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Double bond to one oxygen, single bond to the other. This means one electron left over on nitrogen atom. The result is that the N atom does not have a full octet. This is why nitrogen dioxide tends to dimerise into N2O4, in which the nitrogens can share electrons and achieve full octets.

In nitrogen dioxide, the bond order is actually 1.5, an "average" of the double and single bonds, which are delocalised to form the 1.5 bond order.

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