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 60e
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 60eChapter 1, Problem 60e
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) 
Verified step by step guidance1
Step 1: Identify the central atom in the molecule. Typically, the least electronegative atom (excluding hydrogen) is chosen as the central atom. Arrange the other atoms around it.
Step 2: Determine the total number of valence electrons available for the molecule. Add up the valence electrons of all atoms involved. For this problem, you are given 6 electrons.
Step 3: Place single bonds between the central atom and surrounding atoms. Each bond uses 2 electrons. Subtract the electrons used for bonding from the total valence electrons.
Step 4: Distribute the remaining electrons as lone pairs around the surrounding atoms to complete their octets. If there are still electrons left, place them on the central atom as lone pairs.
Step 5: Check the structure to ensure all atoms (except hydrogen) have a full octet and that the total number of electrons used matches the given number of valence electrons (6 electrons). Adjust bonds if necessary, such as forming double or triple bonds to satisfy the octet rule.
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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 use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the reactivity of compounds.
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Drawing the Lewis Structure for N2H4.
Octet Rule
The octet rule is a chemical rule of thumb that states that atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule is particularly applicable to main group elements and is crucial for determining how atoms will bond in a molecule.
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Valence Electrons
Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds with other atoms. The number of valence electrons determines how an atom can bond and interact with others, making it a key factor in constructing Lewis structures and understanding molecular stability.
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Related Practice
Textbook Question
Draw the Lewis structure for the following molecular formulas.
(j) H2SO4
1
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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.
(a)
Textbook Question
Which atom in each pair would you expect to be the central atom in a Lewis structure?
(f) C vs. F
Textbook Question
By moving an electron pair, draw a better Lewis structure that minimizes formal charges.
(b)
2
views
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)