Textbook Question
Which atom in each pair would you expect to be the central atom in a Lewis structure?
(d) C vs. N
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 59f
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 59fChapter 1, Problem 59f
Which atom in each pair would you expect to be the central atom in a Lewis structure?
(f) C vs. F
Verified step by step guidance1
Identify the general rule for selecting a central atom in a Lewis structure: The central atom is typically the least electronegative element, as it is more likely to share its electrons and form bonds with surrounding atoms.
Compare the electronegativities of carbon (C) and fluorine (F). Carbon has an electronegativity of approximately 2.5, while fluorine has the highest electronegativity of all elements, approximately 4.0.
Since carbon is less electronegative than fluorine, it is more likely to serve as the central atom in a Lewis structure.
Consider the bonding capacity of each atom. Carbon typically forms four bonds due to its four valence electrons, making it well-suited to act as a central atom. Fluorine, on the other hand, usually forms only one bond because it has seven valence electrons and needs only one more to complete its octet.
Conclude that carbon (C) is the preferred central atom in this pair when constructing a Lewis structure, as it is less electronegative and has a higher bonding capacity than fluorine (F).
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.
Recommended video:
Guided course
04:12
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 valency. It is usually the least electronegative atom in a molecule, as it can effectively bond with surrounding atoms to create a stable structure.
Recommended video:
Guided course
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 the context of 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.
Recommended video:
Guided course
1:47Electronegativity
Related Practice
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
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
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
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
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)