Molecular Structure 4.111

(Polar molecules, Non-polar molecules, etc.)

Moderators: Chem_Mod, Chem_Admin

Semi Yoon
Posts: 60
Joined: Fri Sep 28, 2018 12:27 am

Molecular Structure 4.111

Postby Semi Yoon » Wed Nov 14, 2018 11:33 pm

How would you describe the structure of the CH3CN molecule in terms of hybrid orbitals, bond angles, and sigma and pi bonds when the N atom is a terminal atom?

Posts: 18400
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 435 times

Re: Molecular Structure 4.111

Postby Chem_Mod » Thu Nov 15, 2018 9:59 pm

First, draw the lewis structure. You will find that the C in CH3 is bonded to the central C. That central C is also triple bonded to N, which also has a lone pair.

The C in CH3 has 4 regions of electron density, making it sp3 hybridized.
The central C and N both have two regions of electron density and are thus sp hybridized.

The Sp3 hybridized C and its attachments form a tetrahedral shape and has bond angles of 109.5.
Conversely, the central C and N are both sp hybridized and are linear, meaning it has bond angles of 180.

Lastly, single bonds are composed of 1 sigma bond whereas the triple bonds consist of 1 sigma and 2 pi bonds.

Bingcui Guo
Posts: 30
Joined: Fri Sep 28, 2018 12:19 am

Re: Molecular Structure 4.111

Postby Bingcui Guo » Thu Nov 15, 2018 11:51 pm

C in CH3 has 4 bond with no lone electron pairs so it should be tetrahedral with bond angle 109.5 degree. And the C and N forms the triple bond so the bond angle should be 180 degree. for single bond it is sp3 hybridization so C in CH3 has 3 sigma while for triple bond, it is sp hybridization and C with N has 1 sigma and 2 pi

Return to “Determining Molecular Shape (VSEPR)”

Who is online

Users browsing this forum: No registered users and 5 guests