Use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-. Determine which of the following statements are true and which are false.
Use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-. Determine which of the following statements are true and which are false.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter8: Advanced Theories Of Covalent Bonding
Section: Chapter Questions
Problem 40E: Predict the valence electron molecular orbital configurations for the following, and state whether...
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Use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-.
Determine which of the following statements are true and which are false.
True or false? :
Bond length increases with increasing bond order while bond energy decreases.
The number of unpaired electrons in O2- and O2 is, respectively, 1 and 2.
The electron configuration of O2 is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)1.
The electron configuration of O2- is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)3.
The bond order in O2- and O22- is, respectively, 2.5 and 1.
The bond lengths increase in the order: O22- < O2- < O2 < O2+.
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