Textbook Question
Predict the ordering, from shortest to longest, of the bond lengths in CO, CO2, and CO32- .
845
views
Ch.8 - Basic Concepts of Chemical Bonding
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 8, Problem 54c
Consider the formate ion, HCO2-, which is the anion formed when formic acid loses an H+ ion. The H and the two O atoms are bonded to the central C atom. (c) Would you predict that the C—O bond lengths in the formate ion would be longer or shorter relative to those in CO2?
Verified step by step guidance1
To predict the C—O bond lengths in the formate ion relative to those in CO2, we need to consider the type of bonding and resonance structures involved.
In CO2, the carbon atom forms double bonds with each oxygen atom. This results in a linear molecule with two equivalent C=O double bonds.
In the formate ion (HCO2-), the structure can be represented by resonance forms. The negative charge is delocalized between the two oxygen atoms, leading to a resonance hybrid where the C—O bonds are neither purely single nor purely double bonds.
The resonance in the formate ion results in partial double bond character for both C—O bonds, making them shorter than a typical C—O single bond but longer than a C=O double bond.
Therefore, the C—O bond lengths in the formate ion are expected to be shorter than a C—O single bond but longer than the C=O double bonds in CO2, due to the resonance stabilization and partial double bond character.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
3mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Bond Lengths and Strengths
Bond lengths are influenced by the type of bond and the atoms involved. Generally, shorter bonds are stronger due to greater overlap of atomic orbitals. In molecules like CO2, the double bonds between carbon and oxygen result in shorter bond lengths compared to single bonds. Understanding this relationship is crucial for predicting bond lengths in different compounds.
Recommended video:
Guided course
00:36
Average Bond Order
Resonance Structures
Resonance structures are different ways of drawing a molecule that represent the same arrangement of atoms but differ in the distribution of electrons. The formate ion has resonance between two structures, which can affect bond lengths and strengths. This delocalization of electrons can lead to bond lengths that are intermediate between single and double bonds, impacting predictions about bond lengths in comparison to CO2.
Recommended video:
Guided course
01:42Resonance Structures
Electronegativity and Bond Character
Electronegativity refers to the tendency of an atom to attract electrons in a bond. In the case of the formate ion, the difference in electronegativity between carbon and oxygen affects the bond character. The C—O bonds in formate are influenced by the partial charges resulting from this difference, which can lead to variations in bond lengths compared to the purely double-bonded C=O in CO2.
Recommended video:
Guided course
00:56Metallic Character Example
Related Practice
Textbook Question
(c) What would you predict for the lengths of the bonds in NO2- relative to N¬O single bonds and double bonds?
Textbook Question
For each of the following molecules or ions of sulfur and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: (a) SO2 Write a single Lewis structure that obeys the octet rule for SO2 and assign the formal charges on all the atoms. (b) SO3 Write a single Lewis structure that obeys the octet rule for SO3 and assign the formal charges on all the atoms. (c) SO32- Write a single Lewis structure that obeys the octet rule for SO32- and assign the formal charges on all the atoms.
573
views
Textbook Question
Based on Lewis structures, predict the ordering, from shortest to longest, of N¬O bond lengths in NO+, NO2-, and NO3-.
1530
views
1
comments