4. Introducing n-interactions from our M-Lo-only description. a. Using group theory, derive the full MO diagram for the hypothetical ion ReCla in square planar geometry, showing all the metal valence orbitals and all relevant ligand orbitals. For simplicity, you should disregard the n-donor ability (which is pretty weak) of the chlorines in all questions (here and below), and view each Cl atom as presenting a single a-symmetry orbital toward the metal. Also, Re 6s and 5d orbitals are at -8.76 and -9.70 ev, respectively, consider the CI SALCS at -13.67 ev. Populate your diagram with electrons. Your d-splitting diagram should reflect the relative spacing that you expect from the Angular Overlap Method.

4. Introducing n-interactions from our M-Lo-only description. a. Using group theory, derive the full MO diagram for the hypothetical ion ReCla in square planar geometry, showing all the metal valence orbitals and all relevant ligand orbitals. For simplicity, you should disregard the n-donor ability (which is pretty weak) of the chlorines in all questions (here and below), and view each Cl atom as presenting a single a-symmetry orbital toward the metal. Also, Re 6s and 5d orbitals are at -8.76 and -9.70 ev, respectively, consider the CI SALCS at -13.67 ev. Populate your diagram with electrons. Your d-splitting diagram should reflect the relative spacing that you expect from the Angular Overlap Method.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter9: Complexometric And Precipitation Titrations

Section: Chapter Questions

Problem 1P

See similar textbooks

Similar questions

Many transition metal complexes are said to follow the “18-electron rule,” meaning they form particularly stable complexes when the metal + ligand electrons contributing to the MOs add up to a total of 18 electrons. a. Use the full MO diagram for an octahedral metal complex with pi-acidic ligands we derived in class to justify why 18-electrons might be particularly stable. b. Use the 18-electron rule to predict which 1st row transition metal would be most likely to form an octahedral M(CO)6 (Note: there is no charge; the metal retains all its electrons.) c. Qualitatively, how would you expect the CO bond to change when it forms this complex? Would it be stronger, weaker, or the same compared to free CO? (Hint: think about what a ? −???? means and what the orbital does from the perspective of the M–CO interaction as well as the C– O interaction).
Regarding the formation of the tetracyanetoniquelate (II) complex answer:a.Demonstrates hybridization according to the valence bond theory and indicate itsgeometry.b. Demonstrate and explain the unfolding of the crystalline field in the formation of this ioncomplex.c. Demonstrate through a diagram of molecular orbitals and explain the formation of that ioncomplex according to the ligand field theory
For problem 2, I have to assign oxidation states for transition metals by drawing the lewis structure with all the sigma bonds, rmeoving all the ligands on their closed shell configuration and noting the formal charge, and accounting for all the ligand charges, where oxidation number = molecular charge - sum of ligand charges.I am unsure how to identify Lewis acids. How to solve Problem 7?
Sketch structure of Mo(DMe) Cl2 (NMe,)2 , thhen apply ean to this complex showing ligand analysis and oxidation state analysis
1 Show the calculation of electrons for the complexes below using the 18-electron count principle
1,Count up the 18-electron rule of the organometallic complex (Ferrocene) using covalent counting method.2. Draw the molecular orbital diagram for B2 and find the bond order?
Construct an MO correlation diagram for the complex ion[Ni(NH3)6]2+ and populate the orbitals with electrons. Do youexpect p bonding to be important for this complex? Whatfeatures of this diagram correspond to those predicted usingcrystal field theory? What kind of bonding would VB theorypredict for d8 complexes, and how does MO theory accountfor the bonding more accurately, even qualitatively?
Why wouldn't this ruthenium catelyst, with two trans IMes ligands, be good at catalysing alkene metathesis?
In general, would you expect EDTA4- to coordinate to transition metal ions more or less strongly than ethylenediamine does? Justify your answer with a reason other than the different charges on the two ligands.
Comment on the use of IR spectroscopy in the characterisation of transition metal complexes.State one (1) limitation of this technique.
Copy the structure of EDTA4- from your textbook and circle all six atoms that act as Lewis bases. Why does EDTA4- cease to function as a chelating ligand if acid is added to the solution? pls help asap!!
Generally speaking, for a given metal and ligand, the stability of a coordination compound is greater for the metal in the +3 rather than in the +2 oxidation state (for metals that form stable +3 ions in the first place). Suggest an explanation, keeping in mind the Lewis acid–base natureof the metal–ligand bond.