Textbook Question
Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.
(d) AlCl4-
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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 35c
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 35cChapter 1, Problem 35c
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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Draw the Lewis structure of HCO₂H (formic acid). Identify the central atom, which is the carbon atom, and ensure all valence electrons are accounted for. Carbon will form a double bond with one oxygen atom, a single bond with the other oxygen atom (which is also bonded to a hydrogen atom), and a single bond with the hydrogen atom.
Determine the regions of electron density around the central carbon atom. In this case, there are three regions of electron density: one double bond to oxygen, one single bond to oxygen, and one single bond to hydrogen.
Apply the VSEPR (Valence Shell Electron Pair Repulsion) theory. According to VSEPR, the regions of electron density will arrange themselves as far apart as possible to minimize repulsion. For three regions of electron density, the geometry is trigonal planar.
Predict the molecular shape around the central carbon atom. Since there are no lone pairs on the central carbon atom, the molecular shape will also be trigonal planar.
Verify the bond angles. In a trigonal planar geometry, the bond angles are approximately 120°. Confirm that this matches the expected geometry for HCO₂H.
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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 HCO₂H (formic acid), drawing the Lewis structure allows us to identify the central atom and its bonding partners.
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. For HCO₂H, understanding VSEPR helps determine the shape around the central carbon atom.
Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. It is influenced by the number of bonding pairs and lone pairs of electrons around the central atom. In HCO₂H, the molecular geometry can be predicted by analyzing the Lewis structure and applying VSEPR theory, which indicates that the shape will be influenced by the presence of both single and double bonds.
Related Practice
Textbook Question
For the molecules shown, indicate the direction of the dipole moment.
(b)
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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
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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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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