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
Not the one you use?Change textbookSelect a different textbook
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 61c
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?
Verified step by step guidance1
Identify the types of bonds present in the glycine molecule. Glycine typically contains carbon (C), hydrogen (H), nitrogen (N), and oxygen (O) atoms.
Recall that a \(\sigma\) bond (sigma bond) is a single covalent bond formed by the direct overlap of atomic orbitals, while a \(\pi\) bond (pi bond) is formed by the side-to-side overlap of p orbitals.
Count the \(\sigma\) bonds: Each single bond in the molecule is a \(\sigma\) bond. Double bonds consist of one \(\sigma\) bond and one \(\pi\) bond.
Count the \(\pi\) bonds: Look for any double bonds in the molecule, as each double bond contains one \(\pi\) bond.
Sum up the total number of \(\sigma\) bonds and \(\pi\) bonds separately to find the answer.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
2mWas this helpful?
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 help visualize the arrangement of electrons and the types of bonds (single, double, or triple) present in the molecule. Understanding how to draw and interpret Lewis structures is essential for identifying the number of sigma (π) and pi (π) bonds.
Recommended video:
Guided course
04:28
Lewis Dot Structures: Ions
Sigma (π) and Pi (π) Bonds
Sigma (π) bonds are the first bonds formed between two atoms, created by the head-on overlap of atomic orbitals. Pi (π) bonds, on the other hand, are formed by the side-to-side overlap of p orbitals and are present in double and triple bonds. Recognizing the difference between these bond types is crucial for determining the total number of each in a molecule.
Recommended video:
Guided course
03:26Lewis Dot Structures: Sigma & Pi Bonds
Counting Bonds in Molecules
To answer questions about the number of sigma and pi bonds in a molecule, one must systematically analyze the Lewis structure. Each single bond corresponds to one sigma bond, while double bonds consist of one sigma and one pi bond, and triple bonds contain one sigma and two pi bonds. This systematic counting allows for accurate determination of the total bond types present in the molecule.
Recommended video:
Guided course
03:10Homonuclear Diatomic Molecules
Related Practice
Textbook Question
In the formate ion, HCO2-, the carbon atom is the central atom with the other three atoms attached to it. (d) How many electrons are in the p system of 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
(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
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:
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?