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 28d
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 28dChapter 1, Problem 28d
Calculate the formal charge of the indicated atom in the following molecules or ions.
(d) 
Verified step by step guidance1
Step 1: Recall the formula for calculating formal charge: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (1/2 × Bonding Electrons).
Step 2: Identify the atom in question and determine the number of valence electrons it has based on its position in the periodic table.
Step 3: Count the number of non-bonding electrons (lone pairs) around the atom. Each lone pair contributes 2 electrons.
Step 4: Count the number of bonding electrons (shared electrons in bonds) around the atom. Each bond contributes 2 electrons, but only half of these are assigned to the atom in question.
Step 5: Substitute the values for valence electrons, non-bonding electrons, and bonding electrons into the formula to calculate the formal charge of the atom.
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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 based on the number of valence electrons, the number of non-bonding electrons, and the number of bonds. The formula is: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons). This concept helps in understanding the distribution of electrons in a molecule and assessing the stability of different resonance structures.
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Calculating formal and net charge.
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 provide a visual representation of the arrangement of electrons and help in predicting the formal charge of atoms. Understanding how to draw and interpret Lewis structures is essential for calculating formal charges accurately.
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Resonance Structures
Resonance structures are different ways of drawing the same molecule that show the delocalization of electrons. They are used when a single Lewis structure cannot adequately represent the electron distribution. Recognizing resonance structures is important for understanding the stability of a molecule and the implications for formal charge, as the actual structure is a hybrid of all possible resonance forms.
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Related Practice
Textbook Question
Draw the Lewis structure for the following molecules. Be sure to calculate the formal charge of each atom as a way of confirming your structure is correct.
(b) HOBr
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Textbook Question
Using only your intuition, rank the following covalent bonds in terms of their polarity (1 = most polar; 6 = least polar). [You can use the periodic trend of electronegativity, but don't use actual numbers.]
(a) C―C
(b) C―O
(c) C―H
(d) C―F
(e) C―Cl
(f) C―S
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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
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+
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Textbook Question
Draw the Lewis structure for the following molecules. Be sure to calculate the formal charge of each atom as a way of confirming your structure is correct.
(c) CF4
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