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Ch.9 - Chemical Bonding I: The Lewis Model
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.9 - Chemical Bonding I: The Lewis ModelProblem 98e
Chapter 9, Problem 98e

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

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Identify the atoms in the condensed structural formula CH3CHO: 1 carbon (C) in CH3, 1 carbon (C) in CHO, 1 oxygen (O), and 4 hydrogens (H).
Determine the connectivity: The CH3 group is connected to the CHO group, indicating a carbon-carbon bond.
Recognize that the CHO group represents an aldehyde functional group, which consists of a carbonyl group (C=O) bonded to a hydrogen atom.
Draw the carbon skeleton: Connect the two carbon atoms with a single bond, then attach the CH3 group to one carbon and the CHO group to the other.
Complete the structure by adding the double bond between the carbon and oxygen in the CHO group, and attach the hydrogen atoms to the appropriate carbon atoms to satisfy the valency of each atom.

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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 CH3CHO, the formula indicates that there are two carbon atoms, with one being part of a carbonyl group (C=O) and the other connected to three hydrogens, which helps in determining the arrangement of atoms in the Lewis structure.
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Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for forming bonds with other atoms. The number of valence electrons determines how atoms will bond and the overall structure of the molecule. In drawing Lewis structures, it is important to account for the total number of valence electrons available from all atoms involved to ensure accurate representation of the molecule.
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Related Practice
Textbook Question

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

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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.

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Textbook Question

Draw the Lewis structure for urea, H2NCONH2, one of the compounds responsible for the smell of urine. (The central carbon atom is bonded to both nitrogen atoms and to the oxygen atom.) Does urea contain polar bonds? Which bond in urea is most polar?

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Textbook Question

Use Lewis structures to explain why Br3- and I3- are stable, while F3- is not.

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Textbook Question

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

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