## 2.57

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

KNguyen_1I
Posts: 101
Joined: Sat Aug 17, 2019 12:16 am

### 2.57

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

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:
https://ibb.co/xMpvhjD

KNguyen_1I
Posts: 101
Joined: Sat Aug 17, 2019 12:16 am

### Re: 2.57

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

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

For the right carbon you use $sp$ hybridized orbitals while the left carbon uses $sp^{3}$