Question

draw the lewis structure for the nitronium (no₂⁺) ion.

Explanation:

Step1: Calculate valence electrons

N has 5 valence electrons, each O has 6 valence electrons, and the +1 charge means one less electron. So, \(5 + 2\times6- 1=16\) valence electrons.

Step2: Place the central atom

N is the central atom as it is less electronegative than O.

Step3: Connect atoms with single bonds

Connect N to each O with a single bond, using 4 electrons. 12 electrons remain.

Step4: Distribute remaining electrons

Distribute the remaining 12 electrons as lone - pairs on the O atoms first to satisfy the octet rule. But this gives an incomplete octet on N.

Step5: Form double - bonds

Change one lone - pair on each O into a bonding pair to form double - bonds between N and O, giving each atom an octet.

Answer:

O=N=O
The nitrogen atom is in the center, with double - bonds to each of the oxygen atoms. Each oxygen has two lone - pairs of electrons.