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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3:13 minutes

Problem 29b

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⁺

Verified step by step guidance

Step 1: Understand the problem. You are tasked with drawing the Lewis structure for the hydrogen ion (H⁺) and calculating the formal charge to confirm the correctness of the structure.

Step 2: Recall that hydrogen (H) has one valence electron in its neutral state. The H⁺ ion indicates that hydrogen has lost one electron, leaving it with no valence electrons.

Step 3: Draw the Lewis structure for H⁺. Since there are no valence electrons remaining, the Lewis structure for H⁺ is simply the symbol 'H' without any dots or bonds around it.

Step 4: Calculate the formal charge of H⁺ using the formula: Formal charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons / 2). For H⁺, the calculation is: Formal charge = 1 - 0 - 0 = +1.

Step 5: Confirm that the formal charge matches the charge of the ion. The calculated formal charge of +1 aligns with the charge of H⁺, verifying that the Lewis structure is correct.

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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 use dots to represent valence electrons and lines to represent bonds. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

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 assessing the stability of a Lewis structure; structures with formal charges closest to zero are generally more stable.

Ionic Species

Ionic species are atoms or molecules that have gained or lost electrons, resulting in a net charge. For example, H⁺ is a hydrogen ion that has lost its single electron, making it positively charged. Understanding ionic species is crucial for predicting their behavior in chemical reactions and their interactions with other molecules.

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Related Practice

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

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.

(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.

Textbook Question

Looking ahead in Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs.

(a)

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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+

Key Concepts

Lewis Structures

Formal Charge

Ionic Species

Watch next

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⁺