[g13]

I have a molecule I'm working N2O2, and am wondering if it is polar or not. I haven't found anything on google and have not gotten a solid answer from anyone, but here are my thoughts...

I said it is polar because there are lone pairs on the Nitrogen, meaning that there are unattached electrons, so this is where I get my answer from. If this is wrong, please feel free to correct me.

[imanooblar]

Where are you getting the lone pairs on the nitrogen from?

From what it seems like, the structure is O-N-N-O with a triple bond between the nitrogen. Because oxygen is more electronegative than nitrogen, the oxygen atoms will have a slight negative charge and the nitrogens will have a slight positive charge.

However, because they are opposite of each other, they should cancel each other out leading to a non-polar molecule. I may be wrong but that's my best bet.

If you calculate the formal charge, both of the oxygens will have a formal charge of -1, while the nitrogens will have a formal charge of +1, which makes sense due to electronegativity. Also, the overall charge is 0.

Hope that helps.

[g13]

That seems to workout just fine. I originally tried double bonding oxygen and I realize that was the mistake I made. Thanks a lot man.

[imanooblar]

no problem