect rule. One more thing that this structure will have 0 formal charge in all atoms which more stable than having any charges.

[@OperationRevelation]

once again, the best explanation. thanks nate!

[@kenkentaylor9690]

I needed a refresher on how the double bond gets on either side and this helped! HAH was not expecting the ending but instantly subbed

[@SKGaming7-7-7]

that was very helpfulThe assistance you provided was extremely beneficial.

[@jennifergarnica3117]

"who's your daddy" smh lmaoooooo

[@user-vx1zs1zt8o]

jennifer garnica I watched the whole video just to hear him say it lmao

[@elisabettaakrong3604]

🤣 @@user-vx1zs1zt8o

[@moksusu61]

Best video to explain this concept. quick but easy to understand

[@maibee123]

oh my god i’ve been so confused and finally found a vid that helped me get it tysm 😭🙏

[@positiveviber6650]

Super explaination.easy to understand by any language people.thanku

[@pankratz1459]

best chemistry explanation yet XD

[@mon0quie]

I DON'T GET IT 😭😭😭😭😭

[@ghostoflego3390]

Look man, every atom wants stable eight electrons in their valence shell. So they form bonds. Sulphur and oxygen bond but they have a choice. They can remain as the first structure as shown, or they can be the second structure as well. Both have nearly same energy , so it doesn't make a difference. But you know what makes a difference? Both of them at same time Molecules that satisfy certain conditions have the power to switch to both structures instantly. In that switching, energy is lost and the molecule becomes even more stable. So they form a resonance hybrid and this phenomenon is called resonance. I hope you understand. The number one rule in chemistry isn't octet, it is that everyone wants stability

[@kebabcordonbleu57]

French student here in 2020, Thanks for this video, your a rly nice teacher !

[@theguy3406]

Boron, Sulfur, and Phosphorus are exceptions to the octet rule... the more you know

[@angelk2948]

I need this guy to be my hypeman

[@mohameda.4275]

Omg thank u, u made it so much easier to understand

[@trendinglife8971]

Explained so well❤️❤️

[@shutdown3734]

I’m seeing stuff the says O=S=O with 4 dots on each oxygen and 2 on sulfur would be more stable and there fire correct but this makes more sense as it follows the octet rule. Can someone explain?

[@uditaarora3804]

Actually...elements after 2nd period can extend their octet

[@saranyahari7251]

Sulfur belongs to 3 Rd period

[@kaleemhussain5193]

Hello Sir..that s very good way..but i have a question about sulpher's valency.. you have showed 2 electeons for sulpher and you said that sulpher and oxygen both belong to same group so sulpher must have four electrons other than two electrons bonded with oxygen..

[@mallangwazir7445]

Thankyou sooo much for explaning so clearly😆😊👏👏👏

[@lightofthemoon8521]

My teacher has this habit of basically putting one question in our SLAs that seemed irrelevant to us or something we'd only know if we studied further online and this was one of the questions.

[@Jecoliahh]

Your videos are very helpful!!!

[@reneehenry2759]

The S-O bonds are shorter in SO2 (143.1 pm) than in sulfur monoxide, SO (148.1 pm), whereas the O-O bonds are longer in O3 (127.8 pm) than in dioxygen, O2 (120.7 pm). The mean bond energy is greater in SO2 (548 kJ/mol) than in SO (524 kJ/mol), whereas it is less in O3 (297 kJ/mol) than in O2 (490 kJ/mol). These pieces of evidence lead chemists to conclude that the S-O bonds in sulfur dioxide have a bond order of at least 2, unlike the O-O bonds in ozone, which have a bond order of 1.5.

[@arik2916]

This is WRONG. The best structure is the one with the LEAST formal charges, which would be two double bonds to the oxygen's. And we can 'break' the octet rule because Sulfur lies in period 3, so it can have an expanded octet.

[@yasircicek2089]

@Proh Done Because sulfur can contain more than 8 electrons even more than 10 :)

[@bonganemathebula7556]

@Proh Done If you studied it, then why did make the earlier comment?

[@ryanshaffaf8977]

Sulfur is in g16 lol

[@AnkithArunAswath-m8s]

But at 3:34, you say we can't move any electrons around and that we would be breaking the octet rule, can't we simply move 2 electrons from the lone pair of the Oxygen which has 3 lone pairs and make a double bond? Then the formal charge would be 0 for both the Os as well as the S. Please look into that.

[@puromate1286]

why not O=S=O ? help please!

[@Newbport849]

PuroMate I agree, I also came up with that structure.

[@LienNguyen-kz3ow]

[So4] 2-

[@lakmesilva9837]

+Nino Enriquez it is possible.bcoz S is in the 3rd period...isnt it ?

[@kylegolden3299]

+PuroMate This is just an exception you have to know. Just know it's not two double bonds.

[@HanSoloxcs]

+PuroMate Because total valence electrons is 18 (6 from Sulfur, 12 from 2 Oxygens = 18)....O=S=O only uses 2 x 4 = 8 electrons....you have 10 remaining electrons that you still need to fill in

[@scaper8]

This all makes sense, but many sources show that each oxygen has a double bond, not just one, giving the sulfur 10 electrons, thus breaking the octet rule. Are both versions (two double bonds/one double and one single bond) correct? If so, is one _more_ correct that the other? If so _which_ is more correct? And Finally, _how do we know when we're supposed to break the octet rule?!_

[@KeijelloTamu]

I ABSOLUTELY AM FEELING THE SAME WAY! I know this is an incredibly old video, but I'm struggling to know when to break it. Is there an option that is more preferred or more naturally occurring in real life? Is there a more stable option? If so, how would we even know??

[@term88nator79]

@@KeijelloTamu so pretty much many scientists disagree on which model they like the most. My opinion is to pick the model you like the most and stick with it. Ex. in this problem, I normally like to try to achieve a zero formal charge, so O=S=O is the one i would go with, but if you prefer following the octet rule, then O-S=O is also acceptable.

[@siphelelegqwede8213]

wooooooow.........now i get this ....wheew......thank you so much for making this much much easier!!!!!!!!!

[@vivektiwary7065]

Least size > least electronegativity > largest size > highest atomic no. Priority order to choose central atom

[@brainznartz1287]

see you may be good in chemistry but in this video I am gone with my head🤯🤷‍♂️

[@adarshbhadauria6487]

He didn't explained coordinate bond between sulphur and oxygen.

[@pranayharishchandra-vlogs]

Bro indian IIT wale baccho k liye ye mazak hai... Fail to ho gya tha vaise bhi Lewis's structure Useless..,. Utne structure to hum khud hi bnalete hai hai jitne isse bante hai

[@mountyania9321]

@@pranayharishchandra-vlogsTo bhai mujhe samjha de na SO2 ka Levis structure Aur ha 1 aur cheej ye neutral oxide ka covalent bonding kaise Hoti hai plzz jaise CO, NO, N2O Ye kaise hota hai kya neutral oxide neutral nhi hota hai plzz koi bhi Bata do plzz

[@jules7174]

That’s the same thing I was thinking

[@mpugamohammed4738]

Yah exactly...

[@handeaydnlar6275]

Loved the way you say "That's not 8, that's 6!" :D Thank you so much for the video, it really helped

[@L150X]

Very helpful. Thank you!

[@PetterRibeiro]

You are the man !! YOU SAVED MY LIFE !! THANKS hahaha

[@MATHBOSS287]

ربنا يباركلك يبني و يكرمك شارحك ذي العسل

[@AndrewGulickTrueVitalityPlus]

The 'T' in the word "often" is silent so, the word often is pronounced ofen. Good video, by the way but, you should bring 2 electrons over from the first Oxygen and make both oxygen bonds to suffer a double bond. That will give each element a Formal Charge = to 0. As it stands now, the O on the left has a Formal Charge of -1, S has a +1 and the other O has a Formal Charge of 0. With two double bonds, each O will have a FC of 0 and so will S.

[@Dontlook146]

Andrew Gulick I agree

[@jasonwise8957]

Amazingly explained 👏👏👏

[@adrielmarasigan8500]

Im pretty sure any elements from period 3 to 7 are allowed to break the octet rule so it should be like this o=s=o

[@hulaanmo2132]

Correct me if I'm wrong but i think the answer is wrong 😅😅 or if it is correct, there's something more stable than that. And i think not all elements have to satisfy the octet rule, that's why there are compounds having extended octet rule. That's just pure opinion and purely based on what i know 😁😁

[@AdityaSingh-ly9ku]

you are right there will be two double bond between oxygen and sulfer atom, sulfer atom will have 10 electrons which is the most stable as sulfer is stable at covalency 2 4 6 and here it is 4. While octect rule is not followed here having extended octect rule. One more thing that this structure will have 0 formal charge in all atoms which more stable than having any charges.

[@chinmayeemishra2245]

Tq for this information 🙏🙏🙏🙏

[@Iuschneider]

YOU'RE A GOD!!!! THANKS!

[@cht5086]

I just learnt all about Lewis and octet in 4 min. Thanks al ot!

[@therishibansal]

Isn't sulfur able to expand past octet because it is in the 3rd energy level so it has access to 3d orbitals?

[@chemistNATE]

Yes, it can, but there is no need to for SO2

[@myriadmysonid946]

Isn't it O=S=O because sulphure can hold more than 8 electrones

[@Derbisin]

gotta look at the formal charges

[@tayloreasey8533]

O=S=O is better because it has formal charges of 0 for each atom. Also I had a chemistry final question asking for the molecule with resonance and the answer was not SO2.

[@MrAnimatedLegend]

Taylor Easey Suflur has a charge of +2.

[@matimassetti]

+Mr.AnimatedLegend It hasn´t, because Taylor didn´t mention that sulfur has 2 nonboding electrons. So it´s: 6-2-4= 0

[@HanSoloxcs]

+Ozan Erol Because total valence electrons is 18 (6 from Sulfur, 12 from 2 Oxygens = 18)....O=S=O only uses 2 x 4 = 8 electrons....you have 10 remaining electrons that you still need to fill in

[@Shahmeeriqbalqureshi]

thank u for uploading this vedio..helped alot..

[@aminedundar1921]

Çok iyi anladım teşekkürler 🤓🤓

[@delilahmontgomery6367]

I'm here just because my teacher gave us work he didn't teach

[@joelpinhoneto5225]

Super nice! Bewn!!! Thanks!

[@anshpreetkaur4793]

How do we know that the molecule is electron deficient and there is no mistake in making lewis structure and making bonds ?

[@arik2916]

Check out Wayne Breslyn's channel. He explained this very well.

[@sarahkin36]

Oxygen and Sulfur both start out with 6 valence electrons, so they both need two bonds. They can’t just magically have an extra electron. I was trying to figure out how to arrange the Lewis structure so that I could have two bonds for every atom without having sulfur have an extra set of unpaired electrons, and this was not only unhelpful but incorrect

[@kagomeonetwo]

If you put double bonds on both oxygens, you will be missing two valence electrons, and if you put the remaining two on any of the elements they will have 10 instead of 8 which breaks the octet rule.

[@kagomeonetwo]

My teacher taught us the 6n+2 rule. 6+6+6= 18 6(3)+2 = 20 When the valence has a difference of two, it will have 1 double bond. When it's the difference of four, it will have two double bonds or one triple bond.

[@hpfandom]

​@@kagomeonetwoThanks! But, Sulphur doesn't need to satisfy the Octet rule as it has expanded Valence shells so putting them on Sulphur doesn't impact I guess. But your claim about the mismatch in the valence electrons makes sense.

[@pranavi1949]

@@kagomeonetwo Sulfur is part of the 3rd energy level it can break the octet rule

[@mEmE-lk6gm]

YOU MISSED TO SAY THAT YOU DID THE VERTICAL ELECTRONS TO HORIZONTAL ELECTRONS TO THE MIDDLE ATOM OF THE LEFT SIDE IF I AM NO WRONG BUT THE VIDEO IS GREAT JUST NEED TO EXPLAIN MORE CAUSE I GOT IT BUT DON'T KNOW ABOUT OTHERS PLZ EXPLAIN MORE

[@adityahooda5764]

Sir sulpher has 6electrons in outer most she'll but you show it 5 and their is no double bond

[@noblenormie1179]

ikr this is what upsets me this seems to be contridciting thats why ive been looking for a solution to begin with

[@adityaparulekar7159]

Why can't the sulfur atom have 2 lone pairs and 2 single bonds instead of making another a double bond with one of the oxygen atoms. That should be more stable, right?

[@aniketkarkhile6846]

Think about formal charge

[@brendanmulrooney368]

@@aniketkarkhile6846 In the scenario Aditya explained the formal charge of every atom would be 0....so you would actually want Aditya's answer instead of the provided one because it would presumably be more stable. I think the problem is that when the other oxygen(that is unbinded in the video) uses 2 lone pair electrons to form another bond with sulfur, the Sulfur then has 10 electons. This breaks the octet rule, which I'm assuming is more important than making each atom have a formal charge of 0. This explanation is assuming the video is correct. Honestly, I have no idea.

[@at0577]

@@brendanmulrooney368 if we make two double bonds. Then that will be more accurate as Sulphur will try to achieve maximum valency(octet rule can be break)

[@eugefgh]

i'm so glad rn. thank u so much, you helped me a lot bc my teacher really sucks

[@miagottfried5947]

So no one's gonna talk about what he said at the end💀4:55

[@wiwisylvia6130]

So cOmpliCaTed!

[@aamodbk5064]

Dude! you're awesome!!!

[@aseel9911]

احبك انت و شرحك ذا

[@MayXuan69]

thanks for teaching

[@adarsh3714]

Call everybody!😁😂

[@DanielBaurStudent]

Thanks for the video! However, I have seen models where it's bent, shouldn't it be bent and not linear?

[@chemistNATE]

I only drew it as linear in the Lewis diagram. As soon as the lone pair goes onto the S it becomes bent. Bent is correct

[@Dmik424]

I believe this is incorrect, if you made double bonds, the formal charge would be 0 for both the oxygen and Se making it more stable...

[@k_ayush45]

You rocked !!!🤘 thanks

[@oximas]

you got the biggest library of lewis structures i have ever seen

[@jaydope4823]

wait why does oxygen still have six electrons after sharing an electron with sulfur? shouldn't it be 5? im so confused

[@Mhsmm0]

Tebrik ederim çok güzel anlattınız ❤️

[@dmariusallen3349]

The HCN was correct. Thank you.

[@huseyinonatturkglu]

I study in Turkey and I have learnt it better than it was in my mother tongue. But I suppose there is a little calculation problem.

[@shivambhardwaj415]

It is so helpful for me

[@briarsmith8702]

This is wrong. Sulphur has an expanded octet which allows it to bond with more than 8 electrons, so both oxygens should be double bonded to the sulphur giving every atom a formal charge of 0.

[@andrewwee7458]

Can't the single bond between the oxygen on the left and middle sulphur JUST have 2 electrons ONLY from the sulphur and NONE from the oxygen?? Cuz otherwise it won't make sense, because then you'll be saying that the sulphur only has 5 valence electrons instead of 6, which is pretty untrue. Thanks.

[@melip.9027]

Geez!! Thank you!

[@loverlover3437]

Good job

[@Rmiznow]

Be careful, this video is actually totally false

[@chemistNATE]

+Corentin Bovy Actually, the ones I drew turn out to be the most likely contributing structures to SO2, and the expanded-octet version (two double bonds + one lone pair on S) is of less importance. There have been theoretical calculations done and there is hardly any d-orbital hybridization in SO2 which means the octet rule needs to be followed (Cunningham et al, J. Chem. Soc., Faraday Trans., 1997,93, 2247-2254)

[@Rmiznow]

+chemistNATE yes but you can't explain it like this because you will threw people in à wrong way. This structure isn't as easy there is a lot of other rules which are unknown of your viewers. So you should have showed thé other structure which is nearly correct for them to understand. I mean, if you explain it that way, in my point of view that's false.

[@tkdguy5494]

+Kymani Gorham It's not that it's wrong, but the video is incomplete. See, the obvious confusion here is why he didn't use O=S=O (with S having a lone pair). As this would satisfy all formal charges, and because we know that S can have an expanded octet. Also, the O=S-O O-S=O is correct, but remember that neither structure is on its own, a true representation of SO2, because each bond is a hybrid. So while it can be drawn like this, the other structure is valid. And even if it were true that O=S-O is a better representation of SO2 than O=S=O in reality, this should at least be explained. Otherwise, it will confuse students as for why sometimes we use an expanded octet for S and other times we don't. But the resonance of O=S-O and O-S=O is why SO2 does not have a formal charge, which is fully represented in the expanded octet version. And even if the expanded version isn't completely true to reality, we must remember that Lewis structures have their shortcomings to begin with. And btw, for what it's worth, I have a BS in chemistry.

[@robinheo2627]

+Corentin Bovy agree!! I've spent my 4 min to understand the difference between SO2 and N02 but there was no use to it!!!!

[@THROEDCAT]

Corentin Bovy if you have 2 double bonds on both sides of Sulfur, Sulfur will not have an octet. it would be surrounded by 10 electrons.

[@ahmedalgadi515]

+Kyle Golden the correct answer is .. .. .. :O=S=O:

[@mEmE-lk6gm]

NONSENSE ANSWER MIDDLE ATOMOF SULPHUR IS HAVING 10 ELECTRONS YOU SHOULD MAKE 8 ELECTRONS

[@arthurmoulie3745]

JD TALK it s an exception. Look up SF6

[@samuellima1899]

Anounymous 123 BR2

[@hayakhan5861]

in this answer,sulphur make bond in order to complete its octel and its valance shell consist of 6 e .but in this ans sulphur has 10 e .after sharing with two oxygen it has 8 e and 1 lone pair total is 10.how thats possible? sulphur is not completing its shell accordinng to yur methd.

[@martinaidendemaj902]

The video is correct.

[@chandersingh5829]

Please tell me How many lone pair in SO2

[@isaacmolina5500]

What about a dative bond instead a simple bond?

[@aurelieg4937]

i think the simple bond is a dative bond

[@carinakerber8196]

thank you for the video!!

[@kupokins]

I put this answer on my quiz and got it wrong. Just so you all know.

[@aaronc2022]

+ewdgsfhxgjhj In many schools teachers give you the '2 cent' version of chemistry, a lot of what they say isn't completely true, but introducing all full concepts is too complex for beginners. its important to know your schools syllabus and how your teachers want questions to be answered. The internet helps with understanding the concepts but are often not exactly what you need to know.

[@aaronc2022]

+ewdgsfhxgjhj In many schools teachers give you the '2 cent' version of chemistry, a lot of what they say isn't completely true, but introducing all full concepts is too complex for beginners. its important to know your schools syllabus and how your teachers want questions to be answered. The internet helps with understanding the concepts but are often not exactly what you need to know.

[@kylegolden3299]

+ewdgsfhxgjhj This answer is correct. It's a pretty weird molecule.

[@bionicperson6029]

+Kyle Golden The question is, why doesn't sulfur neutralize the formal charge by making a double bond with the negatively charged oxygen? It is able to break the octet rule, so why not?

[@kylegolden3299]

Bionic Person Honestly I have no clue. I'm sure with some research you could find out exactly why it forms this. All I know is that this is the structure that is formed, even though the two double bond structure seems more plausible. This is just one of those things you have to memorize.

[@Chris-wu6jz]

The octet rule isn't a "rule" you have to follow. It's a guide.

[@Gene-cc2np]

Wont the oxygen on the left have to share an electron with the sulfur cause thats how covalent bonding works?

[@nvoewvobwurgfbondoqb]

YOURE NOT MY DAD

[@leyamirg2658]

Get Like Me he's totally my dad

[@deependraverma4382]

I'll pray that for you...hahahaha

[@mewstrum1255]

But can't sulfur have an expanded octet? Wouldn't the ideal structure of SO2 have two double bonds to satisfy the formal charge of the oxygen

[@itsyaboitaco9804]

by doing so its going to compromise the octet rule for sulfur having 10 electrons instead of 8.

[@Andrew-ss2pr]

You're correct. Sulfur has an expanded valence by utilizing d orbitals in this case. I wouldn't count this as wrong on an exam but there is a better structure of O=S=O with two lone pairs on each oxygen and one on sulfur

[@ELamar-my5kt]

"Whos your daddy...I am" lmaoooo

[@Rubyumama]

Omg thank you ive been stuck for half and hour and it turns out it’s super easy ❤️🫂

[@shonalipradhan996]

thanku so much😄

[@user-ww9ef6hc2l]

دمت گرم عامووو

[@qureshahmad7266]

Thank you 👍👍😀😀🤓

[@juiceland4688]

Perfect thxxxx a lot it was really helpful