Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
bartleby

Concept explainers

bartleby

Videos

Textbook Question
Book Icon
Chapter 9, Problem 26PS

Consider the following list of small molecules and ions: C2 O2, CN, O2. CO, NO, NO+, C22, OF. Identify

(a) all species that have a bond order of 3

(b) all species that are paramagnetic

(c) species that have a fractional bond order

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

All the species which have a bond order of 3 should be identified from the given list of molecules. 

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: It is the measure of number of electron pairs shared between two atoms.

Bondorder=12(NumberofelectronsinbondoingMOs-NumberofelectronsinantibondingMOs)

Answer to Problem 26PS

The species which have a bond order of 3 are,

CN-,CO,NO+andC22-

Explanation of Solution

The list of given molecules and their electronic configuration in MO term and bond order are given below,

MoleculeNo.ofelectronsElectronconfigurationBondorder=12(NbNa)C212(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4842=1O217(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)3 1072=1.5CN14(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3O216(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)2 1062=2CO14(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3NO15(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)11052=2.5NO+14(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3C2214(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3OF18(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)41082=1NbNumberofbondingelectrons,NaNumberofantibondingelectrons

According to the above table it is clear that there are four molecules have a bond order of 3. And they are mentioned below,

CN-,CO,NO+andC22-

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

All the species which are paramagnetic should be identified from the given list of molecules. 

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: It is the measure of number of electron pairs shared between two atoms.

Bondorder=12(NumberofelectronsinbondoingMOs-NumberofelectronsinantibondingMOs)

Atoms with unpaired electrons are called Paramagnetic. Paramagnetic atoms are attracted to a magnet.

Atoms with paired electrons are called diamagnetic. Diamagnetic atoms are repelled by  a magnet

Answer to Problem 26PS

The species which have paramagnetic nature are,

O2-andNO

Explanation of Solution

The list of given molecules and their electronic configuration in MO term and bond order are given below,

MoleculeNo.ofelectronsElectronconfigurationBondorder=12(NbNa)C212(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4842=1O217(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)3 1072=1.5CN14(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3O216(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)2 1062=2CO14(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3NO15(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)11052=2.5NO+14(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3C2214(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3OF18(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)41082=1NbNumberofbondingelectrons,NaNumberofantibondingelectrons

Molecules with fractional bond order value will show paramagnetic character. The fractional values are the result of odd number of electrons and odd number of electrons shows the presence of un-paired electrons.

According to the above table it is clear that there are two molecules have fractional bond order; they will exhibit paramagnetic character.

The species which have paramagnetic nature are,

O2-andNO

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

All the species which have fractional bond order should be identified from the given list of molecules. 

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: It is the measure of number of electron pairs shared between two atoms.

Bondorder=12(NumberofelectronsinbondoingMOs-NumberofelectronsinantibondingMOs)

Answer to Problem 26PS

The species which have fractional bond order are,

O2-andNO

Explanation of Solution

The list of given molecules and their electronic configuration in MO term and bond order are given below,

MoleculeNo.ofelectronsElectronconfigurationBondorder=12(NbNa)C212(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4842=1O217(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)3 1072=1.5CN14(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3O216(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)2 1062=2CO14(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3NO15(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)11052=2.5NO+14(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3C2214(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2( π2p)4(σ2p)21042=3OF18(σ1s)2(σ*1s)2(σ2s)2(σ*2s)2(σ2p)2( π2p)4( π*2p)41082=1NbNumberofbondingelectrons,NaNumberofantibondingelectrons

According to the above table it is clear that there are two molecules have a fractional bond order. And they are mentioned below,

O2-andNO

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!
Students have asked these similar questions
If an electron is removed from a fluorine molecule, an F+2molecular ion forms.(a) Give the molecular electron configurations for F2 and F+2 (for the MOs constructed from valence AOs).(b) Give the bond order of each species.(c) Predict which species should be paramagnetic.(d) Predict which species has the greater bond dissociation energy.
The molecular orbitals depicted below are derived from 2p atomic orbitals in F₂⁺. (a) Give the orbital designations. (b) Which is occupied by at least one electron in F₂⁺? (c) Which is occupied by only one electron in F₂⁺?
The nitrosyl ion. NO+, has an interesting chemistry. (a) Is NO+ diamagnetic or paramagnetic? Ifparamagnetic, how many unpaired electrons does it have? (b) What is the highest-energy molecular orbital (HOMO) occupied by electrons? (c) What is the nitrogen-oxygen bond order? (d) Is the N-O bond in NO* stronger or weaker than the bond in NO?

Chapter 9 Solutions

Chemistry & Chemical Reactivity

Ch. 9.3 - The N2+ ions that are formed when electrons with...Ch. 9.3 - What is the empirical formula of Tynan purple?Ch. 9.3 - Butter yellow absorbs light with a wavelength of...Ch. 9.3 - Prob. 2.3ACPCh. 9 - Draw the Lewis structure for chloroform, CHCl3....Ch. 9 - Draw the Lewis structure for NF3. What are its...Ch. 9 - Draw the Lewis structure for hydroxylamine, H2NOH....Ch. 9 - Draw the Lewis structure for 1,...Ch. 9 - Draw the Lewis structure for carbonyl fluoride,...Ch. 9 - Draw the Lewis structure for acetamide, CH3CONH2....Ch. 9 - Specify the electron-pair and molecular geometry...Ch. 9 - Specify the electron-pair and molecular geometry...Ch. 9 - Prob. 9PSCh. 9 - What is the hybrid orbital set used by each of the...Ch. 9 - Draw the Lewis structures of the acid HPO2F2 and...Ch. 9 - Draw the Lewis structures of the arid HSO3F and...Ch. 9 - What is the hybridization of the carbon atom in...Ch. 9 - What is the hybridization of the carbon atoms in...Ch. 9 - What is the electron-pair and molecular geometry...Ch. 9 - What is the electron-pair and molecular geometry...Ch. 9 - Prob. 17PSCh. 9 - For each compound below, decide whether cis and...Ch. 9 - Molecular Orbital Theory (See Examples 9.49.6.)...Ch. 9 - Give the electron configurations for the ions Li2+...Ch. 9 - Calcium carbide, CaC2, contains the acetylide ion,...Ch. 9 - Platinum hexafluoride is an extremely strong...Ch. 9 - When sodium and oxygen react, one of the products...Ch. 9 - When potassium and oxygen react, one of the...Ch. 9 - Among the following, which has the shortest bond...Ch. 9 - Consider the following list of small molecules and...Ch. 9 - Prob. 27PSCh. 9 - The nitrosyl ion. NO+, has an interesting...Ch. 9 - These questions are not designated as to type or...Ch. 9 - What is the OSO angle and the hybrid orbital set...Ch. 9 - Sketch the resonance structures for the nitrite...Ch. 9 - Sketch the resonance structures for the nitrate...Ch. 9 - Sketch the resonance structures for the N2O...Ch. 9 - Compare the structure and bonding in CO2 and CO32...Ch. 9 - Numerous molecules are detected in deep space....Ch. 9 - Acrolein, a component of photochemical smog, has a...Ch. 9 - The organic compound below is a member of a class...Ch. 9 - The compound sketched below is acetylsalicylic...Ch. 9 - Phosphoserine is a less-common amino acid. (a)...Ch. 9 - Lactic acid is a natural compound found in sour...Ch. 9 - Cinnamaldehyde ocaus naturally in cinnamon oil....Ch. 9 - The ion Si2 was reported in a laboratory...Ch. 9 - The simple valence bond picture of O2 does not...Ch. 9 - Nitrogen, N2, can ionize to form N2+ or add an...Ch. 9 - Which of the homonuclear, diatomic molecules of...Ch. 9 - Which of the following molecules or ions are...Ch. 9 - Prob. 47GQCh. 9 - The structure of amphetamine, a stimulant, is...Ch. 9 - Menthol is used in soaps, perfumes, and foods. It...Ch. 9 - Prob. 50GQCh. 9 - Suppose you carry out the following reaction of...Ch. 9 - Ethylene oxide is an intermediate in the...Ch. 9 - The sulfamate ion, H2NSO3, can be thought of as...Ch. 9 - The compound whose structure is shown here is...Ch. 9 - Prob. 55ILCh. 9 - Carbon dioxide (CO2), dinitrogen monoxide (N2O),...Ch. 9 - Draw the two resonance structures that describe...Ch. 9 - Draw a Lewis structure for diimide, HNNH. Then,...Ch. 9 - Prob. 59SCQCh. 9 - Consider the three fluorides BF4, SiF4, and SF4....Ch. 9 - When two amino acids react with each other, they...Ch. 9 - What is the connection between bond order, bond...Ch. 9 - When is it desirable to use MO theory rather than...Ch. 9 - Show how valence bond theory and molecular orbital...Ch. 9 - Three of the four molecular orbitals for...Ch. 9 - Lets look more closely at the process of...Ch. 9 - Borax has the molecular formula Na2B4O5(OH)4. The...Ch. 9 - A model of the organic compound allene is shown...Ch. 9 - Prob. 69SCQCh. 9 - Prob. 70SCQCh. 9 - Bromine forms a number of oxides of varying...Ch. 9 - Prob. 72SCQCh. 9 - Urea reacts with malonic acid to produce...
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
SEE MORE QUESTIONS
Recommended textbooks for you
  • Text book image
    Chemistry & Chemical Reactivity
    Chemistry
    ISBN:9781133949640
    Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
    Publisher:Cengage Learning
    Text book image
    General Chemistry - Standalone book (MindTap Cour...
    Chemistry
    ISBN:9781305580343
    Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
    Publisher:Cengage Learning
    Text book image
    Chemistry: Principles and Reactions
    Chemistry
    ISBN:9781305079373
    Author:William L. Masterton, Cecile N. Hurley
    Publisher:Cengage Learning
  • Text book image
    Chemistry: Principles and Practice
    Chemistry
    ISBN:9780534420123
    Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
    Publisher:Cengage Learning
    Text book image
    Chemistry
    Chemistry
    ISBN:9781133611097
    Author:Steven S. Zumdahl
    Publisher:Cengage Learning
    Text book image
    Chemistry
    Chemistry
    ISBN:9781305957404
    Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
Text book image
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Text book image
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY