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What are the ideal values for the bond angles indicated on the molecule below? 1. H 2. H 3. |L | 0: H

What are the ideal values for the bond angles indicated on the molecule below? 1. H 2. H 3. |L | 0: H

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter6: Covalent Bonding
Section6.11: Aromatic Compounds
Problem 1CE
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**Question:** What are the ideal values for the bond angles indicated on the molecule below? **Diagram Explanation:** The diagram shows a structural formula of acetic acid. It features three specific bond angles marked with red arrows and labeled as 1, 2, and 3. 1. **Angle 1:** This is the bond angle between a hydrogen atom, a carbon atom (forming a single bond with another carbon atom), and another hydrogen atom. 2. **Angle 2:** This bond angle is formed between a hydrogen atom, a carbon atom (connected by a double bond to an oxygen atom), and that oxygen atom. 3. **Angle 3:** This angle involves two lone pairs on an oxygen atom and two hydrogens, one of which is bonded to the oxygen. **Note:** Determine these angles using principles of molecular geometry, such as the tetrahedral angle for single-bonded atoms and the trigonal planar angle for atoms with double bonds. Additionally, lone pairs can affect ideal geometrical angles due to repulsion effects.
Transcribed Image Text:**Question:** What are the ideal values for the bond angles indicated on the molecule below? **Diagram Explanation:** The diagram shows a structural formula of acetic acid. It features three specific bond angles marked with red arrows and labeled as 1, 2, and 3. 1. **Angle 1:** This is the bond angle between a hydrogen atom, a carbon atom (forming a single bond with another carbon atom), and another hydrogen atom. 2. **Angle 2:** This bond angle is formed between a hydrogen atom, a carbon atom (connected by a double bond to an oxygen atom), and that oxygen atom. 3. **Angle 3:** This angle involves two lone pairs on an oxygen atom and two hydrogens, one of which is bonded to the oxygen. **Note:** Determine these angles using principles of molecular geometry, such as the tetrahedral angle for single-bonded atoms and the trigonal planar angle for atoms with double bonds. Additionally, lone pairs can affect ideal geometrical angles due to repulsion effects.
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