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d. Would you expect SO3 to exhibit delocalized 𝜋 bonding?
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Ch.9 - Molecular Geometry and Bonding Theories
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- 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: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 66a
Consider the following Lewis structure:
a. Does the Lewis structure depict a neutral molecule or an ion? If it is an ion, what is the charge on the ion?
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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 it is less, it represents a cation.
Determine the charge by finding the difference between the number of electrons in the Lewis structure and the total number of valence electrons.
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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 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. This distinction affects how the molecule interacts with other substances and its stability.
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03:03Amphoteric Species
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Which of the following statements about molecular orbitals and hybrid orbitals are true?
a. Molecular orbitals and hybrid orbitals are both created by mathematically mixing the wave functions of atomic orbitals.
b. Molecular orbitals are made by combining atomic orbitals from different atoms.
c. Hybrid orbitals and molecular orbitals are different names for the same things.
d. A hybrid orbital can hold more electrons than can a molecular orbital.
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