Structure of no2 molecule [closed]








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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 two covalent bonds. $\ce{N}$ will have a positive 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 negative charge?)
2. $\ce{NO2}$ came from $\ce{HNO2}$ that's from $\ce{O}$ have a negative charge. but in this molecule, there is no $\ce{O}$ with coordinate bond.
3. In one molecule $\ce{N}$ have one electron and positive charge and in other two electrons and no charge?




$\ce{NO2}$ is a free radical. Its resonance structures are as follows:


[![resonance](https://i.stack.imgur.com/5VxJE.png)](https://i.stack.imgur.com/5VxJE.png)


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


[![enter image description here](https://i.stack.imgur.com/eNGRj.png)](https://i.stack.imgur.com/eNGRj.png)


From [Wikipedia](https://en.wikipedia.org/wiki/Nitrogen_dioxide):



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> [![enter image description here](https://i.stack.imgur.com/UFfrF.jpg)](https://i.stack.imgur.com/UFfrF.jpg)
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> 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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