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Using the molecular orbital model, identify the correct (valence) electron configurations for the following diatomic species.

Using the molecular orbital model, identify the correct (valence) electron configurations for the following diatomic species.

Chemistry by OpenStax (2015-05-04)
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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Using the molecular orbital model, identify the correct (valence) electron configurations for the following diatomic species. 02 CN CN+ N₂ CN A. (02s)²(0₂s*)²(1₂)ª(0₂)²(п²*)¹ B. (02s)2(02s*)2(02p)2(n2p)4(n2p*)3 C. (02s)²(02s*)2(₂p)4(0₂p)¹ D. (02s)2(02s*)2(02p)²(n2p)4(n2p*)2 E. (02)²(02s*)2(n₂p)4 F. (02s)²(02s*)²(0₂p)²(п²p)ª(₪²p*)4 G. (02s)²(0₂s*)²(¹₂)4(0₂)²
Transcribed Image Text:Using the molecular orbital model, identify the correct (valence) electron configurations for the following diatomic species. 02 CN CN+ N₂ CN A. (02s)²(0₂s*)²(1₂)ª(0₂)²(п²*)¹ B. (02s)2(02s*)2(02p)2(n2p)4(n2p*)3 C. (02s)²(02s*)2(₂p)4(0₂p)¹ D. (02s)2(02s*)2(02p)²(n2p)4(n2p*)2 E. (02)²(02s*)2(n₂p)4 F. (02s)²(02s*)²(0₂p)²(п²p)ª(₪²p*)4 G. (02s)²(0₂s*)²(¹₂)4(0₂)²
Use the molecular orbital model to fully describe the bonding in O₂+, 0₂, 0₂¯, and 0₂²-. Determine which of the following statements are true and which are false. The electron configuration of O₂ is (02s)²(02s*)²(02p)²(1₂p) 4 (n₂p*)². ✓The bond order in O₂ and O₂2- is, respectively, 2.5 and 1. The number of unpaired electrons in O₂ and O₂ is, respectively, 1 and 0. The electron configuration of O₂¯ is (02)²(02s*)²(02p)²(12p)4(п²*)³. The bond energies increase in the order: 0₂²- < 0₂¯ < 0₂ < 0₂¹. Bond length increases with increasing bond order while bond energy decreases.
Transcribed Image Text:Use the molecular orbital model to fully describe the bonding in O₂+, 0₂, 0₂¯, and 0₂²-. Determine which of the following statements are true and which are false. The electron configuration of O₂ is (02s)²(02s*)²(02p)²(1₂p) 4 (n₂p*)². ✓The bond order in O₂ and O₂2- is, respectively, 2.5 and 1. The number of unpaired electrons in O₂ and O₂ is, respectively, 1 and 0. The electron configuration of O₂¯ is (02)²(02s*)²(02p)²(12p)4(п²*)³. The bond energies increase in the order: 0₂²- < 0₂¯ < 0₂ < 0₂¹. Bond length increases with increasing bond order while bond energy decreases.
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