I find it quite surprising that it is often the unpopular videos that clarify all the doubts, I surfed the web and couldn't find the orbital diagram of O2 molecule. Thank you. :)
This was exactly what I was looking for. I couldn't figure out how the orbital diagram would be visualized onto an overlap diagram and this was amazing. Thanks!
You have drawn singlet oxygen which is the first excited state. Normally oxygen will be in the ground state which is a triplet (di-radical) with no pi bond.
Hey there, wondering why the oxygen MO diagram video is showing unhybridized orbitals while this video shows hybridized orbitals, thanks in advance for your help!
Actually the explanation is very good but the problem is that probably you are WRONG. I mean that in some places,I am seeing that they say that in such diatomic molecules, there is no hybridisation. In oxygen molecule, there will be simply a sigma bond between Pz orbitals of both atoms. I don't support them but please clarify.
You can think of the sphere at the centre as 1s orbital, if you want to. Often the inside orbitals that do not interact with anything else is ignored while drawing diagrams.
@@thechemist6957 only the orbitals that are close in energies can mix together to form hybrid orbitals. that's why the lower energy 1s orbital is ignored as the energy difference is high because of one less electron shell.
I find it quite surprising that it is often the unpopular videos that clarify all the doubts, I surfed the web and couldn't find the orbital diagram of O2 molecule.
Thank you.
:)
He drew diagram for singlet O2, an excited state. Ground state O2 is triplet, aka a diradical.
This was exactly what I was looking for. I couldn't figure out how the orbital diagram would be visualized onto an overlap diagram and this was amazing. Thanks!
Very clear and thorough explanation! Thank you very much, quite appreciated. Not to mention it's the hand acting for me.
Thank you!!!! This was such a good, clear, representation!!!
you made something so complicated literally so simple. thank you so much. may God bless you.
My guy, you saved my brain cells from trying to understand how hybridisation and orbital overlap are related. Thank you
You have drawn singlet oxygen which is the first excited state. Normally oxygen will be in the ground state which is a triplet (di-radical) with no pi bond.
That's art.. Beautiful..
YOU Saved my life thanks !!
How many are from India fill attendance 👍👍
Lol only 24 from India 😂😂😂..
I guess Indians don't like to study
Best explanation ever
Thank you for the explanation
Hey there, wondering why the oxygen MO diagram video is showing unhybridized orbitals while this video shows hybridized orbitals, thanks in advance for your help!
Actually the explanation is very good but the problem is that probably you are WRONG. I mean that in some places,I am seeing that they say that in such diatomic molecules, there is no hybridisation. In oxygen molecule, there will be simply a sigma bond between Pz orbitals of both atoms. I don't support them but please clarify.
i have this objection too
Yes exactly, i was thinking the same thing
All the three sp2 hybrid orbitals are not identical. One sp2 hybrid orbital carry one electron while other two carries two electrons each?
Love this
Thanks a lot for clearing my doubts😊😊
How does oxygen end up with unpaired electrons in o2 then?
Very clear
Thanks sir
thank you king 👑
Why aren’t 1s orbitals depicted in the drawing? Are only the hybridized sp2 orbitals and 2p orbitals(needed for pi bonds) shown?
You can think of the sphere at the centre as 1s orbital, if you want to. Often the inside orbitals that do not interact with anything else is ignored while drawing diagrams.
@@Anandhu-X Thank you. Also, is the 1s orbital ever involved in hybridization?
@@thechemist6957 No, in the above mentioned sp2 hybridization, the s & p subshells belonging to principal quantum number 2 only (2s &2p) are involved.
@@thechemist6957 only the orbitals that are close in energies can mix together to form hybrid orbitals. that's why the lower energy 1s orbital is ignored as the energy difference is high because of one less electron shell.
I just wanna know where the lone pairs go
why is there only 1 leftover p orbital? is it because there's only one pi bond?
I mean here in Switzerland we learn the MO-Theory with O2 having only one bond in high school.
Powerful Sir
Very explanatory
Thank you 🙏 ❤
Thank you sir!!
I love your videos , but the scratching of the sharpies are killing me soooo bad
Thank you
So O2 diamagnetic?
Thanks alot
Good
Thanks sir
Thank u can u make of these informative videos
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2:41. 5:28