Chapter 24: Problem 24
Describe the reaction between \(\mathrm{CO}_{2}\) and \(\mathrm{OH}^{-}\) in terms of a Lewis acid-base reaction.
Short Answer
Expert verified
\(\mathrm{CO}_{2}\) is the Lewis acid and \(\mathrm{OH}^{-}\) is the Lewis base, forming \(\mathrm{HCO}_{3}^{-}\).
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Electron-Pair Acceptor
In chemistry, an electron-pair acceptor is commonly referred to as a Lewis acid. This concept stems from the Lewis theory of acids and bases, which focuses on the ability of atoms and molecules to donate and accept electron pairs. In any Lewis acid-base reaction, the Lewis acid is the entity that accepts a pair of electrons.
In the reaction between carbon dioxide (CO₂) and hydroxide ion (OH⁻), CO₂ acts as the electron-pair acceptor. The carbon atom in CO₂ has a partial positive charge due to the highly electronegative oxygen atoms. This makes it an ideal candidate to attract and accept a pair of electrons, forming a new chemical bond.
Understanding the role of electron-pair acceptors helps in visualizing how atoms or molecules can undergo transformation during chemical reactions. This ability to accept electrons is crucial in many reactions, particularly in the formation of coordinate covalent bonds.
In the reaction between carbon dioxide (CO₂) and hydroxide ion (OH⁻), CO₂ acts as the electron-pair acceptor. The carbon atom in CO₂ has a partial positive charge due to the highly electronegative oxygen atoms. This makes it an ideal candidate to attract and accept a pair of electrons, forming a new chemical bond.
Understanding the role of electron-pair acceptors helps in visualizing how atoms or molecules can undergo transformation during chemical reactions. This ability to accept electrons is crucial in many reactions, particularly in the formation of coordinate covalent bonds.
Electron-Pair Donor
An electron-pair donor is what we call a Lewis base. According to the Lewis theory, a Lewis base donates a pair of electrons to a Lewis acid in a chemical reaction. This donation is an essential aspect of forming new bonds and involves atoms with lone pairs of electrons.
In the interaction between CO₂ and OH⁻, the hydroxide ion (OH⁻) functions as the electron-pair donor. The oxygen in the hydroxide ion has a lone pair of electrons that it can share or "donate". By offering these electrons, OH⁻ can form a bond with CO₂.
This electron-pair donation not only helps stabilize the resultant compound but also drives the entire reaction forward. Understanding electron-pair donors' role aids in predicting and deciphering chemical bonding scenarios in diverse reactions.
In the interaction between CO₂ and OH⁻, the hydroxide ion (OH⁻) functions as the electron-pair donor. The oxygen in the hydroxide ion has a lone pair of electrons that it can share or "donate". By offering these electrons, OH⁻ can form a bond with CO₂.
This electron-pair donation not only helps stabilize the resultant compound but also drives the entire reaction forward. Understanding electron-pair donors' role aids in predicting and deciphering chemical bonding scenarios in diverse reactions.
Bicarbonate Ion
The bicarbonate ion, represented as \(\mathrm{HCO}_{3}^{-}\), is the product of the Lewis acid-base reaction between CO₂ and OH⁻. It forms when OH⁻ donates its lone pair of electrons to CO₂, integrating a subsequent hydrogen shift.
Bicarbonate ions are essential in many chemical and biological processes. They act as buffers in biological systems, helping to maintain pH balance in our blood and other fluids. The creation of bicarbonate in this reaction is a straightforward example of how chemical transformations can lead to biologically significant ions.
In terms of structure, bicarbonate maintains a resonance stabilization, showing different forms of electron arrangement, which contribute to its stability and reactivity in various environments.
Bicarbonate ions are essential in many chemical and biological processes. They act as buffers in biological systems, helping to maintain pH balance in our blood and other fluids. The creation of bicarbonate in this reaction is a straightforward example of how chemical transformations can lead to biologically significant ions.
In terms of structure, bicarbonate maintains a resonance stabilization, showing different forms of electron arrangement, which contribute to its stability and reactivity in various environments.
Chemical Bonding
Chemical bonding is the interaction that holds atoms together in molecules and compounds. In the context of Lewis acid-base reactions, it involves the transfer and sharing of electrons to form new bonds.
When OH⁻ approaches CO₂, the lone pair of electrons from OH⁻ bonds with the carbon atom in CO₂. This results in the formation of a coordinate covalent bond, where both electrons in the bond come from the same atom, which is typical in many Lewis acid-base interactions.
Understanding chemical bonding in such processes is fundamental, as it explains the stable formation of compounds like bicarbonate, and emphasizes how atoms achieve greater stability through electron sharing or transfer.
When OH⁻ approaches CO₂, the lone pair of electrons from OH⁻ bonds with the carbon atom in CO₂. This results in the formation of a coordinate covalent bond, where both electrons in the bond come from the same atom, which is typical in many Lewis acid-base interactions.
Understanding chemical bonding in such processes is fundamental, as it explains the stable formation of compounds like bicarbonate, and emphasizes how atoms achieve greater stability through electron sharing or transfer.
Reaction Mechanism
A reaction mechanism details the step-by-step process by which reactants are converted into products. For the reaction between CO₂ and OH⁻, the mechanism lays out how the electrons are transferred and how bonds are reformed.
Initially, the OH⁻ ion approaches CO₂ and utilizes its lone pair of electrons to attack the carbon atom of CO₂. As the electrons are shared, a new covalent bond is formed between the hydroxide and carbon atoms. During this bonding, the oxygen atoms in CO₂ and the hydrogen ion adjust to stabilize the bicarbonate ion.
Understanding the reaction mechanism is crucial as it allows chemists to predict the course of reactions, design experiments, and synthesize new compounds deliberately. A diligence in following reaction mechanisms reveals much about the dynamics of atoms during chemical changes.
Initially, the OH⁻ ion approaches CO₂ and utilizes its lone pair of electrons to attack the carbon atom of CO₂. As the electrons are shared, a new covalent bond is formed between the hydroxide and carbon atoms. During this bonding, the oxygen atoms in CO₂ and the hydrogen ion adjust to stabilize the bicarbonate ion.
Understanding the reaction mechanism is crucial as it allows chemists to predict the course of reactions, design experiments, and synthesize new compounds deliberately. A diligence in following reaction mechanisms reveals much about the dynamics of atoms during chemical changes.
