Textbook Question
Refer to the following Lewis structures.
(a)
(b)
If an atom is sp² hybridized, how many sp²-hybridized orbitals does it use for bonding? How many p orbitals?
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Ch. 2 - General Chemistry Translated: Finding the Electrons
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
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Table of contents
- Ch. 2 - General Chemistry Translated: Finding the Electrons114
- Ch. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis109
- Ch. 4 - Acids and Bases: Electron Flow144
- Ch. 5 - Chemical Reaction Analysis: Thermodynamics and Kinetics118
- Ch. 6 - Stereoisomerism: Arrangement of Atoms in Space112
- Ch. 7 - Principles of Green (Organic) Chemistry3
- Ch. 8 - Alkenes I: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes II: Oxidation and Reduction150
- Ch. 10 - Alkynes: Electrophilic Addition and Redox Reactions101
- Ch. 11 - Properties and Synthesis of Alkyl Halides: Radical Reactions108
- Ch. 12 - Substitution and Elimination: Reactions of Haloalkanes172
- Ch. 13 - Alcohols, Ethers and Related Compounds: Substitution and Elimination239
- Ch. 14 - Structural Identification I: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification II: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution I: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution II: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems I: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems II: Pericyclic Reactions54
- Ch. 23 - Benzene I: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene II: Reactions Influenced by the Aromatic Ring62
- Ch. 25 - Amines: Structure, Reactions, and Synthesis27
- Ch. 26 - Amino Acids, Proteins, and Peptide Synthesis9
- Ch. 27 - Carbohydrates, Nucleic Acids, and Lipids54
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471Not the one you use?Change textbook
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Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 74b
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 74bChapter 1, Problem 74b
Connect the atoms using the indicated hybrid orbitals.
(b) C (sp2) with C (sp2)
Verified step by step guidance1
Step 1: Understand the hybridization of the carbon atoms. Both carbon atoms are sp² hybridized, meaning they have one unhybridized p orbital and three sp² orbitals arranged in a trigonal planar geometry.
Step 2: Recognize the type of bond formed between two sp² hybridized carbons. The sp² orbitals will overlap to form a sigma (σ) bond, which is the primary bond connecting the two carbon atoms.
Step 3: Account for the unhybridized p orbitals. Each sp² hybridized carbon has one unhybridized p orbital perpendicular to the plane of the sp² orbitals. These p orbitals can overlap side-by-side to form a pi (π) bond.
Step 4: Combine the sigma and pi bonds to describe the overall bonding. The sigma bond forms the single framework connection, while the pi bond adds a second layer of bonding, resulting in a double bond between the two carbon atoms.
Step 5: Visualize the molecular geometry. The double bond (σ + π) between the two sp² hybridized carbons results in a planar structure with bond angles of approximately 120° around each carbon atom.
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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 of combining atomic orbitals to form new hybrid orbitals that can accommodate bonding. In the case of sp² hybridization, one s orbital and two p orbitals from a carbon atom mix to create three equivalent sp² hybrid orbitals, which are oriented 120 degrees apart in a trigonal planar arrangement.
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Using bond sites to predict hybridization
Bonding in Organic Molecules
In organic chemistry, carbon atoms often form covalent bonds with each other and other elements. The type of hybridization determines the geometry and bond angles of the molecule. For sp² hybridized carbons, the formation of sigma bonds occurs through the overlap of sp² orbitals, while pi bonds can form from the unhybridized p orbital.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. The geometry is influenced by the type of hybridization and the number of bonds. For sp² hybridized carbon atoms, the resulting geometry is trigonal planar, which is crucial for understanding the spatial orientation of the bonds and the overall shape of the molecule.
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Related Practice
Textbook Question
For the following partial structures, the σ bond is shown. Add the indicated number of π bonds, being sure to specify the orientation (that is, x, y, or z axis) of the p orbitals used.
(e)
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Textbook Question
Refer to the following Lewis structures.
(c)
(d)
If an atom is sp² hybridized, how many sp²-hybridized orbitals does it use for bonding? How many p orbitals?
2
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Textbook Question
Given the Lewis structures, indicate the direction of the dipole moment, if there is one.
(a)
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Textbook Question
For the following partial structures, the bond is shown. Add the indicated number of bonds, being sure to specify the orientation (that is, x, y, or z axis) of the p orbitals used.
(c)
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Textbook Question
Predict the hybridization of all non-hydrogen atoms.
(e)
(f)
(g)
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