Textbook Question
For the molecules shown, indicate the direction of the dipole moment.
(b)
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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 35d
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 35dChapter 1, Problem 35d
You drew the Lewis structures of the following compounds and ion in Assessment 2.32. Predict their shapes around the central atom based on the Lewis structure.
(d) CO32-
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Draw the Lewis structure for the carbonate ion (CO₂⁻/₃). Start by determining the total number of valence electrons. Carbon has 4 valence electrons, each oxygen has 6 valence electrons, and the ion has a -2 charge, adding 2 more electrons. This gives a total of 24 valence electrons.
Distribute the electrons around the central carbon atom and the three oxygen atoms. Place carbon in the center and connect it to each oxygen atom with a single bond. Then, distribute the remaining electrons to satisfy the octet rule for each oxygen atom.
Check the formal charges on each atom. Adjust the structure by forming double bonds between carbon and one or more oxygen atoms to minimize formal charges, ensuring the most stable resonance structures. The carbonate ion has three resonance structures where the double bond is delocalized among the three oxygen atoms.
Determine the electron geometry using the VSEPR (Valence Shell Electron Pair Repulsion) theory. The central carbon atom is surrounded by three regions of electron density (three oxygen atoms), which corresponds to a trigonal planar electron geometry.
Predict the molecular shape. Since there are no lone pairs on the central carbon atom, the molecular shape of the carbonate ion is also trigonal planar, with bond angles of approximately 120°.
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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 help visualize the arrangement of electrons and the connectivity of atoms, which is crucial for predicting molecular geometry. In the case of CO₂⁻/₃, understanding its Lewis structure will provide insight into the distribution of electrons and the overall shape of the molecule.
VSEPR Theory
Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell of the central atom. According to VSEPR, electron pairs will arrange themselves to minimize repulsion, leading to specific molecular shapes. This theory is essential for determining the three-dimensional arrangement of atoms in CO₂⁻/₃.
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, as predicted by Lewis structures and VSEPR theory. Understanding the molecular geometry of CO₂⁻/₃ is vital for predicting its physical and chemical properties, as well as its reactivity.
Related Practice
Textbook Question
Hydrogen forms bonds without hybridizing. Why?
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Textbook Question
Calculate the formal charge on the non-hydrogen atoms in the molecules shown. Use the arrow-pushing formalism to 'move' an electron pair such that it is shared between two (formerly) charged atoms. Your arrow should account for the formation of the molecule on the right from the molecule on the left.
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Textbook Question
Calculate the formal charge of the indicated atoms in the ions shown.
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Textbook Question
For the molecules shown, indicate the direction of the dipole moment.
(a)
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Textbook Question
You drew the Lewis structures of the following compounds and ion in Assessment 2.32. Predict their shapes around the central atom based on the Lewis structure.
(c) HCO2H
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