The ligand substitution in organometallic complexes is very similar to that of coordination complexes. However, for organometallic complexes, the valence electron at central metal atom should not be more than 18. (a). Show TWO (2) steps synthesis of complex D by considering all of the following requirements: (i). CrO3 as a starting material and source of Cr (ii). only AsPh3 and CO as the ligand sources (can use more than 1 mole each) (iii). appropriate reaction conditions and solvents (iv). appropriate reagent(s) OC OC со Cr AsPh3 CO CO Complex D

The ligand substitution in organometallic complexes is very similar to that of coordination complexes. However, for organometallic complexes, the valence electron at central metal atom should not be more than 18. (a). Show TWO (2) steps synthesis of complex D by considering all of the following requirements: (i). CrO3 as a starting material and source of Cr (ii). only AsPh3 and CO as the ligand sources (can use more than 1 mole each) (iii). appropriate reaction conditions and solvents (iv). appropriate reagent(s) OC OC со Cr AsPh3 CO CO Complex D

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter14: Applications Of Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 14.7QAP: A 3.03-g petroleum specimen was decomposed by wet ashing and subsequently diluted to 500 mL in a...

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A 3.03-g petroleum specimen was decomposed by wet ashing and subsequently diluted to 500 mL in a volumetric flask. Cobalt was determined by treating 25.00-mL aliquots of this diluted solution as follows: Assume that the Co(II)-ligand chelate obeys Beer’s law, and calculate the percentage of cobalt in the original sample.
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
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).
Consider the [Ir2(dimen)4] 2+ complex. Notice that the dimen ligand is asymmetric. There is also a different, symmetric diisocyano ligand referred to as “TM4” (structure shown to the right) that forms the same sort of binuclear complex that dimen does. Answer the following questions with supporting justification: a. How many geometric isomers (ignore any optical ones) of [Ir2(TM4)4] 2+ are there? b. How many geometric isomers (ignore any optical ones) of [Ir2(dimen)4] 2+ are there? c. In the “twisted” deformational isomer, would you expect [Ir2(TM4)4] 2+ or[Ir2(dimen)4] 2+ to be able to rotate polarized light? Justify your answer.
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.
Sketch structure of Mo(DMe) Cl2 (NMe,)2 , thhen apply ean to this complex showing ligand analysis and oxidation state analysis
The anticancer drug cisplatin, cis-[Pt(NH3)2Cl2] (see Figs. 8.12b and 8.33),can be prepared from K2PtCl6 via reduction with N2H4 (hydrazine), givingK2PtCl4, followed by replacement of two chloride ion ligands with ammonia. Give systematic names to the three platinum complexes referred to inthis statement.
Werner prepared two compounds by heating a solution of PtCl₂ with triethyl phosphine, P(C₂H₅)₃, which is an excellent ligand for Pt. The two compounds gave the same analysis: Pt,38.8%; Cl, 14.1%; C, 28.7%; P, 12.4%; and H, 6.02%. Writeformulas, structures, and systematic names for the two isomers
(a) A compound with formula RuCl3 . 5 H2O is dissolved inwater, forming a solution that is approximately the samecolor as the solid. Immediately after forming the solution,the addition of excess AgNO3(aq) forms 2 mol of solid AgClper mole of complex. Write the formula for the compound,showing which ligands are likely to be present in the coordinationsphere. (b) After a solution of RuCl3 . 5 H2O hasstood for about a year, addition of AgNO3(aq) precipitates 3mol of AgCl per mole of complex. What has happened inthe ensuing time?
Provide crystal field splitting diagrams that clearly show orbital names, orbitalelectron population, and 10Dq (i.e. ∆o) for the following complexes. Use your knowledge of the spectrochemical series and crystal field theory to determine LS vs. HS
Explain why the tetrahedral complexes A and B have magnetic moments of 1.89 and 0.0 BM respectively. Comment on the observations.
a) Give one similarity and one difference between “monodentate” and “bidentate” ligands. b) Which one of the types of ligands named in part “b” is more closely related to the term “chelating agent”? Please explain.