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- What role does EDTA4- play as a trace additive to mayonnaise? Would the glycinate ion (H2NCH2CO2-) be an effective substitute for EDTA4-?
Problem 76
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 82b
Write the formula for each of the following compounds.
(c) Tris(ethylenediamine)platinum(IV) sulfate
(d) Triamminetrithiocyanatorhodium(III)
Problem 83a
Write the formula for each of the following compounds.
(a) Diamminesilver(I) nitrate
(b) Potassium diaquadioxalatocobaltate(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-
- How does plane-polarized light differ from ordinary light? Draw the structure of a chromium complex that rotates the plane of plane-polarized light.
Problem 92
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
- The Cr3+(aq) cation is violet, but Y3+(aq) is colorless. Explain why this difference in color occurs.
Problem 109
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
Problem 130
There are three coordination compounds with the empirical
formula Co1NH3231NO223 in which all the nitrite ions
are bonded through the N atom. Two isomers have the
same molar mass but different nonzero dipole moments.
The third compound is a salt with singly charged ions and a molar mass twice that of the other compounds.
(a) Draw the structures of the isomeric compounds.
- 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