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Chapter 10: Problem 38

What is the hybridization state of the central \(\mathrm{N}\) atom in the azide ion, \(\mathrm{N}_{3}^{-} ?\) (Arrangement of atoms: NNN.)

Short Answer

Expert verified
The hybridization state of the central Nitrogen (N) atom in the azide ion (\(\mathrm{N}_{3}^{-}\)) is 'sp'.

Step by step solution

01

Determine the central atom

Identify the central atom in the molecule. In this case, the central atom is the middle Nitrogen (N) atom in the azide ion (\(\mathrm{N}_{3}^{-}\)).
02

Determine the number of sigma bonds and lone pairs around the Nitrogen atom

The Nitrogen (N) atom in the center is bonded to the two other Nitrogen atoms. Each bond counts as 1 sigma bond, which gives us a total of 2 sigma bonds. Since there are no other atoms around the central N atom, there are no lone pairs.
03

Identify the Hybridization state

The Hybridization state is determined by the sum of sigma bonds and lone pairs. This gives 2 (from Step 2). So the hybridization state is 'sp', where 's' represents one of the electron orbitals and 'p' represents the other electron orbital linked by two sigma bonds.

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Most popular questions from this chapter

Predict the geometry of these molecules and ion using the VSEPR method: (a) \(\operatorname{HgBr}_{2}\), (b) \(\mathrm{N}_{2} \mathrm{O}\) (arrangement of atoms is NNO), (c) SCN \(^{-}\) (arrangement of atoms is SCN).

The molecule benzyne \(\left(\mathrm{C}_{6} \mathrm{H}_{4}\right)\) is a very reactive species. It resembles benzene in that it has a sixmembered ring of carbon atoms. Draw a Lewis structure of the molecule and account for the molecule's high reactivity.

The allene molecule \(\mathrm{H}_{2} \mathrm{C}=\mathrm{C}=\mathrm{CH}_{2}\) is linear (the three \(\mathrm{C}\) atoms lie on a straight line). What are the hybridization states of the carbon atoms? Draw diagrams to show the formation of sigma bonds and pi bonds in allene.

Aluminum trichloride \(\left(\mathrm{AlCl}_{3}\right)\) is an electron-deficient molecule. It has a tendency to form a dimer (a molecule made of two \(\mathrm{AlCl}_{3}\) units): $$ \mathrm{AlCl}_{3}+\mathrm{AlCl}_{3} \longrightarrow \mathrm{Al}_{2} \mathrm{Cl}_{6} $$ (a) Draw a Lewis structure for the dimer. (b) Describe the hybridization state of \(\mathrm{Al}\) in \(\mathrm{AlCl}_{3}\) and \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\). (c) Sketch the geometry of the dimer. (d) Do these molecules possess a dipole moment?

List these molecules in order of increasing dipole moment: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{CBr}_{4}, \mathrm{H}_{2} \mathrm{~S}, \mathrm{HF}, \mathrm{NH}_{3}, \mathrm{CO}_{2}\)
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