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Ch.9 - Chemical Bonding I: The Lewis Model
All textbooksTro 4th EditionCh.9 - Chemical Bonding I: The Lewis ModelProblem 98b
Chapter 9, Problem 98b

Draw the Lewis structure for each organic compound from its condensed structural formula. b. CH3OCH3

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1
Identify the atoms in the condensed structural formula CH3OCH3. There are two carbon (C) atoms, one oxygen (O) atom, and six hydrogen (H) atoms.
Determine the connectivity of the atoms. The formula suggests that the oxygen atom is between the two carbon atoms, forming a C-O-C linkage.
Draw the carbon atoms first, and connect them with a single bond to the oxygen atom: C-O-C.
Attach the hydrogen atoms to the carbon atoms. Each carbon atom in CH3 has three hydrogen atoms attached, so add three hydrogens to each carbon.
Ensure that each atom satisfies the octet rule (or duet for hydrogen). Carbon should have four bonds, oxygen should have two bonds, and hydrogen should have one bond.

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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 electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.
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Condensed Structural Formula

A condensed structural formula provides a shorthand way of representing the structure of a molecule, showing how atoms are connected without depicting all the bonds explicitly. For example, in CH3OCH3, the formula indicates that there are two methyl groups (CH3) connected by an oxygen atom, which is crucial for understanding the molecular structure before drawing the Lewis structure.
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Valence Electrons

Valence electrons are the outermost electrons of an atom and are involved in forming bonds with other atoms. Knowing the number of valence electrons for each atom in a molecule is vital for accurately drawing Lewis structures, as it determines how atoms will bond and the overall stability of the molecule.
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Related Practice
Textbook Question

The cyanate ion (OCN-) and the fulminate ion (CNO-) share the same three atoms but have vastly different properties. The cyanate ion is stable, while the fulminate ion is unstable and forms explosive compounds. The resonance structures of the cyanate ion are explored in Example 9.8. Draw Lewis structures for the fulminate ion—including possible resonance forms— and use formal charge to explain why the fulminate ion is less stable (and therefore more reactive) than the cyanate ion.

Textbook Question

Draw the Lewis structure for each organic compound from its condensed structural formula. a. C3H8 d. CH3COOH

Textbook Question

Draw the Lewis structure for each organic compound from its condensed structural formula. c. CH3COCH3

Textbook Question

Draw the Lewis structure for each organic compound from its condensed structural formula. e. CH3CHO