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Which is the correct structure of $\ce{NO2}$ ? While searching the internet I found out that -

  1. $\ce{NO2}$ have a coordinate and 2 covalent bonds. $\ce{N}$ will +ve charge. $\ce{O}$ (coordinate bond )will have a negative charge (this is the part which i don't understand As $\ce{O}$'s octet is complete why will it have a -ve charge )

    1. $\ce{NO2}$ came from $\ce{HNO2}$ that's from $\ce{O}$ have a -ve charge . but in this molecule there is no $\ce{O}$ with coordinate bond.

    2. in one molecule $\ce{N}$ have one electron and +ve charge and in other 2 electrons and no charge ?

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closed as unclear what you're asking by Mithoron, Todd Minehardt, MaxW, Karsten Theis, A.K. May 12 at 21:28

Please clarify your specific problem or add additional details to highlight exactly what you need. As it's currently written, it’s hard to tell exactly what you're asking. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.

  • $\begingroup$ Are you asking about the Lewis structure together with the formal charges? You can have a non-zero formal charge for atoms that have an octet - the way the electrons are counted is different for those two concepts. It would help if you edited your answer to show the Lewis structures you are talking about. As written, I'm not even sure if you mean $\ce{NO2}$ or $\ce{NO2-}$. $\endgroup$ – Karsten Theis May 10 at 19:28
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$\ce{NO2}$ is a free radical. Its resonance structures are as follows:

resonance

Unsurprisingly, $\ce{NO2}$ reacts readily with a variety of substances, including itself at low temperatures to form $\ce{N2O4}$.

enter image description here

From Wikipedia:

enter image description here

Nitrogen dioxide at −196°C, 0°C, 23°C, 35°C, and 50°C. ($\ce{NO2}$) converts to the colorless dinitrogen tetroxide ($\ce{N2O4}$) at low temperatures, and reverts to $\ce{NO2}$ at higher temperatures.

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  • $\begingroup$ where did this minus sign came from? $\endgroup$ – Bhavay May 9 at 23:27
  • $\begingroup$ @Bhavay are you referring to the oxygen? It is just the formal charge on it for that resonance structure. There is no true negative charge on the oxygens. It is a neutral molecule. This may help. $\endgroup$ – ringo May 9 at 23:29
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    $\begingroup$ The molecule is neutral, it can't have an unbalanced negative formal charge. As is the nitrogen should have a positive formal charge (seven valence electrons). $\endgroup$ – orthocresol May 9 at 23:31
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    $\begingroup$ @Bhavay No, $\ce{NO_2^-}$ has one additional electron compared to $\ce{^\cdot NO_2}$. They're not the same. $\endgroup$ – hBy2Py May 9 at 23:37
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    $\begingroup$ Yes, nitrogen has five Valence electrons (@orthocresol seven total). Please count again, because I only see four electrons around nitrogen in either resonance structure you have drawn. A (neutral) molecule can never have an unbalanced formal charge. $\endgroup$ – Martin - マーチン May 9 at 23:42

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