A couple years ago, my student was just about the only one in
her cohort who could correctly draw the structure of NO2 in a major exam. My point is (not about boasting, but
about) most JC teachers don’t focus (not blaming them though, they
have it tough enough) on teaching the relevant, fundamental and
crucial aspects of Chemistry that empower students to understand,
appreciate and enjoy the Science as an Art. JC students most often
fail to allow themselves to do the above (not blaming them though,
they have it tough enough), and instead blindly memorize their way
through JC.
Specifically (for this question), I refer to the concept of
formal charges and resonance (that is ill-taught in JCs), without
an understand of these, drawing structures become senseless and
hopeless.
To answer your question :
Central atom is N (with a +ve charge), single (and dative)
bonded to an O atom (with a -ve charge), and double bonded to a
(neutral) O atom. The N atom thus has 3 bond pairs and an unpaired
electron, the (-ve charged) O atom has 3 lone pairs and 1 bond
pair, the (neutral) O atom has 2 lone pairs and 2 bond pairs.
The electron geometry is trigonal planar, the molecular geometry
is v-shape or bent or non-linear.
The resonance hybrid sees each of both N to O bonds as having
bond lengths & bond strengths equivalent to 1.5 bonds. The
charge on each O atom is an averaged -1/2 charge.
For ‘A’ levels exams, it will suffice to draw a single resonance
contributor.