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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1:42 minutes

Problem 28d

Textbook Question

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

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 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.

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.

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

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

(f)

Textbook Question

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

(e)

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

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⁺

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^-

Textbook Question

Calculate the formal charge of the indicated atoms in the ions shown.

Textbook Question

Calculate the formal charge on the non-hydrogen atoms in the molecules shown. Use the arrow-pushing formalism to 'move' an electron pair such that it is shared between two (formerly) charged atoms. Your arrow should account for the formation of the molecule on the right from the molecule on the left.

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

Key Concepts

Formal Charge

Lewis Structures

Resonance Structures

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