Textbook Question
By moving an electron pair, draw a better Lewis structure that minimizes formal charges.
(a)
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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 61b
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 61bChapter 1, Problem 61b
By moving an electron pair, draw a better Lewis structure that minimizes formal charges.
(b) 
Verified step by step guidance1
Analyze the given Lewis structure: The nitrogen atom has a lone pair and a negative formal charge, while the central carbon atom has a positive formal charge. This suggests that the electron distribution can be adjusted to minimize formal charges.
Recall the rules for formal charge calculation: Formal charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons/2). Use this formula to evaluate the charges on each atom in the structure.
Identify the possibility of moving the lone pair from nitrogen to form a double bond with the central carbon atom. This would redistribute the electrons and potentially neutralize the charges on both nitrogen and carbon.
Redraw the structure with the lone pair on nitrogen converted into a double bond between nitrogen and carbon. This adjustment should result in nitrogen having a formal charge of 0 and carbon also having a formal charge of 0.
Verify the new structure by recalculating the formal charges for all atoms. Ensure that the charges are minimized and the octet rule is satisfied for each atom where applicable.
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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 understanding molecular geometry and reactivity. In this context, drawing a better Lewis structure involves rearranging electron pairs to achieve a more stable configuration.
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Drawing the Lewis Structure for N2H4.
Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and half the number of bonding electrons. It helps assess the stability of a Lewis structure; structures with lower formal charges are generally more stable. Minimizing formal charges is essential for drawing accurate and stable Lewis structures.
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01:34Calculating formal and net charge.
Electron Pair Movement
Electron pair movement refers to the process of shifting lone pairs or bonding pairs of electrons to form new bonds or to create more favorable electron distributions in a molecule. This concept is vital when optimizing Lewis structures, as moving electron pairs can help minimize formal charges and achieve a more stable arrangement of atoms. Understanding how to manipulate electron pairs is key to drawing accurate representations of molecular structures.
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Related Practice
Textbook Question
Draw the Lewis structure for the following molecular formulas.
(j) H2SO4
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Textbook Question
Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet.
(e)
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Textbook Question
Draw the Lewis structure for the following molecular formulas.
(l) SO42-
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Textbook Question
Draw the Lewis structure for the following molecular formulas.
(u) NH4+
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Textbook Question
Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet.
(d)
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