Textbook Question
Ethyl propanoate, CH3CH2COOCH2CH3, gives a fruity pineapple-like smell. (e) What are the approximate bond angles around each carbon atom 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 92b
Ethyl propanoate, CH3CH2COOCH2CH3, gives a fruity pineapple-like smell. (a) Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds. (b) How many s and how many p bonds are in the molecule?
Verified step by step guidance1
To draw the Lewis structure of ethyl propanoate, start by identifying the number of valence electrons for each atom: Carbon (C) has 4, Hydrogen (H) has 1, and Oxygen (O) has 6. Calculate the total number of valence electrons in the molecule.
Arrange the atoms in the molecule. Ethyl propanoate has a backbone of carbon atoms with the ester functional group. The structure is CH3CH2COOCH2CH3, where the COO group is the ester linkage.
Connect the atoms with single bonds initially: Connect the carbon atoms in a chain, then attach the oxygen atoms to the appropriate carbon atoms. Ensure each carbon forms four bonds, and each oxygen forms two bonds.
Add lone pairs to the oxygen atoms to satisfy their octet. Adjust the structure to ensure all atoms have a complete octet, using double bonds if necessary, particularly in the COO group.
Count the sigma (σ) and pi (π) bonds: Sigma bonds are single bonds, and each double bond consists of one sigma and one pi bond. Identify the number of each type of bond in the molecule.
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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 are based on the octet rule, which states that atoms tend to form bonds until they are surrounded by eight valence electrons. In drawing Lewis structures, it is essential to account for the number of valence electrons and ensure that each atom achieves a stable electron configuration.
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Lewis Dot Structures: Ions
Types of Chemical Bonds
Chemical bonds can be classified into two main types: sigma (σ) and pi (π) bonds. Sigma bonds are formed by the head-on overlap of atomic orbitals and are the first bonds formed between two atoms. Pi bonds, on the other hand, result from the side-to-side overlap of p orbitals and are typically found in double and triple bonds. Understanding these bond types is crucial for analyzing molecular structure and reactivity.
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Hybridization
Hybridization is the concept that describes the mixing of atomic orbitals to form new hybrid orbitals, which can accommodate the bonding requirements of atoms in a molecule. For example, in ethyl propanoate, carbon atoms may undergo sp3 hybridization, resulting in four equivalent hybrid orbitals that can form single bonds with other atoms. This concept helps explain the geometry and bond angles in molecules.
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Related Practice
Textbook Question
Fill in the blank spaces in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. Molecule Electron-Domain Hybridization Dipole Geometry of Central Atom Moment? Yes or No CO2 sp3 Yes sp3 No Trigonal planar No SF4 Octahedral No sp2 Yes Trigonal bipyramidal No XeF2
Textbook Question
Although I3- is a known ion, F3- is not. (d) Yet another classmate says F3- does not exist because F is too small to make bonds to more than one atom. Is this classmate possibly correct?
Textbook Question
An AB5 molecule adopts the geometry shown here. (c) Suppose the B atoms are halogen atoms. Of which group in the periodic table is atom A a member: (i) Group 15, (ii) Group 16, (iii) Group 17, (iv) Group 18, or (v) More information is needed?
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Textbook Question
An AB5 molecule adopts the geometry shown here. (b) Do you think there are any nonbonding electron pairs on atom A?