MonkeyXu
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For the structure of NO2, Nitrogen does not fulfill a stable electron configuration. In my drawing, Nitrogen has double bond on both oxygen atoms which makes the two oxygen atoms having stable electron but Nitrogen have nine valence electron. What is the right way to draw the structure of NO2?
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charco
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(Original post by MonkeyXu)
For the structure of NO2, Nitrogen does not fulfill a stable electron configuration. In my drawing, Nitrogen has double bond on both oxygen atoms which makes the two oxygen atoms having stable electron but Nitrogen have nine valence electron. What is the right way to draw the structure of NO2?
You cannot expand the octet around the nitrogen - it must be left electron deficient with one single electron (free radical)

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MonkeyXu
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(Original post by charco)
You cannot expand the octet around the nitrogen - it must be left electron deficient with one single electron (free radical)

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So, the Nitrogen atom doesn't share electron with oxygen?
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charco
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(Original post by MonkeyXu)
So, the Nitrogen atom doesn't share electron with oxygen?
No, the pi orbital actually spreads out over both of the oxygens and the nitrogen to create a delocalised molecular orbital in which each of the N-O bonds has an order of 1.5.

However, you asked for the Lewis structure.
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