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 60a
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 60aChapter 1, Problem 60a
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) 
Verified step by step guidance1
Step 1: Identify the central atom in the structure. Silicon (Si) is the central atom because it can form multiple bonds and is less electronegative than hydrogen (H).
Step 2: Determine the total number of valence electrons available. Silicon has 4 valence electrons, and each hydrogen atom contributes 1 valence electron. With 4 hydrogens, the total is 4 + 4 = 8 valence electrons.
Step 3: Place single bonds between the central atom (Si) and each hydrogen atom. Each bond uses 2 electrons, and since there are 4 hydrogens, this will use up all 8 valence electrons.
Step 4: Verify that the octet rule is satisfied for the central atom. Silicon will have 8 electrons around it (4 bonds × 2 electrons per bond), fulfilling its octet.
Step 5: Confirm that hydrogen atoms are satisfied with their duet rule. Each hydrogen atom is bonded to silicon with a single bond, giving them 2 electrons each, which satisfies their requirement.
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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 in chemical reactions.
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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 particularly applicable to main group elements and is crucial for determining how atoms will bond in a molecule, ensuring that each atom achieves a full octet.
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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 an element's chemical properties and its ability to bond with other elements. In the context of Lewis structures, knowing the number of valence electrons is essential for accurately depicting how atoms connect and ensuring that the octet rule is satisfied.
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Related Practice
Textbook Question
By moving an electron pair, draw a better Lewis structure that minimizes formal charges.
(a)
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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
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)