>
> I have another question, or possibly an answer, to problem 1.22d.
> Instead of just one of the oxygens on the end having a double bond, would
> it not be possible to have both oxygens double bonded to the nitrogen?
> This then would take the positive charge away from the nitrogen and the
> negative charge away from the oxygen by using up two of the oxygen's free
> electrons.
>
> ie. :O:
> : "
> H-O-N (Middle O= technical difficulties; no sideways colons)
> : "
> :O:
>
> {Lori Grimberg | In the space age the most important }
> {Grimbele@pepper.plu.edu | space is between your ears. }
> { | -THOMAS J BARLOW }
>
>
In the above structure there is a total of 10 electrons
surrounding the nitrogen atom. Although the formal charge works out
beautifully, (everything being zero), nitrogen won't form expanded
octets. It is shown on page 12 and it is a resonance hybrid because the
double bond can be on either oxygen, but not both.
I hope this is helpful,
Andy Glandon