   Chapter 12, Problem 12.61E

Chapter
Section
Textbook Problem

Use Figure 12.23 to determine electron configurations for O 2 2 + , O 2 − , and O 2 2 − .

Interpretation Introduction

Interpretation:

The electron configurations for O22+, O2, and O22 are to be determined by using Figure 12.23.

Concept introduction:

Electronic configuration tells about the arrangement of the electrons in each subshell of an atom. The distribution of the electrons in the molecules is described by the molecular orbital theory.

Explanation

The number of electrons in O2 is 16. Thus, the molecular electronic configuration for O2 is (σg1s)2(σg*1s)2(σg2s)2(σg*2s)2(σg2pz)2(πμ2px2,πμ2py2)(πg*2px1,πg*2py1).

The given species are O22+, O2, and O22 respectively.

The number of electrons in O22+ is 14. It is formed by losing two electrons from O2. Thus, the molecular electronic configuration for O22+ is (σg1s)2(σg*1s)2(σg2s)2(σg*2s)2(σg2pz)2(πμ2px2,πμ2py2).

The number of electrons in O2 is 17. It is formed by gaining an electron by O2. Thus, the molecular electronic configurations for O2 is (σg1s)2(σg*1s)2(σg2s)2(σg*2s)2(σg2pz)2(πμ2px2,πμ2py2)(πg*2px2,πg*2py1).

The number of electrons in O22 is 18. It is formed by gaining two electrons by O2

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 