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 55l
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 55lChapter 1, Problem 55l
How many valence electrons does each of the following contribute to a Lewis structure?
(l) ―1 charge
Verified step by step guidance1
Understand the concept of valence electrons: Valence electrons are the outermost electrons of an atom that participate in chemical bonding. For a Lewis structure, we count the valence electrons of all atoms and adjust for any charges present.
Recognize the effect of a negative charge: A negative charge (−1) indicates that the molecule or ion has gained one extra electron. This extra electron must be added to the total count of valence electrons.
Determine the total valence electrons: First, calculate the sum of the valence electrons for all atoms in the molecule or ion. Then, add one additional electron to account for the −1 charge.
Write the Lewis structure: Use the total number of valence electrons (including the extra electron from the −1 charge) to distribute electrons around the atoms, ensuring that each atom satisfies the octet rule (or duet rule for hydrogen) where applicable.
Verify the structure: Ensure that the total number of electrons in the Lewis structure matches the calculated total valence electrons, and confirm that the formal charges on the atoms are consistent with the overall −1 charge.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Valence Electrons
Valence electrons are the outermost electrons of an atom and are crucial for determining how an atom will bond with others. They are involved in chemical bonding and reactions, and their number can vary depending on the element. For example, carbon has four valence electrons, while oxygen has six. Understanding the number of valence electrons helps in predicting the structure and reactivity of molecules.
Recommended video:
Guided course
03:40
Valence Electrons of Transition Metals
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. This visual representation helps chemists understand the arrangement of electrons and the overall geometry of the molecule, which is essential for predicting its chemical behavior.
Recommended video:
Guided course
04:12Drawing the Lewis Structure for N2H4.
Charge Contribution
In the context of Lewis structures, the charge of an ion affects the total number of valence electrons considered. A negatively charged ion (anion) contributes additional electrons, while a positively charged ion (cation) has fewer. For example, a species with a -1 charge contributes one extra valence electron to the Lewis structure, which must be accounted for when drawing the structure and determining the overall electron count.
Recommended video:
Guided course
01:34Calculating formal and net charge.
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
How many valence electrons does each of the following contribute to a Lewis structure?
(j) Al
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Textbook Question
How many valence electrons does each of the following contribute to a Lewis structure?
(i) Cl
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?
(g) S
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