Sodium azide is a shock-sensitive compound that releases N2 upon physical impact. The compound is used in automobile airbags. The azide ion is N3-. (b) State the hybridization of the central N atom in the azide ion.

Verified step by step guidance

1. insert step 1> Identify the central atom in the azide ion (N3-).
2. insert step 2> Recognize that the azide ion is a linear molecule with the structure N-N-N.
3. insert step 3> Determine the number of regions of electron density around the central nitrogen atom.
4. insert step 4> Use the VSEPR theory to predict the hybridization based on the number of electron density regions.
5. insert step 5> Conclude the hybridization of the central nitrogen atom based on the linear geometry.

Key Concepts

Hybridization

Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals can then be used to form covalent bonds in molecules. The type of hybridization depends on the number of electron pairs around the central atom, influencing the geometry and bonding properties of the molecule.

Azide Ion Structure

The azide ion (N3-) consists of three nitrogen atoms connected in a linear arrangement. The central nitrogen atom is bonded to two terminal nitrogen atoms, which can be represented as N=N^+=N^-. Understanding the structure of the azide ion is crucial for determining the hybridization of the central nitrogen atom, as it influences the distribution of electron density and bond angles.

Valence Bond Theory

Valence Bond Theory explains how atomic orbitals combine to form bonds in molecules. It emphasizes the role of electron pairs and the spatial orientation of orbitals. In the case of the azide ion, this theory helps in determining the hybridization state of the central nitrogen atom, which is essential for predicting the molecule's reactivity and stability.