14.2/S2.2.15 Explain hybridization as mixing of orbitals making new orbitals [HL IB Chemistry]
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- Опубликовано: 12 сен 2024
- Minor error at 4:27: pi bonds are PERPENDICULAR (not parallel) to the internuclear axis.
Nasty business this. Once or twice the IB asked a question that needed the details presented here -- but more often than not a simple treatment is required.
![4.3/S2.2.1 Lewis structures of molecules/ions for up to 4 electron pairs per atom [SL IB Chemistry]](http://i.ytimg.com/vi/nw3xVVmEAU8/mqdefault.jpg)
OH MYGOSH. I'M CRYING. TEARS OF JOY BECAUSE I UNDERSTOOD. YOU'RE AMAZING
That makes up for the kid I made cry teaching this!
Wonder if he/she knows about hybridization by now
Most concise and best hybridization video I've come across yet.
it took me weeks to make this one!
thank you very much.
Richard Thornley I love you
Richard Thornley wow amazing work !
This was the only hybridization video on RUclips that I could understand. Good job. These step by step assigning is really understandable.
THANK YOU SO MUCH! After watching around 10/20 different videos, I finally come across one where I ACTUALLY understand hybridisation! Thank you 😊
Richard, you saved my life in high school and I am still going back to your videos years later in university. Thanks so much!
I took SL IB Chemistry and now I'm at University learning HL concepts. Still learning from you.
Thank you, i owe my diploma to you now, 1 day before the final exam, still didnt get sigma pie bonds with hybridization, but now I do thanks
I laughed waaay to hard at the "Delta G must be negative"
I didn’t get itttt HELP
@@sanyamishra2825 same ._.
@@sheaj1872 change in gibbs free energy (delta G) is negative for spontaneous reactions
hv seen so many on hybridisation - this gives the best explanation and understanding - Thanks a Ton !
If I recall the IB did ask this once in detail many moons ago.
thanks mate. i have been studying around 5 hours but didnt understand anything. this 5 min is phenomenal. thanks
Hmm - that is a good point well made - I think you are (gulp) correct. Your comments are consistently excellent. Assuming px is on the internuclear axis (which seems reasonable) then I should have taken it into the hybrid orbital everytime. I thought I had made the definitive video on this -agggggghhhh!
This is brilliant! I finally completely understand hybridization. Many, many thanks for all your videos, keep it up.
Thank you so so much! I have a test on this (and organic chemistry) on Friday, you're a lifesaver!
You hero I have my chem end of year paper tomorrow and you’ve saved me
Why do I only discover your channel one day before my Chem HL exams... It could have saved me so much stress! Thank you anyway!
Get a good nights rest too - and don't neglect the option.
I was taught that for the sp2 orbital it is the 2pz orbital which remains unhybridized, rather than the 2px (3:02 in the video)... I'm a bit confused as to whom I should trust >.
you are correct - the error does not change the IB chemistry answer - but it is a mistake.
Hey no problems - its really great that you reply to our questions etc... I thought it was just an oversight i think we all knew what you meant ! I just wanted to be sure i wasnt missing anything.
Thanks
I was literally crying before I saw this video. Thank you for explaining it very clearly!
You know.....Life became easier after this video.....Could breathe again.Thank You.
best explanation of hybridization on youtube
So the reason as to why atomic orbitals hybridize is to achieve the same energy? Because the s is lower in energy than the p, and if the atomic orbitals didn't hybridize, the first "bonding" electron from a nearby atom would be placed first in the s orbital making it a more "unstable" or "s level favorable bond?" In doing so, does this also limit the number of atoms that can bond with the molecule? If so, why? And now that everything is hybridized, there is even bonding among all orbitals?
2 years well spent! Great Job mate, thx!
I'm at university and your videos are still helping me so many years later
you must have been on of the first subscribers then!
Thank you so much. My lecturer showed it to us, rewatching it again :)
I have been waiting for a video on this syllabus point for 13 months! THANK YOU SO MUCH!
Just great Richard! I understood this topic but something wasn't clicking. Now it has. Thanks =)
YES. That actually makes sense, especially about why each orbital is called what
Thanks for simplest explanation..🙏😊
Great video
How about lone pairs? Do they change the number of paired electricians in the hybrid orbitals?
hey rick! what a coincidence you uploaded this today! they asked this in the november hl chem exam yesterday that i just finished. hehe...
First of all, thank you very much for your videos! They are very helpful and you are an extraordinary teacher!
Secondly, I have a question... Do we need to know how to draw those examples with the orbitals hybridising?
Thanks a lot.
First hybridization video that actually helps. thank you.
Could you please tell which application are you using to make these videos.... loved your work
The board work is activboard, the animation is 3dsmax - i have used it for 20 years and i have barely scratched the surface. It is free if you are a teacher or student.
This really simplified things I understand this much better now!!! Thank you 😭
Orbitals do not need to hybridize every time to make a sigma bond eg H2
If, after hybridisation, there is still a p-orbital left with an electron in it, then there will be a pi bond.
Probably.
Wow never understand it from my teacher, best explanation ever thanks !!
God bless you, Sir for this video. Thank you.
Thanks.. This is fine to realize box form of hybridization
it was definitely worth it. I'm still a little confused by it but this helped a lot!!!
thank you
"are you crying yet" - instant sub
this was absolutely phenomenal. My mind is blown
Great video. I made it all the way to the end without crying. :P
why are you so awesome? GREAT GREAT VIDEOS i really appreciate you doing this! and i know all chemistry IB students all around the world do too!
Hello there Mr. Thornley: When you talk about sp2 hybridization, there's one less electron on the left. so its not a carbon atom anymore, right? The configuration should be 2.3?
it is still a carbon atom, with 1s2 sp2 (which contains 3 electrons) 2p1
Rich,it seems as though the Px orbital is always a pi bond (i.e the orbital that is left behind and not included in the sp and sp2 hybridisation) - but i thought that Px implies sigma bonds? Clarify? Thanks.
very good try to do for 3 days got in 3 mins thnx tell me which software did u use
This excellent. What program did you use to for the graphics?
3d studio max
tough luck buddy! Did the exam go OK?
When the orbitals hybridise, are they only then able to form sigma bonds? Can they not form pi bonds? Thanks so much for your videos by the way - they're really helpful!
It was so helpful. Thank you. 👍
Thank you for this video!
Why are the videos in the playlist in the wrong order? The explanation for sigma and pi bonds come after this video.
+JfernandesTV Thanks - I moved it.
This video help me for understanding of hybridization more easily.
I enjoyed your video, but got confused about one aspect. For methane, your referred to the sp3 orbitals as "it," i.e. you've implied that one sp3 orbital is formed from 1s and 3 p orbitals. However, I am pretty sure that this is not the case, as 4 sp3 orbitals have been formed. Otherwise, wouldn't the molecular orbital theory be violated?
+Ruslan Mushkaev yup 4 orbitals are formed.
That Gibbs free energy joke is genius
thank you sir i understood and god bless u for ur service
Hi Mr. Thornley, I never understood this. For the sp2 hybridization, why couldn't the double bond between C and O in H2CO just be 2 sigma bonds using an sp3 hybridized bond? Why must it be 1 sigma sp2 hybridized bond and 1 pi 2Px bond? Thanks :)
Also, if it is related to the charge centers, how? It seems that in the next video it's only stated, not explained :S Sorry if it's beyond the IB Syllabus
Michael Jonathan
single sigma = 1 charge center
sigma and pi double bond = 2 charge centers
sigma and 2 x pi triple bond = 3 charge centers
lone pair = 1 charge center
I think that a double bond cannot be 2xsigma because the sigma is along the internuclear axis and there is no room for 2 bonds there only room for one.
The pi bond is half above/half below this axis so there is room for it.
probably...
Perfect! Thanks for this. :)
Why do we take pz orbital to hybridize with the s instead of the other two?
in reality it does not matter which orbital you choose.
I see, so it's energy that determines the location of the electrons, i.e. if there are free slots in the hybridized orbital, then there will only be one electron each in the unhybridized p orbitals, and the other electrons will be in the hybridized orbital to minimize energy.
Thank you so much sir
Thanks a lot...u truly are a good lecturer
x y and z axes are interchangeable. so i believe it really does not matter.
amazing amazing amazing
clear all the concept
how do you tell when to use which hybridizing technique
Was absolutely worth it, Thanks
Wow! Thanks for putting this up! Really helped a lot
This literally saved me!! Thank you so much!!!!!
It was worth it, thanks a lot
thank you for the video it's really helpful and cool u helped me to imagine the structure
Helo, Mr. Thornley, how do we show the atomic orbitals leading to hybrid orbitals for SO3 and PO4 3- ??
Can you explain in detail, please ? Thank You...
wow - if I was that smart ... no idea sorry. That is IB+3 chemistry - whereas I am only humble IB.
But why hybridization occurs ? why S +P = Sp^3 etc combine ? . so that carbon can get 8 electron at the outer shell ? . if so why "S" got more then 8 Electron ?
But why and how does hybridization happen? Does it happen as the atom bonds to another and the other atom therefore causes the sublevels to hybridize and change positions...? Is this what causes the energy to be released in formation, as the orbitals drop down a portion of an energy level?
Why does learning chemistry just create more questions...? :(
+Cherry.Bakewell
I had the exact same question...This is the answer I found:
"Hybridization was introduced to explain molecular structure when the valence bond theory failed to correctly predict them."
"According to Valence Bond Theory, carbon should form two covalent bonds, resulting in a CH2, because it has two unpaired electrons in its electronic configuration. However, experiments have shown that CH2 is highly reactive and cannot exist outside of a reaction. Therefore, this does not explain how CH4 can exist. To form four bonds the configuration of carbon must have four unpaired electrons."
Taken from: chemwiki.ucdavis.edu/Core/Organic_Chemistry/Fundamentals/Hybrid_Orbitals
David Peana Ahhh, that makes a lot more sense. Thank you!
you are THE BEST!
What does the 2:4 mean? I know you said that "it has an electron configuration of 2:4," but I don't see how that fits in with anything you did in this video.
First shell of electrons has 2, second shell has 4
hey rick i would like to know what software you are using in this video
activstudio
was definitely worth , thank u very much :)
Outstanding!!! Mr. THornley!! WOW!
God you made it look so easy!!
Thank you soooo much!! :D
U r awsm .... i understood it in a jiffy..nice work.:')
Sir, you saved my life
yea it was actually a pretty good exam, compared to may :) good work ib!
im so confused.. how do you know if something is going to be a sigma or pi bond? what are the rules?
all covalent bonds have one sigma bond - the rest are pi!
Helped so much thank you!!!
it was well worth it! thanks a lot!
BEST OUT OF BEST!!!!
Got full clarity..............................
You are incredible THANK YOU😘❤️
THANKS SO MUCH RICHARD
In my chemistry textbook it says an s orbital + pz orbital is nonbonding, but in the HCN example there is a bond, why is that?
yup - this video is good enough for IB but does contain that error.
the best video ever
3dS max 11
Helping survive another semester in IB
Yes it was worth it!
Thanks much!:)
Beautiful
Nice its amazing
u r AMAZING! THANKSS 😄😄😄
what a video!
Thanks a ton!!!
THANK YOU SO MUCH