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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

The cations O2+ and N2+ are formed when molecules of O2 and N2 are subjected to intense, high-energy solar radiation in Earth’s upper atmosphere. Write the electron configuration for O2+. Predict its bond order and magnetic behavior.

Interpretation Introduction

Interpretation:

The electronic configuration for O2+ has to be written, its bond order and magnetic behavior should be predicted.

Concept Introduction:

Molecular orbital (MO) theory:  is a method for determining molecular structure in which electrons are not assigned to individual bonds between atoms, but are treated as moving under the influence of the nuclei in the whole molecule.

Bond order: The bond order has defined as the net number of bonding electrons pairs linking a pair of atoms. This same concept can be applied directly to molecular orbital theory, but not bond order is defined as.

Bondorder=12(NumberofelectronsinbondoingMOs-NumberofelectronsinantibondingMOs)

Paramagnetic: The Paramagnetic properties are due to the presence of some unpaired electrons, and from the realignment of the electron paths caused by the external magnetic field.

Diamagnetic properties: In diamagnetic materials all the electron are paired so there is no permanent net magnetic moment per atom.

Explanation

The Oxygen (O2+) ion has eight, three electrons for (σ2s)2(σ*2s)2(σ2p)2 ( π2p)4( π*2p)1 each from the respective shells one for the negative charge anti-bonding electrons, ( π*2p)1 these electronic configuration methods shown below.

Atomicnumber of Oxygen (O)  = 8Numberofelectronsin O2molecule=16In O2+oneelectronwillbereducedfrom16electronsinO2moleculeTheelectronicconfigurationofO2+is, (σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2pz)2 ( π2px2=π2py2)( π*

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