Draw the principal resonance forms of the nitronium ion.

First, we need to draw the Lewis Structure of the nitronium ion (NO₂⁺). To do that, we will count the valence electrons of each atom and connect them with single bonds. Nitrogen has 5 valence electrons, and each oxygen atom has 6 valence electrons. Since the molecule has a positive charge, we will remove one electron. In total, there will be (5 + 6 + 6 - 1) = 16 valence electrons in the molecule.

Now, we need to distribute the remaining valence electrons as lone pairs around each atom to satisfy the octet rule (except for the central nitrogen atom in this case). Each oxygen atom is connected to the nitrogen atom with a single bond, which accounts for 4 electrons. We have 12 remaining electrons to distribute as lone pairs. Each oxygen atom will receive 3 lone pairs (6 electrons in total). This accounts for all 16 valence electrons.

Next, we need to identify the π electrons that can be involved in resonance and the atoms they are shared between. The π electrons are the lone pair electrons on oxygen atoms that are not being used for the single bond to nitrogen. The π electrons can be shared between the two oxygen atoms and the central nitrogen atom.

To draw the resonance forms, we will show the alternate position of the π electrons being shared in the form of double bonds. The first resonance structure will have a double bond between nitrogen and one of the oxygen atoms, with the other oxygen atom having a single bond. The second resonance structure is formed by moving the double bond to the other oxygen atom, with the first oxygen atom now having a single bond. Make sure to include the positive charge on nitrogen atom. Here are the resonance structures for NO₂⁺ ion: ``` O O \\ // N⁺ N⁺ // \\ O O ``` The nitronium ion has two principal resonance forms, which represent the resonance-stabilized distribution of electrons between the nitrogen and oxygen atoms.