Textbook Question
Consider the following Lewis structure:
a. Does the Lewis structure depict a neutral molecule or an ion? If it is an ion, what is the charge on the ion?
Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 70
Which of the following statements about molecular orbitals and hybrid orbitals are true?
a. Molecular orbitals and hybrid orbitals are both created by mathematically mixing the wave functions of atomic orbitals.
b. Molecular orbitals are made by combining atomic orbitals from different atoms.
c. Hybrid orbitals and molecular orbitals are different names for the same things.
d. A hybrid orbital can hold more electrons than can a molecular orbital.
Verified step by step guidance1
Step 1: Understand the concept of molecular orbitals. Molecular orbitals are formed by the combination of atomic orbitals from different atoms, which can be bonding or antibonding.
Step 2: Understand the concept of hybrid orbitals. Hybrid orbitals are formed by the mixing of atomic orbitals from the same atom to form new orbitals that are degenerate and oriented in specific directions to form bonds.
Step 3: Evaluate statement a. Both molecular and hybrid orbitals involve the mathematical mixing of atomic orbitals, but they serve different purposes.
Step 4: Evaluate statement b. Molecular orbitals are indeed formed by combining atomic orbitals from different atoms, which is a true statement.
Step 5: Evaluate statements c and d. Hybrid orbitals and molecular orbitals are not the same, and a hybrid orbital does not hold more electrons than a molecular orbital.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Orbitals
Molecular orbitals (MOs) are formed by the linear combination of atomic orbitals (LCAO) from different atoms in a molecule. They describe the probability distribution of electrons in a molecule and can be bonding, antibonding, or non-bonding. MOs allow for the understanding of molecular stability and reactivity, as they determine how electrons are shared or distributed between atoms.
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Hybrid Orbitals
Hybrid orbitals are formed by the mixing of atomic orbitals from a single atom to create new orbitals that are degenerate in energy. This process allows for the formation of bonds with specific geometries, such as sp, sp2, or sp3 hybridization, which correspond to different molecular shapes. Hybrid orbitals are crucial for explaining the bonding in molecules with covalent bonds.
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Differences Between Molecular and Hybrid Orbitals
Molecular orbitals and hybrid orbitals serve different purposes in molecular chemistry. While molecular orbitals involve the combination of atomic orbitals from different atoms to describe electron distribution in a molecule, hybrid orbitals are concerned with the arrangement of atomic orbitals within a single atom to facilitate bonding. Understanding these distinctions is essential for analyzing molecular structure and bonding behavior.
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Related Practice
Textbook Question
Predict the molecular geometry of each of the following molecules: (b) H O C O C O O H
Textbook Question
What hybridization do you expect for the atom indicated in red in each of the following species? (a) CH3CO2-
Textbook Question
Consider the H2+ ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram.
Textbook Question
Consider the H2+ ion. (b) How many electrons are there in the H2+ ion?
Textbook Question
Consider the H2+ ion. (c) Write the electron configuration of the ion in terms of its MOs. (d) What is the bond order in H2+?