2. Consider a hypothetical trigonal bipyramidal Fe(III) complex [FeF2(OH)3]². We need to divide the five donor atoms of the ligands into two groups: 2F and 30. F HO FeOH F OH (a) Identify the point group of the complex and assign x, y, and z to it. (b) Indicate the symmetries of the Fe valence orbitals, i.e., 3d, 4s, and 4p. (c) Derive the symmetries and expressions of the two F σ-SALCs, considering that each F. atom contributes one 2p orbital with a lone pair to form the σ-SALCs. (d) Derive the symmetries and expressions of the three σ-SALCs on the OH ligands, considering that each O atom contributes one 2p orbital with a lone pair to form the σ- SALCs. (e) Draw a σ bonding-only MO energy level diagram for the complex, mark the MOs with symmetry labels, and fill the MOS with the valence electrons. (f) Consider each O atom contributing one perpendicular 2p orbital to form π-SALCs. Derive the symmetries of the three л-SALCS. (g) Identify the MOs in (e) with which the O л-SALCs interact, and discuss the effect of these interactions.

2. Consider a hypothetical trigonal bipyramidal Fe(III) complex [FeF2(OH)3]². We need to divide the five donor atoms of the ligands into two groups: 2F and 30. F HO FeOH F OH (a) Identify the point group of the complex and assign x, y, and z to it. (b) Indicate the symmetries of the Fe valence orbitals, i.e., 3d, 4s, and 4p. (c) Derive the symmetries and expressions of the two F σ-SALCs, considering that each F. atom contributes one 2p orbital with a lone pair to form the σ-SALCs. (d) Derive the symmetries and expressions of the three σ-SALCs on the OH ligands, considering that each O atom contributes one 2p orbital with a lone pair to form the σ- SALCs. (e) Draw a σ bonding-only MO energy level diagram for the complex, mark the MOs with symmetry labels, and fill the MOS with the valence electrons. (f) Consider each O atom contributing one perpendicular 2p orbital to form π-SALCs. Derive the symmetries of the three л-SALCS. (g) Identify the MOs in (e) with which the O л-SALCs interact, and discuss the effect of these interactions.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Isn't An electron-rich transition metal has a low oxidation state, meaning that the metal centre has gained electrons from the nitrogen on NO when it coordinates as a ligand? Therefore, N-O bond length decases.
Draw the crystal field diagram of [W(CO)6]. Determine the (a) Electronic configuration in terms t2geg (b) Number of unpaired electrons (c) Ligand field stabilization energy in terms of ΔO or ΔT
Consider the complex square planar complex NiL4, where Ni2+ (d) is the central ion. Draw the system showing axes and answer the following: 1) Show how Group theory to find symmetries for Sigma bonding 2) Show how Group theory can find symmetries for in- plane and out of plane Pi bonds 3) Use the Projection Operator Method to find out LGOs (all of them) used in the out of plane Pi bonding
!5
In the following list, identify a transition metal cation that cannot be used to distinguish between strong-field and weak-field ligands in octahedral complexes? (A) Cr3+ (B) Fe3+ (C) Co3+ (D) None of them (any of them can be used)
a) Provide the name of the coordination complex Na[COCI,(NH3),] b) Calculate the orbital multiplicity for a Cr** assuming it is a free ion (Not complex). c) Calculate the spin multiplicity of a metal ion Cr* assuming a high spin crystal field. d) Calculate the quantum number S for metal ion Cr 3* assuming a high spin crystal field splitting.
Consider the octahedral complex [FeBr6] 4−. In water solution it has an absorption peak at 864 nm with a molar absorptivity (ε) of 3.6 L mol-1 cm-1 . (I have a, b, and c, I need help with d, e, and f.) (a) What is the energy (in wavenumbers, cm-1 ) of the absorption peak? Show all work. (b) How many valence d electrons does the metal center have? Justify your answer. (c) How many unpaired electrons per molecule would a magnetic susceptibility experiment predict? What would the S number be for this transition metal center? Justify your answers. (d) What electronic transition results from absorption of 864-nm light? (e) Calculate the ligand stabilization energy (in units of ∆o) and units of coulombic (Πc) energy. (f) How would the ligand field strengths (∆o) of [Fe(NH3)6] 2+ and [Fe(bipy)3] 2+ differ from that of [FeBr6] 4−? Why?
(a) There are essentially three bonding concepts used to describe the bonding in coordination compounds. Using the Valence Bond approach, analyse clearly the bonding and magnetism properties of the following complexes: (i) Naz[NIF4] (ii) Ka[Co(Br)s]
1c
(a) What coordination geometries could [AuI4]− take and how might it differ from the [AuCl4]− ion? (b) Which of Ag(NO3) and Ag2S would be expected to be more effective at removing bromide, Br−, from solution? Explain your reasoning.
Several coordination isomers, with both Co and Cr as 3+ions, have the molecular formula CoCrC₆H₁₈N₁₂. (a) Give thename and formula of the isomer in which the Co complex ionhas six NH₃ groups. (b) Give the name and formula of the iso-mer in which the Co complex ion has one CN and five NH₃ groups
In (nº-Cp)Fe(CO),CI, how many coordination sites are occupied by the Cp ligand? * O 1 O 2 O 4 O 5 In oxygenated hemoglobin, oxygen O, is reduced to oxide O2. * 2 O True O False