Borazine, \(\mathrm{B}_{3} \mathrm{~N}_{3} \mathrm{H}_{6}\), has the skeleton Draw the resonance forms of the molecule.

To draw resonance forms, first, draw the basic structure of Borazine with alternating single and double bonds between the B and N atoms. Also, each B and N atom is bonded to a hydrogen atom.

In the structure, there are pi-bonds formed with double bonds between the B and N atoms that can be delocalized, leading to resonance structures.

Move the pi-bonds to create a new structure with the alternating single and double bonds. Make sure to keep proper electron counts and create no new atoms or charges. The change in the pi-bonds will create a new resonance form.

Now that you have drawn two resonance forms, observe how these forms contribute to the overall electron delocalization and stability of the molecule. The two resonance forms of Borazine are as follows: 1. Resonance form 1 (Initial structure): H-B=N-H | | H-N-B-H | | H-B=N-H 2. Resonance form 2 (Alternate double & single bonds): H-N=B-H | | H-B=N-H | | H-N=B-H Both resonance forms have alternating single and double bonds and play a significant role in the overall stability of the Borazine molecule. Keep in mind that these resonance forms are not distinct entities but representations of the electron delocalization of the molecule. The real structure of Borazine is an average of these resonance forms.