Textbook Question
Calculate the formal charge of the indicated atom in the following molecules or ions.
(e)
1
views
Ch. 2 - General Chemistry Translated: Finding the Electrons
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
Not the one you use?Change textbookSelect a different textbook
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
All textbooks
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 27b
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 27bChapter 1, Problem 27b
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
Verified step by step guidance1
Step 1: Identify the total number of valence electrons in the molecule. Hydrogen (H) has 1 valence electron, oxygen (O) has 6 valence electrons, and bromine (Br) has 7 valence electrons. Add these together to determine the total number of valence electrons available for bonding.
Step 2: Determine the central atom. In this case, bromine (Br) is the central atom as indicated in the problem. Arrange the atoms with bromine in the center, oxygen bonded to bromine, and hydrogen bonded to oxygen.
Step 3: Draw single bonds between the atoms. Connect bromine to oxygen with a single bond and oxygen to hydrogen with another single bond. Each bond represents two shared electrons.
Step 4: Distribute the remaining valence electrons around the atoms to satisfy the octet rule for oxygen and bromine. Place lone pairs on oxygen and bromine as needed, ensuring that oxygen has 8 electrons and bromine has 8 electrons (including the bonding electrons). Hydrogen only needs 2 electrons to complete its duet.
Step 5: Calculate the formal charge for each atom to confirm the structure is correct. Use the formula: Formal charge = (Valence electrons of the atom) - (Non-bonding electrons) - (1/2 × Bonding electrons). Ensure the sum of formal charges equals the overall charge of the molecule, which is neutral in this case.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
3mWas this helpful?
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 help visualize the arrangement of electrons and the connectivity of atoms, allowing chemists to predict molecular geometry and reactivity. In drawing Lewis structures, one must account for the total number of valence electrons available from all atoms involved.
Recommended video:
Guided course
04:12
Drawing the Lewis Structure for N2H4.
Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated to help assess the stability of a Lewis structure. It is determined using the formula: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons). A structure is generally more stable when the formal charges are minimized and closer to zero, aiding in the validation of the drawn Lewis structure.
Recommended video:
Guided course
01:34Calculating formal and net charge.
Central Atom Identification
The central atom in a molecule is typically the least electronegative atom that can form multiple bonds, serving as the core around which other atoms are arranged. Identifying the central atom is crucial for accurately constructing the Lewis structure, as it dictates the overall shape and connectivity of the molecule. In the case of HOBr, the central atom is oxygen, which is bonded to both hydrogen and bromine.
Recommended video:
Guided course
01:44The difference between atomic numbers and atomic mass.
Related Practice
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
2
views
Textbook Question
Based on your answer to Assessment 2.22, would you expect a larger atom to be more or less electronegative than a smaller atom?
3
views
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
1
views
Textbook Question
Without looking at Figure 2.20, use your intuition to estimate whether a bond is ionic, polar covalent, or covalent.
(a) Na―Cl
1
views
Textbook Question
Calculate the formal charge of the indicated atom in the following molecules or ions.
(d)
1
views