Textbook Question
(c) Is the p bond in NO2- localized or delocalized?
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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 Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 9, Problem 61c
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?
Verified step by step guidance1
Identify the atoms present in glycine: Glycine has the chemical formula NH2CH2COOH, which includes nitrogen (N), carbon (C), oxygen (O), and hydrogen (H) atoms.
Draw the Lewis structure for glycine: Arrange the atoms to reflect the typical bonding patterns, with carbon as the central atom, and connect the atoms with single bonds initially.
Count the sigma (σ) bonds: Sigma bonds are single covalent bonds. In the Lewis structure, count each single bond between atoms. Remember that each single bond represents one sigma bond.
Count the pi (π) bonds: Pi bonds are found in double or triple bonds. In the Lewis structure, identify any double bonds and count the pi bonds. Each double bond consists of one sigma bond and one pi bond.
Sum the total number of sigma and pi bonds: Add up all the sigma bonds and all the pi bonds separately to find the total number of each type of bond in the glycine molecule.
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 electrons and lines to represent bonds, allowing chemists to visualize the arrangement of atoms and the types of bonds present. Understanding how to draw and interpret Lewis structures is essential for analyzing molecular geometry and bonding characteristics.
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04:28
Lewis Dot Structures: Ions
Types of Chemical Bonds
Chemical bonds can be classified into two main types: sigma (σ) bonds and pi (π) bonds. Sigma bonds are formed by the head-on overlap of atomic orbitals and are the first bonds formed between two atoms, while pi bonds result from the side-to-side overlap of p orbitals and are typically found in double and triple bonds. Recognizing the difference between these bonds is crucial for determining the total number of each type in a molecule.
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Counting Bonds in Molecules
To determine the total number of sigma and pi bonds in a molecule, one must analyze the Lewis structure and count the bonds accordingly. Each single bond is a sigma bond, while double bonds consist of one sigma and one pi bond, and triple bonds contain one sigma and two pi bonds. This counting process is vital for answering questions about molecular structure and reactivity.
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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?
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Textbook Question
Consider the Lewis structure for glycine, the simplest amino acid:
(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?
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Textbook Question
(c) Would you expect N2O to exhibit delocalized p bonding?
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Textbook Question
Consider the Lewis structure for acetic acid, which is known as vinegar:
(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?
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Textbook Question
(a) Write a single Lewis structure for N2O, and determine the hybridization of the central N atom.