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
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not 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
Consider the Lewis structure for glycine, the simplest amino acid:
(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?
Textbook Question
Consider the Lewis structure for acetic acid, which is known as vinegar:
(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
Benzaldehyde, C7H6O, is a fragrant substance responsible for the aroma of almonds. Its Lewis structure is
(a) What is the hybridization at each of the carbon atoms of the molecule?