Textbook Question
Each compound contains both ionic and covalent bonds. Write ionic Lewis structures for each, including the covalent structure for the ion in brackets. Write resonance structures if necessary. b. Ca(OH)2 c. KNO3 d. LiIO
Ch.10 - Chemical Bonding I: The Lewis Model
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Chapter 10, Problem 86b
Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds. b. ClF5
Verified step by step guidance1
Identify the type of compound: ClF5 is a molecular compound because it consists of nonmetals.
Determine the total number of valence electrons: Chlorine (Cl) has 7 valence electrons, and each fluorine (F) also has 7 valence electrons. Therefore, the total is 7 + 5(7) = 42 valence electrons.
Place the least electronegative atom in the center: Chlorine is less electronegative than fluorine, so Cl will be the central atom.
Distribute the electrons: Place a single bond between the central Cl atom and each of the five F atoms. This uses up 10 electrons (5 bonds x 2 electrons per bond).
Distribute the remaining electrons to satisfy the octet rule: Place the remaining 32 electrons as lone pairs on the F atoms (6 electrons per F atom) to complete their octets. The central Cl atom will have 10 electrons, which is acceptable for elements in period 3 or higher.
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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 indicate bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of compounds.
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04:28
Lewis Dot Structures: Ions
Ionic vs. Molecular Compounds
Ionic compounds are formed through the transfer of electrons from one atom to another, resulting in the formation of charged ions that attract each other. In contrast, molecular compounds consist of atoms that share electrons through covalent bonds. Distinguishing between these types of compounds is crucial for accurately representing their structures and understanding their properties.
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02:11Ionic Compounds Naming
Valence Electrons
Valence electrons are the outermost electrons of an atom and are involved in forming bonds with other atoms. The number of valence electrons determines how an atom can bond and interact with others. For example, in the case of ClF5, understanding the valence electrons of chlorine and fluorine is key to constructing its Lewis structure and determining its molecular geometry.
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02:12Transition Metals Valence Electrons
Related Practice
Textbook Question
In the Chemistry and the Environment box on free radicals in this chapter, we discussed the importance of the hydroxyl radical in reacting with and eliminating many atmospheric pollutants. However, the hydroxyl radical does not clean up everything. For example, chlorofluorocarbons—which destroy stratospheric ozone—are not attacked by the hydroxyl radical. Consider the hypothetical reaction by which the hydroxyl radical might react with a chlorofluorocarbon: OH(g) + CF2Cl2(g) → HOF(g) + CFCl2(g) Use bond energies to explain why this reaction is improbable. (The C–F bond energy is 552 kJ/mol.)
Textbook Question
Ethane burns in air to form carbon dixode and water vapor.
2 H3C¬CH3( g) + 7 O2( g)¡4 CO2( g) + 6 H2O( g)
Use average bond energies to calculate ΔHrxn for the reaction.
Textbook Question
Each compound contains both ionic and covalent bonds. Write ionic Lewis structures for each, including the covalent structure for the ion in brackets. Write resonance structures if necessary. a. BaCO3