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?
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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 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 66a
Consider the Lewis structure shown below.
(a) Does the Lewis structure depict a neutral molecule or an ion? If it is an ion, what is the charge on the ion? What is the charge on the ion
Verified step by step guidance1
Identify the total number of valence electrons for the molecule or ion.
Count the number of electrons depicted in the Lewis structure.
Compare the total number of valence electrons with the number of electrons in the Lewis structure.
If the number of electrons in the Lewis structure is greater than the total number of valence electrons, the structure represents an anion. If fewer, it represents a cation.
Calculate the charge by subtracting the total number of valence electrons from the number of electrons in the Lewis structure.
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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 and interpret Lewis structures is essential for determining the molecular geometry and reactivity of compounds.
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04:28
Lewis Dot Structures: Ions
Molecular Charge
The molecular charge refers to the overall charge of a molecule or ion, which can be neutral, positive, or negative. It is determined by the difference between the number of protons (positively charged) and electrons (negatively charged) in the structure. Identifying whether a Lewis structure represents a neutral molecule or an ion involves counting the total valence electrons and comparing it to the expected number based on the constituent atoms.
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01:53Formal Charge
Ionic vs. Neutral Species
Ionic species are charged entities that result from the loss or gain of electrons, while neutral species have an equal number of protons and electrons. In the context of Lewis structures, recognizing whether a structure depicts an ion or a neutral molecule is crucial for understanding its chemical behavior and properties. The charge of an ion can often be inferred from the number of electrons depicted in the Lewis structure compared to the number of valence electrons expected for the atoms involved.
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03:03Amphoteric Species
Related Practice
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?
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Textbook Question
Predict the molecular geometry of each of the following molecules: (b) H O C O C O O H
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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?
Textbook Question
What hybridization do you expect for the atom that is underlined in each of the following species? (a) IO2- (b) NH4+ (c) SCN- (d) BrCl3
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