Question

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

Short answer

Answer: Borazine has two resonance forms, each with alternating single and double bonds between the boron (B) and nitrogen (N) atoms. 1. Resonance form 1: H-B=N-H | | H-N-B-H | | H-B=N-H 2. Resonance form 2: H-N=B-H | | H-B=N-H | | H-N=B-H These resonance forms contribute to the overall stability of the Borazine molecule by allowing electron delocalization through the pi-bonds. The real structure of Borazine is an average of these resonance forms, providing greater stability to the molecule.

Step-by-step solution

Draw the initial structure of Borazine

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.

Identify the electron delocalization

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 resonance forms

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.

Analyze the resonance forms

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.

Key concepts

Borazine Structure

Borazine is an intriguing compound often referred to as "inorganic benzene." Its chemical formula is \(\mathrm{B}_{3} \mathrm{N}_{3} \mathrm{H}_{6}\), and it consists of a ring structure similar to benzene. In Borazine, three boron (B) atoms and three nitrogen (N) atoms form a hexagonal ring by alternating positions with each other.

• This forms a pattern of B-N-B-N-B-N.
• Each B atom connects to a hydrogen (H) atom, and so does each N atom.

The key to understanding Borazine lies in its bonding. Boron prefers three bonds in order to fill its valence shell, while nitrogen typically makes three bonds as well to satisfy its five valence electrons. This characteristic setup establishes alternating single and double bonds between boron and nitrogen in the ring.The resonant characteristics of this structure contribute to its distinctive stability, mimicking that found in the all-carbon benzene molecule.

Electron Delocalization

Electron delocalization is a concept crucial to the understanding of resonance in chemical structures like Borazine. When electrons are delocalized, they are not localized to a specific bond or atom, but rather spread across several atoms.In Borazine, this delocalization occurs because of the alternating double bonds between boron and nitrogen. While one pair of electrons may form a \( \pi \) bond between B and N in one position, shifting electron pairs can relocate the double bonds through all B-N pairs around the ring.

• This gives rise to multiple resonance forms, as electrons are flexible in occupancy.
• Each form is valid because of the delocalization of the \( \pi \) electrons.

Electron delocalization in Borazine leads to a structure that is not rigid but highly dynamic, permitting constructive superimposition of resonance forms. This acts to stabilize the entire molecule by blending the energy configurations into one lower-energy average.

Pi-Bonds in Resonance

Pi-bonds play a vital role in the resonance of compounds such as Borazine. These \( \pi \) bonds allow for increased stability through resonance.In Borazine’s structure, \( \pi \) bonds are formed by lateral overlap of \( p \) orbitals on adjacent B and N atoms. These alternating single and double bonds permit continuous electron flow and shifting, a process known as resonance.

• Resonance showcases the delocalized nature of the \( \pi \) bonds.
• The shifting of these bonds from one atom pair to another leads to an energetic state lower than any of the individual resonance structures.

When identifying resonance in Borazine, it is essential to understand that these \( \pi \) bonds keep alternating. This minimizes energy levels and contributes to a stable, hybrid structure. The result is a form that balances between the resonance forms, effectively spreading out the \( \pi \) electrons to enhance stability across the ring.