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.

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insert step 1> Identify the central atom in the azide ion (N3-).

insert step 2> Recognize that the azide ion is a linear molecule with the structure N-N-N.

insert step 3> Determine the number of regions of electron density around the central nitrogen atom.

insert step 4> Use the VSEPR theory to predict the hybridization based on the number of electron density regions.

insert step 5> Conclude the hybridization of the central nitrogen atom based on the linear geometry.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

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Textbook Question

Which of the following statements about hybrid orbitals is or are true? a. After an atom undergoes sp hybridization, there is one unhybridized p orbital on the atom, b. Under 𝑠𝑝2 hybridization, the large lobes point to the vertices of an equilateral triangle, and c. The angle between the large lobes of 𝑠𝑝3 hybrids is 109.5°.

Textbook Question

The molecule C4H5N has the connectivity shown here. a. After the Lewis structure for the molecule is completed, how many 𝜎 and how many 𝜋 bonds are there in this molecule?

Textbook Question

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-. (a) Draw the Lewis structure of the azide ion that minimizes formal charge (it does not form a triangle). Is it linear or bent?

Textbook Question

In ozone, O3, the two oxygen atoms on the ends of the molecule are equivalent to one another. (d) How many electrons are delocalized in the p system of ozone?

Textbook Question

Butadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths:

(a) Predict the bond angles around each of the carbon atoms and sketch the molecule.

Textbook Question

Butadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths:

(b) From left to right, what is the hybridization of each carbon atom in butadiene?