PRINCIPLES OF MODERN CHEMISTRY
PRINCIPLES OF MODERN CHEMISTRY
8th Edition
ISBN: 9780357671009
Author: OXTOBY
Publisher: CENGAGE L
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Chapter 6, Problem 17P

a)

Interpretation Introduction

Interpretation: The molecular electronic configuration of F2 and F2+ should be determined.

Concept introduction: Two or more than two atomic orbitals overlap to form bond, these orbitals are called molecular orbitals. Count of molecular orbital obtained is same as count of atomic orbitals mixed.

Two forms of molecular orbital are obtained. These are bonding and antibonding orbital.

Bonding orbitals are those in that electrons are in between nucleus of two atom. Antibonding orbitals are those in which electrons are away from nucleus of two-atom. Also, electrons in antibonding orbital have energy high as compared to bonding orbital.

In sigma (σ) bonding orbital, electron density is shared directly between bonding atoms, along bonding axis. In sigma (σ*) antibonding orbital, the orbital is empty. In these orbital’s electrons are along nuclear axis.

In pi (π) bonding orbital, bonding electron lies above and below bonding axis and has no electron on bonding axis.

In pi (π*) antibonding orbital, the orbital is empty. In these orbital, electrons are perpendicular to nuclear axis.

b)

Interpretation Introduction

Interpretation: The bond order of F2 and F2+ should be determined.

Concept introduction: Two or more than two atomic orbitals overlap to form bond, these orbitals are called molecular orbitals. Count of molecular orbital obtained is same as count of atomic orbitals mixed.

Two forms of molecular orbital are obtained. These are bonding and antibonding orbital.

Bonding orbitals are those in that electrons are in between nucleus of two atom. Antibonding orbitals are those in which electrons are away from nucleus of two-atom. Also, electrons in antibonding orbital have energy high as compared to bonding orbital.

In sigma (σ) bonding orbital, electron density is shared directly between bonding atoms, along bonding axis. In sigma (σ*) antibonding orbital, the orbital is empty. In these orbital’s electrons are along nuclear axis.

In pi (π) bonding orbital, bonding electron lies above and below bonding axis and has no electron on bonding axis.

In pi (π*) antibonding orbital, the orbital is empty. In these orbital, electrons are perpendicular to nuclear axis.

c)

Interpretation Introduction

Interpretation: The species that is paramagnetic should be determined.

Concept introduction: Two or more than two atomic orbitals overlap to form bond, these orbitals are called molecular orbitals. Count of molecular orbital obtained is same as count of atomic orbitals mixed.

Two forms of molecular orbital are obtained. These are bonding and antibonding orbital.

Bonding orbitals are those in that electrons are in between nucleus of two atom. Antibonding orbitals are those in which electrons are away from nucleus of two-atom. Also, electrons in antibonding orbital have energy high as compared to bonding orbital.

In sigma (σ) bonding orbital, electron density is shared directly between bonding atoms, along bonding axis. In sigma (σ*) antibonding orbital, the orbital is empty. In these orbital’s electrons are along nuclear axis.

In pi (π) bonding orbital, bonding electron lies above and below bonding axis and has no electron on bonding axis.

In pi (π*) antibonding orbital, the orbital is empty. In these orbital, electrons are perpendicular to nuclear axis.

d)

Interpretation Introduction

Interpretation: The ion that has high bond dissociation energy should be determined.

Concept introduction: Two or more than two atomic orbitals overlap to form bond, these orbitals are called molecular orbitals. Count of molecular orbital obtained is same as count of atomic orbitals mixed.

Two forms of molecular orbital are obtained. These are bonding and antibonding orbital.

Bonding orbitals are those in that electrons are in between nucleus of two atom. Antibonding orbitals are those in which electrons are away from nucleus of two-atom. Also, electrons in antibonding orbital have energy high as compared to bonding orbital.

In sigma (σ) bonding orbital, electron density is shared directly between bonding atoms, along bonding axis. In sigma (σ*) antibonding orbital, the orbital is empty. In these orbital’s electrons are along nuclear axis.

In pi (π) bonding orbital, bonding electron lies above and below bonding axis and has no electron on bonding axis.

In pi (π*) antibonding orbital, the orbital is empty. In these orbital, electrons are perpendicular to nuclear axis.

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Chapter 6 Solutions

PRINCIPLES OF MODERN CHEMISTRY

Ch. 6 - Without consulting tables of data, predict which...Ch. 6 - Without consulting tables of data, predict which...Ch. 6 - Without consulting tables of data, on the same...Ch. 6 - Without consulting tables of data, on the same...Ch. 6 - Suppose we supply enough energy to H2 to remove...Ch. 6 - Suppose we supply enough energy to He2+ to remove...Ch. 6 - Prob. 17PCh. 6 - When one electron is added to an oxygen molecule,...Ch. 6 - Predict the valence electron configuration and the...Ch. 6 - Predict the valence electron configuration and the...Ch. 6 - Prob. 21PCh. 6 - For each of the following valence electron...Ch. 6 - For each of the electron configurations in Problem...Ch. 6 - For each of the electron configurations in Problem...Ch. 6 - Following the pattern of Figure 6.21, work out the...Ch. 6 - Following the pattern of Figure 6.21, work out the...Ch. 6 - The bond length of the transient diatomic molecule...Ch. 6 - The compound nitrogen oxide (NO) forms when the...Ch. 6 - What would be the electron configuration for a HeH...Ch. 6 - The molecular ion HeH+ has an equilibrium bond...Ch. 6 - Prob. 31PCh. 6 - Predict the ground state electronic configuration...Ch. 6 - The bond dissociation energies for the species NO,...Ch. 6 - The ionization energy of CO is greater than that...Ch. 6 - Photoelectron spectra were acquired from a sample...Ch. 6 - Photoelectron spectra were acquired from a sample...Ch. 6 - Prob. 37PCh. 6 - From the n=0 peaks in the photoelectron spectrum...Ch. 6 - The photoelectron spectrum of HBr has two main...Ch. 6 - The photoelectron spectrum of CO has four major...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Both the simple VB model and the LCAO method...Ch. 6 - Both the simple VB model and the LCAO method...Ch. 6 - Write simple valence bond wave functions for...Ch. 6 - Write simple valence bond wave functions for...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Formulate a localized bond picture for the amide...Ch. 6 - Formulate a localized bond picture for the...Ch. 6 - Prob. 51PCh. 6 - Draw a Lewis electron dot diagram for each of the...Ch. 6 - Describe the hybrid orbitals on the chlorine atom...Ch. 6 - Describe the hybrid orbitals on the chlorine atom...Ch. 6 - The sodium salt of the unfamiliar orthonitrate ion...Ch. 6 - Describe the hybrid orbitals used by the carbon...Ch. 6 - Describe the bonding in the bent molecule NF2 ....Ch. 6 - Describe the bonding in the bent molecule OF2 ....Ch. 6 - The azide ion (N3) is a weakly bound molecular...Ch. 6 - Formulate the MO structure of (NO2+) for localized...Ch. 6 - Discuss the nature of the bonding in the nitrite...Ch. 6 - Discuss the nature of the bonding in the nitrate...Ch. 6 - The pyridine molecule (C5H5N) is obtained by...Ch. 6 - For each of the following molecules, construct the...Ch. 6 - (a) Sketch the occupied MOs of the valence shell...Ch. 6 - Calcium carbide (CaC2) is an intermediate in the...Ch. 6 - The B2 molecule is paramagnetic; show how this...Ch. 6 - The Be2 molecule has been detected experimentally....Ch. 6 - Prob. 69APCh. 6 - The molecular ion HeH+ has an equilibrium bond...Ch. 6 - The MO of the ground state of a heteronuclear...Ch. 6 - The stable molecular ion H3+ is triangular, with...Ch. 6 - According to recent spectroscopic results,...Ch. 6 - trans-tetrazene (N4H4) consists of a chain of four...
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Quantum Molecular Orbital Theory (PChem Lecture: LCAO and gerade ungerade orbitals); Author: Prof Melko;https://www.youtube.com/watch?v=l59CGEstSGU;License: Standard YouTube License, CC-BY