Page 1 of 1

### Fall 2012 Q6A

Posted: Mon Oct 31, 2016 12:07 am
Hello,

For this problem I don't understand how you find the hybridizations.

Do we assume the carbon will just make two hydrogen bonds? Or is it possible it may form a double bond? Would we have to calculate FC and figure that out, or can we assume it will just get 2 H bonds as problem only states that H and lone pairs are omitted?

Thanks.

### Re: Fall 2012 Q6A  [ENDORSED]

Posted: Mon Oct 31, 2016 11:39 am
The problem description states that there are "lone pairs omitted" and "...some of the hydrogen atoms attached to carbon atoms are omitted."

Thus, it is helpful to write in the missing H atoms on the ring and the lone pairs on the N and both O atoms.

If you do this, the hybridization (based on the number of regions of electron density) should become apparent.

### Re: Fall 2012 Q6A

Posted: Tue Nov 01, 2016 4:27 pm
I still don't understand this question. Even after writing in the hydrogen atoms, I do not understand hoe the carbon atoms have a sp^3 hybridization. From my point of view, I can only see 3 regions of electron density around the carbon atoms in the ring structure. Thus, I keep getting sp^2. Is there a lone pair somewhere that I am missing? Thanks

### Re: Fall 2012 Q6A

Posted: Tue Nov 01, 2016 5:10 pm
In the ring, the carbons each make two bonds, either to another carbon or to the nitrogen. Since the problem states hydrogens have been omitted and we know carbon likes to make 4 bonds, we would add in two hydrogens to each carbon to fulfill their octet. Therefore, each carbon actually makes 4 bonds. 4 bonds will give us an sp3 hybridization.

Hope that helps.

### Re: Fall 2012 Q6A

Posted: Tue Nov 01, 2016 5:11 pm
It actually has four areas of electron density because each carbon is attached to two carbons (or one carbon and the nitrogen), as well as two hydrogens.