A Brief Introduction to Molecular Orbital Theory
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- čas přidán 29. 07. 2024
- Professor Davis discusses four simple examples of diatomic molecules from the molecular orbital theory standpoint. MO's of hydrogen, helium, nitrogen and oxygen are discussed. Bond orders and even magnetic properties are predicted based upon the energetics of the MO system.
I appreciate the feedback! I will be sure to correct the oversight in the next version of this video!
I love the video and enjoy the orbital vertulization. Although, there may be 2 mistakes in the video: (1) for the N2 molecule, the 2p pi orbitals should be lower in energy than the case of the 2p sigma ( en.m.wikipedia.org/wiki/Molecular_orbital_diagram#Basics).
(2) for the O2 molecule, triplet states should be formed rather than singlet....
-Hai
Great job explaining the molecular orbital theory. I was having trouble understanding it, thank you so much. I highly appreciate this video
concise and very easily to follow. good work y'all!
I am still confused as to how and where pi bonds come from? Is the pi equal to 180 degrees which is why those particular bonds are flat and straight across compared to the others that are vertical or diagonal?
Hi Satyaprakash. I use a combination of several software suites, including Microsoft Office, Adobe Illustrator and Photoshop, as well as some specialty chemical drawing programs. Each 5-10 minute micro-lecture takes anywhere from four to twelve hours of work to complete. They are all written, edited and produced entirely by me. I hope that you feel they are worth it!!!! If you agree that they are, please subscribe and pass on the channel to your friends.
Unbelievable how simple you made it. Thanks alot!
this visual repsresentation was extremely useful for understanding, thank you so much :)
Great video! This clears up any questions I had about MO diagrams.
Thanks, Jordan. You may also want to note that I posted a revised version of this lecture, accounting for sigma-pi mixing here czcams.com/video/KeRRtIZFq-M/video.html
its just awesome thanks alot professor :) stay blessed
Your visualizations are amazing. Let's collaborate together on making the world's best Chemistry guide.
Thank You Prof. It was really helpful.
Great lesson, keep it up!
This was so helpful, thank you!
Thank you... your explanation was very helpful :)
Hi Breanna. I think I was trying to convey that the electrons fail to screen the nuclei from one another, causing the mentioned 'repulsion'. A fair comment, though, as I can see how this could easily be misinterpreted to mean that the electrons are repelling the nuclei (which, of course, they are not!!!).
Thanks
Great job explaining the molecular orbital theory. I was having trouble understanding it, thank you so much.
Thanks!
Thanks, Craig. Please subscribe and share with your friends!
then how does endothermic & exothermic reaction accure,when there antibonding is there
Marvelous. Learnt a lot
that was super clear; thank you so much! :D
Thanks for watching! Please pass it on!
Nice video sir, make it easy to understand MOT, Thank you
how bonding and antibonding orbitals are arranged in a molecule? do they both form at same time and present at same time
very nice can understand clearly
Very helpful!
Thanks professor. Helped a lot
I'm so glad that you found it helpful! Thanks for the feedback.
thank you this helped a lot
why aint we consider ABMO &BO of s subshell in bond order?
Thank you
How I would know that N forms Pi bonds in the diagram of energy..I got sigma bond but this Pi looks like strange..
I mean is any order that I can know how the π bonds form in this diagram...
From which orbital is bonding decided (1s, 2s or 2p)?
Can anyone pls explain me how can 2 molecular orbitals overlap in phase and out of phase simultaneously ...i mean how can they interfere constructively and destructively at the same time ? ...the orbitals should either overlap in phase and form bonding orbital or should overlap out of phase forming anti bonding orbital ..but how can both happen at a same time ?
Thank you very much...
You are welcome! Don't forget to subscribe!
thank you
brilliant!
When you discuss the anti-bonding orbitals as destabalizing the bond...you say that the presence of these electrons in this type of orbital pushes the nucleii closer together by electro-static repulsion. I am certain you mean..."farther apart". Otherwise, a very helpful micro-lesson.
thanks
you are awesome thanks
The presentation is made in which software?
Doesnt oxygen have 6 valence electrons and nitrogen have 5 valence electrons ?
Can yo help me out. What does this line mean"Things look different in different directions for molecules than their constituent atoms(mostly losing symmetry due to another atom interacting with electron). Think only of the simplest example, H-h, to appreciate why. Here space is indelibly marked by line joining(bond) the two nuclei, which defines, once and for all, what was previously an arbitrary Z-axis. There is one special direction plain to see. and (owing to this pointer in space) the molecule is denied of the s-p-d-f orbitals of hydrogen atom. Those familiar wave functions derive slolely from 1/r coulomb potential and spherical symmetry of the atom." ( My question, why did those orbitals were denied in hydrogen gas. This paragraph is talking about shape and how orbitals are not looked. I really don't understand. Can you make it clear)
At 00:02:43, sound volume goes down.
what about 2s - 2p mixing in molecules formed by atoms of less than 16 atomic number ? I guess it decreases the energy of π and increase the energy of sigma bond in nitrogen , If am not wrong .
+divyam sheth You are correct. The sigma and pi relative energies of nitrogen are not accurately represented here. I've been meaning to update/correct that oversight for a while now. I will be creating a new version of this video later this year as some of my other projects wind down.. Thank for the comment!
what is 2s 2p how do they get labeled Tyler dewitt
Also the ordering in energy of the 2p sigma and pi bonds are different for nitrogen and oxygen homonuclear diatomics. You might want to correct and add these things. I would love to help you edit before you publish if you need it.
great
You may use this correct formula. 1/5(bonding orbital* anti bonding orbital)
i want to this ppt sir....
yeah the pi for n2 should be lower than sigma......EXCELLENT VIDEO THOUGH
nice
Only oxygen molecule have 2 unpaired electrons with same direction? en.wikipedia.org/wiki/Oxygen#/media/File:Oxygen_molecule_orbitals_diagram.JPG Thats why that molecule are paramagnetic...?
How you did the bond order and ended up with 1 as final answer. 1*0/2= 0 because of the ZERO in numerator. Thank you and please correct.
it's +, not *
+Ali Alyami The formual is:
(Bonding electrons - Anti bonding electrons)/2
There is a '-' in there not a '*'
gr8
Hi Breanna. I am always down for a little 'peer review' when it comes to my videos. Especially some of my older offerings like this one. Contact me by email through my website if you would like to talk.
8:40 mistake - paired electrons. Must be unpaired, according to Hund`s rule. You got it right on another video (at ca12 min.) czcams.com/video/KeRRtIZFq-M/video.html
or chemical survial
wake wakame.
fr.wikipedia.org/wiki/Oxyg%C3%A8ne_singulet#/media/Fichier:Molek%C3%BClorbital-Sauerstoff.png
what is 2s 2p how do they get labeled Tyler dewitt