There are three possible square-planar trans isomers (trans NO2-Br, trans NO2-py and trans NO2-NH3) of the formula [Pt(NH;)(Py)(NO2)(Br)]. Suggest syntheses of these possible isomers starting from appropriate plantinate(II) ion. Make sure that you assign the correct charge to any intermediates which you draw!!

There are three possible square-planar trans isomers (trans NO2-Br, trans NO2-py and trans NO2-NH3) of the formula [Pt(NH;)(Py)(NO2)(Br)]. Suggest syntheses of these possible isomers starting from appropriate plantinate(II) ion. Make sure that you assign the correct charge to any intermediates which you draw!!

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

(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.
Both ions A2+ (Z=28) and B2+ (Z=46) can coordinate with the same types of ligands (X and Y) to form complex compounds of [AX2Y2] and [BX2Y2], respectively. A compound [AX2Y2] exists in only one geometric isomer, but two geometric isomers of the compound [BX2Y2] exist. Using the electron configuration of A2+ and B2+ to describe the formation of hybrid orbital type and formed compound structure. Compare their magnetic character and explain why the difference of complex formation.
Amines, NR3, are usually only weakly coordinating toward low valent metals. why is this so?Do you think that NF3would be abetter ligand for these metals? Discuss the factors involved.
CFT is applicable to molecules in geometries other than octahedral. In octahedral complexes, remember that the lobes of the eg set point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place,but now we have only four ligands located between the axes (as given). None of the orbitals points directly at the tetrahedral ligands. However, the eg set (along the Cartesian axes) overlaps with the ligands less than does the t2g set. By analogy with the octahedral case, predict the energy diagram for the d orbitals in a tetrahedral crystal field. To avoid confusion, the octahedral eg set becomes a tetrahedral e set, and the octahedral t2g set becomes a t2 set.
The ligand thiocyanate (SCN-) is ambidentate. Which of the following metals will it most likely interact via the sulfur atom? Circle the letter for your choice and write a brief and clear justification fro your answer. a) Tl+ b) Pb2+ c) Cu2+ d) Fe3+ e) Zr4+
Which of the species Fe, Fe2+ or Fe2+ you would expect to react more favourably with CO? Why?
For each of the following ions, draw diagrams (on a piece of paper), like the one to the right below, to show orbital occupancies for both weak and strong octahedral fields. Indicate (on the table below) the total number of unpaired electrons in each case. Ion # UnpairedWeak field # UnpairedStrong field (a) Mo4+ (b) Co4+ (c) Mo3+ (d) Mo5+ (e) Fe2+
It is observed that the substitution reactions of square plane complexes generally follow the SN2 mechanism. Is that true or false?
Strong-field ligands (such as CN-) stabilise the M2* oxidation state. Reflect on the reason.
The metal ion, M2+, formed a paramagnetic tetrahedral complex [MJ4]2+, having three unpaired electrons. Whereas, with the ligand monodentate anionic ligand A-, it forms the paramagnetic octahedral complex [MA6]4-, having the same number of unpaired electrons as that of for [MJ4]2+.Another octahedral, low-spin complex [MG3]2+, which has one unpaired electron. 1.Show the orbital diagrams for the determination of the hybridization of M2+ in the complexes [MA6]4- and [MG3]2+. Give the hybridization of M2+ in the complexes.
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.
Give the electron counts, formal oxidation states, and dn configurations of the following transition metal complexes. Show your work. a) ReH92- b) PtCl2(NH3)2 c) (n5-C5H5)2Ni d) TaMe5 e) MeReO3 Please give solution d & e