Textbook Question
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
(e) How many valence electrons remain in nonbonding pairs in the molecule?
Ch.9 - Molecular Geometry and Bonding Theories
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- 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: 9780137542970Not the one you use?Change textbook
Chapter 9, Problem 60c
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
(c) How many of the valence electrons are used to make s bonds in the molecule?
Verified step by step guidance1
Identify the total number of valence electrons in ethyl acetate (C_4H_8O_2). Carbon has 4 valence electrons, hydrogen has 1, and oxygen has 6. Calculate the total by multiplying the number of each type of atom by its valence electrons and summing them up.
Draw the Lewis structure of ethyl acetate. Start by arranging the carbon atoms in a chain, then add the oxygen atoms and finally the hydrogen atoms. Ensure that each atom satisfies the octet rule (or duet for hydrogen).
Identify the sigma (σ) bonds in the molecule. Sigma bonds are single covalent bonds formed by the direct overlap of atomic orbitals. In the Lewis structure, these are represented by single lines connecting atoms.
Count the number of sigma bonds in the Lewis structure. Each single line between two atoms represents one sigma bond.
Determine how many valence electrons are used in these sigma bonds. Each sigma bond consists of two electrons, so multiply the number of sigma bonds by two to find the total number of valence electrons used in sigma bonds.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Valence Electrons
Valence electrons are the outermost electrons of an atom and are crucial for chemical bonding. In the context of ethyl acetate, understanding how many valence electrons are available helps determine how they are shared or transferred during bond formation. Each atom's valence electrons contribute to the overall structure and reactivity of the molecule.
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Transition Metals Valence Electrons
Covalent Bonds
Covalent bonds are formed when two atoms share pairs of valence electrons. In ethyl acetate, these bonds are primarily between carbon and hydrogen, as well as carbon and oxygen. Identifying the number of covalent bonds in the molecule is essential for calculating how many valence electrons are involved in these bonds.
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Lewis Structure
A Lewis structure is a diagram that represents the bonding between atoms in a molecule and the lone pairs of electrons. It provides a visual representation of how valence electrons are arranged and helps in identifying the number of bonds formed. Analyzing the Lewis structure of ethyl acetate allows for a clear understanding of how many valence electrons are used in sigma bonds.
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Related Practice
Textbook Question
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
a. What is the hybridization at each of the carbon atoms of the molecule?
Textbook Question
Glycine, the simplest amino acid, has the following Lewis structure:
a. What are the approximate bond angles about each of the two carbon atoms, and what are the hybridizations of the orbitals on each of them?
Textbook Question
Propylene, C3H6, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is (a) What is the total number of valence electrons in the propylene molecule?
Textbook Question
Glycine, the simplest amino acid, has the following Lewis structure:
b. What are the hybridizations of the orbitals on the two oxygens and the nitrogen atom, and what are the approximate bond angles at the nitrogen?