Moderators: Chem_Mod, Chem_Admin

Posts: 101
Joined: Sat Aug 17, 2019 12:16 am


Postby KNguyen_1I » Mon Nov 18, 2019 4:09 pm

2.57 Acetonitrile, CH 3 CN, is used as a solvent in the pharmaceutical industry. Describe the structure of the CH 3 CN molecule in
terms of hybrid orbitals, bond angles, and s - and p -bonds. The N atom is a terminal atom.

How would you describe the hybridization of the triple bond? How would you draw the electron configuration of each C atom?

Justin Vayakone 1C
Posts: 110
Joined: Sat Sep 07, 2019 12:19 am

Re: 2.57

Postby Justin Vayakone 1C » Mon Nov 18, 2019 11:07 pm

Image of Lewis Structure: https://ibb.co/FbB3TwM

There are 2 electron densities around the right carbon, so sp hybridized orbitals are used for the triple bond. Here is the electron configuration shown by my epic MS paint skills: https://ibb.co/kQTh67k

For the left carbon atom, sp^3 orbitals are used, so the electron configuration would look like this:

Posts: 101
Joined: Sat Aug 17, 2019 12:16 am

Re: 2.57

Postby KNguyen_1I » Tue Nov 19, 2019 10:23 pm

So no matter what there are always four orbitals in order to indicate the four possible bonds but the hybridization varies?
Also thank u btw your microsoft paint skills are legendary

Ziyan Wang 3J
Posts: 51
Joined: Wed Sep 18, 2019 12:22 am

Re: 2.57

Postby Ziyan Wang 3J » Thu Nov 21, 2019 2:39 pm

My answer is that for first C: sp3,109.5,4 sigma, 0 pi, for second C: sp, 180, 2 sigma, 2 pi

ValerieChavarin 4F
Posts: 99
Joined: Wed Sep 18, 2019 12:18 am

Re: 2.57

Postby ValerieChavarin 4F » Sat Nov 23, 2019 4:05 pm

For the right carbon you use hybridized orbitals while the left carbon uses

Return to “Hybridization”

Who is online

Users browsing this forum: No registered users and 1 guest