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the expected O-C-O bo 12- :Ö: C. O. O

the expected O-C-O bo 12- :Ö: C. O. O

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Understanding the Expected O-C-O Bond Angle in a Carbonate Ion (CO₃²⁻) In this example, we explore the expected bond angle between oxygen, carbon, and oxygen atoms within a carbonate ion (CO₃²⁻). #### Lewis Structures The image displays three resonance structures of the carbonate ion, CO₃²⁻. Each structure is represented within square brackets and accompanied by a 2– superscript, indicating the overall -2 charge of the ion. - **Resonance 1 (leftmost):** - The carbon atom (C) is centrally located. - Two oxygen atoms (O) with a single bond and lone pairs of electrons. - One oxygen atom (O) with a double bond to the carbon atom. - **Resonance 2 (middle):** - Similar structure to the first resonance form with the double bond shifted to another oxygen atom. - **Resonance 3 (rightmost):** - The double bond is shifted to the last oxygen atom, yielding an equivalent resonance structure. All resonance structures highlight that the molecule has delocalized electrons, which implies that the actual molecule is a hybrid of these forms. #### Multiple Choice Question The question accompanying the Lewis structures is: **"What is the expected O-C-O bond angle in a carbonate ion (CO₃²⁻)?"** Options provided are: 1. 90 2. 120 3. <109.5 4. 109.5 #### Explanation of the Answer Given that the carbonate ion features a central carbon atom with three regions of electron density (one for each oxygen atom), the molecular geometry should be **trigonal planar**. - In a trigonal planar geometry, the expected bond angles between atoms are **120°**. Therefore, the correct answer to the question is option (4): **120°.** #### Conclusion Understanding resonance structures and molecular geometry is crucial in predicting bond angles accurately. The carbonate ion is a common example demonstrating these concepts, showing consistent 120° bond angles due to its trigonal planar configuration.
Transcribed Image Text:### Understanding the Expected O-C-O Bond Angle in a Carbonate Ion (CO₃²⁻) In this example, we explore the expected bond angle between oxygen, carbon, and oxygen atoms within a carbonate ion (CO₃²⁻). #### Lewis Structures The image displays three resonance structures of the carbonate ion, CO₃²⁻. Each structure is represented within square brackets and accompanied by a 2– superscript, indicating the overall -2 charge of the ion. - **Resonance 1 (leftmost):** - The carbon atom (C) is centrally located. - Two oxygen atoms (O) with a single bond and lone pairs of electrons. - One oxygen atom (O) with a double bond to the carbon atom. - **Resonance 2 (middle):** - Similar structure to the first resonance form with the double bond shifted to another oxygen atom. - **Resonance 3 (rightmost):** - The double bond is shifted to the last oxygen atom, yielding an equivalent resonance structure. All resonance structures highlight that the molecule has delocalized electrons, which implies that the actual molecule is a hybrid of these forms. #### Multiple Choice Question The question accompanying the Lewis structures is: **"What is the expected O-C-O bond angle in a carbonate ion (CO₃²⁻)?"** Options provided are: 1. 90 2. 120 3. <109.5 4. 109.5 #### Explanation of the Answer Given that the carbonate ion features a central carbon atom with three regions of electron density (one for each oxygen atom), the molecular geometry should be **trigonal planar**. - In a trigonal planar geometry, the expected bond angles between atoms are **120°**. Therefore, the correct answer to the question is option (4): **120°.** #### Conclusion Understanding resonance structures and molecular geometry is crucial in predicting bond angles accurately. The carbonate ion is a common example demonstrating these concepts, showing consistent 120° bond angles due to its trigonal planar configuration.
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