Textbook Question
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
(e) How many valence electrons remain in nonbonding pairs in the molecule?
Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 61b1
Consider the Lewis structure for acetic acid, which is known as vinegar: (b) What are the hybridizations of the orbitals on the two oxygen atoms, and what are the approximate bond angles at the oxygen that is connected to carbon and hydrogen? What are the hybridizations of the orbitals on the two oxygen atoms?
Verified step by step guidance1
Identify the two oxygen atoms in the acetic acid molecule. One oxygen atom is double bonded to a carbon atom (carbonyl group), and the other oxygen atom is single bonded to a carbon atom and also bonded to a hydrogen atom (hydroxyl group).
Determine the hybridization of the oxygen in the carbonyl group. Since it forms two sigma bonds (one with carbon and one as part of the double bond) and has two lone pairs, the hybridization is sp2.
Determine the hybridization of the oxygen in the hydroxyl group. This oxygen forms two sigma bonds (one with carbon and one with hydrogen) and has two lone pairs, leading to sp3 hybridization.
Analyze the bond angles for the oxygen in the hydroxyl group. With sp3 hybridization, the ideal bond angles are approximately 109.5 degrees, but due to the presence of the double bond in the molecule, there might be slight deviations from this ideal angle.
Summarize the findings: The oxygen in the carbonyl group is sp2 hybridized with bond angles approximately 120 degrees around it, while the oxygen in the hydroxyl group is sp3 hybridized with bond angles close to 109.5 degrees.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals are used to explain the geometry of molecular bonding. In acetic acid, the oxygen atoms undergo hybridization to form sp2 and sp3 hybrid orbitals, which influence the molecular shape and bond angles.
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Hybridization
Bond Angles
Bond angles are the angles formed between two bonds that share a common atom, which are crucial for determining the geometry of a molecule. In acetic acid, the bond angles around the oxygen atoms are influenced by their hybridization. The sp2 hybridized oxygen has bond angles close to 120 degrees, while the sp3 hybridized oxygen has bond angles close to 109.5 degrees.
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Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They provide a visual representation of the arrangement of electrons and help predict molecular geometry and reactivity. For acetic acid, the Lewis structure illustrates the connectivity of carbon, hydrogen, and oxygen atoms, which is essential for understanding hybridization and bond angles.
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Related Practice
Textbook Question
Consider the Lewis structure for acetic acid, which is known as vinegar:
(a) What are the approximate bond angles about each of the two carbon atoms, and what are the hybridizations of the orbitals on each of them?
Textbook Question
Consider the Lewis structure for glycine, the simplest amino acid:
(b) What are the hybridizations of the orbitals on the two oxygens and the nitrogen atom, and what are the approximate bond angles at the nitrogen?
Textbook Question
Consider the Lewis structure for glycine, the simplest amino acid:
(c) What is the total number of s bonds in the entire molecule, and what is the total number of p bonds?
Textbook Question
(c) Is the p bond in NO2- localized or delocalized?
Textbook Question
(a) Write a single Lewis structure for N2O, and determine the hybridization of the central N atom.