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Problem 72b
Draw the structure of the following complexes. What are the oxidation state, coordination number, and coordination geometry of the metal in each?
(b) [Cr(NH3)2(C2O4)2]NO2
Problem 73a
Draw the structure of the following complexes. What are the oxidation state, coordination number, and coordination geometry of the metal in each?
(a) Pt(en)2
Problem 73b
Draw the structure of the following complexes. What are the oxidation state, coordination number, and coordination geometry of the metal in each?
(b) [Co(H2O)5Cl]SO4]
- Identify the Lewis acid and the Lewis base in the reaction of oxalate ions (C2O42-) with Fe3+ to form [Fe(C2O4)3]3-. (a) Identify the ligands and donor atoms. (b) Give the coordination number and geometry of the metal in the complex.
Problem 75
Problem 81a
What is the systematic name for each of the following coordination compounds?
(a) [Cu(NH3)4]SO4
(b) Cr(CO)6
Problem 81c
What is the systematic name for each of the following coordination compounds?
(c) K3[Fe(C2O4)3]
(d) [Co(en)2(NH3)CN]Cl2
Problem 82a
Write the formula for each of the following compounds.
(a) Tetraammineplatinum(II) chloride
(b) Sodium hexacyanoferrate(III)
Problem 83b
Write the formula for each of the following compounds.
(c) Hexacarbonylmolybdenum(0)
(d) Diamminebis(ethylenediamine)chromium(III) chloride
Problem 88
Which of the following complexes are chiral?
(a) Pt(en)Cl2
(b) cis-[Co(NH3)4Br2]+
(c) cis-[Cr(en)2(H2O)2]3+
(d) [Cr(C2O4)3]3-
Problem 97
Tris(2-aminoethyl)amine, abbreviated tren, is the tetradentate ligand N(CH2CH2NH2)3. Using to represent each of the three NCH2CH2NH2 segments of the ligand, sketch all possible isomers of the octahedral complex [Co(tren)BrCl]+.
Problem 98
Consider the octahedral complex [Co(en)(dien)Cl]2+, where dien = H2NCH2CH2NHCH2CH2NH2, which can be abbreivated
(a) The dien (diethylenetriamine) ligand is a tridentate ligand. Explain what is meant by 'tridentate' and why dien can act as a tridentate ligand.
(b) Draw all possible stereoisomers of [Co(en)(dien)Cl]2+ (dien is a flexible ligand). Which stereoisomers are chiral, and which are achiral?
Problem 99
The reaction of the octahedral complex Co(NH3)3(NO2)3 with HCl yields a complex [Co(NH3)3(H2O)Cl2]+ in which the two chloride ligands are trans to one another.
(a) Draw the two possible stereoisomers of the starting material [Co(NH3)3(NO2)3]. (All three NO2- ligands are bonded to Co through the N atom.)
(b) Assuming that the NH3 groups remain in place, which of the two starting isomers could give rise to the observed product?
- Use a sketch to explain why the dxy and dx2-y2 orbitals have different energies in an octahedral complex. Which of the two orbitals has higher energy?
Problem 103
Problem 117
In octahedral complexes, the choice between high-spin and low-spin electron configurations arises only for d4 - d7 complexes. Explain.
- Draw a crystal field energy-level diagram, and predict the number of unpaired electrons for each of the following: (c) [FeO4]2-; (b) [Ru(NH3)6]2+ (low spin).
Problem 118
Problem 123a
For each of the following, (i) give the systematic name of the compound and specify the oxidation state of the transition metal, (ii) draw a crystal field energy-level diagram and assign the d electrons to orbitals, (iii) indicate whether the complex is high-spin or low-spin (for d4 - d7 complexes), and (iv) specify the number of unpaired electrons.
(a) (NH4)[Cr(H2O)6](SO4)2
Problem 123c
For each of the following, (i) give the systematic name of the compound and specify the oxidation state of the transition metal, (ii) draw a crystal field energy-level diagram and assign the d electrons to orbitals, (iii) indicate whether the complex is high-spin or low-spin (for d4 - d7 complexes), and (iv) specify the number of unpaired electrons.
(c) [Ni(NH3)4(H2O)2](NO3)2
Problem 123d
For each of the following, (i) give the systematic name of the compound and specify the oxidation state of the transition metal, (ii) draw a crystal field energy-level diagram and assign the d electrons to orbitals, (iii) indicate whether the complex is high-spin or low-spin (for d4 - d7 complexes), and (iv) specify the number of unpaired electrons. (d) K4[Os(CN)6]
Problem 123e
For each of the following, (i) give the systematic name of the compound and specify the oxidation state of the transition metal, (ii) draw a crystal field energy-level diagram and assign the d electrons to orbitals, (iii) indicate whether the complex is high-spin or low-spin (for d4 - d7 complexes), and (iv) specify the number of unpaired electrons.
(e) [Pt(NH3)4](ClO4)2
Problem 123f
For each of the following, (i) give the systematic name of the compound and specify the oxidation state of the transition metal, (ii) draw a crystal field energy-level diagram and assign the d electrons to orbitals, (iii) indicate whether the complex is high-spin or low-spin (for d4 - d7 complexes), and (iv) specify the number of unpaired electrons.
(f) Na2[Fe(CO)4]
- The drug Nipride, Na2[Fe(CN)5NO], is an inorganic complex used as a source of NO to lower blood pressure during surgery. (a) The nitrosyl ligand in this complex is believed to be NO+ rather than neutral NO. What is the oxidation state of iron, and what is the systematic name for Na2[Fe(CN)5NO]? (b) Draw a crystal field energy-level diagram for [Fe(CN)5NO]2-, assign the electrons to orbitals, and predict the number of unpaired electrons.
Problem 124
- Based on the colors of their Cr(III) complexes, arrange the following ligands in a spectrochemical series in order of increasing crystal field splitting (∆): acac- (a bidentate ligand), CH3CO2- (acetate), Cl-, H2O, NH3, and urea. The colors of the Cr(III) complexes are red for Cr(acac)3, violet for [Cr(H2O)6]3+, green for [CrCl2(H2O)4]+, green for [Cr(urea)6]3+, yellow for [Cr(NH3)6]3+, and blue-violet for Cr(CH3CO2)3(H2O)3.
Problem 125
Problem 126a
Give a valence bond description of the bonding in each of the following complexes. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons.
(a) [Ti(H2O)6]3+
Problem 126c
Give a valence bond description of the bonding in each of the following complexes. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons.
(c) [Fe(CN)6]3- (low-spin)
Problem 126d
Give a valence bond description of the bonding in each of the following complexes. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons.
(d) [MnCl6]32 (high-spin)
- For each of the following complexes, describe the bonding using valence bond theory. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons. (c) [Fe(H2O)6]2+ (high-spin) (d) [Fe(CN)6]4- (low-spin)
Problem 127
- Describe the bonding in [Mn(CN)_6]^3-, using both crystal field theory and valence bond theory. Include the appropriate crystal field d-orbital energy-level diagram and the valence bond orbital diagram. Which model allows you to predict the number of unpaired electrons? How many do you expect?
Problem 132
- Spinach contains a lot of iron but is not a good source of dietary iron because nearly all the iron is tied up in the oxalate complex 3Fe(C2O4)3^3-. (a) The formation constant Kf for 3Fe(C2O4)3^3- is 3.3 * 10^20. Calculate the equilibrium concentration of free Fe^3+ in a 0.100 M solution of 3Fe(C2O4)3^3-. (Ignore any acid–base reactions.)
Problem 134
- The percent iron in iron ore can be determined by dissolving the ore in acid, then reducing the iron to Fe2+, and finally titrating the Fe2+ with aqueous KMnO4. The reaction products are Fe3+ and Mn2+. (a) Write a balanced net ionic equation for the titration reaction. (b) What is the mass % Fe in the iron ore if titration of the Fe2+ from a 1.265-g sample of ore requires 34.83 mL of 0.051 32 M KMnO4 to reach the equivalence point? (c) Use the E° values in Appendix D to calculate ΔG° (in kilojoules) and the equilibrium constant for the reaction. (d) Does the paramagnetism of the solution increase or decrease as the reaction proceeds? Explain.
Problem 136
- The complete reaction of 2.60 g of chromium metal with 50.00 mL of 1.200 M H2SO4 in the absence of air gave a blue solution and a colorless gas that was collected at 25 °C and a pressure of 735 mm Hg. (a) Write a balanced net ionic equation for the reaction. (b) How many liters of gas were produced? (c) What is the pH of the solution? (d) Describe the bonding in the blue-colored ion, using both the crystal field theory and the valence bond theory. Include the appropriate crystal field d-orbital energy-level diagram and the valence bond orbital diagram. Identify the hybrid orbitals used in the valence bond description.
Problem 137