Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 70b

Chapter 9, Problem 70b

(b) If you combine two atomic orbitals on one atom to make a new orbital, is this a hybrid orbital or a molecular orbital?

Verified step by step guidance

Understand the concept of atomic orbitals: Atomic orbitals are regions in an atom where there is a high probability of finding electrons. They are described by quantum numbers and can be s, p, d, or f orbitals.

Learn about hybrid orbitals: Hybrid orbitals are formed when atomic orbitals on the same atom mix to form new orbitals. This process is called hybridization, and it typically occurs in covalent bonding to allow atoms to form more stable bonds.

Differentiate between hybrid orbitals and molecular orbitals: Hybrid orbitals are formed from atomic orbitals on the same atom, while molecular orbitals are formed from atomic orbitals on different atoms when they combine during the formation of a molecule.

Apply the concept to the problem: Since the problem involves combining two atomic orbitals on one atom, this process is related to hybridization, resulting in hybrid orbitals.

Conclude the explanation: The combination of two atomic orbitals on one atom to make a new orbital results in a hybrid orbital, not a molecular orbital.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Hybrid Orbitals

Hybrid orbitals are formed when atomic orbitals on the same atom combine to create new orbitals that are degenerate in energy and have different shapes. This process allows for the formation of bonds that are more effective in terms of geometry and energy, such as in sp, sp2, or sp3 hybridization. Hybridization is crucial for understanding molecular geometry and bonding in covalent compounds.

Molecular Orbitals

Molecular orbitals are formed when atomic orbitals from different atoms combine to create new orbitals that belong to the entire molecule rather than to individual atoms. This concept is central to molecular orbital theory, which explains the bonding and electronic structure of molecules. Molecular orbitals can be bonding, antibonding, or non-bonding, influencing the stability and reactivity of the molecule.

Atomic Orbitals

Atomic orbitals are regions in an atom where there is a high probability of finding electrons. They are defined by quantum numbers and include s, p, d, and f types, each with distinct shapes and energy levels. Understanding atomic orbitals is essential for grasping how they can combine to form hybrid or molecular orbitals, which are fundamental to chemical bonding.

Related Practice

Textbook Question

(a) If you combine two atomic orbitals on two different atomsto make a new orbital, is this a hybrid orbital or a molecularorbital?

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⁺?

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Textbook Question

Consider the H₂⁺ ion. (e) Suppose that the ion is excited by light so that an electron moves from a lower-energy to a higher-energy MO. Would you expect the excited-state H₂⁺ ion to be stable or to fall apart?

Consider the H₂⁺ ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram.

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Textbook Question

Predict the molecular geometry of each of the following molecules: (b) H O C O C O O H

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