Textbook Question
For each of the given species:
a. Draw its Lewis structure.
b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.
2. HCN
2
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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 33
Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)Problem 33Chapter 2, Problem 33
Predict the approximate bond angles in
a. the methyl cation.
b. the methyl radical.
c. the methyl anion.
Verified step by step guidance1
Step 1: Understand the hybridization of the central carbon atom in each species. The methyl cation (CH₃⁺) has a positively charged carbon atom with only three bonding pairs and no lone pairs, indicating sp² hybridization. The methyl radical (CH₃•) has three bonding pairs and one unpaired electron, also suggesting sp² hybridization. The methyl anion (CH₃⁻) has three bonding pairs and one lone pair, indicating sp³ hybridization.
Step 2: Recall the bond angles associated with each hybridization. For sp² hybridization, the bond angles are approximately 120°, as the electron pairs are arranged in a trigonal planar geometry. For sp³ hybridization, the bond angles are approximately 109.5°, as the electron pairs are arranged in a tetrahedral geometry.
Step 3: Apply the bond angle predictions to each species. For the methyl cation (CH₃⁺), the sp² hybridization leads to bond angles of approximately 120°. For the methyl radical (CH₃•), the sp² hybridization also leads to bond angles of approximately 120°. For the methyl anion (CH₃⁻), the sp³ hybridization leads to bond angles of approximately 109.5°.
Step 4: Consider any deviations from ideal bond angles due to electronic effects. In the methyl anion (CH₃⁻), the lone pair on the carbon atom may slightly compress the bond angles below the ideal tetrahedral angle of 109.5°.
Step 5: Summarize the bond angle predictions: The methyl cation and methyl radical both have bond angles of approximately 120° due to sp² hybridization, while the methyl anion has bond angles close to 109.5° due to sp³ hybridization, with potential slight compression due to the lone pair.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In organic chemistry, it helps predict the geometry and bond angles of molecules. For example, sp3 hybridization leads to tetrahedral geometry with bond angles of approximately 109.5°, while sp2 and sp hybridizations correspond to trigonal planar (120°) and linear (180°) geometries, respectively.
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Using bond sites to predict hybridization
Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonding pairs and lone pairs of electrons around the central atom. Understanding molecular geometry is crucial for predicting bond angles, as different geometries (like tetrahedral, trigonal planar, and linear) dictate specific angles between bonds.
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Charge Effects on Geometry
The presence of a charge on a molecule can significantly alter its geometry and bond angles. Cations (positively charged) tend to have smaller bond angles due to increased electron density around the central atom, while anions (negatively charged) can lead to larger bond angles due to repulsion from additional electron pairs. This concept is essential for predicting the bond angles in species like the methyl cation, radical, and anion.
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Related Practice
Textbook Question
According to the potential map for the ammonium ion <IMAGE>, which atom has the greatest electron density?
1
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Textbook Question
For each of the given species:
a. Draw its Lewis structure.
b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.
4. H2CO3
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Textbook Question
Describe the orbitals used in bonding and the bond angles in the following compounds:
a. CH3O-
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Textbook Question
For each of the given species:
a. Draw its Lewis structure.
b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.
1. H2CO2
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Textbook Question
Describe the orbitals used in bonding and the bond angles in the following compounds:
c. H2CO
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