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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: theunraveler on September 23, 2006, 02:09:05 PM

Title: Molecular hybridization
Post by: theunraveler on September 23, 2006, 02:09:05 PM

i have a question on hybridization. Generally in a benzene structure u have each carbon bonded to 2 other carbon and 1 hydrogen, the carbon forms an sp2 hybridization with the other atoms. pi bonds above C atom and sigma bonds in a regular hexagon shape along the plane

so my question is will the hydrogen atom will form a sigma bond with the carbon rite? if so, then the carbon it is attached to will be having more than 1 sigma which isnt possible.... rite?

Title: Re: Molecular hybridization
Post by: Yggdrasil on September 23, 2006, 02:14:50 PM

The C-H bond in benzene is a sigma bond.  Since carbon is sp² hybridized, it has three sp² orbitals and one p orbital.  Each sp² orbital participates in a sigma bond (2 C-C bonds and 1 C-H bond), while the p-orbital participates in the conjugated pi-bond system which gives benzene its aromaticity.

Title: Re: Molecular hybridization
Post by: theunraveler on September 23, 2006, 02:39:54 PM

so the pi bond will be above and below the plane rite?

Title: Re: Molecular hybridization
Post by: Dan on September 23, 2006, 02:57:30 PM

http://www.monos.leidenuniv.nl/smo/basics/images/benzene.gif

Don't underestimate google searches.

Title: Re: Molecular hybridization
Post by: Yggdrasil on September 23, 2006, 03:30:10 PM

Yes, as Dan's picture shows, the pi-bond system is ablove and below the plane of the carbon atoms.

Title: Re: Molecular hybridization
Post by: theunraveler on September 25, 2006, 11:55:10 AM

swet ...thanks :)