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Kathleen Vidanes 1E
Posts: 62
Joined: Fri Sep 29, 2017 7:07 am


Postby Kathleen Vidanes 1E » Mon Nov 27, 2017 6:38 pm

Hello, I have a question regarding the Lewis Dot Structure of N2H6.

During my discussion section, my TA drew this so that both N's would each have one valence electron on them (radical). However, if I drew a double bond in between the two N's instead, would I be wrong? I calculated the formal charges and all of them would still equal zero. Also, there would still be the correct number of electron pairs needed (16) if I draw it with a double bond.

Angel Ni 2K
Posts: 50
Joined: Sat Jul 22, 2017 3:01 am

Re: N2H6

Postby Angel Ni 2K » Mon Nov 27, 2017 9:14 pm

The nitrogen is already very unhappy having 9 outer shell electrons in the single bond. I imagine that it will become suicidal if you decide to give it 10 outer shell electrons with the double bond. It wasn't even supposed to have an expanded octet in the first place. Don't force the relationship or else everything will fall apart.

Isaiah Little 1A 14B
Posts: 50
Joined: Fri Sep 29, 2017 7:05 am

Re: N2H6

Postby Isaiah Little 1A 14B » Mon Nov 27, 2017 10:27 pm

That structure with a double bond would work IF nitrogen broke the octet rule, but it cannot since its principle quantum number is 2 and there is no 2d orbital.

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