Which of these three octahedral coordination compounds is/are paramagnetic? (Refer to the spectrochemical series below)
(1) [Sc(H2O)6] 3+
(2) [FeF6] 4–
(3) [Mn(CN)6] 3–
The spectrochemical series:
Cl– < F– < H2O < NH3 < en < CN–
(weak field/high spin) (strong field/low spin)
Please explain.
Which of these three octahedral coordination compounds is/are paramagnetic? (Refer to the spectrochemical series below) (1)...
Using the spectrochemical series, fill the electrons in the correct crystal field diagram (shown below) for the following complex. Is this complex high spin or low spin complex? Also predict is the compound is paramagnetic or diamagnetic. Spectrochemical Series I<Br<C1<F-<OH<H2O<NH3<en< NO2 <CN<CO [Co(en)3]3+ or dxz dyz dxy de dx²-y? d22 dx?-? dxz dyz dxy
Use the following electrochemical series: CN -1 > NO2-1 > en > NH3 > H2O > OH -1 > F -1 > Cl -1 > Br -1 > I -1 Given compound: [Mn(en)3]+3 For octahedral field splitting diagrams, outline in detail how you determine the following: a) neutral metal's electron configuration b) ion's electron configuration c) the number of d electrons in the ion d) drawing the splitting pattern, labeling the orbitals in the splitting pattern, the filling of electrons,...
All of the following complexes are either octahedral or tetrahedral. Determine if the complex is diamagnetic or paramagnetic, if the complex is high spin or low spin, and ii) the number of unpaired electrons. Unpaired Electrons Spin low Magnetism Complex [Fe(CN)6]* [Co(NH3)4]3 13+ 14- 4+ [Ru(CO)6] All of the following complexes are either octahedral or tetrahedral. Determine if the complex is diamagnetic or paramagnetic, if the complex is high spin or low spin, and ii) the number of unpaired electrons....
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
Which of the following octahedral complexes would be substitution inert? Which would be substitution labile ?(using the definition of H. Taube) (H2O)6Co+2, (NH3)6Co+3, (H2O)6Cr+2 , (H2O)6Cr+3, (H2O)6Ti+3, (H2O)6V+2, (H2O)6V+3, (CN)6Rh-3, Think of H2O, Cl- and Br- as weak field ligands, NH3 and CN- as strong field ligands. PLEASE SHOWYOUR WORK
1b Assume two octahedral coordination compounds, each containing the same central metal ion with five unpaired d electrons (e g. Fe3+) One compound contains a weak-field ligand (e.g. F) and the other compound contains a strong-field ligand (e g CN). Compared to the strong-field compound, it is expected that the weak-field compound would have a I. smaller magnetic moment and absorb higher energy light . smaller magnetic moment and absorb lower energy light . larger magnetic moment and absorb higher...
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...
Certain square planar and octahedral coordination compounds have forms that are stereoisomers. In biological systems, this is of importance because one isomer may be an effective treatment for a condition such as cancer, while the other isomer has no effect or is toxic. Below are a series of coordination compounds. Sort the cis and trans isomers into the appropriate category. Stereoisomers (6 images) (Drag and drop into the appropriate area below) CICI H3N.pt.CI HI CI, NH3 H₂N HENNHET HINCH CI...
Q1. The following species a)-c) all contain complex ions of transition metals, which you can assume take up an octahedral geometry. a) [RuCl3(H2O)3] b) [Ir(bpy)3]Cl3 ; bipy = 2,2'-bipyridine c) K2[Mo(NCS)6] For each species: i) draw all the possible isomers of the complex ions; ii) calculate the charge of the metal, and the dn configuration; iii) draw a diagram showing d orbital occupancy and, where high and low spin cases are possible, predict which will be favoured considering the spectrochemical...
For the next three problems, refer to the following coordination compound. [Co(en)2(H2O)(Cl)]3[Ni(CN)4]2 Name the compound: