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-
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 28e
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 28eChapter 1, Problem 28e
Calculate the formal charge of the indicated atom in the following molecules or ions.
(e) 
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 (Nitrogen in this case) and determine its number of valence electrons. Nitrogen belongs to Group 15 in the periodic table, so it has 5 valence electrons.
Step 3: Count the number of non-bonding electrons (lone pairs) on the nitrogen atom. In the structure, nitrogen has one lone pair, which corresponds to 2 non-bonding electrons.
Step 4: Count the number of bonding electrons around the nitrogen atom. Nitrogen is bonded to three hydrogen atoms and one carbon atom, forming four single bonds. Each single bond contributes 2 bonding electrons, so the total bonding electrons are 8.
Step 5: Plug the values into the formula: Formal Charge = 5 (valence electrons) - 2 (non-bonding electrons) - (1/2 × 8 bonding electrons). Simplify the expression to determine the formal charge.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1mWas this helpful?
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 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.
Recommended video:
Guided course
01:34
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, which is essential for calculating formal charges and understanding molecular geometry.
Recommended video:
Guided course
04:12Drawing the Lewis Structure for N2H4.
Valence Electrons
Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds with other atoms. Knowing the number of valence electrons for each atom is crucial for drawing Lewis structures and calculating formal charges, as it directly influences the bonding and stability of the molecule.
Recommended video:
Guided course
03:40Valence Electrons of Transition Metals
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
1
views
Textbook Question
Calculate the formal charge of the indicated atom in the following molecules or ions.
(f)
2
views
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+
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
Calculate the formal charge of the indicated atom in the following molecules or ions.
(d)
1
views