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 55i
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 55iChapter 1, Problem 55i
How many valence electrons does each of the following contribute to a Lewis structure?
(i) Cl
Verified step by step guidance1
Step 1: Recall the concept of valence electrons. Valence electrons are the outermost electrons of an atom that participate in chemical bonding. The number of valence electrons for an element can be determined from its position in the periodic table.
Step 2: Locate chlorine (Cl) on the periodic table. Chlorine is in Group 17 (or Group VIIA in older notations), which is the halogen group.
Step 3: Understand that elements in Group 17 have 7 valence electrons because they are one electron short of completing their octet (8 electrons in the outer shell).
Step 4: Write the electron configuration of chlorine to confirm the number of valence electrons. The electron configuration of Cl is: . The outermost shell (n=3) contains 7 electrons (2 in 3s and 5 in 3p).
Step 5: Conclude that chlorine contributes 7 valence electrons to a Lewis structure, which is consistent with its group number and electron configuration.
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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, as they can be shared or transferred between atoms. For example, in the case of chlorine (Cl), it has seven valence electrons, which influences its reactivity and the types of bonds it can form.
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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. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.
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04:12Drawing the Lewis Structure for N2H4.
Chlorine in Lewis Structures
In Lewis structures, chlorine typically contributes seven valence electrons, which allows it to form one covalent bond while having three lone pairs. This configuration is significant because it helps illustrate chlorine's tendency to gain an electron to achieve a stable octet, making it a highly reactive nonmetal. Recognizing chlorine's electron configuration is key to understanding its role in various chemical reactions.
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