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Chapter 9: Problem 57

Write three resonance structures for hydrazoic acid, \(\mathrm{HN}_{3}\). The atomic arrangement is HNNN. Show formal charges.

Short Answer

Expert verified
The three resonance structures for Hydrazoic acid (\( \mathrm{HN}_{3} \)) consist of different bonding arrangements between the three nitrogen atoms, with formal charges of the nitrogen atoms varying between +1, 0, and -1. The hydrogen atom maintains a formal charge of 0 in all structures.

Step by step solution

01

Draw the initial structure

Start by drawing the basic structure of the molecule. You have a hydrogen atom (H) connected to a nitrogen atom (N). The nitrogen atom is then connected to two other nitrogen atoms (N). Each nitrogen atom has 5 valence electrons, and hydrogen has 1 valence electron.
02

Draw the first resonance structure

The first resonance structure could assume that the middle nitrogen atom forms a single bond with the right nitrogen atom, and a double bond with the left nitrogen atom (connected to Hydrogen). This would imply a formal charge of +1 on the middle nitrogen atom, a formal charge of -1 on the hydroxyl nitrogen atom, and a formal charge of 0 on the last adjacent nitrogen atom.
03

Draw the second resonance structure

For the second resonance structure, we can envision a scenario where the middle nitrogen is forming a double bond with the right nitrogen, and a single bond with the nitrogen atom on its left. As a result, the nitrogen atom on the extreme right gets a formal charge of -1, while the two other nitrogen atoms receive a formal charge of 0. The hydrogen atom always has a formal charge of 0.
04

Draw the third resonance structure

In the third resonance structure, the nitrogen atom (to which Hydrogen is attached) forms a double bond with the adjacent nitrogen and the last nitrogen forms a single bond with that in the middle. This arrangement gives a formal charge of -1 to the middle nitrogen, while the rest of the atoms get a formal charge of 0.

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Most popular questions from this chapter

Explain why the bond enthalpy of a molecule is usually defined in terms of a gas-phase reaction. Why are bond-breaking processes always endothermic and bond-forming processes always exothermic?

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