Textbook Question
Draw the Lewis structure for each organic compound from its condensed structural formula. c. CH3COCH3
741
views
Ch.9 - Chemical Bonding I: The Lewis Model
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Matter, Measurement & Problem Solving107
- Ch.2 - Atoms & Elements100
- Ch.3 - Molecules, Compounds & Chemical Equations127
- Ch.4 - Chemical Quantities & Aqueous Reactions114
- Ch.5 - Gases103
- Ch.6 - Thermochemistry92
- Ch.7 - Quantum-Mechanical Model of the Atom50
- Ch.8 - Periodic Properties of the Elements89
- Ch.9 - Chemical Bonding I: The Lewis Model84
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory74
- Ch.11 - Liquids, Solids & Intermolecular Forces60
- Ch.12 - Solids and Modern Material50
- Ch.13 - Solutions90
- Ch.14 - Chemical Kinetics111
- Ch.15 - Chemical Equilibrium65
- Ch.16 - Acids and Bases135
- Ch.17 - Aqueous Ionic Equilibrium145
- Ch.18 - Free Energy and Thermodynamics92
- Ch.19 - Electrochemistry100
- Ch.20 - Radioactivity and Nuclear Chemistry68
- Ch.21 - Organic Chemistry121
Chapter 9, Problem 98b
Draw the Lewis structure for each organic compound from its condensed structural formula. b. CH3OCH3
Verified step by step guidance1
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.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
49sWas this helpful?
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.
Recommended video:
Guided course
04:28
Lewis Dot Structures: Ions
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.
Recommended video:
Guided course
01:53Condensed Formula
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.
Recommended video:
Guided course
02:12Transition Metals Valence Electrons
Related Practice
Textbook Question
Draw the Lewis structure for each organic compound from its condensed structural formula. e. CH3CHO
879
views
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.
2691
views
Textbook Question
NaCl has a lattice energy of -787 kJ/mol. Consider a hypothetical salt XY. X3+ has the same radius of Na+ and Y3- has the same radius as Cl-. Estimate the lattice energy of XY.
1192
views