2. Explain the following observations: (a) Co(III) forms strong bonds to O- and N-donor ligands, moderately strong bonds to P-donor ligand, and weak bonds to As-donor ligands. (b) EDTA4 forms more stable complexes with trivalent first-row transition metals (M3+) than it does with the corresponding divalent metal (M²+) of each (e.g. Cr²+ vs Cr3+). EDTA is a common ligand which bonds a metal center through four oxygen and two nitrogen atoms in an octahedral geometry (Figure 1). Figure 1. EDTA binds in an octahedral geometry

2. Explain the following observations: (a) Co(III) forms strong bonds to O- and N-donor ligands, moderately strong bonds to P-donor ligand, and weak bonds to As-donor ligands. (b) EDTA4 forms more stable complexes with trivalent first-row transition metals (M3+) than it does with the corresponding divalent metal (M²+) of each (e.g. Cr²+ vs Cr3+). EDTA is a common ligand which bonds a metal center through four oxygen and two nitrogen atoms in an octahedral geometry (Figure 1). Figure 1. EDTA binds in an octahedral geometry

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

Assess the validity of each statement and choose X if the statement is CORRECT, Choose Y if otherwise. 1. Water, ammonia and halide ions are inorganic ligands. 2. Ligands are acceptors. 3. Complexation reactions involve a metal-ion reacting with a ligand 4. Ligands can protonate. 5. EDTA is a hexadentate ligand having 4 amino groups and 2 carboxyl groups. 6. EDTA combines with metal ions in 1:2 ratio 7. EDTA forms unstable chelates with cations. 8. EDTA can be used as sequestering agent, activating metal ions. 9. Eriochrome Black T is an indicator that can be used in the determination of calcium.
Which of the following is responsible for the chelate effect exhibited by multidentate ligands? Only one ΔGo > 0 ΔSo < 0 Formation of an octahedral complex ΔSo > 0 Formation of 1:1 Metal-Ligand complex ΔG < 0
Oxyhemoglobin, with an O2 bound to iron, is a low-spin Fe(II) complex; deoxyhemoglobin, without the O2 molecule, is a high-spin complex. What ligand is coordinated to the iron in place of O2 in deoxyhemoglobin?
In the following blanks, write the chemical formula of the named coordination compounds. Use the proper case for the symbol of each atom/ligand and normal numbers, no subscripts or superscripts. Observe proper spacing and use of parenthesis and brackets.
Hexaamminechromium(III) ion, [Cr(NH³)]³+ is a metal complex containing six ammonia ligands i. ii. Using the Valence Bond Theory, construct the hybridization state of [Cr(NH3)6]³+. Predict the observed colour of the complex ion if the absorbed colour is blue-violet and briefly explain your answer.
Compare the following complexes with respect to their molecular shape and magnetic behaviour : (i) [Cr(NH3)6]3+ (ii) [Fe(CN)6]4- (iii) [NiCl4]2- (At. No. : Cr = 24, Fe = 26, Ni = 28)
(a) Draw labelled d-orbital splitting diagrams for the metal centres in [Co(OH₂)6] Cl2 and (NH4)z[CoCl4]. i) Explain any differences between the diagrams. ii) Calculate the crystal field stabilization energy (CFSE) for each complex in terms of the octahedral crystal field splitting parameter (A.). iii) What spin-only magnetic moments (measured in Bohr magneton, μB) would you expect for each of [CoCl4] and [Co(OH₂)6]²+? Which complexes would exhibit an orbital contribution to their magnetic moments and why?
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?
Draw three coordination compounds with a coordination number greater than 4 and with three different tetradentate ligands: one with C3v symmetry, another Dh4 and another C2 (complete the coordination sphere with monodentate ligands of your choice). For each of them, describe the compound, indicate the oxidation number, the number of electrons and classify the ligand used.
3. For each of the following complexes, identify whether it is a low or high spin complex (if appropri- ate) and give its magnetic properties. [Fe(NH,),]²* [Cr(CO),J²+ [VCIJ³-
Answer the following questions for the transition metal complex Mn(OH)6. Using sigma - only considerations: a) Draw the 5 d orbitals associated with the transition metal center and state whether each one will overlap (strongly, weakly, or not at all) with the ligands (assume sigma bonding only). b) Using your answer for (a), draw and label the energy levels of the d orbitals (i.e. the d orbital splitting diagram). c) Fill in the correct number of electrons. Decide whether the complex should be high spin or low spin. d) Determine the spin state (S) and multiplicity (singlet, triplet, doublet, etc) of the complex.