Textbook Question
(c) Is the p bond in NO2- localized or delocalized?
Ch.9 - Molecular Geometry and Bonding Theories
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 9, Problem 64a
(a) Write a single Lewis structure for N2O, and determine the hybridization of the central N atom.
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Identify the total number of valence electrons in N2O. Nitrogen (N) has 5 valence electrons and Oxygen (O) has 6 valence electrons. Since there are two nitrogen atoms and one oxygen atom, calculate the total valence electrons: 2(5) + 6 = 16 valence electrons.
Determine the skeletal structure of N2O. Typically, the least electronegative atom is central, so arrange the atoms as N-N-O.
Distribute the valence electrons to satisfy the octet rule. Start by forming a single bond between the central nitrogen and each of the terminal atoms. Then, distribute the remaining electrons to complete the octets, starting with the outer atoms.
Consider multiple bonds if necessary to satisfy the octet rule for each atom. Adjust the structure by forming double or triple bonds between the nitrogen atoms or between nitrogen and oxygen, ensuring that the total number of electrons remains 16.
Determine the hybridization of the central nitrogen atom. Count the number of regions of electron density (bonds and lone pairs) around the central nitrogen atom. The hybridization corresponds to the number of these regions: 2 regions = sp, 3 regions = sp², 4 regions = sp³, etc.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules.
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Lewis Dot Structures: Ions
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding and lone pairs of electrons in a molecule. The type of hybridization (e.g., sp, sp2, sp3) is determined by the number of electron domains around a central atom, influencing the molecule's geometry and bond angles.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced 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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Related Practice
Textbook Question
Consider the Lewis structure for acetic acid, which is known as vinegar: (b) What are the hybridizations of the orbitals on the two oxygen atoms, and what are the approximate bond angles at the oxygen that is connected to carbon and hydrogen? What are the hybridizations of the orbitals on the two oxygen atoms?
Textbook Question
(c) Would you expect N2O to exhibit delocalized p bonding?
Textbook Question
In the formate ion, HCO2-, the carbon atom is the central atom with the other three atoms attached to it. (c) Are there multiple equivalent resonance structures for the ion?
Textbook Question
Consider the Lewis structure for glycine, the simplest amino acid:
(c) What is the total number of s bonds in the entire molecule, and what is the total number of p bonds?
Textbook Question
In the sulphate ion, SO42-, the sulphur atom is the central atom with the other 4 oxygen atoms attached to it. (b) What hybridization is exhibited by the S atom?