6. Draw orbital-energy splitting diagrams and use the spectrochemical series to show the orbital occupancy for...
5. Use the spectrochemical series and the color of the following complex ions to write the electron configuration of the d orbitals showing the crystal field splitting. Use 5 horizontal lines for the orbitals, and use arrows to represent the electrons. You do not need to label the orbitals. a. [Mn(H2O)c] is pink (assume H2O is a weak-field ligand in this complex ion) b. [CoCla]? is blue (the complex is tetrahedral) C. [Fe(CN).]" is yellow d. (Co(NH3).]** is orange
The spectrochemical series is < Br<< Cl<F-<OH" <H2O <NH3 <en <NO2- < CN- The complex [Ni(Cl)c] is green and the complex [Ni(en)]2+ is violet, where en corresponds to the ethylenediamine ligand. The reason for the difference in the color of these complexes is: Select one: A. The chloride ligand is green, and the ethylenediamine ligand is violet. B. The difference in the coordination numbers of the chloride complex and the en complex. C. The difference in the oxidation states of...
Please draw the d-orbital splitting diagrams for each [M(H2O)6]^n+ [Cr(H2O)6]^3+ [Fe(H2O)6]^2+ [Co(H2O)6]^2+ [Ni(H2O)6]^2+ [Cu(H2O)6]^2+
The transition metal ion, Fe(III), can form octahedral or tetrahedral complexes depending on the ligand it binds to. (a) (i) [Fe(CN)6]3- is a strong field octahedral complex of Fe(III). Draw a labelled orbital energy level diagram that shows both the splitting of the d-orbitals and their electron occupancy in [Fe(CN)6]. (3 marks) (ii) Fe(III) can also form tetrahedral complexes, most of which are weak field. Draw a labelled orbital energy level diagram that shows both the splitting of the d-orbitals...
Use crystal field theory to work out the d-orbital splittings and electron occupancy for the following complexes: a) [Cr(CN)6]3- b) [Ni(Cl)4]2- (This is a tetrahedral complex) c) [Pd(Cl)4]2- (This is a square planar complex)
A solution of [Ni(H2O)6]2+ is faint green and paramagnetic (μ = 2.90 BM), whereas a solution of [Ni(CN)4]2- is colorless and diamagnetic. (a) Draw the molecular geometry and the d-orbital energy level diagrams for each complex, showing the electronic occupancy of the d-orbitals. (b) Explain the differences in magnetism and color.
[Ni(NH3)6]Cl2 [(CH3CH2)4N]2CoCl4 Draw the crystal field splitting diagrams.
5. The [NI(CN)412- ion has a square-planer geometry, whereas the INca diagrams (with d-orbital labels) for these twe complexes and determine if the compound is paramognetic or diamognet ion is tetrahedral. Drow the crystal field splitting 6. The absorption maximum for the complex ion (Co( Hale ccurs at 410 m. Predict the coler of this complex.Explain your reasoning. the Lewis structure of each and state whether the following are monodentate or bide ntate ligands a. c2042 (oxalate ion, ox) b,sar...
Use the concepts of crystal field theory to predict the highest-energy orbital or group of orbitals among the five d orbitals when a transition metal ion is placed in the following type of ligand field environments (assuming conventional axes definition is used) Draw the geometry and draw the highest energy orbital (label: axis and orbital) to show how your came to your conclusion. Square planar: Trigonal bipyramidal:
Using the crystal field theory approach, draw the d-orbital splitting diagram for octahedral [Cu(OH2)6+, properly label each of the orbitals (i.e. dky etc.), and fill in the electrons. Show the changes in energy of all the d-orbitals under the influence of Jahn-Teller distortions resulting in both axial elongation and in axial compression (tetragonal distortions). Using the crystal field theory approach, draw the d-orbital splitting diagram for octahedral [Cu(OH2)6+, properly label each of the orbitals (i.e. dky etc.), and fill in...