Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Formal Charges

Organic Chemistry

1. A Review of General Chemistry

Formal Charges

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1:51 minutes

Problem 28e

Textbook Question

Calculate the formal charge of the indicated atom in the following molecules or ions.
(e)

Verified step by step guidance

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.

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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 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.

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.

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.

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Textbook Question

By moving an electron pair, draw a better Lewis structure that minimizes formal charges.

(b)

Textbook Question

By moving an electron pair, draw a better Lewis structure that minimizes formal charges.

(a)

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.

Textbook Question

Calculate the formal charge of the indicated atom in the following molecules or ions.

(f)

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.

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

Textbook Question

Calculate the formal charge of the indicated atom in the following molecules or ions.

(d)

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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Calculate the formal charge of the indicated atom in the following molecules or ions. (e)

Key Concepts

Formal Charge

Lewis Structures

Valence Electrons

Watch next

Calculate the formal charge of the indicated atom in the following molecules or ions.
(e)