2E13 part d

(Polar molecules, Non-polar molecules, etc.)

Moderators: Chem_Mod, Chem_Admin

Brynne Burrows 3K
Posts: 52
Joined: Thu Jul 25, 2019 12:16 am

2E13 part d

Postby Brynne Burrows 3K » Mon Nov 18, 2019 8:55 pm

What is the correct way to draw the Lewis structure for N2O? There can either be a triple bond between the Nitrogen molecules and a single bond between Nitrogen and Oxygen, or a double bond between both N-N and N-O. Should the -1 formal charge be assigned to the Nitrogen atom or Oxygen?

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

Re: 2E13 part d

Postby Justin Vayakone 1C » Mon Nov 18, 2019 9:23 pm


Out of these three structures, the top right one is the best structure. Negative formal charge should be placed on the most electronegative atom if possible. In this case, O is more electronegative than N, so O should get the negative formal charge over N.

Edit: Is the image showing? If not, it's the structure with the N-N triple bond and N-O single bond.

Return to “Determining Molecular Shape (VSEPR)”

Who is online

Users browsing this forum: No registered users and 2 guests