Lecture #23


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Melody Haratian 2J
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Lecture #23

Postby Melody Haratian 2J » Sun Nov 29, 2020 10:43 am

Hi guys!
I was going over lecture #23 and had something I was a little confused on.
For the molecule Benzene (C6H6)
where is the electron for the un-hybridized p-orbital located? Also, is it delocalized?
Thanks!

705340227
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Re: Lecture #23

Postby 705340227 » Sun Nov 29, 2020 11:13 am

Each carbon has one unhybridized p-orbital, so therefore there are 6 unhybridized p-orbitals throughout the whole molecule. Because this structure exhibits resonance, some of the electrons are delocalized, do the molecules can share these electrons. I believe that the six unhybridized electrons are shared equally by the six p-orbitals, forming a pi molecular bond above and below the ring structure.

I think that is what he said during lecture, but if someone could confirm that would be great.

Lucy Wang 2J
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Re: Lecture #23

Postby Lucy Wang 2J » Sun Nov 29, 2020 11:17 am

Yes the electrons are delocalized and a pi bond is formed above and below the ring.

Yichen Fan 3A
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Re: Lecture #23

Postby Yichen Fan 3A » Sun Nov 29, 2020 11:33 am

Yes, the electrons in unhybridized 2p orbitals are delocalized; those delocalized electrons form delocalized pi bonds perpendicular to the molecule. Essentially delocalized pi bonds will only appear when there are resonance structures for molecules which involves double or triple bonds.

Reese_Gover2K
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Re: Lecture #23

Postby Reese_Gover2K » Sun Nov 29, 2020 11:49 am

Yes some electrons are delocalized meaning that they are shared between the atoms

rhettfarmer-3H
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Re: Lecture #23

Postby rhettfarmer-3H » Sun Nov 29, 2020 4:30 pm

yes, it is delocalized. I think of it as for the sake of the structure having multiple figures for the double bonds. The overall bond lengths for one of the bonds in each of the carbons have to be different from the rest of the hybridized other bonds. Therefore, these represent that pi bond in the double bond, and each carbon gives one. There have to be these different bonds for the sake of stability.

Varsha Ravi 3E
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Re: Lecture #23

Postby Varsha Ravi 3E » Sun Nov 29, 2020 4:52 pm

Yes, they are delocalized.

Gabe_Ek 1G
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Re: Lecture #23

Postby Gabe_Ek 1G » Sun Nov 29, 2020 5:00 pm

Yes, that's true. Some of the electrons are delocalized which means they form delocalized pi bonds that are perpendicular to the Benzene molecule which can also share these electrons.

FionaHunter21
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Re: Lecture #23

Postby FionaHunter21 » Sun Nov 29, 2020 7:02 pm

Are electrons only delocalized when the shape is a ring or can it happen with any molecules that have resonance structures?

Natallie K 3B
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Re: Lecture #23

Postby Natallie K 3B » Sun Nov 29, 2020 7:39 pm

Electrons are delocalized whenever there is a resonance structure, not just a ring such as benzene.

Giselle_zamora_1L
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Re: Lecture #23

Postby Giselle_zamora_1L » Sun Nov 29, 2020 11:09 pm

Hi all, i also was conceptually confused on the delocalized election?

Mina Tadros 3L
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Re: Lecture #23

Postby Mina Tadros 3L » Sun Nov 29, 2020 11:11 pm

Yes, since it is a resonance structure, they are delocalized.

Nina Tartibi 1F
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Re: Lecture #23

Postby Nina Tartibi 1F » Sun Nov 29, 2020 11:38 pm

Natallie K 3B wrote:Electrons are delocalized whenever there is a resonance structure, not just a ring such as benzene.


This might be redundant but, when electrons are delocalized does it just mean that the structure has resonance or is there more to it than that? I was also a bit confused on this

Edward Castro
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Re: Lecture #23

Postby Edward Castro » Sun Nov 29, 2020 11:42 pm

Yes i agree with the posts above. They can be delocalized.


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