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Problem 21.80
What is the systematic name for each of the following coordination compounds?
(c) [Co(NH3)4Br2]Br
(d) Cu(gly)2
Problem 21.93
What is a racemic mixture? Does it affect plane-polarized light? Explain.
Problem 21.64
What is the oxidation state of the metal in each of the complexes?
a. AgCl2–
b. [Cr(H2O)5Cl]2+
c. [Co(NCS)4]2–
d. [ZrF8]4–
e. [Fe(EDTA)(H2O)]–
Problem 21.38
Predict the number of unpaired electrons for each of the following.
(c) Zn2+
(d) Cr3+
Problem 21.95
The glycinate anion, gly-= NH2CH2CO2 -, bonds to metal ions through the N atom and one of the O atoms. Using to represent gly-, sketch the structures of the four stereoisomers of Co(gly)3.
Problem 21.76
What role does EDTA4- play as a trace additive to mayonnaise? Would the glycinate ion (H2NCH2CH2NH2) be an effective substitute for EDTA4-?
Problem 21.108
The Ni2+(aq) cation is green, but Zn2+(aq) is colorless. Explain.
Problem 21.65
What is the oxidation state of the metal in each of the complexes?
a. [Ni(CN)5]3–
b. Ni(CO)4
c. [Co(en)2(H2O)Br]2+
d. [Cu(H2O)2(C2O4)2]2–
e. Co(NH3)3(NO2)3
Problem 21.91
Draw the three possible diastereoisomers of the triethylenetetramine complex [Co(trend)Cl2]+. Abbreviate the flexible tetradentate trien ligand H2NCH2CH2NHCH2CH2NHCH2CH2NH2 as . Which of the isomers can exist as a pair of enantiomers?
Problem 21.106
For each of the following complexes, draw a crystal field energy-level diagram, assign the electrons to orbitals, and predict the number of unpaired electrons.
(a) [CrF6]3-
(b) [V(H2O)6]3+
(c) [Fe(CN)6]3-
Problem 21.90
Draw all possible diastereoisomers of [Cr(C2O4)2(H2O)2]-. Which can exist as a pair of enantiomers?
Problem 21.86
Which of the following complexes can exist as diastereoisomers?
(a) [Cr(NH3)2Cl4]-
(b) [Co(NH3)5Br]2+
(c) [MnCl2Br2]2- (tetrahedral)
(d) [Pt(NH3)2Br2]2-
Problem 21.113
For each of the following complexes, draw a crystal field energy-level diagram, assign the electrons to orbitals, and predict the number of unpaired electrons.
(d) [Cu(en)2]2+ (square planar)
Problem 21.119
Explain why [CoCl4]2- (blue) and [Co(H2O)6]2+ (pink) have different colors. Which complex has its absorption bands at longer wavelengths?
Problem 21.6
What is the name of the compound [Fe(H2O)5(SCN)]Cl2?
(a) pentaaquathiocyanatoiron(III) chloride
(b) pentaaquachlorothiocyanato iron(III)
(c) pentaaquathiocyanatoiron(III) dichloride
(d) pentaaquathiocyanatoiron(II) chloride
Problem 21.30
Classify the following ligands as monodentate, bidentate, tri-dentate, or tetradentate. Which can form chelate rings?
(a)
(b)
(c)
(d)
Problem 21.2
Based on effective nuclear charge (Zeff), which ion is the strongest oxidizing agent?
(a) Cu2+
(b) Ni2+
(c) Fe2+
(d) Mn2+
Problem 21.87a
Tell how many diastereoisomers are possible for each of the following complexes, and draw their structures.
(a) Pt(NH3)3Cl (square planar)
(b) [FeBr2Cl2(en)]-
Problem 21.129a
Two first-series transition metals have three unpaired electrons in complex ions of the type [MCl4]2-.
(a) What are the oxidation state and the identity of M in these complexes?
(b) Draw valence bond orbital diagrams for the two possible ions.
(c) Based on common oxidation states of first-series transition metals (Figure 21.6), which ion is more likely to exist?
<QUESTION REFERENCES FIGURE 21.6>
Problem 21.78a
What is the systematic name for each of the following ions?
(a) [MnCl4]2-
(b) [Ni(NH3)6]2+
Problem 21.140a
Cobalt(III) trifluoroacetylacetonate, Co(tfac)3, is a sixc oordinate, octahedral metal chelate in which three planar, bidentate tfac ligands are attached to a central Co atom:
(a) Draw all possible diastereoisomers and enantiomers of Co(tfac)3.
Problem 21.127a
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.
(a) [AuCl4]2 (square planar)
Problem 21.80a
What is the systematic name for each of the following coordination compounds?
(a) Cs[FeCl4]
(b) [V(H2O)6](NO3)3
Problem 21.85a
Six isomers for a square planar palladium(II) complex that contains two Cl-and two SCN-ligands are shown below.
(a) Which structures are cis-trans isomers?
(b) Which structures are linkage isomers?
Problem 21.84a
Constitutional isomers of a ruthenium(II) coordination compound are shown below.
(a) Give the formula and name for structures 1-3.
(b) Which structures are linkage isomers?
(c) Which structures are ionization isomers?
Problem 21.79a
Assign a systematic name to each of the following ions.
(a) [AuCl4]-
(b) [Fe(CN)6]4-
Problem 21-113a
For each of the following complexes, draw a crystal field energy-level diagram, assign the electrons to orbitals, and predict the number of unpaired electrons.
(a) [Pt(NH3)4]2+ (square planar)
Problem 21.128a
There are two possible [M(OH)4]- complexes of first-series transition metals that have three unpaired electrons.
(a) What are the oxidation state and the identity of M in these complexes?
(b) Using orbital diagrams, give a valence bond description of the bonding in each complex.
(c) Based on common oxidation states of first-series transition metals (Figure 21.6), which [M(OH)4]- complex is more likely to exist?
<QUESTION REFERENCES FIGURE 21.6>-
Problem 21.118a
Draw a crystal field energy-level diagram, and predict the number of unpaired electrons for each of the following:
(a) [Mn(H2O)6]2+
Problem 21.131a
Nickel(II) complexes with the formula NiX2L2, where X− is Cl− or N-bonded NCS− and L is the monodentate triphenylphosphine ligand P(C6H5)3, can be square planar or tetrahedral.
(a) Draw crystal field energy-level diagrams for a square planar and a tetrahedral nickel(II) complex, and show the population of the orbitals.