Textbook Question
Looking ahead in Chapter 4, we explain that molecules like CH3+ are Lewis acids or electron pair acceptors. Into which orbital would the new electron pair go?
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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 85a
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 85aChapter 1, Problem 85a
Looking ahead in Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs.
(a) 
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Identify the formal charge on each atom in the molecule. Recall that formal charge is calculated using the formula: .
Determine the number of valence electrons for each atom based on its position in the periodic table. For example, oxygen has 6 valence electrons, nitrogen has 5, etc.
Using the formal charge and the number of valence electrons, calculate the number of lone pair electrons for each atom. Lone pairs are the non-bonding electrons that remain after accounting for bonding electrons.
Draw the Lewis structure of the molecule, ensuring that the total number of electrons matches the sum of the valence electrons for all atoms in the molecule. Place lone pairs on atoms to satisfy their formal charges and the octet rule (if applicable).
Double-check the structure to ensure that the formal charges on all atoms are consistent with the given information and that the total charge of the molecule matches the overall charge (if any).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated by taking the number of valence electrons in the free atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. It helps in determining the most stable structure of a molecule by minimizing the formal charges across the atoms.
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Calculating formal and net charge.
Lone Pairs
Lone pairs are pairs of valence electrons that are not involved in bonding and are localized on a single atom. They play a crucial role in determining the geometry and reactivity of molecules, as they can influence the shape and polarity of the molecule due to their repulsive interactions with bonding pairs.
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Electron Pair Geometry
Electron pair geometry refers to the spatial arrangement of all electron pairs (bonding and lone pairs) around a central atom. Understanding this geometry is essential for predicting molecular shapes and angles, which are determined by the repulsion between electron pairs according to VSEPR (Valence Shell Electron Pair Repulsion) theory.
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Related Practice
Textbook Question
Looking ahead in Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs.
(c)
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Textbook Question
The C―N bond in the following amide is much stronger than the C―N bond in the amine. Explain.
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Textbook Question
In Chapter 4, we explain that molecules like CH3- are Lewis bases or electron pair donors. What makes it a Lewis base?
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Textbook Question
In comparison to CH3- in Assessment 2.86, the related molecule BH4- is itself not a Lewis base at boron. Why?
Textbook Question
In comparison to CH3+ in Assessment 2.82, the related molecule H3O+ is not a Lewis acid at oxygen. Why?
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