Problem: Butadiene, C4H6, is a planar molecule that has the following carbon-carbon bond lengths:From left to right, what is the hybridization of each carbon atom in butadiene?

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We are being asked to determine the hybridization of each carbon atom in butadiene.


The figure shows a molecule with the following structure: H2CCHCHCH2, with a double bond between the first and the second and also between the third and the fourth carbon atoms. The bond between the second and the third carbon atoms is single and has the length of 1.48 angstroms. Each double bond has the length of 1.34 angstroms.


Recall: 

Hybridization is a mathematical procedure in which the standard atomic orbitals are combined to form new atomic orbitals called hybrid orbitals that correspond more closely to the actual distribution of electrons in chemically bonded atoms.

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Problem Details

Butadiene, C4H6, is a planar molecule that has the following carbon-carbon bond lengths:

The figure shows a molecule with the following structure: H2CCHCHCH2, with a double bond between the first and the second and also between the third and the fourth carbon atoms. The bond between the second and the third carbon atoms is single and has the length of 1.48 angstroms. Each double bond has the length of 1.34 angstroms.

From left to right, what is the hybridization of each carbon atom in butadiene?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Hybridization concept. You can view video lessons to learn Hybridization. Or if you need more Hybridization practice, you can also practice Hybridization practice problems.

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Based on our data, we think this problem is relevant for Professor Marzal's class at UCF.