Textbook Question
Rank the following compounds from highest dipole moment to lowest dipole moment:
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Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)
Bruice8th EditionOrganic ChemistryISBN: 9780135213711
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Table of contents
- Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 1)31
- Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)65
- Ch. 2 - Acids and Bases: Central to Understanding Organic Chemistry84
- Ch. 3 - An Introduction to Organic Compounds:Nomenclature, Physical Properties, and Structure183
- Ch. 4 - Isomers: The Arrangement of Atoms in Space121
- Ch. 5 - Alkenes: Structure, Nomenclature, and an Introduction to Reactivity • Thermodynamics and Kinetics83
- Ch. 6 - The Reactions of Alkenes • The Stereochemistry of Addition Reactions175
- Ch. 7 - The Reactions of Alkynes • An Introduction to Multistep Synthesis119
- Ch. 8 - Delocalized Electrons: Their Effect on Stability, pKa, and the Products of a Reaction • Aromaticity and Electronic Effects: An Introduction to the Reactions of Benzene148
- Ch. 9 - Substitution and Elimination Reactions of Alkyl Halides212
- Ch. 10 - Reactions of Alcohols, Ethers, Epoxides, Amines, and Sulfur-Containing Compounds131
- Ch. 11 - Organometallic Compounds60
- Ch. 12 - Radicals90
- Ch. 13 - Mass Spectrometry; Infrared Spectroscopy; UV/Vis Spectroscopy62
- Ch. 14 - NMR Spectroscopy95
- Ch. 15 - Reactions of Carboxylic Acids and Carboxylic Acid Derivatives123
- Ch. 16 - Reactions of Aldehydes and Ketones • More Reactions of Carboxylic Acid Derivatives141
- Ch. 17 - Reactions at the Alpha-Carbon101
- Ch. 18 - Reactions of Benzene and Substituted Benzenes144
- Ch. 19 - More About Amines • Reactions of Heterocyclic Compounds49
- Ch. 20 - The Organic Chemistry of Carbohydrates80
- Ch. 21 - Amino Acids, Peptides, and Proteins57
- Ch. 22 - Catalysis in Organic Reactions and in Enzymatic Reactions35
- Ch. 23 - The Organic Chemistry of the Coenzymes—Compounds Derived from Vitamins1
- Ch. 28 - Pericyclic Reactions58
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Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)Problem 72a
Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)Problem 72aChapter 2, Problem 72a
a. Which of the species have bond angles of 109.5°?
b. Which of the species have bond angles of 120°?
H2O H3O+ +CH3 BF3
Verified step by step guidance1
Step 1: Understand the bond angles associated with different molecular geometries. Bond angles of 109.5° are characteristic of tetrahedral geometry, while bond angles of 120° are characteristic of trigonal planar geometry.
Step 2: Analyze the molecular geometry of H2O. H2O has two bonding pairs and two lone pairs of electrons around the central oxygen atom. This results in a bent geometry with bond angles slightly less than 109.5° due to lone pair repulsion.
Step 3: Analyze the molecular geometry of H3O+. H3O+ has three bonding pairs and one lone pair of electrons around the central oxygen atom. This results in a trigonal pyramidal geometry with bond angles close to 109.5°.
Step 4: Analyze the molecular geometry of +CH3. The methyl cation (+CH3) has three bonding pairs and no lone pairs around the central carbon atom. This results in a trigonal planar geometry with bond angles of 120°.
Step 5: Analyze the molecular geometry of BF3. BF3 has three bonding pairs and no lone pairs around the central boron atom. This results in a trigonal planar geometry with bond angles of 120°.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Tetrahedral Geometry
Tetrahedral geometry occurs when a central atom is bonded to four other atoms, resulting in bond angles of approximately 109.5°. This arrangement minimizes electron pair repulsion according to VSEPR (Valence Shell Electron Pair Repulsion) theory, which predicts the spatial arrangement of atoms in a molecule.
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Trigonal Planar Geometry
Trigonal planar geometry is characterized by a central atom bonded to three other atoms, forming bond angles of 120°. This geometry arises from the arrangement of electron pairs around the central atom, which also follows VSEPR theory, allowing for optimal spacing between the electron pairs.
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VSEPR Theory
VSEPR (Valence Shell Electron Pair Repulsion) theory is a model used to predict the shape of molecules based on the repulsion between electron pairs surrounding a central atom. By considering both bonding and lone pairs, VSEPR helps determine the molecular geometry and associated bond angles, which are crucial for understanding molecular behavior and reactivity.
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Related Practice
Textbook Question
In which orbitals are the lone pairs in nicotine?
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Textbook Question
Do the sp2 carbons and the indicated sp3 carbons lie in the same plane?
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Textbook Question
Explain why CH3Cl has a greater dipole moment than CH3F even though F is more electronegative than Cl.
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Textbook Question
a. Which of the species have bond angles of 109.5°?
b. Which of the species have bond angles of 120°?
NH3 +NH4 -CH3
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Textbook Question
a. Draw a Lewis structure for each of the following:
b. Draw a structure for each of the species that shows approximate bond angles.
c. Which species have no dipole moment?
2. HNO3
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