## UA Workshop Number 6a

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

Cecilia Cisneros 1F
Posts: 133
Joined: Wed Sep 30, 2020 9:45 pm

### UA Workshop Number 6a

Hi! I attended Matthew Tran's workshop earlier, but I didn't get to stay at until the end. I was reviewing my answers with the answers from the workshop that someone kindly shared with me, but I was having trouble understanding the answer to 6a.

"6. For each of the following molecules, identify the the orbital hybridization of the
bolded and underlined atom:
a. CH3NNCH3"

I thought the hybridization was sp^3, but the answer was sp^2 does anyone know why?

Thomas Vu 1A
Posts: 108
Joined: Wed Sep 30, 2020 10:08 pm
Been upvoted: 1 time

### Re: UA Workshop Number 6a

So the N is single bonded to a C, double bonded to another N, and has 1 lone electron pair. So there are basically 3 regions available which translates into a sp2 hybridization.

Crystal Pan 2G
Posts: 113
Joined: Wed Sep 30, 2020 10:04 pm
Been upvoted: 2 times

### Re: UA Workshop Number 6a

It is sp^2 because there are three regions of electron density. The double bond with the other N, the lone pair, and the single bond with C. The double bond still counts as 1 region of electron density, so there are 3 regions which means it is sp^2.

Posts: 107
Joined: Wed Sep 30, 2020 9:42 pm

### Re: UA Workshop Number 6a

Here's a lewis structure representation of the compound (let's hope it works lol)

H H
| .. .. |
H - C - N = N - C - H
| |
H H

You can see that the nitrogen atom has 3 regions of electron density (single bond with carbon, double bond with the other nitrogen, and the lone pair). Thus the hybridization is sp^2. Hope this helps!

Posts: 107
Joined: Wed Sep 30, 2020 9:42 pm

### Re: UA Workshop Number 6a

Jillian Labador 2F wrote:Here's a lewis structure representation of the compound (let's hope it works lol)

H H
| .. .. |
H - C - N = N - C - H
| |
H H

You can see that the nitrogen atom has 3 regions of electron density (single bond with carbon, double bond with the other nitrogen, and the lone pair). Thus the hybridization is sp^2. Hope this helps!

Okay clearly that did not work :| but you get the idea