Textbook Question
Which atom in each pair would you expect to be the central atom in a Lewis structure?
(d) C vs. N
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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 60d
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 60dChapter 1, Problem 60d
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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Count the total number of valence electrons available for the molecule. In this case, you are given 12 valence electrons to work with.
Determine the central atom. Typically, the least electronegative atom (excluding hydrogen) is placed at the center of the structure.
Place single bonds (represented as lines) between the central atom and the surrounding atoms. Each single bond uses 2 electrons.
Distribute the remaining electrons as lone pairs around the outer atoms to satisfy their octet rule (8 electrons around each atom, except for hydrogen which only needs 2).
If there are still electrons left after satisfying the octet for the outer atoms, place the remaining electrons as lone pairs on the central atom. If the central atom does not have a full octet, consider forming double or triple bonds by sharing lone pairs from the outer atoms.
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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 behavior of molecules.
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Drawing the Lewis Structure for N2H4.
Octet Rule
The octet rule is a chemical rule of thumb that states 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 fundamental in determining how atoms will bond and interact in a molecule, particularly in covalent bonding.
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02:59The octet rule.
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, influencing the structure and stability of molecules. In the context of the question, knowing the total number of valence electrons available is crucial for completing the Lewis structure correctly.
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Related Practice
Textbook Question
By moving an electron pair, draw a better Lewis structure that minimizes formal charges.
(a)
1184
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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)
1344
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Textbook Question
Which atom in each pair would you expect to be the central atom in a Lewis structure?
(f) C vs. F
1087
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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)
1340
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Textbook Question
By moving an electron pair, draw a better Lewis structure that minimizes formal charges.
(b)
978
views