Formal Charges: Calculating Formal Charge
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- เผยแพร่เมื่อ 23 ส.ค. 2024
- A step-by-step description on how to calculate formal charges. Formal charges are important because they allow us to predict which Lewis structure is the most likely to exist in the real world.
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Often you are given a compound with more than one possible Lewis structure. Often this is the case with elements like Sulfur or Phosphorus which can have more than eight valence electrons. In these cases it is important to calculate formal charges to determine which structure is the best. The structure with formal charges closest to zero will be the best.
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Thank you so much.. my professor was killing me with this.. but you made it so understandable
Good to hear the video helped you understand formal charges. They are a bit tricky at first but are a very useful tool in chemistry. --- Dr. B
Thanks you sir bahut dhanyawad
Had you never studied class XI th???
U feel u are getting killed by ur professor because u can't understand this simple thing,, I think it's not the problem in ur professor but it's the problem in u
You are a beautiful teacher. Best ten minutes i have spent online today cause i watched it twice.
out of the million videos, this one helped me the most thank you.
Thanks for the kind words and letting me know! ---Dr. B
So True
Outstanding job explaining this in such a simple way. Keep up the great work Dr.B!
Thanks, will do!
Dr. B, This is so simple..... Thanks a lot. You're a life saver.....
One of the best chemistry professor i have ever witnessed
I wished you could teach chemistry in my school.
My professor literally overcomplicates everything, and this made my life a lil bit easier tysm.
Hes a clown
Thank you so much Dr.B .Amazingly explained and a very useful technique in chemistry. I wished I would have learnt about this in high school, it would have made structures so much easier to draw. I wish your channel grows much more so more people can benefit from such knowledge and wish you good-luck with it.
you just calmed my late night panicking by so much, thank you sir. now, come teach my class?
i will tech it
XG Frost Killer, Lets hope you don't if the spelling is anything to go by.
@@TheSniper9752 i will teach it
late night panicking.., i relate to that too much
Thank you so much, Dr. B! You're so good at explaining chemistry! You're the Bruce WAYNE of chem!
You are saving me from my online professor that BARELY teaches, THANK YOU SO MUCHH
you are Better than anyone who has ever tried explaining this stuff to me.Thanks
Thank you Dr. B. Your videos helped me realized that I'm capable of learning chemistry.
Thank you so much. This video will really help me. Our teacher just gives us answer sheets without explaining anything and yesterday she just made us answer Lewis Structures lol. Thanks a lot!
Now you are probably graduated 🌝
Thank you so much, I have a test tomorrow and I just couldn't wrap my head around this concept. Your video really made me understand it!
Hope you test went well!
@@wbreslyn it did! Thank you!
Awesome lecture. I understood very well. I didn't saw this type of lectures upto now.
Woah... I actually understood. If only I get the Chem Lectures just as fast I learn in YT. Thanks!
Thanks a lot Sir, I study in Turkey but instead of our differences in language, I clearly understood you. :)
the topic is explained in a very nice and lucid manner. THANK YOU FOR YOUR VIDEO SIR
Glad I could help with formal charges! --- Dr. B
Thx man, you're helping me in final exam :D
Thank you for this video.
I will have a test tomorrow, and this was the one topic that I did not understand, but you made it easy to learn.
All the best on your test! --- Dr. B
Thanks, sometimes videos from less famous channels and less likes are best but often not tried! You did it!
I know what you mean. Just because there are a lot views and likes doesn't necessary mean the videos are better. I did this video on formal charges when my channel was pretty small. --- Dr. B
Yeah, Thanks again!
Yeah, Thanks man. Are you a team or single man?
Just a chemistry teacher/researcher who does some videos on the side!
I am from india ....there are good teachers but you are best
Thanks for the kind words!
Thank you for making everything looks simple and easy usually teachers make it so difficult and complicated
Most welcome 😊
woah you made this easy, thanks man! I appreciate your hard work!
No problem!
My final chemist exam is in a few hours and yet here i am
Thank you so much, my teacher didn't really explain this well in my opinion so this was really helpful
+Lena V Glad I could help! Teachers often make formal charges more complicated than then need to be. --- Dr. B
I'am from Argentina and I love how you teach in this videos, mis teachers are ....:/
Was wondering if there is an O-Chem playlist here? Would be so helpful as you're so good a teacher and your lessons are so good.
Sorry, I'm from the US so I'm not as familiar with O-chem.
I LOVE YOU SO MUCH! You saved me from my chemistry final. Thanks!
thank you soon much , if this will come to me in the exam i'll remember your video. it's so easy thank you again
it was really confusing while i learnt it from the text book but aftrer this video it was like literally so simple.
Thank you so much prof.
Good to hear! --- Dr. B
From faculty of pharmacy in Egypt, big thanks my teacher💜🌸
Glad I could help! I did some pharmaceutical research a will back. Interesting stuff.
There it is: www.ncbi.nlm.nih.gov/pubmed/8620108
--- Dr. B
Thanks I was really stuck on formal charges. Now I realize what octet really meant. Haha it's funny that I thought that the electrons where meant to be place in a regular manner. Haha.. I was searching for it the whole day.🤓😭🤗🙌👏😃
Thank you so much i understand that my teacher was give us a test for the formal charge and you helped me thank you ❤️❤️❤️
So , if I have understood , the formal charge rule is more imprtant than the octet rule, because in the 2nd LEWIS STRUCTURE of SO2, the octet rule for Sulfur has not been respected.
Thank you for this video, it was so helpful and you explained everything so clear. Thank you.
Glad it was helpful!
you make it so easy to understand. thank you so much!
so easy to understand the way you put it! thank you, I appreciate it
Glad I could help. Formal charges aren't too difficult once you understand the steps. --- Dr.B
Thank you so much. Extremely helpful and easy explanation.
Hey
Meet me on fb
Kumar Adarsh Gupta, India
instead of diving he bonding electrons into two (2), you can just first transform those bonding electrons into a line then count them as one, less confusion
Thanks 😊 for the wonderful video because of this I can understand the actual method sir... 💗
Most welcome 😊
Great video... helped me 2 hours before the exam ty
Hope your exam went well! --- Dr. B
Simple and helpful- thanks for the video!
yay i passed my high school test! Thanks m8
thank you I've learned some so much from you
these videos help me a ton, thank you sir!
Hey Tyler, glad I could help. Formal charges are one of those topics that is sort of a hassle but very important. -Dr. B.
I'm confused
Your sulphur is having 10 electrons around it. Why?
Now i am able to understand everything thanks 🙏🏻 For the video.
great video, helps me every time, i need to review ^~^
Glad I could help CatzGoCrazyable! --- Dr. B
Hello Dr.B. Based on the methanal, we also need to make center carbon without lone pair electron right?
Thank you
Thank you so much! My teacher also did not explain it well at all. I am told there is another step, checking the overall charges. Do you explain this step also? I hope so : )
for overall charge just add up the formal charges
@@vers8278 u were answering that to a 4 year old one
@@pavitrarupa8716 😅😬
Thank you! I just had a quick question, when both resonance structures have the same overall formal charge what do you do?
It's best when the negative formal charge is on the more electronegative element. If the resonance structures are equivalent then the final Lewis structure is an average of those resonance structures (like this one: th-cam.com/video/rrps8QujYA8/w-d-xo.html).
- Dr. B
Thank you!
thank you for being so clear and concise
You are most welcome!
--- Dr. B
Thank you so much for your clear and awesome explanation, sir!!!
You are welcome!
OMG thank you!! You’re my hero Prof.
Happy to help!
short and to the point..... keep the good work sir
This is very useful. Thank you so much!
Thank you so much, your videos always help me!!
Thank you sir
Is it right to say that the right structure is the one in which the centeral atom's formal charge is zero?
Thank you...took nothing more than 30 seconds to understand .THANK YOU!!!!!!!!!
Excellent, this is an important chemistry skill! --- Dr. B
Very helpful, step by step to calculate formal charge
Dr. B, ur a real G.
You explained it beautifully, thank you so much
IM SORRY THIS'S THE LAST QUERY
can the first structure of S2O actually exist? or is it just really unstable? sorry for bombarding you with questions XD
No problem, you are asking good questions.
The first structure isn't as stable as the others. So it can exist, but not as frequently. It's a bit more complicated, but that's the general idea. We think of each structure contributing/being an average of the actual Lewis structure (the one we observe in the lab) The first structure in the video doesn't contribute much to the actual Lewis structure. --- Dr. B
thank you dr b
you are awesome man , thanks very much from SYRIA , you explain amazingly ! keep going
Thanks for the motivating comment! --- Dr. B
👍👌
Edit:
Dr. Best!!😀✌️
ap chem test tomorrow over chemical bonding..but this video just made me a little less stressed :)
AP chemistry is all about managing the stress... -Dr. B
Had to give a like, thank you for this explanation.
I have found many different formula's to find the formal charge. One of them says that to find the formal charge, it is:
Valence electrons - (Bonding electrons + Non Bonding electrons). Why are there multiple formula's to find the formal charge?
you cant just say electrons, and memorizing it in parentheses is just stupid
Very good explanation
Thank youu, have my final today and I’m not ready
Hope you do well on your final!
and at 1:40, the oxygen atom on the extreme left isn't sharing any electrons, right? It has its 6 electrons intact and is just using 2 of sulfur's electrons to complete its octet? pls correct me if I've got it wrong...
It would be sharing the two electrons between the O and S atom. Anytime there are electrons between two atoms we consider those to be shared (also called bonding electrons). --- Dr. B
so is that a dative bond? since both the shared electrons are from sulphur?
@@serene9532
Yeah!
It seems to be a dative bond.
@@seamshakeel1999 ok thanks for replying :)
@@serene9532
Welcome!:-)
Great video, very clear:) Thank you!
One second. Didn't both the SO2 structures have a formal charge of 0?? So why are we only saying that the second one where both oxygens are double bonded is correct??
Thank you sir. That video help me I like it .
I am from Saudi Arabia.
Lol...Why do you have to mention that you're from SA?
@@shantanuthakur6081 Attention
Are both molecules containing sulfur and oxygen the same molecule?
I had understood easily by ur's video
My professor gave me a completely different formula but this one makes so much sense. He gave me: # of valence electrons -(e in lone pairs + # bonds)= and it just confused me more. I pass gen chem with a C and now that I am taking O chem I have no idea what is going on.
Thx sir this was helpful love from India✌️✌️✌️
Glad it helped!
AWESOME TEACHER! THANK YOU:)
Quite cool way to teach sit....👍
Thanks! --- Dr. B
Thank you so much for that clear explanation
You are welcome!
Thank you for quick fantastic video helps a lot
Can i ask, why would you divide the bonding electrons by 2?
That's because with formal charge, the electrons in each covalent bond are assumed to be split exactly evenly between the two atoms in the bond (according to Wikipedia and I agree). --- Dr. B
How come 2 lone pair electrons are left in sulphur when it is forming double bond with both oxygen(s)
Thank you so much sir i understood better from this video.
Another excellent explanation. Question: other than S an P what other element can have more the an octet? David L
Pretty much anything in Period 3 and below.
@@wbreslyn Thank you. will remember this. D:)
@@wbreslyn Had to review instruction again....bless you. DVD:)
you are a blessing thank you so much
Ur the G.O.A.T fr fr 🙌🙌
Thanks!
awesome video! watching this in 2018
Thank you so much, this is so easy!
Thank you so much! Helped a lot!
Sir but it should be 6-5 , I mean the bond between oxygen and sulphur is not coordinate
but now sulfure has 10 electrones
That's okay, Sulfur is below Period Two on the Periodic Table and can have an expanded octet (more than eight valence electrons). This is because below Period Two the elements have d orbitals available. -- Dr. B
For more clarification on my part, d orbital can sustain more Valence Electrons. Am I assuming correctly?
P.S. Great Video, extremely helpful.
@@wbreslyn hello sir
Does that mean that there could be another structure of SO2 with 2 triple bonds?
@@alejandramejia663 go watch melissa maribel video about lewis
Thank you mr Wayne for this nice video
No problem!
He made it so simple!!!
which software do you use to create videos ?
but why/how can sulphur (and phosphorus) have 10 electrons?? pls answer
That's because from Period Three (row three) and below on the Periodic Table the elements have d orbitals. This sometimes result in an atom having more than eight valence electrons. The Formal Charges help us figure out when this will happen. --- Dr. B
but does that mean the octet rule is not actually correct? we use it extensively though, even in these lewis structures vids..
@@serene9532
Octet rule is really helpful but in some cases it is violated.
Examples- BeCl2, BF3, XeF4 etc.
@@seamshakeel1999 i see, thanks!
@@serene9532
Welcome :-)
Thanks for a great video, very helpful
Glad it was helpful!