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

Lewis Structure

Organic Chemistry

1. A Review of General Chemistry

Lewis Structure

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4:55 minutes

Problem 62l

Textbook Question

Draw the Lewis structure for the following molecular formulas.
(l) SO₄^2-

Verified step by step guidance

Step 1: Count the total number of valence electrons available for the molecule. Sulfur (S) belongs to Group 16 and has 6 valence electrons. Oxygen (O) also belongs to Group 16 and has 6 valence electrons each. Since the molecule has a charge of -2, add 2 extra electrons to the total count.

Step 2: Determine the central atom. Sulfur (S) is less electronegative than oxygen (O), so it will be the central atom. Arrange the four oxygen atoms around the sulfur atom.

Step 3: Connect the sulfur atom to each oxygen atom using single bonds. Each single bond represents 2 electrons. Subtract these electrons from the total valence electron count.

Step 4: Distribute the remaining electrons as lone pairs around the oxygen atoms to satisfy the octet rule for each oxygen. If there are leftover electrons, place them on the central sulfur atom.

Step 5: Check the formal charges on each atom. Adjust the bonding (e.g., by forming double bonds) if necessary to minimize formal charges while keeping the total charge of the molecule as -2.

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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 indicate bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the molecule's structure and stability. For polyatomic ions like SO₄²⁻, calculating the total number of valence electrons is necessary for accurately constructing the Lewis structure.

Formal Charge

Formal charge is a concept used to determine the distribution of electrons in a molecule or ion. It is calculated by comparing the number of valence electrons in the free atom to the number of electrons assigned to it in the Lewis structure. Minimizing formal charges across a molecule helps identify the most stable structure, which is particularly important for polyatomic ions like sulfate (SO₄²⁻).

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Textbook Question

Which atom in each pair would you expect to be the central atom in a Lewis structure?

(d) C vs. N

Textbook Question

Which atom in each pair would you expect to be the central atom in a Lewis structure?

(f) C vs. F

Textbook Question

Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet.

(d)

Textbook Question

Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet.

(e)

Textbook Question

Draw Lewis structures for the following free radicals.

a. The ethyl radical, CH₃—ĊH₂

b. The tert-butyl radical, (CH₃)₃C•

Textbook Question

In addition to radicals, anions, and cations, a fourth class of reactive intermediates is carbenes. A neutral species, the simplest carbene has a molecular formula of CH₂.

(a) Draw the Lewis structure of CH₂.

Textbook Question

Draw the Lewis structure for the following molecular formulas.

(j) H₂SO₄

Textbook Question

Draw the Lewis structure for the following molecular formulas.

(v) CH₅N

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