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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

Molecular Orbital Theory

(See Examples 9.4–9.6.)

The hydrogen molecular ion, H2+, can be detected spectroscopically. Write the electron configuration of the ion in molecular orbital terms. What is the bond order of the ion? Is the hydrogen–hydrogen bond stronger or weaker in H2+ than in H2s?

Interpretation Introduction

Interpretation:

The electron configuration of H2+ ion in molecular orbital term should be written, its bond order has to calculated and it should be determined that whether the hydrogen-hydrogen bond stronger or weaker in H2+ than in H2.

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)

Explanation

The (H2) molecule has two electrons from the hydrogen atoms. Its electronic configuration in molecular orbital term is σ1s2.

  (Antibondingelectrons)(σ*1s)01s1s(Bondingelectrons)(σ1s)2Molecularorbrbitalenergydiagramfor(H2)atoms

Bond order of H2 molecule can be calculated as,

Bondorder=12(NumberofelectronsinbondoingMOs-NumberofelectronsinantibondingMOs)Bondorder=(20)2=22=1

H2+ ion has only one electron then its electronic configuration in MO term is σ1s1

  

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