Using the molecular orbital model, identify the correct (valence) electron configurations for the following diatomic species.02CNCN+N₂CNA. (02s)²(0₂s*)²(1₂)ª(0₂)²(п²*)¹B. (02s)2(02s*)2(02p)2(n2p)4(n2p*)3C. (02s)²(02s*)2(₂p)4(0₂p)¹D. (02s)2(02s*)2(02p)²(n2p)4(n2p*)2E. (02)²(02s*)2(n₂p)4F. (02s)²(02s*)²(0₂p)²(п²p)ª(₪²p*)4G. (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.

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

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

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.

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