Textbook Question
(b) What is the hybridization of the carbon atoms in each molecule?
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Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 60a
Benzaldehyde, C7H6O, is a fragrant substance responsible for the aroma of almonds. Its Lewis structure is
(a) What is the hybridization at each of the carbon atoms of the molecule?
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Identify the structure of benzaldehyde, C7H6O, which consists of a benzene ring attached to a formyl group (-CHO).
Examine the carbon atoms in the benzene ring. Each carbon in the benzene ring forms three sigma bonds (two with adjacent carbons and one with a hydrogen atom) and one pi bond (part of the delocalized pi system).
Determine the hybridization of the carbon atoms in the benzene ring. Since each carbon forms three sigma bonds and one pi bond, the hybridization is sp2.
Examine the carbon atom in the formyl group. This carbon forms two sigma bonds (one with the hydrogen atom and one with the oxygen atom) and one pi bond (with the oxygen atom).
Determine the hybridization of the carbon atom in the formyl group. Since this carbon forms three sigma bonds and one pi bond, the hybridization is sp2.
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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 in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals are used to form covalent bonds in molecules. The type of hybridization depends on the number of electron pairs around the central atom, influencing the geometry and bond angles of the molecule.
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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. It uses dots to represent valence electrons and lines to represent bonds. Understanding the Lewis structure of a molecule is crucial for determining its hybridization and molecular geometry.
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Valence Shell Electron Pair Repulsion (VSEPR) Theory
VSEPR theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell of the central atom. According to this theory, electron pairs will arrange themselves as far apart as possible to minimize repulsion, which helps in determining the hybridization and shape of the molecule.
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Related Practice
Textbook Question
Propylene, C3H6, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is (a) What is the total number of valence electrons in the propylene molecule?
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
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?