Which of these three octahedral coordination compounds is/are paramagnetic? (Refer to the spectrochemical series below) (1)...
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.
Homework Answers
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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...
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 >...
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 par...
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...
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...
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
Order the extinction coefficients of the following three manganese complexes according to their magnitude. Consider only...
Order the extinction coefficients of the following three manganese complexes according to their magnitude. Consider only d-d transitions, and explain your answers. Note: Consider the type of ligands (weak-field vs. strong-field) when deciding whether the complexes are high-spin or low-spin. [Mn(H2O)6]2+, [MnCl4]- , and [Mn(CN)6]4- .
The spectrochemical series is < Br<< Cl<F-<OH" <H2O <NH3 <en <NO2- < CN- The complex [Ni(Cl)c]...
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...
ANSWER ALL QUESTIONS PLEASE 1. What are the characteristic electron configurations of transition metals? 2. What is...
ANSWER ALL QUESTIONS PLEASE 1. What are the characteristic electron configurations of transition metals? 2. What is the general trend in atomic size across a transition metal series? 3. Which electrons, 3d or 4s, have the lowest ionization energies in a transition metal? 4. What is the general trend of the reducing strength across a transition metal series? 5. Why do transition metals have similar chemical properties? 6. Name four transition metals that are essential to the biological system. 1. Write the...
1b Assume two octahedral coordination compounds, each containing the same central metal ion with five unpaired...
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...
please help :( 9. Suggest a reason why copper(II) compounds are often colored but copper(1) compounds...
please help :(
9. Suggest a reason why copper(II) compounds are often colored but copper(1) compounds are colorless. 10. Sketch the d-orbital energy-level diagram for a square planar complex. Spectrochemical series: CO - CN > phen > NO, >en > NH3 > NCS > H2O > F > RCOO > OH > Cl > Br > 650 nm O 580 nm 750 nm 400 nm 560 nm 430 nm 490 nm
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
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
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...
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...
please help :(
9. Suggest a reason why copper(II) compounds are often colored but copper(1) compounds are colorless. 10. Sketch the d-orbital energy-level diagram for a square planar complex. Spectrochemical series: CO - CN > phen > NO, >en > NH3 > NCS > H2O > F > RCOO > OH > Cl > Br > 650 nm O 580 nm 750 nm 400 nm 560 nm 430 nm 490 nm
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