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How many o bonds and a bonds are there in an anthracene molecule?

How many o bonds and a bonds are there in an anthracene molecule?

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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**Anthracene Structure Exercise** **Introduction:** Anthracene is a yellow, crystalline solid commonly found in coal tar. It is composed of carbon and hydrogen atoms with the molecular formula C₁₄H₁₀. **Exercise:** **Objective:** Complete the structure for anthracene by adding bonds and hydrogen atoms as necessary. **Instructions:** 1. **Structure Layout:** - The diagram shows three connected hexagonal rings representing the carbon atoms in anthracene. - Each vertex in the hexagon represents a carbon atom (C). 2. **Tools Available:** - **Bonds:** Single, double, or triple bonds can be drawn between carbon atoms. - **Atoms:** Carbon (C) and Hydrogen (H) can be added. - **Erase:** Use the eraser tool to remove unnecessary elements. 3. **Steps:** - Begin by selecting the type of bond you need. - Add hydrogen atoms to satisfy the valency of each carbon atom. - Ensure that each carbon has four bonds in total. **Helpful Tips:** - Anthracene consists of three linearly fused benzene rings. - Each of the outer benzene rings contains alternating single and double bonds. - The central ring shares its bonds with the outer rings and typically contains three double bonds. Once completed, your structure should represent the planar, polycyclic aromatic configuration of anthracene.
Transcribed Image Text:**Anthracene Structure Exercise** **Introduction:** Anthracene is a yellow, crystalline solid commonly found in coal tar. It is composed of carbon and hydrogen atoms with the molecular formula C₁₄H₁₀. **Exercise:** **Objective:** Complete the structure for anthracene by adding bonds and hydrogen atoms as necessary. **Instructions:** 1. **Structure Layout:** - The diagram shows three connected hexagonal rings representing the carbon atoms in anthracene. - Each vertex in the hexagon represents a carbon atom (C). 2. **Tools Available:** - **Bonds:** Single, double, or triple bonds can be drawn between carbon atoms. - **Atoms:** Carbon (C) and Hydrogen (H) can be added. - **Erase:** Use the eraser tool to remove unnecessary elements. 3. **Steps:** - Begin by selecting the type of bond you need. - Add hydrogen atoms to satisfy the valency of each carbon atom. - Ensure that each carbon has four bonds in total. **Helpful Tips:** - Anthracene consists of three linearly fused benzene rings. - Each of the outer benzene rings contains alternating single and double bonds. - The central ring shares its bonds with the outer rings and typically contains three double bonds. Once completed, your structure should represent the planar, polycyclic aromatic configuration of anthracene.
**Understanding Bonding in Anthracene** **What type of hybrid orbitals are utilized by carbon in anthracene?** [Text Box for Answer] --- **How many σ bonds and π bonds are there in an anthracene molecule?** - **σ bonds:** [Text Box for Answer] - **π bonds:** [Text Box for Answer] --- **How many valence electrons occupy σ-bond orbitals, and how many occupy π-bond orbitals?** [Text Box for Answer] --- **Explanation** In the study of organic chemistry, understanding the types of bonds and hybridization present in molecules like anthracene is crucial. Anthracene, a polycyclic aromatic hydrocarbon, consists of three fused benzene rings. This structure is vital for determining the hybridization and bonding characteristics of the carbon atoms within the molecule. 1. **Hybridization**: The carbon atoms in anthracene typically utilize sp² hybrid orbitals. These orbitals form the framework for the σ bonds in the molecule, connecting carbon atoms and maintaining the structural integrity of the rings. 2. **σ bonds and π bonds**: In anthracene, σ bonds are formed through the overlap of sp² hybrid orbitals. Additionally, π bonds are formed from the side-by-side overlap of unhybridized p orbitals, contributing to the molecule’s aromaticity. 3. **Valence Electrons**: Understanding the electron distribution in σ and π bonds is key to grasping the molecule’s chemical properties. Typically, each σ bond accommodates two electrons, and π bonds also contain electrons that are delocalized across the molecule, crucial for the stability of the aromatic system. This foundational knowledge aids in predicting reactions and properties of aromatic compounds like anthracene, essential for advanced studies in organic chemistry.
Transcribed Image Text:**Understanding Bonding in Anthracene** **What type of hybrid orbitals are utilized by carbon in anthracene?** [Text Box for Answer] --- **How many σ bonds and π bonds are there in an anthracene molecule?** - **σ bonds:** [Text Box for Answer] - **π bonds:** [Text Box for Answer] --- **How many valence electrons occupy σ-bond orbitals, and how many occupy π-bond orbitals?** [Text Box for Answer] --- **Explanation** In the study of organic chemistry, understanding the types of bonds and hybridization present in molecules like anthracene is crucial. Anthracene, a polycyclic aromatic hydrocarbon, consists of three fused benzene rings. This structure is vital for determining the hybridization and bonding characteristics of the carbon atoms within the molecule. 1. **Hybridization**: The carbon atoms in anthracene typically utilize sp² hybrid orbitals. These orbitals form the framework for the σ bonds in the molecule, connecting carbon atoms and maintaining the structural integrity of the rings. 2. **σ bonds and π bonds**: In anthracene, σ bonds are formed through the overlap of sp² hybrid orbitals. Additionally, π bonds are formed from the side-by-side overlap of unhybridized p orbitals, contributing to the molecule’s aromaticity. 3. **Valence Electrons**: Understanding the electron distribution in σ and π bonds is key to grasping the molecule’s chemical properties. Typically, each σ bond accommodates two electrons, and π bonds also contain electrons that are delocalized across the molecule, crucial for the stability of the aromatic system. This foundational knowledge aids in predicting reactions and properties of aromatic compounds like anthracene, essential for advanced studies in organic chemistry.
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