Asked by Vic
How to get the hybridization of N IN NO2- ?
Answers
Answered by
DrBob222
I do it as an after the fact method.
Draw the Lewis dot structure.
1 N = 1 x 5 electrons = 5 e
2 O = 2 x 6 e = 12 e
1 e for charge = 1 e
total electrons = 18.
<b>
 O
  |
:N=O
</b>
Now place 3 pairs e (6 electrons total) around top O and 2 pairs around side O. That should use up the 18.
Count the regions of high electron density. There are 3 (1 for double bond, 1 for single bond, and 1 for unpaired set electrons on N. Three regions of high electron density = trigonal planar arangement and sp2 hybridization.
Draw the Lewis dot structure.
1 N = 1 x 5 electrons = 5 e
2 O = 2 x 6 e = 12 e
1 e for charge = 1 e
total electrons = 18.
<b>
 O
  |
:N=O
</b>
Now place 3 pairs e (6 electrons total) around top O and 2 pairs around side O. That should use up the 18.
Count the regions of high electron density. There are 3 (1 for double bond, 1 for single bond, and 1 for unpaired set electrons on N. Three regions of high electron density = trigonal planar arangement and sp2 hybridization.