5:34 you just answered my big picture question that's been bugging me for days. That is, as more Zn atoms incorporate into a solid lattice, for whatever reason, the energy levels of the antibonding and bonding orbitals converge into each other past our reference 0 meaning the energy level of a lone atom. So as you add in, or excite into from lower orbitals, electrons to this mixed band of virtual empty orbitals, they will map to both bonding and antibonding addresses (antibonding by definition existing anywhere but the bond ie can travel into neighbor atoms) and that's why this material conducts electricity at room temperature. In semiconductors I believe the band gap is very small and ambient heat is enough to excite them into antibonding orbitals
How can I know if two bands (as in the case with Zinc) will overlap and those which won't (like in your previous example)? Is there a definite way of knowing it or are we supposed to know the cases with all the conductors?
Solid state chemistry is more lovely and easy to catch up comparing to solid state physics(physics student🤔 myself). Thanks for ur valuable lectures. Y can't you show MO diagram for silicon and any insulator. U didn't explain y it have large band gap
are the filled bands always called "valence bands" and the empty bands called "conduction bands"? i wasn't sure because on the first picture you named both "valence bands" but not in the second picture
In hindsight, I don't think that I should have labeled the entire set of levels the "valence band." I think technically the "valence band" is the band of highest energy filled orbitals (like the highest occupied molecular orbital, HOMO, from MO theory) and the conduction band is the lowest energy band of unfilled orbitals (like the lowest unoccupied molecular orbitals, LUMO, of MO theory). Does that help to clarify?
All videos are the same. No one explains why the MOs build up to form bands to begin with, and how does it apply to a 3D array (crystal). And if Cu can form a covalent S-S bond like hydrogen, why does it form crystals and not diatomic molecules??? Useless, just useless.
th-cam.com/video/Bjf9gMDP47s/w-d-xo.html...watching this might be of some help... I mean it's because copper is a metal unlike hydrogen(which forms covalent bond).. Metal forms metallic bonds creating a sea of electrons effecting all the other n number of atoms beside it.
Thank you!!! This helped me so much, my profs powerpoints are useless :(
Plus you have such a happy voice, it makes it more enjoyable ^-^
5:34 you just answered my big picture question that's been bugging me for days. That is, as more Zn atoms incorporate into a solid lattice, for whatever reason, the energy levels of the antibonding and bonding orbitals converge into each other past our reference 0 meaning the energy level of a lone atom. So as you add in, or excite into from lower orbitals, electrons to this mixed band of virtual empty orbitals, they will map to both bonding and antibonding addresses (antibonding by definition existing anywhere but the bond ie can travel into neighbor atoms) and that's why this material conducts electricity at room temperature. In semiconductors I believe the band gap is very small and ambient heat is enough to excite them into antibonding orbitals
Your videos are so underrated! This is amazing. Thank you!
Thank you sir. I had been searching for this particular concept and you perfectly cleared my queries
Thank you a lot . I was studying from slides of a book from which I understood nothing. After watching this video everything became crystal clear.:)
Why did you draw 4p orbital instead of 4s antibonding orbital in zinc example unlike cu?
How can I know if two bands (as in the case with Zinc) will overlap and those which won't (like in your previous example)? Is there a definite way of knowing it or are we supposed to know the cases with all the conductors?
YOU ARE A GREAT MAN THANK YOU THANK YOU THANK YOU. YOU SAVED MY FINAL EXAM THAAAANNNNKKKSSSSS
thank you a lot! i study chemistry in Germany, its hard to understand some explanations in German, but you are really great at explaining the topic!
Dude,you're awesome! definitely subscribing and showing my peers
Thank you so much! Best explanation ever!
the best explanation!
Awesome explanation, thank you so much!
Thanks so much! Really helped me understand.
Awesome...that was a great explanation
why havent you shown 4S electrons in antibonding orbitals of zinc and instead you showed 4p orbitals?
this is super useful! Thanks!
Thank you sir!!
Solid state chemistry is more lovely and easy to catch up comparing to solid state physics(physics student🤔 myself). Thanks for ur valuable lectures. Y can't you show MO diagram for silicon and any insulator. U didn't explain y it have large band gap
are the filled bands always called "valence bands" and the empty bands called "conduction bands"? i wasn't sure because on the first picture you named both "valence bands" but not in the second picture
In hindsight, I don't think that I should have labeled the entire set of levels the "valence band." I think technically the "valence band" is the band of highest energy filled orbitals (like the highest occupied molecular orbital, HOMO, from MO theory) and the conduction band is the lowest energy band of unfilled orbitals (like the lowest unoccupied molecular orbitals, LUMO, of MO theory). Does that help to clarify?
yes, thank you!
thx ...awesome help
Hey, Clayton. Min 0:00 to 3:25 it's "Valence" or "Valency" not "Valance". You're welcome.
you sound like the guy on Animal Planet 101 dogs
Be mine Clayton
All videos are the same. No one explains why the MOs build up to form bands to begin with, and how does it apply to a 3D array (crystal). And if Cu can form a covalent S-S bond like hydrogen, why does it form crystals and not diatomic molecules??? Useless, just useless.
these are my questions exactly
th-cam.com/video/Bjf9gMDP47s/w-d-xo.html...watching this might be of some help... I mean it's because copper is a metal unlike hydrogen(which forms covalent bond).. Metal forms metallic bonds creating a sea of electrons effecting all the other n number of atoms beside it.
why havent you shown 4S electrons in antibonding orbitals of zinc and instead you showed 4p orbitals?
4s is completely filled