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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Answered: Use the molecular orbital model to…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Use the molecular orbital model to fully describe the bonding in O₂⁺, O₂, O₂^-, and O₂^2-.
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 (σ_2s)²(σ_2s*)²(σ_2p)²(π_2p)⁴(π_2p*)¹.
The electron configuration of O₂^- is (σ_2s)²(σ_2s*)²(σ_2p)²(π_2p)⁴(π_2p*)³.
The bond order in O₂^- and O₂^2- is, respectively, 2.5 and 1.
The bond lengths increase in the order: O₂^2- < O₂^- < O₂ < O₂⁺.

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