Textbook Question
d. Would you expect SO3 to exhibit delocalized π bonding?
Ch.9 - Molecular Geometry and Bonding Theories
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 9, Problem 61b
Glycine, the simplest amino acid, has the following Lewis structure:
b. What are the hybridizations of the orbitals on the two oxygens and the nitrogen atom, and what are the approximate bond angles at the nitrogen?
Verified step by step guidance1
Determine the hybridization of the orbitals on the oxygen atoms. Oxygen typically forms two bonds and has two lone pairs, which suggests sp^3 hybridization.
Consider the hybridization of the nitrogen atom. Nitrogen in amino acids like glycine typically forms three sigma bonds and has one lone pair, indicating sp^3 hybridization.
Identify the geometry associated with sp^3 hybridization. For both oxygen and nitrogen, sp^3 hybridization corresponds to a tetrahedral geometry.
Estimate the bond angles around the nitrogen atom. In a perfect tetrahedral geometry, the bond angles are approximately 109.5 degrees.
Note any deviations in bond angles due to lone pairs. Lone pairs can slightly reduce bond angles from the ideal tetrahedral angle due to increased electron repulsion.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of atoms in a molecule. In the case of glycine, the nitrogen atom typically undergoes sp3 hybridization due to its four substituents, while the oxygen atoms may exhibit sp2 hybridization if they are involved in double bonds or resonance structures.
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Hybridization
Bond Angles
Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the hybridization of the central atom. For sp3 hybridized atoms, the ideal bond angle is approximately 109.5 degrees, while sp2 hybridized atoms have bond angles around 120 degrees. Understanding these angles helps predict the molecular geometry and spatial arrangement of atoms.
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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 provide a visual representation of the arrangement of electrons and help in determining the hybridization and bond angles by illustrating how atoms are connected and the distribution of electron density.
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Related Practice
Textbook Question
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
(e) How many valence electrons remain in nonbonding pairs in the molecule?
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
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
(c) How many of the valence electrons are used to make s bonds in the molecule?
Textbook Question
Glycine, the simplest amino acid, has the following Lewis structure:
a. What are the approximate bond angles about each of the two carbon atoms, and what are the hybridizations of the orbitals on each of them?
Textbook Question
Glycine, the simplest amino acid, has the following Lewis structure:
c. What is the total number of π bonds in the entire molecule, and what is the total number of π bonds?