I can't begin to explain the happiness I feel when I type a subject in the search bar and I see that black background with neon numbers and letters pop up. Thanks so much!
Dude, from one teacher to another. You're great at this. (Even if I am 6 years late to the party.) Your accent make's it interesting. "So that's BH3, that's just how it is. You gotta problem wit dat, wise guy?" OH, LOOKAT dis guy, with his exception to the octet rule. "HEY, I'm doin' Chemistry heah." etc. etc.
Thank you! Unlike most people who come to youtube to learn, I have had a phenomenal professor, however even then I was unable to grasp VSEPR and Lewis Structures. you have made it so incredibly clear.
often times in higher chemistry courses, they will be omitted. but yeah you're right, and in gen chem or high school chem, teachers will likely take points off.
Professor Organic Chemistry Tutor, thank you for a fantastic analysis into the Exceptions to the Octet Rule in AP/General Chemistry.The examples/practice problems shows the complete Octet Rule and when they are violated in Modern Chemistry. Professor Organic Chemistry Tutor, thanks to the viewers for finding and correcting the errors in this video.
You're just too much dude. Thanks. Your videos have really helped me. Wish I knew you much earlier, I would have scored a better grade in math and chemistry. But am doing well in the university now. Thanks to your videos.
i just want to say that I have my chemistry final tmrw and you have been a HUGE help you have no idea! Without you, I would have failed most of my chemistry exams! THANKS
Someone help what's happening at NO2 at 12:10? Oxygen isn't donating anything. And given that Nitrogen primarily has 5 ve at the start, im assuming a coordinate bond has been formed with the Oxygen atom on the right? SInce it looks like two electrons have been donated to Oxygen there by Nitrogen solely. If we assume that two have been donated to oxygen by nitrogen on that side, only then does it imply that it had 5 valence electrons in the beginning. Otherwise it doesn't make sense. Am i getting anything wrong?
DOUBT 10:45 DOES IT MATTER IF WE LETS THE NITROGEN ATOM HAVE A ONE FULL LONE PAIR AND ANY OF THE TWO OXYGEN "WITH THE SINGLE BOND" HAVE 2 LONE PAIRS AND A SINGLE UNPAIRED ELECTRON? (and also how can you just give an oxygen atom an electron just because it has to satisfy the octet rule??)
Ido84ba he’s talking about the energy level, that’s why Phosphorus is an exception, if that’s what you’re referring too, but yea you have the electron configuration right
@@Ido84ba You know the quantum numbers? Well period three that includes phosphorus has the principal quantum number(n) of 3(it follows the period number so H has an value of n=1 & C=2), which means that the angular momentum quantum number(lowercase L) is 0, 1, 2. We know this because l = 0 to n-1. And the angular momentum quantum number of 0 means the S-orbital, 1 is the P-orbital and 2 is the d-orbital, so while period three atoms won't put any electrons in the d-orbital it has the possibility to do so if they wish. I hope that cleared it up for you.
Can someone explain how atoms like Phosphorus can have more than 8 valence electrons even though it doesn't use the d orbital. I know he said they do use it, but atoms don't use that orbital until we get to elements like Gallium and Germanium right? Phosphorus only half-fills the 3p orbitals and fills 4s before using the 3d orbitals right?
Orbitals can be mixed to form hybrid orbitals of an energy between the filled and unfilled orbitals. Phosphorus’ d orbital is close enough in energy that it can stably form a hybrid orbital with s and o orbitals
Why without ion charges? We in Germany learn to do it with those and not single electrons. Also the formula to calculate the lone pairs doesn't apply to every molecule. like methylisonitril f ex. Idk if I'm right pls correct me if I'm wrong
@@iislaymelillyiisharif4988 watch his previous video in which he explained the formulae he clearly mentioned that THIS FORMULAE DOES NOT WORK FOR COMPOUNDS CONTAINING HYDROGEN
From what I understand It is because Boron(B) has only 3 valence electrons which means It can only form a maximum of 3 Bonds, and with 3 bonds you will only get 6 electrons and not 8, therefore violating the octet rule.
I think it's b/c the two Oxygen atoms have already achieved 8 e- based on the octet rules, so N atom can have that last e-. Please correct me if I'm wrong. :D
I have an urgent question. 1.Becl2 is below octet where Be would have 4 valance electrons but my question is can't we make double bond with both chlorines and make it 8?☹️??
I know I am missing something... Because i don't know why you should place terminal atoms around the central atom in a particular shape..is it wrong to place terminal atoms randomly around the central atom ...how do you know the shape of these molecules
Very good, I have a question what app or instrument you use? I mean that black board and the way you write on it, I m a teacher and need this good way to teach to my students, thank you
so there are 5 Cl atoms, and each of them got 8 valence electrons, so 5 x 8 = 40, total valence electrons in ICl5 is 42, so 42-40 = 2 electrons; 2/2 = 1 lone pair on the center atom
I see people draw calcium with the 3rd shell with 8 electrons and the valence with 2. Can you explain why? This is in the third row, so it’s a little confusing
The electron configuration for P is not correct in the video brother. its 3s^2 3p^6. You don't get to the d level until 4s^2 3d^10 4p^6. Can u please explain if I am wrong in this regard. Thank you, I love your videos by the way.
Remember like this, the least electonegative atom is the central atom, but Hydrogen is an exeption, it can never be a central atom because it has only 1 electron. ***LITTLE TIP***: Usually(there are some exeptions like H2O) in the chemical formulas, the element which comes first is the central atom
Molecular Geometry - Free Formula Sheet: bit.ly/3YgxHkf
Chemistry 1 Final Exam Review: th-cam.com/video/5yw1YH7YA7c/w-d-xo.html
Chemistry PDF Worksheets: www.video-tutor.net/chemistry-basic-introduction.html
I can't begin to explain the happiness I feel when I type a subject in the search bar and I see that black background with neon numbers and letters pop up. Thanks so much!
Me too, I love hearing this guy.
I thought I was the only one
I thought I was the only one
كلنا كلنا مش انت بس
@@ahmedmousa3358 شرحه احسن من الدروس 💀
you are the ONLY one who explains the concepts in such an excellent way!!!! Please keep making more videos.
3 years later after your comment I feel the same
@@JH-ux1re5years after and I feel the same
@@LinaSlay-md3voYour reply just brought me back to my freshman year😂
4 years later... still a Legend.
Hey there, you're from the future!
Dude, from one teacher to another. You're great at this. (Even if I am 6 years late to the party.)
Your accent make's it interesting. "So that's BH3, that's just how it is. You gotta problem wit dat, wise guy?" OH, LOOKAT dis guy, with his exception to the octet rule. "HEY, I'm doin' Chemistry heah." etc. etc.
no body is perfect..but you are perfect.
Hope my score too.
thank you but you have created a paradox.
Tru
@@monkeyninja7988 No, he is implying that you are a nobody
@@buryakulikov2415 still paradoxical unless he is using "no body" as a name
man i love coming to your videos after I learn this stuff in school. It really helps to embed the information. ur a legend man.
Thank you! Unlike most people who come to youtube to learn, I have had a phenomenal professor, however even then I was unable to grasp VSEPR and Lewis Structures. you have made it so incredibly clear.
Just to help you guys-
when he draws ICl5, he forgets to draw the 6 valence electrons around EACH Cl.
Remember, the valence electrons are still there!
thats what i came to the comment section for!
often times in higher chemistry courses, they will be omitted. but yeah you're right, and in gen chem or high school chem, teachers will likely take points off.
tysm for saying that, i was so confused lmao
Thanks a bunch. Came to the comments hoping someone would confirm this😅😅
Dude you are literally the best teacher out there man
you deserve a nobel prize for saving the next generation of stem majors
Professor Organic Chemistry Tutor, thank you for a fantastic analysis into the Exceptions to the Octet Rule in AP/General Chemistry.The examples/practice problems shows the complete Octet Rule and when they are violated in Modern Chemistry. Professor Organic Chemistry Tutor, thanks to the viewers for finding and correcting the errors in this video.
You're just too much dude.
Thanks. Your videos have really helped me. Wish I knew you much earlier, I would have scored a better grade in math and chemistry.
But am doing well in the university now. Thanks to your videos.
2:02 sounds like "the reason why nitrogen can have 8" -- he meant to say nitrogen CAN'T have more than 8. just a clarification for u guys
how about the first row? can they be expanded? ..no? ....iam stupid
@@enderslot467 No they cannot because the first row only has the 1s orbital, which can only hold 2 electrons maximum.
@@KishoreG2396 so..question sir what is the valence of the column of He
@@enderslot467 He column (Noble gases) have 8 valence electrons
I think it was his accent, I listened to it again and I think he said, "The reason why nitrogen can't have more than eight"
thank you so much, I’ve been struggling for weeks, and I finally understand!!
I struggled with this concept for days. Thankyou so much☺️☺️.
i just want to say that I have my chemistry final tmrw and you have been a HUGE help you have no idea! Without you, I would have failed most of my chemistry exams! THANKS
Thank you for this help I appreciate it! But there should be 3 lone pairs on each Cl atom at 5:45
Your videos gave me success in chemistry
Thankyou, I have been wondering why there were so many exceptions to the octet rule!
better than some of the videos with many more views
Thank you again from the bottom of my heart!!! btw, you should do a face reveal video! :)
You are a God sent! Whenever I need help I know i'll find the answer in your videos and you always have clever ways to figure out problems! Thank you
This channel was underrated
Thank you for making this video! It is helping me study. and you do explain it in a clear way. thank you Mr. Tutor.
Ssc kon year bro?
@@quandagledingle9494 බිත්ති මගේ බිත්ති ඇතුලේ බිත්තිවල තියෙනවා මම ඒවා දකිනවා
I hate chemistry, there are exceptions to everything all the time because no one is able to come up with an all encompassing theory.
Life is very complex
You are the best youtuber on this platform
Well explained. Expectations arise for more in future.
You have been my mentor for so long
Thank you for improving my knowledge in chemistry
organic tutor , god bless you brother and I wish you the very best
Thank you Sir. It was really helpful. I was having difficulties in understanding this topic. Now I have clarity.
Thank you so much!! I think I get the octet rule now :)
Soooo helpful for studying ib chem hl by myself!! Thank u!!!
The moment you have a "system" with exceptions where the only reason is "thats just how it is", your system is wrong and shit.
Someone help
what's happening at NO2 at 12:10?
Oxygen isn't donating anything.
And given that Nitrogen primarily has 5 ve at the start, im assuming a coordinate bond has been formed with the Oxygen atom on the right?
SInce it looks like two electrons have been donated to Oxygen there by Nitrogen solely. If we assume that two have been donated to oxygen by nitrogen on that side, only then does it imply that it had 5 valence electrons in the beginning. Otherwise it doesn't make sense.
Am i getting anything wrong?
DOUBT 10:45
DOES IT MATTER IF WE LETS THE NITROGEN ATOM HAVE A ONE FULL LONE PAIR AND ANY OF THE TWO OXYGEN "WITH THE SINGLE BOND" HAVE 2 LONE PAIRS AND A SINGLE UNPAIRED ELECTRON? (and also how can you just give an oxygen atom an electron just because it has to satisfy the octet rule??)
thank you so much for simplifying it !!!
2:40 I thought the electron configuration of phosphorus is 1s^2 2s^2 2p^6 3s^2 3p^3 (not d^10). Can anyone confirm please?
Ido84ba he’s talking about the energy level, that’s why Phosphorus is an exception, if that’s what you’re referring too, but yea you have the electron configuration right
@@rachelazul1709 Thanks for the reply! Can you please explain what do you mean by energy level? I still don't really understand why he wrote d^10..
@@Ido84ba refer spdf chart , in that 1st row is 1st energy level (1s^2), 2nd energy level is 2nd row ( 2s^2 2p^6 ) and so on
@@Ido84ba You know the quantum numbers? Well period three that includes phosphorus has the principal quantum number(n) of 3(it follows the period number so H has an value of n=1 & C=2), which means that the angular momentum quantum number(lowercase L) is 0, 1, 2. We know this because l = 0 to n-1. And the angular momentum quantum number of 0 means the S-orbital, 1 is the P-orbital and 2 is the d-orbital, so while period three atoms won't put any electrons in the d-orbital it has the possibility to do so if they wish. I hope that cleared it up for you.
I think he got it wrong...
You didn't put dots around Cl, why ? at 5:34
Easy to learn!nice one!👍
at this point, you are my teacher.
you're the best of all time
YOU ARE ABSOLUTELY AMAZING THANK YOU you explained it so well!
thank you so much this videos actually help for understanding chem fully
Ever perfect videos.
ML Tutor 😘
Thank you :) it was very helpful when I doing my homework
Simple and easy to understand
Awesome explanation. Thanks so much
Exams in two hours
this makes soo much sense thank you sooo much (:
You are genius!
GOD BLESS YOU SIR
watching this for online class because my teacher is useless :/
Does that lone pair calculation only work when the central atom doesn’t follow the octet rule?
I have no words for your appreciation. Welldone brother.
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Can someone explain how atoms like Phosphorus can have more than 8 valence electrons even though it doesn't use the d orbital. I know he said they do use it, but atoms don't use that orbital until we get to elements like Gallium and Germanium right? Phosphorus only half-fills the 3p orbitals and fills 4s before using the 3d orbitals right?
Orbitals can be mixed to form hybrid orbitals of an energy between the filled and unfilled orbitals. Phosphorus’ d orbital is close enough in energy that it can stably form a hybrid orbital with s and o orbitals
You are great, sir❤
Thank you so much!
Wait, the electron configuration for P is 1s2,2s2,2p6,3s2,and 3p3. 2+2+6+2+3=15. That is the atomic number of P.
Why without ion charges? We in Germany learn to do it with those and not single electrons. Also the formula to calculate the lone pairs doesn't apply to every molecule. like methylisonitril f ex. Idk if I'm right pls correct me if I'm wrong
hi sir, may i ask when do we need to calculate those lone pairs?
Thnks for ur explanation bro.🖤🙏
2:33 how d is open for P? it's up to 3p
thank you so much, this really helps meeee
Thank you so much for the brilliantly explained videos you make!
Can you use that lone pair formula for all lewis structures with one central atom?
you can! I've been using it all the time :)
But how does it work with ch4 be cause using the lone pair formula you get - 12?
There is always an exception! To get the best structure check it by several ways such as LP and FC and electronegativity!
@@iislaymelillyiisharif4988 watch his previous video in which he explained the formulae he clearly mentioned that THIS FORMULAE DOES NOT WORK FOR COMPOUNDS CONTAINING HYDROGEN
Yaa .. it is applicable for any compound EXCEPT COMPOUND CONTAING HYDROGEN . HE ALREADY MENTIONED THAT IN HIS PREVIOUS VIDEO
I came for the NO!🎉
I have no word for you ❤❤❤
Meru thoupuuu sirrr 😃
2:47 Nice VIDEOS! But I'm confused: what does "3s2 3p6 3d10" MEAN?
electronic configuration bruv
@@quadriibrahim3398 OK, now I know
that lone pair formula 😎 life just got easier
Please can you explain the preparations of different organic compounds
How do i know when to draw a line or lone dots for the bonds?
Lines r only for bonds, dots go around the rest of the elements that don't contain 8 electrons already
wdym 1:11. thats just the way it is. I was hoping for an explanation.
From what I understand It is because Boron(B) has only 3 valence electrons which means It can only form a maximum of 3 Bonds, and with 3 bonds you will only get 6 electrons and not 8, therefore violating the octet rule.
THANK YOU FOR LIVING
Thank you! But, doesn't the last electron on NO2 go to O and not N since O is more electronegative?
yup
I think it's b/c the two Oxygen atoms have already achieved 8 e- based on the octet rules, so N atom can have that last e-. Please correct me if I'm wrong. :D
Always check Ur structure by several ways ,with LP and FC and electronegative best way is to check it by FC(formal charge)!
This was perfect, thank you so much! Could not have found anything better
I have an urgent question.
1.Becl2 is below octet where Be would have 4 valance electrons but my question is can't we make double bond with both chlorines and make it 8?☹️??
I know I am missing something... Because i don't know why you should place terminal atoms around the central atom in a particular shape..is it wrong to place terminal atoms randomly around the central atom ...how do you know the shape of these molecules
brilliant video tysm
Very good, I have a question what app or instrument you use? I mean that black board and the way you write on it, I m a teacher and need this good way to teach to my students, thank you
bro can you apply to be a chem teacher at UIC. we need you
Does that formula of L.P work for ions just as well as for molecules ?
at 4 mins 58 seconds, how did you calculate the number of lone pairs?.. I don't get this part. Subtract from 8. Where did you get 8 from? Sorry!
so there are 5 Cl atoms, and each of them got 8 valence electrons, so 5 x 8 = 40, total valence electrons in ICl5 is 42, so 42-40 = 2 electrons; 2/2 = 1 lone pair on the center atom
I see people draw calcium with the 3rd shell with 8 electrons and the valence with 2. Can you explain why? This is in the third row, so it’s a little confusing
So can an expanded octet create an extra shell if the number of electrons exeed 8?
Thank you so much ❤
The electron configuration for P is not correct in the video brother. its 3s^2 3p^6. You don't get to the d level until 4s^2 3d^10 4p^6. Can u please explain if I am wrong in this regard. Thank you, I love your videos by the way.
This is what I was thinking. Im a little confused.
3 is the same energy level as 3s and 3p "3" while you get 5s2 4d10 5p6 see the 4 is also apart of energy level 4
I thought the exact same thing!
great job myaaan
thanks this video very helpfull
Hi, when I try to get the lone pairs in NO my answer is 3/2, what does this mean?
hi for theast example is a dative bond formed?
In the case of so4 where number of lone pair on the central atom is -1?
Do we show charge on hypervalents or not?
Nice video...thanks
What do u mean by “n”? The “n” is the center atom. How do you know which one is the center atom?
Remember like this, the least electonegative atom is the central atom, but Hydrogen is an exeption, it can never be a central atom because it has only 1 electron.
***LITTLE TIP***: Usually(there are some exeptions like H2O) in the chemical formulas, the element which comes first is the central atom
Wish me luck, first mid-term tomorrow.
how did he derive that formula for loan pairs?