Concept explainers
Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders. Which ones are paramagnetic? Place the species in order of increasing bond length and bond energy.
a. CN+
b. CN
c. CN−
(a)
Interpretation: The electronic configuration for the given diatomic species is to be determined and their bond orders have to be calculated. The paramagnetic species have to be identified. The given molecules have to be placed in the correct order of increasing bond length and bond energy.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
To determine: The electronic configuration of
Answer to Problem 56E
Answer
The configuration of
Explanation of Solution
The electronic configuration of the involved atoms is,
The number of valence electrons present in
The molecular orbital configuration of
Number of bonding electrons
Number of non-bonding electrons
Hence,
Bond order
No unpaired electron is present; hence it is a diamagnetic molecule.
(b)
Interpretation: The electronic configuration for the given diatomic species is to be determined and their bond orders have to be calculated. The paramagnetic species have to be identified. The given molecules have to be placed in the correct order of increasing bond length and bond energy.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
To determine: The electronic configuration of
Answer to Problem 56E
Answer
The configuration of
Explanation of Solution
The electronic configuration of the involved atoms is,
The number of valence electrons present in
The molecular orbital configuration of
Number of bonding electrons
Number of non-bonding electrons
Hence,
Bond order
The
(c)
Interpretation: The electronic configuration for the given diatomic species is to be determined and their bond orders have to be calculated. The paramagnetic species have to be identified. The given molecules have to be placed in the correct order of increasing bond length and bond energy.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
To determine: The electronic configuration of
Answer to Problem 56E
Answer
The configuration of
Explanation of Solution
The electronic configuration of the involved atoms is,
The number of valence electrons present in
The molecular orbital configuration of
Number of bonding electrons
Number of non-bonding electrons
Hence,
Bond order
No unpaired electron is present; hence it is a diamagnetic molecule.
The diatomic configuration of a diatomic species can be determined using the molecular orbital diagram. The difference between the bonding electrons and the non-bonding electrons divided by two gives the bond order of the molecule.
The bond order is inversely proportional to bond length. The molecule having the least bond order value has the greatest bond length.
The bond order is directly proportional to bond energy. The molecule having the least bond order value has the least bond energy.
The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
Want to see more full solutions like this?
Chapter 9 Solutions
OWLv2 with MindTap Reader, 4 terms (24 months) Printed Access Card for Zumdahl/Zumdahl/DeCoste’s Chemistry, 10th Edition
- a Carbonyl fluoride, COF2, is an extremely poisonous gas used in organofluorine synthesis. Give the valence bond description of the carbonyl fluoride molecule. (Both fluorine atoms are attached to the carbon atom.) b Nitrogen, N2, makes up about 80% of the earths atmosphere. Give the valence bond description of this molecule.arrow_forwardFClO2 and F3ClO can both gain a fluoride ion to form stable anions. F3ClO and F3ClO2 will both lose a fluoride ion to form stable cations. Draw the Lewis structures and describe the hybrid orbitals used by chlorine in these ions.arrow_forwardBest Lewis Formula and Molecular Geometry A student writes the Lewis electron-dot formula for the carbonate anion, CO32, as a Does this Lewis formula obey the octet rule? Explain. What are the formal charges on the atoms? Try describing the bonding for this formula in valence bond terms. Do you have any difficulty doing this? b Does this Lewis formula give a reasonable description of the electron structure, or is there a better one? If there is a better Lewis formula, write it down and explain why it is better. c The same student writes the following resonance description for CO2: Is there something wrong with this description? (What would you predict as the geometries of these formulas?) d Is one or the other formula a better description? Could a value for the dipole moment help you decide? e Can you write a Lewis formula that gives an even better description of CO2? Explain your answer.arrow_forward
- Predict the molecular structure (including bond angles) for each of the following. (See Exercises 115 and 116.) a. XeCl2 b. ICl3 c. TeF4 d. PCl5arrow_forwardPredict the molecular structure (including bond angles) for each of the following. (See Exercises 115 and 116.) a. ICl5 b. XeCl4 c. SeCl6arrow_forwardThe formula for nitryl chloride is ClNO2 (in which N is the central atom). (a) Draw the Lewis structure for the molecule, including all resonance structures. (b) What is the NO bond order? (c) Describe the electron-pair and molecular geometries, and give values for all bond angles. (d) What is the most polar bond in the molecule? Is the molecule polar? (e) The computer program used to calculate electrostatic potential surfaces gave the following charges on atoms in the molecule: A = 0.03, B = 0.26, and C = +0.56. Identify the atoms A, B, and C. Are these calculated charges in accord with your predictions?arrow_forward
- Which of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments? (a) CIF5 (b) CIO2 (c) TeCI42 (d) PCl3 (e) SeF4 (f) PH2 (g) XeF2arrow_forwardAmong the following, which has the shortest bond and which has the longest: Li2, B2, C2, N2, O2?arrow_forwardPredict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na,2+ (b) Mg,2 (c) AI,2 (d) Si,2 (e) p2+ (f) s,2 (g) F,2 (h) Ar,2 40. Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. (a) Na22+ (b) Mg22+ (c) Al22+ (d) Si22+ (e) P22+ (f) S22+ (g) F22+ (h) Ar22+arrow_forward
- Predict die molecular structure and bond angles for each molecule or ion in Exercises 88 and 94. a. POCl3, SO42, XeO4, PO43, ClO4 b. NF3, SO32, PO33, ClO3 c.ClO2, SCl2, PCl2 d. Considering your answers to parts a, b, and c. what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons? (O3), sulfur dioxide, and sulfur trioxide.arrow_forwardExplain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.arrow_forwardIt is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning