Textbook Question
Write the Lewis structure for each molecule or ion. c. BrO-
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 61d
Write the Lewis structure for each molecule or ion. d. C2H4
Verified step by step guidance1
Identify the total number of valence electrons in the molecule. Carbon (C) has 4 valence electrons and hydrogen (H) has 1 valence electron. Calculate the total for C2H4.
Determine the central atoms. In C2H4, both carbon atoms are central and will be bonded to each other.
Arrange the hydrogen atoms around the carbon atoms. Each carbon will be bonded to two hydrogen atoms.
Use single bonds to connect the hydrogen atoms to the carbon atoms and a double bond to connect the two carbon atoms, ensuring each carbon atom follows the octet rule.
Verify that all valence electrons are used and that each atom has a complete valence shell, with carbon having 8 electrons and hydrogen having 2 electrons.
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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 the behavior of molecules.
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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 molecule's reactivity and stability. For carbon, which has four valence electrons, and hydrogen, which has one, knowing their counts is vital for constructing accurate Lewis structures.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonds and lone pairs around the central atom, which can affect the molecule's physical and chemical properties. Understanding molecular geometry helps in predicting the shape of the molecule, which is important for its reactivity and interactions.
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Related Practice
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Write the Lewis structure for each molecule or ion. a. H3COCH3