## Fall Quiz 2 2014 prep Question 3 [ENDORSED]

$sp, sp^{2}, sp^{3}, dsp^{3}, d^{2}sp^{3}$

Jose_Arambulo_2I
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### Fall Quiz 2 2014 prep Question 3

This question asks for the hybrid orbitals involved both in the C-C sigma bonds and C-H pi bonds in benzene. I know that each carbon has the hybridization of sp2 because it has three regions of electron density, but how do I find the hybrid orbitals for specific bonds, like what question 3 asks for?

Chem_Mod
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### Re: Fall Quiz 2 2014 prep Question 3  [ENDORSED]

You must consider which hybrid orbitals from each of the two bonding atoms combine to form the bond in question.

In benzene C-H bonds, one sp2 hybrid orbital from carbon forms a single, sigma bond with the unpaired 1s electron in hydrogen.

In benzene C-C bonds, one sp2 hybrid orbital from carbon forms a single, sigma bond with another sp2 hybrid orbital from carbon.

In benzene C=C bonds, one sp2 hybrid orbital from carbon forms a sigma bond with another sp2 hybrid orbital from the other carbon along with the side-to-side overlap pi bond of one unhybridized p orbital electron from each carbon. Thus, the double bond is formed from one sigma and one pi bond.