Skip to main content
Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 69
Chapter 10, Problem 69

Sketch the bonding molecular orbital that results from the linear combination of two 1s orbitals. Indicate the region where interference occurs and state the kind of interference (constructive or destructive).

Verified step by step guidance
1
Identify the two 1s atomic orbitals that will combine. Each 1s orbital is spherically symmetrical around the nucleus of an atom.
Understand that when these orbitals overlap, they can do so in two ways: constructively (in-phase combination) or destructively (out-of-phase combination).
For constructive interference, the wave functions of the two 1s orbitals add together, leading to an increase in electron density between the nuclei. This is the bonding molecular orbital.
Sketch the bonding molecular orbital: Draw two overlapping circles (representing the 1s orbitals) with the overlap area shaded more heavily to indicate increased electron density.
Indicate the region of constructive interference, which is the area where the two orbitals overlap. Label this region as the area of constructive interference, which is responsible for the bonding character of the molecular orbital.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1m
Was this helpful?

Key Concepts

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

Molecular Orbital Theory

Molecular Orbital Theory describes how atomic orbitals combine to form molecular orbitals, which can be occupied by electrons in a molecule. When two atomic orbitals, such as 1s orbitals from two hydrogen atoms, combine, they can form two types of molecular orbitals: bonding and antibonding. The bonding molecular orbital is lower in energy and stabilizes the molecule, while the antibonding orbital is higher in energy and can destabilize it.
Recommended video:
Guided course
03:06
Molecular Orbital Theory

Linear Combination of Atomic Orbitals (LCAO)

The Linear Combination of Atomic Orbitals (LCAO) is a method used to construct molecular orbitals by combining the wave functions of atomic orbitals. In the case of two 1s orbitals, the LCAO results in a bonding molecular orbital formed by the addition of the two wave functions, leading to a region of increased electron density between the nuclei. This combination can also produce an antibonding orbital through subtraction of the wave functions.

Interference of Waves

Interference of waves occurs when two or more wave functions overlap, leading to regions of constructive or destructive interference. Constructive interference happens when wave peaks align, resulting in increased amplitude, while destructive interference occurs when a peak aligns with a trough, leading to reduced amplitude. In the context of molecular orbitals, constructive interference in the bonding orbital enhances electron density between the nuclei, while destructive interference in the antibonding orbital reduces it.
Recommended video:
Guided course
03:37
Electromagnetic Waves
Related Practice
Textbook Question

Sketch the bonding and antibonding molecular orbitals that result from linear combinations of the 2pz atomic orbitals in a homonuclear diatomic molecule. (The 2pz orbitals are those whose lobes are oriented perpendicular to the bonding axis.) How do these molecular orbitals differ from those obtained from linear combinations of the 2py atomic orbitals? (The 2py orbitals are also oriented perpendicular to the bonding axis, but also perpendicular to the 2pz orbitals.)

817
views
Textbook Question

Consider the structure of the amino acid aspartic acid. Indicate the hybridization about each interior atom.

1328
views
Textbook Question

Draw an MO energy diagram and predict the bond order of Li2+ and Li2-. Do you expect these molecules to exist in the gas phase?

2618
views
Textbook Question

Draw an MO energy diagram and predict the bond order of Be2+ and Be2- . Do you expect these molecules to exist in the gas phase?

3726
views
1
comments
Textbook Question

Write a hybridization and bonding scheme for each molecule that contains more than one interior atom. Indicate the hybridization about each interior atom. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. N2H2 (skeletal structure HNNH) b. N2H4 (skeletal structure H2NNH2) c. CH3NH2 (skeletal structure H3CNH2)

Textbook Question

Write a hybridization and bonding scheme for each molecule that contains more than one interior atom. Indicate the hybridization about each interior atom. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. c. C2H6 (skeletal structure H3CCH3)

1291
views