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.
(c) BH4-
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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 33
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 33Chapter 1, Problem 33
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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Identify the formal charge formula: Formal charge = (Valence electrons of the atom) - (Non-bonding electrons) - (1/2 × Bonding electrons).
For each non-hydrogen atom in the molecule on the left, calculate its formal charge using the formula. Count the valence electrons, non-bonding electrons, and bonding electrons for each atom.
Examine the arrow-pushing formalism provided. Arrows indicate the movement of electron pairs. Follow the arrows to determine how electrons are redistributed between atoms.
Recalculate the formal charges for the non-hydrogen atoms in the molecule on the right after the electron redistribution. Use the same formal charge formula.
Compare the formal charges of the atoms in the molecule on the left and the molecule on the right. Verify that the electron movement accounts for the change in formal charges and ensures overall charge conservation.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated by considering the number of valence electrons, the number of bonds, and the number of non-bonding electrons. It helps in determining the most stable structure of a molecule by minimizing the charge separation. The formula is: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons).
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Calculating formal and net charge.
Arrow-Pushing Formalism
Arrow-pushing formalism is a method used in organic chemistry to illustrate the movement of electrons during chemical reactions. Arrows indicate the direction of electron flow, with a double-headed arrow showing the movement of a pair of electrons and a single-headed arrow indicating the movement of a single electron. This technique is essential for visualizing reaction mechanisms and understanding how reactants transform into products.
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Molecular Structure and Bonding
Molecular structure refers to the arrangement of atoms within a molecule and the types of bonds that hold them together. Understanding bonding, including covalent and ionic interactions, is crucial for predicting molecular behavior and reactivity. The formation of new bonds during a reaction often involves the sharing or transfer of electron pairs, which is central to the arrow-pushing formalism and the calculation of formal charges.
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Related Practice
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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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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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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