Inorganic Chemistry
5th Edition
ISBN: 9780321811059
Author: Gary L. Miessler, Paul J. Fischer, Donald A. Tarr
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Question
Chapter 5, Problem 5.23P
Interpretation Introduction
Interpretation : The relative importance of S and N orbitals in the molecular orbitals of thiocyanate ion should be discussed.
Concept Introduction : Molecular orbital theory describes the electronic structure of molecules using
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
The existence of compounds of the noble gases was once a great surprise and stimulated a great deal of theoretical work. Sketch the molecular orbital energy level diagram for XeF and deduce its ground-state electron configurations. Is XeF likely to have a shorter or longer bond than XeF+?
Relate the energies of the orbitals found (these we will use for building Molecular Orbital energy level diagrams) to Z*, also known as Zeff, determined by Slater’s rules Please show calculations for the following:
H (1s electron)
He (1s electron)
Sketch the frontier orbitals of N2 and CO molecules and highlight the differences between them.
Chapter 5 Solutions
Inorganic Chemistry
Ch. 5.1 - Repeat the process in the preceding example for...Ch. 5.2 - Prob. 5.2ECh. 5.3 - Use a similar approach to the discussion of HF to...Ch. 5.4 - Sketch the energy levels and the molecular...Ch. 5.4 - Using the D2h character table shown, verify that...Ch. 5.4 - Using orbital potential energies, show that group...Ch. 5.4 - Prob. 5.7ECh. 5.4 - Prob. 5.8ECh. 5.4 - Prob. 5.9ECh. 5.4 - Use the projection operator method to derive...
Ch. 5.4 - Determine the types of hybrid orbitals that are...Ch. 5.4 - Determine the reducible representation for all the...Ch. 5 - Expand the list of orbitais considered in Figures...Ch. 5 - On the basis of molecular orbitals, predict the...Ch. 5 - On the basis of molecular orbitals, predict the...Ch. 5 - Compare the bonding in O22,O2 and O2 Include Lewis...Ch. 5 - Although the peroxide ion, O22 and the acetylide...Ch. 5 - High-resolution photoelectron spectroscopy has...Ch. 5 - a. Prepare a molecular orbital energy-level...Ch. 5 - a. Prepare a molecular orbital energy-level...Ch. 5 - NF is a known molecule a. Construct a molecular...Ch. 5 - The hypofluorite ion, OF can be observed only with...Ch. 5 - Prob. 5.11PCh. 5 - Although KrF+ and XeF+ have been studied, KrBr+...Ch. 5 - Prepare a molecular orbital energy level diagram...Ch. 5 - Methylene, CH2 plays an important role in many...Ch. 5 - Beryllium hydride, BeH2 is linear in the gas...Ch. 5 - In the gas phase, BeF2 forms linear monomeric...Ch. 5 - For the compound XeF2 do the following: a. Sketch...Ch. 5 - TaH5 has been predicted to have C4v symmetry, with...Ch. 5 - Describe the bonding in ozone, o3 on the basis of...Ch. 5 - Describe the bonding in SO3 by using group theory...Ch. 5 - The ion H3+ has been observed, but its structure...Ch. 5 - Use molecular orbital arguments to explain the...Ch. 5 - Prob. 5.23PCh. 5 - Prob. 5.24PCh. 5 - The isomenc ions NSO (thiazate) and SNO...Ch. 5 - Apply the projection operator method to derive the...Ch. 5 - Apply the projection operator method to derive the...Ch. 5 - A set of four group orbitals derived from four 3s...Ch. 5 - The projection operator method has applications...Ch. 5 - Although the cl2+ ion has not been isolated, it...Ch. 5 - BF3 is often described as a molecule in which...Ch. 5 - SF4 has C2v symmetry. Predict the possible...Ch. 5 - Consider a square pyramidal AB5 molecule. Using...Ch. 5 - Prob. 5.34PCh. 5 - For the molecule PCl5 : a. Using the character...Ch. 5 - Molecular modeling software is typically capable...Ch. 5 - Prob. 5.39PCh. 5 - Calculate and display the orbitals for the linear...Ch. 5 - Prob. 5.41PCh. 5 - Prob. 5.42PCh. 5 - Prob. 5.43PCh. 5 - Diborane, B2H6 , has the structure shown. a. Using...
Knowledge Booster
Similar questions
- The ionosphere lies about 100 km above Earth’s surface.This layer consists mostly of NO, O₂, and N₂, and photoioniza-tion creates NO⁺, O₂⁺, and N₂⁺. (a) Use MO theory to compare the bond orders of the molecules and ions. (b) Does the magnetic behavior of each species change when its ion forms?arrow_forwardSulfur forms oxides, oxoanions, and halides. What is the hy-bridization of the central S in SO₂, SO₃, SO₃²⁻, SCl₄, SCl₆, and S₂Cl₂(atom sequence Cl—S—S—Cl)?arrow_forward(a) Sketch the occupied MOs of the valence shell for the N2 molecule. Label the orbitals as o or ™ orbitals, and specify which are bonding and which are antibonding. (b) If one electron is removed from the highest occupied orbital of N2, will the equilibrium N-N distance become longer or shorter? Explain briefly.arrow_forward
- The diatomic molecule OH exists in the gas phase. OH playsan important part in combustion reactions and is a reactiveoxidizing agent in polluted air. The bond length and bondenergy have been measured to be 97.06 pm and 424.7 kJ/mol,respectively. Assume that the OH molecule is analogous to theHF molecule discussed in the chapter and that the MOs resultfrom the overlap of a pz orbital from oxygen and the 1s orbitalof hydrogen (the OOH bond lies along the z axis).arrow_forwardThe existence of compounds of the noble gases was once a great surprise and stimulated a great deal of theoretical work. Sketch the molecular orbital energy level diagram for XeF and deduce its ground state electron configurations. Is XeF likely to have a shorter bond length than XeF+?arrow_forwardDraw the molecular orbital diagrams for Ne(2), N(2) ^2- and Be(2). Are they stable or unstable?arrow_forward
- The reaction H2C=CH2 + H2 → CH3CH3 occurs more easily in metal catalysis. Explain the reason according to MOT by showing the orbital overlaps.arrow_forwardWhich statement about the charge-minimized Lewis structure of the thiocyanate anion (SCN) is true? (Charges not shown in the Lewis structure.) The central carbon atom has a positive charge in the Lewis structure. The central carbon is sp2-hybridized. There is one formal negative charge. There are two n-bonds oriented at 180° to one another.arrow_forward5. (1) Describe the difference of hybrid orbitals such as sp, sp? and sp3. (2) Why diamond and the lead of a pencil show different electrical properties with same composition by carbon atom?.arrow_forward
- 1A2: Define electron pair domain (EPD), count EPDS on building blocks, and use EPD knowledge to determine 3D geometry and bond angles of a tetrahedral, trigonal planar, linear building block. For the indicated atoms (look for the arrows) in each of the given structures: (a) state how many EPDs are present; (b) Label tetrahedral atoms with "TET," trigonal planar atoms with "TP," and linear atoms with "LIN;" (c) Identify one (1) indicated atom in each structure for which resonance structures bring a change in the number of EPDs from 4++3/3+4 or 3+2/2+3. A resonance structure must be reported to justify your reported EPD changes. H₂C CH3 --С HO 1 Br -CH3 CH3 CI H₂C N CH3 CH3 он оarrow_forwardEstimate the orbital energies to use in a calculation of the molecular orbitals of HCl. For data, see Tables 8B.4 and 8B.5. Take β = −1.00 eV.arrow_forwardWhat is the molecular geometry of the PF4^+ (15P & 9F). Explain your answer brieflyarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
General 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 Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
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
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning