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unhybridized orbitals?

Posted: Tue Dec 03, 2019 3:22 pm
by Giovanni Anguiano-Gutierrez 3L
I am not quite sure how you would obtain an unhybridized orbital for hybridization. Take ethene for example, C is its central atom and its hybridization is sp^2 because of the three electron densities, but when writing it out where does the 2p orbital with an electron come from?

Re: unhybridized orbitals?

Posted: Tue Dec 03, 2019 7:52 pm
by Ryan Yee 1J
In ethene, the carbon has to hybridize its p and s orbitals, so it can create four bonds. My guess is that in order to hybridize, Carbon requires some energy and so it would only create as many hybridized orbitals as it needs. Since, in ethene, it only needs 3 electrons to form sigma bonds, carbon only hybridizes three so that the other one doesn't have to use energy and undergo hybridization.

https://www.chemguide.co.uk/basicorg/bo ... thene.html

Re: unhybridized orbitals?

Posted: Wed Dec 04, 2019 12:28 am
by Jasmine 2C
Giovanni Anguiano-Gutierrez 3L wrote:I am not quite sure how you would obtain an unhybridized orbital for hybridization. Take ethene for example, C is its central atom and its hybridization is sp^2 because of the three electron densities, but when writing it out where does the 2p orbital with an electron come from?

I am very confused about this topic too. How do we know when there are unhybridized orbitals?