The structure of borazine, B₃N₃H₆, is a six-membered ring of alternating B and N atoms. There is one H atom bonded to each B and to each N atom. The molecule is planar. (e) What are the hybridizations at the B and N atoms in the Lewis structures from parts (a) and (b)? Would you expect the molecule to be planar for both Lewis structures? Would you expect the molecule to be planar for both Lewis structures?

Key Concepts

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of a molecule. In borazine, the boron (B) and nitrogen (N) atoms undergo hybridization to form sp2 hybrid orbitals, which allows for the formation of sigma bonds and the necessary geometry for the planar structure of the molecule.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They help visualize the arrangement of electrons and the connectivity of atoms, which is crucial for predicting molecular geometry and hybridization. In borazine, the Lewis structure illustrates the alternating B and N atoms and their respective hydrogen attachments.

Planarity in Molecules

Planarity refers to the arrangement of atoms in a molecule such that they lie in a single plane. This is often a result of hybridization and the presence of double bonds or lone pairs that can influence molecular geometry. In borazine, the sp2 hybridization of B and N leads to a trigonal planar arrangement around each atom, contributing to the overall planar structure of the six-membered ring.