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Chapter 10: Problem 122

Hydrogen azide, \(\mathrm{HN}_{3}\), can exist in two forms. One form has the three nitrogen atoms connected in a line; and the nitrogen atoms form a triangle in the other. Construct Lewis structures for these isomers and describe their shapes. Other interesting derivatives are nitrosyl azide ( \(\mathrm{N}_{4} \mathrm{O}\) ) and trifluoromethyl azide \(\left(\mathrm{CF}_{3} \mathrm{N}_{3}\right) .\) Describe the shapes of these molecules based on a line of nitrogen atoms.

Short Answer

Expert verified
The different arrangements of Nitrogen atoms in HN3 create two main shapes; linear and bent for the linear and triangular isomer respectively. Additional molecules N4O and CF3N3 have molecule shapes described as linear along the Nitrogen atoms and bent where other atoms are connected to Nitrogen. This bending is due to the lone pairs on the Nitrogen atom.

Step by step solution

01

- Lewis structure and shape of linear HN3 isomer

Write the Lewis structure for each of the atoms in the isomer (H and N). The linear structure implies that the Hydrogen (H) atom is bonded to one of the Nitrogen (N) atoms, and the three Nitrogen atoms are bonded linearly. This results in two lone pairs of electrons on the two Nitrogen atoms at the ends of the line, and one lone pair on the Nitrogen in the middle. The shape of the molecule can be described as linear for the three Nitrogen atoms and bent (close to 105 degrees) at the Hydrogen-Nitrogen bond due to the lone pairs on the Nitrogen atom connected to Hydrogen.
02

- Lewis structure and shape of triangular HN3 isomer

Write the Lewis structure for the triangular HN3. This involves three Nitrogen atoms forming a triangle and the Hydrogen atom bonded to one of the Nitrogen atoms. Each Nitrogen atom has one lone pair of electrons. The shape of the molecule can be described as trigonal planar for the three Nitrogen atoms and again bent at the Hydrogen-Nitrogen bond due to the lone pair on the Nitrogen atom connected to Hydrogen.
03

- Lewis structure and shape of N4O

Write the Lewis structure for N4O. Given that Nitrogen atoms form a linear structure, this can be represented with the Nitrogen atoms forming a line. Oxygen is singly bonded to one of the end Nitrogens. This results in each Nitrogen atom carrying a lone pair of electrons where the Oxygen atom carries two lone pairs. The molecule shape can be described as linear for the Nitrogen atoms and bent at the Nitrogen-Oxygen bond due to the lone pairs on the Oxygen atom.
04

- Lewis structure and shape of CF3N3

Write the Lewis structure for CF3N3, with the Nitrogen atoms forming a linear structure. Fluorine atoms are bonded to the Carbon atom which is singly bonded to one of the Nitrogen atoms. Each Nitrogen atom carries a lone pair of electrons. Each Fluorine carries three lone pairs and Carbon atom carries no lone pairs. The molecule shape can be described as linear for the Nitrogen atoms and bent at the Carbon-Nitrogen and Carbon-Fluorine bonds due to the lone pairs on the Nitrogen and Fluorine atoms respectively.

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Most popular questions from this chapter

Write a plausible Lewis structure for crotonaldehyde, $\mathrm{CH}_{3} \mathrm{CHCHCHO},$ a substance used in tear gas and insecticides.

Use the VSEPR theory to predict a probable shape of the molecule \(\mathrm{F}_{4} \mathrm{SCH}_{2}\), and explain the source of any ambiguities in your prediction.

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