Please do both Show the electron counting for the metal center of each of the complexesbelow by using the ionic model. The answer should include the formaloxidation state of the metal, the number of d electrons, ligand charges (ifpresent) and the total electron count.QI.(а)(i)(ii)R2PlMECN-MeCNNCME(iii)MeMeRh(b)Given a pair of metal hydride complexes:1f-Cp*Ru(H)(PME3)2 or V(H)(CO),(where Cp* =C3Mes)Choose the complex with the lower pKa value and explain why.-C=O

Answered: (а) Show the electron counting for the…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter26: Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 26.30QAP

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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.
Explain why the tetrahedral complexes A and B have magnetic moments of 1.89 and 0.0 BM respectively. Comment on the observations.
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
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.
Provide a name for the following complex ion:[AuF4]^-
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).
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?
Draw a Lewis structure for the cyclopentadienyl ligand (C5H5)- and explain why it is more likely to bind it’s aromatic protons to a transition metal center compared to the similar benzene molecule (C6H6).
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.
A hypothetical metal M forms the following complexes with the generalized ligands X, Y, and Z: Complex ion Observed color [M(X)6]3+ green [M(Y)6]3+ blue [M(Z)6]3+ yellow Order these ligands according to their ability to split d orbitals. In other words, set up a spectrochemical series, from strongest to weakest ligand field strength. Rank from strongest to weakest ligand field strength. -X -Z -Y
Explain in detail π backbonding using the molecular orbitals of CO and a d-transition metal. How does this influence Infrared Spectroscopy and explain how the bond order for the C-O bond changes and how the bond order for the metal-ligand bond changes. Provide pictures and explanations. (Inorganic Chemistry)
[V(H2O)6]3+, has absorption bands at 17,800 and 25,700 cm-1. Please answer the following questions using a relevant Tanabe-Sugan diagram. a) How many electronic transitions are possible for this complex? b) Identify these transitions and clearly label the states.

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(а) Show the electron counting for the metal center of each of the complexes below by using the ionic model. The answer should include the formal oxidation state of the metal, the number ofd electrons, ligand charges (if present) and the total electron count.