Textbook Question
Show how the Lewis dot structure for each of the following atoms would overlap to form a single bond.
(b) C and O
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 59d
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 59dChapter 1, Problem 59d
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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Identify the general rule for selecting a central atom in a Lewis structure: The central atom is typically the least electronegative atom, as it is more likely to share electrons with surrounding atoms.
Compare the electronegativities of carbon (C) and nitrogen (N). Carbon has an electronegativity of approximately 2.55, while nitrogen has a higher electronegativity of approximately 3.04.
Since carbon is less electronegative than nitrogen, it is more likely to serve as the central atom in a Lewis structure.
Consider the valency of each atom. Carbon has four valence electrons and can form up to four bonds, making it versatile as a central atom. Nitrogen, with five valence electrons, typically forms three bonds and is less commonly the central atom unless the molecule's structure requires it.
Conclude that carbon (C) is the preferred central atom in this pair for most Lewis structures, based on its lower electronegativity and bonding versatility.
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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 and reactivity.
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Drawing the Lewis Structure for N2H4.
Central Atom
The central atom in a Lewis structure is typically the atom that can form the most bonds or has the highest valence. It is usually the least electronegative atom in a molecule, as it can effectively bond with surrounding atoms to achieve a stable electron configuration.
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01:44The difference between atomic numbers and atomic mass.
Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. In determining the central atom, the atom with lower electronegativity is often preferred, as it is more likely to share its electrons and form bonds with other atoms.
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Related Practice
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
Which atom in each pair would you expect to be the central atom in a Lewis structure?
(b) C vs. O
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Textbook Question
How many valence electrons does each of the following contribute to a Lewis structure?
(l) ―1 charge
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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)