Textbook Question
Write the Lewis structure for each molecule or ion. c. BrO-
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Ch.10 - Chemical Bonding I: The Lewis Model
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 10, Problem 64b
Write the Lewis structure for each molecule or ion. b. OH-
Verified step by step guidance1
Identify the total number of valence electrons in the hydroxide ion (OH-). Oxygen has 6 valence electrons, hydrogen has 1, and the negative charge adds 1 more electron, totaling 8 valence electrons.
Place the oxygen atom in the center and the hydrogen atom bonded to it, as hydrogen can only form one bond.
Draw a single bond between the oxygen and hydrogen atoms. This bond uses 2 of the 8 available valence electrons.
Distribute the remaining 6 valence electrons around the oxygen atom to satisfy its octet, placing them as lone pairs.
Ensure the structure reflects the negative charge by enclosing the structure in brackets and placing a negative sign outside the brackets.
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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 Lewis structures is essential for visualizing molecular geometry and predicting reactivity.
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Lewis Dot Structures: Ions
Valence Electrons
Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the atom's ability to form bonds, either by sharing electrons (covalent bonds) or transferring them (ionic bonds). For the hydroxide ion (OH⁻), knowing the valence electrons helps in constructing its Lewis structure.
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Formal Charge
Formal charge is a concept used to determine the charge distribution within a molecule or ion, calculated based on the number of valence electrons, the number of non-bonding electrons, and half the number of bonding electrons. It helps in assessing the stability of a Lewis structure. For the hydroxide ion, calculating formal charges can confirm that the structure is correct and that the overall charge is -1.
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Related Practice
Textbook Question
Draw the Lewis structure for ClF with an arrow representing the dipole moment.
Textbook Question
Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. a. SeO2
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Textbook Question
Refer to Figure 10.10 to estimate the percent ionic character of the Hbr bond.
Textbook Question
Refer to Figure 10.10 to estimate the percent ionic character of the ClF bond.
Textbook Question
Use formal charges to identify the better Lewis structure.
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