Textbook Question
Calculate the formal charge of the indicated atom in the following molecules or ions.
(e)
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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 29b
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 29bChapter 1, Problem 29b
Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.
(b) H+
Verified step by step guidance1
Step 1: Understand the problem. You are tasked with drawing the Lewis structure for the hydrogen ion (H⁺) and calculating the formal charge to confirm the correctness of the structure.
Step 2: Recall that hydrogen (H) has one valence electron in its neutral state. The H⁺ ion indicates that hydrogen has lost one electron, leaving it with no valence electrons.
Step 3: Draw the Lewis structure for H⁺. Since there are no valence electrons remaining, the Lewis structure for H⁺ is simply the symbol 'H' without any dots or bonds around it.
Step 4: Calculate the formal charge of H⁺ using the formula: Formal charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons / 2). For H⁺, the calculation is: Formal charge = 1 - 0 - 0 = +1.
Step 5: Confirm that the formal charge matches the charge of the ion. The calculated formal charge of +1 aligns with the charge of H⁺, verifying that the Lewis structure is correct.
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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. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.
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Drawing the Lewis Structure for N2H4.
Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and half the number of bonding electrons. It helps in assessing the stability of a Lewis structure; structures with formal charges closest to zero are generally more stable.
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Ionic Species
Ionic species are atoms or molecules that have gained or lost electrons, resulting in a net charge. For example, H⁺ is a hydrogen ion that has lost its single electron, making it positively charged. Understanding ionic species is crucial for predicting their behavior in chemical reactions and their interactions with other molecules.
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Related Practice
Textbook Question
Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.
(c) BH4-
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Textbook Question
Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.
(d) AlCl4-
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Textbook Question
Calculate the formal charge of the indicated atom in the following molecules or ions.
(f)
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Textbook Question
Calculate the formal charge of the indicated atoms in the ions shown.
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Textbook Question
Calculate the formal charge of the indicated atom in the following molecules or ions.
(d)
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