Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

12. Introduction to Organic Chemistry

Condensed Formula

GOB Chemistry

12. Introduction to Organic Chemistry

Condensed Formula

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3:51 minutes

Problem 8b

Textbook Question

Draw a Lewis structure for each of the following compounds:
(b)

Verified step by step guidance

Identify the total number of valence electrons for the compound. To do this, determine the number of valence electrons contributed by each atom in the compound based on their group number in the periodic table.

Determine the central atom in the compound. The central atom is usually the least electronegative element (excluding hydrogen).

Arrange the remaining atoms around the central atom and connect them with single bonds. Each single bond represents two electrons.

Distribute the remaining valence electrons as lone pairs around the outer atoms to satisfy the octet rule (or duet rule for hydrogen). If there are still electrons left, place them on the central atom.

If the central atom does not have a complete octet, consider forming double or triple bonds by sharing lone pairs from the surrounding atoms with the central atom. Ensure all atoms satisfy the octet rule where applicable.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Lewis Structure

A Lewis structure is a diagram that represents the bonding between atoms in a molecule and the lone pairs of electrons that may exist. It uses dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds with other atoms. The number of valence electrons determines how an atom can bond with others, influencing the molecule's structure and reactivity. Knowing how to count and distribute valence electrons is crucial for accurately drawing Lewis structures.

Octet Rule

The octet rule is a chemical rule of thumb that states atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule helps predict how atoms will bond and the arrangement of electrons in Lewis structures, guiding the drawing of accurate representations of molecules.

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Related Practice

Textbook Question

Identify each of the following as a formula of an organic or inorganic compound. For an organic compound, indicate if represented as molecular formula, expanded, or condensed structural formula:

b. CH₃―CH₂―CH₂―CH₃

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