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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblem 52d
Chapter 9, Problem 52d

What is the hybridization of the central atom in (d) NO2?

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1
Identify the central atom in the molecule NO2. In this case, nitrogen (N) is the central atom.
Count the number of atoms directly bonded to the central nitrogen atom. In NO2, there are two oxygen atoms bonded to nitrogen.
Determine the number of lone pairs on the central atom. In NO2, nitrogen has one lone pair.
Add the number of sigma bonds and lone pairs to find the steric number. For NO2, this is 2 sigma bonds + 1 lone pair = 3.
Use the steric number to determine the hybridization: A steric number of 3 corresponds to sp2 hybridization.

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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 are used to explain the geometry and bonding properties of molecules. The type of hybridization depends on the number of electron pairs around the central atom, which influences the molecular shape.
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Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which can be predicted using the VSEPR (Valence Shell Electron Pair Repulsion) theory. Understanding molecular geometry is crucial for predicting the physical and chemical properties of substances.
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Nitrogen Dioxide (NO2)

Nitrogen dioxide (NO2) is a chemical compound consisting of one nitrogen atom and two oxygen atoms. It is a bent molecule due to the presence of a lone pair of electrons on the nitrogen atom, which affects its hybridization. The hybridization of the nitrogen atom in NO2 can be determined by analyzing its bonding and lone pairs, leading to a specific hybridization state.
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Related Practice
Textbook Question
(c) Write the formulas for the analogousspecies of the elements of period 3;
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Textbook Question

What is the hybridization of the central atom in (c) O3?

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Textbook Question

(b) What would you expect for the magnitude and direction of the bond dipoles in this series?

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Textbook Question

Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle. (a)


(b)


(c)

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Textbook Question

Indicate the hybridization of the central atom in (c) P1OH23 (d) AlI3.

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Textbook Question

What is the hybridization of the central atom in (a) PBr5? (b) CH2O?

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