(a) Using the 18-electron rule, predict the number of CO ligands (X, Y, Z) for the most stable form of the following organometallic species, explaining your answers, and sketch the structures of G, H, I: G RU(CO)x H CO₂(CO)Y I Na₂[Fe(CO)z] (b) In the case of species H, discuss how the presence or absence of μ-CO ligands could be determined experimentally and what this would mean for the structure of the complex. (c) Treatment of I with ethyl bromide EtBr leads to the product J Na[EtFe(CO)z]. Explain what other product(s) are formed and why this is therefore a useful synthetic strategy.

(a) Using the 18-electron rule, predict the number of CO ligands (X, Y, Z) for the most stable form of the following organometallic species, explaining your answers, and sketch the structures of G, H, I: G RU(CO)x H CO₂(CO)Y I Na₂[Fe(CO)z] (b) In the case of species H, discuss how the presence or absence of μ-CO ligands could be determined experimentally and what this would mean for the structure of the complex. (c) Treatment of I with ethyl bromide EtBr leads to the product J Na[EtFe(CO)z]. Explain what other product(s) are formed and why this is therefore a useful synthetic strategy.

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

Elimination of an L ligand (as the first step of a D substitution mechanism) from a charge - neutral NiL4 complex has very little tendency to occur for L = P(OMe3), but for L = PMe3, it occurs almost completely. Since the two ligand species have approximately the same cone angle, what factors are responsible for this difference?
Please send me the question in 20 minutes it's very urgent plz find
For the following structure derived from a tetrahedral Ni(CO)4, please determinethe number of infrared and Raman bands for their CO groups. (Please note: Modes withtranslational symmetry (x, y, z) will be infrared active while modes with xy, xz, yz, x2, y2 or z2symmetry are Raman active.)
Q 2. Comment on the Kinetic and thermodynamic stability of metal complexes? (2 marks) (a) Which complex is kinetically labile or inert according to crystal field theory? H₂O OH2 OH2 * H₂O NECHI Mn OH2 OH2 4- 2+ [+] NEC CEN CEN (b) Which complex is most thermodynamically stable and why? Calculate log ẞ to determine stability? H3N 2+ _NH3] 2 [NC-Ag-CN]] NH3 3+ H3N... H3N ,,NH3 Cr NH3 H3N NH3 NH3 K 1.0 x10¹² K 5.4 x 1018 K=2.0 × 105
(a) What are the oxidation states and d-electron counts of the metal(s) in the following complexes? (i) TiCl4 (ii) NiBr2(PPH3)2 (iii) Ru3(CO) 12 (iv) K[Mn(CO)5] (b) Cp Re (CO)3 reacts with hydrogen peroxide to give Cp*Re(0)3 (Cp* = n5-C5Me5). Write a balanced equation for this transformation and give the oxidation states and d-electron counts for rhenium in both complexes. Comment on the nature of CO and oxide ligands within the Pearson hard-soft acid-base theory. (c) The Cp* ligand can be considered to occupy either one or three metal coordination sites. For Cp*Re(CO)3 draw crystal field splitting diagrams for both of these possibilities. (d) Explain briefly the terms diamagnetic and paramagnetic.
Write the name of the structure and the magnetic behaviour of each one of the following complexes: (i) [Pt(NH3)2Cl(N02)] (ii) [CO(NH3)4 Cl2] Cl (iii) Ni(CO)4 (At. nos. Co = 27, Ni = 28, Pt = 78)
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?
(ii) In a historical industrial process Co(CO)4H is generated in-situ from Col2, CO and H₂O. By-products are CO₂ and HI. Give the two relevant half-equations and then construct the full redox equation. Give the chemical structure of platinum complex I which is obtained from the reaction of PtCl₂(PPhMe2)2 with one equivalent of Lit CH₂(CH2)2CH₂ Lit.
Write the name, the structure and the magnetic behaviour of each one of the following complexes :(i) [Pt(NH3)2Cl(NO2)](ii) [Co(NH3)4Cl2]Cl(iii) Ni(CO)4 (Atmos. Co = 27, Ni = 28, Pt = 78)
(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]
6. a) Discuss the relationship between the octahedral splitting energy, (Aoct), for complex ions and the ligand strength of the ligands in the complex ion. b) Considering only the complexes, Ni(en)3²+ (aq), Ni(NH3)²+(aq), and Ni(H₂O)62+ (aq), determine the relative ligand strengths of ammonia, ethylenediamine and water. Place the ligands in increasing order of ligand strength. (weakest ligand to the strongest ligand.) c) Discuss how you arrived at your conclusion in part b. Include in your discussion your data and/or your calculated values for these complex ions to support your conclusion.
For [Co(H2O)6]2+ , Discuss the similarities/dissimilarities in the magnetic moment values with experimentally determined values of 5.0 and 4.4 µB for octahedral and tetrahedral complexes, respectively.