Question

How do you draw the lewis structure for NO2?

Answer 1

Refer to the video in the explanation.

Explanation:

Answer 2

So how many valence electrons we got...?

Explanation:

Five from nitrogen, and 12 from the oxygen atoms...and so we got 8 and a HALF electron pairs to distribute...17 electrons in total

As is typical, the least electronegative atom is placed in the middle to give...

`O=stackrel(dot)N^(+)-O^(-)`

From left to right as we face the page, each atom is associated with SIX, FOUR, and SEVEN valence electrons, giving rise to formal charges of `0`, `+1`, and `-1`. Of course, we could write the other resonance structure...

`""^(-)O-stackrel(dot)N^(+)=O`

And so `NO_2` is a NEUTRAL, BENT molecule...whose geometry is based on a trigonal plane...`/_O-N-O=120^@` to a first approx., but `115^@` in actuality....

Why don't you try it for nitrite ion, `NO_2^(-)`...how does the Lewis structure evolve..?

And just to add, that the formal Lewis structure of `NO_2` is useful when we assess reactivity... `NO_2` can READILY dimerize (alternatively `N_2O_4` can readily undergo dissociation.

`(""^(-)O)O=stackrel(+dot)N + stackrel(+dot)N=O(O^(-)) rarr underbrace(""^(-)(O)O=stackrel(+dot)N-stackrel(+dot)N=O(O^(-)))`

`N_2O_4-="dinitrogen tetroxide"`

The nitrogen atom in `NO_2` or `N_2O_4` is said to be quaternized, i.e. it bears a formal POSITIVE charge....