Textbook Question
Describe the orbitals used in bonding and the bond angles in the following compounds:
d. N2
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 39a
Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)Problem 39aChapter 2, Problem 39a
Describe the orbitals used in bonding and the bond angles in the following compounds:
a. CH3O-
Verified step by step guidance1
Step 1: Identify the central atom in the compound CH3O-. The central atom is oxygen (O) in this case.
Step 2: Determine the hybridization of the central atom. Oxygen in CH3O- is sp3 hybridized because it forms three sigma bonds (one with carbon and two with hydrogen) and has one lone pair.
Step 3: Describe the orbitals involved in bonding. The oxygen atom uses its sp3 hybrid orbitals to form sigma bonds with the carbon atom and the hydrogen atoms. The carbon atom in CH3 is also sp3 hybridized, using its sp3 orbitals to form sigma bonds with the oxygen and hydrogen atoms.
Step 4: Determine the bond angles. In an sp3 hybridized atom, the ideal bond angle is approximately 109.5°. However, due to the presence of a lone pair on oxygen, the bond angle may be slightly less than 109.5°.
Step 5: Consider the effect of the negative charge. The negative charge on the oxygen atom indicates an extra electron, which is accommodated in one of the sp3 hybrid orbitals, contributing to the overall geometry and bond angles.
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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 process by which atomic orbitals mix to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of CH3O-, the central atom (carbon) undergoes sp3 hybridization, resulting in four equivalent hybrid orbitals that can form sigma bonds with hydrogen and oxygen.
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Using bond sites to predict hybridization
Bond Angles
Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the hybridization of the central atom and the repulsion between electron pairs. In CH3O-, the bond angles around the carbon atom are approximately 109.5 degrees, characteristic of sp3 hybridization, while the bond angle between the carbon and oxygen may be slightly less due to lone pair repulsion.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule, which is determined by the number of bonding pairs and lone pairs of electrons around the central atom. For CH3O-, the geometry is tetrahedral around the carbon atom, with the presence of a lone pair on the oxygen affecting the overall shape and bond angles.
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Related Practice
Textbook Question
Predict the approximate bond angles in
a. the methyl cation.
b. the methyl radical.
c. the methyl anion.
2
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Textbook Question
Describe the orbitals used in bonding and the bond angles in the following compounds:
e. BF3
1
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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:
c. H2CO
2
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