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The nitrogen oxide $\ce{NO}$ exists and has an uneven number of valence electrons. This is "impossible". Why does it exist? Why is it not dimerized?

Nitrogen has 5 valence electrons and oxygen 6. Whatever your skill, you cannot get a noble gas configuration for both atoms in a molecule like $\ce{NO}$ .

Of course, $\ce{NO}$ dimerizes at very low temperatures. But why only at low temperatures? $\ce{H}$ atoms and alkyl radicals dimerize easily at room temperatures, and even above. Why is it so hard to dimerize $\ce{NO}$? Why is the bond $\ce{N-N}$ in $\ce{N2O2}$ so weak?

Edit : The following assumption has been published : "This question already has answers here: Why doesn't nitrogen monoxide dimerize? (3 answers)"

I regret to say that none of the three proposed references do answer the question : Why is the bond $\ce{N-N}$ so weak in $\ce{N2O2}$

Maurice
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    https://chemistry.stackexchange.com/questions/32265/which-relatively-simple-molecules-violate-the-octet-rule https://chemistry.stackexchange.com/questions/116841/what-is-dot-sign-in-no – Mithoron Oct 24 '19 at 20:34
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    Oxygen basically has 2 unpaired electrons. Why doesn't it polymerize? – Zhe Oct 24 '19 at 23:32
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    I changed the duplicate target to one that was more appropriate. – orthocresol Jun 24 '22 at 09:22

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