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?
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 68
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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Identify the central atom in the species, which is iodine (I) in IO_2^-.
Determine the number of valence electrons for iodine. Iodine has 7 valence electrons.
Consider the charge of the ion. The negative charge (1-) indicates an additional electron, making it 8 valence electrons to distribute.
Count the number of atoms bonded to iodine. There are two oxygen atoms bonded to iodine.
Use the formula for hybridization: Hybridization = (Number of sigma bonds + Number of lone pairs). Calculate the hybridization based on the number of sigma bonds and lone pairs around iodine.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals are used to explain the geometry of molecular bonding. The type of hybridization depends on the number of electron pairs around the central atom, which can include both bonding pairs and lone pairs.
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Hybridization
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 can be used to determine the hybridization of atoms. By drawing the Lewis structure for IO2-, one can identify the number of electron domains around the iodine atom, which is crucial for determining its hybridization.
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VSEPR Theory
Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs. According to VSEPR, electron pairs will arrange themselves to minimize repulsion, which directly influences the hybridization of the central atom. Understanding VSEPR helps in predicting the shape of the IO2- ion and thus its hybridization.
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Related Practice
Textbook Question
(a) If you combine two atomic orbitals on two different atomsto make a new orbital, is this a hybrid orbital or a molecularorbital?
Textbook Question
(b) If you combine two atomic orbitals on one atom to make a new orbital, is this a hybrid orbital or a molecular orbital?
Textbook Question
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
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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