Textbook Question
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
a. What is the hybridization at each of the carbon atoms of the molecule?
Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 61a
Glycine, the simplest amino acid, has the following Lewis structure:
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?
Verified step by step guidance1
Identify the structure of glycine and locate the two carbon atoms in the molecule.
For the first carbon atom (the one bonded to the amino group), recognize that it is bonded to four groups: the amino group (NH2), a hydrogen atom, the carboxyl group (COOH), and the second carbon atom. This indicates a tetrahedral geometry.
Determine the hybridization of the first carbon atom. Since it has a tetrahedral geometry, the hybridization is sp^3, and the bond angles are approximately 109.5°.
For the second carbon atom (the one in the carboxyl group), note that it is bonded to three groups: the first carbon atom, an oxygen atom (double bond), and another oxygen atom (single bond). This suggests a trigonal planar geometry.
Determine the hybridization of the second carbon atom. With a trigonal planar geometry, the hybridization is sp^2, and the bond angles are approximately 120°.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of atoms in a molecule. In glycine, the carbon atoms undergo hybridization to form sp3 hybrid orbitals, which allows for the formation of four sigma bonds, leading to a tetrahedral geometry around each carbon.
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Hybridization
Bond Angles
Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the hybridization of the central atom. In glycine, the bond angles around the sp3 hybridized carbon atoms are approximately 109.5 degrees, characteristic of a tetrahedral arrangement, although slight deviations may occur due to steric effects from surrounding groups.
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Lewis Structure
A Lewis structure is a diagram that represents the bonding between atoms in a molecule and the lone pairs of electrons that may exist. For glycine, the Lewis structure helps visualize the arrangement of atoms, the types of bonds (single or double), and the overall connectivity, which is essential for determining hybridization and bond angles.
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Related Practice
Textbook Question
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
(c) How many of the valence electrons are used to make s bonds in the molecule?
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?
Textbook Question
Glycine, the simplest amino acid, has the following Lewis structure:
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
Glycine, the simplest amino acid, has the following Lewis structure:
c. What is the total number of 𝜎 bonds in the entire molecule, and what is the total number of 𝜋 bonds?
Textbook Question
d. Would you expect SO3 to exhibit delocalized 𝜋 bonding?