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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 N2+ ions that are formed when electrons with ionization energies of 15.6 eV and 16.7 eV are ejected have longer bond lengths than the ion when an electron with an ionization energy of 18.6 eV is created. Why?

Interpretation Introduction

Interpretation:

The N2+ ions that are formed when electrons with ionization energies of 15.6eV and 16.7eV are ejected have longer bond lengths than the ion when an electron with ionization energy of 18.6eV created. The reason behind this should be given.

Concept Introduction:   

The key to understanding PES is that all of the ejected electrons results from bombarding the atom with photons of the same energy (hν). The energy goes into ejecting the electrons from the atom corresponding to the ionization energy (IE) of the electron with the remainder going into kinetic energy of the electron. The formula of photoelectron spectroscopy hv= IE + KE (electron)

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.

Bonding molecular orbitals are a type of molecular orbitals that are involved in the formation of a chemical bond.

Antibonding molecular orbitals are orbitals containing electrons outside the region between two atomic nuclei.

Explanation

Molecular orbital correlation for Nitrogen molecule

σ*2p(Antibondingelectrons)π*2pπ*2p2px2py2pz2px2py2pzσ2pȀ

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