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Explain the differences shown in the table for 4 ligand in terms of their varying affinity for metal binding
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- Consider K1[MABCD] Ligand Charges: A = -1; B = -1; C = -1; D = -1 Screen Reader User: Charges are either 0 or minus 1. End of note. What is the charge on the metal M?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+Need help with this question. Thank you :)
- Consider the compound (C8H8)Ru(CO)3. Which is likely to be the best description of the C8H8 ligand? а. It is bonded in an no-manner to the Ru atom b. It is bonded in an n4-manner to the Ru atom O C. It is bonded in an n3-manner to the Ru atom d. It is bonded in an n2-manner to the Ru atomTrimethylphosphine, P(CH3)3, can act as a ligand by donating the lone pair of electrons on the phosphorus atom. If trimethylphosphine is added to a solution of nickel(II) chloride in acetone, a blue compound that has amolecular mass of approximately 270 g and contains 21.5% Ni, 26.0% Cl, and 52.5% P(CH3)3 can be isolated. This blue compound does not have any isomeric forms. What are the geometry and molecular formula of the bluecompound?14. The complex ion [Ni(TAP)(CN)]+ has a distorted trigonal bipyramidal structure, the complex ion has a coordination number… A. 4B. 6C. 5D. 7
- What electronic feature must a donor atom of a ligand have?Differentiate between monodentate ligands, bidentate ligands,and polydentate ligands?3a) The nitrosyl ion, NO*, is a very rare case of a cationic ligand that can function as a Lewis base. Draw the Lewis structure of this ligand under consideration of the VSEPR rules and indicate any formal charges on the constituent atoms. 3b) How many electrons does the NO* ligand contribute on the ionic model and the neutral model, respectively? Assume that the Metal-N-O bonding angle is 180° upon coordination.
- Q5 a) What are the geometric shape and the oxidation number of the copper atom, respectively, for the complex ion, [CuCl5]3- ? b) which of these ligands is ambidentate or bidentate or monodentate or tridentate? (F-, ethylenediamine, CNS-, NO2-, C2O4H2, Diethylenetriamine)."The π* orbital of NO is partially filled with an unpaired electron, which makes it less efficient in accepting electron density from the metal’s d orbitals. On the other hand, the fully empty pi*orbital of CO can strongly overlap with the metal’s d orbitals, resulting in a stronger π-back bonding interaction and a stronger metal-ligand bond. " Is this correct and makes NO weaker?2. Consider a hypothetical trigonal bipyramidal Fe(III) complex [FeF2(OH)3]². We need to divide the five donor atoms of the ligands into two groups: 2F and 30. F HO FeOH F OH (a) Identify the point group of the complex and assign x, y, and z to it. (b) Indicate the symmetries of the Fe valence orbitals, i.e., 3d, 4s, and 4p. (c) Derive the symmetries and expressions of the two F σ-SALCs, considering that each F. atom contributes one 2p orbital with a lone pair to form the σ-SALCs. (d) Derive the symmetries and expressions of the three σ-SALCs on the OH ligands, considering that each O atom contributes one 2p orbital with a lone pair to form the σ- SALCs. (e) Draw a σ bonding-only MO energy level diagram for the complex, mark the MOs with symmetry labels, and fill the MOS with the valence electrons. (f) Consider each O atom contributing one perpendicular 2p orbital to form π-SALCs. Derive the symmetries of the three л-SALCS. (g) Identify the MOs in (e) with which the O л-SALCs interact,…
